html5-img
1 / 12

Chapter 5

Chapter 5. Chemical Bonds, Nomenclature, Lewis Structure and Molecular Shapes. 75%. % Ionic Character. 50%. 25%. Electronegativity difference. I. Chemical Bonds B. Ionic Bonds.

keita
Download Presentation

Chapter 5

An Image/Link below is provided (as is) to download presentation Download Policy: Content on the Website is provided to you AS IS for your information and personal use and may not be sold / licensed / shared on other websites without getting consent from its author. Content is provided to you AS IS for your information and personal use only. Download presentation by click this link. While downloading, if for some reason you are not able to download a presentation, the publisher may have deleted the file from their server. During download, if you can't get a presentation, the file might be deleted by the publisher.

E N D

Presentation Transcript

  1. Chapter 5 Chemical Bonds, Nomenclature, Lewis Structure and Molecular Shapes

  2. 75% % Ionic Character 50% 25% Electronegativity difference

  3. I. Chemical Bonds B. Ionic Bonds • Know: Metals combine with nonmetals & form ionic bonds by losing or gaining electrons to mimic closest Inert Gas (VIIIA). IA - Na, K, Li, etc become +1 ions: Na+ IIA - Ca, Mg, etc become +2 ions: Ca+2 IIIA - Al, Ga become +3 ions: Al+3 VA - N, P become -3 ions: N-3 VIA - O, S become -2 ions: O-2 VIIA - F, Cl, Br, I become -1 ions: F-1 • Opposite ions attract in a ratio so that the product is neutral. Inert Gas e- Configurations

  4. I. Chemical Bonds B. Ionic Bonds Example Do not show charges in final formula. NaCl NOT Na+Cl-

  5. I. Chemical Bonds B. Ionic Bonds Example

  6. I. Chemical Bonds B. Ionic Bonds -Examples Na+ + Na+ + O-2Na2O Ca+2+F- + F-CaF2 Mg+2 + S-2 MgS Al+3 + Al+3 + O-2 + O-2 + O-2 Al2O3 Give the formulas for the following: Na & Br Ca & O Ba & I Li & O Al & F Mg & N Many transition metals form ionic bonds & can have several charges such as Fe+2 = Iron (II)Fe+3 = Iron (III). Do not need to know these.

  7. I. Chemical Bonds C. Electron Dot (Lewis) Strucures - A Lewis electron dot structure is a symbol in which the valence electrons are shown as dots. - Examples: Na. Mg: Na+ Ca2+ H:1- (Called Hydride) :C: :Si: - How many valence electrons (dots) would N3- O2- F- or Ne have? What about Mg+2?

  8. II. Covalent Bonds A. Introduction EN = electronegativity - Definition of a covalent bond: A bond formed by the sharing of two electrons. • When two atoms of similar EN combine, neither has the “pull” to take electrons away & a sharing of electrons results. • This occurs when NONMETALS combine with NONMETALS.Note: H is a nonmetal. • Example: H. + H. ---) H—H = H2 - The atoms share valence electrons to get stable group VIIIA e- configurations.

  9. II. Covalent Bonds A. Introduction • Covalent bond = sharing of 2 electrons. • 2 shared electrons with (Single Bond). • 4 shared electrons with (Double Bond). • 6 shared electrons with (Triple Bond). • We frequently show the structure as a Lewis Structure - covalent bonds with lines and nonbonding valence electrons as dots. - Note: Group IVA usually forms 4 bonds; VA three bonds; VIA two bonds; and VIIA (along with H) one bond.

  10. II. Covalent Bonds B. Examples H. + F::: ---) H F::: H. + O + .H ---) H O H :N + N: ---) :N N: :::Cl. + .O. + .Cl::: ---) :::Cl O Cl::: ::O: + :C: + :O:: -----) ::O = C = O::

  11. II. Covalent Bonds C. Lewis Structures 2. Examples H I H2O NH4+ H2O2 CH4 SO2 AlCl4- NO2- CN-

  12. Bonding SummaryTwo General Bonding Types • Ionic: Compound containing metallic element. Atoms lose/gain e to look like nearest inert gas. Add together ions such that neutralize charge. Ia IIa IIIa Va VIa VIIa +1 +2 +3 -3 -2 -1 2. Covalent: Compound containing nonmetals. Atoms obtain inert gas configuration by sharing valence electrons. : :: :::

More Related