Covalent (Molecular) Bonds

Covalent (Molecular) Bond Definition Covalent –“sharing, valence electrons” Non-metals bonded to non-metals Bond based on shared electrons between two atoms Forms a molecule (hence the name)

Covalent (Molecular) Bond Properties Very strong bond, however often not a strong force of attraction between molecules. As a result molecular compounds have the lowest melting/boiling points

Types of Covalent Bonds Single- one shared pair of e- Double- two shared pairs of e- Triple- three shared pairs of e- Strength: 3>2>1 Q:How do you know what types will form? A:Use VSEPR!

Drawing Covalent Bonds using V.S.E.P.R. Valence Shell Electron Pair Repulsion According to VSEPR theory, the repulsion between electron pairs causes molecular shapes to adjust so that the valence-electron pairs stay as far apart as possible. -Like repels like (+ repels +)(- repels -)

VSEPR Steps: Place either the single element or the C in the middle and arrange the others around it Draw the Lewis Dot Diagram for each element Draw a line connecting the valence electrons to represent one pair of electrons until each element fulfills the octet rule

Single Bond Example #1 F2 -Group 17 diatomic molecules are single bonds and formed this way!

Single Bond Example #2 H2O

Single Bond Example #3 CH4

Double Bond Example #1 CO2

Double Bond Example #2 NO

Triple Bond Example #1 N2

Triple Bond Example #1 HCN

On notebook paper, use VSEPR to draw the following: Carbon tetrachloride (CCl4) Ammonia (NH3) Water (H2O) Nitrogen (N2) Hydrogen (H2) Phosphorous trichloride (PCl3) Carbon dioxide (CO2) Ethyne (C2H2)

Carbon tetrachloride (CCl4) Ammonia (NH3)

Water (H2O) Nitrogen (N2) . . . __ . __ __ N N .

Hydrogen (H2) Phosphorous trichloride (PCl3) __ H H

Carbon dioxide (CO2) Ethyne (C2H2)

 Drill Decide whether each substance is composed of covalent or ionic bonds. 1. Methane CH4 2. Carbon Dioxide CO2 3. Potassium Bromide KBr

Naming Covalent Bonds

Steps to Naming Covalent Bonds Write name of first element Use prefix if there’s more than 1 Write name of second element, changing ending to “ide” Use prefix always

Prefixes 1 mono- 2 di- 3 tri- 4 tetra- 5 penta- 6 hexa- 7 hepta- 8 octa- 9 nona- 10 deca-

Practice NCl3 N2H4 CS2 N2O3 Cl2O7 S2F10 Cl4

Practice-ANSWERS NCl3 Nitrogen trichloride N2H4 dinitrogen tetrahydride CS2 carbon disulfide N2O3 dinitrogen trioxide Cl2O7 dichlorine heptoxide S2F10 disulfur decafluoride Cl4 tetrachloride