Question

Why does Calcium float in water?

Answer 1

Because of the enormous size of the $C{a^{2 + }}$ particle, high coordination numbers are normal, up to 24 in some intermetallic mixes, for example, $CaZn13$ . Calcium is promptly complexed by oxygen chelates, for example, $EDTA$ and polyphosphates, which are valuable in insightful science and eliminating calcium particles from hard water.

Complete answer:
Calcium is an exceptionally bendable brilliant metal (some of the time portrayed as light yellow) whose properties are fundamentally the same as the heavier components in its gathering, strontium, barium, and radium. Like different components set in gathering 2 of the intermittent table, calcium has two valence electrons in the peripheral s-orbital, which are handily lost in compound responses to frame a dipositive particle with the steady electron arrangement of an honorable gas, for this situation argon.
The reaction of calcium with water is less rough. In this way, the warmth delivered isn't adequate for the hydrogen to burst into flames. Calcium begins skimming in light of the fact that the air pockets of hydrogen gas which are shaped during the reaction adhere to the outside of the metal and henceforth calcium coasts on water.
The reaction of calcium with water is less violent. The reaction is as per the following:
$C{a_{(s)}} + 2{H_2}{O_{(l)}} \to Ca{(OH)_2}_{(aq)} + {H_{2(g)}}$
Since the reaction is less violent, the warmth delivered isn't adequate for the hydrogen to burst into flames. Calcium begins to coast as the air pockets of hydrogen gas which are framed during the reaction adhere to the outside of the metal and thus calcium glides on a superficial level.
The calcium is a component which is found in the bones and teeth of humans and creatures. The calcium responds with water with freedom of less measure of warmth energy. The warmth delivered isn't sufficient for the hydrogen in water to burst into flames. The calcium starts to coast in light of the fact that the air pockets in the hydrogen gas makes it drift over the outside of water as it is less dense than water.

Note:
Other than the simple oxide $CaO$, the peroxide $Ca{O_2}$ can be made by direct oxidation of calcium metal under a high tension of oxygen, and there is some proof for a yellow superoxide $Ca{({O_2})_2}$. Calcium hydroxide, is a solid base, however it isn't as solid as the hydroxides of strontium, barium or the soluble base metals. Each of the four dihalides of calcium are known. Calcium carbonate and calcium sulfate are especially plentiful minerals. Like strontium and barium, just as the salt metals and the divalent lanthanides europium and ytterbium, calcium metal breaks up straightforwardly in fluid alkali to give a dim blue arrangement.