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Covalent Bonding

Covalent Bonding. Covalent Bonding. Involves the sharing of electrons. Occurs between non-metals. General rule to follow: the octet rule – chemical compounds tend to form so that each atom, by gaining, losing, or sharing electrons, has an octet of electrons in the highest main energy level.

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Covalent Bonding

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  1. Covalent Bonding

  2. Covalent Bonding Involves the sharing of electrons. Occurs between non-metals. General rule to follow: the octet rule – chemical compounds tend to form so that each atom, by gaining, losing, or sharing electrons, has an octet of electrons in the highest main energy level. Of course, there are exceptions… Molecules can be illustrated using Lewis dot diagrams (Lewis structures).

  3. Representing Covalent Bonding • Count up the total number of valence electrons. • Draw the ‘skeleton’ of the molecule . • first atom in the formula is the central atom (*unless H), all others are bonded to it. • Draw in bonds. • a bond = 2 electrons. Drawn as a line: X–X • Draw remaining electrons in pairs around the atoms as lone pairs.(starting outside  in) • Check for octets. • ONLYif necessary, move lone pairs to create double (or triple) bonds.

  4. Covalent Bonding Practice Example 1: CBr4 Example 2: PH3

  5. Covalent Bonding Practice Example 3: O2 Example 4: N2

  6. Covalent bonding Practice Example 5: CS2 Example 6: CH3CH2CH3

  7. Covalent Bonding Practice Example 7: CH3CH2Br Example 8: CH2CH2

  8. Covalent Bonding Practice Example 9: CH3CH2OH Example 10: CH3COCH3

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