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Chemistry > The Composition Of Matter > Flashcards

The Composition Of Matter Flashcards

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1
Q

Atomic theory

A

States that all matter is composed of atoms which can’t be created on destroyed

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2
Q

4 characteristics of matter

A

Has a mass, particles are in constant motion, occupies a volume in space & is made up of particles, atoms, molecules or ions

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3
Q

3 States of matter

A

Solid liquid & gas

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4
Q

Properties of solid

A

Fixed volume, fixed shape, cannot be compressed, attractive forces between particles hold them in a close packed arrangement & particles aerate is fixed positions

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5
Q

Properties of liquids

A

Fixed volume, no fixed shape, cannot be compressed, forces between particles ae weaker than in solids, partially vibrate, rotate & translate

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6
Q

Properties of gas

A

No fixed volume, no fixed shape, can be compressed, forces between particles are taken as zero & parties vibrate, rotate I translate faster then in a liquid

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7
Q

What does the way particles of matter move depend on and how dos it change the movement?

A

Temperature, temp increase causes average kinetic energy to increase causing more vibration/rotation/movement

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8
Q

Si units for temp & absolute zero

A

Fahrenheit, Celsius, Kelvin. Zero Kelvin, -273 Celsius, all movement of particles stop

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9
Q

Changes of state, draw the heating curve for water

A

Page 3

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10
Q

What happens to the particles during changes of state? Ice to water & water to gas

A

Ice to water: solid lattice vibrates more until it reaches melting point & starts to melt.No change in temp while melting occurs. Level of disorder increases.
Water to gas: molecules vibrate more & faster until boiling point is reached & it boils until it all is vaporized. No change in temp. Level of disorder increases

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11
Q

What kind of processes are melting & boiling?

A

Endothermic, energy must be transferred from surrounding & potential energy increases

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12
Q

Cooling brings which processes?

A

Condensation & freezing

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13
Q

What kind of processes are condensation & freezing?

A

Exothermic, energy is transferred to surroundings. Potential energy of molecules decrease

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14
Q

What is evaporation?

A

Vaporization happening below boiling point.

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15
Q

What is sublimation? And what is it’s reverse?

A

State change from solid to gas without becoming a liquid, reverse is deposition

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16
Q

Definition of an element

A

Contains only atoms of one type

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17
Q

Definition of a compound

A

Atoms of elements confined in a fixed ratio, composed of ions or molecules

18
Q

What is a pure substance?

A

Matter that has constant composition, chem & physical properties are distinct & consistent (nitrogen n2, argon ar, water h20)

19
Q

What is a mixture?

A

A combination of pure substances, elements or compounds are not chemically bound together.

20
Q

What is a homogeneous mixture?

A

Has uniform composition & properties

21
Q

What is a heterogeneous mixture?

A

Have non-uniform composition & thus properties vary

22
Q

Ion, anions & cations

A

Charged species, negative, positive

23
Q

What is combination or synthesis reaction?

A

Involves combination of 2 or more substances to produce single product

24
Q

What is a decomposition reaction?

A

Single reactant being broken down into 2 or more products

25
Q

What is a single replacement reaction?

A

Occur when one element replaces another in a compound

26
Q

What is a double replacement/metathesis reaction?

A

Occur between ions in a solution, forms insoluble substances & weak or non-electrolytes

27
Q

What is the physical property viscosity?

A

How resistant a substance is to flow

28
Q

Definition of boiling point

A

The temperature at which a liquid becomes a gas

29
Q

How does pressure affect boiling point?

A

Increase in pressure, increase boiling point

30
Q

Definition of melting point

A

Temperature where a solid becomes a liquid

31
Q

How does pressure affect melting point?

A

Increase pressure, increase melting point
Exception: ice

32
Q

Definition of freezing point

A

The temperature at which a liquid becomes solid

33
Q

How does pressure affect freezing point?

A

Increase pressure, increase freezing point
Exception: ice

34
Q

Is a phase change a physical or chemical process?

A

Physical

35
Q

What determines phase change?

A

Temperature & pressure, what type of chemical

36
Q

What is it the phase change from a gas to plasma called?

A

Ionization

37
Q

What is it the phase change from plasma to gas called?

A

Recombination

38
Q

What is an ideal gas

A

No particle volume & no intermolecular forces

39
Q

What is the volume of one mol of an ideal gas at StP?

A

22.4 L

40
Q

3 parts of the kinetic theory of gases which ideal gases follow

A

More rending & have no volume
Don’t attract or repel eachother (no intermolecular forces)
No kinetic energy is lost when the molecules collide with enchother

41
Q

What are real gases?

A

Gases that don’t follow the kinetic theory of gases

42
Q

What is Boyle’s law?

A

The pressure of a gas increases as its volume decreases, assuming constant mass & temperature

Chemistry (10 decks)

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