chemistry Bonding revision

Q: What are the three types of strong chemical bonds?

Ionic, covalent, and metallic

Q: What particles are involved in ionic bonding?

A: Oppositely charged ions (positive and negative).

How does ionic bonding form?

A: By transfer of electrons from a metal to a non-metal

Q: Where does ionic bonding occur?

In compounds formed from metals and non metals

Q: What particles are involved in covalent bonding?

A: Atoms that share pairs of electrons

Q: Where does covalent bonding occur?

A: In non-metal elements and compounds of non-metals.

Q: What particles are involved in metallic bonding?

A: Positive metal ions and delocalised electrons.

How does metallic bonding work?

A: Metal atoms share delocalised electrons that move freely

Q: Where does metallic bonding occur?

A: In metals and alloys

Q: What causes chemical bonds to form?

A: Electrostatic forces between charged particles (nuclei and electrons or ions).

Q: What does “electrostatic force” mean in bonding?

A: Attraction between opposite charges or repulsion between like charges.

Q: How is ionic bonding explained using electrostatic forces?

• Electrons are transferred from a metal to a non-metal.

• This forms positive and negative ions.

• Oppositely charged ions attract each other strongly.

Q: How is covalent bonding explained using electrons?

A:

• Atoms share pairs of electrons.

• Shared electrons are attracted to both nuclei.

• This attraction holds the atoms together.

How is covalent bonding explained using electrons.

• Atoms share pairs of electrons.

• Shared electrons are attracted to both nuclei.

• This attraction holds the atoms together.

Q: How is metallic bonding explained using electrons?

• Metal atoms lose outer electrons.

• These electrons become delocalised (free to move).

• Positive metal ions are attracted to the delocalised electrons.

Q: Give a full explanation of chemical bonding in terms of electrons and forces.

A:

Chemical bonding occurs because of electrostatic attraction between charged particles. In ionic bonding, electrons are transferred and oppositely charged ions attract. In covalent bonding, electrons are shared between atoms and attracted to both nuclei. In metallic bonding, positive metal ions are attracted to delocalised electrons.

What happens when a metal reacts with a non-metal?

A: Electrons in the outer shell of the metal atom are transferred from the metal to the non-metal.

What happens in ionic bonding?

A: Electrons are transferred from a metal to a non-metal

Q: How do metals form ions?

A: They lose electrons to become positive ions

Q: How do non-metals form ions?

A: They gain electrons to become negative ions.

Why do atoms form ions?

A: To achieve a full outer shell (noble gas configuration

What charge do group 1 metals form

+1

What charge do group 2 metals form

+2

What charge do group 6 non metals form

-2

What charge do group 7 non metals form

-1

Q: What do dot-and-cross diagrams show?

A: The transfer of electrons in ionic compounds.

Q: What structure do ionic compounds form?

A: Giant ionic lattices

What holds ionic compounds together?

A: Strong electrostatic attraction between oppositely charged ions.

Q: Why do ionic compounds have high melting points?

A: Many strong ionic bonds must be broken.

When do ionic compounds conduct electricity?

A: When molten or dissolved in water

Why don’t solid ionic compounds conduct electricity?

A: Ions are fixed in place and cannot move and also have no delocalised electrons that move freely.

Q: How do covalent bonds form?

A: Atoms share pairs of electrons.

Q: What is a simple molecular substance?

A: A substance made of small molecules joined by covalent bonds

What forces exist between molecules?

A: Weak intermolecular forces.

Why do simple molecular substances have low melting points?

A: Weak intermolecular forces are easy to overcome.

Do simple molecular substances conduct electricity?

A: No, because they have no charged particles that can move

Q: Give examples of giant covalent structures.

A: Diamond, graphite, silicon dioxide.

Why do giant covalent structures have high melting points?

A: Many strong covalent bonds must be broken.

Q: Why is diamond very hard?

A: Each carbon atom forms four strong covalent bonds.

Why can graphite conduct electricity?

A: It has delocalised electrons that can move.

Q: What is the structure of metals?

A: Positive metal ions surrounded by delocalised electrons

What holds metals together?

.

A: Attraction between positive ions and delocalised electrons

Q: Why do metals conduct electricity?

A: Delocalised electrons can move through the structure.

Q: Why are metals malleable?

.

A: Layers of ions can slide without breaking the metallic bonds

Q: How does structure affect properties?

A: Strong bonds → high melting points; weak forces → low melting points

Q: Link bonding type to properties.

• Ionic → high melting point, conducts when molten/dissolved

• Simple covalent → low melting point, no conductivity

• Giant covalent → very high melting point

• Metallic → conducts electricity, malleable