Question

Determine whether each of the following has the same number of bonding electrons as the sulfur dioxide molecule, \(\mathrm{SO}_{2}\). (a) \(\mathrm{NO}_{2}^{-}\) (c) \(\mathrm{CO}_{2}\) (e) \(\mathrm{N}_{2}\) (b) \(\mathrm{OF}_{2}\) (d) \(\mathrm{O}_{3}\)

Short answer

(a) NO2- does not have the same amount of bonding electrons as SO2. (c) CO2 has more bonding electrons than SO2. (e) N2 has more bonding electrons than SO2. (b) OF2 does not have the same amount of bonding electrons as SO2. (d) O3 does not have the same number of bonding electrons as SO2

Step-by-step solution

Analyse SO2

First, Draw the Lewis structure for SO2. Each oxygen atom provides 6 electrons, and Sulfur gives 6 as well. Two oxygens share a pair of electrons with sulfur to form two double bonds, S=O. Each sulfur dioxide (SO2) molecule has 4 bonding electrons (two per each double bond between Sulfur and Oxygen).

Analyse NO2-

Draw the Lewis structure for NO2-. Nitrogen atom provides 5 electrons and each oxygen provides 6, one of these oxygens shares a pair of electrons with nitrogen to form a double bond. The other shares just one electron forming a single bond. Hence, each nitrite ion NO2- has 3 bonding electrons.

Analyse CO2

Draw the Lewis structure for CO2. Each oxygen atom provides 6 electrons, and Carbon gives 4 electrons in total. The carbon atom shares 4 electrons with each of the two oxygen atoms to form 4 double bonds in total. Therefore, CO2 atom has 8 bonding electrons.

Analyse N2

Draw the Lewis structure for N2. Each nitrogen atoms provide 5 electrons, they share three pairs of electrons to form triple bond. Hence, each nitrogen molecule has 6 bonding electrons.

Analyse OF2

Draw the Lewis structure for OF2. Oxygen atom provides 6 electrons, each Fluorine gives 7. The oxygen atom shares a pair of electrons with each of the two fluorine atoms to form two single bonds, Yeah each OF2 molecule has 2 bonding electrons.

Analyse O3

Draw the Lewis structure for O3. Each oxygen atom provides 6 electrons. Two of the oxygen atoms share a pair of electrons to form a double bond while the third forms a single bond with another oxygen atom. Hence, each O3 molecule has 3 bonding electrons.

Key concepts

Lewis Structure

The Lewis Structure is a visual representation in chemistry that shows how atoms bond within a molecule by illustrating bonds with lines and electrons as dots. It helps in identifying how the electrons in an atom are shared or transferred when forming chemical bonds. This representation helps in understanding the types of bonds in the molecule, such as single, double, or triple bonds.

• Atoms are surrounded by valence electrons drawn as dots.
• Bonds between atoms are shown as lines.
• It follows the octet rule, where atoms tend to complete their outer shell with eight electrons.

Overall, Lewis structures allow us to visualize how atoms in a molecule share electrons, contributing to the stability and the structure of the compound.

Sulfur Dioxide

Sulfur Dioxide, with the chemical formula \(SO_2\), is a gas with a pungent smell. In its Lewis Structure, the sulfur atom shares electrons with two oxygen atoms. Both bonds between sulfur and oxygen are double bonds.

• Each bond consists of two electron pairs, or four electrons in total, known as bonding electrons.
• This arrangement respects the octet rule for both sulfur and oxygen atoms.

The formation of \(SO_2\) involves sharing four pairs of electrons, highlighting the concept of electron sharing and making bonds between all the involved atoms stronger and more stable.

Chemical Bonds

Chemical bonds are the attractive forces that hold atoms together in compounds. They are crucial for the formation of chemical compounds including molecules like \(SO_2\). Types of chemical bonds in molecules can include single, double, and triple covalent bonds.

• Covalent Bonds: Atoms share electron pairs to attain stability.
• Ionic Bonds: Atoms transfer electrons resulting in charged ions that attract each other.
• Metallic Bonds: Electrons are shared among a lattice of atoms in metals.

The nature of a chemical bond, such as whether it is single, double, or triple, dictates the stability and properties of the compound. Double bonds, like those in \(SO_2\), involve more electron sharing and are generally more rigid than single bonds.

Electron Sharing

Electron Sharing is a fundamental aspect of covalent bonding, where two atoms share one or more pairs of electrons to attain stable electron configurations similar to noble gases. This process can be represented visually through the Lewis Structure.

• Shared electrons contribute to the fulfillment of the octet rule.
• The type of sharing (single, double, or triple bond) affects bond length and bond strength.
• For \(SO_2\), sulfur shares electrons with oxygen to form double bonds, involving substantial electron sharing.

Understanding electron sharing helps us grasp how compounds like \(SO_2\) achieve their three-dimensional structure and chemical behavior. This concept underpins the molecular geometry and the physical and chemical properties of compounds.