Bonding and structure Flashcards
What is an ion?
An atom that has lost or gained electrons
Which kinda of elements form ionic bonds?
Metals and Non-Metals
What charges do ions from Group 1 and Group 2 form?
- Group 1 form 1+
- Group 2 form 2+
What charges of ions do Group 6 and Group 7 form?
- Group 6 form 2-
- Group 7 form 1-
Name the force that holds oppositely charged ions together.
Electrostatic force of attraction.
Describe the structure of a giant ionic lattice.
- Regular structure of alternating ions. (P then N then P then N)
- Held together by the electrostatic force of attraction.
Why do ionic substances have high melting points?
The electrostatic force of attraction is strong between the positive and negative ions. It would require more energy to break causing a high melting point.
Why don’t ionic substances conduct electricity when solid?
The ions are fixed in their position so cannot carry an electric current through the solid.
When can ionic substances conduct electricity?
When melted or dissolved.
Why do ionic substances conduct electricity when melted or dissolved?
Ions are free to move and carry charge.
Describe the structure of a pure metal.
Layers of positive metal ions surrounded by delocalised electrons.
Describe the bonding of a pure metal.
Strong electrostatic forces of attraction between metal ions and delocalised electrons.
What are four properties of pure metals?
- Malleable
- High melting / Boiling points
- Good conductors of electricity
- Good conductors of thermal energy
Explain why pure metals are malleable.
The layers can Slide Over each other easily without breaking.
Explain why metals have high melting and boiling points.
The electrostatic forces of attraction between the positive metals and delocalised electrons is strong and requires a lot of energy to break.
