Electrons are shared between 2 or more nonmetal atoms. Can also be between a nonmetal and a metalloid. Ex: H 2 O, CO 2, C 6 H 12 O 6 EN value less than.

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Presentation transcript:

Electrons are shared between 2 or more nonmetal atoms. Can also be between a nonmetal and a metalloid. Ex: H 2 O, CO 2, C 6 H 12 O 6 EN value less than 1.5

Can be solid, liquid, or gas at room temp. Low melting and boiling points Cannot conduct electricity Insoluble in water Polar Covalent bonds – electrons shared unequally (EN difference 0.5 – 1.5) Nonpolar Covalent bonds – electrons shared equally (EN difference 0 – 0.5) Compounds are called “molecules” Creates partial + and – ends

Lewis Dot Structures Octet Rule: All atoms will form bonds in order to have full (8) valence electrons. Except Hydrogen (2) 1.Arrange element symbols so that first atom is in the middle. 2.Draw Lewis dot structures for each element. 3.Circle electrons that will be shared between atoms. 4.Re-draw atoms with lines as shared electrons. Ex: CCl 4 C Cl Cl Cl Cl CCl Cl Cl Cl

Covalent Bonds between 2 elements can vary! 2 pairs shared = DOUBLE bond 3 pairs shared = TRIPLE bond 1 pair of valence electrons shared = SINGLE bond

Add in these examples under doc camera. H 2 O N 2 NH 3 HF CO 2

1.List the prefix and name of 1 st element. Don’t use “mono” on 1 st element! 2.Prefix and name of 2 nd element + -ide ending. Prefixes 1 = mono 2 = di 3 = tri 4 = tetra 5 = penta 6 = hexa 7 = hepta 8 = octa 9 = nona 10 = deca Examples CO 2 S2O3S2O3 N4FN4F CO Carbon monoxide Disulfur trioxide Tetranitrogen monofluoride Carbon dioxide

1.Write the symbol of the first element and subscript to match the prefix. 2.Repeat for 2 nd element. DO NOT SIMPLIFY SUBSCRIPTS! Diatomic elements: H 2 N 2 O 2 F 2 Cl 2 Br 2 I 2 Ex: Triphosphorus pentachloride P 3 Cl 5 Ex: Tricarbon hexasulfide C3S6C3S6 Ex: Antimony tetrabromide SbBr 4

Lewis Dot Sharing  Draw the Lewis Dot structures and show the SHARING of unpaired electrons by circling. Then show the structural formula. 1. C 2 H 4 2. CH 4 5. CO 2 3. N 2 6. CCl 4 8. F 2 4. HCl 7. S 2

Recap of Covalent Bonding!

Example: C 2 H 4 Dicarbon tetrahydride

Example: C 2 O 4 Dicarbon tetroxide

Example: Cl 2 O 2 Dichlorine dioxide