C2 - atomic structure and bonding
- Created by: kwright17
- Created on: 27-02-16 20:19
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- C2 - Atomic Structure bonding and properties
- Element : A substance that contains only atoms with the same atomic number
- Atom: The smallest part of an element that can exist.
- Atomic number: How much protons / electrons an atom has.
- Mass number: The number of protons and neutrons
- Ionic compounds
- Ion = charged particles that are either positive or negative.
- Group 1 metals form +1 ions because they need to lose an electron which makes them positively charged.
- Cations : Sodium, Magnesium, Iron, Copper.
- Anions: Chloride, Sulphate, Carbonate, Oxide.
- Metal + Non Metal
- Ionic Lattices have high melting points and boiling points.
- Ionic lattices conduct electricity when melted or dissolved in water
- These often form crystals with regular arrangements of ions
- These properties are due to the strong electrostatic forces of attraction.
- These properties are due to the strong electrostatic forces of attraction.
- These often form crystals with regular arrangements of ions
- Ionic lattices conduct electricity when melted or dissolved in water
- Ionic lattices conduct electricity when melted or dissolved in water
- These often form crystals with regular arrangements of ions
- These often form crystals with regular arrangements of ions
- Inside metals
- Solid at room temperature. Good conductors of electricity and heat. High melting point. Malleable. Strong. Dense.
- Metals form metallic bonds
- Covalent molecules
- Non metal + Non Metal
- C2 - Atomic Structure bonding and properties
- Element : A substance that contains only atoms with the same atomic number
- Atom: The smallest part of an element that can exist.
- Atomic number: How much protons / electrons an atom has.
- Mass number: The number of protons and neutrons
- Ionic compounds
- Ion = charged particles that are either positive or negative.
- Group 1 metals form +1 ions because they need to lose an electron which makes them positively charged.
- Cations : Sodium, Magnesium, Iron, Copper.
- Anions: Chloride, Sulphate, Carbonate, Oxide.
- Metal + Non Metal
- Ionic Lattices have high melting points and boiling points.
- Inside metals
- Solid at room temperature. Good conductors of electricity and heat. High melting point. Malleable. Strong. Dense.
- Metals form metallic bonds
- Low melting and boiling points - due to weak intermolecular forces.
- The stronger the intermolecular force the more energy is needed to break them. hence the higher the melting point.
- Do not conduct electricity
- STRONG - a lot of energy is needed to break them
- Giant covalent Molecules
- Most non metals form covalent bonds that form molecules.
- Some form long networks of covalent bonds.
- Diamonds, Silicon Dioxide, Graphite
- Diamond does not conduct electricity because it doesn't have a free delocalised electron
- Graphite has delocalised electrons allowing it to create an electric charge.
- Graphite is slippery because the intermolecular forces between layers are weak and slides over one another.
- Diamond does not conduct electricity because it doesn't have a free delocalised electron
- Allotrope: different forms on the same element in the same physical state. Diamond and Graphite are both allotropes of carbon.
- Most non metals form covalent bonds that form molecules.
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