Module 2

Question 1

principal quantum number

Answer 1

shell number/energy level

Question 2

shapes of orbitals in s and p subshells

Answer 2

s: sphere
p: dumbbell

Question 3

why are ionic compounds generally soluble in polar solvents?

Answer 3

• ion-dipole interactions between ions and polar molecules are stronger than the ionic bonds between ions
• therefore the ionic lattice breaks down and polar molecules surround the ions

(energy released in the formation of ion-dipole interactions is greater than the energy required to break ionic bonds)

Question 4

how do ionic compounds act as electrical conductors when molten or aqueous?

Answer 4

ions act as mobile charge carriers

Question 5

ionic vs covalent bonds

Answer 5

ionic:
- attracts in all directions (in three dimensions)
- stronger

covalent:
- localised attraction (solely between shared pair of e- and nuclei of bonding atoms)
- weaker

Question 6

which periods can expand their octet?

Answer 6

period 3+

Question 7

electronegativity

Answer 7

the ability of an atom to attract an e- pair in a covalent bond

Question 8

why is a molecule polar? (2 marks)

Answer 8

• difference in electronegativity between atom A and atom B causes a dipole
• the dipoles are assymetrical/do not cancel out

Question 9

factors affecting IMF strength between inorganic molecules

Answer 9

• number of e-
• charge of atoms in molecule

Question 10

state and explain two anomalous properties of ice. (4 marks)

Answer 10

• ice is less sense than water
  –> H bonds between water molecules form an open lattice structure
• ice has a relatively high melting point
  –> strong H bonds require a lot more energy to overcome

Question 11

two types of isomerism

Answer 11

• structural
• stereoisomerism

Question 12

types of structural isomerism

Answer 12

• branched
• positional
• functional

Question 13

types of stereoisomerism

Answer 13

• cis/trans
• E/Z
• optical