Bonding
- Created by: JC:A-A-B
- Created on: 23-12-18 09:42
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- Bonding
- Ionic
- Definition
- Electrostatic Force of attraction between oppositely charged ions by electron transfer.
- Metal atoms lose electrons = +ve ions Non-Metal atoms gain electrons to form -ve ions
- Characteristics
- Stronger & melting points higher- ions smaller/ higher charges.
- e.g. MgO - higher melting point than NaCl - has ions ( Mg 2+ & O 2- - smaller and higher charges than Na + & Cl-)
- Stronger & melting points higher- ions smaller/ higher charges.
- Definition
- Covalent
- Definition
- Shared pair of electrons
- Dative Covalent
- Forms
- Shared pair of electrons in covalent bond from 1 of bonding atoms. - also called Co-ordinate.
- E.g. NH4+, H3O, NH3BF3
- Shape in NH4+ - tetrahedral
- Direction of arrow from atom providing lone pair to atom deficient
- Forms
- Definition
- Metallic
- Definition
- Electrostatic force of attraction between positive metal ions & delocalised electrons.
- 3 factors affect strength of bond
- 1. No of Protons/ nuclear attraction - more - stronger
- 2. No. of delocalised electrons per atom (outer electrons) - more- stronger
- 3. Size of ion - smaller- stronger
- Example
- Mg stronger metallic bonding than Na - higher melting point.
- Mg- more electrons in outer shell released to delocalised electrons.
- Mg ion - smaller & 1 more proton - stronger electrostatic attraction & higher energy needed to break bonds
- Mg- more electrons in outer shell released to delocalised electrons.
- Mg stronger metallic bonding than Na - higher melting point.
- Definition
- Ionic
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