Ionic Bonding, Metallic Bonding, And Structure (C3) Flashcards
What is an ion?
Atom that has lost or gained electrons
Which kinds of elements form ionic bonds?
Metals and non-metals
What charges do ions from Groups 1 and 2 bonds?
Group 1 forms 1+, Group 2 forms 2+
What charges do ions from Groups 6 and 7 form?
Group 6 forms 2-, Group 7 forms 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 positive and negative ions, held together by the electrostatic force of attraction
Why do ionic substances have high melting points?
Electrostatic force of attraction between positive and negative ions is strong and requires lots of energy to break
Why don’t ionic substances conduct electricity when solid?
Ions are fixed in position so cannot move, and there are no delocalised electrons
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 in 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
Layers can slide over each other easily
Explain why metals have high melting and boiling points
Electrostatic force of attraction between positive metal ions and delocalised electrons is strong and requires a lot of energy to break
