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POLAR COVALENT BONDS

POLAR COVALENT BONDS ATOMS WITH SIMILAR ATTRACTIONS FOR ELECTRONS (ELECTRON AFFINITY) WILL SHARE ELECTRONS TO FORM COVALENT BONDS. THIS WOULD INCLUDE ELEMENTS CLOSE TOGETHER ON THE PERIODIC TABLE.

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POLAR COVALENT BONDS

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  1. POLAR COVALENT BONDS ATOMS WITH SIMILAR ATTRACTIONS FOR ELECTRONS (ELECTRON AFFINITY) WILL SHARE ELECTRONS TO FORM COVALENT BONDS. THIS WOULD INCLUDE ELEMENTS CLOSE TOGETHER ON THE PERIODIC TABLE. LINUS PAULING, A NOBEL PRIZE WINNING CHEMIST, DEFINED A PROPERTY THAT HE CALLED ELECTRONEGATIVITY – THE ABILITY OF AN ATOM IN A BOND TO ATTRACT A SHARED PAIR OF ELECTRONS.

  2. ATOMS WITH THE SAME OR SIMILAR ELECTRONEGATIVITIES WOULD FORM PURE COVALENT BONDS. • THE RULES ARE: • Non-polar bonds occur when the difference in electronegativity between the two atoms is less than 0.4 • Polar bonds occur when the difference in electronegativity between the two atoms is between 0.4 and 1.7 • Ionic bonds occur when the difference in electronegativity between the two atoms is greater than 1.7

  3. FOR EXAMPLE, IF YOU HAD A BOND BETWEEN CARBON (EN = 2.55) AND HYDROGEN (EN = 2.2), THE DIFFERENCE IS 0.35, SO THE BOND WOULD BE COVALENT. IF YOU HAD A BOND BETWEEN HYDROGEN (EN=2.2) AND OXYGEN (EN = 3.44), THE DIFFERENCE IS 1.24, SO THE BOND IS POLAR COVALENT. IF YOU HAD A BOND BETWEEN SODIUM (EN = 0.93) AND CHLORINE (EN = 3.16), THE DIFFERENCE IS 2.23, SO THE BOND IS IONIC.

  4. BONDS IN WATER ARE POLAR COVALENT. THESE GIVE WATER SOME VERY UNUSUAL PROPERTIES.

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