1. In an ionic compound, the size of the ions affects the internuclear distance

Question

1. In an ionic compound, the size of the ions affects the internuclear distance (the distance between the centers of adjacent ions), which affects lattice energy (a measure of the attractive force holding those ions together). Based on ion sizes, rank these compounds of their expected lattice energy.

Note: Many sources define lattice energies as negative values. Please rank by magnitude and ignore the sign. |Lattice energy| = absolute value of the lattice energy.

CsF, CsCl, CsBr, and CsI

2. The charges and sizes of the ions in an ionic compound affect the strength of the electrostatic attraction holding that compound together. Based on ion charges and relative ion sizes, rank these ionic compounds by their expected melting points.

MgO, MgF2, NaF, and KBr

3. Classify these bonds as ionic, polar covalent, or nonpolar covalent: C-C, Li-Cl, and S-O

Explanation / Answer

Solution :-

Q1 solution

Ranking for the lattice energy for the halides of the Cs is as follows

CsF > CsCl> CsBr>CsI

CsF has greatest lattice energy because the F is the most electronegative atom and CsI has lowest lattice energy because Iodine is the least electronegative atom also the size of the F is smallest and size of the I is largest.

Q 2 solution

the order of the melting point for the ionic compound is as follows

MgO > MgF2 > NaF >KBr

Because the MgO bond is the strongest bond and the KBr bond is the weakest bond.

Q3 Solution

Bond formed by the metal and non metal element is ionic bond and bond formed by the non metal and non metal element is covalent bond

C-C bond is the covalent bond because its non metal – non metal bond

Li-Cl bond is the ionic bond because its metal – non metal bond

S-O is covalent bond because its non metal – non metal bond

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