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Chemistry > Principles Of Chemistry > Flashcards

Principles Of Chemistry Flashcards

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1
Q

When a solid turns into a liquid

1.2

A

Melting

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2
Q

When a liquid turns into a gas

1.2

A

Evaporation

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3
Q

When a gas turns into a liquid

1.2

A

Condensation

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4
Q

When a liquid turns into a solid

1.2

A

Freezing

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5
Q

When a solid turns into a gas

1.2

A

Sublimation

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6
Q

When a gas turns into a solid

1.2

A

Deposition

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7
Q

Solid

1.1

A

Arrangement of Particles: Tightly packed together, very organized

Movement of Particles: Vibrate

Energy of Particles: Low energy

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8
Q

Liquid

1.1

A

Arrangement of Particles: Unorganized, close together but with spaces

Movement of Particles: Switch places, little movement

Energy of Particles: Medium energy

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9
Q

Gas

1.1

A

Arrangement of Particles: Spread out

Movement of Particles: Fast, random

Energy of Particles: High energy

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10
Q

What does a solubility curve show?

1.6

A

It shows how the solubility of a substance changes with temperature

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11
Q

What is the equation for solubility?

1.6

A

Solubility = mass of substance(in grams) / 100g of water*

  • a greater volume of water will dissolve more substance(control variable)
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12
Q

Define Solubility

1.5

A

The (maximum) mass of substance (in grams) that will dissolve in 100g of water

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13
Q

Define Soluble

1.4

A

A substance that will dissolve into a liquid.

Example:
Salt in water
Sugar water
Nail polish in acetone

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14
Q

Define Insoluble

1.4

A

A substance that will not dissolve into a liquid.

Example:
Sand in water
Salt in oil

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15
Q

Define Solvent

1.4

A

The liquid that does the dissolving / dissolves the solute

Example:
Water
Oil
Acetone

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16
Q

Define solute

1.4

A

The substance that is dissolved

Example:
Salt
Sugar
Nail polish

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17
Q

Define Solution

1.4

A

The mixture of dissolved solute in the solvent.

Example:
Salt water
Sugary water

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18
Q

Saturated Solution

1.4

A

A solution that contains the maximum amount of solute that is possible to dissolve.

Example:
Super salty water

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19
Q

Define concentration

1.4

A

The amount of solute particles in a particular volume of solvent

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20
Q

Define diffusion

1.3

A

The process of Particles moving from an area of high concentration to an area of low concentration.

Example:
The reaction of hydrogen chloride gas and ammonia gas

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21
Q

Reaction of hydrogen chloride gas and ammonia gas - diffusion
1.3

A

Hydrogen chloride gas evaporated from the hydrochloric acid solution and ammonia gas evaporates from the ammonia solution.
Particles of each gas move and spread out (diffuse)
A white ring forms near the hydrochloric acid. This happens because the ammonia gas particles travel faster than the hydrochloric particles.

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22
Q

Why do ammonia particles travel faster than hydrochloric particles?
1.3

A

Ammonia particles have a lower mass, therefore travel faster than hydrochloride particles.

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23
Q

Does the rate of evaporation affect where the white ring forms in diffusion?
1.3

A

Rate of evaporation does not affect where the white ring forms.

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24
Q

Why does the state of matter affect diffusion?

1.3

A

Rate of diffusion is fastest in gases because the particles have the greatest amount of energy.

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25
Q

How does the state of matter affect the rate of diffusion?

1.3

A

The diffusion rate will go faster in a gas and slower in a liquid.

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26
Q

How does the temperature affect the rate of diffusion?

1.3

A

Rate of diffusion is greatest when the temperature is highest.

27
Q

Why does changing the temperature affect the speed at which the particles spread?
1.3

A

As temperatures increases, the energy of Particles increases.
Cold temperatures have more packed together particles because it’s close to freezing temperature which is close to a solid where as warm water is not close to a solid and can move freely.

28
Q

What happens when you remove the glass plate between bromine and air in a tube?
1.3

A

The bromine and air particles will diffuse which makes an even balance of bromine and air particles throughout the tube.

29
Q

What is dilution?

1.3

A

The process of decreasing the concentration of a solution by adding water.

30
Q

When you can no longer see the colour of the food dye, are there still particles of dye?
1.3

A

Yes, the particles are so small and there are only a few left so the human eye cannot observe them.
Many particles must be present in order for the eye to an able to observe colour.

31
Q

What are atoms?

1.14

A

The basic unit of a chemical element.
It is the smallest particle of the element.
They are neutral because they have the same number of protons and electrons.

32
Q

What are molecules?

1.14

A

A pure substance containing two or more atoms chemically joined together.

33
Q

What are elements?

1.8

A

A pure substance containing only one kind of atom.

Same number of protons.

34
Q

What are compounds?

1.8

A

A pure substance made of two or more atoms of different elements chemicals joined together in a fixed ratio.

35
Q

What is a mixture?

1.8

A

An impure substance made of two or more elements or compounds in the same container that are not chemically combined

36
Q

What is Filtration?

1.10

A

An experimental technique used to separate a mixture of an insoluble solid in a liquid, such as water.

37
Q

What is crystallization?

1.10

A

An experimental technique used to separate a solution - a mixture of a soluble in water.

38
Q

What happens during crystallization?

1.10

A

Water evaporates out of the solution. As it evaporates, the solution becomes more and more concentrated, to the point that the solid will no longer stay dissolved(the solution becomes a saturated solution). Then crystals of solute appear in the basin.

39
Q

What is simple distillation?

1.10

A

An experimental technique used to separate a mixture of:

A solid in a liquid. E.g. salty water.

Two (or more) liquid with different boiling points. E.g. water and acetone.

40
Q

Describe the changes of state that occur during a distillation experiment.
1.10

A

During distillation the solute begins as a liquid, evaporates to a gas and condensates back to a liquid.

41
Q

What is the boiling point of pure water?

1.9

A

100 C

42
Q

What is paper chromatography?

1.11

A

Used to separate mixtures of colured compounds.

43
Q

What happens during paper chromatography?

1.11

A

Samples are placed on the base line (pencil line) and travel up the paper as they dissolve in the solvent.
Different substances travel different distance based on their solubility.

44
Q

What happens when a substances does not move from the base line(paper chromatography)?
1.11

A

The substance is not soluble so it stays on the base line.

45
Q

How do you calculate the Rf (retardation factor)(paper chromatography)?
1.11

A

Rf = distance travelled by substance / distance travelled by solvent
No units

46
Q

What is a pure substance?

1.9

A

A substance that only contains one type of particle.

47
Q

Define Melting Point

1.9

A

The temperature at which a solid changes on to a liquid.

Melting point: 0 C

48
Q

Define boiling point

1.9

A

The temperature at which a liquid changes into a gas.

Boiling point: 100 C plus

49
Q

Define Freezing Point

1.9

A

The temperature at which a liquid changes into a solid.

Freezing point: 0 C

50
Q

Define condensation point

1.9

A

The temperature at which a gas changes into a liquid

51
Q

What is pure ice?

1.9

A

Pure solid water that melts at exactly 0 C

52
Q

What is pure water?

1.9

A

Pure liquid water that boils at exactly 100 C

53
Q

Pure substances

1.9

A

It’s melting temperature is a fixed value at 0 C. The melting range is sharp ( a small range).
It’s boiling temperature is a fixed value at 100 C. The boiling range is sharp ( a small range).

54
Q

Mixture substances

1.9

A

The melting range is lower than pure substances. E.g. Slaty water is -5 C
The melting temperature range is broad (a large range) -8 - -3

The boiling temperature is higher than pure substances, it boils at 105 C.
The boiling temperature range is broad (a large range).

55
Q

Protons

1.15

A

Symbol: p+

Relative electrical charge: +1

Relative Mass (atomic mass units): 1

Position in the atom: Nucleus

56
Q

Neutrons

1.15

A

Symbol: n+

Relative electrical charge: 0

Relative mass (atomic mass units): 1

Position in atom: Nucleus

57
Q

Electrons

1.15

A

Symbol: e+

Relative electrical charge: -1

Relative mass (atomic mass units): 1/1938

Position in atom: Outer shells

58
Q

What is the atomic number?

1.16

A

The atomic number is the number of protons for atoms of that element.

59
Q

What is the mass number?

1.16

A

The mass number is the sum of the number of protons and the number of neutrons in an atom.

Mass number could also be called nucleon number.

60
Q

What are isotopes?

1.16

A

An atom of an element with the same number of protons but a different number of neutrons.

An atom of an element with the same atomic number but a different mass number.

61
Q

Isotopes

1.16

A

They have the same chemical properties.

They have the same number of electrons in the same electronic configuration.

The physical properties of different isotopes can vary, e.g. density.
Density = mass / volume

62
Q

What is the relative atomic mass (Ar)?

1.16

A

The weighted average of the masses of the isotopes of an element, in comparison to 1/12th of the mass of a carbon-12 atom.

63
Q

How is relative atomic mass (Ar) calculated?

1.17

A

(Mass of isotope 1 * percentage of isotope 1/ 100) + (mass of isotope 2 * percentage of isotope 2 / 100)

E.g. 75% of chlorine atoms have a mass of 35. The other 25% had a mass of 37

Ar= (35*75/100) + (37*25/100)
Ar= 26.25 + 9.25
Ar= 35.5

Chemistry (4 decks)

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