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combined science gcse 2022 > chem paper 1 > Flashcards

chem paper 1 Flashcards

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1
Q

what is the structure of an ionic compound?

A

giant regular lattice structure

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2
Q

what type of force is between what type of ions in ionic compounds?

A

strong electrostatic forces of attraction between oppositely charged ions

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3
Q

what is the melting/boiling point of iconic compounds like?

A

high

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4
Q

why are the melting and boiling points of ionic compounds high?

A

the strong attraction between ions take more energy to break

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5
Q

why can’t ionic compounds not conduct electricity when solid?

A

the ions are fixed into pace and can’t move

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6
Q

why can ionic compounds conduct electricity when molten?

A

the ions are free to move, so they can carry an electric current

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7
Q

in what state can ionic compounds conduct electricity?

A

molten/liquid

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8
Q

what is another way ionic compounds can conduct electricity?

A

when dissolved in a solution

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9
Q

why can ionic compounds conduct electricity when dissolved?

A

the ions are free to move in the solution, so they can carry an electric current

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10
Q

what is ionic bonding?

A

the transfer of electrons between a metal and no metal

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11
Q

what substance is a common example of ionic bonding?

A

salt

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12
Q

in terms of electrons , what happens to the metal and non metal in ionic bonding?

A

the metal loses an electron (becomes positively charged), while the non the metal gains an electron (becomes negatively charged)

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13
Q

what is it commonly called when oppositely charged ions are attracted by electrostatic forces?

A

ionic bonding

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14
Q

what are the 3 types of bonding?

A

ionic, covalent and metallic

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15
Q

what is the structure of an covalent molecule?

A

simple molecular substance

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16
Q

what is covalent bonding?

A

a bond that forms when a pair of electrons are shared between 2 atoms

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17
Q

what diagram is used to show covalent bonding?

A

dot and cross with overlapping shells

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18
Q

what diagram is used to show ionic bonding?

A

dot and cross formed like a reactant to product equation

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19
Q

what are the forces between covalent molecules like in contrast to covalent bonding?

A

very weak

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20
Q

what is the melting/boiling point of simple covalent compounds like?

A

low

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21
Q

why are the melting and boiling points of covalent compounds low?

A

because you only need to break the weak intermolecular forces of attraction

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22
Q

what state are covalent compound usually at room temperature?

A

liquids or gasses

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23
Q

what happens to the intermolecular forces of attraction as a molecule gets bigger?

A

the force increases

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24
Q

what happens to the melting and boiling points of covalent compounds if the molecule gets bigger?

A

increase in temp due to more energy needed to break them

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25
Q

do covalent compound conduct electricity?

A

no

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26
Q

why can’t covalent compounds conduct electricity?

A

they do not have any free electrons or ions

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27
Q

what are polymers?

A

chains of covalently bonded carbon atoms

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28
Q

What is the charge of an electron?

A

Negative

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29
Q

What is the charge of a proton?

A

Positive

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30
Q

What is the charge of a neutron

A

Neutral

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31
Q

What is an ion?

A

An atom or group of atoms with a positive or negative charge

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32
Q

What happens to an atom if it gains or loses and electron?

A

It becomes an ion

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33
Q

What groups are most likely to form ions?

A

Groups 1, 2, 6 and 7

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34
Q

What charge do group 1 and 2 elements typically have?

A

Group 1: 1+

Group 2: 2+

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35
Q

What charge do group 6 and 7 elements typically have?

A

Group 6: 2-

Group 7: 1-

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36
Q

What are group 1 and 2 elements?

A

Metals

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37
Q

What are group 6 and 7 elements?

A

Non metals

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38
Q

What are anions?

A

Negative ions that have gained electrons

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39
Q

What are cations?

A

Positive ions that have lost electrons

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40
Q

What stupid saying is a good way to remember the metals reactivity series?

A

PeopleSayLittleChildrenMakeAZebraIllConstantlySniffingGiraffes.

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41
Q

In which direction does reactivity increase in group 1?

A

Downwards

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42
Q

In with direction does reactivity increase in group 7?

A

Upwards

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43
Q

What do the periods down the side of the periodic table represent?

A

How many shells the element has in its atom

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44
Q

How are giant covalent structures bonded?

A

Atoms are bonded by strong covalent bonds

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45
Q

What are the melting and boiling points of giant covalent structures like?

A

High

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46
Q

Why are the melting and boiling points of giant covalent structures high?

A

The strong covalent bonds require more energy to break them

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47
Q

What are some examples of carbon based giant covalent structures?

A

Dimond, graphite and graphene

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48
Q

What are diamonds make up of?

A

A network of carbon atoms that each form 4 covalent bonds

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49
Q

How is graphite different to diamond?

A

Each carbon atom only forms 3 covalent bonds

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50
Q

What are the forces like between sheets of graphite?

A

Weak intermolecular forces

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51
Q

What do the week intermolecular forces between sheets of graphite make it good for?

A

Dry lubrication

52
Q

What is graphite’s melting point like?

A

High

53
Q

What is the equation to find concentration?

A

Concentration (Gdm³) = mass (g) ÷ volume (dm)

54
Q

What is the molecular formula?

A

The actual number of each atom in a molecule

55
Q

What is the empirical formula?

A

The simplest ratio of atoms of each element in a molecule

56
Q

What would the relative formula mass of H₂O₂ when the mass is H = 1 and O = 16?

A

1 + 1 + 16 + 16 =34

57
Q

What would the empirical formula of H₂O₂ be?

A

HO

58
Q

What does Mr stand for?

A

relative molecular mass

59
Q

What does Ar stand for?

A

Relative atomic mass

60
Q

What is the formula to find the number of moles?

A

of moles = mass of element/compound ÷ Mr or Ar of element

61
Q

What is Avogadro’s constant?

A

6.02 × 10²³

62
Q

What does one mole equal?

A

6.02 + 10²³ (Avogadro’s constant)

63
Q

What is the mass of one mole of a particular atom equal to?

A

The atomic mass on the periodic table

64
Q

What is another way to find the number of moles in a sample?

A

of moles = mass of sample ÷ mass of one mole of that element

65
Q

What is another word for “balance” equation?

A

Stoichiometric

66
Q

What is it called when the atoms of an element go around in pairs?

A

Diatomic molecule

67
Q

What are fullerenes?

A

Molecules of carbon shaped like closed tubes or hollow spheres

68
Q

How are atoms usually arranged in fullerenes?

A

Hexagons (sometimes Pentagons or heptagons)

69
Q

What is the molecular formula of a buckminsterfullerene?

A

C60

70
Q

Are buckminsterfullerene’s stable or unstable?

A

Stable

71
Q

What can fullerenes be used for?

A

‘Caging’ other molecules. This could be used to deliver drugs directly to cells in the body.

72
Q

What do fullerenes have?

A

Huge surface area

73
Q

What is graphene?

A

A type of fullerene that is a single layer of graphite (one atom thick)

74
Q

Why can graphite conduct electricity?

A

Only 3 of the 4 electrons are used in bonds, so the 4th one is delocalised (free)

75
Q

There are 6 steps to an experiment finding the empirical formula of magnesium oxide what is step 1?

A
  1. Weigh the mass of my ribbon an dthe mass of the crucible
76
Q

There are 6 steps to an experiment finding the empirical formula of magnesium oxide what is step 2?

A
  1. Coil mg ribbon and place it in the crucible with the lid at an angle to allow oxygen to enter
77
Q

There are 6 steps to an experiment finding the empirical formula of magnesium oxide what is step 3?

A
  1. Place the crucible into a pipe-clay triangle on a tri pod and light a bunsen burner
78
Q

There are 6 steps to an experiment finding the empirical formula of magnesium oxide what is step 4?

A
  1. After 5 mins/once mg has stopped glowing remove from bunsen burner and allow to cool
79
Q

There are 6 steps to an experiment finding the empirical formula of magnesium oxide what is step 5?

A
  1. Once the crucible is cool to touch, weigh the crucible and its contents
80
Q

There are 6 steps to an experiment finding the empirical formula of magnesium oxide what is step 6?

A
  1. Subtract the mass of the crucible and the Mg from the MgO to find the mass of the oxygen.
    From there you can calculate the empirical formula.
81
Q

What does it mean by a limiting reactant?

A

Reactions stop when on reactant has been used up. This limits the amount of product formed.

82
Q

If the amount of limiting reactant is decreased, then the amount of product made will…….

A

Decrease

83
Q

If the amount of limiting reactant is increased, then the amount of product made will…….

A

Increase

84
Q

If the amount of an excess reactant is increased, then the amount of product made will…….

A

Not change

85
Q

What do acids form in water?

A

H+ ions

86
Q

What do soluble alkaline bases form in water?

A

OH- ions

87
Q

What is produced during a naturalisation reaction?

A

Salt and water

88
Q

What produces a naturalisation reaction?

A

An acid and a base

89
Q

What is the ionic equation of a naturalisation reaction?

A

H+ + OH- → H²O

90
Q

What is the neutralisation equation for hydrochloric acid and sodium hydroxide?

A

NaOH (base) + HCl (acid) → H2O (water) + NaCl (salt)

91
Q

What colour would litmus paper change to in acidic solutions?

A

Red

92
Q

What colour would litmus paper change to in neutral solutions?

A

Purple

93
Q

What colour would litmus paper change to in alkaline solutions?

A

Blue

94
Q

What colour would methyl orange change to in acidic solutions?

A

Red

95
Q

What colour would methyl orange change to in neutral or alkaline solutions?

A

Yellow

96
Q

What colour would phenolphthalein change to in acidic or neutral solutions?

A

It would remain colour less

97
Q

What colour would phenolphthalein change to in alkaline solutions?

A

Pink

98
Q

All acids ionise in solutions, what does this mean?

A

Splitting up to produce H+ ions and another ion

99
Q

What do strong acids do?

A

Ionise almost completely in water

100
Q

What are examples of strong acids?

A

Sulfuric, hydrochloric and nitric acid

101
Q

What pH do strong acids tent to have?

A

Low pH (0-2)

102
Q

What do weak acids do?

A

Not fully ionise in solutions

103
Q

What examples of weak acids are there?

A

Ethanoic, citric and carbonic acid

104
Q

What pH do weak acids tent to have?

A

High pH (2-6)

105
Q

What does acid strength tell you?

A

What proportion of the acid molecules ionise in water

106
Q

What does concentration of an acid measure?

A

How much acid there is in a litre

107
Q

An acid with a large number of acid molecules compared to the volume of water is said to be…..

A

Concentrated

108
Q

An acid with a small number of acid molecules compared to the volume of water is said to be…..

A

Dilute

109
Q

What can concentration be measured in?

A

g dm‐³ or mol dm‐³

110
Q

What does the concentration of H+ ion increase by?

A

A factor of 10

111
Q

If the concentration of H+ ions increases by a factor of 10, what does the pH decrease by?

A

1

112
Q

If you decrease the H+ ion concentration by a factor of 10 what happens to the pH?

A

Increases by 1

113
Q

What salt would hydrochloric acid produce?

A

Chloride salt

114
Q

What salt would sulfuric acid produce?

A

Sulfate salts

115
Q

What salt would nitric acid produce?

A

Nitrate salts

116
Q

Acid + ______or______ → salt + water

A

Acid + metal oxide or metal hydroxide → salt + water

117
Q

Acid + metal carbonate → salt + water + _________

A

Acid + metal carbonate → salt + water + carbon dioxide

118
Q

How do you test for hydrogen?

A

Lit splint test in a test tube. It should a “squeaky pop”

119
Q

What is the cause of the “squeaky pop” in the test for hydrogen?

A

The hydrogen burning with oxygen in the air to produce water

120
Q

How do you test for carbon dioxide?

A

Bubbling carbon dioxide thought lime water will turn cloudy

121
Q

Common salts of sodium, potassium and ammonium are…..

A

Soluble

122
Q

Nitrates are….

A

Soluble

123
Q

Common chloride are…..

A

Soluble (except silver chloride and lead chloride)

124
Q

Common sulfates are…..

A

Soluble (except lead, barium and calcium sulfate)

125
Q

Common carbonated and hydroxide are……

A

Insoluble (except sodium, potassium and ammonium ones)

combined science gcse 2022 (7 decks)

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