Question 1b
State the type of bonding in potassium chloride which melts at 1043 K.
Question 1c
Describe the structure and bonding in solid magnesium oxide.
Question 1d
Outline why solid magnesium chloride does not conduct electricity.
State the type of bonding in potassium chloride which melts at 1043 K.
Describe the structure and bonding in solid magnesium oxide.
Outline why solid magnesium chloride does not conduct electricity.
Predict whether phosphorus(V) oxide and sodium oxide conduct electricity in their solid and molten states. Complete the boxes with “yes” or “no”.
Phosphorus(V) oxide | Sodium oxide | |
Solid state | ||
Molten state |
State the formula of the compounds formed between the elements below.
i) Sodium and sulfur:
ii) Magnesium and phosphorus:
Describe the covalent bond present in a chlorine molecule and how it is formed.
Using section 8 of the data booklet to state which of the following single covalent bonds is the most polar.
C-O | C-H | O-H |
Using section 10 of the data booklet, list the following molecules in order of increasing bond length between the carbon atoms.
C2H6 | C2H4 | C2H2 |
Using section 11 of the data booklet, list the following molecules in order of decreasing bond strength between the carbon atoms.
C2H6 | C2H4 | C2H2 |
CO contains three covalent bonds, one of which is a coordinate bond.
Describe how a coordinate bond arises in CO.
Calcium nitrate contains both covalent and ionic bonds.
State the formula of both ions present and the nature of the force between these ions.
State the formula of the compound that boron forms with chlorine.
Explain why boron trichloride is able to form coordinate (covalent) bonds with other molecules.