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DAT > Chemistry > Flashcards

Chemistry Flashcards

1
Q

go do Anki flashcards or review the table

A

okay

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2
Q

allotropes

A

elemental molecules with different formulas like O2 vs O3

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3
Q

binary acid naming

A

hydro-ic

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4
Q

oxyacids

A

ate-ic, ite-ous

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5
Q

unit conversion tip

A
  • remember that -ve exponent in denominator changes to +
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6
Q

Terra (T)

A

10^12

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7
Q

Giga

A

10^9

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8
Q

Mega

A

10^6

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9
Q

KILO

A

10^3

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10
Q

Centi

A

10^-2

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11
Q

Milli

A

10^-3

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12
Q

Micro

A

10^-6

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13
Q

Nano

A

10^-9

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14
Q

beer Lambert law

A

absorbance= constant times concentration times distance between light source and detector

** brighter the colour, higher the constant

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15
Q

add__to ___

A

acid to water

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16
Q

heat a test tube

A

in a water bath

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17
Q

transparent solution absorbance and transmission

A

0 absorbance and 100% transmission

*opaque is opposite

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18
Q

greatest least sign

A

greatest then it will be the far right

least will also be far right

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19
Q

empirical formula steps

A

don’t forget to divide grams by mM to get moles!

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20
Q

when given percent yield or something

A

instead of using percents, just use mass itself like 100 g to 70 grams for 30% impure

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21
Q

theoretical yield conversion?

A

no need to covert. can just use moles

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22
Q

** always balance eqn!

A

YES

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23
Q

orbitals, shape and L

A

s orbital= sphere and l=0
p orbital= dumbbell and l=1
D orbital= clover, l=2

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24
Q

quantum numbers

A 
n= 1,2,3 shell
l= 0-n-1 (limit of 3) subshell type
ml= -l, to -l orientation
ms= = +1/2 and -1/2 spin
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25
Q

valence electrons

A

only elements in d block do d block electrons count to wards valence!

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26
Q

exceptions to electron configuration

A

Cr, Mo, Cu, Ag and Au

* bump electrons to half fill

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27
Q

line spectra

A

each element has unique line spectra as E fall back to ground state

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28
Q

paramagnetic

A

“unPAIR” attracted to magnets

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29
Q

diamagnetic

A

all paired. repelled by magnets

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30
Q

energy, frequency and wavelength

A

increased energy means increased frequency and less wavelength

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31
Q

Heisenberg uncertainty

A

impossible to determine a particle’s position and momentum with accuracy

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32
Q

photoelectric effect

A
  • if you energize a metal plate, it will eject e- when hit with enough energy
  • KinE= Ephoton- (energy required to expel electron)
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33
Q

photoelectric effect eqn

A
  • KinE= Ephoton- (energy required to expel electron)
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34
Q

compound ranking of strength (ions, molec etc.)

A

ionic, network covalent, metallic and then molecular

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35
Q

lattice energy

A

more charges and shorter bond distance is more lattice energy

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36
Q

exception o octet rule

A

Be, B and Al

- third row can have many

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37
Q

bond order

A

count up each bond, and divide by total number of things around the center

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38
Q

isoelectronic atomic radius

A

more protons and less E is tightest

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39
Q

ionization energy

A

removing valence, and half filled is a lot!

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40
Q

electron affinity

A

energy released when atom gains an E=

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41
Q

hund’s rule

A

every orbital in a certain subshell fills up with electrons before pairing

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42
Q

aufbau

A

electrons fill lowest energy first

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43
Q

pauli

A

no two electrons can have same quant #

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44
Q

K= C+

A

273

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45
Q

pressure is

A

Force/Area

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46
Q

1 atm=

A

760 Torr, and 760 mmHg

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47
Q

manometer

A

sample pushes down, then you add the pressures as its greater

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48
Q

combined gas law

A

PV/Nt

multiplication means inverse proportionality

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49
Q

1 mol of gas at STP in L?

A

22.4 L

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50
Q

R for gases

A

0.0821 l atm/ mol K

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51
Q

STP

A

1 atm and 273 K

0 degrees C

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52
Q

real gas behaves ideal at

A

high temp and LOW pressure

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53
Q

gas density

A

Pressure times MM/ RT

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54
Q

dalton’s laws

A

Pa= XaPtot

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55
Q

graham’s law of effusion

A

r1/r2= sqrt M2/ M1

R1 and M2 are onTOP

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56
Q

real gas eqn corrects for

A

imp and volume

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57
Q

cubic body shapes

A

simple cubic: 1
body centred: 2
face centered: 4

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58
Q

crystallization is

A

going from liquid to solid

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59
Q

Hbonding

A

is anything with HFON

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60
Q

volatile

A

means substances boil quick

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61
Q

molality

A

moles Solute / kg solvent

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62
Q

solubility of ionic compounds

A
  1. most group 1 metal cations, NO3, CLO4, acetate and NH4+ are SOLUBLE
  2. most ag, pb, s2-, hg, co3, po4 are insoluble
    * * soluble trumps insoluble
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63
Q

y’s law

A

Pa= kh concentration

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64
Q

freezing point depression

A

delta Temp f=ikfm

  • Molality and tf is always plus
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65
Q

boiling point elevation

A

delta Tb= ikbm

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66
Q

vapor pressure depression

A

Pa= XaPpure

Xa is percent solvent in new solution
P pure is original solvent pressuer

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67
Q

colligative properties

A
  1. decrease vp
  2. increase BP
  3. freezing point depression
  4. osmotic pressure
68
Q

osmotic pressure

A

P = iMRT

R= 0.08

69
Q

rate law constant units

A

rate is M/s and each concentration is M order rate law graph

70
Q

integrated rate law zero graph

A

concentration vs time,

slope is - k

71
Q

integrated rate law first graph

A

Ln[A] vs time. slope is -K

72
Q

integrated rate law second graph

A

1/[A] vs time. slope is K

73
Q

concentration vs time graphs. curved

A

zero: plot is line. half life decreases with [A]
first: curved. half life is independent
second: half life increases with concentration

74
Q

rate and K, Temp, and Ae

A

reaction rate is directly related to its rate constant

  • increasing temp means increasing rate constant and then reaction rate,
  • decreasing activation energy increases K and increases rate
75
Q

K eq

A

production over reactants!

76
Q

pressure doesn’t change by adding an inert gas

A

le chat

77
Q

ice table tips

A

disregard X if 1000

remember to SQUARE and 2x

78
Q

Ksp tips

A

best to keep solubilities separate as x, makes math easy

79
Q

precipitation qns

A

write out run, write out kip and see if Q/ ksp then precipitate

80
Q

Arrhenius and bronstead and lewis

A

Arrhenius is Oh and H, while brown stead is H+ donor. lewis is electron donor and acceptor

81
Q

strong bases

A

are Mg, Ca, Sr, and Ba OH2!!

82
Q

strongest acid?

A

HI is the strongest!!!

83
Q

pH tips

A

when a strong acid is less than 10^-7 concentration, the pH is just 7

  • more stuff means lower or higher pH based on if its basic or acidi
84
Q

larger ka means smaller

A

pKa and stronger acid

85
Q

SHORTCUT FOr PH in EQ

A

[H+]= sqrt of ka[HA]

[OH-]= sort of Kb [A-]

86
Q

normality

A

how much can contribute Oh and O. always include in dilution

87
Q

buffers

A

1:1 ratio of weak acid and conjugate base
OR

2:1 ratio of weak acid and STRONG BASE

88
Q

changing pH can change salt solubility

A

salt is basic, adding acid will increase sol and acid will react with basic ion, shifting eq

89
Q

hydrolysis of salts

A

neutral are all metals, and strong acid stuff.

all other cations are acids, anions are bases

90
Q

buffer eqn

A

pH= pKa + log [A-]/ [HA]

or HAHAHA

91
Q

buffers have a ph range of

A

+/- 1 pK

92
Q

titration names

A

titrant; known

titrand is unknown

93
Q

state function

A

everything except work and heat

94
Q

laws of thermo

A
  1. creation/ destroy of energy
  2. entropy is always increasing
  3. perfect crystal has zero entropy
95
Q

enthalpy of formation vs bond

A

bond has a good RP

formation is pR

96
Q

energy and work eqna

A

E= P + w

W= -Pdelta V

97
Q

convection is transfer due to

A

fluid

98
Q

bomb calorimeter eqn

A

Q= -c delta T

99
Q

in heat transfer questions

A

the two heats equal each other, not zero

100
Q

entropy

A

P-R

101
Q

draw out molecule for bond energy

A

yes

102
Q

delta g negative is

A

spontaneous

103
Q

delta g eqn

A

delta G= Delta H - T delta S

104
Q

delta g eqn signs

A
  • delta g is always - delta H, + S and any temp above is spontaneous
105
Q

delta d to standard delta g

A

delta G= delta G not + RTlnQ

106
Q

delta d to standard delta g with K

A

delta g not= -RTlnK

107
Q

balancing redox in basic

A

write out full eqn, then add OH to both sides with same H+ number and turn to water

108
Q

voltaic and galvanic cell

A

spontaneous )+ Ecell

anode is -ve
- salt bridge is present

109
Q

electrolytic cell

A
  • non spontaneous
  • anode is +
  • make elements!
  • sea of electrons, no salt bridge
110
Q

Aq electrolysis

A

water is also a factor, more positive means reaction will happen

111
Q

top of reduction potential chart

A

highest reduction agent (gets ox)

112
Q

ox and red agent

A
  • Oxidizing agent and oxidant both refer to what is beingreduced, while reducing agent and reductant both refer to what is beingoxidized.
113
Q

Nernst equation

A

E cell = E not - 0.06/ n logQ

n is electrons transferred

114
Q

eq and nernst

A

shifting to the right, means an increase in E cell

115
Q

electroplating formula

A

Time times current over n and 100,000

n is electrons transferred

116
Q

alpha particle

A

4.2 He

helium is alpha

117
Q

neutron

A

1.0 N

118
Q

proton

A

1.1 P

hydrogen is a proton

119
Q

beta particle

A

high speed E
0.-1 B

beta is bad

120
Q

positron particle

A
  1. +1 e

positron is positive

121
Q

gamma particle

A

0.0 gamma

122
Q

decay or fission rxn

A

decompose and energy

123
Q

capture and fusion

A

adding and energy

124
Q

belt of stability

A

first 20 elements: must have 1:1 ratio of N and P to be stable

beyond: N can exceed

** as protons increase, neutrons increase but neutrons increase FASTEr

125
Q

see chart for radioactive deca

A

pg 76

126
Q

nuclear fusion is always what order

A

1st order so half life is o.69/k

rate constant

127
Q

fission

A

larger nuclei decay

128
Q

fusion

A

small combines with large

129
Q

binding energy formula

A

E= mc^2

c= 3 times 10^8

130
Q

mass defect

A

nucleus weighs less than its addition of particles. this energy is binding energy

MUST convert AMU to kg!!

131
Q

AMU to kg

A

1 g/ 6.02 x 10^23 and then 1 kg/ 1000 kg

132
Q

percent yield eqn

A

actual/ theoretical x 100%

133
Q

MO theory

A

there are 4 boxes for s, 6 boxes for P, with 2 for 2 pi and 1 for 2 sigma

134
Q

atomic radius depends on

A

effective nuclear charge

135
Q

be careful with ranking atoms and periodic trends

A

please

136
Q

p and v gas law

A

p1v1= p2v2

137
Q

v and t gas law

A

v/t = v/t

138
Q

P and t gas law

A

P/t = p/t

139
Q

combined gas law

A

pv/t = pv/t

140
Q

density and gases

A

pressure x Molar mass/0.08 and T in K

141
Q

higher the vapour pressure

A

easier to boil the liquid (lower boiling point) and more volatile it is

142
Q

2 liquids and vapour pressure

A

the BP will be between them

- more volatile is more PRESENT in compound

143
Q

solubility OH

A

oh containing salts are INSOLUBLE

144
Q

arrhenius eqn

A

says that if u increase temp, increase K, increase rate

decrease ea= increase K and increase rate

145
Q

pH and solubility

A

decreasing pH can help solubility, think of Wa/ B

146
Q

please write equilibrium equations carefully

A

products / reactants

147
Q

convert scienfitic notation

A

to full numbers

148
Q

be careful about solubility in g/l vs g/ ml

A

yep

149
Q

precipitate formation

A

find qsp, and ksp. BALANCE EQN. write out ksp eqn over again. and multiple the products not reactants

150
Q

oxygen and resonance

A

serves to delocalize E and stabilize the conjugate

151
Q

weaker conjugate base

A

means more basic

152
Q

nitrogen with three groups is always

A

basic

153
Q

bomb calorimeter eqn

A

Q = -CT

  • mass is factored in here, so u must divide by 2 to get per gram
154
Q

entropy decreases with

A

temp, volume (increased pressure) or decrease in gas particles

155
Q

heat capacity from graph

A

is the slope. higher slope means lower heat capacity

156
Q

larger k means what for delta g?

A

more -ve delta G

157
Q

thermo laws

A
  1. energy 2. delta s universe is + 3. entropy approches 0 as temp approaches 0
158
Q

oxidizing agent and oxidant

A

same thing

159
Q

balancing redox

A

balance H20 by adding H+

160
Q

more positive the reduction potential

A

the greater reduction and the better the ox agent. more likely to be reduced

the cathode is the more positive one

161
Q

electroplating

A

amp up the time/ moles and F

162
Q

what happens when N/Z ratio is too high

A

beta decay. produces beta particle

163
Q

large nuclei nuclear reaction?

A

alpha decay. produces alpha particle

164
Q

too low N/z ratio

A

positron particle is produced

165
Q

too low N/z ratio reactant

A

electron capture. add -ve, so beta particle is reactant

166
Q

increase in atomic number nuclear?

A

only if its -ve particle produced or added as reactant

167
Q

MORE RIGHT in atomic radius, no matter the electrons

A

is always smaller

DAT (8 decks)

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