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college chem 117 > midterm exam 3 > Flashcards

midterm exam 3 Flashcards

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1
Q

which theory shows a model with bond overlap between two half filled atomic orbitals

A

Valance Bond Theory

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2
Q

what is the most common model to describe bonding in organic molecules

A

orbital hybridization

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3
Q

hybridization recognizes that orbitals in a molecule are (same/different) than orbitals in an atom

A

same

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4
Q

what are the 3 things to remember when forming hybrid orbitals

A
  1. The # of atomic orbitals added is the same as # of hybrid orbitals formed
  2. the exact combination of atomic orbitals added together determines molecular geometry
  3. the type of hybrid orbitals formed is determined by which yields the lowest energy in the molecule
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5
Q

can hybrid orbitals content lone pair electrons?

A

yes they HAVE to

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6
Q

the first Bond is a ____ bond and the second or third bond is a _____ bond

A

sigma, pi

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7
Q

what breaks/changes regarding water molecules when boiled

A

the intermolecular attractive forces

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8
Q

Iron reacts with oxygen to form rust. Given sufficient time, an iron nail will eventually convert entirely to rust and disintegrate.If the mass of the resulting rust was measured, the weight of the rust would be…

A

More than the nail it came from

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9
Q

the reactant that is completely consumed in a chemical reaction and limits the amount of product.

A

limiting reactant

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10
Q

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

A

reactant in excess

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11
Q

the amount of product that can be made in a chemical reaction based on the amount of limiting reactant

A

theoretical yield

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12
Q

Sodium chloride is a crystalline

compound made up of

A

ions

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13
Q

Sucrose is a crystalline compound made

up of

A

molecules

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14
Q

A crystal or crystalline solid is a solid material whose constituents (e.g. molecules or ions) are arranged in a ________, forming a _________ that extends in all directions

A

highly ordered structure, crystal lattice

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15
Q

homo genius mixtures are called

A

solutions

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16
Q

A mixture can be either homogeneous or heterogeneous depending on what

A

how uniformly the particles that compose the mixture combine

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17
Q

A homogeneous mixture has the _____ composition throughout.

A

same

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18
Q

A heterogeneous mixture is one in which the ________ varies from
one region to another

A

composition

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19
Q

Ionic compounds dissolve by _______, where water surrounds the separated ions.

A

dissociation

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20
Q

Molecular compounds interact with water, but most ________

A

do not dissociate

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21
Q

All substances dissolve by _______, surrounding of the solute by solvent

A

solvation

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22
Q

what is solvation

A

substances dissolved in something that doesn’t have to be water

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23
Q

The minor component of the solution is called the _______, The major component of the solution is called the ______

A

solute, solvent

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24
Q

what is the solvent in air

A

Nitrogen

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25
Q

when water mixes with NaCl, The Hydrogen ends of water are attracted to the ____ ions and the Oxygen ends of water are attracted to the ____ ions

A

Cl-, Na+

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26
Q

is water polar or non polar

A

polar

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27
Q

Attractive forces hold together the ions/molecules of solute in the crystal. what needs to be done for the solute to dissolve?

What will happen between the solute ions/molecules and the solvent after what is done above?

A

These attractive interactions need to be broken,

New attractive forces will be established

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28
Q

what is the quantity of a solute that is contained in a particular quantity of solvent or solution.

A

the concentration of a solution

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29
Q

what are intensive properties, examples

A

properties that do not depend on the actual amount of solution, just on the concentration

boiling point, freezing point, density

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30
Q

what are extensive properties, examples?

A

properties that depends on the actual amount,

mass, volume

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31
Q

what is Molarity

A

mol/L

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32
Q

if we add more solute, we _______ the concentration. if we add more solvent we _______ the concentration.

A

increase, decrease

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33
Q

what is the term for the maximum amount of solute that can dissolve in a given amount of solvent at a given temperature

A

solubility

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34
Q

when is a term said to be saturated

A

when its concentration equals the solubility

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35
Q

ml of solution (does/ doesn’t) equal mL of solvent

A

DOES NOT

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36
Q

what is a 25-fold dilution

A

1:25 dilution, initial is 25 times stronger than the new solution

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37
Q

what is a 10-fold dilution

A

1:10 dilution, initial is 10 times stronger than the new solution

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38
Q

what is a concentrated solution of a common reagent, which can be diluted into a working (lower) concentration when needed

A

stock solution

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39
Q

what is something that is 100-fold

A

1:100 dilution, initial is 100 times stronger than the new solution

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40
Q

try all practice problems in Solutions 2

A

okay

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41
Q

A molecule with no interaction is always in the ____ phase

A

gas

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42
Q

Why is H2O a solid at ‐10 C? Why is H2O a liquid at +10 C? Why is H2O a gas at +110 C?

A

The way that atoms and molecules interact with eachother, IMF

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43
Q

what do most physical properties represent

A

Intermolecular forces

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44
Q

What is the only thing that changes w the H2O molecules in solid, liquid, and gas phases

A

the IMF’s holding them together, the atoms stay the same. WATER IS WATER

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45
Q

how do the attraction between molecules and the attraction between atoms within a molecule compare

A

The interaction between molecules is much smaller in magnitude than the interaction between atoms in a molecule

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46
Q

what is the numerical difference between the kJ/mol of an H-O bond in H2O or an H—-O bond connecting to H2O bonds together

A

the kJ/mol of the bond within the water molecule is about 10-20 times more than the kJ/mol connecting to molecules

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47
Q

the stronger the interaction, the _____ the bond

A

shorter

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48
Q

what is energy that is moving

A

kinetic energy

49
Q

velocity is changing all the time, when does it have an average

A

temperature

50
Q

is temperature the same thing as energy or heat?

A

Niether

51
Q

what is temperature manifest to

A

Kinetic Energy

52
Q

IMF bring molecules _______, while KE keeps them

A

close together, apart and moving

53
Q

what is the energy of a body due to its motion

A

Kinetic Energy

54
Q

average kinetic energy is directly proportional to what

A

temperature

55
Q

what is the average KE of a system

A

temperature

56
Q

the higher the Intermolecular interaction, the ______ the boiling point

A

higher

57
Q

Is one molecule of water liquid at room temperature?

A

no, you need more than 1 molecule to have an intermolecular force in order for it to be a solid liquid or gas

58
Q

what are the types of IMF’s between neutral molecules

A

Dispersion forces
Dipole–dipole forces
Hydrogen bonding

59
Q

what are the types of IMF’s that are referred to as van Der Waals forces

A

Dispersion forces,

Dipole–dipole forces

60
Q

what two elements have very similar electronegativity/IMF

A

C and H

61
Q

what is a bond with unequal sharing of e-

A

polar bond

62
Q

why is HCl a polar molecule

A

it has a net dipole moment, electrons are pulled more towards the Cl because it is more electronegative

63
Q

why is CO2 not polar

A

it does not have a net dipole moment, the two O’s pull at the C evenly so one side is not different than the other

64
Q

why is H2O polar

A

it has a net dipole moment, since it is bent from O lone pair e-, the H atoms create a weird angle to pull the electronegativity

65
Q

in a net dipole moment, the magnitude is in units called what

A

Debye

66
Q

in a dipole-dipole interaction, the positive end of a polar molecule is attracted to the ______ end of its neighbor

A

negative

67
Q

the more polar the molecule, the ______ the boiling Point

A

higher

68
Q

A nonpolar particle (helium atoms below) can be temporarily _______

A

polarized

69
Q

The tendency of an electron cloud to distort is called its what

A

polarizability.

70
Q

The magnitude of these IMF’s ______ with the size of the atom/molecule

A

increases

71
Q

For molecules of similar mass, the magnitude of the dispersion force depends on ______

A

the shape of the molecule

72
Q

The higher the dispersion force, the _____ the boiling point

A

higher

73
Q

what would have a higher dispersion force, a linear or spherical molecule

A

linear because linear has larger surface area which creates more intermolecular contact which increases dispersion forces

74
Q

why does induced dipole forces increase in strength as atoms get larger

A

Induced dipole forces are stronger with more electrons

75
Q

can London forces exist in polar molecules?

A

YES!

76
Q

Dispersion forces and dipole‐dipole forces are referred to collectively as ________

A

van der Waals

forces.

77
Q

If two molecules are of comparable size and shape, what will likely be the dominating force?

A

dipole–dipole interactions

78
Q

If one molecule is much larger than another, dispersion forces will likely determine its ______

A

physical properties

79
Q

what causes an outlier or extreme jump in boiling points

A

hydrogen bonding

80
Q

what is an attraction between a hydrogen atom attached to a highly electronegative atom and a nearby small electronegative atom in another molecule or chemical group

A

a hydrogen bond

81
Q

what elements participate in hydrogen bonding

A

F, O, N

82
Q

electron geometry for 2 electron regions

A

linear

83
Q

electron geometry for 3 electron regions

A

trigonal planar

84
Q

electron geometry for 4 electron regions

A

tetrahedral

85
Q

electron geometry for 5 electron regions

A

trigonal bipyramidal

86
Q

electron geometry for 6 electron regions

A

octahedral

87
Q

why is NH3 a trigonal pyramid but BCl3 a trigonal planar

A

N has a lone pair of electron that changes geometry

88
Q

why is H2O bent but CO2 linear

A

CO2 has 2 double bonds with no lone pairs while H2O only has single bonds and has two lone pairs on Oxygen

89
Q

more e- accounts for _____ London attractive forces

A

stronger

90
Q

what is the reason why water is liquid at room temperature instead of gas

A

hydrogen bonds

91
Q

whats the lifetime of a single hydrogen bond

A

1 ps

92
Q

how much is the molecular dynamics simulation about liquid water slowed down to

A

10^11 times

93
Q

strength of dispersion forces

A

.05-20 kJ/mol

94
Q

strength of dipole-dipole forces

A

3-20 kJ/mol

95
Q

strength of hydrogen bonding forces

A

10-40 kJ/mol

96
Q

strength of ion-dipole forces

A

30-100 kJ/mol

97
Q

example of ion-dipole forces

A

ionic compound (like NaCl) dissolved in water

98
Q

what is an excellent solvent for many ionic substances

A

water

99
Q

what are DNA strands held together by

A

strong interaction, hydrogen bonds

100
Q

why is DNA more stable as a double helix than a single?

A

because the Hydrogen bonds make it very stable

101
Q

As IMF’s increase, what happens to the trend of vapor pressure

A

It decreases

102
Q

electron domain, hybridization, and bond angle of linear

A

2, sp, 180

103
Q

electron domain, hybridization, and bond angle of trigonal planar

A

3, sp2, 120

104
Q

electron domain, hybridization, and bond angle of tetrahedral

A

4, sp3, 109.5

105
Q

electron domain, hybridization, and bond angle of trigonal bipyramidal

A

5, sp3d, 120 and 90

106
Q

electron domain, hybridization, and bond angle of octahedral

A

6, sp3d2, 90

107
Q

electron domain, hybridization, and bond angle of trigonal pyramid

A

4, sp3, 109.5

108
Q

electron domain, hybridization, and bond angle of bent

A

4, sp3, 104

109
Q

molecular geometry of 5 electron domains with 1 lone pair

A

see saw

110
Q

molecular geometry of 5 electron domains with 2 lone pairs

A

T-shaped

111
Q

molecular geometry of 5 electron domains with 3 lone pairs

A

linear

112
Q

molecular geometry of 6 electron domains with 1 lone pair

A

square pyramidal

113
Q

molecular geometry of 6 electron domains with 2 lone pairs

A

square planar

114
Q

molecular geometry of 6 electron domains with 3 lone pairs

A

T-shaped

115
Q

molecular geometry of 6 electron domains with 4 lone pairs

A

linear

116
Q

does Hydrogen bonding exist is 1 water molecule

A

no, it only exists if there is at least 2 water molecules

117
Q

does dipole dipole interactions exist with only one polar molecule

A

no, you need at least two polar molecules

118
Q

If a molecule is larger, is the polarizability higher or lower

A

Higher

college chem 117 (7 decks)

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