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State of Matter Flashcards

1
Q

Substances are made up of tiny particles called

A

Atoms

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2
Q

Particles move in ______ motion

A

random motion

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3
Q

Particles mix by colliding each other and bouncing off all directions is called

A

Diffusion

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4
Q

Solid have ______ shape and _______ volume

A

fixed,fixed

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5
Q

Liquids shape and volume

A

Fixed volume
Takes the shape of the container

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6
Q

Gases shape and volume

A

No fixed shape
No fixed volume
Takes the shape and volume of its container

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7
Q

Compressibility of solid,liquid and gases

A

Solid-slightly compressible
Liquid-slightly compressible
Gases-highly compressible

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8
Q

Phase change

A

Solid——>Liquid-Melting
Liquid———>Gases-Evaporation
Solid———>Gases-Sublimation

All of the above 3 are endothermic reaction,and heat is absorbed

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9
Q

Phase Change

A

Liquid——>Solid-Freezing
Gases——->Liquid-Condensation
Gases ———>Solid-Deposition

All of the above are exothermic reaction and heat is released during reaction

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10
Q

How much heat is required for phase change?

A

The stronger the forces between molecules,more heat energy is required to break them

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11
Q

Gas pressure depends on

A

1.Temperature
2.Volume

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12
Q

Gas pressure and Temperature relation

A

As the temperature increases,the pressure of the gases also increases

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13
Q

Gas pressure and volume relation

A

As the volume of the container decreases,the gas pressure increases

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14
Q

Rate of diffusion of gas depends on

A

1.Mass of the particle or relative molecular mass
2.Temperature

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15
Q

Diffusion of gas and relative molecular mass

A

The lower its relative molecular mass,the faster a gas will diffuse

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16
Q

Temperature and rate of diffusion of gases

A

The higher the temperature,the faster a gas will diffuse

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17
Q

Mass of a molecule is called

A

Relative molecular mass

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18
Q

What are the three states of matter?

A

Solid- rigid, definite shape

Liquid- flows and takes up the shape of the container, definite volume

Gas- takes up the volume and shape of the container

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19
Q

What is fourth type of matter ?

A

Plasma- found naturally in interiors of the stars, gaseous materials which have electrically charged particles, which classify themselves from gaseous matter.

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20
Q

Why can some sample of matter appear to have mixed properties of solid, liquid, and or gases at the same time?

A

Bcuz they are composed of many small pieces. Eg clouds seem to be gases but actually they are composed of gases and tiny particles of water (liquid or solid)

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21
Q

What are homogenous and heterogenous mixture?

A

Homogenous mixture- uniform composition and visually the same throughout

Heterogenous- not uniform composition, composition that varied from point to point.

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22
Q

What are pure substances and mixture?

A

Pure substances- element and compounds

Mixture- composition of two or more different matter and can be separated by physical changes

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23
Q

What type of element constitutes nearly one half of the earth?

A

Oxygen.

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24
Q

What types of matter are called fluids?

A

Liquids and gases bcuz they can flow from place to place

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25
Is the density of solid always greater than liquid?
No. Example- solid water is less dense than liquid water
26
What is sublimation and is it exothermic or endothermic?
Solid———>gas It is endothermic
27
What is condensation? Exo or endo
Gas to liquid. It is exothermic.
28
How do we change gas to plasma and what is the process called?
By heating or putting a lot of energy. The atoms that make up the gas start to lose their electrons and become positively charged ions. The lost electrons are then able to float freely. This process is called ionization.
29
How are plasma changed back to gases?
By a process known as recombination process by which positive ions of a plasma capture a free (energetic) electron and combine with electrons or negative ions to form new neutral atoms (gas).
30
What are extensive and intensive properties?
Extensive property- property that depends on the amount of matter Intensive- property that does not depend on amount of matter
31
What are extensive and intensive properties?
Extensive property- property that depends on the amount of matter Intensive- property that does not depend on amount of matter
32
Is concentration extensive or intensive?
Intensive
33
extensive or intensive? 1. Length 2. Mass 3. Solubility 4. Temp 5. Heat 6. Conc 7. BPT/MTP
1. E 2. E 3. I 4. I 5. E 6. I 7. I
34
Homogenous or heterogenous? Blood Vinegar Gasoline Bronze Metals
Heterogenous Homo Homo Homo Homo
35
What are the four states of matter?
Solid, Liquid, Gas, Plasma
36
What is a pure substance?
Matter with the same composition and same properties.
37
What are the types of pure substances?
Elements and Compounds.
38
What is an element?
A substance that cannot be broken down into simpler substances (e.g., Chlorine, Sodium, Carbon).
39
What is a compound?
A substance that can be broken down into elements or other compounds by chemical reaction (e.g., Sodium chloride, Glucose).
40
What is a mixture?
Matter containing two or more substances that can be separated by physical means (e.g., evaporation, distillation).
41
What is a heterogeneous mixture?
A mixture with a composition that varies from point to point (e.g., salad, sand & sugar).
42
What is a homogeneous mixture?
A mixture with uniform composition, also known as a solution (e.g., air, vinegar).
43
What is a physical property?
A characteristic of matter that can change in state but not in chemical composition.
44
What is a chemical property?
Change from one type of matter to another
45
What is the law of conservation of mass?
Mass remains constant during a physical or chemical change.
46
What is an intensive property?
A property that does not depend on the amount of matter (e.g., density, boiling point).
47
What is an extensive property?
A property that depends on the amount of matter (e.g., mass, volume).
48
What are the properties of plasma?
1. Gas with electrical particles, 2. Conducts electricity, 3. Formed at high temperatures, 4. Gases cannot conduct electricity but plasma can.
49
What is melting?
Change from solid to liquid (endothermic reaction, absorbs energy).
50
What is freezing?
Change from liquid to solid (exothermic reaction, releases energy).
51
What is vaporization?
Change from liquid to gas (endothermic reaction, absorbs energy).
52
What is condensation?
Change from gas to liquid (exothermic reaction, releases energy).
53
What is sublimation?
Change from solid to gas (endothermic reaction, absorbs energy).
54
What is deposition?
Change from gas to solid (exothermic reaction, releases energy).
55
What is ionization?
Change from gas to plasma (endothermic reaction, absorbs energy).
56
What is recombination?
Change from plasma to gas (exothermic reaction, releases energy).
57
What are the properties of solids?
Fixed shape and volume, high density, incompressible, strong intermolecular forces.
58
What are the properties of liquids?
Fixed volume, no fixed shape, mid to high density, slightly compressible.
59
What are the properties of gases?
No fixed shape or volume, low density, highly compressible, particles move freely.
60
How are carbon atoms arranged in graphite?
Planar layers, each carbon is bonded to three others in hexagonal rings.
61
Why can graphite conduct electricity?
It has delocalized electrons that move freely between layers.
62
Why is graphite soft?
Weak van der Waals forces allow layers to slide over each other.
63
How are carbon atoms arranged in diamond?
Each carbon is bonded to four others in a tetrahedral structure.
64
Why is diamond hard?
Strong covalent bonds in a 3D network make it extremely strong.
65
Why doesn’t diamond conduct electricity?
All electrons are involved in bonding, so no free electrons.
66
What is graphene?
A single layer of graphite, with strong bonds and excellent electrical conductivity.
67
What are fullerenes?
Hollow carbon molecules (buckyballs or nanotubes) used in nanotechnology.
68
What is the kinetic theory of gases?
Gas molecules are in constant motion, with no forces of attraction or repulsion.
69
What are ideal gases?
Gases that fit the kinetic theory perfectly.
70
When do real gases differ from ideal gases?
At high pressure and low temperature, due to intermolecular forces.
71
What is an ionic lattice?
A 3D arrangement of alternating positive and negative ions.
72
What are the properties of ionic lattices?
Hard, brittle, high melting & boiling points, soluble in water, conduct electricity when molten or in solution.
73
What is a metallic lattice?
Metal ions surrounded by delocalized electrons in a 3D arrangement.
74
Why are metals malleable and ductile?
Because metal layers slide easily while maintaining metallic bonds.
75
What are the four allotropes of carbon?
Graphite, Diamond, Graphene, and Fullerenes.
76
Why is graphene the best electrical conductor?
It has free-moving delocalized electrons in a single layer of carbon atoms.
77
Why do solids have a fixed shape?
Because their particles are tightly packed in a regular structure with strong intermolecular forces.
78
Why do gases expand to fill their container?
Because gas particles move freely and have weak intermolecular forces.
79
Why are liquids able to flow?
Because their particles are close together but can move past each other.
80
Describe the structure of graphite.
Graphite consists of layers of hexagonally arranged carbon atoms, with weak van der Waals forces between layers allowing them to slide.
81
Describe the structure of diamond.
Each carbon atom in diamond is bonded to four other carbon atoms in a tetrahedral structure, creating a strong, rigid 3D lattice.
82
Why are metals malleable and ductile?
Because metal layers can slide over each other while maintaining metallic bonds.
83
What are the four main allotropes of carbon?
Graphite, Diamond, Graphene, and Fullerenes.
84
Why is graphene the best electrical conductor?
It has freely moving delocalized electrons in a one-atom-thick layer, offering minimal resistance.

Chemistry (13 decks)

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