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Electrostatics Flashcards

9492915997	electrostatics	the science dealing with static electric charge	0
9492924665	charge	a special state of the body in which it is able to take part in electric interactions	1
9492934022	positive charge	the charge of a glass rod rubbed with silk	2
9492936017	negative charge	the charge which is attracted by the positive one	3
9492954555	basic electric phenomena	-attraction -repulsion -influence -charging up -neutralization -grouding	4
9492964534	attraction	unlike charges attract eachother	5
9492966804	repulsion	like charges repell eachother	6
9492968775	influence	positive and negative charges separate inside an originally neutral body as the effect of a charged body	7
9492978103	grounding	when connectin an electrically charged body and the Earth with a conductor the charge flows to the Earth	8
9492987958	neutralization	seperated positive and negative chrages equlize eachother inside a body or a system	9
9492993065	neutral body	the body has no charge OR it has both positive and negative charges of the same quantity	10
9493000080	electric conductor	material in which charge flows freely	11
9493005796	electric insulator	material in which charge does not flow freely	12
9493009667	electrolyte	a substance producing an electrically conducting solution when dissolved in a polar solvent such as water	13
9493024007	electroscope	a device for detecting the presence and determining the sign of electric charges by means of attraction and repulsion	14
9493034676	plazm state	a state of matter in which ions and electrons move freely (electrolized gas)	15
9493040617	source body	a body which generates an electric field	16
9493044707	test body	a body used to investigate an electric field	17
9493049422	electrically closed system	charge can not enter or leave the system	18
9493051878	electric force	a type a force exerted by a charged body on its surroundings	19
9493071108	Coulomb's law	the electric force depends on the 2 charges and the distance between them	20
9493084431	principle of the conservation of electric charge	in an electrically closed system the totl amount of charge is constant in time	21
9493090093	electric field	a special region of space in which electric effects can be observed	22
9493097344	homogeneous electric field	the field lines are parallel and the density of them is constant	23
9493103465	inhomogeneous field	the field lines aren't parallel and their density is not constant (e.g.: radial structure of a pointlike source body)	24
9493109673	electric field strength	it gives the value of the electric force on a unit positively craged test body	25
9493120012	the vector of electric field stregth	a vector which has always the same direction as that of the electric force exerting on a positively charged test body	26
9493128339	electric field lines	imaginery curves indicating the direction of the electric field strengt vectors. at any point of the field line the direction of the electric field vector is always tangential	27
9493142739	properties of electric field lines	-field lines always start from a positively charged source body -field lines always terminate at a negatively charged source body -field lines never intersect eachother	28
9493154115	electric flux	the number of field lines intersecting a unit imaginary surface parallelly (in rality there are infinite number of field linesí)	29
9493169982	linear density of electric charge	the electric charge of a unit length	30
9493173528	surface density of electric charge	the electric charge of a unit surface	31
9493175587	shielding	there is no electric charge inside a conductor	32
9493178972	stable equilibrium position	when removing the body from its equilibrium position it will return after the force exerting on it ceases	33
9493190414	unstable equilibrium position	when removing the body from its equilibrium position it will not return after the force exerting on it ceases	34
9493199192	work done by an electric field	the electric field does work when the test body moves along the field lines; the work only depends on the initial and final position of the object and not the path connecting the two positions	35
9493212347	level	the set of points in the electric field when moving a test body between these points there is no work done by the electric field on the test body	36
9493222876	conservative field	the amount of work done on the test body by the field is independent of the shape of the path	37
9493228357	voltage	voltage gives the work done on a unit positively charged test body by the electric field while carrying it from one level to another	38
9493237668	potential	the needed amount of work to carry a unit positively chraged test body from zero level to a certain point	39
9493247732	potential energy	the amount of energy gained by the test body while carrying it from the zero level to another one	40
9493258403	principle of energy conservation in an electric field	the total amount of energy of a test body in an electric field is constant in time	41
9493272578	conductors in an electric field	-the charges accumulate on the surface of the conductor as a result of the repulsion of like charges -field lines started from a conductor behaving as a source body are perpendicular to the surface -all the points of the surface of a conductor have the same potential->they form a level -when placing a conductor in an electric field a new electric field is generated in which the field lines are the opposite of the original ones. Because of this the resultant electric force inside a conductor is always 0, so no electric effects can be experienced inside the conductor. This is the phenomenom of shielding	42
9493318094	pinpoint effect	electric charge is accumulated on the surface of a metalic conductor at positions of biggest curvature	43
9493326648	electric wind	the wind blowing from a source body as a result of repulsoin of like charges	44
9493336518	electric capacitance	capacitance gives the needed amount of charge to generate a unit potential difference	45
9493366473	condensor	a special type of electric instrument consisting of two pieces of oppositely charged metal which can store a large amount of charge on the surface	46
9493377096	polarization	in an insulator bc of the rotation of the dipole molecules the resultant electric field stregth decreases when putting it between two condensor plates	47
9493401718	series combination of condensors	-all the charges are equal -the total amount of voltage is equal to the sum of the voltages -there is inverse propotion between the voltages dropping between the two plates of the condensors and the capacitances -the reciprocal of the equivalent capacinótance is equal to the sum of the reciprocals of the capacitances of the original condensors	48
9493473125	equivalent capacitance	the capacitance of the imaginery condensor substituting the original ones so that it has the same effects as them	49
9493481750	main branch	from the positive pole to the first junction and from the last junction to the negative pole	50
9493489752	junction	where the brances meet	51
9493492177	parallel combination of condensors	- the total amount of charge is equal to the sum of the charges -all the voltages are equal -there is direct propotion between the charges and the capacitances -the equivalent capacitance is the sum of the capacitance of the original condensors	52
9493518421	electric energy	the amount of energy stored inside the electric field of the condensor	53
9493524165	electric current	the ordered flow of electric charge	54
9493528904	direct current	charge flows to the same direction	55
9493533689	alternating current	there is periodic change in the direction of the flow of the charge	56
9493539972	current intensity	the amount of charge flowing through a certain crossection of the wire in a unit time	57
9493548038	superconductors	special type of metals or coils of metals in which when starting an electric current the current intensity will be constant without applying an electric source	58
9493557860	heat effect of electric current	it is a direct and compulsory effect e.g.: oven, hairdryer, electric heat radiator...	59
9493569446	magnetic effect of electric current	it is a direct and compulsory effect e.g.: electromagnet (coil of wire+iron core; current->magnetization->good bc its strength can be easily changed)	60
9493576824	chemical effect of electric current	direct effect of direct current but not alternating current	61
9493595155	electrolysis	any type of process during which chemical reactions are started as the effect of the electric current driven into certain materials	62
9493618945	electrode	a piece of metal submerged into an electrolyte	63
9493623900	indifferent electrode	an electrode made of stable materilas so that it carries the current inside the water solution but it doesn't take part in chemical reactions	64
9494713863	biological effect of electric current	it is a consequence of the other effects (heat nad chemical): muscles contract, burn- the human body acts as a watersolution	65
9494724950	light effect of electric current	it is a consequence of the other effects	66
9494731613	conditions of the flow of the electric current between two points	-there is potential difference between the points -the points are connected with a conductor	67
9494739636	technical direction of current	by definition current cosists of positive charges	68
9494745732	real direction of current	in reality electrons (negative charges) flow	69
9494752867	electric source	an instrument carrying electric charge from the position of lower potential to the position of higher potential (work is done)	70
9494761785	types of electric sources	-galvanic cell -generator -solar cell	71
9494764016	galvanic cell	electric source producing electricity with the help of chemical reactions	72
9494769974	redoxi reaction	electron transport from a certain material to another	73
9494773641	generator	an instrument producing electricity with the help of electromagnetic induction (e.g.:dynamo)	74
9494780126	motional induction	current is induced inside a coil of wire surrounding a rotating magnet	75
9494789067	solar cell	an instrument made of semiconducting materials in which electron transportation is generated when exposed to light	76
9494794293	diod	any type of instrument which regulates the direction of the current	77
9494799304	consumer	any type of instrument which uses the energy of the current	78
9494803288	electric resistor	any type of instrument on which the current has heat effect	79
9494808526	electric resistance	it gives the value of the needed voltage generating unit current intensity between two points	80
9494815383	resistance depends on	-length of wire -cross section of wire -material of the wire -temperature of the wire	81
9494830377	series combination of resistors	-the current intensities are the same everywhere -the total amount of voltage is equal to the sum of the voltages of the original resistors -the equivalent resistance is equal to the sum of the original resistances -there is direct propotion between the voltages dropping on the resistors and the resistance values -advantage: many resistors of small resistance values have enough resistance together to work -disadvantage: if one of the resistors goes wrong none of them work -e.g.: christmas lights	82
9494849549	equivalent resistor	an imaginery resistor substituting the original ones so that it has the same effect as that of the original ones	83
9494886540	parallel combination of resistors	-the total current intensity is equal to the sum of the current intensities flowing through the original resistors -the voltage dropping on the resistors are equal everywhere -the reciprocal of the equivalent resistance is equal to the sum of the reciprocals of the resistances of the original resistors -there is inverse propotion between the current intensities and the resistance values -advantage: independent use -disadvantage: too many consumers can not work together -e.g.: electrical multi-outlet	84
9494922329	Wheatstone-bridge	a type of bridge combination in which the ratio of the resistances in the two brances are equal	85
9494929998	Kirchoff's first law	the algebraic sum of current intensities flowing towards or away from a junction is equal to 0	86
9494937356	Kirchoff's second law	the algebraic sum of the voltages dropping on the single resistors or generated by the sources is equal to 0 for a full cycle/loop in the circuit	87
9494947695	power of electric current	the amount of heat developed in unit time	88
9494952263	short circuit	two points in a circuit are connected with a wire of 0 resistance	89
9494956288	potentiometer	any type of instrument whose resistance can be changed easily	90
9494961056	internal resistance	the resistance inside the source which is always present	91
9494965331	internal voltage	the voltage dropping on the source itself	92
9494968251	full circuit	always contains the internal resistance of the source	93
9494972428	electromotoric force	the maximum voltage which can be generated by the source	94
9494978101	the special case of opened circuit	-the external resistance is infinite -the current intensity is 0 -the internal voltage is 0 -the electromotoric force is equal to the external voltage	95
9494991545	the special case of short circuit	-the external resistance is 0 -the equivalent resistance is equal to the internal resistance -maximum current intensity	96
9494998536	ammeter	an instrument measuring current intensity; it is always combined serially to get proper results	97
9495005046	ideal ammeter	its resistance is almost 0	98
9495007511	measurement limit	maximum current intensity/voltage which can be observed without the instrument going wrong	99
9495015482	shunt	a resistor combined parallelly with the ammeter to extend its measurement limit	100
9495021790	voltmeter	a type of instrument measuring voltage ; it is always combined parallelly to get the proper results; another serially combined resistor is neede to extend its measurement limit	101
9495033850	ideal voltmeter	its resistance is close to infinite	102

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Physics Formulas, Physics Formulas Flashcards

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10515690642	Torque	Force applied x lever arm length	0
10515690643	Local gravitational potential energy	PE= mgh	1
10515690644	General gravitational potential energy	PE= -GMm/r	2
10515690645	3 types of conservative forces	Fg, Felastic, Felectric	3
10515690646	4 types of nonconservative forces	Ff, Air, Fn, Ft	4
10515690647	What makes a force conservative?	2 ways: 1. If the work done by the force on an object moving from one point to another depends only on the initial and final positions and is INDEPENDENT of the particular path 2. Net work done by the force on an object moving around a closed path is zero	5
10515690648	Work-energy theorem	Work due to non-conservative force= change in kinetic + change in potential + any change in internal energy	6
10515690649	Conservation of mechanical energy	Total mechanical energy of a system remains constant as the object moves, provided that the net work done by non-conservative forces is zero	7
10515690650	Angular displacement	arc length/radius	8
10515690651	Moment of inertia	Torque= moment of inertia x angular acceleration	9
10515690652	Energy used in rotating something	1/2 I(inertia)w^2	10
10515690653	Buoyant force	Fb= density x volume displaced x g	11
10515690654	Doppler effect	The apparent frequency of the source is increased as the source approaches the observer, and is decreased at it leaves	12
10515690655	Elastic vs Inelastic collisions (in regards to KE and momentum)	Elastic: KE and momentum are conserved Inelastic: KE is NOT conserved, momentum is	13
10515690656	Angular momentum	L= moment of inertia x angular velocity	14
10515690657	Electric field due to a point charge	E=kQ/r^2	15
10515690658	Electric potential energy	kQ1Q2/r	16
10515690659	Electric potential	V=kQ/r	17
10515690660	Force in a constant electric field	F= qE	18
10515690661	Electric potential in a constant electric field	V=Ed	19
10515690662	Electric potential energy in a constant electric field	U= qEd=Vq	20
10515690663	Force on a charge moving in a magnetic field	F=qvBsin(theta)	21
10515690664	Electric power	P=IV=I^2R= V^2/R	22
10515690665	Electric potential energy stored by a capacitor	U= 1/2 CV^2 = 1/2QV= 1/2Q^2/C	23
10515690666	Total internal reflection	critical angle= n2/n1	24
10515690667	Index of refraction	n=c/v, v2/v1=n1/n2	25
10515690668	The lens equation	1/object distance + 1/image distance= 1/focal length	26
10515690669	When is the focal length of the lens positive/negative	positive= converging negative= divergine	27
10515690670	When is object distance positive/negative	positive= on the side where light is coming from negative= on the opposite side	28
10515690671	When is image distance positive/negative	Positive= opposite side of the lens from light Negative= same side	29
10515690672	Lateral magnification	m=hi/ho= -di/do	30
10515690673	Power of a lense	P=1/focal length	31
10515690674	Focal length of a spherical mirror	f=1/2 of the radius of curvature	32
10515690675	Power (kinematics)	Power=work/time=Force x velocity	33
10515690676	centripetal acceleration	acceleration= velocity^2/r	34
10515690677	Work (rotation)	Work= torque x change in angular displacement	35
10515690698	Conservation of angular momentum		36
10515690699	Speed of a wave on a stretched string		37
10515690700	Speed of sound		38
10515690701	Frequency and period		39
10515690702	Frequency and angular velocity of a mass spring		40
10515690703	Frequency and angular velocity of a pendulum		41
10515690704	Four expressions for the density of water		42
10515690705	SI unit for pressure		43
10515690706	Relationship between pressure and depth		44
10515690707	Archimedes principle		45
10515690678	Displacement as a function of time	x= vot + xo + 1/2at^2	46
10515690679	Velocity of a ball you dropped from a building	v= square root(2gh)	47
10515690680	Velocity in the x or y direction	Vx= vcos(theta) Vy=vsin(theta)	48
10515690681	Force of static friction	Force is less than or equal to the coefficient of static friction times the normal force	49
10515690682	Force on an inclined plane	F=mgsin(theta)	50
10515690683	Impulse	I=force x change in time= mv	51
10515690684	Work done by constant force	W=fdcos(theta)	52
10515690685	Sound decibels	B=10log(Io/I)	53
10515690686	Beat frequency	Fb= f2-f1	54
10515690687	Electric force	Kq1q2/r^2	55
10515690688	Speed of light	c=E/B	56
10515690689	Energy of a photon	E=hv/wavelength	57
10515690690	Resistance of a wire	density(L/A)	58
10515690691	sin(30)	.5	59
10515690692	cos(30)	.886	60
10515690693	sin(60)	.886	61
10515690694	cos(60)	.5	62
10515690695	tan(30)	.577	63
10515690696	tan(45)	1	64
10515690697	tan(60)	1.7 (square root of 3 over 1)	65
10515690709	Wave Speed	v = F * Lambda(wavelength)	66
10515690710	Average speed	total distance / time	67
10515690711	MOTION formula 1 without a	displacement = 1/2(Vo + V)t	68
10515690712	MOTION formula 2 without v	displacement = Vot + 1/2at^2	69
10515690713	MOTION formula 3 without Vo	displacement = vt - 1/2at^2	70
10515690714	MOTION formula 4 without displacement	V = Vo + at	71
10515690715	MOTION formula 5 without	V^2 = Vo^2 +2a(displacement)	72
10515690716	Newtons second law	F = ma	73
10515690717	strength of Gravitational Force	F = G * (M1*M2/r^2)	74
10515690718	Weight	Fg = g * m	75
10515690719	PE	mgh	76
10515690720	KE	1/2 mv	77
10515690721	Power	Work/Time	78
10515690722	Conversion of Mechanical Energy	K1 + U1 = Kf + Uf	79
10515690723	Impulse	Average Force * time	80

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AP US History Decades Review Flashcards

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8045232540	1491 - 1607	Discovery of America, Christopher Columbus, Columbian Exchange, Conquistadors, Encomienda system, Diseases	0
8045232541	1607 - 1700	Jamestown, Chesapeake Colonies, New England Colonies, Middle Colonies, Slave trade, indentured servants, Puritans, House of Burgesses, Pilgrims-Mayflower Compact, 1676/ Bacon's Rebellion, Salem Witch Trials, Tobacco	1
8045232542	1700 - 1750	The First Great Awakening, Enlightenment, Stono Rebellion	2
8045232543	1760s	Stamp Act, Proclamation of 1763, Townshend Acts, Pontiac's Rebellion	3
8045232544	1770s	Common Sense, Declaration of Independence, The Townsend Acts, The Continental Congress appointed George Washington, American Revolution	4
8045232545	1780s	Constitution ratified, Shays Rebellion, Land ordinances - western settlement, Federalists vs Antifederalists, First us president (washington)	5
8045232546	1790s	Bank of the United States, Report on Manufactures, Washington's neutrality proclamation, Jay's Treaty, Whiskey Rebellion, Inauguration of John Adams, XYZ affair, Alien and Sedition Acts, John Fries's Rebellion	6
8045232547	1800s	United States Presidential Election, The Michigan Territory, The Illinois Treaty , Louisiana purchase	7
8045232548	1810s	Panic of 1819, The American System, War of 1812	8
8045232549	1820s	The Second Great Awakening, Missouri Compromise, Monroe Doctrine, Andrew Jackson elected president	9
8045232550	1830s	Indian Removal Act, Worcester v Georgia, Nat Turner's Rebellion, Nullification Crisis, Bank War, Trail of Tears	10
8045232551	1840s	Mexican-American War, Free Soil Party, Treaty of Guadalupe Hidalgo, Seneca Falls Convention, Wilmot Proviso	11
8045232552	1850s	Bleeding Kansas, Compromise of 1850, Kansas-Nebraska Act, Dred Scott Decision, Fugitive Slave Act	12
8045232553	1860s	Civil War, Emancipation Proclamation, President McKinley assassinated, Homestead Act, Reconstruction, Radical Republicans, KKK, 13th and 14th amendments, Civil Rights Act	13
8045232554	1870s	15th Amendment, Compromise of 1877	14
8045232555	1880s	Sitting Bull imprisoned, Civil Service Act, Elk v. Wilkins, Haymarket affair, Wabash v. Illinois, Statue of Liberty dedicated, Dawes Act, Interstate Commerce Commision created	15
8045232556	1890s	Wounded Knee Massacre, Plessy v. Ferguson, President McKinley, US gains Puerto Rico, Guam, the Philippines and Cuba following the Spanish-American war	16
8045232557	1900s	The Platt Amendment, Cuban Independence, Roosevelt President, William Taft President, The Pure Food and Drug Act and the Meat Inspection Act is passed	17
8045232558	1910s	WW1, Sixteenth Amendment Ratified, Seventeenth Amendment Ratified, Federal Reserve Established, Clayton Act, Lusitania sinks, Zimmerman Telegram, Espionage Act, "Fourteen Points", Red Scare, 18th Amendment	18
8045232559	1920s	Prohibition, Stock market crash , Flappers (rebellion) , Scopes Trial, ERA, Women gain the right to vote(19th amendment)	19
8045232560	1930s	FDR, New Deal, End of Prohibition, The Dust Bowl, Social Security, GD	20
8045232561	1940s	WWII, FDR still president, D-Day, First Atomic Bomb testing, Pearl Harbor, Hiroshima and Nagasaki Atomic bombs, Jackie Robinson, Marshall Plan, NATO	21
8045232562	1950s	Baby Boomers, Beat Generation, Sputnik, Ethel and Julius Rosenberg, Korean War, Desegregation of public schools	22
8045232563	1960s	Cold War Continuation, LBJ, Kennedy Years, Great Society, Woodstock, Space race, bay of pigs invasion	23
8045232564	1970s	Carter Administration, Roe v Wade, Feminist Movement, Stagflation, Vietnam War	24
8045232565	1980s	Triumph of conservatism, Title IX, Ronald Reagan	25
8045232566	1990s	Bill Clinton, End of Soviet Union, NAFTA, OKC bombing, Computer revolution, rapid globalization, Multiculturalism, unprecedented diversity	26
8045232567	2000s	George Bush Elected President, 9/11, No Child Left, Behind Act, USA Patriot Act, Department of Homeland Security Established, Obama elected	27
8045232568	2010s	Obama Administration, Mobilization of Tea Party, Gay marriage legalized	28

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AP Chemistry Flashcards

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13906489454	Oxidation	loss of electrons	0
13906489455	Reduction	gain of electrons	1
13906498904	Oxide	a binary compound of oxygen with another element or group.	2
13906504333	Oxidizing agent	electron acceptor	3
13906507347	Reducing agent	electron donor	4
13906516611	Strong Acids	HCl, HBr, HI, HNO3, H2SO4, HClO4	5
13906520013	Strong bases	1A and heavy 2A hydroxides	6
13906546900	gas forming reactions	H2CO3 -> H2O + CO2 S + H2 -> H2S(g)	7
13906557366	Electrolyte	dissociates	8
13906562144	strong electrolyte	dissociates completely	9
13906566466	weak electrolyte	partially dissociate	10
13906577040	Periodicity	the repeating pattern of chemical and physical properties of the elements	11
13906577042	Coulombs Law	F=K q₁*q₂/r²	12
13906585298	Zeff (effective nuclear charge)	Z (Atomic #) - S (Screening constant = #inner electrons)	13
13906602440	Size of Atom trend	Increases down and left (Zeff increases)	14
13906614909	Size of ions	- Cations are smaller than original atom - Anions are larger - Ion size increases down a group - From left to right they get smaller (because nuclear charge increases), then suddenly larger (once it changes from cations to anions)	15
13906620512	Ionization energy	The amount of energy required to remove an electron from an atom	16
13906625198	Ionization energy trend	increases up and to the right	17
13906635480	Smaller atoms have ___ ionization energies	higher	18
13906642143	electron affinity	the energy change that occurs when an electron is acquired by a neutral atom	19
13906646192	electron affinity trend	increases to the right and up	20
13906655655	lattice energy	the energy released when one mole of an ionic crystalline compound is formed from gaseous ions	21
13906657346	Lattice energy trend	increases up and to the right	22
13906660713	Electronegativity	A measure of the ability of an atom in a chemical compound to attract electrons	23
13906660715	electronegativity trend	increases up and to the right	24
13906667326	Lewis dot structure steps		25
13906698255	free radicals	chemical particles with an odd number of electrons	26
13906700408	Hypervalent	molecules and ions with more than an octet of electrons around the central atom	27
13906702753	electron domain	in the VSEPR model, a region about a central atom in which an electron pair is concentrated	28
13906706501	Kinetic Molecular Theory of Gases	1. gases made up of negligible volume 2. no intermolecular attractions/repulsions 3. elastical collisions 4. constant random motion 5. kinetic energy of gas is related to T 6. same moles of gas=same kinetic energy	29
13906738308	Celcius to Kelvin	K=C+273	30
13906742475	van der Waals equation	[P+(an^2)/(V^2)][V-nb]=nRT a = strength of attraction b = Size of molecule	31
13906756410	Real Gas Law	Real gasses only conform to PV=nRT at Low pressures High temps	32
13906774475	Effusion	A process by which gas particles pass through a tiny opening	33
13906776273	Diffusion	Movement of molecules from an area of higher concentration to an area of lower concentration.	34
13906780719	Kinetic energy of gas	KE=1/2mv^2 Same Temp - KE = KE	35
13906789700	Grams law of effusion		36
13906803854	van der Waals forces	a slight attraction that develops between the oppositely charged regions of nearby molecules	37
13906808402	London dispersion forces	- Attractions between momentary dipole - All molecules - Polarizability	38
13906823114	London Dispersion forces are effected by...	Usually Weak Shape - Long skinny have stronger Weight - Increases with molecular weight. Larger clouds are easier to polarize	39
13906832748	dipole-dipole forces	attractions between oppositely charged regions of polar molecules	40
13906837310	dipole-dipole forces are effected by...	Polarity - Increases with increase in polarity	41
13906856563	Hydrogen Bonding	Very Strong Dipole-Dipole interaction with H + N, O, or F	42
13906867447	Viscosity	resistance to flow	43
13906868963	surface tension	A measure of how difficult it is to stretch or break the surface of a liquid	44
13906868964	Vapor Pressure	- As temp rises, the fraction of molecules having enough energy to escape increases - Pressure increase	45
13906905665	Boiling poing	When its Vapor pressure = Atmospheric Pressure	46
13906908591	Normal Boiling Point	The T that VP is 760 torr or 1 ATM	47
13906914380	Heat of fusion	Amount of energy required to change a substance from the solid phase to the liquid phase.	48
13906914381	heat of vaporization	The amount of energy required for the liquid at its boiling point to become a gas	49
13906916823	Triple Point	3 phases coexist	50
13906923821	rate of reaction depends on	Catalyst Higher Temp Concentration Homogeneous mixture	51
13906933541	Reaction rate equation (change in concentration	-Δ[A]/Δt = Δ[B]/Δt	52
13906942699	steric factor	Size + Orientation	53
13906950394	Rate Equation	rate = K[A]^a[B]^b	54
13923106378	Activated complex	a transitional structure that results from an effective collision and that persists while old bonds are breaking and new bonds are forming	55
13923112000	Maxwell-Boltzmann distribution	The distribution of energies (and therefore speeds) of the molecules in a gas or liquid.	56
13923138907	Arrhenius equation	K=Ae^(-Ea/RT) k is the rate constant A is pre-exponential factor: how often particles collide in correct orientation.	57
13923212924	reaction mechanism	the step-by-step sequence of reactions by which the overall chemical change occurs	58
13923222789	elementary reaction	a reaction in which reactants are converted to products in a single step	59
13923240000	molecularity	the number of molecules that participate as reactants in an elementary reaction	60
13923245948	rate law and order for elementary reactions is determined by	Coefficients	61
13923295642	Kp to Kc	Kp = Kc(RT)^delta n	62
13923303754	Kp = Kc when	there are the same number of moles of gas on each side of the equation	63
13923308986	Keq > 1	products are favored	64
13923311526	Keq < 1	reactants favored	65
13923330309	k = q when	System is in equilibrium	66
13923339118	Equilibrium Quotient	Q = [Products]/[Reactants]	67
13923905469	Q > K	shift left	68
13923908069	Q < K	shift right	69
13923917227	Amphiprotic	A species that can either accept or donate a proton.	70
13923917228	Amphoteric	a substance that can act as both an acid and a base	71
13923930504	Kw	1.0 x 10^-14	72
13923930505	pH	= -log[H+]	73
13923944849	% Ionization	[H3O+eq]/[HAinitial] x 100	74
13923964716	Ka	acid dissociation constant	75
13923964717	Kb	base dissociation constant	76
13923972850	Higher Kb	stronger base	77
13923972851	Lower Ka	weaker acid	78
13923975356	Higher Ka	stronger acid	79
13923975357	Lower Kb	weaker base	80
13923981939	polyprotic acid	an acid that can donate more than one proton per molecule	81
13923987418	Ka * Kb	Kw	82
13923991850	pH + pOH =	14	83
13923991852	pKa + pKb =	pKw = 14	84
13924011211	Factors affecting acid strenght	- Polarization of Hx bond - Stronger bond = weaker acid - Less stability = weaker acid	85
13924023595	If x is in same group bond strenght is _ important	more	86
13924048284	If x is in the same period, bond polarity is _ important	more	87
13924059537	Carboxilic Acid	COOH	88
13924078269	Carboxilic Acids draw ___ from ___ Increase ___ of bond Increases ____	- Electron density, OH bond - Polarity - Acidity	89
13924094001	Bottom Line of acid strenght	Anything that pulls electrons away from the ionizable hydrogen (making a weaker bond) makes the acid more acidic	90
13924113626	common ion effect	a decrease in the solubility of an ionic compound caused by the addition of a common ion	91
13924116202	Buffer	compound that prevents sharp, sudden changes in pH	92
13924119509	Henderson-Hasselbalch equation	pH = pKa + log [A-]/[HA]	93
13924124516	Strong acid-strong base titration curve	equivalence point: pH=7	94
13924134039	Weak acid-strong base titration curve	Equivalence point is greater than 7, has a halfway equivalence point	95
13924144006	strong acid weak base titration	Slow decline in pH followed by a rapid decrease at equivalence point. End point of indicator should be < 7.	96
13924196420	Ksp =	[prodA][prodB] (the bigger, the more soluble)	97
13924207529	Heat up and cool down	q = mc{delta}t	98
13924216368	Phase Change	q = n{delta}h fus/vap	99
13924230060	Hess's law	the overall enthalpy change in a reaction is equal to the sum of enthalpy changes for the individual steps in the process	100
13924238421	calorimetry equation	mcdeltaT=mcdeltaT	101
13924286760	deltaSsurr=	-deltaH/T	102
13924300068	Oxidation occurs at the	anode	103
13924302664	Reduction occurs at the	cathode	104
13924307321	electromotive force (emf)	The power supplied by the supply per unit current.	105
13924328654	A stronger oxidizing agent exhibits more _______	Positive reduction potential	106

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13722069404	atomic number	number of electrons/protons in the atom	0
13722069405	molar mass	average mass of a single atom measured in amus; also the average mass for one mole of the atom in grams	1
13722069406	periods	horizontal rows	2
13722069407	groups	vertical rows	3
13722069408	alkali metals	G1 elements	4
13722069409	alkaline earth metals	G2 elements	5
13722069410	transition metals	G3 through G12	6
13722069411	halogens	G17	7
13722069412	noble gases	G18	8
13722069413	lanthanides and actinides	rare earth elements; inner transition metals	9
13722069414	proton	positively charged particle in the nucleus; # of which determines the properties of an element	10
13722069415	neutron	neutral particles in the nucleus of an atom	11
13722069416	electron	small, negatively charged particle surrounding an atom in orbitals	12
13722069417	mass number	sum of protons and neutrons	13
13722069418	isotope	element with a different number of neutrons	14
13722069419	mass spectrometry	mass of various isotopic elements to create a mass spectrum graph	15
13722069420	mole	unit used to represent large numbers of small particles such as atoms, molecules, electrons, or ions	16
13722069421	avogadros number	6.022 E23	17
13722069422	ideal gas law	pv=nrt	18
13722069423	? L/mol	22.4 L	19
13722069424	percent composition	percent by mass of each element that makes up a compound; mass part/mass whole	20
13722069425	empirical formula	simplest ratio of the molecules making up a compound	21
13722069426	molecular formula	actual formula for a substance	22
13722069427	aufbau principle	e- are placed in orbitals, subshells, and shells in order of increasing energy	23
13722069428	quantized	e- can only exist at specific energy levels separated by specific intervals	24
13722069429	pauli exclusion principle	two electrons who share an orbital cannot have the same spin (must be clockwise and counterclockwise); magnetic moment	25
13722069430	hunds rule	when an electron is added to a subshell it will always occupy an empty orbital if one is available	26
13722069431	coulombs law	the amount of energy that an electron has depends on its distance from the nucleus of an atom; e=k(q1*q20)/r	27
13722069432	quantum theory	electromagnetic energy is quantized; for a given frequency of light or radiation, all possible energies are multiples of a certain unit (a quantum)	28
13722069433	quantum energy equation	e=hv	29
13722069434	bohr model	each energy level is represented by a row in the periodic table	30
13722069435	electromagnetic radiation	the form in which atoms absorb energy	31
13722069436	when electron drops to a lower energy level	then electromagnetic radiation is released (energy)	32
13722069437	frequency and wavelength are	inversely proportional; c=hv	33
13722069438	ionization energy	amount of energy necessary to remove electrons from an atom (electromagnetic energy exceeds binding energy)	34
13722069439	unit for binding energy	kj/mol or Mj/mol	35
13722069440	kinetic energy	energy of motion	36
13722069441	photoelectron spectra (pes)	charted amounts of ionizations energies for electrons ejected from a nucleus; can be used to identify elements	37
13722069442	ion	an atom which has either gained or lost electrons	38
13722069443	anion	particle with more electrons than protons; negatively charged	39
13722069444	cation	particle with less electrons than protons; positively charged	40
13722069445	dalton	modern atomic theory; elements combined in different ratios; are never created nor destroyed in chemical reactions	41
13722069446	mendeleev & meyer	independent proposals of early periodic tables	42
13722069447	thomsons experiment	cathode ray tube; deflection of charges that concluded atoms are composed of positive and negative particles	43
13722069638	plum pudding model		44
13722069448	millikans experiment	calculated charge on an electron by examining the behavior of charged oil drops in an electric field	45
13722069449	rutherfords experiment	fired alpha particles at gold foil and observed how they scattered; concluded that all of the positive charge was concentrated in the center and that an atom is mostly empty space	46
13722069450	heisenberg uncertainty principle	it is impossible to know both the position and momentum of an electron at a particular instant; means electron orbitals do NOT represent specific orbits	47
13722069451	shielding electrons	electrons between a valence electron and the nucleus that decreases the attraction between the nucleus and the valence electron	48
13722069452	stable atoms have	... completed shells	49
13722069639	metalloids		50
13722069453	atomic radius	approximate distance from the nucleus of an atom to its valence electrons	51
13722069454	periodic trend: left to right	periodic trend: atomic radius decreases; protons are added to the nucleus so valence electrons are more strongly attracted ionization energy increases (protons are added to the nucleus)	52
13722069455	periodic trend: down a group	periodic trend: atomic radius increases; shells of electrons are added which shield the more distant shells and valence e- get farther away ionization energy decreases (shells of e- added, each inner shell shields more and reduces the pull on valence e- so they are easier to remove)	53
13722069456	periodic trend: cations	periodic trend: ... are smaller than atoms; e- is removed and a shell is lost and electron-electron repulsions are reduced	54
13722069457	periodic trend: anions	periodic trend: ... are larger than atoms; e- is added, electron-electron repulsions increase and valence electrons move farther apart	55
13722069458	ionization energy magnitudes	subsequent energies are larger because the e-e repulsion decreases and the remaining valence e- are closer to the nucleus; once a shell is empty the energy required to remove an e- from a full shell is significantly greater than previous energies	56
13722069459	electronegativity	how strongly the nucleus of an atom attracts the electrons of other atoms in a bond	57
13722069460	factors that affect electronegativity	smaller atom; greater EN closer the element is to having a full energy level; higher EN	58
13722069461	EN trends	left to right; EN increases down a group; EN decreases	59
13722069462	bonding	transfer or sharing of electrons	60
13722069463	ionic solid	compound held together by electrostatic attractions that are in a lattice structure; weak conductors (e- are localized around a single atom); no IMFs	61
13722069464	ionic bond	bond between metal and nonmetal; electrons are NOT shared: the cation gives an e- up to the anion	62
13722069465	properties of ionic solids	are solid at room temperature; high melting and boiling points	63
13722069466	2 factors that affect melting points in ionic substances	primary factor: charge on the ions (greater charges, greater Coulombic attraction) secondary factor: smaller atoms (greater Coulombic attraction)	64
13722069467	salts have __________ bonding	ionic bonding	65
13722069468	metallic bonding	bond between two metals; sea of electrons that make metals such good conductors; delocalized structure allows for malleability and ductility	66
13722069469	interstitial alloy	metal atoms with vastly different radii combine; ex. steel	67
13722069470	substitutional alloy	metal atoms with similar radii combine; ex. brass	68
13722069471	covalent bonds	bond in which two atoms share electrons; each atom counts the e- as a part of its valence shell	69
13722069472	single bonds	one sigma bond, one e- pair; longest bond, least energy	70
13722069473	double bonds	one sigma bond, one pi bond; two e- pairs	71
13722069474	triple bonds	one sigma bond, two pi bonds; 3 e- pairs; shortest bond, most energy	72
13722069475	network covalent bonds	lattice of covalent bonds; network solid (acts similar to one molecule); very hard, high melting/boiling points; poor conductors	73
13722069476	the common network solids	SiO2,	74
13722069477	doping	the addition of an impurity to an existing lattice	75
13722069478	p-doping	create a hole (positively charged) that draws electrons through the substance (add a substance with one LESS valence e-) i.e. si + al	76
13722069479	n-doping	add a substance with one MORE valence e- which leaves a free e- to travel freely i.e. si + p	77
13722069480	polarity	exists when a molecule has a clustering of negative charge on one side due to unequal sharing of electrons (e- are pulled to the more electronegative side); creates dipoles in molecules	78
13722069481	dipole moment	the measurement of the polarity of a molecule; the unit of measurement is a debye (D)	79
13722069482	more polar molecule....	.... larger dipole moment	80
13722069483	intermolecular forces (IMFs)	forces that exist between molecules in a covalently bonded substance; not bonds	81
13722069484	dipole-dipole forces	the positive end of one polar molecule is attracted to the negative end of another molecule; relatively weak attraction force	82
13722069485	hydrogen bonding	strong IMF between two moelcules; F, O, N; have higher melting and boiling points than molecules with other IMFs	83
13722069486	london dispersion forces	IMFs that occur between all molecules; occur because of the random motions of electrons on atoms within molecules to create instantaneous polarities; molecules with more e- will have greater _________________ forces	84
13722069487	substances with only london dispersion forces usually...	... are gases at room temp, and boil/melt at extremely low temps	85
13722069488	melting & boiling points of a covalent substance is almost always _____________ than that of ionic substances	lower	86
13722069489	vapor pressure	the pressure exerted by a vapor over a liquid	87
13722069490	vaporization	the process by which molecules with enough KE inside a liquid break the surface of the liquid and transition into the gaseous phase; no outside energy is needed i.e. no heating	88
13722069491	vapor pressure is primarily dependent on	dependent on IMFs	89
13722069492	resonance structures	structures that occur when it is possible to draw two or more valid lewis electron dot diagrams that have the same number of electron pairs for a molecule or ion	90
13722069493	formal charge	used to find which structure is most likely to occur; valence - assigned	91
13722069494	assigned e-	lone pairs of e- count as two and bonds count as one	92
13722069495	valence shell electron-pair repulsion model (VSEPR)	model used to predict molecular geometry based on the principle that electrons repel each other and therefore are as far apart as possible in a structure	93
13722069496	hybrid orbitals	orbitals that have the properties to explain the geometry of bonds between atoms	94
13722069497	linear geometry	sp hybridization 0 lone pairs ex. BeCl2 & CO2	95
13722069498	trigonal planar geometry	sp2 hybridization bond angles 120 0 lone pairs: trigonal planar (three bonds) 1 lone pair: bent (two bonds)	96
13722069499	tetrahedral geometry	4 e- pairs, sp3 hybridization angles 109.5 0 lone pairs: tetrahedral (four bonds) [CH4, NH4+, ClO4-, SO4 2-, PO4 3-] 1 lone pair: trigonal pyramidal (3 bonds) [NH3, PCl3, SO3 2-] 2 lone pairs: bent (2 bonds) [H2O, OF2, NH2-]	97
13722069500	trigonal bipyramidal geometry	5 e- pairs, sp4 hybridization 0 lone pairs: trigonal bipyramidal (5 bonds) [PCl5, PF5] 1 lone pair: seesaw (4 bonds) [SF4, IF4+] 2 lone pairs: t-shaped (3 bonds) [ClF3, ICl3] 3 lone pairs: linear (2 bonds) [XeF2, I3-]	98
13722069501	octahedral geometry	6 e- pairs, sp5 hybridization 0 lone pairs: octahedral (6 bonds) [SF6] 1 lone pair: square pyramidal (5 bonds) [BrF5, IF5] 2 lone pairs: square planar (4 bonds) [XeF4]	99
13722069502	kinetic molecular theory	the theory that all matter is composed of particles (atoms and molecules) moving constantly in random directions	100
13722069503	KE=0.5mv^2	average kinetic energy of a single gas molecule (ideal gas)	101
13722069504	ideal gas	(gas) high temperature, low pressure, no attractive forces, in constant motion without losing energy	102
13722069505	maxwell-boltzmann diagrams	shows the range of velocities for molecules of a gas	103
13722069506	effusion	the rate at which a gas will escape from a container through microscopic holes in the surface of the container	104
13722069507	factors that affect rate of effusion	speed of gas molecules (so ________ increases with higher temperature and lower mass)	105
13722069508	combined gas law	(P1V1)/T1=(P2V2)/T2	106
13722069509	boyles law	if temperature is constant: as pressure increases, volume decreases as volume increases, pressure decreases	107
13722069510	charles law	if pressure is constant: as temp increases, volume increases	108
13722069511	if volume is constant:	as pressure increases, temperature increases	109
13722069512	daltons law	the total pressure of a mixture of gases is just the sum of all the partial pressures of the individual gases in the mixture	110
13722069513	partial pressure	the pressure of each gas in a mixture; is directly proportional to the number of moles of gas in the mixture Pa = (Ptotal) (moles of A/total moles)	111
13722069514	molarity	the concentration of a solution in terms of moles of solution/volume (L)	112
13722069515	mole fraction	moles of substance/total moles in solution	113
13722069516	solute	substance being dissolved	114
13722069517	solvent	a liquid substance capable of dissolving other substances	115
13722069518	dissociation	when ionic substances break up into ions into solution	116
13722069519	electrolytes	free ions in solution that conduct electricity	117
13722069520	paper chromatography	the separation of a mixture by passing it through a medium in which the components of the solution move at different rates	118
13722069521	retention factor	stronger the attraction between the solute and the solvent front is, the larger the Rf value will be	119
13722069522	column chromatography	a column is packed with stationary substance, then the solution to be separated (analyte) is injected into the column where it adheres to the stationary phase, then the eluent solution is injected into the column. as the eluent solution passes through the stationary phase the analyte molecules will be attracted to it with varying degrees of strength based on polarity	120
13722069523	distillation	the process that separates the substances in a solution based on their boiling points	121
13722069524	salt	an ionic compound made from the neutralization of an acid with a base	122
13722069525	synthesis reaction	when elements or simple compounds are combined to form a single, more complex compound	123
13722069526	decomposition reaction	a reaction where a single compound os split into two or more elements or simple compounds, usually in the presence of heat; opposite of a synthesis	124
13722069527	acid-base reaction	a reaction when an acid reacts with a base to form water and a salt	125
13722069528	oxidation-reduction reaction	a reaction that results in the change of the oxidation states of some participating species	126
13722069529	hydrocarbon combustion	hydrocarbon + oxygen --> carbon dioxide + water a substance is ignited (usually a hydrocarbon) and it reacts with oxygen in the atmosphere; products are always CO2 and H2O	127
13722069530	precipitation reaction	a reaction in which an insoluble substance (salt) forms and separates from the solution	128
13722069531	net ionic equation	an equation for a reaction in solution showing only those particles that are directly involved in the chemical change	129
13722069532	limiting reactant	the substance that controls the quantity of product that can form in a chemical reaction; moles of each reactant divided by moles used in reaction	130
13722069533	hydrocarbon	an organic compound composed only of carbon and hydrogen	131
13722069534	law of conservation of mass	matter can be neither created nor destroyed during a chemical reaction	132
13722069535	gravimetric analysis	a type of quantitative analysis in which the amount of a species in a material is determined by converting the species to a precipitate that can be isolated completely and weighed	133
13722069536	when bonds are formed	...energy is released	134
13722069537	when bonds are broken	...energy is absorbed	135
13722069538	exothermic	products have stronger bonds than the reactants; heat is released, - ΔH	136
13722069539	endothermic	reactants have stronger bonds than the products; heat is absorbed, + ΔH	137
13722069540	activation energy	the minimum amount of energy required to start a chemical reaction	138
13722069541	catalyst	substance that speeds up a reaction by reducing the activation energy required by the reaction; provides an alternate reaction pathway; no effect on equilibrium conditions	139
13722069542	oxidation number: H	+1	140
13722069543	oxidation number: alkali metals	+1	141
13722069544	oxidation number: alkaline earth metals	+2	142
13722069545	oxidation number: oxygen	-2	143
13722069546	oxidation number: halogens	-1	144
13722069547	hydroxide	OH-	145
13722069548	nitrate	NO3-	146
13722069549	acetate	C2H3O2-	147
13722069550	cyanide	CN-	148
13722069551	permanganate	MnO4-	149
13722069552	carbonate	CO3 2-	150
13722069553	sulfate	SO4 2-	151
13722069554	dichromate	Cr2O7 2-	152
13722069555	phosphate	PO4 3-	153
13722069556	ammonium	NH4+	154
13722069557	half-reactions	the two parts of an oxidation-reduction reaction, one representing oxidation, the other reduction	155
13722069558	titration	the slow addition of a solution at a known concentration to another solution in order to determine the concentration of the unknown solution; color change is often used as an end point	156
13722069559	galvanic (voltaic) cell	a favored redox reaction in a cell is used to generate an electric current	157
13722069560	current	unit: amperes (amps); the flow of electrons from one place to another	158
13722069561	anode	where oxidation takes place	159
13722069562	cathode	where reduction takes place	160
13722069563	electrolyctic cell	an outside source id used to force an unfavored redox rxn to take place	161
13722069564	purpose of a salt bridge	maintains electrical neutrality in the cell	162
13722069565	favored redox reaction	+E	163
13722069566	unfavored redox reaction	-E	164
13722069567	elecroplating	a process that uses electric current to reduce dissolved metal cations so that they form a thin metal coating on an electrode	165
13722069568	rate law	an expression relating the rate of a reaction to the concentration of the reactants	166
13722069569	first order rate law	y= ln[a] subscript (t) m= -k x= time b= ln[a] subscript (0)	167
13722069570	half-life	the amount of time it takes for half of a sample to disappear; t1/2=0.693/k	168
13722069571	second order rate law	[a] sub. (t) = concentration of reactant A at time (t) [a] sub. (0) = initial conc. of A k = rate constant t = time elapsed	169
13722069572	zero order rate laws	rate does not depend on the concentration of the reactants at all therefore rate is always the same at a given temperature; rate=k	170
13722069573	collision theory	theory that collisions occur because reactants are constantly moving around and colliding with one another	171
13722069574	effective collisions	collisions in which the conditions of the collision theory are met (and therefore the reaction occurs)	172
13722069575	ineffective collisions	collisions in which the conditions of the collision theory are not met (and therefore reaction does not occur)	173
13722069576	spectrophotometer	an instrument that measures the proportions of light of different wavelengths absorbed and transmitted by a pigment solution	174
13722069577	beer's law	A=abc A=absorbance a=molar absorptivity b=path length; the distance the light is traveling through the solution c=concentration of the solution	175
13722069578	rate-determining step	the slowest step in a reaction mechanism that determines the overall rate of the reaction	176
13722069579	elementary steps	a series of simple reactions that represent the progress of the overall reaction at the molecular level	177
13722069580	work	force exerted on an object that causes it to move	178
13722069581	first law of thermodynamics	the energy of the universe is constant	179
13722069582	second law of thermodynamics	if a process is favored in one direction, then it cannot be favored in the reverse reaction; and an increase in entropy promotes favored reactions	180
13722069583	entropy	ΔS; a measure of the randomness or disorder of the system	181
13722069584	enthalpy	ΔH; heat of a system at constant pressure	182
13722069585	Gibbs free-energy	ΔG; a measure of whether or not a process will proceed without the input of outside energy ∆G=∆H-T∆S (T in degrees Kelvin) when ΔG=0, the reaction is at equilibrium	183
13722069586	state functions	functions that depend only on the change between the initial and final states of a system and therefore independent of the reaction pathway (catalyst has no effect) ΔS, ΔH, ΔG	184
13722069587	standard state conditions	all gases are 1 atm all liquids are pure all solids are pure all solutions are 1 molar the energy of formation of an element in its normal state is defined as zero the temperature used is 25C or 273K	185
13722069588	ΔH°f (heat of formation)	the change in energy that takes place when one mole of a compound is formed from its pure components under STP	186
13722069589	STP	standard temp. and pressure	187
13722069590	bond energy	the energy required to break a bond; endothermic process (add energy)	188
13722069591	hess's law	if a reaction can be described by a series of steps, then ΔH for the overall reaction is the sum of the ΔH values for all the steps	189
13722069592	rules of hess's law	1. if you flip the equation, flip the sign on ΔH 2. if you multiply or divide an equation by a #, multiply ΔH by the same # 3. if several equations in summation create a new equation, you can also add the ΔH values of those component equations to get the ΔH value for the new equation	190
13722069593	enthalpy of solution	the amount of energy released or absorbed as heat when a specific amount of solute dissolves in a solvent	191
13722069594	solid to liquid	melting	192
13722069595	liquid to solid	freezing	193
13722069596	liquid to gas	vaporization	194
13722069597	gas to liquid	condensation	195
13722069598	solid to gas	sublimation	196
13722069599	gas to solid	deposition	197
13722069600	heat of fusion	the energy that must be absorbed by a solid to melt it	198
13722069601	heat of vaporization	the energy that must be put into a liquid to turn it into a gas	199
13722069640	phase diagram (water)		200
13722069602	calorimetry	the measurement of heat changes during chemical reactions	201
13722069603	specific heat	the amount of heat required to the temperature of one gram of a substance by one degree celsius	202
13722069604	heating/cooling curves	curves that display what happens to the temperature of a substance as heat is added	203
13722069605	spontaneous	thermodynamically favored; -ΔG	204
13722069606	nonspontaneous	thermodynamically unfavored; +ΔG	205
13722069607	at low temperature	enthalpy is dominant; ΔH	206
13722069608	at high temperature	entropy is dominant; ΔS	207
13722069609	voltage vs favorability	a redox reaction is favored if voltage is (+)	208
13722069610	hydration energy	the energy required to break hydrogen bonds	209
13722069611	law of mass action	the rate of a chemical reaction is proportional to the product of the concentrations of the reactants	210
13722069612	a solution is at equilibrium when	the rate of the forward reaction is equal to the rate of the reverse reaction	211
13722069613	large k eq value	products are favored at equilibrium	212
13722069614	small k eq value	reactants are favored at equilibrium	213
13722069615	le chateliers principle	states that if a stress is applied to a system at equilibrium, the system shifts in the direction that relieves that stress	214
13722069616	reaction quotient	Q	215
13722069617	Q > K	precipitate forms; reaction shifts left	216
13722069618	Q < K	precipitate does not form; reaction shifts right	217
13722069619	Q = K	the reaction is at equilibrium; voltage in a voltaic cell reaches zero	218
13722069620	common ion effect	a decrease in the solubility of an ionic compound caused by the addition of a common ion	219
13722069621	Arrhenius acids	a substance that ionizes in water and produces hydrogen ions	220
13722069622	Arrhenius bases	a substance that ionizes in water and produces hydroxide ions	221
13722069623	Brønsted-Lowry acids	a substance that is capable of donating a proton	222
13722069624	Brønsted-Lowry bases	a substance that is capable of accepting a proton	223
13722069625	pH	-log [H+]	224
13722069626	pOH	-log [OH-]	225
13722069627	pKa	-log [Ka]	226
13722069628	pKb	-log [Kb]	227
13722069629	amphoteric	a substance that can act as both an acid and a base; ex. H2O	228
13722069630	strong acids	dissociate completely in water; reaction goes to completion and never reaches equilibrium	229
13722069631	weak acid	most of the acid molecules remain in solution and very few dissociate	230
13722069632	percent dissociation	the ratio of the amount of a substance that is dissociated at equilibrium to the initial concentration of the substance in a solution, multiplied by 100	231
13722069633	oxoacids	acids that contain oxygen; the more oxygens, the stronger the acid	232
13722069634	polyprotic acids	acids that can donate more than one H+	233
13722069635	Kw	1.0x10^-14	234
13722069636	henderson hasselbach	pH = pKa + log([A-]/[HA])	235
13722069637	buffers	weak acids or bases that can react with strong acids or bases to prevent sharp, sudden changes in pH	236

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14322669041	Phagocytosis	defend body against bacteria neutrophils ingest invading pathogens	0
14322683068	chemotaxis	neutrophils are attracted to bacterial chemical products	1
14322692406	Diapedesis	process by which wbc travel through capillaries to fight off infection	2
14322697038	hemophilia	coagulation factor deficiency	3
14322745294	Neutrophils	50-70% phagocytize bacteria	4
14322759249	Eosinophils	2-4% attack parasite worms	5
14322763277	basophils	.5- 1 percent heparin- anticoagulant	6
14322769798	Monocytes	3-8% crucial in defense against virus	7
14322790534	lymphocytes	25% or more critical in immunity	8
14322794552	Platelets	blood clotting	9

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