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DAT chem > DAT FINAL REVIEW FOR CHEM > Flashcards

DAT FINAL REVIEW FOR CHEM Flashcards

1
Q

compare energy levels 1 and 2 with 4 and 5

A

the difference between energy levels 1 and 2 is larger than the difference between energy levels 4 and 5

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2
Q

why are transition metals brightly colored?

A

Also known as the metals in the d block….. its because the funky way that d orbitals absorb colored light and promoted to higher energy orbitals

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3
Q

what is pauli exclusion principle

A

no 2 electrons in same atom can have same 4 quantum numbers

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4
Q

what is hunds rule

A

electrons fill up orbitals one at a time

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5
Q

what is aufbau principle?

A

electrons fill the lowest energy orbital first

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6
Q

what is paramagnetic attracted to magnets

A

because it has unpaired electrons

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7
Q

why is diamagnetic repelled by magnets?

A

it has all paired electrons

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8
Q

02 is what

A

paramagnetic

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9
Q

N2 is what

A

diagmagnetic

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10
Q

Odd number of electrons can indicate what

A

paramagnetic

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11
Q

and even number of electrons can indicate what

A

either paramagnetic or diamagetic

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12
Q

what is the mnemonic for wave frequency

A

roman men invented very unusual x ray guns

The R in roman is the lowest energy = highest wave length

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13
Q

___ in energy equals ____ in frequency equals ___ in wavelenth

A

increase
increase
decrease

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14
Q

ionic bonds properties

A

high melting point, high bp

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15
Q

molecular bonds properties

A

low melting point do not conduct electricity

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16
Q

net work covalent bond properties

A

high melting point, high boiling point, hard, do not conduct electricity…. EX.

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17
Q

metallic bond properties

A

variable hardness and melting point
conduct electricity and heat
shiny and malleable

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18
Q

what is lattice energy

A

amount of energy to completely separate an ionic compound

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19
Q

sp angle

A

180 linear

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20
Q

sp2 angle

A

120 trigonal planar

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21
Q

sp3 angle

A

109.5 tetrahedral

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22
Q

geometry of sp2 with a pair of electrons

A

bent

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23
Q

geometry of sp3 with a a pair of electrons

A

trigonal pyramidal

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24
Q

geometry of sp3 with 2 pairs of electrons

A

bent

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25
Q

alkali metals have ___ ionization energy

A

low

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26
Q

alkaline earth metal have ___ ionization energy

A

low

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27
Q

halogens are ______ oxidizing agents

A

good

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28
Q

compare o2 and o3 in terms of oxidizing agent and what it likes to react with?

A

o2 is good oxidizing agent but o3 is a better one!

likes to react with metal to form metal oxides

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29
Q

ion sizes in terms of minus and positive

A

the more minus the ion is…. the bigger

the more positive the ion is…. the smaller

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30
Q

what is electron affinity?

A

energy given off when an atom gains electrons

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31
Q

what is ionization energy

A

energy required to remove electron from an atom

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32
Q

gas behaves most ideally in what conditions

A

low pressure and high temp

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33
Q

what is the ideal gas assummption

A
  1. volume/ size of gas are insignificant
    - most accurate at low pressure
  2. gas collision are elastic, no intermolecular forces
    - most accurate at hig temp and low intermolecular forces
  3. average kinetic energy of gas depends on only temp
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34
Q

increase in intermolecular forces causes what?

A

increase bp, viscosity, surface tension

decreased vapor pressure

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35
Q

simple cubic

A

1 atom per unit cell

36
Q

body centered cubic

A

2 atoms per unit cell

37
Q

face centered cubic

A

4 atoms per unit cell

38
Q

top part of solid - liquid - gas is what???

going from gas to solid

A

consume heat (endothermic, positive delta h and positive delta s)

39
Q

bottom part of solid- liquid - gas is what???

going from gas to solid

A

produce heat (exothermic, - delta h and - s)

40
Q

another word for melting is w

A

fusion

41
Q

going from gas to solid is known as what

A

depostion

42
Q

going from solid to gas is known as what

A

sublimination

43
Q

liquid water is _____ dense than solid while other solids are denser as solid

A

more
Water’s lower density in its solid form is due to the way hydrogen bonds are oriented as it freezes: the water molecules are pushed farther apart compared to liquid water. 1: Ice Density: Hydrogen bonding makes ice less dense than liquid water.

44
Q

what is normal boiling point?

A

temp at which vapor pressure of liquid is equal to 1 atm

45
Q

solubility rule (solubles)

A 
group 1 metal cations
no3- 
clo4-
acetate c2h3o2-
nh4+
46
Q

solubility rule insolubles

A 
silver ag
lead pb
sulfide S2-
hydroxide Oh-
dimercury Hg22+
carbonate Co32-
phosphate Po43-
47
Q

what is colligative property?

A

depend on # of solute and not nature of solute present in solvent

48
Q

how to find spectator ions from net ionic equation

A

NO REACTION
—– if all the states are aq. reaction only happens if there is aleast one solid
step 0. balance
step 1. determine the solubility if not given
step 2. pair the cations and anions to give reactant and product
step 3. cut everything in half
step 4. cancel out things that are the same
step 5. the things you canceled out are the spectator ions

49
Q

what happens to the solids solubility as temp increases?

A

the solubility of the solid also increases

think of hot chocolate mix

50
Q

what happens to the gas solubility as temp increases

A

lowers…..
when temp gets higher that means it will increase the gas molecules speeds. which will cause more and more of those gas molecules to escape and leave the liquidt

51
Q

what happens to gas solubility when theres an increase in pressure?

A

goes up! when you compress a cup with gases in it… it will keep more gasses in it therefore keeping more gas molecules in the cup

52
Q

increase in solute in solid will do what to the freezing point?

A

decrease it

53
Q

increase solute in liquid will do what to the freezing point?

A

raise it

54
Q

breaking bonds is an what kind of process

A

endothermic… heat is consumed as this happens

55
Q

making bonds is what kind of process?

A

exothermic… heat releases as this happens

56
Q

what never appears in a rate law?

A

intermediates

57
Q

what only appears in rate law

A

the reactant

58
Q

zero order ____- concentration = ____ half life

A

decreased

decreased

59
Q

first order ___- half life - independent of

A

constant

[A]

60
Q

second order ____ concentration = ___ half life

A

decreased

increased

61
Q

larger activation energy =

A

slower step

62
Q

intermediates are only found in the

A

middle… not in the reactant or the product

63
Q

what does catalyst do

A

lowers EA
provides alternative pathway
does not shift equilibrium

64
Q

collision theory

A
  1. both molecule collide
  2. collide with enough energy
  3. collide with correct 3d orientation
65
Q

___ temp = ___ K = ____ rate

A

increase
increase
increase

66
Q

__ Ea = __ K= __ rate

A

decrease
increase
increase

67
Q

for any part of equilibrium constant Ex. Kc Kp and Keq what is ONLY included

A

aq and gas

68
Q

Q is less than K.. what is the result

A

shift rights (products)

69
Q

what is the difference between Q and K

A

K is equilibirum

Q may or may not be equilibrium

70
Q

Q is greater than K.. what is result

A

shift left (reactant)

71
Q

Q=K what is result?

A

equilibrium

72
Q

Q > ksp equals what

A

precipitation

73
Q

Q < ksp equals what

A

no precipitation

74
Q

what is le chateliers principle

A

if a system at equilibrium is disturbed, then it will shift in which ever direction it has to, to restore that equilibrium

75
Q

strong acids in order

A

HI HBR HCl ( binary acids)
Hclo3 Hclo4
h2s04
Hno3

76
Q

trend for strong acid

A

electronegativity and down

77
Q

strong base

A

Group 1 metals with OH

these are group 2
Mg(OH)2
Ca(OH)2
Sr(OH2
Ba(OH)2
78
Q

types of heat transfer
conduction
convection
radiation

A

conduction - direct contact: bites pizza
convection - motion of fluid: cook by hot air (oven)
radiation - electromagnetic radiation ( Infrared light)

79
Q

anode is the site of what?

A

oxidation

80
Q

cathode is the site of what

A

reduction

81
Q

electrons always flow in what direction in voltaic cell

A

anode to cathod

82
Q

the voltaic and galvanic cells the anode is ___ and cathode is ____

A

negative and positive

83
Q

in electrolytic cells, the anode is _____ and the cathode is ____

A

positive

negative

84
Q

function of salt bridge

A

let counter anions flow into the anode, and cations to the cathode

85
Q

anode metals _____ mass and cathode metal ____ mass

A

loses

gains

86
Q

the ideal gas law assumptions

A
  1. all gas molecules are in constant, raid, and random motion
  2. there are no attractive or repulsive forces (IM forces) between the gases
  3. the volume of the molecules is negligibly small compared to the volume of the gas
  4. all collisions within the gas are perfectly elastic
  5. the average kinetic energy of the gas molecules depends only on the temp of the system

DAT chem (8 decks)

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