Explanation: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.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 nitratescompounds 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 nitratesMost nitrates tend to decompose on heating to give the metal oxide, brown FUMES of nitrogen dioxide, and oxygen.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 nitratesMost 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: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 nitratesMost 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.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 nitratesMost 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.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 nitratesMost 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.