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CHM012 > TOPIC 6- Liquids and Solids > Flashcards

TOPIC 6- Liquids and Solids Flashcards

1
Q

The fundamental difference between states of matter is the strength of the

A

Intermolecular forces of attraction

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2
Q

Stronger intermolecular force

A

bring molecules closer together

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3
Q

What are the condensed state of matter?

A

Liquids and Solids

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4
Q

Liquids and Solids are formed by forces that may involve?

A

Covalent bonding
Ionic Bonding
Intermolecular Forces

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5
Q

They are forces that occur between molecules

A

Intermolecular Forces (IMF)

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6
Q

The attraction between molecule are not nearly as strong as

A

intermolecular attractions (bonds)

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7
Q

What are the physical properties that reflect IMF?

A

Boiling points
Melting points
Viscosity
Surface Tension
Capillary action

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8
Q

What are the types of IMFs?

A

Dispersion forces
Dipole-dipole forces
Hydrogen Bonding
Ion-dipole forces

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9
Q

What forces are van der Waals forces

A

Dispersion forces
Dipole-Dipole forces

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10
Q

Instantaneous dipole that occurs in a given atm induces a similar dipole in a neighboring atom which instigates weak and short-lived interatomic attraction.

A

London Dispersion Forces

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11
Q

It is the tendency of an electron cloud to distort

A

Polarizability

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12
Q

Factors that affect dispersion force in a molecule are?

A
  1. number of electrons in an atom
  2. size of atom or molecule/molecular weight
  3. Shape of molecules with similar masses
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13
Q

In London dispersion, more electrons

A

more dispersion force

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14
Q

In London dispersion, more compact

A

less dispersion force

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15
Q

It is exhibited by molecules with polar bonds that behave in an electric field

A

Dipole-dipole Forces

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16
Q

In dipole-dipole forces, as distance between dipoles increase

A

forces grow weaker

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17
Q

For molecules of approximately equal mass and size, the more polar the molecule

A

the higher its boiling point

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18
Q

Strong dipole-dipole forces can be noticed when H is bound to highly electronegative atoms like N, O, and F.

A

Hydrogen Bonding

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19
Q

In Hydrogen bonding, strength can be characterized by:

A
  1. Polarity of the bond
  2. Close approach of the dipoles
  3. Small size of the H atom
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20
Q

If two molecules are of comparable size and shape,

A

dipole dipole interaction will likely be dominating force

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21
Q

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

A

physical properties

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22
Q

are found in solutions of ions and the strength of these forces is what makes it possible for ionic substance to dissolve in polar solvent

A

Ion-dipole interactions

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23
Q

Liquids exhibit?

A

low compressibility, lack of rigidity and high density

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24
Q

it is the resistance of a liquid to an increase surface area

A

Surface Tension

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25
Q

Liquids with large intermolecular forces tend to have

A

high surface tensions

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26
Q

is a spontaneous rising of a liquid in a narrow tube

A

Capillary Action

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27
Q

attract the liquid to the wall of the tube

A

Adhesive forces

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28
Q

attract the liquid to itself

A

Cohesive forces

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29
Q

this refers to the measure of a liquid’s resistance to flow

A

Viscosity

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30
Q

Liquids with high IMF tend to be?

A

Highly Viscous

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31
Q

It is the conversion from one state of matter to another

A

Phase Change

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32
Q

Energy is either _________ or __________ in a phase change

A

Added, released

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33
Q

what heat is required to change a solid at its melting point to a liquid

A

Heat of fusion

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34
Q

what heat is required to change a liquid at its boiling point to a gas

A

heat of vaporization

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35
Q

what heat is required to change a solid directly to a gas

A

heat of sublimation

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36
Q

A plot of temperature vs. heat added is called

A

heating curve

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37
Q

the amount of heat needed to raise the temperature of a substance is the product of

A

specific heat, sample mass, and temperature change

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38
Q

Why does the temperature of a substance does not rise during a phase change?

A

because the added energy is used to overcome the attractive forces between molecules

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39
Q

During phase change, what is the product of mass and the heat of fusion or vaporization?

A

Heat

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40
Q

At any temperature, some liquid molecules have enough energy to escape the surface and become gas

A

Vapor Pressure

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41
Q

As more molecules escape the liquid,

A

the pressure they exert increases

42
Q

The vapor pressure present at equilibrium is also called

A

Equilibrium vapor pressure

43
Q

Liquids with large intermolecular forces have relatively

A

low vapor pressure since molecules need a higher energy to escape the vapor phase

44
Q

Substances with large molar masses have

A

low vapor pressure since it attributes to larger dispersion forces

45
Q

Is the temperature at which its vapor pressure equals atmospheric pressure

A

Boiling Point

46
Q

is the temperature at which its vapor pressure is 760 torr or 1atm

A

Normal Boiling Point

47
Q

temperature at which solid and liquid states have identical vapor pressure and total pressure=1atm

A

Normal melting point

48
Q

The natural log of the vapor pressure of a liquid is INVERSELY proportional to its temperature

A

Clausius-Claude Clapeyron Equation

49
Q

Convenient way of representing the phase of substance as function of its temperature

A

Phase Diagrams

50
Q

The temperature at which all three phases exist simultaneously

A

Triple Point

51
Q

The critical pressure and critical temperature, together, define this point.

A

Critical Point

52
Q

Pressure required to produce liquefaction at critical temperature.

A

Critical Pressure

53
Q

The temperature above with a liquid cannot be liquified, irrespective of pressure applied.

A

Critical Temperature

54
Q

What are the two classification of solids?

A
  1. Amorphous Solids
  2. Crystalline Solids
55
Q

Have disordered structures

A

Amorphous solids

56
Q

have a highly regular arrangement of components.

A

Crystalline Solids

57
Q

In crystalline solids, position of the components are represented by

A

lattices

58
Q

It is a three-dimensional system of points that designates the position of the components of a substance

A

Lattices

59
Q

It is the basis of a repeating pattern

A

Unit Cell

60
Q

The structure of the crystalline solid is defined by:

A
  1. Size and shape of the unit cell
  2. The locations of atoms within the unit cell.
61
Q

Positions that define the overall structure of the crystalline compound

A

Lattice Points

62
Q

They connect the points and define the unit cell

A

Lattice Vectors

63
Q

have atoms only in lattice points

A

Primitive Lattices

64
Q

have atoms in another regular location most commonly the body-center or the face-center.

A

Centered Lattice

65
Q

Is used to determine the structure of crystalline solids

A

X-ray Diffraction

66
Q

Is used to carry out X-ray analysis of crystals.

A

Diffractometer

67
Q

What are the types of crystalline solid?

A
  1. Ionic Solids
  2. Molecular Solids
  3. Atomic Solids
68
Q

Possess ions at the points of the lattice that describe their structure.

A

Ionic Solids

69
Q

Have discrete covalently bonded molecules at each lattice point(s)

A

Molecular Solids

70
Q

has atoms at the lattice points that describe its structure

A

Atomic Solids

71
Q

Is an arrangement that assumes that metal atoms are hard, uniform spheres

A

Closest Packing

72
Q

Forms of closest packing:

A
  1. ABA Packing
  2. ABC Packing
73
Q

2nd layer is like the first but it is displaced so that sphere in the second layer occupies a dimple in the 1st layer. the spheres in the 3rd layer occupy dimples in the 2nd layer and lie directly over those in the 1st.

A

ABA Packing

74
Q

The resultant structure of ABA packig

A

Hexagonal closest packed (hcp) structures.

75
Q

When the spheres are aba closest packed, the unit cell is a

A

hexagonal prism

76
Q

The spheres in the 3rd layer occupy dimples in the 2nd layer.

A

ABC packing

77
Q

Resultant structure in ABC packing

A

cubic closest packed (CCP) structure

78
Q

In ABC packing, the unit cell is

A

Face-centered cubic

79
Q

Common characteristics of the hcp and the ccp structures

A

Each sphere in both structure possesses 12 equivalent nearest neighbors

80
Q

A successful bonding model for metals must consider:

A
  1. Malleability
  2. Ductility
  3. Efficient uniform conduction of heat and electricity
81
Q

Bonding models of metal include;

A
  1. Electron sea model
  2. Band Model (molecular orbital model)
82
Q

A regular array of metal cations are considered to be in a

A

electron sea model

83
Q

Mobile electrons conduct

A

heat and electricity

84
Q

In electron sea model __________ are explained

A

thermal conductivity, ductility, and malleability of metals

85
Q

As the energy of atoms in a chain increases, the energy gap between bonding orbitals and between antibonding orbitals _________-

A

disappears

86
Q

Is a substance that contains a mix of elements and possesses metallic properties

A

Alloy

87
Q

What are the classifications of alloy

A
  1. Substitutional alloy
  2. Interstitial alloy
  3. Heterogeneous alloys
88
Q

some of the host metal atoms are replaced by other metal atoms of similar size

A

Substitutional Alloy

89
Q

Some of the holes in the closest packed metal structure are occupied by small atoms

A

Interstitial alloy

90
Q

Components not dispersed uniformly

A

Heterogeneous alloys

91
Q

are those atomic solids that contain directional covalent bonds which form solids that can be viewed as “giant solids”

A

Network solids

92
Q

Properties of network solids:

A
  1. Brittle nature
  2. Ineffective conductors of heat and electricity
93
Q

Important elements in network solids

A

Carbon and Silicon

94
Q

Each C atom is surrounded by a tetrahedral arrangement of other C atoms

A

Diamond

95
Q

Slippery, Black, and a conductor of heat and electricity

A

Graphite

96
Q

Structure is based on layers of C atoms arranged in fused six-membered rings

A

Graphite

97
Q

They have gap between the occupied MOs and the unoccupied ones

A

Semiconductors

98
Q

It is changing the conductivity of semiconductors by adding an element with more or fewer electrons

A

Doping

99
Q

have more valence electrons than those in the host crystal

A

N-type semiconductor

100
Q

have fewer valence electrons than those in the host crystal

A

P-type semiconductor

101
Q

Possess strong covalent bonding with molecules but weak forces between molecules

A

Molecular Solids

102
Q

the lattice comprises alternately charged ions. held together by strong electrostatic forces

A

Ionic solids

CHM012 (9 decks)

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