3.1.3 Bonding PPQs Flashcards
describe the structure of iron oxide and the attraction broken when it is melted or boiled.
Structure: Giant ionic lattice
Attraction: Electrostatic attraction between oppositely charged ions
describe the structure of CH3SH and the attraction broken when it is melted or boiled.
Structure: Simple molecular
Attraction: Covalent bonding between atoms
describe the structure of graphite and the attraction broken when it is melted or boiled.
Structure: Macromolecular
Attraction: Covalent bonding between atoms
describe the structure of sodium bromide and the attraction broken when it is melted or boiled.
Structure: Giant ionic lattice
Attraction: Electrostatic attraction between oppositely charged ions
describe the structure of magnesium and the attraction broken when it is melted or boiled.
Structure: Giant metallic lattice
Attraction: Electrostatic attraction between positive ions and delocalised electrons
describe the structure of diamond and the attraction broken when it is melted or boiled.
Structure: Macromolecular
Attraction: Covalent bonding between atoms
describe the structure of PF3 and the attraction broken when it is melted or boiled.
Structure: Simple molecular
Attraction: Intermolecular attractions between molecules
describe the structure of CH3Br and the attraction broken when it is melted or boiled.
Structure: Simple molecular
Attraction: Intermolecular attractions between molecules
describe the structure of H2O and the attraction broken when it is melted or boiled.
Structure: Simple molecular
Attraction: Intermolecular attractions between molecules
describe the structure of barium and the attraction broken when it is melted or boiled.
Structure: Giant metallic lattice
Attraction: Electrostatic attraction between positive ions and delocalised electrons
what is the ionic formula for potassium nitride
K3N
what is the ionic formula for Rubidium Chlorate (I)
RbClO
what is the ionic formula for Calcium Dichromate
CaCr2O7
what is the ionic formula for Calcium Hydroxide
Ca(OH)2
what is the ionic formula for Zinc Carbonate
ZnCO3
what is the ionic formula for Strontium Sulphate
SrSO4
what is the ionic formula for Iron (III) Hydrogencarbonate
Fe(HCO3)3
name the ionic compound: Al2(CO3)3
Aluminium Carbonate
name the ionic compound: Fe2(CO3)3
Iron (III) Carbonate
name the ionic compound: TiO2
Titanium Dioxide or Titanium (IV) Oxide
Which polymer has hydrogen bonding between the polymer chains?
kevlar
The melting point of XeF4 is higher than the melting point of PF3
Explain why the melting points of these two compounds are different.
In your answer you should give the shape of each molecule, explain why each molecule has that shape and how the shape influences the forces that affect the melting point.
- XeF4 4BP and 2LP around Xe
- PF3 3BP and 1LP around P
- XeF4 is square planar
- PF3 is pyramidal (allow tetrahedral)
- Electron pairs repel as far as possible or Lone pair repels more than bonding pairs
- XeF4 has vdw forces and PF3 has dipole-dipole forces (and vdw)
- Stronger/more intermolecular forces in XeF Due to larger Mr or more electrons or larger molecules or packs more closely
Fluoroantimonic acid contains two ions, SbF6– and H2F+ Draw the shape of the SbF6–ion and the shape of the H2F+
ion. Include any lone pairs that influence the shape. Name the shape of each ion.
Draw a diagram to show the strongest type of interaction between two molecules of ethanol (C2H5OH) in the liquid phase. Include all lone pairs and partial charges in your diagram.
Which statement about barium sulfate is correct?
A It is soluble in water at a temperature of 100 °C.
B It is used in medicine because it does not dissolve in
body fluids.
C It is a pale yellow solid.
D It reacts with acidified barium chloride solution.
B
Explain why the second ionisation energy of calcium is lower than the second ionisation energy of potassium.
- In Ca+ outer electron is further from nucleus and from a higher (energy) orbital
- more shielding in Ca+
A student added 6 cm3 of 0.25 mol dm–3 barium chloride solution to 8 cm3 of 0.15 mol dm–3 sodium sulfate solution.
The student filtered off the precipitate and collected the filtrate. Give an ionic equation for the formation of the precipitate. Show by calculation which reagent is in excess.
Calculate the total volume of the other reagent which should be used by the student so that the filtrate contains only one solute.
- Ba2+ + SO42– → BaSO4
- n BaCl2 (6/1000 × 0.25) = 1.5 × 10–3 and n Na2SO4 = (8/1000 × 0.15) = 1.2× 10–3 so BaCl2 in excess
- 10 cm3 (of 0.15 mol dm–3 sodium sulfate)
