2.2 Intermediate Bonding and Bond Polarity

Electronegativity
1. The measure of attraction of an atom in a molecule for a pair of electrons in a covalent bond
2. The Pauling Scale- electronegativity increases across a period and down a group, making flourine the most electronegative element
Ionic and Covalent bonding
1. They are the extremes of a continuum of bonding type
2. To find what degree a bond in a molecule is covalent or ionic, find the difference in electronegativity then use a table to find the result
3. Less electronegative is covalent, more elctronegative is ionic
Polar bonds
1. The more electronegative element atom attracts the electron pair more so it will have a delta negative charge whilst the other atom has a lesser share of the elctron pair so has a delta positive charge.
2. A covalent bond in which there is a separation of charge (one end delta negative and the other delta positive)
3. Can only form between two different molecules as two of the same molecules have the same amount of electronegativity so the electron charge is in the middle
4. The more electronegative a molecule, the more the elctron pair will move towards it, making it more ionic than covalent
Polar molecules
1. Just because a molecule has polar bonds, it doesn't mean that it a polar molecule
2. Lacks symmetry, is linear, has a single H atom, has an OH at one end, has an end at one end.
3. Uneven distribution of charge- if negative is on the outside and positive on the inside then the molecule will not be polar
Non-polar molecule
1. Symmetrical, an element or a carbon compound

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2.2 Intermediate Bonding and Bond Polarity

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