What are the reactions of Group 2 elements?

(i) The Reactions of Group 2 Elements with Oxygen. All Group 2 elements tarnish in air to form a coating of the metal oxide. They react violently in pure oxygen producing a white ionic oxide. When these metals (M) are heated in oxygen they burn vigorously to produce a white ionic oxide, M2+O2-.

What is the trend in reactivity in group 2?

The reactivity of the group 2 elements increase as you go down the group. This is because, as explained previously, it is much easier to remove an outer shell electron as you go further down the group (lower ionisation energies).

What happens when Group 2 elements react with acids?

Reactions of the Group 2 elements with acids. This page looks at the reactions of the Group 2 elements – beryllium, magnesium, calcium, strontium and barium – with common acids. All the metals react with dilute hydrochloric acid to give bubbles of hydrogen and a colourless solution of the metal chloride.

Why does the reactivity of Group 2 elements increase?

The first electron to react will be on the outer shell. The reactivity increases down the group from Mg to Ba. This is because the further away an electron is from the nucleus, the weaker its attraction and the more likely it is to react with another atom.

What are the chemical properties of Group 2 elements?

Group 2: Chemical Properties

relatively reactive, but less than high reactive alkali metals.
form halides when reacted with halogens.
form oxides when reacting with air, leading to a dull appearance in pure form.
form 2+ charge in cationic form.
form ionic bonds with other negatively charged ionic forms of elements.

Why does reactivity increase down group 2 A level chemistry?

As you progress down Group 2, the reactivity increases. This is due to a decrease in ionisation energy as you progress down the group. As it requires less energy to form the ions, the reactivity increases.

Does the reactivity of group 2 appear to increase or decrease as you go down the column explain this in terms of ionization energies of the metals?

As you go down group 2 from top to bottom, the value of first ionisation energy decreases, it is progressively easier to remove the first valence electron. As you go down group 2 from top to bottom, the value of the second ionisation energy decreases, it is progressively easier to remove the second valence electron.

What happens when metals react with concentrated acids?

When a metal reacts with an acid, the metal usually reduces hydrogen ions to hydrogen gas. The elemental metal is oxidized to metal cations in the process. However, nitrate ions are easily reduced to nitrogen monoxide and nitrogen dioxide.

What is produced when a metal reacts with an acid?

Acids react with most metals and, when they do, a salt is produced. But unlike the reaction between acids and bases, we do not get water. Instead we get hydrogen gas. It doesn’t matter which metal or which acid is used, if there is a reaction we always get hydrogen gas as well as the salt.

How does the reactivity change in group 2?

Reactivity. Reactivity of Group II elements increases down the group. This can be explained by the increase in ease at losing two outer electrons as we descend the group. The loss of electrons becomes easier due to the decreasing ionisation energy required.

Why does the reactivity of the elements increase as we go down the group?

Explaining trends The reactivity of Group 1 elements increases as you go down the group because: the outer electron gets further from the nucleus as you go down the group. the attraction between the nucleus and outer electron gets weaker as you go down the group – so the electron is more easily lost.

This page looks at the reactions of the Group 2 elements – beryllium, magnesium, calcium, strontium and barium – with common acids. Reactions with dilute hydrochloric acid. All the metals react with dilute hydrochloric acid to give bubbles of hydrogen and a colourless solution of the metal chloride.

Why are reactions easier as you go down a group?

The reactions become easier as the energy needed to form positive ions falls. This is mainly due to a decrease in ionisation energy as you go down the Group. This leads to lower activation energies, and therefore faster reactions. Questions to test your understanding

How does beryllium react with other Group 2 metals?

The other hydroxides of the Group 2 metals are all basic. They react with acids to form salts. For example: Calcium hydroxide reacts with dilute hydrochloric acid to give calcium chloride and water. Beryllium hydroxide Beryllium hydroxide reacts with acids, forming solutions of beryllium salts.

Can a metal in a group react with oxygen?

“X” in the equation can represent any of the metals in the Group. It is almost impossible to find any trend in the way the metals react with oxygen. It would be quite untrue to say that they burn more vigorously as you go down the Group.