Question

a metal above sodium whose nitrate decomposes to give metal nitrite and oxygen​

Answer 1

Explanation:

caesium

The rest of the Group, however, don't decompose so completely (at least not at Bunsen temperatures) - producing the metal nitrite and oxygen, but no nitrogen dioxide. All the nitrates from sodium to caesium decompose in this same way, the only difference being how hot they have to be to undergo the reaction.

Answer 2

Answer:

Most nitrates tend to decompose on heating to give the metal oxide, brown fumes of nitrogen dioxide, and oxygen. For example, a typical Group 2 nitrate like magnesium nitrate decomposes like this: In Group 1, lithium nitrate behaves in the same way - producing lithium oxide, nitrogen dioxide and oxygen.

Explanation:

SOME COMPOUNDS OF THE GROUP 1 ELEMENTS

This page looks at some compounds of the Group 1 elements (lithium, sodium, potassium, rubidium and caesium) - limited to various bits and pieces required by various UK A level syllabuses. You will find some information about the nitrates, carbonates, hydrogencarbonates and hydrides of the metals.

We will first look at what happens to some of the compounds on heating, and then their solubility. At the end, you will find a section about the preparation and reactions of the metal hydrides.

The effect of heat on Group 1 compounds

The facts

Group 1 compounds are more stable to heat than the corresponding compounds in Group 2. You will often find that the lithium compounds behave similarly to Group 2 compounds, but the rest of Group 1 are in some way different.

Heating the nitrates

Most nitrates tend to decompose on heating to give the metal oxide, brown fumes of nitrogen dioxide, and oxygen.

For example, a typical Group 2 nitrate like magnesium nitrate decomposes like this:

In Group 1, lithium nitrate behaves in the same way - producing lithium oxide, nitrogen dioxide and oxygen.

The rest of the Group, however, don't decompose so completely (at least not at Bunsen temperatures) - producing the metal nitrite and oxygen, but no nitrogen dioxide.

All the nitrates from sodium to caesium decompose in this same way, the only difference being how hot they have to be to undergo the reaction. As you go down the Group, the decomposition gets more difficult, and you have to use higher temperatures

Note: The more modern name for sodium nitrite is sodium nitrate(III). On this basis, sodium nitrate should properly be called sodium nitrate(V). Most people still call nitrates and nitrites by the older names.

Heating the carbonates

Most carbonates tend to decompose on heating to give the metal oxide and carbon dioxde.

For example, a typical Group 2 carbonate like calcium carbonate decomposes like this:

In Group 1, lithium carbonate behaves in the same way - producing lithium oxide and carbon dioxide.

The rest of the Group 1 carbonates don't decompose at Bunsen temperatures, although at higher temperatures they will. The decomposition temperatures again increase as you go down the Group.