Chem Kaplan And DATB review Flashcards
(206 cards)
1
Q
Glassware can be made of
A
plastic, or rubber. if organic, can’t use plastic
2
Q
round bottom flask adv
A
- used for reaction, heating or vaccuum applications
- allow it to be clamped and heated
3
Q
retort glassware adv
A
- used for distillation and must be placed in a stand
- the weird round thing with a handle
4
Q
separatory funnel adv
A
- used to separate by polarity
5
Q
funnel adv
A
used for large amounts
6
Q
transfer pipets
A
made of plastic
7
Q
pasteur pipets
A
made of glass. require a separate bulb
8
Q
bell jars
A
contain vaccuums
- (upside down lid thing)
9
Q
watch glasses
A
AKA evaporating dish
- covers beaker (the concave thing)
10
Q
meniscus of graduated cylinder
A
- if meniscus is concave, then its attracted to glass
- convex if its not (like mercury)
11
Q
buret adv
A
used for titrations and drop by drop stuff
12
Q
volumetric pipet adv
A
deliver single volume with lots of precision and accuracy
13
Q
volumetric flask
A
used to make molar solutions
14
Q
pH determination by probe
A
more points measured is more accurate
15
Q
litmus paper
A
red under acid (less than 4.5)
blue in basic (greater than 8.3)
16
Q
analytical balance
A
the door one. very precise
17
Q
how to use bomb calorimeter
A
can be constant pressure or constant volume
- heat the thing up and measure change in water
18
Q
** don’t need to use the most precise instrument all the time
A
bruh
19
Q
Dalton’s atomic theory
A
- elements are made of atoms
- compounds have more than one element
- reaction leaves atoms the same
20
Q
protons weigh
A
a lot
21
Q
smaller the distance between orbitals, the __ the energy
A
higher
22
Q
heisenberg uncertainty
A
more you know about momentum, the less you know about position
23
Q
pauli exclusion principle
A
ONLY ONE e can have a certain number
24
Q
parallel spins
A
having both + or - spin
25
paired spins
opposite spins
26
aufbau principle
old man says must be filled from low energy first
27
Hund's rule
fill one up spin first
28
** always write out electron configuration
YES
29
COLUMN
is downward
30
representative elements
S or p sublevels
31
nonrepresentative elements
f and d
32
alkaline earth metals have ___ electron affinity
low
33
mentally think about the metalloids
staircase
34
PLEASE DEAR GOD memorize the polyatomic ions
see screenshot
35
group 0 is
noble gases
36
terra
10^12
37
giga
10^9
38
mega
10^6
39
kilo
10^3
40
centi
10^02
41
mili
10^-3
42
micro
10^-6
43
nano
10^-9
44
percent error
actual - theoretical/ theoretical
45
parallax error
misreading meniscus
46
beer Lambert law
absorbance = length, concentration and E (higher for bright colours)
- absorbance and concentration are proportional
47
percent composition steps
1) assume 100g
2) get moles
3) divide answers by smaller # of moles
4) multiply to get whole #s
48
BCC stands for
balance, convert ALL to moles, coefficient
49
*** convert everything to moles
yes
50
transition metals
brightly coloured due to d orbitals
51
*** use electron configuration to determined para or dia
yes
52
photon energy
more energy = more frequencies = less wavelength
53
photoelectric effect
energy of E = E photon - e excitation
54
exceptions to octet rule
- Li and Be, B and elements beyond phosphorus and sulfur
55
bond length
more bonds means less bond length
56
bond energy
stronger bond if its shorter
57
So4 2- resonance
** has 6 structures since S can accept more
58
coordinate covalent bond use
found in Lewis acid and base
59
lewis acid
accepts an electron pair to form a covalent bond
60
lewis base
a compound that can donate an electron pair to form a covalent bond
61
sigma bond overlap is from
two orbitals overlap head to head
62
pi bond overlap is from
parallel p orbitals interact
63
hydrogen bonding
- must have an H bonded to FON to bond
64
when arranging compounds in order of boiling pt or something
PLEASE WRITE OUT THEIR FORCES
65
to find paramagnetic
add up valence electrons, and if odd number, then its paramagnetic
66
careful that if double bonds have resonance, they are weaker than no resonance
co2, vs co3
67
use mol highway in yield problems
YES
68
group 1
low ionization energy, react with h20, form metal hydroxides
69
group 2
low ionization energy, get more reactive with water as you move down
70
transition metals
brightly coloured with many ox states
71
molality
moles solute / kg solvent
72
soluble compounds
group 1, NO3, CLO4, acetate, and nh4
73
insoluble compounds
ag, pb, s, oh, hg, co3, and PO4
74
metathesis reaction
is also double displacement
75
reducing agent or reductant
is oxidized
76
oxidizing agent or oxidant
is reduced
77
Oxygen oxidation number
when more electronegative atom like F it is not -2, but +2
| - also in peroxides it is -1
78
oxidation is at the
Anode
79
galvanic cells are
spontaneous with a -ve delta g
80
cations from the salt bridge flow to the
cathode
81
shorthand cell diagram
on left is anode, then anode solution. right is cathode solution then anode
82
electrolytic cells
positive delta G and therefore nonspontaneous
83
SHE e cell
0
84
higher E cell means
reduction
85
delta g with faraday eqn
delta G (in J) = - n FEcell
86
faraday constant value
96500
87
Nernst equation e cell from e standard
E cell = E standard cell - (0.06/n)(lnQ)
88
draw a reaction diagram when given
energies and stuff
| - delta H is difference between products and reactants
89
half life eqn AKA decay constant
0.693/k
90
catalyst does
increase rate of forward and reverse rxns
| - sometimes induce steric strain on a molecule
91
factors affecting reaction rate
MEDIUM affects too!
92
isolated system
can't exchange matter or energy
93
standard conditions
298K, 1 atm, 1 M
| *** not STP as this is used for NOT gases
94
enthalpy of formation
is the 0 one where its PR
95
bond enthalpy
R-P usually positive
96
entropy calculation
products - reactants
| - positive means that it increases disorder
97
gibbs free energy eqn
delta G = H - t s
98
negative delta g
spontaneous rxn
| - zero means equilibrium
99
when delta h is negative and s is positive
spontaneous all the time
100
when delta h is positive and s is negative
nonspontaneous
101
when both delta h and s are positive
spontaneous at HIGH T only
102
when both delta h and s are negative
spontaneous at LOW t
103
delta G rxn
products - reactnats
104
Isobaric process
constant pressure system
105
isochoric process
constant volume system
106
isothermal system
no change in temp system
107
adiabatic system
no heat exchange system
108
delta G can also be used for
work
109
C of water with calories
1 calorie!
110
when reaction Q is less than K, G is
negative!
| reaction proceeds forward
111
when reaction Q is greater than K, G is
positive and reaction proceeds in reverse
112
rate units
just s-1
rate has a thing of just M, not m/s
113
integrated rate law 0
[A] and slope is -k
114
integrated rate law 1
ln[A] slope is -k
115
integrated rate law 2
1/[A] and slope is K
116
see notes for curved rate law
**
117
Arrhenius eqn
increase temp, increase K means increase rate
| - decrease Ea means increase K
118
what can change k
only temp
119
reverse Keq is
inverse
120
finding molar solubility with ksp
write out eqn, then assume 1 molar concentration for the compound!!!
121
COMMON ion effect
write out eqn of what's added
| - ICE
122
precipitation calculation
eqn, see if Q> ksp
| - if it is, then PRECIPITation happens
123
simple cubic
1 atom
124
face entered cubic
4 atm
125
body centred cubic
2 atom
126
phase changes going to gad
positive delta H and increase in delta s
127
boiling pt
when valour pressure equals external pressure
128
at sea level
The boiling point is lower at sea level because you experience less atmospheric pressure
129
at lower altitudes
higher pressure and higher bp
130
specific heat capacity and graph
is the slope. higher slope is higher C
131
Kelvin eqn
T plus 273
132
1 cm3 to ml
1 ml
133
1atm to torr and mmhg
760
134
ideal gases
ideal at low pressures and high temp
135
real gas law corrects for
IMP and repulsions
136
gases: volume and pressure
Boyle: volume up, pressure down
137
gases: volume and temp
Charles: both increase
138
gases: moles and volume
Avogadro: volume up as moles up
139
combined gas law
PV/ NT
140
ideal gas law
pv= nRT
| R is 0.0821 L atm / mol K
141
STP
273 K and 1 atm
142
at stp, gases are volume
22.4L
143
Density eqn for gases
Pressure times MM/ RT
| ** useful for Gas id
144
dalton's law
add up P of gas to find total
| ** to find one, multiply fraction by total
145
graham's law
Rate 1/ rate 2 = Sqrt M2 / M1
146
colligative properties
freezing point down, boiling pt up
| * use m not M
147
higher i in colligative
means higher colligative property!
148
Boiling point Raoult's law
P solution = XaPa + XbPB
x is mol fraction
pa is vp pressure
149
osmotic pressure eqn
IMRT
| R is 0.0821
150
Henry's law
gas pressure is proportional to the amount of dissolved gas in a liquid
- more pressure means more gas
- Pa = kh [A]
151
crystaline solids
ordered structure
152
amorphous solid
disordered
153
ionic compound properties
high melting and bp, hard and brittle
| use lattice energy
154
molecular solid
low MP, no e conduction
uses IMF
ex. Water
155
network covalent
VERY HIGh Mp, bp
network of covalent bonds
C, sio2
156
metallic solid
conduct e, shiny,
use metallic bonds
iron, mg
157
lattice energy
energy required to separate an ionic compound
158
in phase diagram if given a RANGE of temp, solid is
amorphous
159
when calculating Tf and Tb remember
THAT ITS JUST CHANGE
| - must subtract (freezing) or add from 0 to get actual freezing or boiling pt
160
Arrhenius acid
H and Oh
161
bronstead Lowry bases
H+ donor and receiver
162
lewis acid
electron donor and acceptor
163
strong acid
HI, Her, ccl, hclo4, hclo3, h2so4, Hno3
164
strong base
group 1, Mg, Ca,Sr and Ba OH
165
strongest acid is?
Hi
166
Oxyacid trend is?
more O2 is higher acidity because it increases the stability of acid's conjugate. base
167
remember pH
SAME with pOH
| LOWEr when it's 3.2 x 10-5
168
weak acid H+ concentration shortcut
H+ = sort of ka times HA
169
weak base OH- concentration shortcut
OH-= sqrt Kb times A-
170
Ka and acid
larger Ka means smaller pKA and stronger acid
171
which salts are neutral cations
group 1,2, and metals with +
172
which salts are neutral anions
strong acid anions
173
acidic/ basic salts
cations usually acids, anions are basic. **Hs04 is acid, F- is basic
174
how to increase solubility with pH
- see if comp is acid or basic
| - ex. adding acid lowers pH so eq becomes more BASIC
175
how to make a buffer
- 1:1 ratio of weak acid and Cb
- 2:1 ratio of weak acid and SB
- work at +/-1 of desired range
176
buffer eqn
Pka + Log [A-]/[HA]
177
diprotic major species then pH is less than Pka1
H2a dominates
178
diprotic major species then pH is between Pka1 and pka2
HA- dominates
179
diprotic major species then pH is more than Pka2
then A2- dominates
180
delta E and w
delta E = q+ w
181
work and volume
w= -p delta v
182
conduction
heat transfer via agitation of material
183
convection
heat transfer due to motion of fluid
184
radiation
heat transfer via electromagnetic radiation
185
bomb calorimeter eqn
q= -c delta T
186
c in graph is
the /. more slope is more c
187
bond energy
R-P
188
delta G and k
delta g= - RT ln eq
| * 8.314
189
delta g standard to delta g
delta g= delta G standard + RT ln Q
190
when k is greater than one, what is delta g
spontaneous, -ve
191
if e cell increases in Nernst eqn, then eq
is shifted right
192
electroplating qn
Current times Time in S/ Moles (F)
193
nuclear binding energy
```
E= Mc^2
c= 3 x 10^8
```
194
converting amu to kg
1 g/ 6.022 x 10^23 times 1 kg/ 1000 g
195
most stable nuclear is
Fe 56
196
vp and boiling point of two things is?
between them
197
watch x squared and KSP
please
198
watch wording on pH questions
please
199
Titrant
is what u know, so ITS NOT THE CURVE
200
when determining H and S signs,
just write out the eqn
201
Bomb calorimetry is different from specific heat
watch eqn
202
Phase change on graph is
FLAT PART
203
Watch wording and DON”T ASSUME in redox reactions
please
204
when comparing standard reduction potentials, switch them to be the same - or +
please
205
MORE POSITIVE REDUCTIoN POTENTIAL MEANS MORE LIKELY TO BE REDUCED
lol
206
nuclear capture reaction
A nuclear capture reaction, otherwise known as nuclear fusion, involves the combining of two or more reactants to make a single product and energy.
