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Group 2: ionisation energy and properties

Group 2: ionisation energy and properties

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Explainer Video

Tutor: Alexander

Summary

Group 2: ionisation energy and properties

In a nutshell

As you go down Group 222​ in the periodic table, the atomic radius and reactivity increase, whilst the ionisation energy and melting points decrease for Group 222​ metals. 


Chemistry; Inorganic chemistry and the periodic table; KS5 Year 12; Group 2: ionisation energy and properties



Electron configuration


Element

Atom

Ion

​BeBeBe​​
​1s22s21s^22s^21s22s2​​
1s21s^21s2​​
​MgMgMg​​
​1s22s22p63s21s^22s^22p^63s^21s22s22p63s2​​
1s22s22p61s^22s^22p^61s22s22p6​​
​CaCaCa​​
​1s22s22p63s23p64s21s^22s^22p^63s^23p^64s^21s22s22p63s23p64s2​​
​1s22s22p63s23p61s^22s^22p^63s^23p^61s22s22p63s23p6​​


As Group222​ elements react, they tend to lose their two outermost electrons and form 2+2+2+​ ions. 



Atomic radius

For Group 222​ elements the atomic radius decreases as you go down the group. This is because electron shells are added as you go down the group which causes an increase in radius.



​​First ionisation energy

For Group 222​ elements as you go down the group an extra electron shell is added. The inner shells shield the outer shell from the nucleus. This weakens the attraction of the outer electrons to the nucleus making them easier to remove. Thus, decreasing the first ionisation energy as you go down the group.



​​Reactivity

As you do down Group 222​, reactivity increases. This is due to the first ionisation energy decreasing as you go down the group. Since less energy is required to remove the outermost electrons as you go down the group, this means it's easier for the metals to react. Therefore reactivity of the Group 222​ metals increases down the group.



Melting points

Group 222​ metals have metallic structures with positive ions surrounded by delocalised electrons. Going down the group the metal ions get bigger, but the charge remains the same, 2+2+2+​. This means that charge density decreases resulting in a weaker attraction between atoms. This means less energy is required to separate the atoms. 



Group 2 and water

When Group 222​ elements react with water they are oxidised and their oxidation number changes from 000​ to +2+2+2​. This forms M2+M^{2+}M2+ ions. ​


Example

​Ca + 2H2O → Ca(OH)2 + H20 +2 Ca Ca2+ Ca\ +\ 2H_2O\ \rightarrow\ Ca(OH)_2\ +\ H_2\\0 \, \,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,+2 \,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\, \,\,\,\,\,\,\,\,\,\\Ca \,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,Ca^{2+}\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,Ca + 2H2​O → Ca(OH)2​ + H2​0+2CaCa2+​​


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Electron energy levels and ionisation

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Electron energy levels and ionisation

Ionisation energies

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Ionisation energies

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Group 2: ionisation energy and properties

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Group 2: ionisation energy and properties

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FAQs - Frequently Asked Questions

How does the reactivity change as you go down Group 2?

The reactivity increases down Group 2. This is due to lower ionisation energy which means less energy is required to cause the Group 2 metals to react.

How does the ionisation energy change as you go down Group 2?

As you go down Group 2 the ionisation energy decreases. This is due to the atomic radius and the shielding effect.

What sort of ions do Group 2 metals normally form?

Group 2 metals normally form 2+ ions in compounds (M^2+). Group 2 metals lose their two outermost electrons.

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