Question

A. Atoms can bond together in several different ways. Name three types of chemical bonding. Explain what happens to electrons in each type of bonding.
b. Why are the elements in the far right column of the periodic table nonreactive?

c. What type of element gains electrons in ionic bonding, and what type of charge will it create?

d. Why do nonmetals make poor electrical conductors?

Answer 1

Explanation:

a) Three types of chemical bondings:

• Ionic bonding: Complete transfer of electrons from an electropositive atom to an electronegative atom.
• Covalent bonding: Equal sharing of electrons between the atoms with less or zero electronegativity difference.
• Metallic bonding: The bonding between the conduction electrons(electron cloud of delocalised electrons) and positively charged metal ions

b) Those elements are named as Noble gases which inert in nature that is less reactive due to fully filled electronic configuration.

Their general electronic configuration is given by:

$ns^2np^6$

n = principle quantum number

c) In an ionic bonding, electrons are transferred to the electronegative atom from the electropositive atom.

Electronegative: An atom which gains an electrons.Negative charge carrying ion is formed.

Electropositive : An atom which looses electrons.Positive charge carrying ion is formed.

d) This because the band width between the conduction band and valence band is large due to which electrons will not able to jump from valence band to conduction band.This makes the non metal poor electrical conductors.

Answer 2

a) Ionic bonding - forms between ions of opposite charges

Metallic bonding - electrostatic interaction between positive ions and sea of unbounded electrons

Covalent  bonding - when both atoms share an electron.

b) They are called noble gases and nonreactive because they have full valence shell. They don't need more electrons.

c) Electrons are attracted by a more electronegative atoms.

d) Because they don't have sea of electrons that can migrate freely between atoms.