Chp 7 Book Flashcards
(144 cards)
1
Q
The kinetic Molecular Theory of Matter attempts to describe
A
All the states of matter & the conversion between the states
2
Q
What are the 3 encountered states of matter?
A
Solid, Liquid & Gas
2
Q
Solids are classifies as having
A
A definite shape & volume
3
Q
In solids, what is holding the molecules, atoms, or ions in place?
A
Intermolecular forces
4
Q
Liquids are characterized by
A
A definite volume but NOT shape
5
Q
The forces between liquid particles are
A
Weak
6
Q
The particles comprising both liquid & solid are essentially
A
Touching
7
Q
Which 2 states are not easily compressible?
A
Solids & Liquids
(condensed states of matter)
8
Q
Gases have neither a
A
Definite Shape nor Volume
9
Q
A gas will expand to fill the
A
Available space
10
Q
Melting is the conversion of a
A
Solid into a Liquid
11
Q
The reverse process of a liquid to a solid is called
A
Freezing
12
Q
What is vaporization?
A
Liquid vaporizing into a gas
13
Q
Conversion of a gas into a solid is called
A
Deposition
14
Q
What is sublimation?
A
Conversion of a solid directly into a gas
15
Q
Chemical bonds may hold
A
Atoms together into molecules
16
Q
Intermolecular forces determine how
A
Molecules interact with one another
17
Q
Intermolecular forces are determined by chemical bonding & it is the intermolecular forces that
A
Most directly impact the macroscopic properties of a sample
18
Q
The collective inert repulsion is known as
A
Intermolecular forces because they occur between different molecules
18
Q
All molecules & atoms & oppositely charged ions have an
A
Inert attraction for each other as long as they do not get too close
19
Q
Intermolecular forces are ________ in nature
A
Electrostatic
20
Q
What is responsible for the type & strength of the intermolecular forces?
A
Organization of electrons & 3-D arrangement
21
Q
What are the 2 limiting chemical bonds?
A
Ionic bonds
Covalent Bonds
22
Q
What is the overarching driving force in the formation of chemical bonds
A
Octet Rule
23
Every atom wants
8 valence electrons
24
What are valence electrons?
The electrons in the highest energy or valence shell
25
What has filled valence shells?
Noble gases
26
Isoelectric species have the same
Electron configuration
27
Elements that are only 1 or 2 atomic numbers away from a noble gas form
Ions
28
Metals will _____ an electron or two to achieve a noble gas-like electron configuration, forming a ______
Give Up
Cation
29
Non-metals _____an electron or two, forming______
Acquire
Anion
30
Ionic compounds are formed between
Metals & Non-metals
31
Metals are good
Electrical conductors because they do not hold onto their electrons strongly
32
What is more better at attracting electrons?
Non-metals
33
The capacity of each shell is equal to the
Number of electrons in that specific row of the periodic table
34
Helium is chemically
Inert
35
Electrons in filled shells are called
Core/Kernel Electrons
36
Core electrons are virtually
Inert because the represent complete "collections" of electrons
37
Electrons in partially filled shells are called
Valence Electrons
38
Valence electrons are used in forming
Chemical Bonds
39
For representative elements, the number of valence electrons is
Equal to the group number
40
An ionic bond results from
Coulombic attraction between oppositely charged ions
41
Ionic bonds are stronger than
Covalent bonds
42
Every ionic compound is a
Solid at room temperature & pressure
43
Ionic melts conduct
Electricity
44
45
46
47
48
49
50
51
52
53
Covalent bonds result from sharing
One or more pairs of electrons
53
54
Electron shells are divided into
Subshells, then orbitals
55
The shell, subshell & orbital quantum numbers describes the
Quantum state or energy of an electron in a given orbital
56
The orbital describes a
Region in space
57
Electrons also behave as
Waves
58
An orbital is a mathematical function that describes
The wave nature of an electron
59
A covalent bond results from sharing one or more
Pairs of electrons between two atoms through the overlap of their valence electron clouds
60
The electron is bound to the nucleus because the ______________is attracted to the ____________by Coulomb's Law
Negatively Charges Electrons
Positively Charged Nucleus
61
A covalent bond results from sharing of the
Negatively charged electrons between two positively charged nuclei
62
The presence of electrons between 2 nuclei will
Shield the nuclei from each other, reducing the magnitude of the Coulombic repulsive force
This stabilizes the molecule by lowering its overall energy
63
Having less energy means
More stable
64
The closer the electrons
The weaker the bond
65
In the Lewis Structure, the lines represent
Shared pairs
66
Hydrogens are often bonded to
Oxygen
67
What is an isomer?
Compounds that are different but have the same molecular formula
68
Only the ______are used in forming covalent bonds
Valence Electrons
69
What is resonance?
There is more than once acceptable Lewis structure for a compound
70
Atoms are bound into molecules by
Shared pairs of electrons
71
What is VSEPR?
Valence Shell Electron Pair Repulsion Theory
72
VSEPR is helpful in predicting
The shapes of molecules
73
Molecular geometry describes the
Spatial arrangement of atoms
74
Diatomic has a
Linear geometry
75
Linear molecules include the molecular geometry class known as
AX2
A=central atom
X= stick on groups (ligand)
76
Trigonal planar species has bond angles of
120
(no lone pairs)
77
Molecules that consist of central atom with 4 stick on groups are denoted as
AX4
78
Tetrahedral bond angles increase just over
109
79
Molecules belonging to the geometry classes AX2E2 are
Bent or non-linear
80
Water is a good example of a
Bent molecule
81
AX3E will have
A pyramidal geometry
82
What is electronegativity?
Atoms pulling electrons towards themselves
83
Which element is the most electronegative?
Fluorine
84
What makes a bond non-polar?
If 2 atoms of IDENTICAL electronegativity are bonded together
85
What is an electron hot spot?
Where excess electron density leads to the accumulation of electric charges
86
Homodiatomic molecules are always
Non-polar
87
If 2 atoms of different electronegativity are bonded, the bond is
Polar
88
The uneven sharing of electrons leads to the formation of
Partial charge
89
An ionic charge is a full
Integral multiple of the charge on an electron or proton
90
Electrons have what type of charge?
Negative
91
The increase in electron density around the more electronegative atom leads to a
Buildup of partial negative charge on that atom
92
The less electronegative atom has a lower electron density & develops
A partial positive charge
93
Bond dipoles are
Vectors
94
The overall polarity of a molecule depends on the
Vector sum of the bond dipoles
95
What are the 3 principal interactions?
Dipole-Dipole
Hydrogen Bonding
London Forces
(ion-dipole)
96
What is the Dipole-Dipole Attraction?
Attraction between the opposite (partial) charges of polar molecules
97
Dipole attractions only occur between
Polar molecules
98
What is stronger than a dipole-dipole attraction?
Hydrogen bonding
99
Hydrogen bonding is a type of ______interaction
Dipole
100
When is a hydrogen bond made possible?
Only when a hydrogen atom is directly bonded to F, O, or N
101
Which is the most important intermolecular force?
Hydrogen bonding
(holds DNA)
101
Which is the weakest intermolecular force?
London forces, but most important
102
Larger molecules will show
More/stronger London forces because large molecules have more electrons
103
A London force is the result of an
Instantaneous dipole that is created whenever electrons in a molecule are unevenly distributed
104
All molecules & atoms that have electrons exhibit
London forces
105
Larger atoms & molecules have more electrons so,
Uneven distribution of electrons is greater
106
Ion-dipole attractions occur between an
Ion & a polar molecule
107
The strength of what force varies widely & depends on the magnitude of the dipole moment of the polar species & the size of the ion?
Ion-Dipole
108
Water is a very
Polar molecule
109
Polar molecules that can participate in dipole-dipole interaction tend to have
Much greater degree of attraction between molecules than non-polar species
110
Ionic compounds are soluble in
Water
111
Hydrocarbons are
Non-polar
112
Majority of organic compounds are
Not soluble in water
113
Substances that have greater intermolecular attractions have greater
Surface tension
114
Molecules in a liquid state are attracted to all neighboring molecules by
Intermolecular forces
115
A molecule near the surface experiences
Attractive forces to all of the surrounding surface molecules & with the molecules below it in the liquid
116
Water has a high
Surface tension
117
Cohesive forces/cohesion cause
A substance to be more attracted to itself
118
The amount of curvature & the height of the droplet depends on the
Intermolecular forces between the liquid & the surface, as well as on the surface tension of the liquid
119
The contact angle is the angle between the
Surface & the line tangent to the point where the edges of the droplet meets the surface
120
As the radius of the tube decreases,
The curvature of the meniscus also decreases
121
Capillary rise/action is a second effect caused by
Surface tension
122
Capillary rise is the tendency of a fluid to
Rise into a narrow-diameter tube
(amount of rise depends on the diameter)
123
When a liquid is in contact with another surface, what happens to the pressure difference?
The curling of the liquid causes a pressure difference (Laplace Law)
124
What is the surface tension of water?
0.073
125
Tension is proportional to
The radius of the vessel
126
Surfactant improve
A solvents ability to be a solvent by reducing the surface tension of the solvent
127
A fatty acid is a
Long chained carboxylic acid having 12-18 carbon atoms
128
Detergents can be
Positively, negatively & uncharged
129
Polar is hydro
Philic
130
Non polar is hydro
Phobic
131
What are the 3 ways in which a surfactant molecule will react
Formation of monolayers, bilayers or micelles
132
Adding a surfactant will decrease
The surface tension of the water due to surfactant molecule disrupting the hydrogen bonding
133
How is a bilayer formed?
The tail of the surfactant molecule dissolves in each other to form a double layer
134
Polar solutes like ions will not
Enter the nonpolar region unless carried/forced
135
Soaps & detergents lose their
Bactericidal property at low concentrations
136
What is a Micelle?
Spherical, a formation that creates a non polar microenvironment
137
Viscosity increases with
Increasing intermolecular forces
138
Viscosity increases with
Increasing intermolecular forces
139
Viscosity is a measure of a fluids
Resistance to flow
140
Substances with greater intermolecular forces have low
Vapor pressure
