2D: Bonding and Structure
- Created by: Strelly22
- Created on: 15-02-21 17:57
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- 2D: Bonding and Structure
- Bonding
- Ionic bonding
- an electrostatic attraction between oppositely charged ions
- between a metal and a non metal
- Covalent bonding
- the strong electrostatic attraction between a shared pair of electrons and the nuclei of bonded atoms
- determine how many valence electrons each bonding atom has by using the group number on the periodic table
- pair up unpaired electrons between atoms to form covalent bonds
- bonding pair = shared pair of electrons
- lone pair = a pair of electrons in the outer shell not used in bonding
- dative covalent bond = a shared pair of electrons in which the bonded pair has been provided by one of the bonding atoms only
- average bond enthalpy = the average enthalpy change which takes place when breaking by homolytic function one mole of a given type of bond in the molecules of a gaseous species
- Metallic bonding
- the electrostatic attraction between positive metal ions and delocalised electrons
- lattic of positive ions held together by a sea of delocalised electrons
- High mp and bp
- good conductors of electricity when solid or molten
- insoluble in water or non polar solvents (though some metals react to form a soluble product)
- Ionic bonding
- Shapes of molecules
- VSEPR
- Valence electrons in bonding pairs and lone pairs repel each other as far apart as possible
- lone pairs repel slightly more than bonding pairs
- linear
- 2bp, 0lp
- 180
- non linear
- 2 bp, 2lp
- trigonal planar
- 3bp, 0lp
- 120
- tetrahedral
- 4bp, 0lp
- 109.5
- octahedral
- 4bp, 0lp
- 90
- trigonal pyramidal
- 3bp, 0lp
- 107
- VSEPR
- Intermolecular forces
- london Forces
- the more electrons, the stronger the forces
- the the contact area, the stronger the forces
- temporary attraction between molecules
- hydrogen bonding
- polar covalent bond = a bond with a permanent dipole, having positive and negative partial charges on the bonded atoms
- polar molecule = a molecule with an overall dipole, having taken into account any dipoles across bonds and the shape of the molecule
- a strong permanent dipole attraction between a delta positive hydrogen on one molecule and a lone pair on a delta negative O, F or N on a different molecule
- ice floats on water ? open structure / lattic
- permanent dipole dipole interactions
- a small charge difference that does not change across a bond, with partial charges
- electronegativity = the ability of an atom to attract the bonding electrons in a covalent bond
- F = 4, O = 3.5, N = 3, Cl = 3
- london Forces
- Bonding
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