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Eddie - IGCSE Chemistry > Solids, liquids, and gases > Flashcards

Solids, liquids, and gases Flashcards

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1
Q

What are the four state symbols

A

Aqueous (aq), Liquid (l), Gas (g), solid (s)

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2
Q

Describe structure of a solid

A

Particles arranged in a fixed lattice
Particles can vibrate

Properties - 
Fixed shape
Fixed volume
Do not flow
Higher density than liquids/ gases
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3
Q

Describe structure of a liquid

A

Particles close together
Particles can move about

Properties - 
Shape can change
Fixed volume
Can flow
Higher density than gas, lower than solids
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4
Q

Describe structure of a gas

A

Particles far apart
Particles move quickly

Properties - 
Shape can change
Volume can change
Can flow
Lower density than solid/ liquid
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5
Q

Definition of melting

A

Solid changes into liquid (at the melting point)

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6
Q

Definition of boiling

A

Liquid changes into a gas (at the boiling point)

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7
Q

Definition of freezing

A

Liquid changes into solid (at the freezing point)

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8
Q

Definition of condensation

A

Gas changes into liquid (at the boiling point)

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9
Q

Definition of sublimation

A

Solid changes into gas (without going through liquid state)

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10
Q

Definition of diffusion

A

The process by which particles in liquids and gases mix together or spread out by colliding with each other.

Particles move down a concentration gradient rom a high concentration to a low concentration.

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11
Q

What factors affect rate of diffusion

A

Tempurature - faster diffusion with higher temp

Molecular mass - higher molecular mass = slower diffusion

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12
Q

What is an experiment to demonstrate diffusion

A

There is a tube which at one end had cotton wool soaked in HCl and at the other soaked in Ammonia solution. a white ring of ammonia chloride forms where the two gases meet showing one has diffused quicker than the other

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13
Q

What is Brownian motion

A

The random movement of large particles in a gas or suspended in a liquid.

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14
Q

What causes Brownian motion

A

Caused by collision of molecules in the surrounding gas or liquid with the large particles

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15
Q

What evidence is there for Brownian motion

A

Pollen grains move randomly in water when observed under microscope
Dust particles move randomly in the air

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16
Q

What is an atom made up of

A

Protons, electrons and neutrons

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17
Q

What is a proton

A

Mass - 1
Charge - +1
Location - nucleus

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18
Q

What is a neutron

A

Mass - 1
Charge - 0
Location - nucleus

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19
Q

What is an electron

A

Mass - 1/2000
charge - -1
location - Shells orbiting the nucleus

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20
Q

What is the nucleon number

A

Total number of protons and neutrons

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21
Q

What is the proton number

A

Number of protons

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22
Q

What are valency electrons

A

The electrons in the most outer shell

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23
Q

How is the stability of atoms related to their electronic structure

A

Atoms with a full outer shell are stable

this is achieved by losing or gaining electrons

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24
Q

What is an atom

A

The smallest particle of a chemical element, which cannot be broken down any further (by chemical means)

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25
Q

What is an element

A

A group of atoms which all have the same number of protons

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26
Q

What are isotopes

A

Atoms with the same number of protons but different numbers of neutrons

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27
Q

what is a compound

A

A substance in which two or more elements are chemically combined

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28
Q

What is a mixture

A

A combination of two or more substances that are not chemically combined

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29
Q

What is an ion

A

An atom where the number of electrons is different from the number of protons, so it has an overall charge

Cation - A positively charged ion
Anion - A negatively charged ion

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30
Q

What is an allotrope

A

Different forms of the same element e.g. diamond and graphite

31
Q

Radioisotopes

A

Unstable isotopes which give out radiation when they decay, They can be used for Tracers, Radiotherapy, Sterilisation

32
Q

What is ionic bonding

A

Occurs between metal and non-metal

Attraction between positive metal ions and negative non-metal ions

33
Q

How are ions formed

A

Metals lose electrons to form positive ions

Non-metals gain electrons to form negative ions

34
Q

What is covalent bonding

A

Occurs between non-metals

Covalent bonds are a shared pair of electrons

35
Q

What are two types of covalent structure

A

Simple molecular

Giant covalent lattice

36
Q

What is a molecule

A

a group of atoms being held together by covalent bonds

37
Q

What are intermolecular forces

A

weak forces between covalently bonded molecules

38
Q

Name three covalent macromolecules

A

Diamond, Graphite, Silicon (IV) Oxide

39
Q

Properties of diamond

A

Hardest known substance, Does not conduct electricity, very high melting point, cut diamonds sparkle

40
Q

Properties of Graphite

A

Soft and slippery, conducts electricity, dark in colour

41
Q

Properties of silicon (IV) dioxide

A

Hard (can scratch things), doesn’t conduct electricity, ,light passes through it, high melting point

42
Q

What is metallic bonding

A

Occurs in metallic elements, The attraction between +ve metal ions and -ve electrons

43
Q

Describe properties of metals

A 
High mp and bp
malleable and ductile
good electrical conductors
good heat conductors
insoluble in water
44
Q

What is an alloy

A

A mixture of a metal with other elements

45
Q

Why are alloys more useful than pure metals

A

harder and stronger than pure metals, some are more resistant to corrosion

46
Q

Define exothermic reaction

A

Reaction that gives out energy (temp increase)

47
Q

Define endothermic reaction

A

Reaction that take in energy from surroundings (temp decrease)

48
Q

What is bond energy

A

The energy required the break a particular bond

49
Q

Equation for calculating energy change of reaction

A

Total energy of bonds broken - total energy of bonds formed

50
Q

What four ways can energy be released

A

Burning fuels, nuclear fuels, fuel cells, electrochemical cells

51
Q

What are “Photochemical reactions”

A

reactions which obtain the energy they need from light

52
Q

What is a reversible reaction

A

A reaction that can take place in both directions

53
Q

What is meant by equilibrium

A

The forward and backward reactions that take place at the same rate. No overall change in conc.

54
Q

How is equilibrium affected by concentration, tempurature, pressure

A

equilibrium moves to the products side if reaction conc. increases, the product concentration decreases.
If temp increases it becomes a endothermic reaction. If pressure increases equilibrium position moves to the side.

55
Q

How is yield related by equilibrium position

A

The yield will be higher if the equilibrium if closer to the products side

56
Q

Define “rate of reaction”

A

amount of reactant used up per unit time

57
Q

what factors affect rate of reaction

A

increase the concentration, increase the tempurature, increase surface area, use a cataylst

58
Q

What is “collision theory”

A

Where for two particles to react successfully they must collide with sufficient energy to break the necessary bonds

59
Q

What is “empirical formula”

A

Shows the simplest ratio in which atoms combine to form a compound

60
Q

What is “molecular formula”

A

shows the actual numbers of atoms that combine to form a molecule

61
Q

What is “structural formula”

A

shows how the atoms are arranged in the molecule

62
Q

What is “relative atomic mass”

A

The average mass of naturally occurring atoms of an element relative to the mass of carbon-12

63
Q

What is “Relative formula mass”

A

the sum of the relative atomic masses

64
Q

What is a “mole”

A

the amount of a substance that contains the same number of particles as the number of carbon atoms in 12g of carbon-12

65
Q

What is “Avogadro constant”

A

The number of particles in one mole of an element or compound

66
Q

What is “molar solution”

A

A solution that contains 1-mole of solute per dm3 of solution, written as 1mol/dm3

67
Q

What is “molar volume of gas”

A

1 mole of gas occupies 24dm3 at room tempurature and pressure

68
Q

What is the equation for number of moles

A

mass/molecular mass

69
Q

What is the equation for concentration

A

molar concentration = amount of solute(g)/volume of solution

mass conc. = amount of solute(mol)/ volume of solution

70
Q

What is the equation for moles of a gas

A

volume of a gas (in dm3)/24dm3

71
Q

What is the equation for percentage yield

A

actual mass obtained/ theoretical mass

72
Q

What is the equation for percentage composition

A

total Ar of element in compound/ mr of compound x 100

73
Q

What is the equation for percentage purity

A

mass of substance in mixture/total mass of mixture x 100

74
Q

What does aqueous mean

A

Dissolved in water

Eddie - IGCSE Chemistry (5 decks)

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