ap chem exam

5.0(1)
learnLearn
examPractice Test
spaced repetitionSpaced Repetition
heart puzzleMatch
flashcardsFlashcards
Card Sorting

1/91

flashcard set

Earn XP

Description and Tags

Study Analytics
Name
Mastery
Learn
Test
Matching
Spaced

No study sessions yet.

92 Terms

1
New cards
buffers
* resist change in pH with small amounts of H+ or OH- added
* weak acid/conjugate base or weak base/conjugate acid
* buffer capacity: ability to react with added H+ or OH-. higher concentration of components = greater capacity
2
New cards
average atomic mass
decimal percentages of each isotope multiplied by isotope’s atomic mass
3
New cards
changes to K
* flip reaction = flip K
* double reaction = square K
4
New cards
exothermic reactions
* -deltaH
* energy required to break bonds in reactants must be less than energy released in forming bonds in products
* heat as product
5
New cards
polarity
6
New cards
polarizability
7
New cards
percent ionizations
* how much an acid dissociates compared to initial concentration
* greater the Ka = greater the percent ionization
* (concentration of dissociated compound/initial concentration) x 100
8
New cards
thermal equilibrium
* higher temperature decreases
9
New cards
mass percent
* (mass/molar mass) x 100
* (found mass of sample at certain time/mass of the sample) x 100
10
New cards
equivalence point
* equimolar amount of conjugate acid/base is added to base/acid.
* reaction has essentially gone to completion
* concentration of conjugate acid/base is greater than that of base/acid
11
New cards
empirical formua
simplest whole # ratio of atoms for a compound
12
New cards
molecular formula
chemical formula for compound
13
New cards
mass spectroscopy
mass to charge ratio of compounds
14
New cards
electron configuration rules
* electrons fill the lowest energy level orbital first
* no two e- can have the same spin
* e- occupy separate subshells before sharing one
15
New cards
photoelectron spectroscopy
measures the amount of energy electrons release
16
New cards
periodic trend for electronegativity
increases as you go from left to right (number of protons increases)

decreases as you go down (shielding increases)
17
New cards
periodic trend for atomic radius
decreases as you move from left to right (number of protons increases)

increases as you go down (shielding increases)
18
New cards
periodic trend for ionization energy
increases as you go left to right (number of protons increases)

decreases as you go down (shielding increases)
19
New cards
homogenous mixture
* uniform composition
* not chemically bonded
* 2+ substances
* e.g. salt water
20
New cards
heterogeneous mixture
* non-uniform composition
* not chemically bonded
* 2+ substances
21
New cards
ionic bonds
* between metal and nonmetals
* e- transferred
22
New cards
covalent bonds
* between nonmetals
* e- shared
23
New cards
lattice energy
energy of ionic bonds
24
New cards
metallic bonds
sharing of free e- between metal atoms
25
New cards
alloys
* compounds of different metals
* interstitial: smaller metal atoms inserted between spaces
* substitutional: similar size metal atoms substituted
26
New cards
hybridization
atomic orbitals fuse to form new orbitalss
27
New cards
formal charge
* charge of element in a molecule
* number of valence electrons of that atom and subtract number of assigned electrons in Lewis structure
* lone pairs = 2 assigned electrons
* bonds = 1 assigned electron
28
New cards
resonance
* molecules bonding structure is a combination of other possible structures
* best resonance structure is that which has total formal charge of 0/close to 0
29
New cards
Coulomb’s Law
* shorter distances and higher charges = stronger attractions
* F = q1xq2/r^2
* q1 = charge of nucleus
* q2 = charge of electron
* r = distance between charges
30
New cards
strongest to weakest IMFs

1. ion-ion
2. ion-dipole: ionic compounds and liquid
3. hydrogen bonding: fluorine, oxygen, nitrogen; polar
4. dipole-dipole: between two polar molecules (polar = asymmetrical)
5. dipole-induced dipole:
6. London Dispersion Forces: exist in every sample
31
New cards
melting point
32
New cards
boiling point
33
New cards
viscosity
resistance of fluid (liquid or gas) to change in shape, or movement of neighboring portions relative to one another
34
New cards
ionic solid
* ions held in fixed positions in giant 3D lattice
* not malleable or ductile
* brittle: disrupt structure → repulsion → split solid
* high b.p. and m.p.
* low vapor pressures and volatility
* only conduct electricity when molten or in solution
35
New cards
volatility
tendency of substance to evaporate at normal temperatures
36
New cards
covalent network solids
* continuous network of covalently bonded atoms that span entire surface
* very hard
* high m.p.
* do not conduct electricity
37
New cards
molecular solids
* made from non-metals
* weak IMFs
* low melting points
* do not conduct electricity
* hydrogen bonding, dipole-dipole, LDFs
38
New cards
metallic solids
* Close packed lattice of positive atoms/ions surrounded by sea of electrons
* Good conductor of electricity and heat (closely packed)


* Metallic bond: electrostatic attraction between positive and negative charge
* Malleable and ductile
39
New cards
kinetic molecular theory

1. far apart
2. are in constant motion
3. elastic collisions
4. no attractions/repulsions
5. average k.e. = temperature
40
New cards
ideal gas law
PV = nRT
41
New cards
solutions
* like dissolves like
42
New cards
Beer’s Law
A = abc represents the change in light’s energy as it passes through a material.
43
New cards
photons
carry energy in waves
44
New cards
limiting reactant
compound that runs out during reaction, which stops it
45
New cards
net ionic equations
* remove spectator ions to show the species that actually interact in a reaction.
46
New cards
combustion reactions
hydrocarbon + O2 → H2O + CO2
47
New cards
redox reactions
transfer of electrons
48
New cards
acid-base reactions
transfer of protons
49
New cards
precipitation reactions
formation of insoluble solids
50
New cards
titrations
finding equivalence point for acid-base reactions
51
New cards
rates of reaction
The rate at which reactants turn into products.
52
New cards
rate laws
* Relates to the concentration of reactants and the reaction order.
* rate = k(concentration of reactants)
53
New cards
integrated rate law
time affects concentration of reactant
54
New cards
collision theory
* collide in right orientation
* collide with enough energy
* faster this happens, the faster reaction rate.
55
New cards
reaction mechanisms
elementary reactions that describe steps in reaction
56
New cards
rate determining step
* slowest step of reaction
* limits reaction
57
New cards
specific heat
energy required to raise the temperature of 1g of a substance by 1°C.
58
New cards
enthalpy of reaction
ΔH, the amount of heat absorbed or released by a reaction.
59
New cards
calorimetry
* Experimental way to measure the enthalpy of reaction
* q=mCΔT
60
New cards
Hess’ Law
The total enthalpy of reaction is a sum of the enthalpies for each step.
61
New cards
enthalpy of formation
The change in enthalpy of forming 1 mole of a compound.
62
New cards
bond enthalpy
ÎŁ energy of bonds broken - ÎŁ energy of bonds formed
63
New cards
equilibrium conditions
* forward rate = reverse rate
* concentrations are constant
64
New cards
equilibrium expression and constant
* ratio of products to reactants at equilibrium
* signified by K
65
New cards
reaction quotient
* ratio of products to reactants at any point in reaction
* signified by Q
66
New cards
solubility product
* Ratios/products of soluble compounds.
* soluble: Na, K, NH4 + , and nitrate salts, SPAN
67
New cards
Le Chatelier’s Principle
* add concentration: shift to other side
* dilute concentration/add volume: shift toward side with more species
* increase temperature
* endothermic: shift toward product
* exothermic: shift toward reactant
* decrease temperature:
* endothermic: shift toward reactant
* exothermic: shift toward product
* decrease volume/increase pressure: shift to side with least moles of gas
* increase volume/decrease pressure: shift to side with more moles of gas
68
New cards
acids
* produce H+
* H+ donors
* strong: completely dissociate into ions in water
69
New cards
bases
* produce OH-
* H+ acceptors
* strong: completely dissociate into ions in water
70
New cards
acid and base dissociation constant
* less than 1, reaction favors the reactants.
* If greater, favors products.
* signified by Ka/Kb
71
New cards
percent dissociation
(change in concentration/initial) x 100
72
New cards
Henderson-Hasselbach Equation
used to find equivalence point
73
New cards
titration curves
pH v volume of titrant added
74
New cards
equivalence point
* pH = pKa
* (HA) = (A-)
75
New cards
entropy
* delta S
* disorder
* The amount of entropy will always increase over time.
76
New cards
Gibbs Free Energy
* Available energy that can be converted into work
* Spontaneous = -ΔG = Thermodynamically favorable
77
New cards
voltaic cells
* spontaneous reactions
* positive cell potential
78
New cards
standard cell potential
potential energy difference between electrodes in volts
79
New cards
salt bridge
* balances charge
* anions flow to anode
* cations flow to cathode
80
New cards
electrolytic cells
* requires outside energy force
* I = q/t
81
New cards
strong acids
HCl, HBr, HClO4, HI, HNO3, H2SO4
82
New cards
strong bases
LiOH, NaOH, KOH, Ca(OH)2, Sr(OH)2, Ba(OH)2
83
New cards
solubility rules
* soluble
* group 1 elements
* NH4+, NO3-, salts with Cl-, Br-, or I-
* except AgCl, PbBr2, Hg2Cl2
84
New cards
London Dispersion Forces
* present in all molecules
* nonpolar
85
New cards
Dipole-Dipole Forces
* polar
86
New cards
hydrogen bonds
* FON
* polar
87
New cards
heating diagram
* use q = (moles)(delta H of fusion/vaporization) for change in temperature
* use q= mcat for phase change
88
New cards
sig fig rules
* non-zero digits are always sig
* zeroes in between sig digits are sig
* leading zeroes are never sig, regardless of whether or not it comes after decimal point
* zeroes are only sig if they follow decimal point
89
New cards
phase diagrams
* triple point: where solid, liquid, and gas all exist
* critical point: liquid and gas coexist, weird stuff happens above this
90
New cards
ideal gas law
* PV=nRT
* increase volume = decrease pressure
* decrease volume = increase pressure
* use when big volumes, low pressure, high temperature!
91
New cards
vapor pressure
* collecting gas over pressure
* Ptot - vapor pressure = partial pressure
* vapor
92
New cards