A tetrahedral carbon is hybridized while a linear carbon is hybridized. Two different compounds that have the same molecular formula are known as . Pi (π) bonds are generally than sigma (σ) bonds. Hybridization is the combination of two or more orbitals to form the same number of orbitals, each having the same shape and energy. A bond is formed by side-by-side overlap of two p orbitals. The is a measure of an atom’s attraction for electrons in a bond and indicates how much a particular atom "wants" electrons. Two Lewis structures that have the same atomic placement and σ structure but a different arrangement of π electrons are called . All single bonds are bonds.

1. Sp^3; Sp.

2. Isomers.

3. Weaker.

4. Atomic; hybrid.

5. Pi.

6. Electronegativity.

7. Resonance structures.

8. Sigma.

Explanation:

1. A tetrahedral carbon is Sp^3 hybridized while a linear carbon is Sp hybridized. A tetrahedral carbon typically comprises of four bonds that are 109. 5° apart while a linear carbon atom comprises of two (2) bonds that are 180° apart.

2. Two different compounds that have the same molecular formula are known as isomer. For example Butane and Isobutane, Methoxyethane and Propanol have the same molecular formula (numbers of hydrogen and carbon atoms) but different structural formula.

3. Pi (π) bonds are generally weaker than sigma (σ) bonds. This is because the orbital paths of Pi bonds are parallel thereby causing an overlap.

4. Hybridization is the combination of two or more atomic orbitals to form the same number of hybrid orbitals, each having the same shape and energy.

5. A Pi bond is formed by side-by-side overlap of two p orbitals.

6. The electronegativity is a measure of an atom’s attraction for electrons in a bond and indicates how much a particular atom "wants" electrons.

7. Two Lewis structures that have the same atomic placement and σ structure but a different arrangement of π electrons are called resonance structures.

8. All single bonds are Sigma bonds.