Molecular orbitals and bonding

Question 1

Skeletal formula points to remember

Answer 1

Functional group should be written in.
If nitrogen is bonded to a hydrogen draw that in.

Question 2

Sigma bonds

Answer 2

σ end on overlap of atomic orbitals - single bonds

Question 3

Pi bonds

Answer 3

π side on overlap of atomic orbitals - double bonds (or triple bonds)

Question 4

Molecular orbitals are ….. stable than atomic orbitals

Answer 4

More

Question 5

Molecular orbitals have …. energy compared to atomic orbitals

Answer 5

Less

Question 6

How do two 1s orbitals combine I.e. 2H to H2?

Answer 6

Two 1s spherical orbitals will turn into bead shape.

Question 7

What is an orbital?

Answer 7

The area which an electron can be found in.

Question 8

Hybridisation

Answer 8

When orbitals combine to form new identical degenerate hybrid orbitals.

Question 9

SP^3 hybrid

Answer 9

Mixing of three p orbitals and one s orbitals

Question 10

SP^2 hybrid

Answer 10

Mixing of two p orbitals and one s orbital

Question 11

SP hybrid

Answer 11

Mixing of one p orbital and one s orbital

Question 12

What are stronger sigma bonds or pi bonds?

Answer 12

Sigma bonds as end on overlap is more efficient

Question 13

Hybrid orbitals are…

Answer 13

Degenerate - equal energy

Question 14

How can bonding in ethane be described as?

Answer 14

SP^3 hybridisation and sigma bonds.

Question 15

How can bonding in ethene be described as?

Answer 15

SP^2 hybridisation and one pi bond and the rest sigma bonds.

Question 16

How can bonding in ethyne be described as?

Answer 16

SP hybridisation and two pi bonds and three sigma bonds

Question 17

What will determine the type of bonding present in a molecule?

Answer 17

Symmetry and position of bonding orbitals

Question 18

Pure covalent molecular bonding -

Answer 18

there is no or very little difference in electronegativity between the atoms involved in the bond the bonding orbital will be symmetrical around a point where the bonding electrons are predicted to be found. A fluorine molecule F2 would be an example of where this would be found.

Question 19

Polar covalent -

Answer 19

For example (Hδ+-Clδ‑) where there is a difference in electronegativity between the two atoms involved in the bond the bonding orbital will be asymmetrical with the bonding electrons more likely to found around chlorine due to it having a larger electronegativity.

Question 20

Ionic bonds

Answer 20

(Na+Cl‑) where the difference in electronegativity between the two atoms involved in the bond is large, the bonding orbital will be extremely asymmetrical and almost entirely around one of the atoms. In this case it would be around chlorine due to it having a larger electronegativity compared to sodium.