Draw The Lewis Dot Structures Of N2 And CCl4

Which of the following correctly represents the Lewis dot structures of N2 and CCl4?

a) N≡N and Cl:Cl:Cl:Cl

b) N:N and Cl≡Cl

c) N≡N and C≡Cl4

d) N:N and CCl4

Correct Answer: a) N≡N and Cl:Cl:Cl:Cl

Explanation:

Lewis dot structures are diagrams that show the bonding between atoms of a molecule and the lone pairs of electrons that may exist in the molecule. These diagrams use dots and lines to represent the valence electrons of atoms and the bonds between them. Let's look at the Lewis dot structures of N2 and CCl4.

Lewis dot structure of N2:

Nitrogen is in Group 5A and has five valence electrons. When two nitrogen atoms come together to form N2, they share their valence electrons to form a triple bond. The Lewis dot structure of N2 is:

N ≡ N

Each nitrogen atom has a full outer shell with three shared pairs of electrons and one lone pair of electrons. The triple bond between the nitrogen atoms is represented by three lines (≡) instead of the usual two lines for a double bond.

Lewis dot structure of CCl4:

Carbon is in Group 4A and has four valence electrons. Chlorine is in Group 7A and has seven valence electrons. When one carbon atom bonds with four chlorine atoms, the Lewis dot structure of CCl4 is:

Cl:Cl:Cl:Cl

|

C

Each chlorine atom has a full outer shell with one shared pair of electrons and three lone pairs of electrons. The carbon atom also has a full outer shell with four shared pairs of electrons. The four single bonds between the carbon and chlorine atoms are represented by lines (|).

Therefore, the correct answer is a) N≡N and Cl:Cl:Cl:Cl. Option b) N:N and Cl≡Cl is incorrect because it incorrectly represents the bonding in both molecules. Option c) N≡N and C≡Cl4 is incorrect because it incorrectly represents the bonding in CCl4. Option d) N:N and CCl4 is incorrect because it incorrectly represents the bonding in N2.

Lewis dot structures are a useful tool in understanding the bonding in molecules. By drawing these diagrams, we can see the arrangement of electrons around each atom and determine the overall structure and properties of the molecule.

It is important to note that the Lewis dot structures only represent the valence electrons of the atoms in a molecule. These are the outermost electrons that are involved in bonding and determine the reactivity and chemical behavior of the molecule. The Lewis dot structures do not show the inner core electrons, which are not involved in bonding and do not participate in chemical reactions.

In addition, Lewis dot structures do not always accurately represent the true three-dimensional structure of a molecule. In some cases, the atoms may be arranged in a way that deviates from the predicted structure based on the Lewis dot structure. This is due to factors such as the repulsion between electron pairs and the presence of lone pairs of electrons.

Overall, understanding Lewis dot structures is an important aspect of studying chemistry, as it allows us to better understand the bonding and properties of molecules.