Asample of a compound analyzed in a chemistry laboratory consists of 5.34 g of carbon, 0.42 g of hydrogen, and 47.08 g of chlorine. what is the percent composition of this compound?

10.1 % Carbon, 0.8 % Hydrogen and 89.1 % Chlorine.

Explanation:

The total mass of the compound is 5.34 + 0.42 + 47.08 = 52.84 g.

The percentage of carbon is:   × 100  = 10.1 %

The percentage of hydrogen is:   × 100 = 0.8 %

The percentage if chlorine is:   × 100 = 89.1 %

the number of valence electrons for each molecule or ion is shown beneath the structure. remember hydrogen will not have more than two electrons. this hydrogen is part of a covalent bond (sharing two electrons). a double bond here would cause hydrogen to share four electrons with phosphorus.

metals are good conductor of electricity. it has free electrons on their surface. according to electron pool theory, each atom present in a metal crystal losses all of its valence electron and as a result a pool of free is form. these pool of electrons are free to move and   conduct electricity easily   while making metal as good conductor.

the correct answer is a. the ability of electrons to flow throughout the metal.

if it's not useful, feel free to report for mistake in answer.