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Quiz 2/9/05

ionic - iron (II) chloride ionic -lead (II) oxide ionic - copper (I) chromate covalent- carbon dioxide covalent- diphosphorous pentoxide covalent- silicon dioxide ionic – iron (II) oxide ionic – sodium chloride covalent – carbon tetrachloride ionic – sodium hydroxide. FeCl 2 PbO

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Quiz 2/9/05

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  1. ionic - iron (II) chloride ionic -lead (II) oxide ionic - copper (I) chromate covalent- carbon dioxide covalent- diphosphorous pentoxide covalent- silicon dioxide ionic – iron (II) oxide ionic – sodium chloride covalent – carbon tetrachloride ionic – sodium hydroxide FeCl2 PbO Cu2CrO4 CO2 P2O5 SiO2 FeO NaCl CCl4 NaOH Quiz 2/9/05 Name all of the following Cl1- Fe? Cl1- O2- Pb? O2- CrO42- Co? CrO42- Co? CrO42-

  2. CO2 covalent carbon dioxide

  3. FeCl2 ionic iron (II) chloride

  4. 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 We will do the lab on Thursday.

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

  6. Naming Organic Compounds meth = 1 eth = 2 prop = 3 but = 4 pent = 5 hex = 6 hept = 7 oct = 8 non = 9 … • Butane = 4 carbons • CH3CH2CH2CH3 • Heptane = 7 carbons • CH3CH2CH2CH2CH2CH2CH3 • Octane = 8 carbons • CH3CH2CH2CH2CH2CH2CH2CH3

  7. 13 c page 178 6 hydrogen atoms 3 carbon atoms

  8. 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

  9. 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.

  10. C6H12O6 H2O2 Hg2I2 C6H14 CH2O HO HgI C2H7 Molecular and Empirical Formulas

  11. Coefficients: How many sets of a particular compound/element • 2 C6H12

  12. Coefficients: How many sets of a particular compound/element • 5 C6H12

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