The necessary steps required to show the formation of \(\mathrm{CCl}_{4}\) by Lewis electron dot diagram have been jumbled. Arrange them in a sequence. (1) Thus, an electron pair is shared between \(\mathrm{C}\) and Cl. This is the Lewis electron dot diagram for \(\mathrm{CCl}_{4}\) (2) Write the symbol of chlorine and represent its valence electrons with the help of crosses, i.e., (3) Write the symbol of carbon and represent its valence electrons with the help of dots, i.e., - (4) When carbon combines with four chlorine atoms, the carbon atom contributes four electrons for sharing, whereas each chlorine atom contributes only one electron for sharing. Thus, both the atoms in \(\mathrm{CCl}_{4}\) attain an octet. (a) 1324 (b) 2134 (c) 4321 (d) 3241

When we talk about chemical bonding, we're referring to the force that holds atoms together in molecules or compounds. This force arises from the interactions between the electrons of one atom and the nucleus of another. In the context of the exercise involving the formation of carbon tetrachloride ((CCl_4)), the chemical bond in question is the covalent bond.

Covalent bonding occurs when pairs of electrons are shared by atoms. In the case of CCl_4, carbon shares its four valence electrons with four chlorine atoms, allowing each to reach a stable electron configuration. This shared pair of electrons constitutes a single bond between the carbon and each chlorine atom. Understanding the step-by-step formation of CCl_4 outlined in option D, showcases how individual covalent bonds form to result in a stable molecule.

Valence electrons play a crucial role in chemical bonding because they are the electrons that are involved in forming bonds. They are located in the outermost shell of an atom, and the number of valence electrons an atom has can determine its bonding capacity. In our example of CCl_4, carbon has four valence electrons, which are represented as dots in the Lewis electron dot diagram. Each chlorine atom has seven valence electrons, represented by crosses.

The complete transfer or sharing of these electrons leads to the formation of chemical bonds. In the exercise, the accurate representation of valence electrons is essential for visualizing and understanding how the carbon and chlorine atoms share electrons to create stable bonds, as seen in the correct sequence of steps.

The octet rule is a principle that atoms tend to combine in such a way that each atom has eight electrons in its valence shell, resulting in a stable electron configuration similar to that of noble gases. The CCl_4 molecule is a perfect example of the octet rule in action. Carbon, which only has four electrons in its outer shell, shares these electrons with four chlorine atoms, each contributing one electron. This equitable sharing allows all five atoms to reach an electron configuration that satisfies the octet rule.

As shown in the solution sequence, it is crucial to understand how atoms share electrons to form covalent bonds and fulfill the octet rule. Recognizing the significance of the octet rule assists in predicting the bonding patterns of atoms and the stability of the resulting molecules.