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PMT OCR A-Level Chemistry > Module 3 – Periodic Table & Energy > Flashcards

Module 3 – Periodic Table & Energy Flashcards

1
Q

What is a common name given to group 2 metals?

A

Alkaline earth metals

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2
Q

What is the most reactive metal of group 2?

A

Barium

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3
Q

List 3 physical properties of group 2 metals

A
  1. High melting and boiling points 2. Low density metals 3. Form colourless (white) compounds
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4
Q

The highest energy electrons of group 2 metals are in which subshell?

A

S subshell

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5
Q

Does reactivity increase or decrease going down group 2? Why?

A
  • Increases - Electrons are lost more easily because larger atomic radius and more shielding
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6
Q

What happens to the first ionisation energy as you go down group 2? Why?

A

Decreases because: - Number of filled electron shells increases down the group, therefore increased shielding - Increased atomic radius therefore weaker force between outer electrons and nucleus - So less energy needed to remove an electron

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7
Q

What type of reaction is the reaction between group 2 elements and oxygen?

A

Redox reaction

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8
Q

Write an equation for the reaction of calcium and oxygen

A

2Ca (s) + O2 (g) -> 2CaO (s)

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9
Q

What is the product when group 2 elements react with water?

A

Hydroxide and hydrogen gas

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10
Q

Which group 2 element doesnt react with water?

A

Beryllium

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11
Q

Which group 2 element reacts very slowly with water?

A

Magnesium

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12
Q

What type of reaction is the reaction between group 2 metals and water?

A

Redox reaction

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13
Q

Write an equation for the reaction of Barium and water

A

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

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14
Q

What is oxidised and what is reduced in a reaction between a group 2 metal and water?

A

The metal is oxidised One hydrogen atom from each water is reduced

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15
Q

What are the products when a group 2 element reacts with dilute acid?

A

Salt and hydrogen gas

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16
Q

Write an equation for the reaction of calcium and hydrochloric acid?

A

Ca (s) + 2HCl (aq) -> CaCl2 (s) + H2 (g)

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17
Q

What is formed when group 2 oxides react with water?

A

Metal hydroxide

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18
Q

Write an equation for the reaction between a group 2 oxide (M) and water

A

MO (s) + H2O (l) -> M(OH)2 (aq)

19
Q

What group 2 metal oxide is insoluble in water?

A

Beryllium oxide

20
Q

What is the trend in hydroxide solubility down group 2?

A
  • Increases down the group - Mg(OH)2 is slightly soluble - Ba(OH)2 creates a strong alkaline solution
21
Q

What is Ca(OH)2 used for? Write an equation related to one of its uses

A

Used to neutralise soil Ca(OH)2 (aq) + 2HCl (aq) -> 2H2O (l) + CaCl2 (aq)

22
Q

What is Mg(OH)2 used for?

A

An antacid to treat indegestion, heartburn, ect

23
Q

What is calcium carbonate used for?

A

Present in limestone and marble Used in building construction

24
Q

What is the drawback of using calcium carbonate in construction? Write a related equation

A

Group 2 carbonates react with acid CaCO3 (s) + 2HCl (aq) -> CaCl2 (aq) + H2O (l) + CO2 (g)

25
Q

How are the elements arranged in a periodic table?

A

They are arranged in the order of increasing atomic numbers

26
Q

What is a period on the periodic table?

A

The horizontal rows in the periodic table

27
Q

What is a group on a periodic table?

A

The vertical columns

28
Q

What is meant by periodicity?

A

The repeating trends in chemical and physical properties

29
Q

What change happens across each period?

A

Elements change from metals to non-metals

30
Q

How can the electron configuration be written in short?

A

The nobel gas before the element is used to abbreviate
E.g. Li -> 1s22s1 ; Li -> [He] 2s1

31
Q

Define first ionisation energy

A

The energy required to remove one electron from each atom in one mole of the gaseous element to form one mole of gaseous 1+ ions

32
Q

Write an equation for the first ionisation energy of magnesium

A

Mg (g) -> Mg+ (g) + e-

33
Q

What are the factors that affect ionisation energy?

A

Atomic radius
Nuclear charge
Electron shielding or screening

34
Q

Explain the trend on this graph

A

First ionisation energy increases across period 3 because of: Increased nuclear charge
Decreased atomic radius
Same electron shielding
So more energy is needed to remove the first electron
Dips at Al because:
Outer electron is in a 3p orbital
3p orbital is higher energy than 3s orbital
Less energy is needed to remove the electron
Dips at S because:
One 3p orbital contains 2 electrons
Repulsion occurs between the paired electrons
Less energy is needed to remove an electron

35
Q

Why does first ionisation energy decrease between group 2 and 3?

A

In group 3 the outermost electrons are in p orbitals
In group 2 the outermost electrons are in s orbitals
Electrons in p orbitals are easier to remove

36
Q

Why does first ionisation energy decrease between group 5 to 6?

A

Group 5 electrons in p orbital are single electrons
Group 6 electrons are spin paired, with some repulsion
So group 6 electrons are easier to remove

37
Q

Does first ionisation increase or decrease between the end of one period and the start of the next? Why?

A

Decrease
Atomic radius increases
Electron shielding increases

38
Q

Does first ionisation increase or decrease down a group? Why?

A

Decrease
Shielding increases so attraction is weaker
Atomic radius increases
Distance between the outer electrons and nucleus increases
Attraction is weaker
Increase in number of protons is outweighed by increase in distance and shielding

39
Q

What are the properties of giant metallic lattices? (4)

A

High melting and boiling point
Good electrical conductors
Malleability
Ductility

40
Q

What is a ductile metal?

A

A metal which can be stretched
E.g. can be made into wires

41
Q

What is a malleable metal?

A

The metal can be shaped into different forms

42
Q

Describe the structure, forces and bonding in every element across period 2

A

Li and Be -> giant metallic; strong attraction between positive ions and delocalised electrons; metallic bonding
B and C -> giant covalent; strong forces between atoms; covalent
N2, O2, F2 and Ne -> simple molecular; weak intermolecular forces between molecules; covalent bonding within molecules and intermolecular forces between molecules

43
Q

Describe the structure, forces and bonding in every element across period 3

A

Na, Mg, Al -> giant metallic; strong attraction between positive ions and delocalised electrons; metallic bonding
Si -> giant covalent; strong forces between atoms; covalent
P4, S8, Cl2, Ar -> simple molecular; weak intermolecular forces between molecules; covalent bonding within molecules and intermolecular forces between molecules

PMT OCR A-Level Chemistry (3 decks)

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