Bonding questions

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Bonding question collection

Review Bonding questions for Chemistry, with correct answers shown and coverage across ionic bonding and ions; covalent molecules and giant covalent structures; metallic bonding.

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Question 1

How is an ionic bond formed?
  1. By attraction between oppositely charged ions
  2. By sharing pairs of electrons between atoms
  3. By attraction between neutral molecules
  4. By proton transfer between non-metals

Question 2

What is the formula of magnesium oxide formed from Mg2+ and O2-?
  1. MgO
  2. Mg2O
  3. MgO2
  4. Mg2O3

Question 3

Why do ionic compounds usually have high melting points?
  1. Strong attractions act throughout a giant ionic lattice
  2. They contain weak intermolecular forces
  3. Ionic bonds break easily at low temperatures
  4. Ions are not bonded in the solid state

Question 4

Why does solid sodium chloride not conduct electricity?
  1. Its fixed ions cannot carry charge
  2. It has no charged particles
  3. Its electrons are free to move
  4. Sodium chloride has covalent bonding

Question 5

When does sodium chloride conduct electricity?
  1. When molten or dissolved in water
  2. When solid
  3. When cooled below room temperature
  4. As a gas

Question 6

What is a covalent bond?
  1. A shared pair of electrons between atoms
  2. A transferred pair of protons
  3. An attraction between positive metal ions
  4. A force between ions in solution

Question 7

Why do simple molecular substances like CO2 often have low boiling points?
  1. Weak intermolecular forces are overcome on boiling
  2. Covalent bonds inside molecules are weak
  3. Their molecules are ionic lattices
  4. They contain no electrons

Question 8

What type of structure does diamond have?
  1. A giant covalent structure where each carbon bonds to four others
  2. Layers of carbon with weak forces between layers
  3. A giant ionic lattice of carbon ions
  4. Small molecules with weak forces

Question 9

Why can graphite conduct electricity?
  1. It has delocalised electrons that can move through the structure
  2. It contains mobile ions in the solid
  3. Each carbon atom has no outer electrons
  4. It is made of metallic bonds

Question 10

Why is graphite soft and slippery?
  1. Its layers can slide because weak forces act between layers
  2. Its covalent bonds are weak within each layer
  3. It has no bonds between carbon atoms
  4. It is a liquid at room temperature

Question 11

Which statement about graphene is correct?
  1. It is a single carbon layer that conducts electricity
  2. It is a gas made of C60 molecules
  3. It is an ionic compound of carbon and oxygen
  4. It is an insulator because it has no electrons

Question 12

What best describes metallic bonding?
  1. Attraction between positive metal ions and delocalised electrons
  2. Attraction between neutral metal atoms
  3. Sharing electron pairs between metal and non-metal atoms
  4. Attraction between negative ions and protons

Question 13

Why are metals good conductors of electricity?
  1. Delocalised electrons are free to move through the metal
  2. Metal ions can leave the lattice in the solid state
  3. Metals contain free protons that move
  4. Metals are made of simple molecules

Question 14

Why are alloys usually harder than pure metals?
  1. Different-sized atoms distort layers and make sliding harder
  2. Different atoms create gaps that help layers slide
  3. Mixed atoms remove the delocalised electrons
  4. Mixed atoms arrange the layers more regularly

Question 15

Which substance has a giant covalent structure?
  1. Silicon dioxide (SiO2)
  2. Methane (CH4)
  3. Oxygen (O2)
  4. Hydrogen chloride (HCl)

Question 16

What size range defines nanoparticles?
  1. About \(1\text{ to }100\,\mathrm{nm}\)
  2. About \(1\text{ to }100\,\mathrm{mm}\)
  3. About \(1\text{ to }100\,\mathrm{\mu m}\)
  4. About \(1000\text{ to }10{,}000\,\mathrm{nm}\)

Question 17

Why are nanoparticles often more reactive than larger particles of the same substance?
  1. They have a larger surface-area-to-volume ratio
  2. Their atoms contain more protons
  3. Their chemical bonds become stronger as size falls
  4. Their smaller surface gives fewer collisions

Question 18

What is one concern about widespread nanoparticle use?
  1. Possible health or environmental effects may be uncertain
  2. Bulk-material tests are assumed to predict their effects
  3. Small size is assumed to stop entry into cells
  4. Low mass is assumed to make them unreactive

Question 19

Which statement about polymers is correct?
  1. Long-chain molecules made from repeating units
  2. Giant lattices made from alternating ions
  3. Metal ions surrounded by delocalised electrons
  4. Small molecules joined by temporary intermolecular forces

Question 20

Why does iodine (I2) have a much lower boiling point than sodium iodide (NaI)?
  1. I2 has weak intermolecular forces; NaI has strong ionic attractions
  2. I2 has weak ionic attractions; NaI has strong covalent bonds
  3. I2 has strong intermolecular forces; NaI has weak ionic attractions
  4. Both have identical bonding; NaI simply has greater relative mass

Question 21

Why do ionic compounds conduct electricity when dissolved?
  1. Their ions are free to move
  2. Their electrons move between ions
  3. Their covalent bonds break into protons
  4. Their ions become neutral atoms

Question 22

Why is diamond hard?
  1. Each carbon atom forms four strong covalent bonds
  2. It has weak forces between molecules
  3. Its ions are free to move
  4. It contains delocalised electrons

Question 23

How can nanoparticles be useful in drug delivery?
  1. They can carry medicine to target tissues
  2. They spread medicine throughout the body without targeting
  3. They release medicine before reaching the target
  4. They prevent medicine entering target cells

Question 24

Why do nanoparticles have different properties from bulk materials?
  1. They have a very high surface area to volume ratio
  2. They contain different elements
  3. They have more atoms per particle
  4. They are gases at room temperature

Question 25

What is a simple molecular substance made of?
  1. Small covalent molecules
  2. A giant ionic lattice
  3. A giant metallic lattice
  4. A network of mobile ions

Question 26

Why do polymers have a wide range of properties?
  1. Their structures and intermolecular forces can vary
  2. All polymers have identical chain lengths
  3. They contain no covalent bonds
  4. All polymers are metals

Question 27

Why do many metals have high melting points?
  1. Strong attraction links ions and delocalised electrons
  2. Weak forces act between separate metal molecules
  3. Metal ions move freely through the solid lattice
  4. Covalent bonds join each pair of metal atoms

Question 28

Why are metals malleable?
  1. Layers of atoms can slide while metallic bonding remains
  2. Their ions shatter when layers move
  3. Their atoms are joined by weak covalent bonds
  4. Their electrons are fixed between atoms

Question 29

What shape is a C60 fullerene molecule?
  1. Hollow sphere
  2. Flat sheet
  3. Straight chain
  4. Giant cubic lattice

Question 30

Why is graphene useful in electronics?
  1. It conducts electricity and is very strong
  2. It conducts electricity but breaks under small forces
  3. It is strong but lacks mobile charge carriers
  4. It is flexible but dissolves in water

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Review Bonding questions for Chemistry, with correct answers shown and coverage across ionic bonding and ions; covalent molecules and giant covalent structures; metallic bonding.

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