electonegativity and polarity
- Created by: jp3louis
- Created on: 09-11-16 19:42
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- Electronegativity and polarity
- Polarity
- Non- polar bonds
- The bonded electron is shared equally between bonded atoms.
- A bond is non-polar when the bonded atoms have similar electronegativity numbers.
- A non-polar bond in H,O or Cl is called a pure covalent bond
- An example of a pure covalent bond is hydrogen chloride. h has a 2.1 electronegativity whereas cl has 3.0.
- The separation of charges is called a dipole. A dipole in a polar covalent bond doesn't change so its a permanent dipole
- Non- polar bonds
- Electronegativity
- Definition: The attraction of a bonded atom for a pair of electrons in a covalent bond.
- The bonded pair of electrons is shared equally unless
- The nuclear charges are different
- Atoms are different sizes
- Shared electrons may be closer to one nucli than the other
- How is it measured?
- The pauling scale - across the table where the nuclear charge increases and the atomic radius decreases
- Ionic or covalent?
- If electronegativity is large, one bonded atom will have a much greater attraction for the shared pair.
- Covalent = no difference (0) Polar covalent = 0 to 1.8 difference. Ionic is then anything more than 1.8
- Quick points
- Big differences in electronega' means the compound is most likely ionic
- Polar - uneven distribution of charge.
- When drawing the dipole arrows, the arrows will cancel eachother out(like H2O)
- Non-polar - bonded e- pair is shared equally.
- When drawing the dipole arrows, the arrows will not cancel eachother out. Like Co2
- Polarity
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