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Fall 2017 > CHEM 105 Test 3 (Ch. 6-8) > Flashcards

CHEM 105 Test 3 (Ch. 6-8) Flashcards

1
Q

paramagnetic

A

unpaired e-s

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2
Q

the valence electrons of the atoms in a molecule reside in

A

quantum-mechanical atomic orbitals; orbitals can be s,p,d,f or hybrid combos of these

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3
Q

a chemical bond results from

A

the overlap of two half-filled orbitals and spin-pairing of the two valence electrons

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4
Q

to interact, the orbitals must either

A

be aligned along the axis b/w the atoms or be parallel to each other and perpendicular to the interatomic axis

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5
Q

hybridization

A

mixing different types of orbitals in the valence shell to make a new set of degenerate orbitals

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6
Q

the number of hybrid orbitals formed equals

A

the number of standard atomic orbitals combined

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7
Q

the particular kind of hybridization that occurs is the one that

A

yields the lowest overall energy for the molecule

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8
Q

sp3 hybridization

A

atom with 4 electron groups around it; tetrahedral geometry; 109.5* angles between hybrid orbitals; atom uses hybrid orbitals for all bonds and lone pairs

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9
Q

sp2 hybridization

A

atom with 3 electron groups around it; trigonal planar system; 120* bond angles; flat; atom uses orbitals for sigma bonds and lone pairs and uses nonhybridized orbital for pi bond

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10
Q

sigma bond

A

results when the interacting atomic orbitals point along the axis connecting the two bonding nuclei; either standard atomic orbitals or hybrids

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11
Q

pi bond

A

results when the bonding atomic orbitals are parallel to each other and perpendicular to the axis connecting the two bonding nuclei; between unhybridized parallel p orbitals

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12
Q

? bonds are stronger than ? bonds

A

sigma; pi

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13
Q

overlap between a hybrid orbital on one atom with a hybrid or nonhybridized orbital on another atom results in a ? bond

A

sigma

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14
Q

overlap between unhybridized p orbitals on bonded atoms results in a ? bond

A

pi

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15
Q

? bonds require the breaking of the interaction between the orbitals to rotate

A

pi

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16
Q

sp hybridization

A

atom with 2 electron groups; linear shape; 180* bond angle; atom uses hybrid orbitals for sigma bonds or lone pairs and uses nonhybridized p orbitals for pi bonds

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17
Q

sp3d hybridization

A

atom with five electron groups; trigonal bipyramidal; seesaw, T-shaped, linear; 120* and 90* bond angles; ues empty d orbitals from valence shell; d oritals used to make pi bonds

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18
Q

sp3d2 hybridization

A

atom with six electron groups; octahedral electron geometry; square pyramidal, square planar; 90* bond angles; use empty d orbitals from valence shell to form hybrid; d orbitals used to make pi bonds

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19
Q

2 e- groups

A

linear e- geometry; sp hybridization

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20
Q

3 e- groups

A

trigonal planar e- geometry; sp2 hybridization

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21
Q

4 e- groups

A

tetrahedral e- geometry; sp3 hybridization

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22
Q

5 e- groups

A

trigonal bipyramidal; sp3d hybridization

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23
Q

6 e- groups

A

octahedral; sp3d2 hybridization

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24
Q

valence bond theory doesn’t account for

A

magnetic behavior of O2; delocalization of e-s

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25
Q

Molecular Orbital (MO) Theory

A

applies Shrodinger’s wave equation to the molecule to calculate a set of molecular orbitals; in this treatment, the e-s belong to the whole molecule, so the orbitals melong to the whole molecule (delocalization)

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26
Q

Linear Combination of Atomic Orbitals (LCAO)

A

atomic orbitals of the atoms add together to make molecular orbitals; b/c the orbitals are wave functions, the waves can combine either constructively or destructively

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27
Q

when the wave functions combine constructively, the resulting molecular orbital has (more/less) energy than the original atomic orbitals; called ?

A

less; called a bonding molecular orbital (designated sigma or pi)

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28
Q

when the wave functions combine destructively, the resulting molecular orbital has (more/less) energy than the original atomic orbital; called?

A

more; called an antibonding molecular orbital (designated sigma* or pi*)

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29
Q

electrons in bonding MOs are (stabilizing/destabilizing) and have (lower/higher) energy than the atomic orbitals

A

stabilizing, lower

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30
Q

electrons in antibonding MOs are (stabilizing/destabilizing) and have (lower/higher) energy than the atomic orbitals

A

destabilizing, higher

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31
Q

electrons in antibonding orbitals ? stability gained by electrons in bonding orbitals

A

cancel

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32
Q

bond order =

A

1/2 (# bonding e-s - #antibonding e-s)

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33
Q

higher bond order means

A

stronger and shorter bonds

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34
Q

if bond order = 0, then the bond

A

will not form

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35
Q

if all e-s are paired, the substance is

A

diamagnetic

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36
Q

when the combining atomic orbitals are identical and of equal energy, the contribution of each atomic orbital to the molecular orbital is

A

equal

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37
Q

when the combining atomic orbitals are different types and energies, then

A

the atomic orbital closest in energy to the molecular orbital contributes more to the molecular orbital

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38
Q

the more electronegative an atom is, the

A

lower in energy its orbitals are

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39
Q

lower energy atomic orbitals contribute more to the ? MOs

A

bonding

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40
Q

higher energy atomic orbitals contribute more to the ? MOs

A

antibonding

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41
Q

nonbonding MOs remain ? on the atom donating its atomic orbitals

A

localized

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42
Q

when many atoms are combined together, the atomic orbitals of all the atoms are

A

combined to make a set of molecular orbitals, which are delocalized over the entire molecule

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43
Q

physical changes

A

changes that alter only the state or appearance, not composition; identity of the atoms or molecules does not change

44
Q

chemical changes

A

changes that alter the composition of matter; atoms rearrange, transforming the original substances into different substances

45
Q

percent yield =

A

actual / theoretical x 100%

46
Q

limiting reactant/reagent

A

the reactant that makes the least amount of product

47
Q

theoretical yield

A

the amount of product that can be made from the limiting reactant

48
Q

reactant in excess

A

any reactant that occurs in a quantity greater than is required to completely react with the limiting reactant

49
Q

a combustion reaction involves

A

a reaction of a substance with O2 for form one or more oxygen-containing compounds; products are water and heat (energy)

50
Q

common reaction for alkali metals is

A

with halogens

2M + X2 -> 2MX

51
Q

the alkali metals react vigorously with water to form

A 
dissolved alkali metal ion, the hydroxide ion, and hydrogen gas
2 M (s) + 2 H2O (l) -> 2 M+ (aq) + 2 OH- (aq) + H2 (g)
52
Q

the halogens react with metals to form ? and hydrogen to form ?

A

metal halides, hydrogen halides

53
Q

homogeneous mixtures are called

A

solutions

54
Q

the minor component of the solution is called the

A

solute

55
Q

the major component of the solution is called the

A

solvent

56
Q

dilute solutions have a ? amount of solute compared to solvent

A

small

57
Q

concentrated solutions have a ? amount of solute compared to solvent

A

large

58
Q

Molarity (M) =

A

moles solute / Liter of solution

59
Q

equation to determine change in concentration or volume for solutions

A

M1V1 = M2V2

60
Q

electrolytes

A

materials that dissolve in water to form a solution that will conduct electricity

61
Q

nonelectrolytes

A

materials that dissolve in water to form a solution that will NOT conduct electricity

62
Q

strong electrolytes

A

completely dissociate into ions

63
Q

weak electrolytes

A

partially dissociate into their ions

64
Q

strong acid

A

dissociates completely in water; would be a strong electrolyte

65
Q

weak acid

A

dissociates partially; would be a weak electrolyte

66
Q

most molecular compounds dissolve in water as

A

intact molecules > nonelectrolyte solution

67
Q

compounds containing the following ions are generally soluble

A

Li+, Na+, K+, NH4+, NO3-, and C2H3O2-
Cl-, Br-, and I- except for with Ag+, Hg22+, Pb2+
SO42- except with Sr2+, Ba2+, Pb2+, Ag+, or Ca2+

68
Q

compounds containing the following ions are generally insoluble

A

OH- and S2- except with Li+, Na+, K+, NH4+, Ca2+, Sr2+, or Ba2+
CO32- and PO43- except with Li+, Na+, K+, or NH4+

69
Q

precipitation reactions

A

reactions in which a solid forms when two solutions are mixed

70
Q

the insoluble product is called a

A

precipitate

71
Q

predicting precipitation reactions

A
  1. determine what ions each of the aqueous reactants has
  2. determine formulas of possible products
  3. determine the solubility of each product in water
  4. if neither product will precipitate, write “no reaction” after the arrow
  5. if products are insoluble, write (s) after formula to indicate solid; if soluble, write (aq) to indicate aqueous
  6. balance the equation
72
Q

molecular equation

A

an equation showing the complete neutral formula for each compound in the aqueous reaction as if they existed as molecules

73
Q

complete ionic equations

A

equations that describe the material’s structure when dissolved

74
Q

spectator ions

A

ions that do not participate in the reaction

75
Q

net ionic equation

A

differs from a complete ionic equation because it does not include the spectator ions

76
Q

acids

A

molecular compounds that form H+ when dissolved in water; composed of Hydrogen, usually written first in their formulas, and 1+ nonmetals, written second

77
Q

Arrhenius Definitions:

A

acid: substance that produces H+
base: substance that produces OH-

78
Q

polyprotic acids

A

acids that contain more than one ionizable proton (H+) and release them sequentially

79
Q

binary acids

A

have H+ cation and nonmetal anion

80
Q

oxyacids

A

have H+ cation and polyatomic anion

81
Q

how to name a binary acid

A

hydro + (base name of nonmetal + -ic) + acid

82
Q

how to name an oxyacid

A

if ends in -ate, change suffix to -ic
if ends in -ite, change suffix to -ous
(follow binary rules aside from this)

83
Q

neutralization reaction

A

an acid reacts with a base, and the two neutralize each other, producing water; the anion from one reactant combines with the cation of another

84
Q

a neutralization reaction is completed when

A

moles of acid = moles of base

85
Q

the endpoint of titration

A

when the indicator color changes - the equivalence point

86
Q

gas-evolution reaction

A

a gas forms, resulting in bubbling; many are also acid-base reactions

87
Q

types of compounds that undergo gas-evolution reactions

A

sulfides > H2S
carbonates & bicarbonates > CO2
sulfites and bisulfites > SO2
ammonium > NH3

88
Q

oxidation-reduction reactions

A

the reactions in which electrons are transferred from one reactant to the other

89
Q

atoms that lose electrons are being

A

oxidized

90
Q

atoms that gain electrons are being

A

reduced

91
Q

oxidation will (increase/decrease) the oxidation state

A

increase

92
Q

reduction will (increase/decrease) the oxidation state

A

decrease

93
Q

rules for assigning oxidation states

A
  1. free elements have an oxidation state = 0
  2. monatomic ions have an oxidation state equal to their charge
  3. a) the sum of the oxidation states of all the atoms in a compound is zero
    b) the sum of the oxidation states of all the atoms in a compound is zero
  4. a) Group I metals have an oxidation state of +1 in all their compounds
    b) Group II metals have an oxidation state of +2 in all their compounds
  5. in their compounds, nonmetals have oxidation states according to the table
94
Q

oxidation state of fluorine

A

-1

95
Q

oxidation state of hydrogen

A

+1

96
Q

oxidation state of oxygen

A

-2

97
Q

oxidation state of Group 7A

A

-1

98
Q

oxidation state of Group 6A

A

-2

99
Q

oxidation state of Group 5A

A

-3

100
Q

oxidizing agent

A

the reactant that oxidizes an element in another reaction; contains the element that is reduced

101
Q

reducing agent

A

the reactant that reduces an element in another reaction; contains the element that is oxidized

102
Q

an activity series table lists metals in order of (increasing/decreasing) tendency to lose e-s

A

decreasing; so higher up is more likely to be oxidized and lower down is more likely to be reduced

103
Q

AgCl, HgCl2, PbCl2
AgBr, HgBr2, PbBr2
AgI, HgI2, PbI2

A

insoluble

104
Q

SrSO4, BaSO4, PbSO4, Ag2SO4, CaSO4

A

insoluble

105
Q

LiOH, NaOH, KOH, NH4OH, Ca(OH)2, Sr(OH)2, Ba(OH)2

Li2S, Na2S, K2S, (NH4)2S, CaS, SrS, BaS

A

soluble

106
Q

Li2CO3, Na2CO3, K2CO3, (NH4)2CO3

Li3PO4, Na3PO4, K3PO4, (NH4)3PO4

A

soluble

Fall 2017 (24 decks)

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