| 1898571928 | This lab equipment contains deionized water and is used to rinse glassware such as test tubes. | Wash Bottle |  | 0 |
| 1898571929 | This piece of lab equipment is used along with a ring and ring stand to hold a beaker over a flame. | Wire Gauze |  | 1 |
| 1898571930 | This piece of lab equipment has a lid and is made of heat resistant porcelain which allows for heating/melting chemicals such as metals and ores to very high temperatures. | Crucible and Cover |  | 2 |
| 1898571931 | This piece of lab equipment is used with a ring and ring stand to hold a crucible over a flame. | Clay Triangle |  | 3 |
| 1898571932 | What piece of lab equipment would you use to ACCURATELY measure liquids? | Graduated Cylinder |  | 4 |
| 1898571933 | When reading a graduated cylinder you get at eye level and view the _____. How many places after the decimal do you round your measurement and what are the units? | Meniscus, 2 places after the decimal with the last number (hundredths) being estimated, mL
The picture shows accurately 36.5 but there has to be an estimated number so you would record 36.53 mL. |  | 5 |
| 1898571934 | This piece of glassware is used for mixing, measuring, and storing chemicals. It has a "neck" which allows you to hold it, use a clamp and ring stand, and seal it with cork or stopper. | Erlenmeyer Flask |  | 6 |
| 1898571935 | This is a very common piece of glassware used in the lab when obtaining liquids and for APPROXIMATE measurements. | Beaker |  | 7 |
| 1898571936 | This porcelain item resembles a shallow bowl with a spout. It is traditionally used to evaporate excess water - or other solvents - to ensure that a concentrated solution or the dissolved substance is left behind. | Evaporating Dish |  | 8 |
| 1898571937 | This piece of glassware is a circular, slightly convex-concave piece of glass used as a surface to evaporate a liquid, to hold solids while being weighed, or as a cover for a beaker. | Watch Glass |  | 9 |
| 1898571938 | What is the proper/safe technique used to smell chemicals? | Wafting |  | 10 |
| 1898571939 | When diluting an acid do you pour .....
A: Acid into water
B: Water into acid | Acid into Water |  | 11 |
| 1898571940 | This lab technique is a method of separating and analyzing mixtures of chemicals such as separating color components in different ink samples. | Chromatography |  | 12 |
| 1898571941 | When needing to separate a liquid from a solid this technique is used which is a process of removing, or pouring, a liquid out of a container while still leaving the solid, or the sediment, in the bottom of the container. | Decanting |  | 13 |
| 1898571942 | This lab technique is used for separation based on particle size. Typically a funnel and filter is used as a medium which allows liquids and gasses to pass through collecting solids on the paper. | Filtration |  | 14 |
| 1898571943 | This lab technique is used when the liquid can evaporate leaving the solid behind. | Evaporation |  | 15 |
| 1898571944 | This lab technique is used to separate liquids based on boiling points. | Distillation |  | 16 |
| 1898571945 | This lab technique is used to determine the concentration/molarity of an unknown substance. | Titration |  | 17 |
| 1898571946 | What two pieces of lab equipment can be used to measure pH? | Litmus Paper and pH Probe |  | 18 |
| 1898571947 | What two pieces of lab equipment can be used to measure change in temperature or heat? | Temperature Probe and Thermometer |  | 19 |
| 1898571948 | Define and explain how to calculate the mean, median and mode for a set of data. | Mean = average
Median = middle (like the median in the middle of the highway)
Mode = occurs most often |  | 20 |
| 1898571949 | Which is the solute and which is the solvent in a glass of salt water? | Salt = solute
Water = solvent
*Note: Water is the universal solvent |  | 21 |
| 1898571950 | What term means: How close a measurement is to the true/actual value. | Accuracy |  | 22 |
| 1898571951 | Is the Independent Variable on the (X or Y) axis? | X Axis
*Note: The variable manipulated by the experimenter . |  | 23 |
| 1898571952 | What is the purpose of a control group in an experiment? | Used as a standard of comparison in an experiment. All variables are constant/unchanging.
*Note: A control is required in every experiment |  | 24 |
| 1898571953 | True or False: When studying the effect of a catalyst on a reaction, the control group will NOT have any catalyst added. | True
Answer to SOL question: J
Trial 4 is the control because it does not have any catalyst added which is what is being studied.
Only ONE variable can be changed at a time. |  | 25 |
| 1898571954 | When moving the decimal to the left to put a number in scientific notation you (add or subtract) to the exponent. | Add
Answer to SOL question: B |  | 26 |
| 1898571955 | Determining Significant Figures Rules | |  | 27 |
| 1898571956 | Determining Significant Figures SOL Practice Problem | Answer to SOL question: H
*Note: Ignore the exponent when determining significant figures |  | 28 |
| 1898571957 | Determining Significant Figures SOL Practice Problem | Answer to SOL question: G |  | 29 |
| 1898571958 | When calculating addition and subtraction problems do you look (after the decimal or at the whole number) to determine significant figures? | After the decimal |  | 30 |
| 1898571959 | What are the units for Molar Mass and where do you find the molar mass for each element? | g/mol ; found on the periodic table |  | 31 |
| 1898572103 | Law of Multiple Proportions | Compounds contain elements in small, whole number, ratios.
Ex: NaCl = 1:1 | | 32 |
| 1898572104 | Law of Definite Proportions | Two samples of the same compound always contains the same elements combined in the same proportions by weight.
Ex: NaCl- no matter where you get NaCl it is always going to be a 1:1 ratio. | | 33 |
| 1898572105 | Law of Conservation of Mass | Mass cannot be created or destroyed in ordinary chemical and physical changes.
i.e. the total mass of the reactants must equal the total mass of the products
Ex: 5gNa + 5gCl --> 10gNaCl | | 34 |
| 1898571960 | Density Triangle | |  | 35 |
| 1898571961 | Molarity Equation | Remember the given numbers must be in units of MOLES and LITERS. If the are not you must convert them before you calculate. |  | 36 |
| 1898572106 | Specific Heat Definition | The amount of energy needed to raise 1 gram of a substance 1 degree Celsius. | | 37 |
| 1898571962 | Specific Heat Equation with Units | |  | 38 |
| 1898571963 | Molar Enthalpy Equation with Units | |  | 39 |
| 1898571964 | Positive Enthalpy= (endo or exo)thermic
Negative Enthalpy = (endo or exo)thermic | |  | 40 |
| 1898571965 | Atomic Mass Equation | Remember you don't have to divide by 100 if the % is already converted to a decimal. |  | 41 |
| 1898571966 | Equation for % Yield | |  | 42 |
| 1898571967 | Molar Heat of Fusion and Vaporization Equation | Q = joules or calories
m = grams
H(fusion) = they must give you this number |  | 43 |
| 1898571968 | % Error Equation | Needs to be < 2% |  | 44 |
| 1898571969 | Equilibrium Constant Problem | |  | 45 |
| 1898571970 | Dilution Equation | M = molarity or a concentration |  | 46 |
| 1898571971 | Metric Prefix Conversions | Kile-Had-Dirrehea-BASE-During-Coles-Midterm |  | 47 |
| 1898572107 | SI Units of Mass | Kilograms
*FYI: The reason it is kilograms and not grams is because the mass of 1 cm³ of water is 1kg. | | 48 |
| 1898572108 | SI Units of Volume | Liters | | 49 |
| 1898572109 | SI Units of Temperature | Kelvins | | 50 |
| 1898572110 | SI Units for Pressure | Pascals | | 51 |
| 1898571972 | If you are converting atoms to moles, what number would you need to place on the bottom of the "T" chart? What is that number? | |  | 52 |
| 1898571973 | If you are converting grams to moles, what number would you need to place on the bottom of the "T" chart? Where would you find this number? | Molar Mass, Periodic Table |  | 53 |
| 1898572111 | Convert degree Clesius to Kelvin | Add 273.15 | | 54 |
| 1898572112 | What can cause a physical change in state? | Increase in temperature, pressure or motion | | 55 |
| 1898571974 | What is a physical change? Give examples. | Change in state. |  | 56 |
| 1898571975 | Properties of Solids, Liquids, and Gases | |  | 57 |
| 1898571976 | List the 6 Phase Changes:
Solid to Liquid, Liquid to Solid
Liquid to Gas, Gas to Liquid
Solid to Gas, Gas to Solid | |  | 58 |
| 1898571977 | Know each step of the heating/cooling graph. | Point B = Molar Heat of Fusion
Point D = Molar Heat of Vaporization
Points A,C,E = Kinetic Energy
Points B,D = PotentialEnergy |  | 59 |
| 1898571978 | Know all points on a phase diagram | Triple Point = all three phases coexist at equilibrium
Critical Point = above this point is supercritical fluid (properties of both liquid and gas) |  | 60 |
| 1898572113 | List some physical properties | Density, conductivity, melting point, boiling point, malleability, ductility | | 61 |
| 1898571979 | 4 things that are evidence a chemical change has occured | 1. Evolution of a Gas (Bubbles, Odor, Sound)
2. Formation of a Precipitate
3. Release or Absorption of Energy (temp increase or decrease, light)
4. Color Change (be careful) |  | 62 |
| 1898572114 | Describe a chemical change and give examples. | Can not get the original substance back.
Ex: Oxidation (rusting), Combusion, Burning, Fermentation | | 63 |
| 1898571980 | What makes water have a very high melting and boiling point? | Hydrogen Bonds |  | 64 |
| 1898572115 | What 2 things effect melting and freezing point? | Change in atmospheric pressure and certain solutes. | | 65 |
| 1898571981 | Law of Conservation of Energy | Total quantity of energy remains constant during physical and chemical changes. |  | 66 |
| 1898571982 | Solid Sphere Model | Dalton- an atom is little more than a singular, solid particle without other components. |  | 67 |
| 1898571983 | Plum Pudding Model | JJ Thompson- electrons are embedded in a central mass |  | 68 |
| 1898571984 | Nuclear Model | Rutherford- the atom consists of a dense positive center called the nucleus and is orbited by negatively charged electrons |  | 69 |
| 1898571985 | Planetary Model | Bohr- electrons move in circular orbitals at fixed distances from the nucleus (ie: specific energy levels) |  | 70 |
| 1898571986 | Quantum Mechanical Model | Heisenberg, deBroglie, Schrodinger |  | 71 |
| 1898571987 | John Newland | First to discover the periodic table
Noticed a pattern every 8 elements- called it the law of octaves |  | 72 |
| 1898571988 | Mendeleev | Father of the Periodic Table
Arranged by increasing atomic mass
Credit becuause he predicted missing elements |  | 73 |
| 1898572116 | Mosely | Modern Day Periodic Table
Arranged by increasing atomic number | | 74 |
| 1898571989 | JJ Thompson's Experiment and Discovery | Cathode Ray Tube
Electron and it's negative charge by using a magnet
Deducted that there must be a positive charged particle as well |  | 75 |
| 1898571990 | Rutherford's Experiment and Discovery | Gold Foil
Nucleus is small and dense
Atom is mostly empty space |  | 76 |
| 1898571991 | What did Dalton try to explain with his atomic theory? | How atoms combine |  | 77 |
| 1898571992 | The atomic number indicates the number of _____. | |  | 78 |
| 1898571993 | How to find the number of neutrons: | |  | 79 |
| 1898571994 | Be able to determine number of electrons, protons and neutrons when the legend is arranged like this: | 79 protons, 79 electrons, and 197-79= 118 neutrons |  | 80 |
| 1898571995 | A neutral atom has equal number of _____ & _____. | Electrons and Protons
Ex: Carbon at ground state has 6 protons, 6 electrons, and 6 neutrons |  | 81 |
| 1898571996 | What is the charge of the 3 subatomic particles, electrons, protons, and neutrons? | |  | 82 |
| 1898571997 | Where are each of each of the 3 subatomic particles found in the atom? | |  | 83 |
| 1898571998 | The atomic mass is composed of _____ & _____ found in the nucleus. Which of the two subatomic particles weighs the most? | Neutrons and Protons
Neutrons weighs the most, making up most of the weight of the atom |  | 84 |
| 1898571999 | Explain the difference between C-12 and C-14. What are these called? | C-14 has two more neutrons than C-12 which means it weighs more.
An element with different number of neutrons are called Isotopes. |  | 85 |
| 1898572000 | What type of bond conducts electricity? | Ionic
Metal (+) and Nonmetal (-) |  | 86 |
| 1898572117 | Group 1 elements tend to react with group ___. Why? | Group 17 b/c group 17 wants to gain 1 electron where as group 1 wants to lose 1 electron. | | 87 |
| 1898572118 | Group 2 elements tend to react with group ___. Why? | Group 16 b/c group 16 wants to gain 2 electrons where as group 2 wants to lose 2 electrons. | | 88 |
| 1898572001 | Describe what happens when an element becomes ionized. | It either gains electrons and becomes negative or looses electrons and becomes positive. |  | 89 |
| 1898572119 | A negative ion is called an _____. | Anion | | 90 |
| 1898572002 | A positive ion is called a _____. | Cation |  | 91 |
| 1898572120 | What is an alloy? Give examples. | Mixture of two or more metals (ie: soild solution)
Ex: Brass, steel, 14k gold, and sterling silver. | | 92 |
| 1898572003 | All elements in the same group have similar _____ properties. Why? | Chemical Properties due to them all having the same number of valence electrons. |  | 93 |
| 1898572004 | Locate the Metals and Nonmetals on the Periodic Table | |  | 94 |
| 1898572005 | Know the name for group 1, 2, 3-12, 17 and 18. | |  | 95 |
| 1898572006 | What are the elements on the "stairstep" called? How are they special? | Metalloids- they have properties of both metals and nonmetals
**Called semiconductors- used in computer chips |  | 96 |
| 1898572007 | What are groups 1,2 and 13-18 called as a whole? | Main Group Elements- This leaves out the transition metals because of their inconsistent electron configurations. |  | 97 |
| 1898572008 | The molecular formula is (reduced or before reduced)? | Before being reduced |  | 98 |
| 1898572009 | The empericaa formula is (reduced or before reduced)? | Reduced |  | 99 |
| 1898572121 | Moving across a period each element is increased by one _____. This is what makes the atomic number increase by one. | Proton | | 100 |
| 1898572010 | Know what each part of an electron configuration corresponds to on the periodic table. | |  | 101 |
| 1898572011 | Know the order of electron configurations: | |  | 102 |
| 1898572012 | How would you determine the number of valence electrons from an electron configuration? | |  | 103 |
| 1898572013 | List the 4 Quantum Numbers and their meaning: | n= main energy level (the big numbers in electron configurations)
l= shape (the letters s, p, d, f in electron configurations)
m= tells which way the dumbbells are facing
s= spin (one electron spins +1/2 and the other -1/2) represented with up and down arrows when drawing Hund's Rule. |  | 104 |
| 1898572014 | What is the shape of the s, p, d, and f orbitals? | |  | 105 |
| 1898572015 | Locate the s, p, d, and f blocks on the periodic table: | |  | 106 |
| 1898572016 | Pauli Exclusion Principle | An orbital can hold a maximum of 2 electrons. |  | 107 |
| 1898572017 | Pauli Exclusion Joke | |  | 108 |
| 1898572018 | Afbau Principle | Electrons are added to the lowest energy level first, or the energy level that requires the least amount of energy to fill. |  | 109 |
| 1898572019 | Write the electron configuration for Iron (26 electrons) | 4= outermost energy level = period 4
2 valence electrons = group 2 or 12 |  | 110 |
| 1898572020 | List the seven diatomic molecules. What does it mean to be diatomic and when do we use them? | Nitrogen, Oxygen, Fluorine, Chlorine, Bromine, Iodine, Hydrogen
Diatomic means 2, so 2 atoms bonded together
These elements are only diatomic when they are written by themselves. This is how they are found in nature. |  | 111 |
| 1898572021 | Hund's Rule | Every orbital in a subshell is singly occupied with one electron before any one orbital is doubly occupied, and all electrons in singly occupied orbitals have the same spin. |  | 112 |
| 1898572022 | Explain the Group and Period Trend for Atomic Radius | Down a Group = Increases due to addition of energy levels
Across a Period (Lt-->Rt) = Decreases due to stronger pull on electrons by the nucleus due to the desire to gain electrons
*Snowman Poop |  | 113 |
| 1898572023 | Explain the Group and Period Trend for Shielding Effect | Down a Group = Increases
Across a Period (Lt-->Rt) = Constant due to same energy level
*Same as Atomic Radius
** As energy levels increase more distance and electrons are put between the outer electrons and the nucleus shielding them from the complete pull of the nucleus. |  | 114 |
| 1898572024 | Explain the Group and Period Trend for Ionization Energy | Down a Group = Decreases due to electrons moving farther away from nucleus and not being held as tightly
Across a Period (Lt-->Rt) = Increases due to wanting to gain electrons (16 & 17 want to gain 1 and 2 electrons very badly), therefore it will take a lot of energy to remove an electron.
* The energy it takes to remove a valence electron |  | 115 |
| 1898572025 | Explain the Group and Period Trend for Electronegativity and Electron Affinity | Down a Group = Decreases due to electrons moving farther away from nucleus and not being held as tightly
Across a Period (Lt-->Rt) = Increases due to wanting to gain electrons
*Stops at Halogens
**Fluorine has the highest electronegativity = 4.0 |  | 116 |
| 1898572026 | Electronegativity and Ionization Energy Overview | |  | 117 |
| 1898572027 | London Dispersion Force | A temporary attractive force that results when the electrons in two adjacent atoms occupy positions that make the atoms form temporary dipoles.
*The weakest intermolecular force |  | 118 |
| 1898572028 | Dipole-Dipole Moment | Occurs when the partial positive and partial negative ends, on 2 polar molecules, attract one another.
*Similar to ionic bonds but MUCH weaker |  | 119 |
| 1898572029 | Explain the difference in intERmolecular forces and intRAmolecular forces. | |  | 120 |
| 1898572030 | What is the term for the different molecular forms of an element? | |  | 121 |
| 1898572031 | List 2 allotropes of oxygen | |  | 122 |
| 1898572032 | List 3 allotropes of hydrogen | |  | 123 |
| 1898572033 | List 3 allotropes of carbon | |  | 124 |
| 1898572034 | Sulfate | |  | 125 |
| 1898572035 | Carbonate | |  | 126 |
| 1898572036 | Hydroxide | |  | 127 |
| 1898572037 | Phosphate | |  | 128 |
| 1898572038 | Ammonium | |  | 129 |
| 1898572039 | Ammonia | |  | 130 |
| 1898572040 | Hydrogen Carbonate (Bicarbonate) | |  | 131 |
| 1898572041 | Cyanide | |  | 132 |
| 1898572042 | Nitrate | |  | 133 |
| 1898572043 | Sulfite | |  | 134 |
| 1898572122 | ending -ide | Just the element on the periodic table
Ex: Sulfide = S Chloride = Cl like in Sodium Chloride NaCl | | 135 |
| 1898572123 | ending -ate | Polyatomic ions you had to memorize | | 136 |
| 1898572124 | ending -ite | Polyatomic ions you had to memorize BUT..... with one less oxygen! | | 137 |
| 1898572044 | Know the first 10 Hydrocarbons and their Formulas | |  | 138 |
| 1898572045 | How can you tell if an organic compound is saturated or unsaturated? What type is the following compound? | This is organic because is contains both hydrogen and carbons
Saturated because all bonds are single bonds! |  | 139 |
| 1898572046 | How can you tell if an organic compound is saturated or unsaturated? What type is the following compound? | This is organic because is contains both hydrogen and carbons
Unsaturated because NOT all bonds are single bonds. When there are double or triple bonds it is unsaturated. |  | 140 |
| 1898572047 | Is this reaction endothermic or exothermic?
AB + energy --> A + B | When the word "energy" or "heat" is with the reactants the reaction is endothermic. |  | 141 |
| 1898572048 | Endothermic Graph | Up the Hill |  | 142 |
| 1898572049 | Is this reaction endothermic or exothermic?
A + B --> AB + heat | When the word "energy" or "heat" is with the products the reaction is exothermic. |  | 143 |
| 1898572050 | Exothermic Graph | Down the Hill |  | 144 |
| 1898572051 | Tetrahedron | The prefix "tetra" means 4 therefore the central atom has four atoms attached |  | 145 |
| 1898572052 | Trigonal Planar | Notice there is no lone pair on the central atom therefore the arms stick straight out like an "airplane" |  | 146 |
| 1898572053 | Linear | The central atom does not have any lone pairs therefore the arms stay straight out like a line |  | 147 |
| 1898572054 | Bent | This is what happens when the linear structure has two lone pairs around the central atom. The lone pairs push down on each arm until the hydrogens repel each other.
** Water is the #1 example of Bent |  | 148 |
| 1898572055 | Pyramidal | The lone pair on the central atom pushes down on the arms giving the appearance of a pyramid. |  | 149 |
| 1898572056 | What type of bond is formed between a metal and a nonmetal? | Ionic Bond = very strong |  | 150 |
| 1898572057 | What type of compound is held together with ionic bonds? | Ionic Compounds |  | 151 |
| 1898572058 | How do we name ionic compounds? | Element + Element(ide)
**May need polyatomic ions |  | 152 |
| 1898572059 | How do you write the formula for an ionic compound? | Find the charge for each element on the periodic table and criss cross. |  | 153 |
| 1898572060 | What type of bond is formed between a nonmetal and a nonmetal? | Covalent Bond |  | 154 |
| 1898572125 | What type of compound is held together with covalent bonds? | Molecular Compound | | 155 |
| 1898572061 | How do you name molecular compounds? | With prefixes representing the number of atoms.
**Never use mono- with the first element
Ex: CO2 = Carbon Dioxide NOT Monocarbon Dioxide |  | 156 |
| 1898572062 | Know prefixes 1-10 for naming molecular compounds | |  | 157 |
| 1898572063 | Do ionic bonds share or transfer electrons to form a bond? | Transfer |  | 158 |
| 1898572064 | Oxidation and Reduction | LEO says GER
LEO = Loses Electrons- Oxidation
GER = Gains Electrons- Reduction |  | 159 |
| 1898572065 | Do covalent bonds share or transfer electrons to form a bond? | Share |  | 160 |
| 1898572066 | If electrons are shared unequally in a covalent bond is it a polar covalent bond or nonpolar covalent bond? | Polar Covalent |  | 161 |
| 1898572067 | If electrons are shared equally in a covalent bond is it a polar covalent bond or nonpolar covalent bond? | Nonpolar Covalent |  | 162 |
| 1898572068 | What type of bond is formed between two metals? | Metallic Bond |  | 163 |
| 1898572069 | A + BC ---> B + AC | Single Displacement
** There is a single element on each side |  | 164 |
| 1898572070 | AC + BD ---> AD + BC | Double Displacement
** Everything is in twos on both sides |  | 165 |
| 1898572071 | A + B ---> AB | Synthesis
** Like synthesize which means make |  | 166 |
| 1898572072 | AB ---> A + B | Decomposition
** Decompose means to break apart |  | 167 |
| 1898572073 | Hydrocarbon + Oxygen ---> Carbon Dioxide + Water | Combustion
** The hydrocarbon is the only part of the reaction that changes |  | 168 |
| 1898572074 | Acid + Base ---> Salt + Water | Neutralization
** To neutralize an acid you must have a base |  | 169 |
| 1898572075 | What type of reaction does the following picture depict? | Decomposition |  | 170 |
| 1898572126 | Based on Le Chatelier's Principle what can shift the equilibrium of a reaction? | Temperature, Pressure, Concentration, Volume
**NOT CATALYST!!!!!!!! | | 171 |
| 1898572076 | Determine which direction the reaction will shift based on Le Chatelier's Principle | |  | 172 |
| 1898572077 | Polar will dissolve other _____ substances. | Polar
** This follows the general rule that "like dissolves like" |  | 173 |
| 1898572078 | Nonpolar will dissolve other _____ substances. | Nonpolar
** This follows the general rule that "like dissolves like" |  | 174 |
| 1898572079 | When deciding if two substance will dissolve in each other you follow the general rule that "like dissolves _____". | Like
i.e. "polar dissolves polar" and 'nonpolar dissolves nonpolar" |  | 175 |
| 1898572080 | The amount of energy required to start a chemical reaction. | Activation Energy |  | 176 |
| 1898572081 | The addition of a _____ lowers the activation energy. | Catalyst |  | 177 |
| 1898572082 | Be able to describe Arrhenius Acids and Bases | Arrhenius just described the properties of both acids and bases |  | 178 |
| 1898572083 | Bronsted Lowery Acid and Bronsted Lowery Base | Bronsted Lowery Acid = proton donor
Bronsted Lowery Base = proton acceptor
** Bronsted Lowery Acids and Bases are found in the reactants side of the reaction |  | 179 |
| 1898572084 | Conjugate Acid and Conjugate Base | Conjugate Acid = Forms when a base gains a proton (opposite of the Bronsted Lowery Base)
Conjugate Base = Forms when an acid loses a proton (opposite of a Bronsted Lowery Acid)
** Conjugate Acids and Bases are found in the products side of the reaction |  | 180 |
| 1898572085 | pH Scale | 0 to 14
0 to 6 = acidic (red)
7 = neutral
8 to 14 = basic/alkalinity (blue) |  | 181 |
| 1898572086 | Acids vs Bases | Acids typically begin with a hydrogen and the name ends with the ending -ic
Bases typically have a hydroxide (OH-). One common base that's an exception is NH3 = ammonia |  | 182 |
| 1898572087 | pH + pOH = ? | |  | 183 |
| 1898572088 | In water, Arrhenius Acids dissociate into ___ ions. | Hydrogen Ions |  | 184 |
| 1898572089 | In water, Arrhenius Bases dissociate into ___ ions. | Hydroxide Ions |  | 185 |
| 1898572090 | Ideal Gas Law Equation (know what each part means) | Remember that "n" HAS to be in moles. So if the problem give you grams convert it to moles using the molar mass first!
*Gas Constant depends on pressure units. See Gas Constant Flashcard for options. |  | 186 |
| 1898572091 | Common Gas Constants used for the "R" in the Ideal Gas Law Equation: When pressure units are kPa and atm. | |  | 187 |
| 1898572092 | Gay-Lussac's Gas Law | Pressure and Temperature
Directly Proportional |  | 188 |
| 1898572093 | Combined Gas Law | Combines Boyle's, Charles and Gay-Lusacc's
**Make sure all units match before calculating!! |  | 189 |
| 1898572094 | Boyle's Gas Law | Pressure and Volume
Inversely Proportional (The ONLY one!)
* Be sure to keep the correct pressure and volumes together. |  | 190 |
| 1898572095 | Charles Gas Law | Volume and Temperature
Directly Proportional
* Make sure temperature units are in Kelvins |  | 191 |
| 1898572096 | Dalton's Law of Partial Pressure | For a mixture of gases in a container |  | 192 |
| 1898572127 | Kinetic Molecular Theory | Explains gas behavior- Gas is in constant, rapid, random motion. | | 193 |
| 1898572097 | Gas Law Summary | |  | 194 |
| 1898572098 | Molar Volume Conversion of a gas at STP | |  | 195 |
| 1898572099 | The randomness or disorder of particles is called _____. | Entropy |  | 196 |
| 1898572100 | Determine which equation shows a decrease in entropy. | Remember entropy is disorder, therefore going from a liquid to solid would decrease disorder.
Answer: A |  | 197 |
| 1898572101 | Standard Temperature | |  | 198 |
| 1898572102 | Standard Pressures (STP): 1atm = ?torr, ?mmHg, ?Pa, ?kPa | |  | 199 |
