1. Chapter 7

6.  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+

7.  Most transition metals can have a few different charges.  Example:  Fe 2+, Fe 3+  Fe 2 O 3  FeO

9.  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 -

10.  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-

11.  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

12.  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

13. Chapter 8

16.  CO 2  SO 2  NF 3  CCl 4  What is the formula of Diarsneic trioxide?

17.  Fluorine, and some other common elements, usually exist as a molecule of F 2.  Fluorine’s electron configuration is….  Fluorine’s structure is…

19.  PH 3  HCl  PBr 3  CCl 4  SiH 4  NH 3  NF 3

20.  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-

21.  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