1. Ionic Compound Molecular Compound Ionic Compounds are the result of oppositely charged ions attracting to each other after an electron transfer has occurred. This occurs between metals and non-metals. Molecular compounds form when two non-metals share their valence electrons with each other in order to fulfill the octet rule. Sec. 9.3, 9.4 & 22.1: Naming and Writing Compounds (Nomenclature)

2. I. Naming compounds made from atoms of the same element. Compounds such as these are called diatomic molecules and can be simply named using their elemental names. H 2 - HydrogenF 2 - FluorineI 2 - Iodine N 2 - NitrogenCl 2 - Chlorine O 2 - OxygenBr 2 - Bromine Sec. 9.3, 9.4 & 22.1: Naming and Writing Compounds (Nomenclature)

3. II. Naming molecular compounds made from atoms of two different elements (Binary Compounds). Example: CCl 4 1-mono 2-di 3-tri 4-tetra 5-penta 6-hexa 7-hepta 8-octa 9-nano 10-deca carbonchlorine carbontetrachloride carbon tetrachloride Sec. 9.3, 9.4 & 22.1: Naming and Writing Compounds (Nomenclature)

4. Name the following compounds: 1.NO____________________________ 2.N 2 ____________________________ 3.BCl 3 ____________________________ 4.CsI____________________________ 5.Li 2 O____________________________ 6.SO 2 ____________________________ 7.Al 2 O 3 ____________________________ 8.F 2 ____________________________ nitrogen monoxide nitrogen boron trichloride cesium iodide lithium oxide sulfur dioxide aluminum oxide fluorine Sec. 9.3, 9.4 & 22.1: Naming and Writing Compounds (Nomenclature)

5. Ionic Compounds Molecular Compounds Example: Potassium Oxide 1.) Write the symbol and charge of each ion. K +1 O -2 2.) Criss-Cross the oxidation numbers so that they become the other ion’s subscript. K 2 O 1 3.) Reduce subscripts, if necessary, and write formula. K2OK2O Example: Dinitrogen Pentoxide 1.) Write the symbol of each element. NONO 2.) Each prefix identifies the number used for the subscript. 25 3.) Write formula. N2O5N2O5 Sec. 9.3, 9.4 & 22.1: Naming and Writing Compounds (Nomenclature)

6. Write formulas for each compound below: 1.sodium peroxide__________________________ 2.potassium chloride__________________________ 3.carbon tetrachloride__________________________ 4.silicon dioxide__________________________ 5.lead (IV) chloride__________________________ 6.lithium acetate__________________________ 7.aluminum carbonate__________________________ 8.dinitrogen pentoxide__________________________ Na 2 O 2 KCl CCl 4 SiO 2 PbCl 4 LiC 2 H 3 O 2 Al 2 (CO 3 ) 3 N2O5N2O5 Sec. 9.3, 9.4 & 22.1: Naming and Writing Compounds (Nomenclature)

7. * An acid is any compound that has hydrogen as the first element listed in the formula. Examples: HCl, HF, HNO 3, HBr, etc. Example #1: HCl Example #2: HNO 3 Example #3: HClO 2 Common Name: hydrogen chloride Acid Name: 1. Replace hydrogen with the prefix hydro- 2. Change chloride’s ide to ic. 3. Add the word acid hydrochloric acid Common Name: hydrogen nitrate Acid Name: 1. Drop the word hydrogen 2. Change the “ate” of nitrate to “ic”. 3. Add the word acid nitric acid Common Name: hydrogen chlorite Acid Name: 1. Drop the word hydrogen 2. Change the “ite” of chlorite to “ous”. 3. Add the word acid chlorous acid Sec. 9.3, 9.4 & 22.1: Naming and Writing Compounds (Nomenclature)

8. Name the following acids: 1.HI______________________________ 2.HIO 3 ______________________________ 3.HF______________________________ 4.HNO 2 ______________________________ 5.HNO 3 ______________________________ 6.HClO 4 ______________________________ 7.HClO______________________________ 8.HCl ______________________________ hydroiodic acid iodic acid hydrofluoric acid nitrous acid nitric acid perchloric acid hypochlorous acid hydrochloric acid Sec. 9.3, 9.4 & 22.1: Naming and Writing Compounds (Nomenclature)

9. Example: Write formulas for the following acids: hydrochloric acidchloric acidchlorous acid 1. The prefix hydro- identifies this acid as being hydrogen bonded to a typical anion. Identify the anion: chloride “ic” becomes “ide” 2. Identify the ions in the acid. H +1 Cl -1 3. Criss-Cross HCl 1. The absence of the prefix hydro- identifies this acid as being hydrogen bonded to a poly-atomic anion. Identify the anion: “ic” becomes “ate” chlorate 2. Identify the ions in the acid. H +1 ClO 3 -1 3. Criss-Cross HClO 3 1. The absence of the prefix hydro- identifies this acid as being hydrogen bonded to a poly-atomic anion. Identify the anion: “ous” becomes “ite” chlorite 2. Identify the ions in the acid. H +1 ClO 2 -1 3. Criss-Cross HClO 2 Sec. 9.3, 9.4 & 22.1: Naming and Writing Compounds (Nomenclature)

10. Write formulas for the following acids: 1.hydrofluoric acid______________________________ 2.carbonic acid______________________________ 3.nitric acid______________________________ 4.acetic acid______________________________ 5.nitrous acid______________________________ 6.hydrophosphoric acid______________________________ 7.phosphoric acid______________________________ 8.hydrosulfuric acid______________________________ HF H 2 CO 3 HNO 3 HC 2 H 3 O 2 HNO 2 H3PH3P H 3 PO 4 H2SH2S Sec. 9.3, 9.4 & 22.1: Naming and Writing Compounds (Nomenclature)

11. Names and Formulas for Bases Bases are compounds containing the OH -1 (hydroxide ion) NaOH is sodium hydroxide Ca(OH) 2 is calcium hydroxide To write the formula: 1)Write the symbol for the metal cation 2)followed by the formula for the hydroxide ion (OH 1- ) 3)then use the criss-cross method to balance the charges. Sec. 9.3, 9.4 & 22.1: Naming and Writing Compounds (Nomenclature)

12. Practice by writing the formula for the following: Magnesium hydroxide Iron (III) hydroxide Zinc hydroxide Sec. 9.3, 9.4 & 22.1: Naming and Writing Compounds (Nomenclature)

13. Hydrocarbons are molecular compounds that contain only two different elements, hydrogen and carbon. Examples: CH 4, C 5 H 10, C 3 H 8, etc. 1 meth- 2 eth- 3 prop- 4 but- 5 pent- 6 hex- 7 hept- 8 oct- 9 non- 10 dec- Alkane Alkene Alkyne C 2 H 6 C 2 H 4 C 2 H 2 1. Identify # of carbons and assign prefix. 2 (eth-) 2. Identify relationship between # of carbons and hydrogens. C n H 2n+2 (-ane) C n H 2n (-ene) C n H 2n-2 (-yne) ethane ethene ethyne Sec. 9.3, 9.4 & 22.1: Naming and Writing Compounds (Nomenclature)

14. Name the following hydrocarbons: 1.CH 4 ______________________________ 2.C 3 H 8 ______________________________ 3.C 2 H 2 ______________________________ 4.C 4 H 8 ______________________________ 5.C 7 H 16 ______________________________ 6.C 10 H 18 ______________________________ 7.C 9 H 18 ______________________________ 8.C 6 H 14 ______________________________ methane propane ethyne butene heptane decyne nonene hexane Sec. 9.3, 9.4 & 22.1: Naming and Writing Compounds (Nomenclature)

15. When trying to write formulas for hydrocarbons you must remember the prefixes and the carbon to hydrogen relationships. 1 meth- 2 eth- 3 prop- 4 but- 5 pent- 6 hex- 7 hept- 8 oct- 9 non- 10 dec- C n H 2n+2 (-ane) C n H 2n (-ene) C n H 2n-2 (-yne) Examples: 1.propene 2.hexyne 3.butane C3H6C3H6 C 6 H 10 C 4 H 10 Sec. 9.3, 9.4 & 22.1: Naming and Writing Compounds (Nomenclature)

16. Write Formulas for the Following Hydrocarbons: 1.ethyne______________________________ 2.propane______________________________ 3.decane______________________________ 4.heptene______________________________ 5.pentane______________________________ 6.butyne______________________________ 7.ethene______________________________ 8.methane______________________________ C2H2C2H2 C3H8C3H8 C 10 H 22 C 7 H 16 C 5 H 12 C4H6C4H6 C2H4C2H4 CH 4 Sec. 9.3, 9.4 & 22.1: Naming and Writing Compounds (Nomenclature)