Structure and Bonding
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?- Created by: RevisingBird
- Created on: 29-03-18 11:08
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- Bonding + Structure
- Ionic Compounds
- Ionic bonding
- Electrostatic forces of attraction
- Between positively and negatively charged ions
- Example: Li+ S2- = Li2S
- Properties
- Conduct when put in water
- The charged ions in a solid structure can't move around
- When put in a liquid they can move around and carry charge
- High melting + boiling point
- Strong electrostatic forces between oppositely charge ions
- Vast amount of heat energy needed to overcome them
- Vast amount of heat energy needed to overcome them
- Strong electrostatic forces between oppositely charge ions
- Strong covalent bonds between atoms in a small molecule
- Strong covalent bonds between atoms in a small molecule.
- Conduct when put in water
- Between a metal and a non - metal
- Ionic bonding
- Covalent Bonding
- Diagrams
- Draw outer electron shell
- Use group number
- Examples
- Simple molecules - water
- Giant covalent structures - diamond
- Large molecules in chains - polymers
- With a non - metal and a non - metal
- Small covalent molecules
- Don't conduct electricity
- Small molecules have no overall charge
- Can't carry electric charge
- Low melting and boiling points
- Weak intermolecular forces between molecules
- Not a lot of heat energy to overcome
- Don't conduct electricity
- Giant covalent molecules
- High melting and boiling point
- Huge network of covalent bonds
- Large amount of heat energy to overcome
- Diamond
- Very hard
- Carbon atoms bonded to four others
- Many strong covalent bonds
- Doesn't conduct
- No delocalised electrons
- All electrons are bonded
- Very hard
- Graphite
- Soft
- Giant layers of atoms can slide over each other easily
- Weak intermolecular forces between the layers
- Giant layers of atoms can slide over each other easily
- Conduct electricity
- Delocalised electrons are free to move around
- Four outer electrons of carbon are bonded and one is delocalised
- Soft
- Carbon
- Diamond
- Very hard
- Carbon atoms bonded to four others
- Many strong covalent bonds
- Doesn't conduct
- No delocalised electrons
- All electrons are bonded
- Very hard
- Graphite
- Soft
- Weak intermolecular forces between the layers
- Weak intermolecular forces between the layers
- Conduct electricity
- Delocalised electrons are free to move around
- Four outer electrons of carbon are bonded and one is delocalised
- Soft
- Fullerenes
- Huge carbon molecules on hexagon rings
- Diamond
- High melting and boiling point
- Diagrams
- Carbon
- Fullerenes
- Huge carbon molecules on hexagon rings
- Fullerenes
- Metals + Alloys
- Metallic bonding
- Electrostatic attraction between positively charged metal ions and delocalised electrons
- Metal ions held together by electrons from outermost shell
- The positive ions produced are held together by strong electrostatic forces
- The electrons in the metals are free to move around
- The positive ions produced are held together by strong electrostatic forces
- Diagram
- Alloys are harder than pure metals
- Alloys have different sizes of atoms
- Makes it harder to slide over each other because the rows of atoms are distorted
- Alloys can conduct and metals can't
- Alloys have a sea of delocalised electrons that carry charge around
- They can carry electrical and thermal energy
- Metallic bonding
- Ionic Compounds
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