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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
What are allotropes?
Different molecular forms of the same element.
26
What are the properties of graphite?
High melting points
27
Why is graphite soft?
Weak van der Waals forces between layers.
28
Why does graphite conduct electricity?
Delocalized electrons move along layers.
29
What are the properties of diamond?
Hard
30
Why is diamond hard?
Strong 3D covalent bonds.
31
What is silicon(IV) oxide similar to?
Diamond.
32
What happens to particles during evaporation?
High-energy particles escape
33
How does boiling differ from evaporation?
Boiling occurs at a specific temperature
34
Why do ionic lattices have high melting points?
Strong electrostatic attraction between ions.
35
What type of lattice does NaCl form?
Giant ionic lattice.
36
What is the structure of giant molecular substances?
3D network of covalent bonds.
37
What is the main property of giant metallic structures?
Delocalized electrons maintain bonds.
38
Why are metals good conductors of electricity?
Free-moving delocalized electrons.
39
What happens to particles in condensation?
Slow down
40
What are delocalized electrons?
Electrons not bound to a specific atom or bond.
41
Why do alloys have varied properties?
Mixed lattice structure.
42
What is an example of a simple molecular substance?
Carbon dioxide.
43
What is an example of a simple atomic substance?
Argon.
44
What type of structure does silicon(IV) oxide form?
Giant covalent structure.
45
What holds particles together in metallic lattices?
Attraction between ions and delocalized electrons.
46
Why do metals have high boiling points?
Strong bonds between ions and electrons.
47
Why do ionic compounds conduct electricity when molten?
Free-moving ions.
48
What happens to kinetic energy during freezing?
Decreases.
49
How do forces of attraction change during melting?
Weaken as particles vibrate more.
50
What is an example of an ionic lattice?
Magnesium oxide.
51
What property of ionic crystals changes with charge density?
Melting/boiling point.
52
What determines vapour pressure?
Temperature and intermolecular forces.
53
Why do metals resist breaking under tension?
Strong ion-electron attraction.
54
What is bronze made of?
Copper and tin.
55
What type of bond is in diamond?
Covalent.
56
What is the boiling point of magnesium oxide?
2852 °C.
57
Why is water vapor pressure higher at higher temperatures?
Increased particle energy.
58
What happens at equilibrium in vapor and liquid?
Evaporation equals condensation.
59
What is the key property of van der Waals forces in graphite?
Weak between layers.
60
What defines malleability in metals?
Ability to be hammered into shapes.
61
How do delocalized electrons affect metallic strength?
Maintain bonds during deformation.
62
Why does sodium chloride dissolve in water?
Attraction to water molecules.
63
Why does boiling require more energy than evaporation?
All forces must break.
64
What bonds are in giant ionic lattices?
Electrostatic.
65
What bonds hold diamond's structure together?
Covalent.
66
Why is argon a gas at room temperature?
Weak intermolecular forces.
67
Why is quartz hard?
Strong covalent bonds.
68
What causes liquid particles to slide past one another?
Weak forces.
69
What allows metal wires to form?
Ductility.
70
Why does graphite conduct better than diamond?
Delocalized electrons in layers.
71
What are the main states of matter?
Solid
72
Why does freezing release heat?
Loss of particle energy.
73
Why do ionic compounds have high melting points?
Strong ionic bonds.
74
What is the structure of metals?
Layers of ions in a lattice.
75
What is the difference between graphite and diamond?
Layered vs. 3D structure.
76
Why is zinc used in brass?
Strengthens copper.
77
What is an example of an amorphous solid?
Glass.
78
Why are alloys corrosion-resistant?
Modified lattice.
79
What determines a metal's malleability?
Ion-electron attraction.
80
How does boiling affect liquid particles?
Forces completely broken.
81
Why do metals have luster?
Reflective delocalized electrons.

IMAT Chem (9 decks)

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