Ultimate Guide Flashcards
(161 cards)
1
Q
A
2
Q
electrostatic force
A
attraction between opposite charges and the strength can vary depending on how far the charges are from each other.
3
Q
subshell
A
shape of the space an electron can be found in
4
Q
ionization energy
A
the energy an atom must absorb to eject an electron
5
Q
aufbau principle
A
electrons must fill up orbitals, subshells, and shells in order of increasing energy.
6
Q
electromagnetic radiation
A
electrons can jump to higher energy levels when absorbing this energy
7
Q
Bohr model
A
demonstrates the electron organization of an atom
8
Q
avogadro’s number
A
number of atoms in a single mole of any given element
9
Q
anions
A
have an overall negative charge
10
Q
cations
A
have an overall positive charge
11
Q
electronegativity
A
how much an element attracts electrons to it’s nucleus
12
Q
molarity (M)
A
expresses the concentration of a solution in terms of volume
13
Q
Coulomb’s law
A
the closer an electron is to the nucleus, the stronger the attraction and the less potential energy there is
14
Q
valence electrons
A
electrons in the outermost shell
15
Q
photoelectron spectrum
A
graph of the ionization energies for all electrons when ejected from the nucleus.
16
Q
electrons
A
have significantly less mass than protons and neutrons and do not contribute to the mass.
17
Q
isotopes
A
atoms of an element with different numbers of neutrons, but same amount of protons.
18
Q
percent compostition
A
percent by mass of each element in a compound.
19
Q
substitutional alloys
A
a molecule with a similar radius replaces a metal atom
20
Q
potential energy
A
stored, motionless energy
21
Q
kinetic energy
A
energy in motion
22
Q
covalent bond
A
between two nonmetals
23
Q
metallic bond
A
between two metals
24
Q
ionic bond
A
between a metal and nonmetal
25
interstitial alloy
an atom with a smaller radii fills the space between metal atoms with larger radii
26
network covalent bonds
strongest bond, held together in lattice structure
27
sea of electrons
electron organization for metallic bonds
28
resonance form
different yet equally likely forms of a molecule’s structure f
29
formal charge
the most likely version of a lewis dot structure to form
30
molecular geometry
three-dimensional structure of a molecules arrangement
31
london dispersion forces (LDFs)
IMF between all molecules, very weak attraction, caused by random electron movements
32
dipoles
oppositely charged ends of a molcule
33
effusion
the rate at which a gas will escape a pin-sized hole from high to low pressure
34
polar covalent bonds
an unequal share of electrons
35
nonpolar covalent bonds
equally shared electrons
36
dipole-dipole forces
IMF that occurs when a positive dipole of a molecule is attracted to the negative dipole of another molecule
37
hydrogen bond
IMF between hydrogen and oxygen, nitrogen, or fluorine
38
acid
a compound that can donate a proton
39
base
compound capable of accepting a proton
40
amphoteric
a compound that can behave as both an acid or a base
41
catalyst
a substance that speeds up a reaction rate
42
intermediate
a substance created in one elementary step and used up in another
43
half-life
how long it takes for half of a substance to decompose
44
activation energy
energy required for a reaction to start/occur
45
exothermic
when energy is transferred from system to surroundings (beaker feels hot)
46
endothermic
heat transfers from surroundings to system (beaker feels cold)
47
when bonds are formed, energy is ____
releasedw
48
when bonds are broken, energy is ____
absorbed
49
ΔH
enthalpy change
50
enthalpy
total heat content of a system (H)
51
enthalpy of formation
amount of energy released when one mole of a compound is produced from pure substances
52
reaction quotient, Q
the relative amount of products and reactants at any point in time
53
K
equilibrium constant
54
Le Chatelier’s Principle
when a stress is added to a reaction, the equation will change to adjust for the stress and return to equilibrium
55
common ion effect
when an element is added to a solution with a salt, the salt equilibrium will change if the element is similar to the salt
56
equilibrium reaction
reaction is reversible and constantly occurring with no change in concentrations of product or reactants
57
only ____ stress/change can change the equilibrium constant value
temperature
58
neutralization reactions
acid and base react, producing water and a salt
59
strong acid
dissolves completely in water
60
Kw value
1.0 x 10^-14
61
buffer solution
can resist pH change when small amounts of strong acid or base added
62
polyprotic acid
can give up more than one proton
63
equivalence point
just enough acid/base added to base/acid to neutralize
64
Gibbs Free Energy
G, determines thermodynamic favorability based on the entropy, enthalpy, and temperature
65
entropy
S, the disorder of a system, “chaos”
66
standard conditions
25 celsius, 1 atm, 1M
67
mass spectrometry
determine the average mass for different isotopes of a specific element
68
pauli exclusion principle
when two electrons fill up an orbital, they must spin in opposite directions: clockwise and counterclockwise.
69
hund’s rule
when electrons are filling the orbitals of the subshell, they will only have two in one orbital when it is not possible to have each electron in its own orbital.
70
noble gas
has all shells completely full of electrons
71
linear molecular geometry
two electron pairs
72
trigonal planar geometry
three electron pairs
73
tetrahedral electron geometry
four electron pairs
74
trigonal bipyramidal geometry
five electron pairs
75
octahedral geometry
six electron pairs
76
kinetic molecular theory
gases are composed of a large number of particles that behave like hard, spherical objects in a state of constant, random motion.
77
kinetic molecular theory does not work at ____ temperature
low
78
kinetic molecular theory does not work at ____ pressure
high
79
absorbance
the amount of light that does not get through (gets absorbed) by a colored solution
80
gravimetric analysis
used to determine an unknown element in a precipitate reaction
81
hydrocarbon combustion
carbon + hydrogen (and sometimes oxygen) is ignited and produces CO2 and waters
82
synthesis reaction
when elements or simple compounds are combined to form a single, more complex compound.
83
redox reaction
electrons are swapped between reactants and the oxidation states of the reactants are changed.
84
decomposition reaction
opposite of synthesis- occurs usually in the presence of heat
85
precipitation reaction
two aqueous solutions mixing to create a solid precipitate.
86
acid-base reaction
when an acid (H+) reacts with a base (OH)- to form water and a salt.
87
compounds with these 3 substances are ALWAYS soluble
alkali metals, ammonium, nitrate
88
any neutral atom not bonded has an oxidation state of ____
zero
89
a single atom has an oxidation state equal to ____
most common charge
90
he oxidation state of a compound is equal to the ____
total charge
91
when hydrogen is bonded to a nonmetal, it has an oxidation state of ____
1
92
when hydrogen is bonded to a metal, it has an oxidation state of ____
-1
93
Arrhenius Constant, k
based on the activation energy for a reaction and the temperature
94
first order rate law
log[A]=-kt+ln[A]₀
95
zero order rate law
rate = k
96
collision theory
reactions only occur when chemicals collide with each other with sufficient energy (activation energy)
97
second order rate law
1/[A] = kt+ 1/[A]₀
98
first order half life equation
t= .693/k
99
heterogenous mixture
not evenly mixed, not all parts are equal
100
homogeneous mixture
evenly mixed, all parts are equal
101
elementary step
the steps that occur in a reaction
102
a ____ concentration will cause a reaction to occur more
high
103
a ____ temperature will cause a reaction occur less
low
104
stirring will help a reaction occur if the mixture is ____
heterogeneous
105
first and zero order graphs have a ____ slope
negative
106
second order reaction has a ____ slope
positive
107
first order
rate = k[A]
108
second order
Rate = k[A]²
109
hess’s law
if a reaction can be broken into a series of steps, the sum of the ΔH of those steps are equal to the ΔH of the reaction.
110
____ remains constant during a phase change.
temperature
111
calorimetry
measurement of heat changes during a chemical reaction.
112
enthalpy of vaporization
how much energy is required to turn a liquid to a gas.
113
vapor pressure
amount of pressure given off by molecules as they go from solid /liquid to gas.
114
heat of vaporization
the energy given off when a gas condenses.
115
enthalpy of fusion
the amount of energy required to cause a solid to melt.
116
ΔHf°
enthalpy of formation
117
solid to gas phase change
sublimation
118
gas to solid
deposition
119
Ksp
solubility product constant
120
law of mass action
equilibrium expression that determines the relationship between reactant and product concentrations.
121
Kc
molar concentration constant
122
if Q = K
not shift
123
if Q < K
reaction shifts right
124
if Q > K
reaction shifts left
125
if a reaction shifts right, it makes more ____
products
126
if a reaction shifts left, it will make more ____
reactants
127
Ka
acid dissociation constant
128
Kb
base dissociation constant
129
If water evaporates from a solution with a salt, the reaction will shift to the side with ____
more mole aqueous
130
If water is added to a solution with a salt, the reaction will shift to the side with ____
less moles aqueous
131
If pressure is added to a container, the reaction will shift to the side with ____
less moles gas
132
If pressure is removed from a container, the reaction will shift to the side with ____
more moles gas
133
indicators
weak acids that change color based on pH change
134
pH + pOH =
14
135
[H+][OH-] =
Kw value (1 x 10^-14)
136
half-equivalence point
when exactly half of the amount of acid/base is turned into its conjugate in a titration
137
increased pH decreases ____
[H+]
138
as Ka value increases…
acid strength decreases
139
as Kb increases…
the base strength increases
140
Strong acid and strong base reaction results
complete dissociation, only hydrogen and hydroxide ions remain
141
strong acid and weak base reaction results
Proton is donated, conjugate of base is created
142
weak acid and strong base reaction
Protons accepted, created conjugate of acid and water
143
weak acid and weak base reaction
Simple proton transfer
144
positive ∆G
not TFP
145
negative ∆G
TFP
146
TFP meaning
thermodynamically favorable process
147
galvanic cells use ____ to generate current
redox reaction
148
electrolytic cells use ____ to generate current
outside voltage sources
149
oxidation takes place at the ____ electrode
anode
150
reduction takes place at the ____ electrode
cathode
151
Faraday’s constant value
96,500 coulombs/mol
152
cell total potential energy is always ____
negative
153
if a reaction goes from less moles reactants to more moles products, the ∆S values is ____
positive
154
If a reaction goes from liquid to gas, the ∆S value is ____
positive
155
positive ∆S
TFP
156
negative ∆S
not TFP
157
Gibb’s Free Energy Units
kJ/mol*K
158
negative ∆G, K >1, reaction favors ____
products
159
If ∆G is positive, K < 1, reaction favors ____
reactant
160
positive ∆H
not TFP
161
negative ∆H
TFP
