ch. 7 ionic and metallic bonding 7.1 ions. i. valence electrons a. # of electrons in highest...
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Ch. 7 Ionic and Metallic Bonding
7.1 Ions
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I. Valence Electrons• A. # of electrons in highest occupied S and P orbitals• B. Based on P.T. location• C. Only valence electrons used in bonding
1 2 3 4 5 6 7 8Valence electrons
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II. Electron Dot Models• A. Write valence electrons as dots around
atomic symbol (maximum 2 e- per side)
• B. Ex. Carbon (4 valence electrons)
Try These:
Sodium (Na) Fluorine (F) Aluminum (Al)
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III. Octet Rule• A. Having 8 valence e- is the most stable
• B. Atoms lose or gain e- to have an octet
• C. Become charged (ions); + cations, - anionsValence: 1 2 3 4 5 6 7 8
Lose or Gain: 1 2 3 3 2 1 0
Charge: +1 +2 +3 -3 -2 -1 0
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IV. Why Form an Ion?• A. Cation Example: Magnesium (12e-)
– Mg atom : 1s2 2s2 2p6 3s2 (loses 2e-)– Mg2+ ion : 1s2 2s2 2p6
• B. Anion Example: Oxygen (8e-)–O atom : 1s2 2s2 2p4 (gains 2e-)–O2- ion : 1s2 2s2 2p6
Octet
Octet
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V. Transition Metals• A. Can form pseudo-noble gas configurations
• B. Ex. CopperCu (29 e-) 1s2 2s2 2p6 3s2 3p6 4s2 3d9 is what you
would expect
Actual config: 1s2 2s2 2p6 3s2 3p6 4s1 3d10 (because full D more stable than full S)
Lose 1 e- from 4s: 1s2 2s2 2p6 3s2 3p6 ___ 3d10 (Cu+)
Pseudo-Noble gas Configuration
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7.2 Ionic Bonds and Ionic Compounds
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I. Formation• A. Ionic Bonds: electrostatic attractions
between oppositely charged ions
• B. Ionic compounds neutral, opposite charges cancel
• C. Example: Sodium (Na) and Chlorine (Cl)
•D. Na+ and Cl- will form ionic bonds to become NaCl
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II. Using Electron Dot Models• A. Electron dot models can show ionic bonding• B. Example: Sodium (Na) and Oxygen (O)
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III. Properties• A. Most ionic compounds form crystals in solid state• B. Formula unit: lowest ratio of cations to anions
• C. Strong bonds, cause high melting temperatures
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7.3 Metallic Bonds
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I. Metallic Bonds Properties• A. Attraction between valence electrons and
positively charged metal ions• B. free floating valence electrons (“sea of electrons” allow metals to be molded (malleability)
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II. Metal Crystals• A. Body-centered cubic: metal in middle
of cube and at each corner• B. Face-centered cubic: in center of each side and at corners• C. Hexagonal close-packed: metals in
hexagon shape with three in middle
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III. Alloys• A. Mixture of a metal and other elements• B. Ex. Brass = Copper and Zinc• C. Better properties than their parts• D. Elements can replace metals (substitutional)
or be incorporated into the spaces between them (interstitial)
Substitutional Alloy Interstitial Alloy