Covalent Bond

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Slide 1: 

BONDING

Slide 2: 

Covalent Bonds

Slide 3: 

LET’S FIRST REVIEW IONIC BONDING

Slide 4: 

In an IONIC bond, electrons are lost or gained, resulting in the formation of IONS in ionic compounds.

Slide 5: 

F K

Slide 6: 

F K

Slide 7: 

F K

Slide 8: 

F K

Slide 9: 

F K

Slide 10: 

F K

Slide 11: 

F K

Slide 12: 

F K The compound potassium fluoride consists of potassium (K+) ions and fluoride (F-) ions

Slide 13: 

F K + _ The ionic bond is the attraction between the positive K+ ion and the negative F- ion

Slide 14: 

So what are covalent bonds?

Slide 15: 

In covalent bonding, atoms still want to achieve a noble gas configuration (the octet rule).

Slide 16: 

In covalent bonding, atoms still want to achieve a noble gas configuration (the octet rule). But rather than losing or gaining electrons, atoms now share an electron pair.

Slide 17: 

In covalent bonding, atoms still want to achieve a noble gas configuration (the octet rule). But rather than losing or gaining electrons, atoms now share an electron pair. The shared electron pair is called a bonding pair

Slide 18: 

Cl2 Chlorine forms a covalent bond with itself

Slide 19: 

Cl Cl How will two chlorine atoms react?

Slide 20: 

Cl Cl Each chlorine atom wants to gain one electron to achieve an octet

Slide 21: 

Cl Cl Neither atom will give up an electron – chlorine is highly electronegative. What’s the solution – what can they do to achieve an octet?

Slide 22: 

Cl Cl

Slide 24: 

Cl Cl

Slide 25: 

Cl Cl

Slide 26: 

Cl Cl octet

Slide 27: 

Cl Cl circle the electrons for each atom that completes their octets octet

Slide 28: 

Cl Cl circle the electrons for each atom that completes their octets The octet is achieved by each atom sharing the electron pair in the middle

Slide 29: 

Cl Cl circle the electrons for each atom that completes their octets The octet is achieved by each atom sharing the electron pair in the middle

Slide 30: 

Cl Cl circle the electrons for each atom that completes their octets This is the bonding pair

Slide 31: 

Cl Cl circle the electrons for each atom that completes their octets It is a single bonding pair

Slide 32: 

Cl Cl circle the electrons for each atom that completes their octets It is called a SINGLE BOND

Slide 33: 

Cl Cl circle the electrons for each atom that completes their octets Single bonds are abbreviated with a dash

Slide 34: 

Cl Cl circle the electrons for each atom that completes their octets This is the chlorine molecule, Cl2

Slide 35: 

O2 Oxygen is also one of the diatomic molecules

Slide 36: 

How will two oxygen atoms bond?

Slide 37: 

Each atom has two unpaired electrons

Slide 44: 

Oxygen atoms are highly electronegative. So both atoms want to gain two electrons.

Slide 45: 

Oxygen atoms are highly electronegative. So both atoms want to gain two electrons.

Slide 50: 

O O Both electron pairs are shared.

Slide 51: 

6 valence electrons plus 2 shared electrons = full octet O O

Slide 52: 

6 valence electrons plus 2 shared electrons = full octet O O

Slide 53: 

two bonding pairs, O O making a double bond

Slide 54: 

For convenience, the double bond can be shown as two dashes.

Slide 55: 

This is the oxygen molecule, O2