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IB Chemistry > Structure 1.1 Introduction to the particulate nature of matter > Flashcards

Structure 1.1 Introduction to the particulate nature of matter Flashcards

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1
Q

What is matter?

A

Any substance that has mass and volume. Composed of atoms/ions/molecules/etc.

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2
Q

What is an element?

A

pure substance made out of atoms with the same number of protons, and cannot be chemically broken into a simpler substance

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3
Q

What is a compound?

A

Pure substance composed of two or more atoms of different elements chemically bonded in a fixed ratio

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4
Q

What is a pure substance?

A

Form of matter with consistent chemical composition, fixed properties and cannot be separated into simpler substances by physical means

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5
Q

What is a mixture?

A

More than one element or compound in no fixed ratio, which is not chemically bonded and can be separated by physical methods into pure substances (mixed but not chemically combined). Can have variable properties depending on composition

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6
Q

Heterogenous mixture

A

Mixture that does not have a uniform composition and properties throughout (e.g. rocky road)

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7
Q

Homogeneous mixture

A

mixture with a uniform composition and properties (e.g. steel, air, any aqueous solution)

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8
Q

Physical change

A

reversible change in the physical properties of a substance in which no new substances are formed

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9
Q

Solute

A

solid/liquid/gas that dissolves in a liquid solvent to form a solution of solvated ions or molecules

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10
Q

Solvent

A

A usually liquid substance that is capable of dissolving a solute

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11
Q

Solution

A

Liquid mixture in which the solute is uniformly distributed within the solvent i.e. homogenous

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12
Q

Solvated

A

(of a solute) surrounded by the solvent’s molecules

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13
Q

Hydrated

A

ions solvated with water (surrounded by water molecules)

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14
Q

Anhydrous

A

Containing no water/opposite of hydrated

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15
Q

Identify the solvent, solution and solute with sodium chloride dissolving in water

A

Solvent: water
Solute: sodium chloride
Solution: aqeuous mixture of sodium and chloride ions solvated with water

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16
Q

Soluble

A

dissolves readily in a solvent, particularly water

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17
Q

Saturated solution

A

a solution where no more solute can dissolve at a particular temperature

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18
Q

Solubility (of a substance)

A

amount of solute needed to form a saturated (maxed out) solution

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19
Q

What is the solubility of a substance expressed as?

A

Often expressed as the mass that will dissolve into 100cm3 at a particular temperature

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20
Q

Miscible

A

when liquids mix together, they form one uniform layer of homogeneous mixture

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21
Q

Immiscible

A

when liquids mix together, they do not mix and instead form two separate layers

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22
Q

What are the separation techniques?

A

Filtration
Evaporation
Recrystallisation
Distillation
Paper chromatography

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23
Q

What is filtration?

A

physical separation process that separates solid matter and fluid by the use of a filter medium that permits only the fluid to pass through

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24
Q

What does filtration work on?

A

heterogeneous, insoluble solid + liquid

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25
Q

What is the difference in physical property that allows separation in filtration?

A

Solubility

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26
Q

What is Evaporation?

A

type of vaporization that occurs on the surface of a liquid as it changes into the gas phase. This technique involves heating the solution, so that the liquid evaporates. This leaves the solid behind, separating the two substances

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27
Q

Mixture type for evaporation?

A

soluble solid and a liquid, homogenous

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28
Q

What is the difference in physical property that allows separation for evaporation?

A

Volatility

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29
Q

What is recrytillisation for?

A

Purify organic compounds

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30
Q

What type of solvent is needed for recrytillisation?

A

solvent that dissolves the desired product more readily at a high temperature than at a low temperature (making a hot solution) + allowing the product to crystallize on cooling

31
Q

What are the steps of recrytillisation?

A

Shake sample with the solvent and warm to dissolve

Filter solution hot.
Throw away residue

Allow the solution to cool slowly.
(If not crystals appear, add a single crystal as a seed/stir vigorously. If not crystals appear, you’ve added too much solvent)

Filter the solution cold.
Keep the residue

Wash the residue with a small amount of cold solvent (has to be cold to remove the soluble impurities)

Dry the product on a watch glass, either at room temperature or in an oven

32
Q

In recrytillisation, what is the result of shaking the sample with solvent + warming to dissolve?

A

Product and soluble impurities also dissolve into the solvent. Insoluble impurities don’t

33
Q

In recrytillisation, what is the result of filtering the hot solution + throwing away residue?

A

Insoluble impurities are trapped on filter paper

34
Q

In recrytillisation, what is the effect of allowing the solution to cool slowly?

A

Product becomes less soluble as it cools -> eventually become crystals.
Soluble impurities stay in solvent

35
Q

In recrytillisation, what is the effect of filtering it cool after allowing it to cool?

A

Filtration lets the soluble impurities (in solvent) pass through.
Keep the desired product. It will be contaminated with a small amount of solvent

36
Q

In recrytillisation, what is the effect of washing the reside (after cold filtration) with solvent?

A

rinses off contaminated solvent

37
Q

In recrytillisation, what is the effect of leaving the product (final step) on a watch glass to dry?

A

Leaves no residue + give final product

38
Q

What is distillation?

A

process during which a liquid is heated to boiling point in order to vaporise it. The liquid is then condensed back into a liquid, separated from impurities and other solutes.

39
Q

What type of mixture is distillation for?

A

two or more miscible (able to mix properly) liquids

40
Q

What difference in physical property is needed for distillation?

A

Boiling point (lower one leaves first)

41
Q

What is paper chromatography?

A

technique used to separate soluble solids from each other, based on how far they travel up a stationary phase

42
Q

What type of mixture is required for paper chromatography?

A

soluble solids

43
Q

What are the differences in physical property that allow paper chromatography to occur?

A

Aolubility in mobile phase

Attraction to stationary phase

44
Q

What is the mobile phase in paper chromatography?

A

Liquid/gas that the molecules can move in (i.e. solvent)

45
Q

What is the stationary phase in paper chromatography?

A

solid that the molecules cannot move in (i.e. chromatography paper)

46
Q

Why is water an exception to the density rule of solids and liquids?

A

Liquid water is denser than solid water

47
Q

What are the features of a solid?

A

definite shape
lattice configuartion
definite volume
no ability to flow
limited compressibility
highest density (usually)
Strongest force of attraction between particles
Particles are close together and vibrate in fixed positions, but don’t move around

48
Q

What are the features of a liquid?

A

Attractive forces between particles are weaker than in solids
Particles vibrate, rotate and move around
variable shape
fixed volume
ability to flow
limited compressibility
greater density than gases + less than solid (usually)

49
Q

What are the traits of a gas?

A

Attractive forces between particles are negligible
Able to move around
Always spread out
Particles vibrate, rotate and move around faster than in a liquid
shape expands to fit containers
variable volume
diffuses easily
high compressibility
lowest density

50
Q

What causes a solid -> liquid?

A

Heat causes the particles to vibrate enough to cause this

51
Q

What is the density of a substance?

A

Mass per unit volume (g cm-3)

52
Q

What is the formula for density?

A

mass / volume

53
Q

What is kinetic energy?

A

energy a particle possesses due to its motion

54
Q

What is the formula for kinetic energy?

A

(mass x velocity^2) / 2

55
Q

What is the relationship between heat, particle movement and temperature?

A

increased heat = increased particle movement = increased temperature

56
Q

What is temperature?

A

A measure of the average kinetic energy of the particles in a substance

57
Q

What occurs to particles when temperature is increased?

A

Average kinetic energy of particles increases + a greater proportion of them will have sufficient energy to overcome the forces of attraction between particles and change states

58
Q

What is melting?

A

Solid -> liquid

59
Q

What is boiling?

A

liquid -> gas

60
Q

What is evaporation?

A

particles @ liquid’s surface -> gas (below boiling point)

61
Q

What is condensing?

A

gas -> liquid

62
Q

What is freezing?

A

liquid -> solid

63
Q

What is sublimation?

A

solid -> gas without melting

64
Q

What is deposition?

A

gas -> solid without condensing

65
Q

What is boiling point?

A

temperature liquid transitions to become gas. (more specific: the temperature at which liquid and gas exist in equillibrium)

66
Q

What is melting point?

A

temperature solids transition to liquids (solids and gases exist in equillibrium at this point)

67
Q

What is absolute zero?

A

The temperature at which particles stop moving (i.e. -273.15 degrees Celsius)

68
Q

What is an endothermic process?

A

Energy is absorbed by particles from surroundings (i.e. solid -> liquid OR liquid -> gas / more condensed -> less condensed)

69
Q

Why does temperature not increased during a transitional phase between states of matter, despite heat being added?

A

supplied heat is exclusively utilised to overcome the attractive forces between the water molecules in the liquid phase

70
Q

What is the Celsius scale based on?

A

100 degree range between the melting and boiling point of pure water under standard conditions

71
Q

What is Kelvin?

A

the standard SI unit for temperature with the same increment size as Celsius

72
Q

What is the formula for temperature in K?

A

temperature (C) + 273.15

73
Q

What is the change in temperature (K) equal to?

A

Change in temperature (C)

IB Chemistry (10 decks)

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