THINGS TO MEMORIZE Flashcards
(114 cards)
1
Q
what are the 7 diatomic elements
A
Have No Fear Of Ice CoLd BeeR
Hydrogen
Nitrogen
Fluorine
Oxygen
Iodine
Chlorine
Bromine
2
Q
what the charges for Al, Zn and Cd, and Ag
A
Al = +3
Zn and Cd = +2
Ag = + 1
3
Q
what are the 7 strong acids
A
hydrochloric acid = HCL
hydrobromic acid = HBr
hydroiodic acid = HI
chloric acid = HClO3
perchloric acid = HClO4
nitric acid = HNO3
sulfuric acid = H2SO4
4
Q
what are the important SI units
A
Terra = 10^12
Giga = 10^9
Mega = 10^6
Kilo = 10^3
Centi = 10^-2
Milli = 10^-3
Micro = 10^-6
Nano = 10^-9
5
Q
what is a spectrophotometer
A
measures soln’s concentration with light
6
Q
what are separatory funnel used for
A
extract (separate) heterogenous mixture in polar (aqueous) vs. nonpolar (organic) layers
7
Q
what are condensers
A
used for distillation (seperates homogenous liquids)
8
Q
what is a centrifuge
A
seperates heterogenous mixtures based on density (spin at high speed)
9
Q
what is lab equipment is often used for titration
A
erlenmeyer flask
10
Q
what is a burette
A
transfers precise amount of liquids (titration)
11
Q
what is a volumetric pipet
A
measures very accurate liquid volumes (only measure one specific volume)
12
Q
what is the order of least accurate to most accurate lab equipment
A
beaker and erlenmeyer –> graduated cylinder –> buret –> volumetric flask –> volumetric pipet
13
Q
density formula
A
mass / volume
14
Q
% error formula
A
|(actual - theoretical) / theo| x 100
15
Q
why do we add the acid to water
A
when strong acid dissolves in H2O its exothermic releasing lots of heat and water helps disperse the heat
16
Q
% yield formula
A
(actual = given in problem) / (theoretical (calculated from LR)) x 100
17
Q
how to find % comp when given formula
A
- find total mass of comp
- find element your looking for and it’s total mass within comp
- (element mass / total mass) x 100
18
Q
how to find % comp given %’s
A
- assume 100g (17.3% –> 17.3)
- (grams (%)) / element mass = #
- divide by wtv number was smaller in prev step
- if not close to whole # mulitply by 2 or 3
19
Q
how to go from empirical –> molecular form
A
- find molecular weight of comp
- molecular / empirical = #
- multiply # in prev step to subscripts
20
Q
what is the photon and wavelength equation
A
Ephoton = hf = hc / wavelength
21
Q
what is the kinetic energy of a photon equation
A
Kinetic energy photon = Ephoton - work function
22
Q
what are the electron configuration exception
A
Cr = [Ar] 4s1 3d5
Mo = [Kr]5s1 4d5
Cu = [Ar]4s1 3d10
Ag = [Kr] 5s1 4d10
Au = [Xe]6s1 5d10
23
Q
whats the difference between paramagnetic and diamagnetic
A
para = unpaired e- (magnet) ODD number of e-
dia = paired (NO magnet) even or odd
24
Q
what is the order of radiation from long–> short wavelength
A
radio (least energy –> micro –> infrared –> visible –> ultraviolet –> x-rays –> gamma (shortest wave = most energy)
25
what is polar vs nonpolar
polar = more OH bonds (truck moves) soluble in H2O and polar solvent
- unequal sharing of electrons
- significant difference in electronegativity
nonpolar = more CH bonds (truck NO move) soluble in NONPOLAR (hexane, benzene, toluene)
- equal sharing of electrons
- no significant difference in electronegativeity
26
what are characteristics of ionic compounds what holds them together
high MP and BP (brittle and hard)
ionic interactions (lattice)
EX: NaCl and MgO
27
what are characteristics of molecular compound and what holds them together
low MP and no electricity
intermolecular forces
H2O / Cl2 / CH2w
28
what are characteristics of network covalent and what holds them together
high MP and BP, hard, NO electricity
network of covalent bonds
EX: diamond, graphite, SiO2 (quartz)
29
what are characteristics of metallic compounds and what holds them together
variabile in hardness and MP
conduct heat/electricity
luscious (shiny), malleable, and ductile
metallic bond
Fe Mg
30
what is molarity equation
moles solute / soln volume (L)
31
molar mass equation
compound mass / moles compound
32
molality equation
mol solute / kg solvent
33
rank single / double / triple bon from strongest to smalles
single < double < triple
34
which is diamagnetic and paramagnetic between O2 and N2
O2 = PARA
N2 = DIA
35
what are the exceptions of valence electrons for lewis structures
H = only needs 2
B and Al = only needs 6
Be = only needs 4
36
Metals have low ____ energies and ____ so they tend to ___ electrons and form ____ charged ions.
low ionization energies and electronegativity so they lose electrons and form positively charged ions (CATIONS)
37
Which of the following explains why along the same period, halogens have a smaller atomic radius than alkali metals?
halogens have a greater effective nuclear charge because they are nonmetals
38
what is electron affinity
energy released when atom gains an electron
39
which group requires extra precaution in a lab setting
alkali (group 1) metals
40
what is the trend for increasing ionization energy
increases as we go up and right in the periodic table
41
what bonds have greatest bond dissociation
bonds b/w smaller atoms = stronger = higher bond dissociation
42
what is the trend for ion radii of the same element
give e- (- charge) = larger
take e- (+ charge) = smaller
43
what is the relationship between protons and atomic size
more protons = smaller
44
what is the trend for electronegativity and melting points
large electronegativity difference = increaseing ionic character = increase MP
45
what element gives a STINKY scent
sulfur (specifically SULFIDE (2-))
46
elements with low ionization energy form ____ compunds
low ionization = ionic compounds
47
what are characteristics of alkali metals
1. low ionization (easy to remove e-)
2. react with H2O and pure oxygen vigorously
3. form IONIC compounds
4. reaction with H2O is EXOTHERMIC (BOOM)
5. LOW MP
48
what are characteristics of alkaline earth metals
1. low ionization but not as low as alkali
2. react with H2O and pure oxygen but not as violently
3. more reactive with H2O as you go down a group
49
what are the characteristics of halogens
1. high electronegativity and e- affinities
2. only one valence e-
3. easily REDUCED and want an extra e-
4. reactive with metals good oxidizing agent
50
what are the characteristics of noble gases
INERT (UNREACTIVE) b/c it's happy with its full octet
51
what are the characteristics of transition metals
1. brightly colored compounds because of partially filled d-subshells (promoted to higher energy levels)
2. multiple oxidation states
52
what are the characteristics of the oxygen group "chalcogens"
1. 2 forms of molecular oxygen (O2 and O3)
2. O2 = good oxidizing agent and O3 = even better
3. metals love reacting with O to form metal oxides (EX: Li2O)
53
what are characteristics of nonmetals metals and metalloids
non = dull / low MP / poor conductivity
metal = metallic / high MP / good conductivity
metalloid = props of both metal and non-metal, high MP and semi-conductive
54
what is the formula for pressure
force / area
inc pressure = inc force = dec area
55
1 atm = ___ torr = ___ mmHg
1 atm = 760 torr = 760 mmHg
56
what are the 5 assumptions for the ideal gas law
1. gas particles' volumes insignificant compared to volume of gas (most accurate at LOW pressures)
2. gas particles experience ZERO INTERmolecular forces w/ each other and container (most accurate at HIGH temp and LOW pressure
3. gas particles are always continously / rapidly / randomly moving
4. gas molecules collision are perfectly elastic = ZERO LOSS or GAIN of kinetic energy (no attractive or repulsive forces)
5. avg kinetic energy (Ek) of gas depends on systems TEMP
57
what is Boyle's Law
volume and pressure are inversely related
dec vol = inc pressure
58
what is Charles Law
volume is directly proportional to temp
inc vol = inc temp (molecules move faster)
59
what is Avogadro's Law
volume directly proportional to number of gas molecules (n)
inc vol = inc n
60
what is the combined gas law
P1V1 / n1T1 = P2V2 / n2T2
61
what is the ideal gas law
PV = nRT
R = 0.0821 L * atm / mol * K
62
what is STP
standard temp = 273 K and pressure = 1 atm (760 torr)
1 STP = 22.4 L
63
what is Daltons Law of Partial Pressure
total pressure inside container = sum of individual gas pressures
64
what is the formula for partial pressure
P molec = mol fraction x P total
65
what is Graham's law of effusion and what is the formula
lighter gases = escape quickly
heavier gases = escape slowly
rate 1 / rate 2 = sqrt (mass 2 / mass 1)
66
as temperature of gas is lowered what increases
rate of condensation
67
what temperature does volume of an ideal gas equal 0
- 273 C
(-273 + 273) = 0
68
what does it mean when temperature and gas is in a SEALED container
they are DIRECTLY PROPORTIONAL
if one goes up so does the other
69
what happens to molecules when pressure of gas increases and volume decreases at constant temperature
molecules strike container more because they are colliding with each other
70
what does it mean for a gas when a container is rigid or sealed
rigid = volume and moles constant
sealed = volume constant
71
what are examples of intramolecular forces and intermolecular
INTRA
- metallic
- ion-ion
- network covalent
INTER
- hydrogen bonding (N/O/F)
- dipole dipole
- dispersion (hydrocarbons) or NONPOLAR
72
what is the order of strongest forces (weak --> strong)
dispersion --> dipole --> hydrogen --> ionic dipole
73
what is the characteristic of dipole force
polar (high electronegativity difference) with nonmetal + nonmetal
- double bonds
74
what's important to note about dispersion forces in terms of BP
high BP = high molecular mass
75
if there is strong intermolecular, how does that correlate to BP, viscosity, surface tension, vapor pressure
high BP
- increased vaporization
high viscocity
- thicker = slower
high surface tension LOW vapor pressure
- DIRECTLY related to temp (high temp = high vapor pressur)
76
what happens when vapor pressure becomes equal to or exceeds atmospheric pressure
liquid goes to gas because molecules escape = low BP = low temp
77
how many atoms are in each unit cell for simple cubic
body-centered cubic
face-centered cubic
simple = one total
body centered = 2 per cell (8 corners x 1/8) + 1 center atom
face-centered = four total per cell (8 corners x 1/8) + (6 faces x 1/2)
78
what is it called for the transition of each of these
solid --> liq
liq --> gas
solid --> gas
gas --> liquid
liquid --> solid
gas --> solid
s --> l = melting (fusion)
l --> g = vaporization (boiling)
s --> g = sublimation
g --> l = condensation
l --> s = crystallization (freezing)
g --> s = deposition
79
what phase changes consume heat and which release? what are the delta H and S?
CONSUME HEAT
- fusion
- vaporization
- sublimation
(ENDOTHERMIC = +H, disorder = +S = + entropy)
RELEASE HEAT
- crystallization
- condensation
- deposition
(EXOTHERMIC = -H = orderly = -S = - entropy (spontaneous)
80
what is the normal BP for a substance
temperature of substance boils (l ->g) at 1 atm
81
what does volatity mean
how easily a liquid vaporizes (high vapor = dec. forces)
82
what is a good definition for boiling
pressure exerted by the liquid molecules upward (vapor) equals the pressure exerted by the pressure down upon the liquid molecules (atmospheric)
83
what ionic compounds will be soluble (aq) in H2O (solubility rules)
1. group 1 metals
2. nitrate (NO3-)
3. perchlorate (ClO4-)
4. acetate (C2H3O2-)
5. ammonium (NH4+)
84
what ionic compounds are INSOLUBLE (s) in H2O (solubility rules)
1. silver (Ag+)
2. lead (Pb 2+)
3. sulfide (S2-)
4. hydroxide (OH-)
5. dimercury (Hg2 2+)
6. carbonate (CO3 2-)
7. phosphate (PO4 3-)
85
what are the trend for solid solubility and temperature
increase temp = increase solubility
86
what are the trend for gas solubility and temperature and pressure
increase temperature = increase pressure = decrease solubility
87
what is henry's law and it's equation
sealed vessel with dissolved gas (pressure and conc proportional)
Pa = kh [A]
Pa = gas pressure
kH = constant
[A] = gas conc mol / L
88
what is the trend for solutes and their FP and BP
increase solute = decrease freezing pt (more things)
increase solute = decrease boiling pt
89
what is the freezing point equation and freezing point depression equation
delta Tf = iKfm
depression: delta Tf = Kf(m)
90
what is boiling point equation
delta Tb = iKbm
(multiple "things" with m)
91
what occurs to osmotic pressure, vapor pressure, BP and FP when solute is added to liquid
osmotic pressure = increase
vapor pressure = decrease
boiling point = increase
freezing point = decrease
92
what is Raoult's Law and its equation
one or more solutes (s) or (l)
PA = XA x Ppure
Pa = solns new vapor pressure
Xa = % of solvent
Ppure = solvent pure
93
what is rate law equation
rate = k[A]^m [B]^n
94
what are the units for K for rate law for
zero order
1st order
2nd order
3rd order
zero = M1 x s-1
first = s-1
second = M-1 x s-1
third = M-2 x s-1
95
what is the order of the rxn for integrated rate laws for straight line on y-axis
0 order
1st order
2nd order
0 = [conc]
1 = ln[conc]
2 = 1 / [conc]
96
what is delta H in a rxn coordinate diagram? what is the common trend
difference between energy levels of reactants / products
delta H = Eprods - Ereacts
- products lower than reacts = -H = exothermic = hot
- products higher than reacts = +H = endothermic = cold
97
what is delta E (Eactiavtion) mean in a rxn coordinate diagram and what is the usual trend
height between reactants and top of the hill
exothermic = Ea-reverse LARGER than Ea-forward
endothermic = Ea-reverse SMALLER than Ea-forward
98
How is the rate of a reaction studied?
measuring the concentrations of the reactants and products over time
99
What describes the overall activation energy of a reaction?
the difference in energy between the reactants and highest point in the reaction path
100
what is the plot for zero order kinetics and the relation between half life and conc.
straight line plot
half-life and conc are directly proportional
101
what is the plot for first order kinetics and the relation between half life and conc.
NOT. straight line
half-life is INDEPENDENT of concentration
102
what is the plot for second order kinetics and the relation between half life and conc.
not a straight line
half-life and concentration are inversely proportional
103
what is the equation for integrated rate law zero order, 1st order, and 2nd order
0: [A]t = -kt + [A]0
1. ln[A]t = -kt + ln[A]0
2. 1 / [A]t = kt + 1 / [A]0
104
what three things need to occur between 2 molecules for a reaction to occur
1. both molecules must collide with each other
2. molecules need to collide with enough energy for reaction to happen
3. molecules need to hit each other with correct 3-D orientation
105
what is the trend between temperature and rate constant k?
increase temp = increase k = increase rxn rate
106
what is the trend between activation energy and rate constant k?
lower Ea = higher k = higher rxn rate
107
what is the rate of disappearance formulae
- (delta [A]) / delta time)
108
what is the equilibrium rate constant for a generic equilibrium rxn
Kc = [C]^c [D]^d / [A]^a [B]^b
109
what are the 4 important Kc details
1. Kc has NO units
2. solids and liquids are NOT included in Kc expression
3. Kc is equilibrium constant in terms of concentration = Molarity (mol solute / L soln)
4. only TEMP can change equilibrium constant
110
what is the equation for Kp equilibrium constant expression
Kp = (Pc)^c (Pd)^d / (Pa)^a (Pb)^b
111
what does is mean when K > 1 and K < 1
K > 1 = products favored
K < 1 = reactants favored
112
What is the equation for Qc
[B may or may not be at equilibrium] / [A may or may not be at equilibrium]
113
what does it mean when Q > K, Q < K, Q = K
Q > K: not at equilib; Q is too big; too much product = shift left
Q < K: not at equilib; Q too small; too much reactants = shift right
Q = K: equilibrium :)
114
what are the kinds of disturbances for LeChat Principle
1. adding/removing reactants and products
2. change temp (increase temp = increase heat)
3. change volume and pressure (dec vol = increase pressure = shift with fewer gas molecules)
4. adding catalysts (do NOT shift equilibrium)
