Bonding, Structure and Properties Chemistry Topic 2 Flashcards
What happens when a metal and non-metal react? (in terms of bonding)
An ionic bond is formed
Explain the process of ionic bonding
• Metal loses an electron, forms a positive ion
• Non metal gains that electron, forms a negative ion
Describe an ionic substance’s structure
• Ionic substances form giant ionic lattices containing oppositely charged ions
What force holds ionic bonds together? Why does it happen?
• Strong electrostatic forces of attraction between oppositely charged ions
• Because positive ions and negative ions attract
How much energy is needed to break an ionic bond?
A lot. Very strong forces
Are ionic compounds able to conduct electricity?
No. There are no delocalised electrons since the ions have full outer shells. Current can’t move.
+(It can when molten)
When happens when a non-metal bonds with a non-metal?
A covalent bond is formed
What happens in a covalent bond?
• In order for the atoms to have a full outer shell, they share electrons
Describe the structure of a metallic bond
• A giant lattice of positively charged atoms arranged in a regular pattern
• Electrons are delocalised, free to move around the structure
• Strong force of attraction between the positive nucleus and negative delocalised electrons
What happens when a metal bonds with another metal?
A metallic bond is formed
What properties do metals gain because of the strong forces of attraction?
• Strong
• High melting and pooling point, bonds are very strong = needs a lot of energy to break
What properties do metals gain because of their delocalised electrons?
• Able to conduct electricity by carrying the current
• Able to conduct heat by carrying thermal energy
What property do pure metals gain because of their regular structure?
• Malleable (Able to be shaped/formed) because layers are able to slide over each other
What are alloys?
A mixture of metal with two or more different elements
Why would you choose differently sized atoms in an alloy?
• Different sizes disrupts the regular lattice making it more difficult for layers to slide over each other (becomes harder)
