Question

Statement 1: Ionic bonds are always stronger than covalent bonds
Statement 2: They only break when bombarded with electrons.
A.Statement 1 is true; Statement 2 is true and Statement 2is the correct explanation of Statement 1
B.Statement 1 is true; Statement 2 is true but Statement 2is not the correct explanation of Statement 1
C.Statement 1 is true, Statement 2 is false
D.Statement 1 is false, Statement 2 is true

Answer 1

To answer this question you should recall the concept of bonding in ionic bonds and covalent bonds. Chemical Bonding is a process where there is a formation of a bond between two or more atoms, molecules, or ions to give rise to a new chemical compound. Ionic bonds are formed by donating or accepting electrons, while covalent bonds are formed on sharing of electrons.

Complete step by step answer:
-Ionic bonding refers to that type of chemical bonding where there is a transfer of electrons from one atom or molecule to another. There exist electrostatic forces of attraction between the charged particles. More the charge disparity between the cation and the anion, the stronger the ionic bond.
-In the other type of bond known as a covalent bond, there is a sharing of electrons between atoms. Ionic bonds are stronger than covalent bonds as ionic bonds are formed by complete charge transfer, so a coulombic interaction.
-Ionic bonds can be broken by supplying high enough energy to the bonds to break the electrostatic interaction between them. It can be in the form of electrons, heat etc. Thus, statement 2 is false.

Hence C is the correct answer.

Note:
In ideal cases, it can be said that any bond is hundred percent ionic or covalent. But in reality, any bond shows partial ionic and covalent character. The components of any molecular: the cations polarize the anions and try to pull the electronic charge towards themselves and this increases the electric charge between the two ions. This is the case with a covalent bond, that is an electron charge density is built up around the nuclei. Fajan’s rule is based on the fact that:
1.Smaller the size of cation, more large the size of the anion will result in a more covalent character of the ionic bond.
2.More the charge density of cation, greater is the covalent character of the ionic bond.
3.Electronic configuration: For cations with same charge and size, the one, with $\left( {n - 1} \right){d^{n\;}}n{s^o}\;$which is found in transition elements have greater covalent character than the cation with $n{s^{2\;}}n{p^6}\;$electronic configuration, generally present s- block elements.