Bonding Flashcards
(29 cards)
2 bonds, 0 lone pairs
Linear, 180
3 bonds, 0 lone pair
trigonal planar, 120
2 bonds, 1 lone pair
Bent or Angular <120
4 bond pairs, 0 lone pairs
Tetrahedral, 109.5
3 bond pairs, 1 lone pair
Trigonal pyramid, <109
2 bond pairs, 2 lone pairs
Bent or angular «109
5 bonds, 0 lone pairs
trigonal bipyramidal, 90, 120
4 Bond Pairs, 1 Lone Pair
Seesaw 90, 120
3 bond pairs, 2 lone pairs
T-shaped, 90
2 bond pairs, 3 lone pairs
Linear, 180
6 Bond Pairs, 0 Lone Pairs
Octahedral, 90
5 bond pairs, 1 lone pair
square pyramidal, <90
4 bond pairs, 2 lone pairs
square planar, 90
3 bond pairs, 3 lone pairs
T-shaped, 90
2 bond pairs, 4 lone pairs
Linear 180
Give one reason why ice is less dense than water
Water molecules are held further apart than in liquid water
Coordinate bonding
Shared pair of electron from..
Explain how the lone pairs of electrons on the oxygen atom influences the bond angle on oxygen difluoride
Lone pairs repel more than bond pairs, bond angle will be lower
Explain how permanent dipole-dipole forces arise between hydrogen chloride molecules.
- Differences in electronegativity leads to bond polarity
- Attractions between δ+ on one molecule and δ- on another molecule
Chlorine has a lower boiling point because the forces between the molecules are weak.
Explain how these forces arise between chlorine molecules.
- Random movement of electrons in one molecule creates temporary dipole (creates an imbalance in electron density)
- induces a dipole in neighbouring molecules
- these temporary dipoles attract temporary attraction between δ+ and δ-
Ammonium chloride
Covalent bond
Dative covalent bond
Ionic bond
Describe the structure and bonding in magnesium (2)
- Giant lattice of mg2+ cations
- Electrostatic attractions between cations and delocalised electrons
Ionic bonding
The electrostatic attraction between oppositely charged ions formed by electron transfer
Covalent bond
Share a pair of electrons
