1.3 Bonding

Question 1

Give example of octahedral molecule

Answer 1

SF6

Question 2

Give example of trigonal planar molecule

Answer 2

BF3

Question 3

Give example of linear molecule

Answer 3

CO2

Question 4

What is the bond angle of an octahedral molecule?

Answer 4

90*

Question 5

What is the bond angle of a trigonal planar molecule?

Answer 5

120*

Question 6

What is the bond angle of a linear molecule?

Answer 6

180*

Question 7

What do the molecules: CO2, BF3 and SF6, all have in common?

Answer 7

Molecules with multiple bonds, to form one shape within molecule.

Question 8

What the molecules: CH4, H2O and NH3, all have in common?

Answer 8

They are all molecules with for electron pairs (so all electrons in the outer most shell are paired and currently, repelling one another).

Question 9

Give an example of a tetrahedral molecule

Answer 9

CH4

Question 10

Give an example of a pyramidal molecule

Answer 10

NH3

Question 11

Give an example of a non-linear molecule

Answer 11

H2O

Question 12

What is the bond angle of a tetrahedral molecule?

Answer 12

109.5*

Question 13

What is the bond angle of a pyramidal molecule?

Answer 13

107*

Question 14

What is the bond angle of a non-linear molecule?

Answer 14

104.5*

Question 15

Explain electron-pair repulsion theory (1)

Answer 15

Electron pairs in the outer most shell of an atom or ion determines the shape.

Question 16

Explain electron-pair repulsion theory (2).

Answer 16

• Electron pairs in the outer most shell of an atom or ion determines the shape.
• An electron has a negative charge. And like charges repel one another.

Question 17

Explain electron-repulsion theory (3).

Answer 17

• Electron pairs in the outer most shell of an atom or ion determines the shape.
• An electron has a negative charge. And like charges repel one another.
• Electron pairs repel each other as far as possible, but lone pairs repel more. This repulsion in covalently bonded molecules forms the shapes molecules take.