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1
Q

Define a compound

A

A pure substance that can be simplified. They are made up of two or more DIFFERENT elements chemically combined in a fixed ratio

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2
Q

Define a molecule

A

A molecule is 2 atoms (can be the same or different) that are chemically bonded together

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3
Q

Define a mixture

A

A mixture is impure and consists substances that are not chemically joined and not in a fixed ratio

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4
Q

Name the 7 properties of metals

A
  • lustrous fresh surface
  • good conductors of electricity
  • good conductors of heat
  • malleable
  • ductile
  • solid and room temp
  • relatively dense
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5
Q

Proton - state where it is found, charge and size

A 
In nucleus (therefore a nucleon)
Positive charge
Relatively large (1amu)
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6
Q

Neutron- state where it is found, charge and size

A 
In nucleus (therefore a nucleon) 
Neutral charge
Relatively large (1amu)
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7
Q

Electron- state where it is found, charge and size

A 
In orbit in shells outsider of atom 
Negative charge
Relatively small (0amu)
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8
Q

Define a physical change

A

Physical changes are changes affecting the form of a chemical substance, but not its chemical composition. A change in state, no new substance is made

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9
Q

Define a chemical change

A

A chemical change occurs when a substance combines with another to form a new substance. They are difficult to reverse. Reactant =products

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10
Q

Characteristics of a physical change

A

Change in colour, temperature, state, shape and volume

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11
Q

Characteristics of a chemical change

A

Change in colour, temperature, odor/smell, production of light, bubbles, precipitate

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12
Q

Solid to a liquid

A

Fusion

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13
Q

Solid to a gas

A

Sublimation

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14
Q

Gas to solid

A

Deposition

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15
Q

Gas to liquid

A

Condensation

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16
Q

Liquid to solid

A

Solidification

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17
Q

Liquid to gas

A

Vapourisation

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18
Q

Define an ion

A

An ion is an atom that has gained or lost on or more electrons.

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19
Q

Name given to a positive ion

A

Cation

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20
Q

Name given to a negatively charged ion

A

A ion

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21
Q

The periodic table is a list of elements in order of increasing ________

A

Atomic numbers

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22
Q

The symbol for atomic number

A

Z

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23
Q

Symbol for number of neutrons

A

N

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24
Q

What does the atomic number show?

A

How many protons and electrons in an atom

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25
Q

Symbol for atomic mass number

A

A

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26
Q

What is the atomic mass number?

A

The number of protons and neutrons (number of nucleons)

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27
Q

What is an isotope?

A

Isotopes are atoms of the same element (same proton number) but with different atomic masses (different neutron number)

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28
Q

What is the density formula?

A

D= M divided by V

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29
Q

Define the electronic structure

A

1st shell = 2
2nd shell = 8
For the first 20 elements, the 3rd shell appears to be full with 8 electrons

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30
Q

Name the properties of group 1 elements

A

All very reactive metals
Known as the alkali metals
They react violently with water e.g sodium

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31
Q

Name the property of group 2 elements

A

All are reactive metals

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32
Q

Name the properties of group 7 elements

A

All very reactive
Non-metals
All are found in diatomic molecules

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33
Q

Name the properties of group 8 elements

A

Are very non reactive
Are caller the noble gases
Have a full Valence shell

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34
Q

Define an ionic bond

A

Ionic bonds form following a transfer of electronics between atoms resulting in the formation of ions.
They bond with atoms on the opposite side of the periodic table

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35
Q

Define a covalent bond

A

Covalent bonds form when electrons are shared between atoms. When the atoms both need to gain electrons to complete their valency shells.

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36
Q

Groups in a periodic table refer to

A

The number of electrons in the valency shell.

E.g. Group 5 have 5 electrons in the outer shell

37
Q

List the properties of acids

A 
Have a sour taste
Change litmus from blue to red
Conduct an electric current
Corrode most metals 
React with carbonates
Neutralise bases
38
Q

Name 3 strong acids

A

Hydrochloride acid, sulfuric acid and nitric acid

39
Q

Name 3 weak acids

A

Acetit acid, carbonic acid, Citric acid

40
Q

List the properties of bases

A

A bitter taste
Change colour of red litmus to blue
Conduct an electric current
Have a slippery feel

41
Q

Name some common alkalis (bases)

A

Sodium hydroxide NaOH
Potassium hydroxide KOH
calcium hydroxide Ca(OH)2

42
Q

An alkali is any substance that produces ______ in water

A

OH- ions

43
Q

an alkali has a ph of

A

More than 7

44
Q

A base will ______ an acid

A

Neutralise

45
Q

Alkalis are ______ and _______ substances

A

Alkalis are HARMFUL and CORROSIVE substances

46
Q

List the properties of an ionic compound

A 
Made up of both + and - ions
Solid at room temp
Have high melting points 
Dissolve in water to form aqueous solutions
Conduct electricity
47
Q

Ionic compounds usually form ______ of positive and negative ions rather than individual molecules

A

Lattices

48
Q

What is a lattice?

A

A lattice is an ordered structure of ions held together by the electrostatic attraction between + and - ions

49
Q

What is a bonding electron

A

The name given to the shared electron in the covalent compound

50
Q

Characteristics of covalent compounds are

A

Low melting points, as the attraction between molecules is weak
Generally do not conduct electricity bc the aren’t made up of ions
insoluble in water

51
Q

What is a chemical formula

A

A chemical formula is a set of symbols showing the elements present in the compound and shows their ratio

52
Q

How is a valency of an element determined?

A

The Valencia determined by the number of electrons and element wants to gain or lose

53
Q

Covalent bonds form between elements that are —— on the periodic table

A

Close together on the right hand side of the periodic table

54
Q

Mono means

A

1

55
Q

Di means

A

2

56
Q

Tri means

A

3

57
Q

Tetra means

A

4

58
Q

Pent means

A

5

59
Q

Define an element

A

A pure substance that cannot be simplified. Are made up of one type of atom only.

60
Q

Name the 2 liquids in the periodic table

A

Mercury and bromine

61
Q

Name the 6 semi metals in the periodic table

A

Silicon, germanium, arsenic, antimony, selenium and tellurium

62
Q

Name the 11 gases in the periodic table

A

Hydrogen, helium, nitrogen, oxygen, fluorine, neon, chlorine, argon, krypton, xenon, radon

63
Q

Describe the dalton model

A

Thought atoms were hard indivisible spheres

64
Q

Describe the Thomson model

A

Though that the whole atom was + charged, with - electrons embedded in it like a plum pudding

65
Q

Describe the Rutherford model

A

He was the first to discover the nucleus, and that electrons orbited around. Only flaw was that the electrons would lose energy and special inwards

66
Q

Describe bohrs model

A

Had the same as rutherfords, only that electrons could only exist in specific shells with a certain amount of energy. Also explained why they didn’t special inwards

67
Q

Describe chadwicks model

A

Chadwick is the model we use today

He found that the nucleus contained neutrons

68
Q

Describe aristotles model

A

Thought that everything was made up of earth, fire, water and air composed of different ratios

69
Q

What is a binary compound

A

A compound of 2 elements. The 1st one being the metal involved, the 2nd is the name of the non metal - ending in ide

70
Q

What is an ionic compound

A

A compound where ions are held together in a structure by electrostatic forces

71
Q

What is a covalent compound

A

Covalent compounds form between 2 or more NON METALS. The atoms share electrons to gain a full outer shell

72
Q

Metal + oxygen =

A

Metal oxide

73
Q

Metal + acid =

A

Salt + hydrogen

74
Q

Metal oxide + acid =

A

Salt + water

75
Q

Alkali + acid =

A

Salt + water

76
Q

Metal carbonate + acid =

A

Salt + carbon dioxide + water

77
Q

Very active metal + water =

A

Metal hydroxide + hydrogen

78
Q

Define an acid

A

An acid is a compound containing hydrogen that gives free hydrogen ions in solution

79
Q

Define a base

A

A base is a compound that neutralises an acid

80
Q

Define an alkali

A

An alkali is a soluble base. They give free hydrogen ions in solutions

81
Q

Define a salt

A

A salt is the IONIC compound formed when the hydrogen of an acid is replaced by a metal ion

82
Q

Chemical reactions that absorb energy are called

A

Endothermic - temp gets colder

83
Q

Chemical reactions that produce energy are called

A

Exothermic - get warmer

84
Q

Define the term valency

A

The number of un paired electrons in an atoms outermost shell

85
Q

What is a polyatomic ion?

A

An ion containing more than one atom

86
Q

Define pH

A

Ph means potential hydrogen. It is a measure of the acidity or alkalinity of a solution

87
Q

Define diatomic molecule and explain why they form

A

A diatomic molecule forms via a covalent bond, as both want to gain more stability (full valence shell)

88
Q

What is a homonuclear diatomic molecule

A

A homonuclear diatomic molecule is the covalent bond of two SAME elements. Each atom in the molecule has an equal electro negativity

89
Q

What is a heteronuclear atomic molecule

A

A heteronuclear diatomic atom consists of 2 DIFFERENT atoms- thus different in electro negativity. They have polar covalent bonds

Science - Chemistry (2 decks)

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