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Covalent (Molecular) Bonds

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.

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Covalent (Molecular) Bonds

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  1. Covalent (Molecular) Bonds

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

  3. 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

  4. 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!

  5. 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 -)

  6. 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

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

  8. Single Bond Example #2 • H2O

  9. Single Bond Example #3 • CH4

  10. Double Bond Example #1 • CO2

  11. Double Bond Example #2 • NO

  12. Triple Bond Example #1 • N2

  13. Triple Bond Example #1 • HCN

  14. 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)

  15. Carbon tetrachloride (CCl4) Ammonia (NH3)

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

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

  18. Carbon dioxide (CO2) Ethyne (C2H2)

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

  20. Naming Covalent Bonds

  21. 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

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

  23. Practice • NCl3 • N2H4 • CS2 • N2O3 • Cl2O7 • S2F10 • Cl4

  24. Practice-ANSWERS • NCl3 Nitrogen trichloride • N2H4 dinitrogentetrahydride • CS2 carbon disulfide • N2O3 dinitrogen trioxide • Cl2O7 dichlorineheptoxide • S2F10 disulfurdecafluoride • Cl4 tetrachloride

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