Unit 3 Packet - Page 1 of 23Honors Chemistry - Unit 3Chapter 7 - NomenclatureVocab Due: Polyatomic Ion Quiz(zes): Element Project: Problem Set Due: Test Date:

VOCABULARY: monatomic ion cation anion binary

compoundionic compound transition metal polyatomic ions nomenclaturemolecular compound

molecular formula empirical formula

FORMULAS/CONSTANTS/INFO TO BE MEMORIZED:Charges from periodic table; Common polyatomic ions; Numerical prefixes; Common AcidsOBJECTIVES:Chapter 7 Understand how to find oxidation numbers from the periodic table and be able

to use them in writing formulas. Memorize the common polyatomic ions. Be able to write and name ionic and molecular formulas. Be able to name transition compounds. Be able to identify the location of the metals and nonmetals on the periodic

table. Be able to find oxidation numbers in compounds and polyatomic ions. Know the names of the families on the periodic table

Others: Peroxide: O22- Hydride: H1- Mercury (I): Hg22+

Common Acids

Unit 3 Packet - Page 2 of 23Hydrochloric Acid HCl Sulfuric Acid H2SO4Nitric Acid HNO3 Phosphoric acid H3PO4Acetic Acid HC2H3O2 Carbonic acid H2CO3

Unit 3 Packet - Page 3 of 23Unit 3 PROBLEM SET:

Follow the instructions for the cover page for Problem Sets.Show your work on all problems. Credit will not be given without work. Include units on your answers.

Review Questions:1. An 8.47 g sample of a solid is placed in a 25.00 ml flask. The remaining volume

in the flask is filled with benzene in which the solid is insoluble. The solid and the benzene together weigh 24.54 g. The density of the benzene is 0.879 g/ml. What is the density of the solid?

2. The US quarter has a mass of 5.67 g and is approximately 1.55 mm thick. A. How many quarters would have to be stacked to reach 2421 ft., the height of Pilot Mountain?B. How much money (in $) would this stack contain?

3. What type of energy is released when an electron jumps from the 4th energy level to the 1st energy level in the Bohr’s Model?

3. Copy and fill in the following table:

Element/ion # of protons # of neutrons # of electronsPbCu+

24 21N3-

92 146

5. There is an old method for naming cations (still used by chemical supply companies) where -ic and -ous are used for endings. Research the stannic ion, stannous ion, cuprous ion and cupric ion and explain how this naming system works. What would the formula of stannous nitrate be? What about cuprous sulfate?

6. Name the following compounds:Ba(ClO4)2 Ni(NO3)2Mg(CN)2 Mn2S3

7. Find the oxidation numbers for the elements in each of the above compounds.

8. Write the formulas for the following:A. lead (IV) oxideB. dintirogen pentoxideC. strontium chlorideD. carbon monoxideE. silver nitrateF. ammonium phosphate

Unit 3 Packet - Page 4 of 23Chapter 7 Chemical Formulas and Chemical Compounds

7-1 Chemical Names and Formulas

I. Ionic Compounds (ionic bonds and formula units) VS.Molecules (covalent bonds and molecular formulas)

A. Ionic compounds are composed of metals and nonmetals and are bonded together by ionic bonds.

B. Molecules are composed of nonmetals and nonmetals and are bonded together by covalent bonds.

C. Sample problems: circle the correct answers.

1. CaO2 is a(n) { ionic compound / molecule }. 2. The formula for CaO2 is known as a { formula unit / molecular

formula }3. CaO2 is bonded by { ionic / polar covalent / covalent } bonds. 4. An oxygen molecule, O2, is a(n) { ionic compound / molecule }.5. O2 is bonded by { ionic / polar covalent / covalent } bonds.

II. Chemical Formulas

A. A chemical formula could be either a molecular formula or a formula unit.B. Either way, the chemical formula indicates the relative number of each

atom in a chemical compound.C. Parentheses around a polyatomic ion identify it as one unit and any

subscripts written next to parentheses apply to all the atoms inside the parentheses.

D. Sample problems: circle or fill in the correct answers.

1. Butane, C4H10, is a(n) { ionic compound / molecule } that has carbon atoms and hydrogen atoms.

2. Aluminum oxide, Al2O3, is a(an) { ionic compound / molecule } that has aluminum ions and oxide ions in its simplest ratio.

3. Calcium chlorate, Ca(ClO3)2, has calcium ions Ca2+, chlorate ions ClO3-, chlorine atoms Cl, and oxygen atoms O.

4. Magnesium phosphate, Mg3(PO4)2, has magnesium ions Mg2+, phosphate ions PO43-, phosphorous atoms P, and oxygen atoms O.

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Unit 3 Packet - Page 6 of 23III. Naming monatomic cations – alkali and alkaline-earth metals.

A. Naming ions for alkali and alkaline-earth metals is easy. Just use the element’s name plus the word ion (or cation if you prefer).B. Complete the table:

Atom Ion formed Ion nameLi ________ ____________________________Na ________ ____________________________Mg ________ ____________________________Ca ________ ____________________________

IV. Naming monatomic cations – transition metals

A. When naming ions for transition metals, the Stock system is used; a Roman numeral in parentheses is added to the name to indicate the charge of the ion.

B. For example; Cu1+ is copper(I) and Cu2+ is copper(II).C. Complete the table:

Ion Ion namePb2+ _______________________________Pb3+ ___________________________________ iron(III)____ iron(II)

V. Naming monatomic anions – nonmetals

A. When naming anions for the nonmetals, drop the ending of the elements name and add the suffix –ide.

B. Complete the table;

Atom Ion formed Ion nameF ________ ___________________________I ________ ___________________________O ________ ___________________________N ________ ___________________________

Unit 3 Packet - Page 7 of 23VI. Forming binary ionic compounds

A. In a binary ionic compound the total positive charges must equal the total negative charges. The best way to write correct formula units for ionic compounds is to use the “Criss Cross Method”.

B. Sample problem: What ionic compound would form when calcium ions combine with bromide ions?Steps to the Criss Cross Method:

1. Write the ions with their charges, cations are always first. Ca2+ Br-

2. Cross over the charges by using the absolute value of each ion’s charge as the subscript for the other ion. Ca Br2

3. Check to make sure the subscripts are in the lowest whole number ratio possible. Then write the formula. CaBr2

VII. Naming binary ionic compounds

A. Combine the names of the cation and the anion. B. Example; BaBr2 is named barium bromide.C. First write the ions formed for the following elements. Then use the Criss

Cross method to determine the formula. Then name the compounds.

Elements Ions formedFormula Unit Name1. magnesium and iodine __________ ___________ ________________

2. potassium and sulfur __________ ___________ ________________

3. chlorine and aluminum __________ ___________ ________________

4. zinc and bromine __________ ___________ ________________

5. sulfur and cesium __________ ___________ ________________

6. strontium and oxygen __________ ___________ ________________

7. calcium and nitrogen __________ ___________ ________________

8. calcium and oxygen __________ ___________ ________________

9. copper(I) and oxygen __________ ___________ ________________

10. copper(II) and chlorine __________ ___________ ________________

11. mercury(II) and oxygen __________ ___________ ________________

12. nitrogen and aluminum __________ ___________ ________________

Unit 3 Packet - Page 8 of 23VIII. Naming binary ionic compounds that contain polyatomic ions

A. The polyatomic ions on p. 210 and on your common ions list should be memorized.

B. The most common oxyanions – polyatomic anions that contain oxygen, end in –ate. Oxyanions with one less oxygen end in –ite. For example:

NO3-1 is nitrate SO42- is sulfateNO2-1 is nitrite SO32- is sulfite

C. Anions with one less oxygen than the –ite ion are given the prefix hypo-.D. Anions with one more oxygen than the –ate ion are given the prefix per-.

ClO-1 is hypochlorite ClO3-1 is chlorateClO2-1 is chlorite ClO4-1 is perchlorate

E. Naming compounds with polyatomics is the same as naming other compounds, just name the cation and then the anion. If there is a transition metal involved, be sure to check the charges to identify which ion (+1, +2, +3, +4….) it may be so that you can put the correct Roman numeral in the name. Name the following.

1. NaOH _____________________________

2. KClO3 _____________________________

3. Ca(NO3)2 ___________________________

4. NaCH3COO _________________________

5. NH4NO2 ___________________________

IX. Determining the formula unit when the compound has a polyatomic ionA. Use the Criss Cross Method. Parentheses are used around polyatomic

ion if more than one polyatomic ion is present. Determine the formula for the following;

Ions formed Formula unit

1. potassium hydroxide _____________ ______________

2. ammonium acetate _____________ ______________

3. potassium permanganate _____________ ______________

4. iron(III) nitrate _____________ ______________

5. sodium sulfate _____________ ______________

Unit 3 Packet - Page 9 of 23XI. Naming binary molecular compounds

A. With molecules, the prefix system is used.

Number Prefix1 mono-2 di-3 tri-4 tetra-5 penta-6 hexa-7 hepta-8 octa-9 nona-10 deca-

B. The less-electronegative element is always written first. It only gets a prefix if it has more that one atom in the molecule.

C. The second element gets the prefix and the ending –ide.D. The o or a at the end of the prefix is dropped when the word following the

prefix begins with another vowel, for example monoxide or pentoxide.E. Name the following molecules.

1. As2O5 ___________________________

2. SF6 ___________________________

3. CO ___________________________

4. N2O3 ___________________________

5. CI4 ___________________________

XI. Naming AcidsA. Memorize the names and formulas for the following acids.

HCl hydrochloric acidH3PO4 phosphoric acidHNO3 nitric acidH2SO4 sulfuric acidCH3COOH acetic acidH2CO3carbonic acid

Congratulations! You now know how to name compounds and molecules. All you have to do is practice.

Additional Notes and Practice Examples are located on the chemistry classroom website.

1. Does it start with an H?

Is it Binary?(2 elements)Yes Yes

1. Name like ionic compoundTHEN2. Hydro---------ic Acid

No 1. Name like ionic compoundTHEN2. Drop hydrogen3. ---ate goes to –ic Acid4. ---ite goes to –ous Acid

No

2. Does it have a metal and a nonmetal?

7 NONMETAL?

No1. It is a molecular compound!2. Use prefixes to name it.

Yes

3. It must be ionic! Is the cation in Group 1, 2 or Al, Zn, or Ag?

1. Cation Name plus Anion Name!Cation name plus anion name.Must calculate the charge on the cation!Use Roman numeral to indicate the charge in the name.

Yes

No

Naming Compounds Flow ChartChemical Formula Chemical

Name

Unit 3 Packet - Page 10 of 23

Unit 3 Packet - Page 11 of 23Writing Formulas with the Criss-Cross Method

Write the formulas of the compounds produced from the listed ions.

Unit 3 Packet - Page 12 of 23Naming Ionic Compounds

Name the following compounds using the rules for naming ionic compounds.

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Naming Molecular Compounds

Unit 3 Packet - Page 14 of 23Name the following covalent compounds using the rules for naming binary molecular compounds.

Unit 3 Packet - Page 15 of 23Writing Formulas from Names

Write the formulas for the following compounds.

Unit 3 Packet - Page 16 of 23Writing Chemical Formulas – Mixed Practice

Use the nomenclature rules and the flowchart to write formulas for the following compounds:

1 calcium chloride 23 manganese (II) nitrate

2 calcium carbonate 24 chromium (III) sulfate

3 sodium cyanide 25 ammonium sulfide

4 magnesium oxide 26 iron (II) iodide

5 sodium fluoride 27 phosphorus dinitride

6 zinc iodide 28 dinitrogen monoxide

7 aluminum chloride 29 cerium (III) phosphate

8 rubidium acetate 30 sulfur trioxide

9 cobalt (II) chloride 31 barium nitrite

10 potassium hydride 32 chromium (III) nitride

11 copper (II) carbonate

33 lithium sulfite

12 potassium hydroxide

34 magnesium hydroxide

13 hydrogen bromide 35 dinitrogen trioxide

14 rubidium cyanide 36 strontium hydroxide

15 potassium fluoride 37 magnesium nitrate

16 calcium telluride 38 aluminum sulfate

17 manganese (III) oxide

39 potassium cyanide

18 magnesium phosphate

40 tin (IV) chloride

19 mercury (II) cyanide 41 dinitrogen tribromide

20 nickel (II) oxide 42 carbon tetrachloride

21 potassium nitrate 43 ammonium sulfide

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22 sodium hydroxide 44 mercury (II) chloride

Unit 3 Packet - Page 18 of 23Writing Chemical Formulas – Mixed Practice

Use the nomenclature rules and the flowchart to write formulas for the following compounds:

1 BaCl2 23 Na3PO4

2 Zn(NO3)2 24 NH4Cl

3 CsC2H3O2 25 NaCl

4 H2S (g) 26 NaNO3

5 K2CO3 27 (NH4)2SO4

6 FeCl3 28 Fe(NO3)3

7 Al(NO2)3 29 NaC2H3O2

8 NH4C2H3O2 30 BaSe

9 Ba(OH)2 31 CuSO4

10 Ca(C2H3O2)2 32 FeO2

11 NaOH 33 Cd3P2

12 HCl (aq) 34 N2O5

13 KCl 35 Co3(PO4)2

14 KBr 36 LiH

15 Ga2Te3 37 P2O3

16 Hg2Cl2 38 PCl517 CuSe 39 SF6

18 Pb(CN)2 40 PCl

19 HgI2 41 MgH2

20 NH4NO3 42 MnO

21 Na2SO4 43 P2O3

22 Na2O 44 HNO3

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Assigning Oxidation Numbers:

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Unit 3 Packet - Page 22 of 23Review Sheet-Nomenclature

Chemistry

Answer the following questions.1. Give three examples of elements that are metals. 2. Give three examples of elements that are non-metals. 3. Give three examples of metalloids.

Write the common oxidation number (charge) for the following monoatomic and polyatomic ions.4. silver 5. alkali metals 6. halogens 7. chloride 8. carbonate 9. magnesium 10. nitrate 11. sodium 12. phosphate

Write the chemical formula or name of each of the following compounds. Remember that a compound always has a neutral charge.13. calcium chloride 27. Al2SO4 14. potassium chloride 28. NaF

15. lithium fluoride 29. Li2O 16. barium iodide 30. MgCl2

17. iron (II) nitrate 31. CuO2 18. beryllium carbonate 32. N2O5

19. barium chlorate 33 Find the oxidation numbers for

the 20. cobalt (III) nitride elements in sulfuric acid21. ammonium chloride 22. hydrochloric acid 23. potassium sulfate 24. rubidium phosphate 25. sodium acetate 26. carbon monoxide

Answers:1. various: Li, Na, Cu etc.2. Various, F, Cl, He3. Various, Si, As, Sb4. 1+ 5. 1+ 6. 1- 7. 1- 8. 2- 9. 2+10. 1- 11. 1+ 12. 3- 13. CaCl2 14. KCl 15. LiF16. BaI2 17. Fe(NO3)2 18. BeCO3 19. Ba(ClO3)2 20. CoN 21. NH4Cl22. HCl 23. K2SO4 24. Rb3PO4 25. NaC2H3O2 26.CO

Unit 3 Packet - Page 23 of 2327. aluminum sulfate 28. Sodium fluoride 29. Lithium oxide 30. Magnesium chloride 31. Copper (II) oxide 32. Dinitrogen pentoxide 33. H = 1+ S= 6+ and O = 2-