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Starter. What ions do Chlorine form? Imagine you have 2 chlorine ions – how could they help EACH OTHER to reach a stable state? It might help if you draw out the Lewis structures for 2 chlorine ions!. LET’S FIRST REVIEW IONIC BONDING. K. F. In an IONIC bond,
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Starter • What ions do Chlorine form? • Imagine you have 2 chlorine ions – how could they help EACH OTHER to reach a stable state? • It might help if you draw out the Lewis structures for 2 chlorine ions!
LET’S FIRST REVIEW IONIC BONDING
K F In an IONIC bond, electrons are lost or gained, resulting in the formation of IONS in ionic compounds.
K F
K F
K F
K F
K F
K F
_ + K F
_ + K F The compound potassium fluoride consists of potassium (K+) ions and fluoride (F-) ions
_ + K F The ionic bond is the attraction between the positive K+ ion and the negative F- ion
So what are covalent bonds?
In covalent bonding, atoms still want to achieve a noble gas configuration (8 valence electrons).
In covalent bonding, atoms still want to achieve a noble gas configuration. But rather than losing or gaining electrons, atoms now share an electron pair.
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
Fluorine forms a covalent bond with itself F2
How will two fluorine atoms react? F F
F F Each fluorine atom wants to gain one electron to have 8 valence electrons.
F F Neither atom will give up an electron What’s the solution –what can they do to achieve 8 valence electrons?
F F
F F
F F
F F
F F 8 valence electrons
F F 8 valence electrons circle the electrons for each atom that completes their octets
F F Bysharing the electron pair in the middle, each fluorine atom feels like it has 8 valence electrons circle the electrons for each atom that completes their octets
F F The electron pair in the middle (the circled one) is shared by the two atoms of fluorine. circle the electrons for each atom that completes their octets
F F This is called the bonding pair circle the electrons for each atom that completes their octets
F F It is a single bonding pair circle the electrons for each atom that completes their octets
F F It is called aSINGLE BOND circle the electrons for each atom that completes their octets
F F Single bonds are shown with with a dash circle the electrons for each atom that completes their octets
F F This is the fluorine molecule, F2 circle the electrons for each atom that completes their octets
O2 How will this molecule form?
O O
O O Each atom has two unpaired electrons
O O
O O
O O
O O
O O
O O
O O Both atoms want to gain two electrons.
O O Oxygen atoms are highly electronegative. So both atoms want to gain two electrons.
O O
O O
O O
O O
O O Both electron pairs are shared.
O O 6 valence electrons plus 2 shared electrons = 8 valence electrons
