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Chemical Bonding 2 (Definitions (Electronegativity- relative attraction…
Chemical Bonding 2
Definitions
- Electronegativity- relative attraction that a atom in a molecule has for the shared pair of electrons in a covalent bond
- Polar covalent bond- unequal sharing of the pair of electrons. Causes one end of the bond to be slightly pos & the other slightly negative
- Intramolecular bonding- bonding that takes place within a molecule e.g covalent & polar covalent bonding
- Intemoleculer forces- forces of attraction that exist between molecules e.g van der waals, dipole dipole & hydrogen bonding
- Van der waals forces- weak attractive forces between molecules resulting from the formation of temporary dipoles, only between non-polar molecules
Sigma & Pi bonding
- S- formed by the head on overlap of 2 orbitals
- P- formed by the sideways overlap of p orbitals
- Sigma bonds are stronger than pi bonds as there is more overlapping of orbitals
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VSEPR Theory
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- Shape of a molecule depends on the number of pairs of electrons around the central atom
Definitions
- Dipole-dipole forces- forces of attraction between the neg pole of one polar molecule & the pos pole of another polar molecule
- Hydrogen bonds- particular types of dipole-dipole attractions between molecules in which hydrogen atoms are bonded to nitrogen, oxygen or fluorine
Transition metal
- One that forms at least one ion with a partially filled d sublevel
Molecule
- Group of atoms joined together. Smallest particle of an element that can exist independently
Covalent bond
- Force that involve the sharing of electrons between atoms
Valency
- Number of atoms of hydrogen or any other monovalent element with which each element of the element combines
Bonds
- Linear (180°)
- Triangular Planar (120°)
- Tetrahedron (109.5°)
- Pyramidal (107°)
- V-shaped (104.5°)