# Effects of electronegativity on the bonding on an ionic compound? AgBr

• 3vo
In summary, the difference in electronegativity between silver and bromine leads to the polarisation of the bond in AgBr, resulting in the formation of an ionic compound.
3vo

## Homework Statement

Use the concepts of electronegativity and polarisation to interpret the bonding in AgBr

## Homework Equations

I have always understood electronegativity as the ability of an atom in a molecule to attract a pair of shared electrons towards itself. So this would usually have to be a covalent bond, as electrons would need to shared.

I understand that differences in electronegativity can cause polarization in a covalent molecule, forming a dipole due to the uneven distribution of the shared electrons within the bond. (BTW would this be known as a polarised covalent bond?)

But what impact could electronegativity have on an ionic compound? After all, ionic bonding involves electrons being transferred from a cation to an anion (and does not involve sharing).

Could someone please explain to me how electronegativity could effect the bonding within an ionic compound and what effect it would have on a compound such as AgBr?

The AnswerElectronegativity is an important concept in understanding the bonding in AgBr. The difference in electronegativity between silver (1.93) and bromine (2.96) creates a large disparity in how strongly each atom will attract the electrons of the bond. This creates a partially ionic bond, where the electrons are not shared equally between the two atoms, but rather are more heavily attracted to the bromine atom. This results in an unequal charge distribution in the molecule, making it polarised. This polarization of the bond gives rise to the formation of an electrostatic attraction between the positive and negative end of the molecule, resulting in the stable compound that we know as AgBr.

## 1. How does electronegativity affect the bonding in an ionic compound?

The difference in electronegativity between two atoms in an ionic compound determines the type of bonding that occurs. If the difference is large, the bond will be more ionic, with one atom gaining electrons and the other losing them. If the difference is small, the bond will be more covalent, with the electrons being shared more equally.

## 2. What is the electronegativity of AgBr?

The electronegativity of silver (Ag) is 1.93 and the electronegativity of bromine (Br) is 2.96. This results in a large electronegativity difference of 1.03, indicating that the bonding in AgBr is more ionic in nature.

## 3. How does the electronegativity difference in AgBr affect its properties?

The large electronegativity difference in AgBr results in a strong ionic bond, giving the compound a high melting and boiling point. It also makes AgBr a good conductor of electricity in its molten or dissolved state, but not in its solid form.

## 4. Can the bonding in AgBr be classified as purely ionic or purely covalent?

The bonding in AgBr cannot be classified as purely ionic or purely covalent. While the electronegativity difference indicates a more ionic bond, there is still some degree of electron sharing between the silver and bromine atoms. This makes the bonding in AgBr a mix of both ionic and covalent characteristics.

## 5. How does electronegativity affect the lattice structure of AgBr?

The strong ionic bond in AgBr results in a crystal lattice structure, with alternating layers of positively charged silver ions and negatively charged bromide ions. The size of the ions and the strength of the bond are also affected by electronegativity, resulting in a specific arrangement of ions in the crystal lattice.

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