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DAT > Chem Kaplan And DATB review > Flashcards

Chem Kaplan And DATB review Flashcards

1
Q

Glassware can be made of

A

plastic, or rubber. if organic, can’t use plastic

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2
Q

round bottom flask adv

A
  • used for reaction, heating or vaccuum applications

- allow it to be clamped and heated

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3
Q

retort glassware adv

A
  • used for distillation and must be placed in a stand

- the weird round thing with a handle

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4
Q

separatory funnel adv

A
  • used to separate by polarity
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5
Q

funnel adv

A

used for large amounts

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6
Q

transfer pipets

A

made of plastic

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7
Q

pasteur pipets

A

made of glass. require a separate bulb

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8
Q

bell jars

A

contain vaccuums

- (upside down lid thing)

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9
Q

watch glasses

A

AKA evaporating dish

- covers beaker (the concave thing)

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10
Q

meniscus of graduated cylinder

A
  • if meniscus is concave, then its attracted to glass

- convex if its not (like mercury)

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11
Q

buret adv

A

used for titrations and drop by drop stuff

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12
Q

volumetric pipet adv

A

deliver single volume with lots of precision and accuracy

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13
Q

volumetric flask

A

used to make molar solutions

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14
Q

pH determination by probe

A

more points measured is more accurate

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15
Q

litmus paper

A

red under acid (less than 4.5)

blue in basic (greater than 8.3)

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16
Q

analytical balance

A

the door one. very precise

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17
Q

how to use bomb calorimeter

A

can be constant pressure or constant volume

- heat the thing up and measure change in water

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18
Q

** don’t need to use the most precise instrument all the time

A

bruh

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19
Q

Dalton’s atomic theory

A
  • elements are made of atoms
  • compounds have more than one element
  • reaction leaves atoms the same
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20
Q

protons weigh

A

a lot

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21
Q

smaller the distance between orbitals, the __ the energy

A

higher

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22
Q

heisenberg uncertainty

A

more you know about momentum, the less you know about position

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23
Q

pauli exclusion principle

A

ONLY ONE e can have a certain number

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24
Q

parallel spins

A

having both + or - spin

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25
Q

paired spins

A

opposite spins

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26
Q

aufbau principle

A

old man says must be filled from low energy first

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27
Q

Hund’s rule

A

fill one up spin first

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28
Q

** always write out electron configuration

A

YES

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29
Q

COLUMN

A

is downward

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30
Q

representative elements

A

S or p sublevels

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31
Q

nonrepresentative elements

A

f and d

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32
Q

alkaline earth metals have ___ electron affinity

A

low

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33
Q

mentally think about the metalloids

A

staircase

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34
Q

PLEASE DEAR GOD memorize the polyatomic ions

A

see screenshot

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35
Q

group 0 is

A

noble gases

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36
Q

terra

A

10^12

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37
Q

giga

A

10^9

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38
Q

mega

A

10^6

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39
Q

kilo

A

10^3

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40
Q

centi

A

10^02

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41
Q

mili

A

10^-3

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42
Q

micro

A

10^-6

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43
Q

nano

A

10^-9

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44
Q

percent error

A

actual - theoretical/ theoretical

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45
Q

parallax error

A

misreading meniscus

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46
Q

beer Lambert law

A

absorbance = length, concentration and E (higher for bright colours)
- absorbance and concentration are proportional

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47
Q

percent composition steps

A

1) assume 100g
2) get moles
3) divide answers by smaller # of moles
4) multiply to get whole #s

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48
Q

BCC stands for

A

balance, convert ALL to moles, coefficient

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49
Q

*** convert everything to moles

A

yes

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50
Q

transition metals

A

brightly coloured due to d orbitals

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51
Q

*** use electron configuration to determined para or dia

A

yes

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52
Q

photon energy

A

more energy = more frequencies = less wavelength

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53
Q

photoelectric effect

A

energy of E = E photon - e excitation

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54
Q

exceptions to octet rule

A
  • Li and Be, B and elements beyond phosphorus and sulfur
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55
Q

bond length

A

more bonds means less bond length

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56
Q

bond energy

A

stronger bond if its shorter

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57
Q

So4 2- resonance

A

** has 6 structures since S can accept more

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58
Q

coordinate covalent bond use

A

found in Lewis acid and base

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59
Q

lewis acid

A

accepts an electron pair to form a covalent bond

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60
Q

lewis base

A

a compound that can donate an electron pair to form a covalent bond

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61
Q

sigma bond overlap is from

A

two orbitals overlap head to head

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62
Q

pi bond overlap is from

A

parallel p orbitals interact

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63
Q

hydrogen bonding

A
  • must have an H bonded to FON to bond
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64
Q

when arranging compounds in order of boiling pt or something

A

PLEASE WRITE OUT THEIR FORCES

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65
Q

to find paramagnetic

A

add up valence electrons, and if odd number, then its paramagnetic

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66
Q

careful that if double bonds have resonance, they are weaker than no resonance

A

co2, vs co3

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67
Q

use mol highway in yield problems

A

YES

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68
Q

group 1

A

low ionization energy, react with h20, form metal hydroxides

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69
Q

group 2

A

low ionization energy, get more reactive with water as you move down

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70
Q

transition metals

A

brightly coloured with many ox states

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71
Q

molality

A

moles solute / kg solvent

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72
Q

soluble compounds

A

group 1, NO3, CLO4, acetate, and nh4

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73
Q

insoluble compounds

A

ag, pb, s, oh, hg, co3, and PO4

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74
Q

metathesis reaction

A

is also double displacement

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75
Q

reducing agent or reductant

A

is oxidized

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76
Q

oxidizing agent or oxidant

A

is reduced

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77
Q

Oxygen oxidation number

A

when more electronegative atom like F it is not -2, but +2

- also in peroxides it is -1

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78
Q

oxidation is at the

A

Anode

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79
Q

galvanic cells are

A

spontaneous with a -ve delta g

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80
Q

cations from the salt bridge flow to the

A

cathode

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81
Q

shorthand cell diagram

A

on left is anode, then anode solution. right is cathode solution then anode

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82
Q

electrolytic cells

A

positive delta G and therefore nonspontaneous

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83
Q

SHE e cell

A

0

84
Q

higher E cell means

A

reduction

85
Q

delta g with faraday eqn

A

delta G (in J) = - n FEcell

86
Q

faraday constant value

A

96500

87
Q

Nernst equation e cell from e standard

A

E cell = E standard cell - (0.06/n)(lnQ)

88
Q

draw a reaction diagram when given

A

energies and stuff

- delta H is difference between products and reactants

89
Q

half life eqn AKA decay constant

A

0.693/k

90
Q

catalyst does

A

increase rate of forward and reverse rxns

- sometimes induce steric strain on a molecule

91
Q

factors affecting reaction rate

A

MEDIUM affects too!

92
Q

isolated system

A

can’t exchange matter or energy

93
Q

standard conditions

A

298K, 1 atm, 1 M

*** not STP as this is used for NOT gases

94
Q

enthalpy of formation

A

is the 0 one where its PR

95
Q

bond enthalpy

A

R-P usually positive

96
Q

entropy calculation

A

products - reactants

- positive means that it increases disorder

97
Q

gibbs free energy eqn

A

delta G = H - t s

98
Q

negative delta g

A

spontaneous rxn

- zero means equilibrium

99
Q

when delta h is negative and s is positive

A

spontaneous all the time

100
Q

when delta h is positive and s is negative

A

nonspontaneous

101
Q

when both delta h and s are positive

A

spontaneous at HIGH T only

102
Q

when both delta h and s are negative

A

spontaneous at LOW t

103
Q

delta G rxn

A

products - reactnats

104
Q

Isobaric process

A

constant pressure system

105
Q

isochoric process

A

constant volume system

106
Q

isothermal system

A

no change in temp system

107
Q

adiabatic system

A

no heat exchange system

108
Q

delta G can also be used for

A

work

109
Q

C of water with calories

A

1 calorie!

110
Q

when reaction Q is less than K, G is

A

negative!

reaction proceeds forward

111
Q

when reaction Q is greater than K, G is

A

positive and reaction proceeds in reverse

112
Q

rate units

A

just s-1

rate has a thing of just M, not m/s

113
Q

integrated rate law 0

A

[A] and slope is -k

114
Q

integrated rate law 1

A

ln[A] slope is -k

115
Q

integrated rate law 2

A

1/[A] and slope is K

116
Q

see notes for curved rate law

A

**

117
Q

Arrhenius eqn

A

increase temp, increase K means increase rate

- decrease Ea means increase K

118
Q

what can change k

A

only temp

119
Q

reverse Keq is

A

inverse

120
Q

finding molar solubility with ksp

A

write out eqn, then assume 1 molar concentration for the compound!!!

121
Q

COMMON ion effect

A

write out eqn of what’s added

- ICE

122
Q

precipitation calculation

A

eqn, see if Q> ksp

- if it is, then PRECIPITation happens

123
Q

simple cubic

A

1 atom

124
Q

face entered cubic

A

4 atm

125
Q

body centred cubic

A

2 atom

126
Q

phase changes going to gad

A

positive delta H and increase in delta s

127
Q

boiling pt

A

when valour pressure equals external pressure

128
Q

at sea level

A

The boiling point is lower at sea level because you experience less atmospheric pressure

129
Q

at lower altitudes

A

higher pressure and higher bp

130
Q

specific heat capacity and graph

A

is the slope. higher slope is higher C

131
Q

Kelvin eqn

A

T plus 273

132
Q

1 cm3 to ml

A

1 ml

133
Q

1atm to torr and mmhg

A

760

134
Q

ideal gases

A

ideal at low pressures and high temp

135
Q

real gas law corrects for

A

IMP and repulsions

136
Q

gases: volume and pressure

A

Boyle: volume up, pressure down

137
Q

gases: volume and temp

A

Charles: both increase

138
Q

gases: moles and volume

A

Avogadro: volume up as moles up

139
Q

combined gas law

A

PV/ NT

140
Q

ideal gas law

A

pv= nRT

R is 0.0821 L atm / mol K

141
Q

STP

A

273 K and 1 atm

142
Q

at stp, gases are volume

A

22.4L

143
Q

Density eqn for gases

A

Pressure times MM/ RT

** useful for Gas id

144
Q

dalton’s law

A

add up P of gas to find total

** to find one, multiply fraction by total

145
Q

graham’s law

A

Rate 1/ rate 2 = Sqrt M2 / M1

146
Q

colligative properties

A

freezing point down, boiling pt up

* use m not M

147
Q

higher i in colligative

A

means higher colligative property!

148
Q

Boiling point Raoult’s law

A

P solution = XaPa + XbPB
x is mol fraction
pa is vp pressure

149
Q

osmotic pressure eqn

A

IMRT

R is 0.0821

150
Q

Henry’s law

A

gas pressure is proportional to the amount of dissolved gas in a liquid

  • more pressure means more gas
  • Pa = kh [A]
151
Q

crystaline solids

A

ordered structure

152
Q

amorphous solid

A

disordered

153
Q

ionic compound properties

A

high melting and bp, hard and brittle

use lattice energy

154
Q

molecular solid

A

low MP, no e conduction
uses IMF
ex. Water

155
Q

network covalent

A

VERY HIGh Mp, bp
network of covalent bonds
C, sio2

156
Q

metallic solid

A

conduct e, shiny,
use metallic bonds
iron, mg

157
Q

lattice energy

A

energy required to separate an ionic compound

158
Q

in phase diagram if given a RANGE of temp, solid is

A

amorphous

159
Q

when calculating Tf and Tb remember

A

THAT ITS JUST CHANGE

- must subtract (freezing) or add from 0 to get actual freezing or boiling pt

160
Q

Arrhenius acid

A

H and Oh

161
Q

bronstead Lowry bases

A

H+ donor and receiver

162
Q

lewis acid

A

electron donor and acceptor

163
Q

strong acid

A

HI, Her, ccl, hclo4, hclo3, h2so4, Hno3

164
Q

strong base

A

group 1, Mg, Ca,Sr and Ba OH

165
Q

strongest acid is?

A

Hi

166
Q

Oxyacid trend is?

A

more O2 is higher acidity because it increases the stability of acid’s conjugate. base

167
Q

remember pH

A

SAME with pOH

LOWEr when it’s 3.2 x 10-5

168
Q

weak acid H+ concentration shortcut

A

H+ = sort of ka times HA

169
Q

weak base OH- concentration shortcut

A

OH-= sqrt Kb times A-

170
Q

Ka and acid

A

larger Ka means smaller pKA and stronger acid

171
Q

which salts are neutral cations

A

group 1,2, and metals with +

172
Q

which salts are neutral anions

A

strong acid anions

173
Q

acidic/ basic salts

A

cations usually acids, anions are basic. **Hs04 is acid, F- is basic

174
Q

how to increase solubility with pH

A
  • see if comp is acid or basic

- ex. adding acid lowers pH so eq becomes more BASIC

175
Q

how to make a buffer

A
  • 1:1 ratio of weak acid and Cb
  • 2:1 ratio of weak acid and SB
  • work at +/-1 of desired range
176
Q

buffer eqn

A

Pka + Log [A-]/[HA]

177
Q

diprotic major species then pH is less than Pka1

A

H2a dominates

178
Q

diprotic major species then pH is between Pka1 and pka2

A

HA- dominates

179
Q

diprotic major species then pH is more than Pka2

A

then A2- dominates

180
Q

delta E and w

A

delta E = q+ w

181
Q

work and volume

A

w= -p delta v

182
Q

conduction

A

heat transfer via agitation of material

183
Q

convection

A

heat transfer due to motion of fluid

184
Q

radiation

A

heat transfer via electromagnetic radiation

185
Q

bomb calorimeter eqn

A

q= -c delta T

186
Q

c in graph is

A

the /. more slope is more c

187
Q

bond energy

A

R-P

188
Q

delta G and k

A

delta g= - RT ln eq

* 8.314

189
Q

delta g standard to delta g

A

delta g= delta G standard + RT ln Q

190
Q

when k is greater than one, what is delta g

A

spontaneous, -ve

191
Q

if e cell increases in Nernst eqn, then eq

A

is shifted right

192
Q

electroplating qn

A

Current times Time in S/ Moles (F)

193
Q

nuclear binding energy

A 
E= Mc^2
c= 3 x 10^8
194
Q

converting amu to kg

A

1 g/ 6.022 x 10^23 times 1 kg/ 1000 g

195
Q

most stable nuclear is

A

Fe 56

196
Q

vp and boiling point of two things is?

A

between them

197
Q

watch x squared and KSP

A

please

198
Q

watch wording on pH questions

A

please

199
Q

Titrant

A

is what u know, so ITS NOT THE CURVE

200
Q

when determining H and S signs,

A

just write out the eqn

201
Q

Bomb calorimetry is different from specific heat

A

watch eqn

202
Q

Phase change on graph is

A

FLAT PART

203
Q

Watch wording and DON”T ASSUME in redox reactions

A

please

204
Q

when comparing standard reduction potentials, switch them to be the same - or +

A

please

205
Q

MORE POSITIVE REDUCTIoN POTENTIAL MEANS MORE LIKELY TO BE REDUCED

A

lol

206
Q

nuclear capture reaction

A

A nuclear capture reaction, otherwise known as nuclear fusion, involves the combining of two or more reactants to make a single product and energy.

DAT (8 decks)

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