GPS 9 Formula Writing and Nomenclature

Targets CH-3a I can name binary covalent (molecular) compounds. I can name binary ionic compounds using Roman numerals for oxidation numbers when appropriate. I can use the following polyatomic ions for naming of ionic compounds:  Carbonate  Sulfate  Nitrate  Hydroxide  Phosphate  Ammonium  Chlorate  Acetate

Targets CH-3c I can explain the Law of Multiple Proportions. I can write chemical formulas, including the following common substances: I can use polyatomic ions for writing formulas of ionic compounds:  Ammonia  Water  Carbon monoxide  Carbon dioxide  Sulfur dioxide  Carbon tetrafluoride  Carbonate  Sulfate  Nitrate  Hydroxide  Phosphate  Ammonium  Chlorate  Acetate

Targets CH-6a I can describe how saturation affects shape and reactivity of carbon compounds. I can draw Lewis dot structures, identify geometries, and describe polarities of the following: I can identify and name simple alkanes, alkenes, and alkynes. I can identify organic functional groups.  CH 4  C 2 H 6  C 2 H 4  C 2 H 2  C 6 H 6  CH 3 COOH  CH 3 CH 2 OH  CH 2 O  Alcohol  Acid  Aldehyde  Ester  Ether

Practice p. 2 Resource Notes Write formulas for compounds containing the following ions: 1.B +3 and Cl -1 2.Cu +2 and O -2 3.Al +3 and Br -1 4.Fe +2 and C 2 H 3 O Ca +2 and SO K +1 and PO 4 -3

Practice p.2 Resource Notes Assign oxidation numbers, then write formulas for compounds containing the following ions: 1.magnesium and chlorine 2.francium and sulfur 3.cesium and sulfate 4.aluminum and nitrate 5.sodium and phosphate 6.calcium and carbonate

Practice p. 3 Resource Notes (Hint: Underline all transition metals, lead and tin and circle all polyatomic ions to help with naming) 1.NaBr 2.Sc(OH) 3 3.NH 4 F 4.CaCO 3 5.NiPO 4 6.Li 2 SO 4 7.Sr(C 2 H 3 O 2 ) 2 8.Cu 2 O 9.CuNO 3 10.LiMnO 4

Practice p. 4 Resource Notes 1.N 3 O 7 2.PCl 5 3.NO 4.BF 3 5.P 2 O 6.BeCl 2

Practice p. 4 Resource Notes 1.Pentacarbon decahydride 2.Diphosphorus octachloride 3.Carbon tetrachloride 4.Triboron hexahydride

Common Substances Water Ammonia Methane

Types of Formulas

Law of Definite Proportions States that regardless of the amount, a pure compound always contains the same elements in the same proportions by mass.

Law of Multiple Proportions States that when one element combines with another to form more than one compound, the mass ratios of the elements in the compounds are simple whole numbers of each other.

Organic Chemistry Study of carbon-containing compounds Watch

Hydrocarbons Any compound containing only hydrogen and carbon Example: methane, CH 4 Classified by the type of bonds that connect the carbon atoms

Alkane hydrocarbon with only single bonds connecting the carbon atoms Example:

Alkene Hydrocarbon that contains at least one double bond Example:

Alkyne hydrocarbon that contains at least one triple bond Example:

Naming Organic Compounds 1.Draw the structural formula to determine bond types. 2.Name using appropriate root depending on the number of carbons and suffix depending on bond type between carbon atoms. # of C RootMeth-Eth-Prop-But-Pent-Hex-Hept-Oct-Non-Dec-Undec-Dodec- Bond Type between carbon atoms Alkane, Alkene, or Alkyne Suffix All single bondsAlkane-ane At least one double bondAlkene-ene At least one triple bondAlkyne-yne

Naming Organic Compounds CH 4 C 2 H 6 C 3 H 6 C 2 H 4 1.Draw the structural formula to determine bond types. 2.Name using appropriate root depending on the number of carbons and suffix depending on bond type between carbon atoms.

Functional Groups

Alcohol, Aldehyde, Ketone, Ether, Ester, or Carboxylic Acid? Ketone Alcohol

Alcohol, Aldehyde, Ketone, Ether, Ester, Carboxylic Acid Ketone

Alcohol, Aldehyde, Ketone, Ether, Ester, or Carboxylic Acid? Carboxylic Acid Aldehyde

Alcohol, Aldehyde, Ketone, Ether, Ester, or Carboxylic Acid? Ether

Alcohol, Aldehyde, Ketone, Ether, Ester, Carboxylic Acid Ester

Identify all functional groups present by circling the functional group and giving name of functional group.