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Chemistry > End Of Year S3 > Flashcards

End Of Year S3 Flashcards

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1
Q

How are elements in the periodic table arranged?

A

In order of increasing atomic number

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2
Q

What can the periodic table be used to determine

A

Whether an element is a metal or non metal

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3
Q

What does a nucleus contain

A

Contains protons neutrons and electrons that orbit the nucleus

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4
Q

Protons charge ?

A

1positive

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5
Q

Charge if neutrons?

A

Neutral

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6
Q

Electron charge?

A

1 negative

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7
Q

What has the approximate mass of 1 atomic mass unit

A

Protons and neutrons

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8
Q

How do u know the number of protons given from an atom

A

Is given by the atomic number

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9
Q

In a neutral atom the number of electrons is eaqual to the…?

A

Number of protons

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10
Q

The mass number of an atom is equal to….?

A

The number of protons added to the number of neutrons

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11
Q

What are isotopes defined as

A

Atoms with the same atomic number but differnt mass numbers

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12
Q

What is nuclide notation used to show?

A

Atomic number
Mass number
Charge of atoms from which the number of protons electrons and neutrons can be determined

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13
Q

How many isotopes do elements normally have

A

1 or 2

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14
Q

How was the average atomic mass calculated for each element ?
And what are the values known as

A

By using the mass and proportion of each isotope present

These are known as relative atomic masses

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15
Q

What forms between non metal atoms

A

Covalent bonds

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16
Q

When do covalent bonds form ?

A

When 2 positive nuclei are held together b their common attraction for a shared pair of elements

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17
Q

What are the 7 diatomic elements

A

Hydrogen
Nitrogen
Oxygen
Fluorine
Chlorine
Bromine
Iodine

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18
Q

What does the shape of covalent molecules depend on

A

Number of bonds and the orientation of these bonds around the central atom

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19
Q

What are the 4 shapes of covalent molecules

A

Linear
Angular
Trigonal pyramidal
Tetrahedral

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20
Q

What does more than 1 forming between atoms lead to

A

Double or triple covalent bonds

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21
Q

What can covalent substances form?

A

Discrete molecular or giant network structures

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22
Q

Covalent molecular substances have strong….?

A

Covalent bonds within the molecules and only weak attractions between the molecules

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23
Q

Covalent molecular substances have low….?

A

Melting and boiling points as only weak forces of attraction between the molecules are broken when a substance changes state

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24
Q

Covalent molecular substances have a network of……?

A

Strong covalent bonds within one giant structure

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25
Q

Covalent molecular substances do not conduct…?

A

Electricity because they do not have charged particles which are free to move

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26
Q

Covalent molecular substances which are…?

A

Insoluble in water may dissolve in other solvents

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27
Q

Covalent network structures have a network of…?

A

Strong covalent bonds within a giant structure

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28
Q

Covalent network structures have very high…?

A

Melting and boiling points because the network of strong covalent bonds is not easily broken

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29
Q

Covalent network structures do not….?

A

Dissolve in general

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30
Q

Covalent network substances do not…?

A

Conduct electricity this is because they do not have charged particles which are free to move

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31
Q

When are ions formed

A

Ions are formed when when atoms lose or gain electrons to the stable electron arrangement of a noble gas

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32
Q

In general metal atoms lose……?

A

electrons forming positive ions and non metal atoms to gain electrons forming negative ions

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33
Q

What are ionic bonds .?

A

Are the electrostatic attraction between positive and negative ions

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34
Q

Ionic compounds form…?

A

Lattice structures of oppositely charged ions with each a positive ion surrounded by negative ions and each negative ion surrounded with each positive ions

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35
Q

Ionic compounds have high…?

A

Melting and boiling points because strong ionic bonds must be broken in order to break up the lattice

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36
Q

Many ionic compounds are..?

A

Soluble in water

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37
Q

What happens as ionic compounds dissolve ?

A

The lattice structure breaks up allowing water molecules to surround the separated ions

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38
Q

Ionic compounds can … only when molten or in solution

A

Conducts electricity

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39
Q

How can conduction be explained in ionic compounds ?

A

By the movements of ions towards oppositely charged electrodes

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40
Q

What are compound names derived from

A

From the names of the elements from which they are formed

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41
Q

What does a compound ending ide mean

A

It contains 2 elements

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42
Q

What does compound ending in ite or ate mean

A

It has oxygen in it

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43
Q

What are group ions ?

A

Ions containing more than one type of atom

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44
Q

What is the mass of a mole in grams equal to

A

To the gram of formula mass can be calculated using relative atomic masses

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45
Q

What is formed when a solute is dissolved in a solvent

A

A solution

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46
Q

What is the ph scale an indication of?

A

Hydrogen ion concentration and runs from 0-14

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47
Q

What does a neutral solution have equal of

A

H+ and OH- ions

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48
Q

What ph is water

A

Neutral
As it dissociates producing equal concentrations of hydrogen and hydroxide ions at any time

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49
Q

The symbol of 2 arrows represents what

A

That the reaction is reversible and occurs in both directions

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50
Q

Acidic solutions have a higher….?

A

Concentration H+ions than OH-and have ph below 7

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51
Q

Alkaline solutions have higher…?

A

Concentration of OH- ions than H+ ions and have a ph above 7

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52
Q

Dilution of an acidic solution with water will…?

A

Decrease the concentration oh H+ and the ph will increase towards 7

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53
Q

Dilution of an alkaline solution with water will …?

A

Decrease the concentration of OH- and the ph will decrease towards to 7

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54
Q

Soluble non metal Oxides will….?

A

Dissolve in water to forming acidic solutions

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55
Q

Soluble metal oxides…?

A

Dissolve in water to form alkaline solution

56
Q

What neutralises acids
Name some ?

A

Bases
Metal oxides ,metal hydroxides, metal carbonates

57
Q

What is a neutralisation reaction ?

A

Which a base reacts with an acid to form water

58
Q

What does the name of a salt produced depend on

A

On the acid and base used

59
Q

What does hydrochloric acid produce

A

Chlorides

60
Q

What does sulphuric acid produce

A

Sulphates

61
Q

What does nitric acid produce

A

Nitrates

62
Q

What are spectator ions

A

Ions that remain unchanged by the reaction

63
Q

What can an indicator do at the end of an experiment

A

Be added to show the result

64
Q

What does titration do

A

Produce a soluble salt

65
Q

What is used to produce soluble salts

A

Insoluble metal carbonates and insoluble metal oxides

66
Q

What are reactants

A

The chemicals you start a reaction with

67
Q

How can you speed up a chemical reaction?

A

Heating them up
Increasing the surface area
Add a catalyst
Increasing concentration

68
Q

Formula for average rate

A

/\quantity
—————
/\ time

69
Q

What is an element ?

A

A substance made up of the same type of atom

70
Q

What is an isotope

A

Atoms of the same element which have differnt mass snumbers but same atomic number

71
Q

How do elements in groups 1-7 become stable like elements in group 8

A

By sharing electrons
Transferring electrons

72
Q

Where does ionic Bonding occur

A

Between non metals and metal

73
Q

Some examples of ionic compounds ?

A

Sodium chloride
Copper sulphate
Sodium hydroxide

74
Q

What state are ionic compounds at room temperature

A

Solid

75
Q

Mono means ?

A

1

76
Q

Di means

A

2

77
Q

Tri means

A

3

78
Q

Tetra means?

A

4

79
Q

Penta means?

A

5

80
Q

Hexa means

A

6

81
Q

Hepta means?

A

7

82
Q

SVISS how to produce an ionic formula ?

A

(S)ymbols down
(V)alency under symbol
(I)nclude charge
(S)wap valency
(S)implify valency if possible

83
Q

Name some common acids

A

Hydrochloric acid
Sulfuric acid
Nitric acid

84
Q

Formula for hydrochloric acid ?

A

HCL
(H+Cl-)

85
Q

Formula for sulfuric acid

A

H2SO4
((H+)2SO2-4)

86
Q

Formula for nitric acid

A

HNO3
(H+NO3-)

87
Q

Name some common bases

A

Sodium hydroxide
Potassium hydroxide
Sodium carbonate

88
Q

Formula for sodium hydroxide

A

NaOH
(Na+OH-)

89
Q

Formula for potassium hydroxide

A

KOH
(K+OH-)

90
Q

Formula for sodium carbonate

A

Na2Co3
((Na+)2Co2-3

91
Q

Word equation for how to make a base

A

Metal oxide +water ->metal hydroxide

92
Q

Word equation for how to make an acid

A

Non metal oxide + water -> acid

93
Q

What is metallic bonding

A

Electrostatic attraction between 2 positively charged ions and delocalised electrons

94
Q

Why are metallic elements conductors

A

They contain delocalised electrons

95
Q

What can metals be used to produce

A

Soluble salts

96
Q

What is reduction in metals

A

A gain of electrons in a reactant in any reaction

97
Q

what is oxidation in metals

A

A loss of electrons by a reactant in any reaction

98
Q

What happens in a redox reaction

A

Reduction and oxidation takes place at the same time

99
Q

What happens during the extraction of metals

A

Metal ions are reduced forming metal atoms

100
Q

What are the methods to remove a metal from an ore

A

Heat alone
Electrolysis
heat + C/CO

101
Q

What is electrolysis

A

The decomposition of the ionic compound into its elements using electricity

102
Q

What happens to ions in electrolysis

A

Positive ions gain electrons at the negative electrode and negative ions lose electrons at the positive electrode

103
Q

What are electrolytes

A

Solutions that conduct electricity containing ions

104
Q

How can a simple cell be made

A

By placing 2 metals in an electrolyte

105
Q

What does growing plants require

A

Nutrients

106
Q

What must a fertiliser contain to be effective

A

Nitrogen
Phosphorus
Potassium

107
Q

What are fertilisers

A

Substances which restore elements , essential for healthy plant growth

108
Q

What are ammonia and nitric acid important for

A

To produce soluble nitrogen contains salts (fertilisers)

109
Q

Describe ammonia

A

Pungent clear colourless gas which dissolves in water

110
Q

What happens if u dissolve ammonia in water

A

It produces an alkaline solution

111
Q

What is the Haber process

A

Production of ammonia required for fertiliser production

112
Q

What is the catalyst used in the haber process

A

Iron

113
Q

What is the starting material for the production of nitric acid

A

Ammonia

114
Q

What does the Ostwald process use

A

Ammonia
Oxygen
Water

115
Q

What is the catalyst used in the Ostwald process

A

Platinum

116
Q

What does radioactive decay involve

A

Changes in nuclei of atoms

117
Q

How can radioisotopes become more stable

A

By giving out alpha, beta or gamma radiation

118
Q

Alpha particles consist of?

A

2 protons and 2 neutrons and carry. A double positive charge

119
Q

What stops alpha radiation

A

A piece of paper

120
Q

Alpha particles will be attracted towards…..

A

Negatively charged plates

121
Q

What are beta particles

A

Electrons ejected from the nucleus of an atom

122
Q

What stops beta rays of radiation

A

A thin sheet of aluminium

123
Q

Beta particles are attracted to…..

A

Towards a positively charged plate

124
Q

What are gamma rays

A

waves emitted from within the nucleus of an atom

125
Q

What can stop gamma rays

A

Barriers like lead or concrete

126
Q

Gamma rays are not….

A

Deflected by an electric field

127
Q

What are the 3 radiation types

A

Gamma alpha beta

128
Q

How can an alpha particle be represented

A

4
He
2

129
Q

How can a beta particle be represented

A

0
e
-1

130
Q

How can proton be represented

A

1
P
1

131
Q

How can a neutron be represented

A

1
n
0

132
Q

What is a half life

A

The time for half of the nuclei of a particular isotope to decay

133
Q

The half life of an isoptope is a constant
What does this mean?

A

It is unaffected by chemical or physical conditions

134
Q

What can be used to date materials

A

Radioactive isotopes

135
Q

How do you determine a half life of an isotope

A

For a. Graph showing a decay curve

Chemistry (6 decks)

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