Ionic Bonding: Formation, Strength & Misconceptions

Solubility is influenced by a variety of factors, not just ionic charge. The solvent's ability to interact with the ions and the strength of the ionic bonds both play a role.

Melting points vary based on crystal structure, ion size, and ion charge. Not all ionic compounds have uniformly high melting points.

The relative sizes of ions dictate how they pack together in a crystal lattice. This arrangement influences the crystal's properties, like its stability and density.

<p>Cations are smaller because they lose electrons and anions are larger because they gain electrons. Therefore, they do not maintain the same size.</p> Signup and view all the answers

<p>Ions may exhibit slight distortions due to factors like polarization effects and the electron distribution around the ion core.</p> Signup and view all the answers

<p>Ionic bond strength varies. Factors like ion size, charge, and lattice geometry influence the strength of the bond.</p> Signup and view all the answers

<p>When the thermal energy overcomes the electrostatic interactions, making the compound liquid or gaseous.</p> Signup and view all the answers

<p>Some metal-metal compounds exhibit aspects of ionic bonding. For instance, transition metal compounds with significant electronegativity differences between metallic components can exhibit ionic characteristics.</p> Signup and view all the answers

<p>Not all ions are single atoms; polyatomic ions consist of multiple atoms covalently bonded with a net charge. An example is sulfate ($SO_4^{2-}$).</p> Signup and view all the answers

<p>Ionic compounds are electrolytes because they dissociate into ions when dissolved, allowing the solution to conduct electricity. It's the ability to break apart into ions, not just bond strength, that matters.</p> Signup and view all the answers

<p>Smaller ions with higher charges generally result in stronger ionic bonds. This is because they create a greater concentration of charge and a shorter distance between ions, according to Coulomb's law.</p> Signup and view all the answers

<p>The melting points differ due to variations in ionic charge and size. $MgO$ has a higher melting point than $NaCl$ because $Mg^{2+}$ and $O^{2-}$ ions have greater charges than $Na^+$ and $Cl^-$ , resulting in stronger electrostatic forces.</p> Signup and view all the answers

<p>The statement is inaccurate. Ionic bonds are formed through the complete transfer of electrons from one atom to another, not through sharing. This creates oppositely charged ions that are attracted via electrostatic forces.</p> Signup and view all the answers

Solubility of ionic compounds depends on ionic bond strength and solvation ability of the solvent.

The attraction between an ion and polar molecules, crucial for solubility in polar solvents.

The energy required to separate ions in an ionic solid, impacting melting point and solubility.

Melting points vary based on crystal structure, ion size, and ion charge, not just ionic nature.

Cations are generally smaller than their neutral atoms; anions are larger due to electron gain.

Electrostatic attraction between oppositely charged ions formed by electron transfer.

Atoms gain or lose electrons to achieve a stable electron configuration resembling noble gases.

Ionic bond strength varies based on ion size, charge, and lattice geometry.

Not all ionic compounds are solids; some can be liquids or gases due to thermal energy.

Ionic bonds can form between metals under certain conditions, especially with high electronegativity differences.

Ions can be monatomic (like Na⁺) or polyatomic (like SO₄²⁻) with multiple atoms.

Substances that dissociate into ions in solution, enabling electric conduction.

Ionic compounds break apart into ions in water or when melted, not due to bond strength.