1. 1.iron (III) bromide 2.calcium oxide 3.nickel (II) chromate 4.carbon disulfide 5.carbon tetrabromide 6.calcium hydroxide 7.diphosphorous pentoxide Quiz 2/9/05 1.FeBr 3 2.CaO 3.NiCrO 4 4.CS 2 5.CBr 4 6.Ca(OH) 2 7.P 2 O 5 Fe ? Br 1- Ni ? CrO 4 2- Br 1- 14 points each

2. Electronegativity: the relative tendency of an atom to attract electrons to itself when participating in a chemical bond. Most bonds have some ionic character. If more than 50% of the time one ion has possession of the electron, the compound is considered ionic. This means that if the difference in electronegativity is greater than 1.67, the compound is considered ionic. The more ionic a bond, the more easily a solution of the compound will conduct electricity. Electricity is defined as the flow of electrons. Do pre-lab for lab 21

3. Ca(OH) 2 Fe 2 O 3 MnO 2 iron I(I) oxide CO carbon dioxide dinitrogen trioxide Li 2 S AsCl 3 Ca 3 N 2 potassium oxide lead (II) oxide GeCl 4 SiC OF 2 CaC 2 iron (III) sulfide magnesium chloride zinc oxide Sr(CN) 2 SO 3 iron (II) sulfide iron (II) sulfite iron (II) sulfate silver oxide PCl 3 NH 4 Cl (NH 4 ) 2 SO 4 BaBr 2 SF 6 BrF 3 GaF 3 IF 5 Pb(NO 3 ) 2 Cr(OH) 3 FeSO 4 ZnSO 4 MnSO 4 Na 2 CrO 4 PbCrO 4 calcium hydroxide iron (III) oxide manganese (IV) oxide FeO carbon monoxide CO 2 N 2 O 3 lithium sulfide arsenic trichloride calcium nitride K 2 O PbO germanium tetra chloride silicon monocarbide oxygen difluoride

4. CaC 2 iron (III) sulfide magnesium chloride zinc oxide Sr(CN) 2 SO 3 iron (II) sulfide iron (II) sulfite iron (II) sulfate silver oxide PCl 3 NH 4 Cl (NH 4 ) 2 SO 4 BaBr 2 SF 6 BrF 3 GaF 3 IF 5 Pb(NO 3 ) 2 Cr(OH) 3 FeSO 4 ZnSO 4 MnSO 4 Na 2 CrO 4 PbCrO 4 barium bromide sulfur hexafluoride bromine tri fluoride gallium trifluoride iodide pentafluoride lead (II) nitrate chromium (III) hydroxide iron (II) sulfate zinc sulfate manganese (II) sulfate sodium chromate lead (II) chromate

5. CaC 2 iron (III) sulfide magnesium chloride zinc oxide Sr(CN) 2 SO 3 iron (II) sulfide iron (II) sulfite iron (II) sulfate silver oxide PCl 3 NH 4 Cl (NH 4 ) 2 SO 4 calcium carbide Fe 2 S 3 MgCl 2 ZnO strontium cyanide sulfur trioxide FeS FeSO 3 FeSO 4 Ag 2 O phosphorous trichloride ammonium sulfate Lab 21: Conductivity of substances

6. Naming Organic Compounds Organic compounds have one or more carbons, surrounded with hydrogens. They may have double or triple bonds, and may include oxygen, or other atoms. They are named by counting the “carbon backbone” and applying a prefix “Functional Groups” provide the rest of the name. meth = 1 eth = 2 prop = 3 but = 4 pent = 5 hex = 6 hept = 7 oct = 8 non = 9 …

7. Naming Organic Compounds Butane = 4 carbons CH 3 CH 2 CH 2 CH 3 Heptane = 7 carbons CH 3 CH 2 CH 2 CH 2 CH 2 CH 2 CH 3 Octane = 8 carbons CH 3 CH 2 CH 2 CH 2 CH 2 CH 2 CH 2 CH 3 meth = 1 eth = 2 prop = 3 but = 4 pent = 5 hex = 6 hept = 7 oct = 8 non = 9 …

8. 13 c page 178 3 carbon atoms 6 hydrogen atoms

9. 13 f page 178 6 carbon atoms 12 hydrogen atoms http://jchemed.chem.wisc.edu/JCESoft/CCA/CCA5/MAIN/1ORGANIC/ORG02/TRAM02/E/NOMOVIE/MISC.HTM

10. Molecular and Empirical Formulas. Molecular: adj. Pertaining to, consisting of, caused by, or existing between molecules. Empirical: adj. 1. Relying upon or derived from observation or experiment. 2. Guided by practical experience and not theory, especially in medicine. Formula: n 1. an established form of words for use in a ceremony or procedure. 3. Chemistry: a. a symbolic representation of the composition or of the composition and structure of a chemical compound. b. The chemical compound so represented. c. A prescription in exact proportion: recipe.

11. Molecular and Empirical Formulas C 6 H 12 O 6 H 2 O 2 Hg 2 I 2 C 6 H 14 CH 2 O HO HgI C2H7C2H7

12. Coefficients: How many sets of a particular compound/element 2 C 6 H 12

13. Coefficients: How many sets of a particular compound/element 5 C 6 H 12