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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
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
Cl-, Na+
26
is water polar or non polar
polar
27
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?
These attractive interactions need to be broken, New attractive forces will be established
28
what is the quantity of a solute that is contained in a particular quantity of solvent or solution.
the concentration of a solution
29
what are intensive properties, examples
properties that do not depend on the actual amount of solution, just on the concentration boiling point, freezing point, density
30
what are extensive properties, examples?
properties that depends on the actual amount, mass, volume
31
what is Molarity
mol/L
32
if we add more solute, we _______ the concentration. if we add more solvent we _______ the concentration.
increase, decrease
33
what is the term for the maximum amount of solute that can dissolve in a given amount of solvent at a given temperature
solubility
34
when is a term said to be saturated
when its concentration equals the solubility
35
ml of solution (does/ doesn't) equal mL of solvent
DOES NOT
36
what is a 25-fold dilution
1:25 dilution, initial is 25 times stronger than the new solution
37
what is a 10-fold dilution
1:10 dilution, initial is 10 times stronger than the new solution
38
what is a concentrated solution of a common reagent, which can be diluted into a working (lower) concentration when needed
stock solution
39
what is something that is 100-fold
1:100 dilution, initial is 100 times stronger than the new solution
40
try all practice problems in Solutions 2
okay
41
A molecule with no interaction is always in the ____ phase
gas
42
Why is H2O a solid at ‐10 C? Why is H2O a liquid at +10 C? Why is H2O a gas at +110 C?
The way that atoms and molecules interact with eachother, IMF
43
what do most physical properties represent
Intermolecular forces
44
What is the only thing that changes w the H2O molecules in solid, liquid, and gas phases
the IMF’s holding them together, the atoms stay the same. WATER IS WATER
45
how do the attraction between molecules and the attraction between atoms within a molecule compare
The interaction between molecules is much smaller in magnitude than the interaction between atoms in a molecule
46
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
the kJ/mol of the bond within the water molecule is about 10-20 times more than the kJ/mol connecting to molecules
47
the stronger the interaction, the _____ the bond
shorter
48
what is energy that is moving
kinetic energy
49
velocity is changing all the time, when does it have an average
temperature
50
is temperature the same thing as energy or heat?
Niether
51
what is temperature manifest to
Kinetic Energy
52
IMF bring molecules _______, while KE keeps them
close together, apart and moving
53
what is the energy of a body due to its motion
Kinetic Energy
54
average kinetic energy is directly proportional to what
temperature
55
what is the average KE of a system
temperature
56
the higher the Intermolecular interaction, the ______ the boiling point
higher
57
Is one molecule of water liquid at room temperature?
no, you need more than 1 molecule to have an intermolecular force in order for it to be a solid liquid or gas
58
what are the types of IMF's between neutral molecules
Dispersion forces Dipole–dipole forces Hydrogen bonding
59
what are the types of IMF's that are referred to as van Der Waals forces
Dispersion forces, | Dipole–dipole forces
60
what two elements have very similar electronegativity/IMF
C and H
61
what is a bond with unequal sharing of e-
polar bond
62
why is HCl a polar molecule
it has a net dipole moment, electrons are pulled more towards the Cl because it is more electronegative
63
why is CO2 not polar
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
why is H2O polar
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
in a net dipole moment, the magnitude is in units called what
Debye
66
in a dipole-dipole interaction, the positive end of a polar molecule is attracted to the ______ end of its neighbor
negative
67
the more polar the molecule, the ______ the boiling Point
higher
68
A nonpolar particle (helium atoms below) can be temporarily _______
polarized
69
The tendency of an electron cloud to distort is called its what
polarizability.
70
The magnitude of these IMF's ______ with the size of the atom/molecule
increases
71
For molecules of similar mass, the magnitude of the dispersion force depends on ______
the shape of the molecule
72
The higher the dispersion force, the _____ the boiling point
higher
73
what would have a higher dispersion force, a linear or spherical molecule
linear because linear has larger surface area which creates more intermolecular contact which increases dispersion forces
74
why does induced dipole forces increase in strength as atoms get larger
Induced dipole forces are stronger with more electrons
75
can London forces exist in polar molecules?
YES!
76
Dispersion forces and dipole‐dipole forces are referred to collectively as ________
van der Waals | forces.
77
If two molecules are of comparable size and shape, what will likely be the dominating force?
dipole–dipole interactions
78
If one molecule is much larger than another, dispersion forces will likely determine its ______
physical properties
79
what causes an outlier or extreme jump in boiling points
hydrogen bonding
80
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 hydrogen bond
81
what elements participate in hydrogen bonding
F, O, N
82
electron geometry for 2 electron regions
linear
83
electron geometry for 3 electron regions
trigonal planar
84
electron geometry for 4 electron regions
tetrahedral
85
electron geometry for 5 electron regions
trigonal bipyramidal
86
electron geometry for 6 electron regions
octahedral
87
why is NH3 a trigonal pyramid but BCl3 a trigonal planar
N has a lone pair of electron that changes geometry
88
why is H2O bent but CO2 linear
CO2 has 2 double bonds with no lone pairs while H2O only has single bonds and has two lone pairs on Oxygen
89
more e- accounts for _____ London attractive forces
stronger
90
what is the reason why water is liquid at room temperature instead of gas
hydrogen bonds
91
whats the lifetime of a single hydrogen bond
1 ps
92
how much is the molecular dynamics simulation about liquid water slowed down to
10^11 times
93
strength of dispersion forces
.05-20 kJ/mol
94
strength of dipole-dipole forces
3-20 kJ/mol
95
strength of hydrogen bonding forces
10-40 kJ/mol
96
strength of ion-dipole forces
30-100 kJ/mol
97
example of ion-dipole forces
ionic compound (like NaCl) dissolved in water
98
what is an excellent solvent for many ionic substances
water
99
what are DNA strands held together by
strong interaction, hydrogen bonds
100
why is DNA more stable as a double helix than a single?
because the Hydrogen bonds make it very stable
101
As IMF’s increase, what happens to the trend of vapor pressure
It decreases
102
electron domain, hybridization, and bond angle of linear
2, sp, 180
103
electron domain, hybridization, and bond angle of trigonal planar
3, sp2, 120
104
electron domain, hybridization, and bond angle of tetrahedral
4, sp3, 109.5
105
electron domain, hybridization, and bond angle of trigonal bipyramidal
5, sp3d, 120 and 90
106
electron domain, hybridization, and bond angle of octahedral
6, sp3d2, 90
107
electron domain, hybridization, and bond angle of trigonal pyramid
4, sp3, 109.5
108
electron domain, hybridization, and bond angle of bent
4, sp3, 104
109
molecular geometry of 5 electron domains with 1 lone pair
see saw
110
molecular geometry of 5 electron domains with 2 lone pairs
T-shaped
111
molecular geometry of 5 electron domains with 3 lone pairs
linear
112
molecular geometry of 6 electron domains with 1 lone pair
square pyramidal
113
molecular geometry of 6 electron domains with 2 lone pairs
square planar
114
molecular geometry of 6 electron domains with 3 lone pairs
T-shaped
115
molecular geometry of 6 electron domains with 4 lone pairs
linear
116
does Hydrogen bonding exist is 1 water molecule
no, it only exists if there is at least 2 water molecules
117
does dipole dipole interactions exist with only one polar molecule
no, you need at least two polar molecules
118
If a molecule is larger, is the polarizability higher or lower
Higher

college chem 117 (7 decks)

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