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IMAT Chem > Chapter 5: States of Matter > Flashcards

Chapter 5: States of Matter Flashcards

1
Q

Front

A

Back

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2
Q

What are the key properties of gases?

A

No fixed shape or volume; compressible; random particle arrangement; free movement.

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3
Q

What are the key properties of liquids?

A

Take container shape; fixed volume; slightly compressible; limited movement.

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4
Q

What are the key properties of solids?

A

Fixed shape and volume; incompressible; regular particle arrangement; vibrational movement only.

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5
Q

Name the five types of structures found in elements and compounds.

A

Simple atomic

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6
Q

What determines the state of a substance at room temperature?

A

Its structure and bonding.

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7
Q

What are the assumptions of the ideal gas model?

A

Rapid random motion; negligible volume; no intermolecular forces; elastic collisions.

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8
Q

What is an elastic collision in gases?

A

A collision where no kinetic energy is lost.

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9
Q

What happens during the melting of a solid?

A

Particles vibrate more

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10
Q

What happens during freezing of a liquid?

A

Particles lose energy

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11
Q

What happens during vaporization of a liquid?

A

Particles move faster

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12
Q

What happens during condensation of a gas?

A

Particles lose energy

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13
Q

What is vapour pressure?

A

Pressure exerted by a vapour in equilibrium with its liquid.

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14
Q

How does temperature affect vapour pressure?

A

Vapour pressure increases with temperature.

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15
Q

What is a crystal lattice?

A

A regular repeating arrangement of ions

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16
Q

What are the properties of ionic lattices?

A

Hard

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17
Q

Why are ionic crystals brittle?

A

Same-charge ions align during a blow

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18
Q

What are metallic lattices made of?

A

Metal ions surrounded by delocalized electrons.

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19
Q

Why are metals malleable and ductile?

A

Layers slide while delocalized electrons maintain bonds.

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20
Q

What gives metals high tensile strength?

A

Strong attraction between ions and delocalized electrons.

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21
Q

What is an alloy?

A

A mixture of metals or a metal with a non-metal.

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22
Q

Why are alloys stronger than pure metals?

A

Less regular lattice structure prevents easy sliding of layers.

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23
Q

What is brass made of

A

and where is it used?

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24
Q

What are lightweight aluminum alloys used for?

A

Applications needing strength and corrosion resistance.

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25
Q

What are allotropes?

A

Different molecular forms of the same element.

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26
Q

What are the properties of graphite?

A

High melting points

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27
Q

Why is graphite soft?

A

Weak van der Waals forces between layers.

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28
Q

Why does graphite conduct electricity?

A

Delocalized electrons move along layers.

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29
Q

What are the properties of diamond?

A

Hard

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30
Q

Why is diamond hard?

A

Strong 3D covalent bonds.

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31
Q

What is silicon(IV) oxide similar to?

A

Diamond.

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32
Q

What happens to particles during evaporation?

A

High-energy particles escape

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33
Q

How does boiling differ from evaporation?

A

Boiling occurs at a specific temperature

34
Q

Why do ionic lattices have high melting points?

A

Strong electrostatic attraction between ions.

35
Q

What type of lattice does NaCl form?

A

Giant ionic lattice.

36
Q

What is the structure of giant molecular substances?

A

3D network of covalent bonds.

37
Q

What is the main property of giant metallic structures?

A

Delocalized electrons maintain bonds.

38
Q

Why are metals good conductors of electricity?

A

Free-moving delocalized electrons.

39
Q

What happens to particles in condensation?

A

Slow down

40
Q

What are delocalized electrons?

A

Electrons not bound to a specific atom or bond.

41
Q

Why do alloys have varied properties?

A

Mixed lattice structure.

42
Q

What is an example of a simple molecular substance?

A

Carbon dioxide.

43
Q

What is an example of a simple atomic substance?

A

Argon.

44
Q

What type of structure does silicon(IV) oxide form?

A

Giant covalent structure.

45
Q

What holds particles together in metallic lattices?

A

Attraction between ions and delocalized electrons.

46
Q

Why do metals have high boiling points?

A

Strong bonds between ions and electrons.

47
Q

Why do ionic compounds conduct electricity when molten?

A

Free-moving ions.

48
Q

What happens to kinetic energy during freezing?

A

Decreases.

49
Q

How do forces of attraction change during melting?

A

Weaken as particles vibrate more.

50
Q

What is an example of an ionic lattice?

A

Magnesium oxide.

51
Q

What property of ionic crystals changes with charge density?

A

Melting/boiling point.

52
Q

What determines vapour pressure?

A

Temperature and intermolecular forces.

53
Q

Why do metals resist breaking under tension?

A

Strong ion-electron attraction.

54
Q

What is bronze made of?

A

Copper and tin.

55
Q

What type of bond is in diamond?

A

Covalent.

56
Q

What is the boiling point of magnesium oxide?

A

2852 °C.

57
Q

Why is water vapor pressure higher at higher temperatures?

A

Increased particle energy.

58
Q

What happens at equilibrium in vapor and liquid?

A

Evaporation equals condensation.

59
Q

What is the key property of van der Waals forces in graphite?

A

Weak between layers.

60
Q

What defines malleability in metals?

A

Ability to be hammered into shapes.

61
Q

How do delocalized electrons affect metallic strength?

A

Maintain bonds during deformation.

62
Q

Why does sodium chloride dissolve in water?

A

Attraction to water molecules.

63
Q

Why does boiling require more energy than evaporation?

A

All forces must break.

64
Q

What bonds are in giant ionic lattices?

A

Electrostatic.

65
Q

What bonds hold diamond’s structure together?

A

Covalent.

66
Q

Why is argon a gas at room temperature?

A

Weak intermolecular forces.

67
Q

Why is quartz hard?

A

Strong covalent bonds.

68
Q

What causes liquid particles to slide past one another?

A

Weak forces.

69
Q

What allows metal wires to form?

A

Ductility.

70
Q

Why does graphite conduct better than diamond?

A

Delocalized electrons in layers.

71
Q

What are the main states of matter?

A

Solid

72
Q

Why does freezing release heat?

A

Loss of particle energy.

73
Q

Why do ionic compounds have high melting points?

A

Strong ionic bonds.

74
Q

What is the structure of metals?

A

Layers of ions in a lattice.

75
Q

What is the difference between graphite and diamond?

A

Layered vs. 3D structure.

76
Q

Why is zinc used in brass?

A

Strengthens copper.

77
Q

What is an example of an amorphous solid?

A

Glass.

78
Q

Why are alloys corrosion-resistant?

A

Modified lattice.

79
Q

What determines a metal’s malleability?

A

Ion-electron attraction.

80
Q

How does boiling affect liquid particles?

A

Forces completely broken.

81
Q

Why do metals have luster?

A

Reflective delocalized electrons.

IMAT Chem (9 decks)

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