Physical & Chemical Trends in Group 2 (Cambridge International A-Level Chemistry)

Physical & Chemical Trends in Group 2

Chemical trends

• All elements in Group 2 (also called alkali earth metals) have the two electrons in their outermost principal quantum shell
• All Group 2 metals can form ionic compounds in which they donate these two outermost electrons(so they act as reducing agents) to become an ion with +2 charge (so they themselves become oxidised)
• Going down the group, the metals become more reactive
• This can be explained by looking at the Group 2 ionisation energies:

Graph of the first and second ionisation energies of the Group 2 elements

The graph shows that both the first and second ionisation energies decrease going down the table

• The first ionisation energy is the energy needed to remove the first outer electron of an atom

• The second ionisation energy is the energy needed to remove the second outer electron of an atom

• The graph above shows that going down the group, it becomes easier to remove the outer two electrons of the metals

• Though the nuclear charge on the nucleus increases going down the group (because there are more protons);

  • Factors such as an increased shielding effect and a larger distance between the outermost electrons and the nucleus outweigh the attraction of the higher nuclear charge

• The elements become more reactive going down the group as it gets easier for the atoms to lose two electrons and become 2+ ions

• This trend is shown by looking at the reactions of the Group 2 metals:

  • With dilute hydrochloric acid;

    • Bubbles of hydrogen gas are given off much faster indicating that the reactions become more vigorous

  • With oxygen;

    • The metals get more reactive with oxygen down the group (Ba is so reactive, that it must be stored in oil to prevent it from reacting with oxygen in air)

Physical trends

• Going down the group, the elements become larger as the outer two electrons occupy a new principal quantum shell which is further away from the nucleus

The atomic radius of the Group 2 elements

The atomic radius of the Group 2 elements increases going down the group due to the addition of an extra principal quantum shell

Graph of the atomic radius descending Group 2

The graph shows an increase in atomic radius going down the group

• The melting point of the elements decreases going down the group as the outer electrons get further away from the nucleus
• This means that the attraction between the nucleus and the bonding electrons decreases causing a decrease in melting point

Graph of the melting points descending Group 2

The graph shows a general decrease in melting point going down the group

• As you go down the group, the density of the alkali earth metals increases

Graph of the density descending Group 2

The graph shows an overall increase in density going down the group

Worked Example Predicting properties of radium

Radium, Ra, is a radioactive element found below barium, at the bottom of Group 2.

Applying your knowledge of the Group 2 elements, predict:

1. The formula of the ion formed by radium.
2. The formula radium's oxide and hydroxide.
3. The first ionisation energy of radium.
4. The reactivity of radium compared to barium.
5. The relative pH of a saturated radium hydroxide solution compared with a saturated calcium hydroxide solution.
6. The solubility of radium sulfate compared with strontium sulfate.
7. The equation for the reaction of solid radium oxide with dilute hydrochloric acid.
8. What you would expect to see if you mixed radium hydroxide solution with dilute sulfuric acid.

Answer

• Answer 1:

  • Since Ra is in Group 2, it will form an ion with a +2 charge to give Ra²⁺

• Answer 2:

  • The Group 2 oxides and hydroxides have the general formula XO and X(OH)₂ respectively, where X is the Group 2 element
  • Therefore, radium oxide is RaO and radium hydroxide is Ra(OH)₂

• Answer 3:

  • Radium is below barium, so its atomic radius is larger than the atomic radius of barium.
  • This means that radium’s outermost electrons are even further away and are therefore even more easily removed than barium’s outermost electron pair.
  • The first ionisation energy is between 450 - 480 kJ mol^-1

• Answer 4:

  • Radium’s outermost electrons are even further away than in barium and are therefore more easily removed, making radium more reactive than barium

• Answer 5:

  • The Group 2 hydroxides become more soluble going down the group
  • Radium hydroxide will therefore be more soluble than calcium hydroxide

• Answer 6:

  • The Group 2 sulfates become less soluble going down the group
  • Radium sulfate will therefore be less soluble than strontium sulfate

• Answer 7:

  • The general equation for the reaction of Group 2 oxides with dilute hydrochloric acid is:

XO (s) + 2HCl (aq) → XCl₂ (aq) + H₂O (l)

• where X is the Group 2 element

  • The reaction of radium oxide with dilute hydrochloric acid is therefore:

RaO (s) + 2HCl (aq) → RaCl₂ (aq) + H₂O (l)

• Answer 8:

  • Radium sulfate will be formed in this reaction
  • However, the solubility of Group 2 sulfates decreases going down the group
  • Therefore, a white precipitate of radium sulfate will be formed in this reaction