Question

Which of the following compounds contain (s) no covalent bond (s)?
KCl, PH^3, O^2,B^2H^6,H^2SO^4.

Answer 1

the answer is
KCl
since,
KCl → K⁺ +Cl⁻
here, K is metal and Cl is non-metal
Thus, K and Cl form ionic bonds, not covalent.

Here, K is Potassium and Cl is Chlorine

Answer 2

Answer: Option (a) is the correct answer.

Explanation:

A covalent bond is formed when there is sharing of electrons between the atoms. Whereas an ionic bond is formed by the transfer of electrons.

Potassium (K) has atomic number 19 and chlorine (Cl ) has atomic number 17. So, there is deficiency of one electron in Cl atom to complete its octet. Thus, K will transfer its one electron to the Cl atom. Thus, KCl will be an ionic compound as the bond formation is due to the transfer of electron.

Similarly, the atomic number of phosphorous (P) is 15 and atomic number of hydrogen (H) is 1. Thus, there will be sharing of electrons between $PH_3$ molecule. Hence, it is a covalent compound.

Atomic number of oxygen is 16. Thus, in order to complete the octet there will be sharing of electrons between $O_2$ molecule. Hence, it is a covalent compound.

Atomic number of boron (B) is 5 and atomic number of hydrogen (H) is 1. Thus, in order to complete the octet there will be sharing of electrons between $B_2H_6$ molecule.

In the same way, in order to complete the octet there will be sharing of electrons between the hydrogen and sulfate molecules. Hence, $H_2SO_4$ is also a covalent compound.

Thus, we can conclude that out of the given options KCl contains no covalent bond.