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GCSE Chemistry > GCSE Topic 6 - Periodic table > Flashcards

GCSE Topic 6 - Periodic table Flashcards

1
Q

Cation

A

Positively charge ion, such as Na+

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2
Q

Anion

A

Negatively charge ion, such as Cl-

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3
Q

What happens to group 1 metals in a reaction, in terms of electrons?

A

Group 1 metal atoms lose 1 electron to become a cation with a charge of 1+

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4
Q

What happens to group 2 metals in a reaction, in terms of electrons?

A

Group 2 metal atoms lose 2 electrons to become a cation with a charge of 2+

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5
Q

What happens to group 3 metals in a reaction, in terms of electrons?

A

Group 3 metal atoms lose 3 electron to become a cation with a charge of 3+

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6
Q

What happens to group 5 non-metals in a reaction, in terms of electrons?

A

Group 5 non-metal atoms in a molecule each gain 3 electrons to become a cation with a charge of 3-

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7
Q

What happens to group 6 non-metals in a reaction, in terms of electrons?

A

Group 6 non-metal atoms in a molecule each gain 2 electrons to become a cation with a charge of 2-

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8
Q

What happens to group 7 non-metals in a reaction, in terms of electrons?

A

Group 7 non-metal atoms in a molecule each gain 1 electron to become a cation with a charge of 1-

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9
Q

Oxidation, in terms of electrons

A

Loss of electrons

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10
Q

Reduction, in terms of electrons

A

Gain of electrons

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11
Q

Redox reaction

A

A reaction where one substance is oxidised and another substance is reduced.

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12
Q

Trend in reactivity of group 1 metals

A

Reactivity increases down the group

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13
Q

Explanation for the trend in reactivity of group 1 metals

A

This would be a grade 9 answer

  • Reactivity increases down the group
  • This is because atomic radius increases
  • So the distance between the positive nucleus and negative outer electron increases
  • Number of shells increases
  • So electron shielding increases
  • Both of these factors cause the electrostatic attraction between the nucleus and outer electron to decrease
  • So the metal atom more easily loses its outer electron
  • And is more easily oxidized
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14
Q

Symbol equation for the reaction of lithium with water

A

2 Li (s) + 2 H2O (l) → 2 LiOH (aq) + H2 (g)

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15
Q

Symbol equation for the reaction of sodium with water

A

2 Na (s) + 2 H2O (l) → 2 NaOH (aq) + H2 (g)

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16
Q

Symbol equation for the reaction of potassium with water

A

2 K (s) + 2 H2O (l) → 2KOH (aq) + H2 (g)

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17
Q

Symbol equation for the reaction of sodium with oxygen

A

2 Na (s) + O2 (g) → Na2O (s)

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18
Q

Symbol equation for the reaction of potassium with oxygen

A

2 K (s) + O2 (g) → K2O (s)

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19
Q

Symbol equation for the reaction of magnesium with oxygen

A

2 Mg (s) + O2 (g) → 2 MgO (s)

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20
Q

Symbol equation for the reaction of sodium with chlorine

A

2 Na (s) + Cl2 (g) → 2 NaCl (s)

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21
Q

Symbol equation for the reaction of potassium with chlorine

A

2 K (s) + Cl2 (g) → 2 KCl (s)

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22
Q

Type of reaction between a metal and a non-metal

A

Redox reaction

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23
Q

pH of a potassium hydroxide solution

A

pH 12 to 14

Strongly alkaline

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24
Q

Ion that makes solutions alkaline

A

Hydroxide ion

OH- (aq)

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25
Q

Half equation for the reactions of sodium

A

Na → Na+ + e-

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26
Q

Half equation for the reactions of chlorine

A

Cl2 + 2 e- → 2 Cl-

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27
Q

Observations for the reaction of lithium with water

A
  • Effervescence
  • Lithium floats on the surface (it has half the density of water)
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28
Q

Observations for the reaction of sodium with water

A
  • Effervescence
  • Sodium melts into a ball
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29
Q

Observations for the reaction of potassium with water

A
  • Effervescence
  • Potassium melts into a ball
  • Lilac flame (the reaction is highly exothermic, causing the hydrogen gas to ignite)
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30
Q

Trend in melting points of group 1 metals

A

Decreases down the group

The metals can be cut with a knfe

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31
Q

Explanation for the trend in melting points of alkali metals

A
  • Melting points decrease down the group
  • This is because metallic bond strength decreases
  • Metallic bonding is the electrostatic attraction between the cations and sea of delocalised electrons
  • This electrostatic attraction gets weaker from Li to Na to K
  • Because the charge density decreases
  • As the charge stays the same but the atomic radius increases
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32
Q

Colour of potassium hydroxide solution with universal indicator

33
Q

Compare the reactivity of the alkali metals with water

A
  • General equation is 2 M (s) + 2 H2O (l) à 2 MOH (aq) + H2 (g) , where M is a group 1 metal
  • Lithium, sodium and potassium all effervesce as hydrogen gas is produced
  • They all react with water to produce a soluble hydroxide
  • And strongly alkaline solution of pH 12 to pH14 owing to production of the hydroxide, OH- ion
  • Sodium and potassium melt into a ball
  • Potassium reacts with water to produce a lilac flame
  • Reactivity increases from Li to Na to K
  • The reactions get progressively more exothermic
  • The reaction between potassium and water is sufficiently exothermic to ignite the hydrogen gas produced
34
Q

Number of available electron shells for a sodium ion

35
Q

Number of occupied electron shells for a sodium ion

36
Q

Number of occupied electron shells for a sodium atom

37
Q

Colour of fluorine

38
Q

Colour of chlorine

A

yellow-green

39
Q

Colour of bromine

A

orange-red

40
Q

Colour of solid iodine

A

shiny black solid

41
Q

Colour of aqueous iodine

42
Q

Colour of iodine vapour

43
Q

Colour of iodine in hexane

44
Q

Trend in melting point for the halogens

A
  • Increases down the group
  • Fluorine is a gas
  • Chlorine is a gas
  • Bromine is a liquid
  • Iodine is a solid
45
Q

Explanation for the trend in melting point for the halogens

A
  • Intermolecular forces become greaterr from F2 to I2
  • More thermal energy is required to overcome these forces
46
Q

Trend in reactivity for the halogens

A

Decreases down the group

47
Q

Explanation for the trend in reactivity of the halogens

A

This would be a grade 9 answer

  • Reactivity DECREASES down the group
  • This is because atomic radius increases
  • So the distance between the positive halogen nucleus and the negative outer electron of a NEIGHBOURING atom increases
  • Number of shells increases
  • So electron shielding increases
  • Both of these factors cause the electrostatic attraction between the halogen nucleus and the negative outer electron of a NEIGHBOURING atom increases
  • So the non-metal atom LESS easily gains an electron
  • And is LESS easily reduced
48
Q

Symbol equation for the reaction of fluorine with potassium chloride

A

F2 (g) + 2 KCl (aq) → Cl2 (g) + 2 KF (aq)

There will be NO colour change. Potassium iodide is colourless and chlorine gas dissolves in water to make a colourless solutuion, unlike bromine and iodine.

49
Q

Symbol equation for the reaction of chlorine with potassium bromide

A

Cl2 (g) + 2 KBr (aq) → Br2 (l) + 2 KCl (aq)

There will be a colour change from colourless to orange. Note that the bromine that is produced will be dissolve in water to produce an orange solution.

50
Q

Symbol equation for the reaction of chlorine with potassium iodide

A

Cl2 (g) + 2 KI (aq) → I2 (s) + 2 KCl (aq)

There will be a colour change from colourless to brown. Note that the iodine that is produced will be dissolve in water to produce a brown solution.

51
Q

Symbol equation for the reaction of bromine with potassium iodide

A

Br2 (l) + 2 KI (aq) → I2 (s) + 2KBr (aq)

There will be a colour change from colourless to brown. Note that the iodine that is produced will be dissolve in water to produce a brown solution.

52
Q

Ionic equation for the reaction of fluorine and potassium chloride

A

F2 (g) + 2 Cl- (aq) → Cl2 (g) + 2 F- (aq)

Only the molecules and ions involved in the reaction appear in the ionic equation. The other ions are spectator ions and do not take place in the reaction.

These reactions are redox reactions. The more reactive halogen is reduced, the less reactive halogen is oxidized.

53
Q

Ionic equation for the reaction of chlorine and potassium bromide

A

Cl2 (g) + 2 Br- (aq) → Br2 (l) + 2 Cl- (aq)

Only the molecules and ions involved in the reaction appear in the ionic equation. The other ions are spectator ions and do not take place in the reaction.

These reactions are redox reactions. The more reactive halogen is reduced, the less reactive halogen is oxidized.

54
Q

Ionic equation for the reaction of chlorine and potassium iodide

A

Cl2 (g) + 2 I- (aq) → I2 (s) + 2Cl- (aq)

Only the molecules and ions involved in the reaction appear in the ionic equation. The other ions are spectator ions and do not take place in the reaction.

These reactions are redox reactions. The more reactive halogen is reduced, the less reactive halogen is oxidized.

55
Q

Ionic equation for the reaction of bromine and potassium iodide

A

Br2 (l) + 2 I- (aq) → I2 (s) + 2Br - (aq)

Only the molecules and ions involved in the reaction appear in the ionic equation. The other ions are spectator ions and do not take place in the reaction.

These reactions are redox reactions. The more reactive halogen is reduced, the less reactive halogen is oxidized.

56
Q

Half equation for fluorine

A

F2 (g) + 2 e- → 2 F- (aq)

These reactions show what is happening in terms of electrons. Only ONE halogen appears in this equation.

Each halogen atom in a halogen molecule gains one electron to become a halide 1- ion.

57
Q

Half equation for chlorine

A

Cl2 (g) + 2 e- → 2 Cl- (aq)

These reactions show what is happening in terms of electrons. Only ONE halogen appears in this equation.

Each halogen atom in a halogen molecule gains one electron to become a halide 1- ion.

58
Q

Half equation for bromine

A

Br2 (l) + 2 e- → 2 Br- (aq)

These reactions show what is happening in terms of electrons. Only ONE halogen appears in this equation.

Each halogen atom in a halogen molecule gains one electron to become a halide 1- ion.

59
Q

The least reactive group of elements

A

Noble gases

NOT Nobel gases

60
Q

This noble gas reacts with fluorine

A

Xenon

Xenon tetrafluoride is formed, XeF4

61
Q

This noble gas is the least reactive element

62
Q

Explanation for the low reactivity of the noble gases

A

The atoms have a full outer shell of electrons

63
Q

Uses of noble gases

A
  • Flammable or highly reactive liquids are placed in a container with an atmosphere of a noble gas
  • Fill balloons with helium as its density is a lot less than the density of air
64
Q

Trend in boiling point for the noble gases

A

Increases down the group

GCSE Chemistry (5 decks)

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