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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
alkali metals have ___ ionization energy
low
26
alkaline earth metal have ___ ionization energy
low
27
halogens are ______ oxidizing agents
good
28
compare o2 and o3 in terms of oxidizing agent and what it likes to react with?
o2 is good oxidizing agent but o3 is a better one! | likes to react with metal to form metal oxides
29
ion sizes in terms of minus and positive
the more minus the ion is.... the bigger | the more positive the ion is.... the smaller
30
what is electron affinity?
energy given off when an atom gains electrons
31
what is ionization energy
energy required to remove electron from an atom
32
gas behaves most ideally in what conditions
low pressure and high temp
33
what is the ideal gas assummption
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
34
increase in intermolecular forces causes what?
increase bp, viscosity, surface tension | decreased vapor pressure
35
simple cubic
1 atom per unit cell
36
body centered cubic
2 atoms per unit cell
37
face centered cubic
4 atoms per unit cell
38
top part of solid - liquid - gas is what??? | going from gas to solid
consume heat (endothermic, positive delta h and positive delta s)
39
bottom part of solid- liquid - gas is what??? | going from gas to solid
produce heat (exothermic, - delta h and - s)
40
another word for melting is w
fusion
41
going from gas to solid is known as what
depostion
42
going from solid to gas is known as what
sublimination
43
liquid water is _____ dense than solid while other solids are denser as solid
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
what is normal boiling point?
temp at which vapor pressure of liquid is equal to 1 atm
45
solubility rule (solubles)
``` group 1 metal cations no3- clo4- acetate c2h3o2- nh4+ ```
46
solubility rule insolubles
``` silver ag lead pb sulfide S2- hydroxide Oh- dimercury Hg22+ carbonate Co32- phosphate Po43- ```
47
what is colligative property?
depend on # of solute and not nature of solute present in solvent
48
how to find spectator ions from net ionic equation
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
what happens to the solids solubility as temp increases?
the solubility of the solid also increases | think of hot chocolate mix
50
what happens to the gas solubility as temp increases
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
what happens to gas solubility when theres an increase in pressure?
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
increase in solute in solid will do what to the freezing point?
decrease it
53
increase solute in liquid will do what to the freezing point?
raise it
54
breaking bonds is an what kind of process
endothermic... heat is consumed as this happens
55
making bonds is what kind of process?
exothermic... heat releases as this happens
56
what never appears in a rate law?
intermediates
57
what only appears in rate law
the reactant
58
zero order ____- concentration = ____ half life
decreased | decreased
59
first order ___- half life - independent of
constant | [A]
60
second order ____ concentration = ___ half life
decreased | increased
61
larger activation energy =
slower step
62
intermediates are only found in the
middle... not in the reactant or the product
63
what does catalyst do
lowers EA provides alternative pathway does not shift equilibrium
64
collision theory
1. both molecule collide 2. collide with enough energy 3. collide with correct 3d orientation
65
___ temp = ___ K = ____ rate
increase increase increase
66
__ Ea = __ K= __ rate
decrease increase increase
67
for any part of equilibrium constant Ex. Kc Kp and Keq what is ONLY included
aq and gas
68
Q is less than K.. what is the result
shift rights (products)
69
what is the difference between Q and K
K is equilibirum | Q may or may not be equilibrium
70
Q is greater than K.. what is result
shift left (reactant)
71
Q=K what is result?
equilibrium
72
Q > ksp equals what
precipitation
73
Q < ksp equals what
no precipitation
74
what is le chateliers principle
if a system at equilibrium is disturbed, then it will shift in which ever direction it has to, to restore that equilibrium
75
strong acids in order
HI HBR HCl ( binary acids) Hclo3 Hclo4 h2s04 Hno3
76
trend for strong acid
electronegativity and down
77
strong base
Group 1 metals with OH ``` these are group 2 Mg(OH)2 Ca(OH)2 Sr(OH2 Ba(OH)2 ```
78
types of heat transfer conduction convection radiation
conduction - direct contact: bites pizza convection - motion of fluid: cook by hot air (oven) radiation - electromagnetic radiation ( Infrared light)
79
anode is the site of what?
oxidation
80
cathode is the site of what
reduction
81
electrons always flow in what direction in voltaic cell
anode to cathod
82
the voltaic and galvanic cells the anode is ___ and cathode is ____
negative and positive
83
in electrolytic cells, the anode is _____ and the cathode is ____
positive | negative
84
function of salt bridge
let counter anions flow into the anode, and cations to the cathode
85
anode metals _____ mass and cathode metal ____ mass
loses | gains
86
the ideal gas law assumptions
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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