Question

The bonds present in \(\mathrm{N}_{2} \mathrm{O}_{5}\) are (a) only ionic (b) covalent and coordinate (c) only covalent (d) covalent and ionic

Short answer

(c) only covalent

Step-by-step solution

Analyze the Compound Structure

First, we need to understand the structure of \( \mathrm{N}_2\mathrm{O}_5 \). This compound is called dinitrogen pentoxide. It consists of two nitrogen atoms and five oxygen atoms.

Identify Bond Types in the Compound

In \( \mathrm{N}_2\mathrm{O}_5 \), the nitrogen and oxygen atoms form covalent bonds. There is no presence of metal and non-metal combo to suggest ionic bonds, nor any indication of unshared pairs suggesting coordinate bonds.

Determine Presence of Coordinate Bonds

Consider whether any coordinate or dative bonds exist. Coordinate bonds occur when one atom provides both electrons for a bond. In \( \mathrm{N}_2\mathrm{O}_5 \), no such bond is evident since all bonds are symmetric with shared electrons.

Conclude the Bond Type

Since no metal-ion interaction or coordinate bonding is present, the compound comprises only covalent bonds. The structure confirms all electron sharing occurs between atoms without donation from a single atom.

Key concepts

Covalent Bonds

Covalent bonds are formed when two non-metal atoms share valence electrons to achieve a stable electron configuration. This sharing allows the atoms to "hold hands" through the electrons. In a covalent bond, each atom contributes at least one electron to the shared pair, but they don't have to contribute equally.
Covalent bonds can be polar or non-polar, depending on the electronegativity difference between the atoms involved. A polar covalent bond occurs when the electron sharing is unequal, causing a partial charge. Non-polar covalent bonds have equal sharing of electrons, typically found in molecules like \(\text{O}_2\).
Examples of covalent compounds include water (\(\text{H}_2\text{O}\)), carbon dioxide (\(\text{CO}_2\)), and methane (\(\text{CH}_4\)).

• Nature of Bond: Non-metal to non-metal.
• Strength: Determined by shared electrons, with multiple bonds being stronger than single bonds.
• Examples: Found in organic molecules and many gases.

Coordinate Bonds

Also known as dative bonds, coordinate bonds are a special type of covalent bond where one atom provides both electrons for the bond. This happens when a lone pair from one atom fills up an empty orbital of another atom.
In typical covalent bonds, each atom shares its electrons. However, in coordinate bonds, one atom acts as a donor and the other as an acceptor. Despite this difference in origin, once formed, coordinate bonds exhibit similar properties to regular covalent bonds.
An example of a coordinate bond is found in the ammonium ion \(\text{NH}_4^+\), where nitrogen shares a lone pair with a proton to form the ion.

• Nature of Bond: One atom provides both electrons.
• Examples: Common in complex ions and certain coordination compounds.
• Visual Representation: Often represented with an arrow indicating electron donation.

Ionic Bonds

Ionic bonds form through the complete transfer of electrons between atoms, usually between a metal and a non-metal. This transfer results in the formation of charged ions: positively charged cations and negatively charged anions.
The electrostatic attraction between these oppositely charged ions holds the compound together. Ionic bonds typically form crystalline structures and have high melting and boiling points.
An example of an ionic compound is sodium chloride (\(\text{NaCl}\)), where sodium donates its outer electron to chlorine, forming \(\text{Na}^+\) and \(\text{Cl}^-\).

• Nature of Bond: Metal donates, non-metal accepts electrons.
• Strength: Strong due to electrostatic attraction.
• Examples: Salts, minerals, and some ceramics.