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

What is a chemical bond?
  1. A force of attraction between atoms
  2. A reaction that always releases light
  3. A mixture of two elements
  4. A change of state from liquid to gas

Question 2

Ionic bonding forms when?
  1. Electrons are transferred from one atom to another
  2. Electrons are shared equally in pairs
  3. Neutrons move between nuclei
  4. Atoms overlap to form mixtures

Question 3

Covalent bonding involves?
  1. Sharing pairs of electrons
  2. Losing all outer-shell electrons
  3. Gaining protons in the nucleus
  4. Separating atoms into ions only

Question 4

Metallic bonding is the attraction between?
  1. Positive metal ions and delocalized electrons
  2. Negative ions and shared electron pairs
  3. Neutral atoms and neutrons
  4. Molecules and hydrogen ions

Question 5

Why do ionic compounds usually have high melting points?
  1. Strong electrostatic attractions act throughout a giant lattice
  2. They contain only weak intermolecular forces
  3. Their atoms are not bonded at all
  4. They always have very small molecules

Question 6

Why do simple molecular substances often have low melting and boiling points?
  1. Forces between molecules are relatively weak
  2. Covalent bonds inside molecules are weak
  3. Their nuclei are unstable
  4. They always contain metals

Question 7

Why can graphite conduct electricity?
  1. It has delocalized electrons that can move
  2. It has ionic bonds between carbon atoms
  3. It contains free protons
  4. It is made from metal atoms

Question 8

Why is diamond very hard?
  1. Each carbon atom is strongly covalently bonded in a giant 3D structure
  2. It contains layers that slide over each other
  3. It is made of ionic molecules
  4. It has weak forces between small molecules

Question 9

Which substance has ionic bonding?
  1. Sodium chloride (NaCl)
  2. Oxygen (O2)
  3. Methane (CH4)
  4. Carbon dioxide (CO2)

Question 10

Which substance is a simple molecular covalent substance?
  1. Carbon dioxide (CO2)
  2. Sodium chloride (NaCl)
  3. Magnesium oxide (MgO)
  4. Silicon dioxide (SiO2)

Question 11

When does solid sodium chloride conduct electricity?
  1. When molten or dissolved in water, not when solid
  2. Only when solid
  3. Only as a gas
  4. Always in every state equally

Question 12

Why are metals malleable?
  1. Layers of metal ions can slide while metallic bonding is maintained
  2. Metals are made of separate molecules with weak forces
  3. Metals contain no electrons
  4. Metal atoms are not arranged in a structure

Question 13

What is a polymer?
  1. A very large molecule made from repeating smaller units
  2. A pure metal with delocalized electrons
  3. A compound made from ionic crystals only
  4. A gas with a low boiling point

Question 14

Which statement about water (H2O) is correct?
  1. It is a covalent compound with shared electrons
  2. It is an ionic compound with transferred electrons only
  3. It is a metallic structure of hydrogen and oxygen ions
  4. It is a mixture, not a compound

Question 15

Why are ionic solids brittle?
  1. Shifting layers can bring like charges together so they strongly repel
  2. Ions can move freely in the solid
  3. They contain no fixed structure
  4. They are made from neutral molecules only

Question 16

Which formula represents methane?
  1. CH4
  2. C2H6
  3. CO2
  4. H2O

Question 17

Which substance has a giant covalent structure?
  1. Silicon dioxide (SiO2)
  2. Oxygen (O2)
  3. Hydrogen chloride (HCl)
  4. Water (H2O)

Question 18

Why does copper conduct electricity as a solid?
  1. Its delocalized electrons are free to move through the lattice
  2. Copper ions are free to flow as a liquid
  3. It contains covalent molecules with weak forces
  4. Electrons are fixed in place on each atom

Question 19

In covalent bonding, atoms share electrons mainly for what reason?
  1. Fill their outer electron shells and become more stable
  2. Increase their number of protons
  3. Become positively charged ions
  4. Remove all electrons from the atom

Question 20

Which pair of element types most often forms an ionic compound?
  1. A metal and a non-metal
  2. Two non-metals
  3. Two noble gases
  4. Two transition metals only

Question 21

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

Question 22

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

Question 23

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

Question 24

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

Question 25

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

Question 26

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 only
  4. A force between ions in solution only

Question 27

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 28

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 29

Why can graphite conduct electricity?
  1. It has delocalized 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 only

Question 30

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 31

Which statement about graphene is correct?
  1. It is a single layer of carbon atoms and is a good electrical conductor
  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 32

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

Question 33

Why are metals good conductors of electricity?
  1. Delocalized 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 34

Why are alloys usually harder than pure metals?
  1. Different-sized atoms distort layers and make sliding harder
  2. Alloys contain no metallic bonds
  3. Alloys always have weaker bonding than pure metals
  4. Alloy atoms are perfectly aligned so layers slide easily

Question 35

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

Question 36

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 37

Why are nanoparticles often more reactive than larger particles of the same substance?
  1. They have a much larger surface area to volume ratio
  2. Their atoms have more protons
  3. They always have ionic bonding
  4. They contain no electrons

Question 38

What is one concern about widespread nanoparticle use?
  1. Possible health or environmental effects are not always fully known
  2. Nanoparticles cannot enter any living cells
  3. Nanoparticles always behave exactly like bulk materials
  4. All nanoparticles are non-reactive in the body

Question 39

Which statement about polymers is correct?
  1. Polymers are long-chain molecules made from many repeating units
  2. Polymers are always giant ionic lattices
  3. All polymers are metals
  4. Polymers are mixtures with no chemical bonds

Question 40

Why does iodine (I2) have a much lower boiling point than sodium iodide (NaI)?
  1. I2 is simple molecular with weak intermolecular forces, while NaI is ionic with strong electrostatic attractions
  2. I2 has stronger ionic bonds than NaI
  3. NaI is made of simple molecules with weak forces
  4. Both have identical bonding and boiling points

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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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