Chemistry Flashcards

6437296146	PEL 1	2 Electrons	0
6437297915	PEL 2	8 Electrons	1
6437297916	PEL 3	18 Electrons	2
6437299707	PEL 4	32 Electrons	3
6437299708	PEL 5	50 Electrons	4
6437308756	nucleons	protons and neutrons	5
6437310667	mass number	number of neutrons in nucleus	6
6437312704	atomic number	number of protons in nucleus	7
6437324153	isotopes	same number of protons and electrons but different number of neutrons	8
6437347645	average atomic mass	based on the percentage of isotopes found in nature	9
6437350387	valence electrons	electrons in the outermost shell (can be easily shared, gained or lost)	10
6437354677	core electrons	electrons in the inner shell	11
6437368738	atomic spectra	the electromagnetic emission from atoms and molecules	12
6437418715	spectroscopy	A technique measuring electromagnetic emissions that is widely used in chemical analysis and in studies of the properties of atoms, molecules, ions, etc.	13
6437437774	wave mechanical model	Modern model of the atom, atoms have electrons in "orbitals" that are like clouds around the nucleus	14
6437447617	quantum numbers	specify the properties of atomic orbitals and the properties of electrons in orbitals	15
6437449966	Pauli Exclusion Principle	An atomic orbital may describe at most two electrons, each with opposite spin direction	16
6437473575	Hund's Rule	electrons do not pair up until they have to	17
6437475422	Aufbau Principle	An electron occupies the lowest-energy orbital that can receive it	18
6437487157	lewis Structures		19
6437490119	Nobel Gas Notation	shortcut→ find the closest noble gas (column 18) with fewer electrons than the element then finish configuration	20
6437503453	transition elements	What are the elements in groups 3-12 called?	21
6437518993	transition element properties	elements that have high melting points, often paramagnetic, tend to form salts when reacted w/ halogens ex; iron, copper, gold, silver, and titanium	22
6437575781	electronegativity	A measure of the ability of an atom in a chemical compound to attract electrons	23
6437578634	ionization energy	The amount of energy required to remove an electron from an atom	24
6437583074	alpha decay	A nuclear reaction in which an atom emits a ________ particle consisting of two protons and two neutrons. This increases the atomic number by 2 and the mass number by 4.	25
6437586693	beta decay	A nuclear reaction in which a neutron changes into a proton and into an electron, and the atoms emits a ______ particle, which is the electron. It increases the atomic number of the atom without changing the mass.	26
6437590735	gamma radiation	electromagnetic radiation emitted during radioactive decay and having an extremely short wavelength	27
6649993024	covalent bond	A chemical bond that involves sharing a pair of electrons between atoms in a molecule	28
6649993305	dipole-dipole attraction	attractive force resulting when polar molecules line up so that the positive and negative ends are close to each other	29
6649993853	electrostatic repulsion	Describes a force between particles with opposite electrical charges that causes them to push apart from one another	30
6649994166	hybridization	Several atomic orbitals mix to form the same total number of equivalent hybrid orbitals	31
6649995145	hydrogen bond	A relatively weak bond formed between any hydrogen atom (which is covalently bound to a nitrogen or oxygen atom) and a nitrogen or oxygen with an unshared electron pair	32
6649995457	ionic bond	Formed when one or more electrons are transferred from one atom to another	33
6649995861	London dispersion forces	The intermolecular attractions resulting from the constant motion of electrons and the creation of instantaneous dipoles	34
6649996089	metallic bond	a bond formed by the attraction between positively charged metal ions and the electrons around them	35
6649996364	pi bond	when two p orbitals line up in parallel and electron clouds overlap. it exsits over a single bond.	36
6649997810	resonance structure	a structure that occurs when it is possible to draw two or more valid electron dot structures that have the same number of electron pairs for a molecule or ion	37
6649998908	stable octet	the arrangement of eight electrons in the outermost shell of an atom	38
6649999221	sigma bond	a bond formed when two atomic orbitals combine to form a molecular orbital that is symmetrical around the axis connecting the two atomic nuclei	39
6649999573	van der Waals forces	a slight attraction that develops between the oppositely charged regions of nearby molecules	40
6649999929	VSERP	Valance Electron Pair Repulsion model / Unshared electron pairs around the central atom	41
6650001132	binary compound	What ionic compounds are called when they are composed of only two different kinds of atoms.	42
6650001133	coefficient	A number in front of a chemical formula in an equation that indicates how many molecules or atoms of each reactant and product are involved in a reaction.	43
6650001514	emperical formula	simplest whole # ration of atoms in a compound	44
6650001886	formula mass	the sum of the average atomic masses of all the atoms represented in the formula of any molecule, formula unit, or ion	45
6650002556	molecular mass	The sum of the masses of all the atoms in a molecule	46
6650002927	Law of Definite Composition	Chemical compounds are composed of a fixed ratio of elements as determined by mass.	47
6650003224	Law of Multiple Proportions	whenever two elements form more than one compound, the different masses of one element that combine with the same mass of the other element are in the ratio of small whole numbers	48
6650003732	net ionic equation	Includes only those compounds and ions that undergo a chemical change in a reaction in an aqueous solution	49
6650003932	percentage composition	the percentage by mass of each element in a compound	50
6650004295	polyatomic ion	A covalently bonded group of atoms that has a positive or negative charge and acts as a unit	51
6650004466	products	The elements or compounds produced by a chemical reaction.	52
6650004676	reactants	a substance that takes part in and undergoes change during a reaction	53
6650005137	Stock system	A method for naming ions of elements that can form more than one possible positive charge by using a Roman numeral after the ion name to denote the ion's charge.	54
6650005556	ternary compound	A compound that consists of three or more elements, usually containing	55
6650005557	true formula	chemical formula that indicates the actual number of atoms of each element in one molecule of a substance	56
6650006770	atmosphere	Layers of different gases that surround the Earth.	57
6650008025	atmospheric pressure	the pressure exerted by atoms and molecules in the atmosphere surrounding Earth, resulting from collisions of these particles with objects	58
6650008249	greenhouse effect	Natural situation in which heat is retained in Earth's atmosphere by carbon dioxide, methane, water vapor, and other gases	59
6650008555	manometer	A device used to measure the pressure of a sample of gas in a container.	60
6650008880	Boyle's Law	PV = k	61
6650009301	Charles's Law	V/T = k	62
6650010778	Combined Gas Law	P1V1/T1=P2V2/T2 (constant n)	63
6650012519	Ideal Gas law	PV = n R T	64
6650013191	Dalton's Law of Partial Pressures	Total pressure of a gas is equal to the sum of the partial pressure of the component gases	65
6650013612	Graham's Law	Rate of diffusion of a gas is inversely proportional to the square root of its molecular weight.	66
6650013613	Kinetic-Molecular Theory	a theory that explains that the behavior of physical systems depends on the combined actions of the molecules constituting the system	67
6650015459	mercury barometer	An instrument that measures changes in air pressure, consisting of a glass tube partially filled with mercury, with its open end resting in a dish of mercury.	68
6650015460	ozone	A form of oxygen that has three oxygen atoms in each molecule instead of the usual two.	69
6650015633	pascal	the SI unit of pressure equal to one newton per square meter	70
6650015634	standard pressure	1 atm or 101.3 kPa	71
6650017208	standard temperature	One atmosphere and 273 K.	72
6650017607	torr	the force per unit area exerted by the gas on its container, usually measured in atmospheres	73
6650021978	acidic anhydride	a nonmetallic oxide that, when placed in water, reacts to form an acid solution	74
6650021979	aeration	Air is forced through the water to release unwanted gases, which reduces odor and improves taste	75
6650022257	alloy	A mixture of two or more metals	76
6650022258	boiling point	The temperature at which a liquid changes to a gas	77
6650022585	Brownian movement	kinetic energy spreads small suspended particles throughout the cytoplasm of the cell	78
6650022981	colligative property	A property of a solution that depends on the number, not the identity, of the solute particles.	79
6650022982	concentrated	Describes a solution that has a relatively large amount of dissolved solute	80
6650023325	critical pressure	the lowest pressure at which the substance can exist as a liquid at the critical temperature	81
6650023806	critical temperature	the temperature above which the substance cannot exist in the liquid state	82
6650024569	crystal	An orderly, three-dimensional pattern of ions or atoms in a solid	83
6650024845	deliquescent	compounds that remove sufficient water from the air to dissolve completely and form solutions	84
6650024846	dilute	to lessen the concentration, force, or purity of by adding something	85
6650025555	dynamic equilibrium	Result of diffusion where there is continuous movement of particles but no overall change in concentration	86
6650026102	endothermic	A chemical reaction that absorbs energy (heat)	87
6650026527	efflorescent	hydrated crystals that lose the water of hydration on exposure to air at ordinary temperatures	88
6650026847	exothermic	A chemical reaction that releases energy (heat)	89
6650028696	heat of fusion	Amount of energy required to change a substance from the solid phase to the liquid phase.	90
6650028697	heat of vaporization	The amount of energy required for the liquid at its boiling point to become a gas	91
6650029172	"heavy" water	water containing an elevated concentration of molecules with deuterium	92
6650029662	deuterium	An isotope of hydrogen with one proton and one neutron in the nucleus having an atomic weight of 2.014	93
6650030344	hydrate	A compound that has a specific number of water molecules bound to its atoms	94
6650030896	Le Chatelier's Principle	States that if a stress is applied to a system at equilibrium, the system shifts in the direction that relieves the stress.	95
6650030897	melting point	The temperature at which a solid becomes a liquid	96
6650031287	miscible	Describes two liquids that are soluble in each other	97
6650031288	immiscible	Liquid solutes and solvents that are not soluble in each other	98
6650031477	molality	the concentration of a solution expressed in moles of solute per kilogram of solvent	99
6650031995	molarity	A common measure of solute concentration, referring to the number of moles of solute per liter of solution.	100
6650031996	mole fraction	The ratio of the moles of solute in solution to the total number of moles of both solvent and solute	101
6650032383	normality	Gram equivalent weight of solute per liter of solution, often denoted by N.	102
6650032384	phase equilibrium	when the rates of evaporation and condensation equalize	103
6650032887	polarity	A lack of electrical symmetry in a molecule. Charge differences on opposite ends of a structure.	104
6650033121	saturated	unable to dissolve any more solute	105
6650033434	solute	A substance that is dissolved in a solution.	106
6650033435	solvent	A liquid substance capable of dissolving other substances	107
6650033746	specific gravity	Density of an object realtive to water. No units.	108
6650034165	sublimation	A change directly from the solid to the gaseous state without becoming liquid	109
6650034446	surface tension	An inward force that tends to minimize the surface area of a liquid; it causes the surface to behave as if it were a thin skin	110
6650034988	temporary hardness	Temporary hardness is a type of water hardness caused by the presence of dissolved bicarbonate minerals (calcium bicarbonate and magnesium bicarbonate)	111
6650034989	viscosity	A liquid's resistance to flowing	112
6650080779	activation energy	the minimum amount of energy required to start a chemical reaction	113
6650080780	catalyst	a substance that initiates or accelerates a chemical reaction without itself being affected	114
6650081865	collision theory	atoms, ions, and molecules can react to form products when they collide, provided that the particles have enough kinetic energy	115
6650082891	factors affecting reaction rates	temperature, concentration ,particle size, and the use of a catalyst	116
6650084106	Law of Mass Action	The rate of a chemical reaction is proportional to the product of the concentrations of the reactants	117
6650084249	reaction mechanism	a series of elementary reactions that take place during the course of a complex reaction	118
6650084804	acid ionization constant	the value of the equilibrium constant expression for the ionization of a weak acid	119
6650084805	common ion effect	a decrease in the solubility of an ionic compound caused by the addition of a common ion	120
6650085201	enthalpy	The heat content of a system at constant pressure	121
6650085702	entropy	A quantitative measure of disorder or randomness, symbolized by S.	122
6650086167	equilibrium	A dynamic condition in which two opposing changes occur at equal rates in a closed system	123
6650087617	equilibrium constant	the ratio of product concentrations to reactant concentrations at equilibrium, with each concentration raised to a power equal to the number of moles of that substance in the balanced chemical equation	124
6650088220	free energy	Measures the portion of a system's energy that can perform work when temperature and pressure are uniform throughout the system, as in a living cell.	125
6650088758	Gibbs free-energy equation	ΔG= ΔH(enthalpy)- TΔS(entropy)	126
6650089547	solubility product constant	an equilibrium constant applied to the solubility of electrolytes; it is equal to the product of the concentrations of the ions each raised to a power equal to the coefficient of the ion in the dissociation equation	127
6650090633	acid	A substance that increases the hydrogen ion concentration of a solution.	128
6650090642	amphoteric	a substance that can act as both an acid and a base	129
6650090805	base	A substance that decreases the hydrogen ion concentration in a solution.	130
6650091025	buffer solution	A solution made from a weak acid and its conjugate base that neutralizes small amounts of acids or bases added to it	131
6650091352	conjugate acid	the particle formed when a base gains a hydrogen ion	132
6650092115	Arrhenius Theory	acids are characterized by their sour taste, low Ph, and the fact that they turn litmus red. Bases are characterized by their bitter taste, slippery feel, high pH, and the fact that they turn litmus paper blue	133
6650092859	conjugate base	particle that remains when an acid has donated a hydrogen ion	134
6650093074	end point	the point in a titration at which the indicator changes color	135
6650093415	equivalence point	the point at which the two solutions used in a titration are present in chemically equivalent amounts	136
6650093416	indicator	A compound that changes color in the presence of an acid or a base	137
6650094196	litmus	an indicator paper that turns red in an acid and blue in a base	138
6650094685	Bronsted-Lowery Theory	Defines acids as proton donors and bases as proton acceptors; recognizes that acids and bases do not need to exist in aqueous (water) solutions; explains how acids and bases react to neutralize each other and produce water and salts when combined	139
6650094808	neutralization	A reaction of an acid with a base, yielding a solution that is not as acidic or basic as the starting solutions were.	140
6650095326	pH	a numeric scale used to specify the acidity or basicity of an aqueous solution	141
6650096224	salt	An ionic compound made from the neutralization of an acid with a base.	142
6650096787	titration	a measured amount of a solution of unknown concentration is added to a known volume of a second solution until the reaction between them is just complete	143
6650097094	volumetric analysis	a technique for determining the amount of a certain substance by doing a titration.	144
6650097629	Lewis Theory	An acid is defined as an electron pair acceptor (e.g. BF3) and a base is an electron donator (e.g. NH3).	145
6650099243	anions	Negatively charged ions	146
6650099795	burning	a type of oxidation reaction	147
6650100758	cations	Positively charged ions	148
6650101178	combustion	A rapid reaction between oxygen and fuel that results in fire	149
6650101179	dissociation	the separation of ions that occurs when an ionic compound dissolves	150
6650101550	ionization	Process in which electrolytes dissolve in water and separate into charged particles	151
6650101862	natural gas	A gas with high methane content, found along with various fossil fuels and is used as a fuel.	152
6650102141	oxidation	A chemical change in which a substance combines with oxygen, as when iron oxidizes, forming rust	153
6650102142	oxidation states	A concept that provides a way to keep track of electrons in oxidation-reduction reactions according to certain rules	154
6650102677	oxidizing agent	the substance that oxidizes another substance by accepting its electrons	155
6650103151	redox	The chemical reasction in which the oxidizing agent is reduced and the reducing agent is oxidized is	156
6650103408	reducing agent	the substance that reduces another substance by losing electrons	157
6650103757	reduction	Any process in which electrons are added to an atom or ion (as by removing oxygen or adding hydrogen)	158
6650104544	acid salt	a salt formed by replacing part of the hydrogen ions of a dibasic or tribasic acid with metallic ions	159
6650104545	allotropic form	Forms of the same element that differ in their crystalline structures.	160
6650105137	basic oxygen furnace	Molten pig iron is injected with supersonic oxygen blast	161
6650105895	blast furnance	How are metals proced	162
6650105896	brass	An alloy of copper and zinc.	163
6650106267	bronze	Copper and tin	164
6650106268	electric arc furnace	enormous amounts of electricity generated through graphite cathodes that are lowered into the molten iron to purify it and produce a high grade of steel	165
6650107648	metaloid	Demonstrate properties of both metals and nonmetals. Examples are silicon and arsenic.	166
6650108068	normal salt	A salt in which all the hydrogen of the acid has been displaced by a metal.	167
6650108069	open-hearth furnace	large oven with a disk-shaped area, alternating blasts of flame are directed across the surface of the melted metal until the proper proportions of additives are established for that "heat"	168
6650108381	pig iron	iron that had not had its impurities removed	169
6650109386	rhombic	Crystal structure of sulfur - heated in mineral oil to dissolve	170
6650109387	monoclinic	Mineral with three planes of cleavage, two are perpendicular, the third is not	171
6650110220	amorphous	shapeless, without definite form; of no particular type or character; without organization, unity, or cohesion	172
6650110724	semiconductor	A substance that can conduct electricity under some conditions	173
6650111822	alcohol	An organic compound with a hydroxyl group attached to one of its carbon atoms.	174
6650112124	aldehyde	An organic molecule with a carbonyl group located at the end of the carbon skeleton.	175
6650112125	alkane	a hydrocarbon containing only single covalent bonds	176
6650112529	alkene	A hydrocarbon that contains a double bond.	177
6650112884	alkyl groups	Groups of atoms that are formed when one hydrogen atom is removed from an alkane molecule	178
6650112885	alkyne	a carbon compound with a carbon-carbon triple bond.	179
6650113237	amine	organic compounds that contain only hydrogen, carbon , and nitrogen	180
6650113481	amino acid	The building blocks of proteins	181
6650113482	aromatics	Certain unsaturated cyclic compounds. High stability. Every carbon bond has intermediate single doublr bonds	182
6650114032	diamond	carbon arranged in a crystal lattice	183
6650114377	ester	an organic compound made by chemically combining an alcohol and an organic acid	184
6650114378	ether	n oxygen atom connected to two alkyl or aryl groups	185
6650115619	fullerene	a form of carbon that consists of atoms arranged in the shape of a hollow sphere	186
6650115796	functional groups	chemical groups attached to carbon skeletons that give compounds their functionality	187
6650116845	hydrocarbon	Compounds composed of only carbon and hydrogen	188
6650117168	hydrogenation	The process of converting unsaturated fats to saturated fats by adding hydrogen	189
6650117876	isomer	Compounds with the same formula but different structures.	190
6650117877	ketone	An organic compound with a carbonyl group of which the carbon atom is bonded to two other carbons.	191
6650119752	photosynthesis	Conversion of light energy from the sun into chemical energy.	192
6650120132	saturated hydrocarbon	A hydrocarbon in which all the bonds between carbon atoms are single bonds	193
6650120804	unsaturated hydrocarbon	A hydrocarbon in which one or more of the bonds between carbon atoms is double or triple	194
6650122352	gravimetric balance	direct readings to thousandths of a gram instead of a triple-beam balance	195
6650122876	pH meters	Electronic instruments: sensor responds to Hydronium ions by producing a current	196
6650122877	salt bridge	A tube that allows the slow transfer of ions and maintains the neutrality of the electrolyte solutions.	197
6650123135	spectrophotometer	An instrument that measures the proportions of light of different wavelengths absorbed and transmitted by a pigment solution.	198