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Periodicity > Topic 7 & 8 > Flashcards

Topic 7 & 8 Flashcards

1
Q

What are the properties of giant metallic lattices?

A
  1. High melting and boiling point.
  2. Good electrical conductors.
  3. Malleability
  4. Ductility
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2
Q

What is a ductile metal?

A

Metal that can be stretched eg. Wires.

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3
Q

What is a malleable metal?

A

Metal that can be shaped into different forms

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4
Q

Describe structure, forces and bonding between every element across period 2.

A

Li & Be: Giant covalent; Strong attraction between +ions and delocalised electrons; metallic bonding.

B & C: Giant covalent; strong forces between atoms; covalent bonding.

N2; O2; F2; Ne: Simple molecular; weak intermolecular forces between molecules; covalent intramolecular forces and intermolecular forces between molecules l.

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5
Q

How are atoms arranged in the periodic table?

A

Increasing atomic number

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6
Q

Define ‘Periodicity’

A

Repeating trends in chemical and physical properties.

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7
Q

What change happens across a period?

A

Elements change from metals to non metals

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8
Q

Define first ‘ionisation energy.’

A

Minimum energy required to remove one mole of electrons from one mole of an atom in its gaseous state.

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9
Q

Write an equation to show first ionisation of Ca

A

Ca(g) —> Ca+ (g) + e-

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10
Q

Name all factors affecting ionisation energy

A
  1. Atomic Radius
  2. Nuclear charge
  3. Electron shielding
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11
Q

Why does first ionisation decrease between group 2 to 3?

A

Group 3’s outer electrons are in p orbitals and Group 2’s are in s orbitals. P orbitals are further away so less attraction between nucleus and outer electrons.

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12
Q

Why does first Ionisation decrease between the end of one period and the start of the next?

A

There is an increase of atomic radius and shielding.

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13
Q

Why does first ionisation decrease down a group?

A
  1. Increased shielding.

2. Increased atomic radius

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14
Q

What is the common name of group 2 metals?

A

Alkaline earth metals

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15
Q

What is the most reactive metal of group 2?

A

Barium

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16
Q

State three physical properties of group 2 metals.

A
  1. High melting points
  2. Low density metals
  3. Form colourless (white) compounds
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17
Q

What subshell has the highest energy electrons in group 2?

A

S subshell

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18
Q

What happens to reactivity down group 2? Why?

A

Reactivity increases

Because electrons are lost more easily due to increased atomic radius and shielding.

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19
Q

What happens to first ionisation energy down group 2? Why?

A
  1. Filled electron shells increase —> increases shielding
  2. Increased atomic radius —> weaker force between nucleus and outer electron
  3. Less energy required to remove the electron.
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20
Q

State the reaction that takes place between a group 2 metal and oxygen.

A

Redox reaction

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21
Q

Write the equation for the reaction of calcium and oxygen.

A

2Ca(s) + O2(g) —> 2CaO(s)

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22
Q

What products are formed when group 2 elements react with water?

A

Metal Hydroxide and Hydrogen gas.

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23
Q

What group 2 element doesn’t react with water?

A

Beryllium

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24
Q

What group 2 element reacts very slowly with water?

A

Magnesium

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25
Q

Name the type of reaction that takes place between group 2 metals and water.

A

Redox reactions.

26
Q

Write an equation showing the reaction between barium and water.

A

Ba(s) + 2H2O(l) —> Ba(OH)2(aq) + H2 (g)

27
Q

What is oxidised and reduced between group 2 metal and water?

A

Metal = oxidised

Hydrogen from water = reduced

28
Q

What products are formed when a group 2 metal reacts with a dilute acid?

A

Salt and hydrogen gas.

29
Q

Write a reaction between calcium and hydrochloric acid

A

Ca(s) + 2HCl(aq) —> CaCl2(s) + H2(g)

30
Q

What products are formed when group 2 reacts with a water?

A

Metal hydroxide

31
Q

State an equation for the reaction between a group 2 oxide and water.

A

MO(s) + H2O(l) —> M(OH)2(aq)

32
Q

What group 2 metal oxide is insoluble in water?

A

Beryllium oxide

33
Q

State the trend in hydroxide solubility down group 2.

A
  1. Increases down group
  2. Mg(OH)2 is slightly soluble
  3. Ba(OH)2 creates a strong alkaline solution.
34
Q

State a use of Ca(OH)2.

Write an equation for the use.

A

Ca(OH)2(aq) + 2HCl(aq) —> 2H2O(l) + CaCl2(aq)

35
Q

What is Mg(OH)2 used for.

A

Antacid to treat indigestion

36
Q

What is calcium carbonate used for?

A

Found in Limestone and used for building construction.

37
Q

What is a drawback of using calcium carbonate in construction?

A

Group 2 metals react with acids.

38
Q

What group are known as the ‘halogens’?

A

Group 7

39
Q

State two properties of halogens.

A
  1. Low melting & boiling points

2. Exist as diatomic molecules eg. Cl2

40
Q

State the trend in boiling points down group 7, provide reasons for your answer.

A

Increases down the group.

  1. Atomic size increases down the group
  2. This means there are stronger london forces hence more energy needed to overcome these intermolecular forces.
41
Q

State the trend in reactivity down group 7, provide reasons for your answer.

A

Reactivity decrease down the group.

  1. Increased atomic radius
  2. Increased shielding
  3. Ability to gain electron decreases.
42
Q

State the trend of oxidising ability down group 7. Provide reasons for your answer.

A

Decreases down a group.

  1. Cl has smallest atomic radius meaning pull of nucleus is strongest compared to I.
  2. Cl is easily reduced.
  3. Cl is the best oxidising agent
43
Q

What is a ‘displacement reaction’

A

When a halogen displaces a less reactive halide.

44
Q

What colour is ‘Chlorine water’?

A

Pale green

45
Q

What colour is ‘bromine water’?

A

Orange

46
Q

What colour is ‘iodine in water’?

A

Brown

47
Q

What colour is chlorine in cyclohexane?

A

Pale green.

48
Q

What colour is bromine in cyclohexane?

A

Orange

49
Q

What colour is iodine in cyclohexane?

A

Violet

50
Q

Between halides Cl- Br- & I-, which ones can be oxidised by Cl2?

A

Br- and I- ions.

51
Q

State the equation of chlorine oxidising bromide ions.

A

Cl2(aq) + 2Br-(aq) —> 2Cl(aq) + Br2(aq)

52
Q

Show the equation for Cl2 oxidising 2I-

A

Cl2(aq) + 2I-(aq) —> 2Cl-(aq) + I2(aq)

53
Q

Between Cl-, Br- and I- which ones can be oxidised by bromine?

A

I- ions

54
Q

Show the equation for bromine oxidising iodide ions.

A

Br2 + 2I- —> 2Br- + I2

55
Q

Between Cl-, Br- and I- which of these can be oxidised by iodine?

A

None.

56
Q

What is ‘disproportionation’?

A

Oxidation and reduction of the same species in a redox reaction.

57
Q

Show the reaction of Cl2 and water.

A

Cl2(g) + H2O(l) —> HClO(aq) + HCl (aq)

58
Q

What type of reaction happens between chlorine and water?

A

Disproportionation.

Chlorine is oxidised and reduced

59
Q

Why is chlorine added to drinking water?

A

Kills bacteria in the water

60
Q

What are the two forms of the chlorite ion?

A

ClO- is chlorate (I)

ClO3- is chlorate (V)

61
Q

What is the formula for bleach?

A

NaClO

62
Q

Show the equation for the formation of bleach

A

Cl2 + 2NaOH(aq) —> NaCl + NaClO + H2O

Periodicity (2 decks)

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