Quiz 2 Structure and Bonding Flashcards
(17 cards)
Tetrahedral Arrangement
- 4 reigons of electron density
- Bond angle between electron reigons=109 degrees
Linear Arrangement
- 2 reigons of electron density
- Bond angle between electron reigons= 180 degrees
Trigonal Planar Arrangement
- 3 reigons of electron density
- Bond angle between electron reigons=120 degrees
Bent/V shape
Number of electron reigons: 4
Tetrahedral arrangement
Results when there are non bonded pairs of electrons
Trigonal Pyramidal shape
Number of electron reigons: 4
Tetrahedral arrangement
Results when there are non bonded pairs of electrons
Tetrahedral shape
Number of electron reigons: 4
Tetrahedral arrangement
Non Polar bonds
occur when there is a small or no difference in electronegativity between the bonded atoms
Polar bonds
occur when there is a greater electronegativity difference between the bonded atoms, thus the more electronegative atom attracts the shared pair of electrons closer to itself leaving each of the atoms with delta charges.
Slightly positive/negative charge
occurs because the more electronegative pulls the shared electron pair away from the other bonded atom,
thus the electron density around the less electronegative atom is pulled towards the more electronegative atom leaving it with a slightly positive/negative charge
Methane
CH4
Electronegativity
A measure of an atom’s ability to attract the shared pair of electrons
VSEPR theory
pairs of electrons that surround the central atom arrange themselves as far as possible to avoid electron electron repulsion. This can be used to predict the shapes of molecules
Dipoles
one side of the molecule possesses a partially negative charge and the other side a partially positive charge
Slightly positive
Less electronegative
Slightly negative
More electronegative
Polar Molecules
Occur when a molecule is asymmetrical
Non Polar Molecules
Occur when a molecule is symmetrical, so the bond dipoles cancel out.
