Ionic Bonding, Covalent Bonding, Metallic Bonding and Giant Structures

1. Element X has electronic configuration 2,8,2. Element Y has electronic configuration 2,6.

Which formula and bonding are most likely in the compound formed?

A XY, ionic
B XY, covalent
C XY2, ionic
D X2Y, covalent

2. Which statement about magnesium chloride is correct?

A Magnesium atoms gain two electrons and chlorine atoms lose one electron each.
B Magnesium ions and chloride ions are held together by covalent bonds.
C Magnesium forms Mg2+ ions and chlorine forms Cl– ions.
D Magnesium chloride conducts electricity when solid because electrons move through the lattice.

3. Aluminium reacts with oxygen to form aluminium oxide.

Which formula is correct?

A AlO
B Al2O
C Al2O3
D Al3O2

4. Which pair of ions has the same electronic configuration?

A Na+ and Cl–
B Mg2+ and O2–
C Al3+ and S2–
D K+ and F–

5. A compound contains X3+ ions and Y2– ions.

What is the simplest formula of the compound?

A XY
B X2Y3
C X3Y2
D X6Y6

6. Which statement explains why solid sodium chloride does not conduct electricity?

A It contains no charged particles.
B Its ions are fixed in position.
C Its electrons are shared between atoms.
D Its ions are neutralised by water.

7. Which substance conducts electricity when molten but not when solid?

A graphite
B copper
C sodium chloride
D sulfur

8. Which statement about ionic bonding is correct?

A It is the attraction between positive ions and delocalised electrons.
B It is the attraction between oppositely charged ions.
C It is the sharing of electrons between non-metal atoms.
D It is the weak force between simple molecules.

9. Which compound is most likely to be ionic?

A CO2
B CH4
C MgO
D HCl

10. A student says, “Ionic compounds conduct electricity because they contain electrons.”

Which correction is best?

A They conduct because their ions can move when molten or aqueous.
B They conduct because their molecules can move when molten.
C They conduct because electrons move through the solid lattice.
D They conduct only when their ions are fixed in place.

Written and Compiled By Sir Hunain Zia (AYLOTI), World Record Holder With 154 Total A Grades, 11 World Records and 7 Distinctions, Educate A Change.

11. Which dot-and-cross description is correct for calcium oxide?

A Calcium shares two electrons with oxygen.
B Calcium gains two electrons and oxygen loses two electrons.
C Calcium loses two electrons and oxygen gains two electrons.
D Calcium and oxygen both lose two electrons.

12. Which row correctly describes sodium oxide?

	formula	type of bonding
A	NaO	ionic
B	Na2O	ionic
C	NaO2	covalent
D	Na2O3	covalent

13. Which substance has a giant ionic lattice?

A iodine
B sodium chloride
C methane
D diamond

14. Which property is typical of ionic compounds?

A low melting point and poor solubility in water
B high melting point and electrical conduction when molten
C low boiling point and electrical conduction when solid
D high volatility and simple molecular structure

15. Beryllium forms Be2+ ions and nitrogen forms N3– ions.

What is the formula of beryllium nitride?

A BeN
B Be2N3
C Be3N2
D Be6N6

16. Which statement about covalent bonding is correct?

A Electrons are transferred from a metal to a non-metal.
B A pair of electrons is shared between atoms.
C Positive ions are attracted to delocalised electrons.
D Ions are arranged in a giant lattice.

17. Which molecule contains exactly four electrons involved in covalent bonds?

A H2O
B NH3
C CH4
D CO2

18. Which molecule contains the greatest number of electrons involved in covalent bonds?

A H2O
B CH4
C N2
D CO2

19. Which pair of substances both have simple molecular structures?

A diamond and graphite
B methane and carbon dioxide
C sodium chloride and magnesium oxide
D copper and aluminium

20. Why does carbon dioxide have a low boiling point?

A Strong covalent bonds inside molecules are broken during boiling.
B Weak forces between molecules are overcome during boiling.
C Ionic bonds between carbon and oxygen are weak.
D Carbon dioxide has no bonds at all.

Written and Compiled By Sir Hunain Zia (AYLOTI), World Record Holder With 154 Total A Grades, 11 World Records and 7 Distinctions, Educate A Change.

21. Which substance has molecules with a triple covalent bond?

A oxygen
B nitrogen
C chlorine
D hydrogen

22. Which statement about a molecule of methane, CH4, is correct?

A Carbon transfers four electrons to hydrogen atoms.
B Carbon forms four covalent bonds by sharing electrons.
C Methane contains CH4+ and H– ions.
D Methane has a giant covalent structure.

23. Which substance is covalent but has a giant structure?

A carbon dioxide
B silicon(IV) oxide
C water
D ammonia

24. Which row correctly compares diamond and graphite?

	diamond	graphite
A	conducts electricity	does not conduct electricity
B	each carbon bonded to 3 carbons	each carbon bonded to 4 carbons
C	very hard	soft/slippery
D	simple molecular	giant covalent

25. Why does graphite conduct electricity?

A It contains mobile ions between layers.
B Each carbon atom has one delocalised electron.
C Covalent bonds between layers are weak.
D Carbon atoms become positive ions in water.

26. Why is diamond very hard?

A It has layers that slide over each other.
B Each carbon atom forms four strong covalent bonds in a giant lattice.
C It contains strong ionic bonds between carbon ions.
D It contains weak intermolecular forces only.

27. Which statement about silicon(IV) oxide is correct?

A It has a simple molecular structure and low melting point.
B It has a giant covalent structure and high melting point.
C It conducts electricity because it has delocalised electrons.
D It is made of Si4+ and O2– ions in a giant ionic lattice.

28. In graphite, each carbon atom is bonded to how many other carbon atoms?

A 1
B 2
C 3
D 4

29. In diamond, each carbon atom is bonded to how many other carbon atoms?

A 1
B 2
C 3
D 4

30. Which statement explains why graphite is used as a lubricant?

A Strong covalent bonds break easily within each layer.
B Layers can slide because weak forces exist between layers.
C Graphite melts at room temperature.
D Graphite reacts with water to form a slippery solution.

Written and Compiled By Sir Hunain Zia (AYLOTI), World Record Holder With 154 Total A Grades, 11 World Records and 7 Distinctions, Educate A Change.

31. Which substance has a giant structure and conducts electricity?

A diamond
B graphite
C iodine
D sulfur

32. Which substance has a giant structure but does not conduct electricity?

A copper
B graphite
C diamond
D sodium chloride solution

33. Which statement about metallic bonding is correct?

A It is the attraction between positive metal ions and delocalised electrons.
B It is the attraction between positive and negative ions.
C It is the sharing of electron pairs between metal atoms only.
D It is the weak force between metal molecules.

34. Why can metals conduct electricity when solid?

A Positive ions move through the lattice.
B Delocalised electrons move through the lattice.
C Metal atoms evaporate and carry charge.
D Negative ions move between layers.

35. Which property of metals is explained by layers of particles sliding without breaking the metallic bond?

A high density
B malleability
C high melting point
D electrical insulation

36. Which substance has metallic bonding?

A aluminium
B aluminium oxide
C carbon dioxide
D silicon(IV) oxide

37. Which row correctly describes copper?

	structure	electrical conduction
A	simple molecular	does not conduct
B	giant ionic	conducts only when molten
C	giant metallic	conducts when solid
D	giant covalent	conducts only in solution

38. Why do most metals have high melting points?

A Weak forces between metal molecules are easy to overcome.
B Strong attractions exist between positive ions and delocalised electrons.
C Metal atoms are covalently bonded into small molecules.
D Metals contain alternating positive and negative ions.

39. Which substance is malleable and conducts electricity by delocalised electrons?

A graphite
B sodium chloride
C copper
D silicon(IV) oxide

40. Which comparison is correct?

A Ionic compounds conduct as solids; metals conduct only when molten.
B Metals conduct as solids; ionic compounds conduct when molten or aqueous.
C Simple molecular substances conduct because molecules move freely.
D Giant covalent substances always conduct electricity.

Written and Compiled By Sir Hunain Zia (AYLOTI), World Record Holder With 154 Total A Grades, 11 World Records and 7 Distinctions, Educate A Change.

41. A substance has a high melting point, is brittle, dissolves in water and conducts electricity when dissolved.

Which structure is most likely?

A simple molecular
B giant ionic
C giant metallic
D giant covalent

42. A substance has a low boiling point and does not conduct electricity in solid, liquid or aqueous form.

Which substance is most likely?

A sodium chloride
B copper
C methane
D graphite

43. A solid conducts electricity, has a very high melting point and is soft/slippery.

Which substance is most likely?

A diamond
B graphite
C sodium chloride
D iodine

44. A solid has a very high melting point, does not conduct electricity, and is extremely hard.

Which substance is most likely?

A diamond
B graphite
C copper
D sodium chloride solution

45. Which statement about simple molecular substances is correct?

A They usually have low melting points because weak intermolecular forces are overcome.
B They usually have high melting points because covalent bonds inside molecules are weak.
C They conduct electricity when liquid because molecules contain shared electrons.
D They are usually giant lattices of ions.

46. Why does iodine sublime easily compared with diamond?

A Iodine has weak forces between molecules; diamond has strong covalent bonds throughout a lattice.
B Iodine has ionic bonds; diamond has metallic bonds.
C Iodine contains delocalised electrons; diamond contains molecules.
D Iodine atoms are smaller than carbon atoms.

47. Which statement about water is correct?

A It is ionic because hydrogen is a metal.
B It is covalent because hydrogen and oxygen share electrons.
C It is metallic because oxygen has delocalised electrons.
D It is giant covalent because it has a high boiling point compared with methane.

48. Which substance contains both covalent bonds and weak forces between molecules?

A sodium chloride
B magnesium oxide
C hydrogen chloride
D copper

49. Which row correctly identifies the bonding or structure?

	substance	bonding/structure
A	magnesium oxide	simple molecular
B	sulfur	metallic
C	silicon(IV) oxide	giant covalent
D	methane	giant ionic

50. A student compares magnesium oxide and carbon dioxide.

Which statement is correct?

A Both have low melting points because both contain molecules.
B Magnesium oxide has a high melting point due to strong ionic attractions; carbon dioxide has a low boiling point due to weak intermolecular forces.
C Magnesium oxide conducts electricity when solid; carbon dioxide conducts when gaseous.
D Both substances have giant covalent structures.

Written and Compiled By Sir Hunain Zia (AYLOTI), World Record Holder With 154 Total A Grades, 11 World Records and 7 Distinctions, Educate A Change.

1. A

X = 2,8,2, so X forms X2+.
Y = 2,6, so Y forms Y2–.
Charges balance as XY.

A right: XY is ionic.
B wrong: Bonding is ionic, not covalent.
C wrong: XY2 gives unbalanced charges.
D wrong: Formula and bonding are both wrong.

2. C

A wrong: Magnesium loses two electrons; chlorine gains one electron each.
B wrong: MgCl2 has ionic bonding, not covalent bonding.
C right: Mg forms Mg2+ and chlorine forms Cl–.
D wrong: Solid MgCl2 does not conduct because ions are fixed.

3. C

Al forms Al3+.
O forms O2–.
Balance charges: 2Al3+ = +6, 3O2– = –6.
Formula = Al2O3.

A wrong: AlO gives +3 and –2.
B wrong: Al2O gives +6 and –2.
C right: Al2O3 balances charges.
D wrong: Al3O2 gives +9 and –4.

4. B

A wrong: Na+ has 10 electrons; Cl– has 18 electrons.
B right: Mg2+ has 10 electrons; O2– has 10 electrons.
C wrong: Al3+ has 10 electrons; S2– has 18 electrons.
D wrong: K+ has 18 electrons; F– has 10 electrons.

5. B

X3+ and Y2– must balance.
2X3+ = +6
3Y2– = –6
Formula = X2Y3.

A wrong: Charges do not balance.
B right: X2Y3 balances charges.
C wrong: X3Y2 gives +9 and –4.
D wrong: X6Y6 can simplify and is not the simplest ratio.

6. B

A wrong: Sodium chloride contains charged ions.
B right: Solid NaCl does not conduct because ions are fixed in position.
C wrong: Electrons are not shared; bonding is ionic.
D wrong: Water is not present in solid sodium chloride.

7. C

A wrong: Graphite conducts when solid.
B wrong: Copper conducts when solid and molten.
C right: Sodium chloride conducts when molten, but not when solid.
D wrong: Sulfur does not conduct.

8. B

A wrong: This describes metallic bonding.
B right: Ionic bonding is attraction between oppositely charged ions.
C wrong: This describes covalent bonding.
D wrong: Weak forces between molecules are intermolecular forces.

9. C

A wrong: CO2 is covalent.
B wrong: CH4 is covalent.
C right: MgO forms between a metal and non-metal, so it is ionic.
D wrong: HCl is covalent as a molecule.

10. A

A right: Ionic compounds conduct when molten or aqueous because ions are free to move.
B wrong: Ionic compounds do not contain molecules.
C wrong: Electron movement through a solid lattice is metallic/graphite conduction, not ionic conduction.
D wrong: Fixed ions cannot carry charge.

Written and Compiled By Sir Hunain Zia (AYLOTI), World Record Holder With 154 Total A Grades, 11 World Records and 7 Distinctions, Educate A Change.

11. C

A wrong: Calcium oxide is ionic, not covalent.
B wrong: Calcium loses electrons; oxygen gains electrons.
C right: Calcium loses two electrons to form Ca2+; oxygen gains two electrons to form O2–.
D wrong: Oxygen does not lose electrons in calcium oxide.

12. B

Sodium forms Na+.
Oxygen forms O2–.
Two Na+ ions balance one O2– ion, so Na2O.

A wrong: NaO gives +1 and –2.
B right: Na2O, ionic.
C wrong: Formula and bonding are wrong.
D wrong: Formula and bonding are wrong.

13. B

A wrong: Iodine is simple molecular.
B right: Sodium chloride has a giant ionic lattice.
C wrong: Methane is simple molecular.
D wrong: Diamond is giant covalent, not ionic.

14. B

A wrong: Ionic compounds usually have high melting points.
B right: Ionic compounds have high melting points and conduct when molten.
C wrong: They do not conduct when solid.
D wrong: They are not volatile simple molecules.

15. C

Be2+ and N3– must balance.
3Be2+ = +6
2N3– = –6
Formula = Be3N2.

A wrong: Charges do not balance.
B wrong: Charges do not balance.
C right: Be3N2 balances charges.
D wrong: Not simplest ratio.

16. B

A wrong: This describes ionic bonding.
B right: Covalent bonding is sharing a pair of electrons.
C wrong: This describes metallic bonding.
D wrong: This describes ionic lattice arrangement.

17. A

A right: H2O has two single covalent bonds = 4 bonding electrons.
B wrong: NH3 has three single bonds = 6 bonding electrons.
C wrong: CH4 has four single bonds = 8 bonding electrons.
D wrong: CO2 has two double bonds = 8 bonding electrons.

18. Faulty question

H2O has 4 bonding electrons.
CH4 has 8 bonding electrons.
N2 has 6 bonding electrons.
CO2 has 8 bonding electrons.

B is correct because CH4 has 8 bonding electrons.
D is also correct because CO2 has 8 bonding electrons.

So the question has two correct answers: B and D. To fix it, replace CH4 with NH3 or replace CO2 with O2.

19. B

A wrong: Diamond and graphite are giant covalent.
B right: Methane and carbon dioxide are simple molecular substances.
C wrong: Sodium chloride and magnesium oxide are giant ionic.
D wrong: Copper and aluminium are giant metallic.

20. B

A wrong: Covalent bonds inside CO2 molecules are not broken during boiling.
B right: Only weak intermolecular forces between molecules are overcome.
C wrong: CO2 is not ionic.
D wrong: CO2 has covalent bonds within molecules.

Written and Compiled By Sir Hunain Zia (AYLOTI), World Record Holder With 154 Total A Grades, 11 World Records and 7 Distinctions, Educate A Change.

21. B

A wrong: Oxygen has a double covalent bond.
B right: Nitrogen has a triple covalent bond, N≡N.
C wrong: Chlorine has a single covalent bond.
D wrong: Hydrogen has a single covalent bond.

22. B

A wrong: Methane is covalent, so electrons are shared, not transferred.
B right: Carbon forms four covalent bonds by sharing electrons with hydrogen atoms.
C wrong: Methane does not contain ions.
D wrong: Methane is simple molecular.

23. B

A wrong: Carbon dioxide is simple molecular.
B right: Silicon(IV) oxide has a giant covalent structure.
C wrong: Water is simple molecular.
D wrong: Ammonia is simple molecular.

24. C

A wrong: Diamond does not conduct; graphite conducts.
B wrong: Diamond has 4 bonds per carbon; graphite has 3.
C right: Diamond is very hard; graphite is soft/slippery.
D wrong: Both diamond and graphite are giant covalent.

25. B

A wrong: Graphite does not conduct by mobile ions.
B right: Each carbon atom has one delocalised electron that can move and carry charge.
C wrong: Weak forces between layers explain slipperiness, not electrical conduction.
D wrong: Carbon atoms do not become ions in water.

26. B

A wrong: Layers sliding describes graphite.
B right: Diamond is hard because each carbon atom forms four strong covalent bonds in a giant lattice.
C wrong: Diamond is not ionic.
D wrong: Diamond is not simple molecular.

27. B

A wrong: Silicon(IV) oxide is not simple molecular.
B right: It is giant covalent and has a high melting point.
C wrong: It does not conduct electricity.
D wrong: It is not giant ionic.

28. C

A wrong: Graphite carbon is not bonded to only 1 carbon.
B wrong: It is not bonded to only 2 carbons.
C right: Each carbon atom in graphite is bonded to 3 other carbon atoms.
D wrong: 4 bonds per carbon describes diamond.

29. D

A wrong: Diamond carbon is not bonded to only 1 carbon.
B wrong: It is not bonded to only 2 carbons.
C wrong: 3 bonds per carbon describes graphite.
D right: Each carbon atom in diamond is bonded to 4 other carbon atoms.

30. B

A wrong: Strong covalent bonds within layers do not break easily.
B right: Layers slide over each other because weak forces exist between layers.
C wrong: Graphite does not melt at room temperature.
D wrong: Graphite does not form a slippery solution with water.

Written and Compiled By Sir Hunain Zia (AYLOTI), World Record Holder With 154 Total A Grades, 11 World Records and 7 Distinctions, Educate A Change.

31. B

A wrong: Diamond is giant but does not conduct.
B right: Graphite is giant covalent and conducts electricity.
C wrong: Iodine is simple molecular.
D wrong: Sulfur is simple molecular.

32. C

A wrong: Copper has a giant metallic structure and conducts.
B wrong: Graphite conducts.
C right: Diamond has a giant covalent structure but does not conduct electricity.
D wrong: Sodium chloride solution conducts, but it is not a solid giant structure.

33. A

A right: Metallic bonding is attraction between positive metal ions and delocalised electrons.
B wrong: This describes ionic bonding.
C wrong: Metallic bonding is not shared electron pairs.
D wrong: Metals do not have metal molecules held by weak forces.

34. B

A wrong: Positive metal ions are fixed in the lattice.
B right: Delocalised electrons move and carry charge.
C wrong: Metal atoms do not need to evaporate to conduct.
D wrong: Metals do not contain negative ions moving between layers.

35. B

A wrong: Density is not mainly explained by sliding layers.
B right: Malleability occurs because layers can slide while metallic bonding remains.
C wrong: High melting point is due to strong metallic bonding.
D wrong: Metals are not electrical insulators.

36. A

A right: Aluminium has metallic bonding.
B wrong: Aluminium oxide is ionic.
C wrong: Carbon dioxide is covalent molecular.
D wrong: Silicon(IV) oxide is giant covalent.

37. C

A wrong: Copper is not simple molecular.
B wrong: Copper is not giant ionic.
C right: Copper has a giant metallic structure and conducts as a solid.
D wrong: Copper is not giant covalent.

38. B

A wrong: Metals do not have simple molecules with weak forces.
B right: Strong attractions between positive ions and delocalised electrons require much energy to overcome.
C wrong: Metals are not small covalent molecules.
D wrong: Alternating positive and negative ions describe ionic compounds.

39. C

A wrong: Graphite conducts by delocalised electrons but is not malleable like a metal.
B wrong: Sodium chloride is ionic and brittle.
C right: Copper is malleable and conducts by delocalised electrons.
D wrong: Silicon(IV) oxide is giant covalent and does not conduct.

40. B

A wrong: Ionic compounds do not conduct as solids; metals conduct as solids.
B right: Metals conduct as solids; ionic compounds conduct when molten or aqueous.
C wrong: Simple molecular substances usually do not conduct.
D wrong: Giant covalent substances do not always conduct; graphite is the key exception.

Written and Compiled By Sir Hunain Zia (AYLOTI), World Record Holder With 154 Total A Grades, 11 World Records and 7 Distinctions, Educate A Change.

41. B

A wrong: Simple molecular substances usually have low melting points and do not conduct.
B right: High melting point, brittleness, water solubility and conduction when dissolved suggest giant ionic.
C wrong: Metals conduct as solids and are malleable, not brittle.
D wrong: Giant covalent substances usually do not dissolve in water or conduct when dissolved.

42. C

A wrong: Sodium chloride has a high melting point and conducts when aqueous/molten.
B wrong: Copper conducts electricity.
C right: Methane is simple molecular, has a low boiling point and does not conduct.
D wrong: Graphite conducts electricity.

43. B

A wrong: Diamond is hard and does not conduct.
B right: Graphite conducts, has very high melting point and is soft/slippery.
C wrong: Sodium chloride does not conduct as a solid and is brittle.
D wrong: Iodine has a low sublimation point compared with giant structures and does not conduct.

44. A

A right: Diamond is extremely hard, has a very high melting point and does not conduct.
B wrong: Graphite is soft/slippery and conducts.
C wrong: Copper conducts and is malleable.
D wrong: Sodium chloride solution is not a solid and conducts.

45. A

A right: Simple molecular substances have low melting points because weak intermolecular forces are overcome.
B wrong: Covalent bonds inside molecules are strong, but they are not broken during melting.
C wrong: Molecules are neutral, so simple molecular liquids usually do not conduct.
D wrong: Simple molecular substances are not giant lattices of ions.

46. A

A right: Iodine has weak forces between molecules; diamond has strong covalent bonds throughout a giant lattice.
B wrong: Iodine is not ionic and diamond is not metallic.
C wrong: Iodine does not conduct using delocalised electrons, and diamond is not molecular.
D wrong: Atomic size is not the main explanation.

47. B

A wrong: Hydrogen is not a metal.
B right: Water is covalent because hydrogen and oxygen share electrons.
C wrong: Water is not metallic.
D wrong: Water is simple molecular, not giant covalent.

48. C

A wrong: Sodium chloride is ionic.
B wrong: Magnesium oxide is ionic.
C right: Hydrogen chloride has covalent bonds within molecules and weak forces between molecules.
D wrong: Copper has metallic bonding.

49. C

A wrong: Magnesium oxide is giant ionic.
B wrong: Sulfur is simple molecular covalent, not metallic.
C right: Silicon(IV) oxide is giant covalent.
D wrong: Methane is simple molecular.

50. B

A wrong: Magnesium oxide does not contain molecules and has a high melting point.
B right: MgO has strong ionic attractions; CO2 has weak intermolecular forces between molecules.
C wrong: Solid MgO does not conduct, and gaseous CO2 does not conduct.
D wrong: MgO is giant ionic; CO2 is simple molecular.

Written and Compiled By Sir Hunain Zia (AYLOTI), World Record Holder With 154 Total A Grades, 11 World Records and 7 Distinctions, Educate A Change.