bonding

Question 1

ionic bonding

Answer 1

electrostatic attraction between anions and cations

Question 2

ionic compounds

Answer 2

electrostatic forces not localised - attract in all directions to form giant ionic lattices

Question 3

ionic compound melting/boiling points

Answer 3

high temperatures provide lots of energy
need to overcome strong electrostatic attraction between ions
higher charge density, higher bp

Question 4

ionic compounds solubility

Answer 4

dissolve in polar solvents
polar molecules break down lattice and surround ions
high Q density: more energy to overcome ionic
more energy released
(ion-dipole)

Question 5

charge density

Answer 5

higher charge on the atom, higher charge density
smaller size, higher charge density
very electro(negative/positive)

Question 6

Soluble Salts

Answer 6

All ammonium, Group 1 and nitrate salts
All halide salts (except silver and lead)
All sulfate salts (except calcium, barium, silver and lead)

Question 7

Insoluble salts

Answer 7

All carbonate / Hydroxide salts (except Group 1 and ammonium)
All silver and lead salts (except nitrates)

Question 8

Covalent Bonds

Answer 8

Strong electrostatic attraction between a shared pair of electrons and the nuclei of bonded atoms
overlap of orbitals = localised

Question 9

no. of covalent bonds
“octet expansion”

Answer 9

depends on the shell number
n=2 means a max of 8 electrons
n=3 means max 18 electrons (fill 3d)

Question 10

dative covalent bonds

Answer 10

lone pair on an atom fills orbital in other bonding atom

Question 11

ionic vs covalent

Answer 11

0.0<ΔEN<0.5 - covalent
0.5<ΔEN<1.8 - polar covalent
ΔEN>1.8 - ionic