Topic 2 Bonding Flashcards
Molecular formula of these ions:
Hydroxide, Nitrate, ammonium, sulfate, carbonate
OH-, NO3 -,NH4 +, SO4 2-, CO3 2-
Why do ionic compounds dissolve
Water is polar so can attract positive and negative ions to break up the structure.
In what state are ionic compounds conductors and why
Liquid (molten or dissolved) as ions are free to move and carry charge
What determines strength of ionic lattices
Charge density (small highly charged are stronger)
Are double bonds stronger than single
Yes - higher electron density
Shape and bond angle with 2 bonding pairs
Linear 180
Shape and bond angle with 3 bonding pairs
Trigonal planar 120
Shape and bond angle with 4 bonding pairs
Tetrahedral 109.5
Shape and bond angle with 5 bonding pairs
Trigonal bipyramidal 90,120
Shape and bond angle with 6 bonding pairs
Octahedral 90
Shape and bond angle with 2 bonding pairs and 1 lone pair
Bent 118
Shape and bond angle with 3 bonding pairs and 1 lone pair
Pyramidal 107
Shape and bond angle with 2 bonding pairs and 2 lone pairs
Bent 104.5
Shape and bond angle with 4 bonding pairs and 1 lone pair
Distorted tetrahedral 88, 118
Shape and bond angle with 3 bonding pairs and 2 lone pairs
T shaped 88,178
Shape and bond angle with 5 bonding pairs and 1 lone pair
Square pyramidal 88,178
Shape and bond angle with 4 bonding pairs and 2 lone pairs
Square planar 90,180
What 4 things does metallic bonding strength depend on
Size of ion, charge of ion, number of delocalised electrons and charge density
Three things required for a substance to dissolve
- Substance bonds must break
- Solvent bonds must break
- Bonds form between solvent and solute
Give an example of an ionic compound that doesn’t dissolve
Al2O3
Name 6 compounds that contain coordinate bonds
- NH4 +
- H3O +
- AlCl4 -
- Al2Cl6
- BNF6
6.NO3 -
