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Chem 101 > Intermolecular Forces, Liquids, Solids and Materials > Flashcards

Intermolecular Forces, Liquids, Solids and Materials Flashcards

1
Q

Solids

A

Ordered, particles do not change position, close together, no diffusion, incompressible.

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2
Q

Liquids

A

Some disorder, particles move, close together, slow diffusion, incompressible.

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3
Q

Gas

A

Total disorders, empty space, rapid diffusion, compressible.

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4
Q

Kinetic Energy

A

The kinetic energy of a particle is temperature depended and keeps particles separated. One of the factors that changes states of a substance. Higher kinetic energy over powers intermolecular forces, causing them to break (gases.)

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5
Q

Strength of attraction

A

The strength of attraction between particles draws particles together. Higher the attraction, the stronger the intermolecular forces.

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6
Q

Intermolecular forces (van der Waals)

A

Strength depends on polarity. More polar or highly charged = stronger the attraction. Larger molecules have more intermolecular forces

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7
Q

Ion-dipole forces

A

Attraction of a full charge to a partial charge, in soluble solids, anion and cation dipole moments cancel out the lattice energy (dissolve). Responsible for ionic substances dissolving in polar solvents.

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8
Q

Dipole-dipole forces

A

Partial neg and pos ends on polar molecules are attracted to each other. Increases with electronegativity.

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9
Q

Hydrogen bonding

A

Strongest dipole bond, occurs when a hydrogen molecule bonds to a highly electronegative molecule - F, N, O and the nucleus is consequentially exposed.

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10
Q

Water properites

A

Very strong H-bonding (2 bonds). Has stronger bonding in its liquid form because molecules can move to fill empty space. The density of ice is lower because of empty spaces in the bonding structure.

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11
Q

London Dispersion forces

A

Present in all molecules, more so in larger ones. Attraction of an instantaneous dipole to an induced dipole. Electrons are asymmetrically arranged around the nucleus, making the atom slightly polarized. Long, skinny molecules have stronger dispersion forces than short, broad ones.

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12
Q

Boiling point

A

Increases with molecular weight and electronegativity. Occurs when vapour pressure is equal to the external pressure. The normal boiling point is the temperature when the liquid’s vapour pressures is 1 atm.

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13
Q

Melting point

A

Increases with electronegativity and efficient packing of molecules.

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14
Q

Order of intermolecular forces

A

Ionic > covalent > ion-dipole > H-bonds > dipole-dipole > dispersion

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15
Q

Liquids

A

Properties depend on a balance between kinetic energy and intermolecular attractive forces.

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16
Q

Viscosity

A

Resistance to flow, increases with stronger intermolecular forces, higher molecular weights and molecules that get easily entangled.

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17
Q

Surface tension

A

Created by an imbalance of forces at the top of a liquid. Related to the work required to increase surface area by a unit amount and interfacial behavior.

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18
Q

Interfacial behavior

A

Cohesive and adhesive forces.

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19
Q

Cohesive forces

A

Binds molecules to one another

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20
Q

Adhesive forces

A

Binds molecules to the surface

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21
Q

Concave surface

A

Adhesive forces > cohesive forces. ex) water

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22
Q

Convex surface

A

Cohesive forces > adhesive forces ex) mercury

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23
Q

Capillary action

A

Strong adhesive forces draw liquid along the sides of tubes and pores, cohesive forces pull along the rest of the liquid.

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24
Q

Evaporation

A

When energetic molecules/atoms near the surface of a liquid exceed intermolecular forces to transition from liquid to gas. Ease of this dictates boiling point and vapour pressure.

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25
Q

Open system

A

Molecules evaporate and are removed

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26
Q

Closed system

A

Molecules evaporate and condense at the same rate (equillibrium)

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27
Q

Vapour pressure

A

Increases with temperature and thus increases with kinetic energy and decreases with stronger intermolecular forces.

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28
Q

Vapourization

A

When molecules escape the surface of the liquid into a gas, increases with temperature (kinetic energy, low boiling point) and surface area. Decreases with strong intermolecular forces.

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29
Q

Volatile liquids

A

Evaporate easily, have high vapour pressure at room temperature.

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30
Q

Phase changes

A

Changes in a physical state with no change in composition. Involves energy changes.

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31
Q

Phase diagrams

A

Plot changes in matter states as a function of pressure and temperature.

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32
Q

Deposition

A

Change from gas to solid

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33
Q

Sublimation

A

Change from solid to gas

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34
Q

Freezing

A

Change from liquid to solid

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35
Q

Melting

A

Change from solid to liquid

36
Q

Condensing

A

Change from gas to liquid

37
Q

Boiling

A

Change from liquid to gas

38
Q

Supercritical fluid

A

Has properties between a liquid and a gas

39
Q

Triple point

A

A point where the temperature and pressure allows all three matter states to exist in equilibrium.

40
Q

Critical point

A

Transition to supercritical fluid

41
Q

Liquid Crystals

A

Have some order. Exhibit one or more ordered phases at a temperature above the melting point. Long and rod-like, normal liquid phases are randomly oriented.

42
Q

Nematic crystals

A

Ordered along the long axis

43
Q

Smectic

A

Ordered along the long axis and in another dimension

44
Q

Cholesteric

A

Ordered along the long axis of the molecule and twisted in layers

45
Q

Solids

A

Intermolecular forces are strong enough to lock particles in fixed positions.

46
Q

Crystalline solids

A

Particles arranged in a repeating pattern - metals, minerals

47
Q

Amorphous solids

A

Randomly arranged particles - glass, wax.

48
Q

Molecular solids

A

Atoms or molecules held together by intermolecular forces. Usually soft, low melting points, low thermal and electrical conductivity. Efficient packing of molecules is important.

49
Q

Metallic solides

A

Metallic bonding, conduct electricity, made of metal atoms. Valence electrons are delocalized throughout the solid, vary greatly in bond strength - best described via band theory.

50
Q

Ionic solids

A

Ions held together by ionic bonds. Larger the charges and smaller the distance on the periodic table, stronger the ionic bonds. They are hard, brittle and have high melting points. Structure depends on charges on the ions and sizes.

51
Q

Covalent network solids

A

Atoms held together in large network of chains with strong covalent bonds. Have higher melting points and are much harder than molecular solids. 3D array of solids. Sometimes layers (ie. graphite) are held together with weak dispersion forces.

52
Q

Semiconductors

A

Inorganic compounds that are semiconductors (silicon) have average 4 valence electrons and conductivity can be increased via doping.

53
Q

Doping

A

Addition of controlled amounts of a second element to a semiconductor. Dopant is usually the 2nd element added.

53
Q

N-type semiconductors

A

Addition of electrons to the conduction band. Dopant atom has more valence electrons than the host atom.

54
Q

P-type semiconductors

A

Subtraction of electrons, which leads to holes in the valence band. Dopant atom has less valence electrons that the host atom.

55
Q

Solar energy cells

A

Produced from semiconductors. Light (photons) shone at the appropriate wavelength promotes electrons to the conduction band and make the material more conductive - generates a current. Formed from n-type and p-type semiconductors in the same direction.

56
Q

Photoconductivity

A

Electrons are promoted by photons to generate a current and make the material more conductive.

57
Q

Light-emitting diodes (LEDs)

A

Opposite of solar cells, voltage is applied to electrons in the conduction band from the n-side to combine with the holes on the p-side. So n-type and p-type are facing each other. Light is emitted when the photons have energy equal to the band gap.

58
Q

Polymers

A

Involve simple molecules (monomers) linked together to make chains, rings, networks and folded constructs. Attracted to each other by variety of covalent and intermolecular forces.

59
Q

Cellulose

A

Polysaccharide chain made of repeating glucose molecules. Found in cotton and paper.

60
Q

Chitin

A

Repeating glucose unit with an attached amide group. Found in insects and crustaceans.

61
Q

Cyclodextrin

A

Ring-shaped molecule that captures odor molecules

62
Q

Lignin

A

Polymer in wood that is resistant to rot, has a complex cross-linked structure.

63
Q

Tannins

A

Small lignin molecules

64
Q

Bakelite

A

First commercial plastic made of phenolic resin

65
Q

Addition polymerization

A

The coupling of monomers through multiple bonds. Formed by breaking the double carbon pi bond and forming a new carbon sigma bond between the monomer and polymer chain. Hard to depolymerize because sigma bonds are stronger than pi bonds.

66
Q

Synthetic polymers

A

Have a backbone of C-C bonds.

67
Q

Plastics

A

Polymeric materials that form various shapes with heat and pressure

68
Q

Themoplastics

A

Materials can be reshaped

69
Q

Themosetting plastics

A

Materials are shaped by an irreversible process

70
Q

Condensation polymerization

A

Two molecules are joined to form a larger molecule via the elimination of a small molecule. HOOC - X - COOH + H2N - Y - NH2 –> …X - CONH - Y…

71
Q

Copolymers

A

Polymers formed by two different monomers

72
Q

Proteins

A

Formed by amino acid monomers that contain amines and carboxylic functional groups.

73
Q

Polypeptide

A

Chain of condensed amino acids that fold to form proteins.

74
Q

Natural polymeric proteins

A

Collages, keratin, fibroin

75
Q

Structure and physical properties of polymers

A

Synthetic and natural polymers commonly consist of a collection of macromolecules of different molecular weights. Intermolecular forces between chains give order to polymers.

76
Q

Crystallinity

A

Order in polymers. Stretching or extruding a polymer can increase it. Strongly influenced by average molecular mass.

77
Q

Factors that affect polymer properties

A

Chain length, branching, polar groups, cross-linking, double bonds, aromatic rings, substituents, stereochemistry (chirality), fabrication, additives.

78
Q

Plasticizers

A

Decrease interactions between chains of polymers and makes them pliable.

79
Q

Cross-linked polymers

A

Crosslinking of natural polymers makes them harder (keratin).

80
Q

Vulcanized rubber

A

More elastic and less reactive than natural rubber due to crosslinking with an unsaturated polymer of sulfur. More rigid than straight chain polymers.

81
Q

Nanomaterials

A

Quantum dots, some metals, carbon nanotubes, graphene

82
Q

Nanoscale semiconductors

A

Semiconductor particles with 1-10nm diameters. Band gaps change substantially with size in this range.

83
Q

Quantum dots

A

Nanoscale semiconductors. Colour is dependent on band gap in the semiconductor. As particles get larger, the colour moves to red. As band gap gets smaller, the colour moves to red. Vice versa is purple. (More energy and shorter wavelength = small particles big band gap. Less energy and larger wavelengths = large particles and small band gap.)

84
Q

Nanoscale metals

A

Used in stained glass

85
Q

Carbon nanotubes

A

Sheets of graphite rolled up and capped at one or both ends. Very long but only 1nm wide. Can be single or multi-walled. Used in nanowires and are mechanically very strong.

86
Q
A

Chem 101 (4 decks)

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