In each of the following sets, specify the one compound that...

In each of the following sets, specify the one compound that is likely to have completely ionic bonds in its solid state. $\begin{array}{llll}\text { (a) } \mathrm{CCl}_{4} & \mathrm{HCl} & \mathrm{NaAt} & \mathrm{K}_{2}\end{array}$ (b) $\mathrm{CS}_{2}$ $\begin{array}{llll}\mathrm{CsF} & \mathrm{HF} & \mathrm{XeF}_{2} & \mathrm{BF}_{3}\end{array}$

In each of the following sets, specify the one compound that is likely to have completely ionic bonds in its solid state.
$\begin{array}{llll}\text { (a) } \mathrm{CCl}_{4} & \mathrm{HCl} & \mathrm{NaAt} & \mathrm{K}_{2}\end{array}$
(b) $\mathrm{CS}_{2}$
$\begin{array}{llll}\mathrm{CsF} & \mathrm{HF} & \mathrm{XeF}_{2} & \mathrm{BF}_{3}\end{array}$

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Key Concepts

Crystal Lattice Structure

Ionic compounds in the solid state form well-organized, repeating three-dimensional structures known as crystal lattices. This arrangement maximizes the attractive interactions between oppositely charged ions while minimizing repulsive forces, contributing to the high melting and boiling points typical of ionic solids.

Lattice Energy

Lattice energy is the energy released when ions in the gas phase come together to form an ionic solid. It is a measure of the strength of the ionic bonds and reflects the stability of the crystalline structure in the solid state.

Ionic Bonding

Ionic bonding involves the complete transfer of electrons from one atom to another, resulting in the formation of positively charged cations and negatively charged anions. These oppositely charged ions attract each other strongly via electrostatic forces, which is the primary reason for the formation of ionic compounds.

Electronegativity Difference

A significant difference in electronegativity between two atoms tends to favor the transfer of electrons over sharing, thus leading to the formation of ionic rather than covalent bonds. This concept is crucial in predicting whether a bond in a compound is predominantly ionic.

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