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Published byBruce Shelton Modified over 9 years ago
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Chapter 7
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Representative elements of the same groups usually have the same ionic charges. Group 1: H +, Li +, Na + Group 2: Be 2+, Mg 2+, Ca 2+ Group 15: N 3-, P 3-, As 3- Group 16: O 2-, S 2-, Se 2- Group 17: F -, Cl -, Br - Transition elements can usually have more than one charge. Example Fe 2+ and Fe 3+
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Most transition metals can have a few different charges. Example: Fe 2+, Fe 3+ Fe 2 O 3 FeO
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Polyatomic ions are ions that are made up of more than one atom. Ammonium: NH 4 + Nitrite: NO 2 - Nitrate: NO 3 - Hydroxide: OH - Hypochlorite: ClO -
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Chlorite: ClO 2 - Chlorate: ClO 3 - Perchlorate: ClO 4 - Carbonate: CO 3 2- Sulfite: SO 3 2- Sulfate: SO 4 2- Peroxide: O 2 2- PO 4 3-
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NH 4 Cl Fe(NO 3 ) 3 TiBr 3 Pb(SO 4 ) 2 Chromium (VI) Phosphate Tin (II) Nitrate Cobalt (III) Oxide Chromium (III) Hydroxide
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Barium Carbonate Aluminum Hydroxide Copper (I) Sulfide Lead (II) Phosphate Zinc (II) Iodide Chromium (III) Sulfite NH 4 Br NaClO 3 Fe 2 S 3 AgNO 3 CuF 2 Ni(ClO) 3 Ru 3 (PO 4 ) 4
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Chapter 8
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CO 2 SO 2 NF 3 CCl 4 What is the formula of Diarsneic trioxide?
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Fluorine, and some other common elements, usually exist as a molecule of F 2. Fluorine’s electron configuration is…. Fluorine’s structure is…
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PH 3 HCl PBr 3 CCl 4 SiH 4 NH 3 NF 3
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To draw a lewis structure of a polyatomic ion we first figure out how many valence electrons we have, then add or subtract electrons to account for the charge. SO 4 2-
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A small group of molecules have have an odd number of valence electrons and be unable to form an octet around each atom. NO 2 An other group of molecules have expanded octets. SF 6
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