Why does calcium nitrate decompose in a similar way to magnesium nitrate, but require a higher temperature for decomposition?
Calcium ions (Ca2+) have the same charge as magnesium ions (Mg2+) but Ca2+ ions have a larger ionic radius (as ionic radius increases down the group). This means Ca2+ has a lower charge density than Mg2+. With a lower charge density, Ca2+ ions cause less polarisation and distortion of the nitrate (NO3-) electron cloud (and N-O/N=O bonds) than Mg2+ions making decomposition harder. Therefore, calcium nitrate requires more heat to be decomposed.
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