WORKSHEET 1: Determination of oxidation number or valence ...

[Pages:11]WORKSHEET 1: Determination of oxidation number or valence number

Rules to apply:

1. a. The net charges on all molecules is zero therefore, the sum of the positive charges equals the sum of the negative charges

2. a. The charge on all free elements is zero. b. The charge on all metals of group 1 of the periodic table is +1 c. The charge on all metals of group 2 of the periodic table is +2 d. The charge on aluminum is +3 e. The charge on hydrogen is +1, except in hydrides where it is ?1 f. The charge on fluorine is ?1 g. The charge on the other halogens is usually ?1. When united with a more electronegative element the charge is positive. h. The charge on oxygen is ?2 (except in peroxides, such as H2O2 and Na2O2, where it is ?1). (Oxygen is a +2 when

bonded to fluorine only such as in the compound OF2)

To determine the oxidation number of an element in a compound, use all the "known" oxidation states first by applying the above rules. The "unknown" oxidation state is the number that must be added to the total of the "known" oxidation states to make the total of the oxidation states of the compound zero. For example, to find the oxidation state of sulfur in H2SO4,

H2SO4

H 2(+1)=+2 O 4(2)= 8

6 S = ?? + (6) = 0 overall charge

= +6

Find the oxidation state of each of the following

1. Se in H2SeO3 2. N in Al(NO3)3 3. H in BaH2 4. Si in Na4SiO4 5. I in NaIO4 6. O in Na2O2 7. Br in HBrO 8. N in N2O3 9. C in (NH4)2CO3 10. Si in NH4AlSiO4 11. Cr in K2Cr2O7 12. Cl in Mg(ClO4)2

_____________ _____________ _____________ _____________ _____________ _____________ _____________ _____________ _____________ _____________

___________________

_____________

13. B in NaCaBO3 14. Sb in Sb2O3 15. P in H3PO4 16. O in OF2 17. Mn in MnO2 18. P in Ca3(PO4)2 19. Cr in K2CrO4 20. As in Na3AsO3 21. Mn in NaMnO4 22. S in CaS 23. P in H(NH4)2PO4 24. S in KHSO3 25. Mn in MnBr2

_____________ _____________ _____________ _____________ _____________ _____________ _____________ _____________ _____________ _____________ _____________ _____________ _____________

Chemistry

Chapter 7 Worksheets--Chemical Formulas and Nomenclature

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WORKSHEET 2: Fix the Formula

Using your periodic table, which shows the common oxidation states of the elements, and tables in your textbook that show the oxidation state of polyatomic ions, check the total oxidation states of the compounds on this page. If the total oxidation state equals zero, write "CORRECT" in the blank. If it does not equal zero, write the correct formula in the blank. If there is more than once combination possible, write them all.

RULES:

1) Transition metals with negative ions ? show all transition metal's oxidation states:

CuNO3 and Cu(NO3)2

(Cu+1) Copper I and (Cu+2) Copper II

2) Two nonmetals ? the element with the lowest electronegativity will use only its positive oxidation state the other element will use only its negative oxidation state:

CO (Carbon+2) and CO2 (Carbon+4) Oxygen is ?2. Carbon will not use its negative states oxygen will not use any positive states.

3) Metals and nonmetals ? Ionic compounds. The nonmetals will use only the negative oxidation states the give them noble gas configuration:

Complete the following:

1. Pb(SO4)__________________ 2. ZnN _____________________ 3. Cd(ClO4)__________________ 4. Li (CrO4)__________________ 5. Ca(PO4)___________________ 6. AlF______________________ 7. NaNO2___________________ 8. Ba(ClO3)__________________ 9. Ca(CN)___________________ 10. Cd(NO3)_________________ 11. MgBr____________________ 12. PbCl____________________ 13. Al(C2H3O2)_______________ 14. Fe(SO4)3_________________ 15. SiF _____________________ 16. NH4I_____________________ 17. CuBr____________________ 18 CS _____________________ 19. CaF_____________________

20. PbO____________________ 21. (NH4)(SO3)________________ 22. KF _____________________ 23. AgS_____________________ 24. Zn(BrO3)_________________ 25. CaCO3__________________ 26. Cs(Cr2O7)________________ 27. Li(SO3)__________________ 28. Zn(ClO3)_________________ 29. BaN_____________________ 30. HI _____________________ 31. AlO_____________________ 32. CO _____________________ 33. Cd(C2H3O2)_______________ 34. Na(PO4)_________________ 35. Zn(CN)__________________ 36. K(CO3)__________________ 37. Li(MnO4)_________________ 38. CdI_____________________

39. Ag(CO3)_________________ 40. BaCl____________________ 41. MgO____________________ 42. (NH4)S__________________ 43. LiN _____________________ 44. CsCl____________________ 45. HO _____________________ 46. H(SO3)__________________ 47. HgI2_____________________ 48. CaO____________________ 49. Al(OH)__________________ 50. Al(SO4)__________________ 51. Mn(NO3)_________________ 52. SiCl_____________________ 53. (NH4)(OH)________________ 54. Mg(BrO3)_________________ 55. (NH4)Br__________________ 56. Ag(SO4)_________________

Chemistry

Chapter 7 Worksheets--Chemical Formulas and Nomenclature

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Rules to apply:

WORKSHEET 3: Naming Compounds and Nomenclature

A. Binary compounds ? Metals + Nonmetals

A binary compound is one containing only two elements.

1. The element with the lower electronegativity is named first, followed by the element with higher electronegativity. Metal is named first, usually.

2. The suffix of the second element is changed to ?ide.

CaO = Calcium oxide

CaCl2 = Calcium chloride

CaS = Calcium sulfide

CaH2 = Calcium hydride

3. The ammonium ion, NH4+, the hydroxide ion, OH and the cyanide ion, CN--retain their ?ide suffix.

NH4OH = Ammonium hydroxide

NaCN = Sodium cyanide

4. Transition metal capable of more than one oxidation state use roman numerals in their name to indicate their

oxidation state. Place in ( ) .

FeCl3 = Iron (III) chloride

CuO = Copper (II) oxide

FeCl2 = Iron (II) chloride

Cu2O ? Copper (I) oxide

5. Mercury I is a diatomic ion therefore, it is found in the Hg2+2 form only. Mercury II is Hg+2.

Apply the above rules as you name the following compounds:

1. Ca(OH)2 ________________________________

11. K(CN) ________________________________

2. AlCl3

________________________________

12. MgO

________________________________

3. FeI2

________________________________

13. PbCl2

________________________________

4. Hg2Cl2

________________________________

14. Fe(OH)3 ________________________________

5. NaH

________________________________

15. Ag2O

________________________________

6. MgCl2

________________________________

16. HgO

________________________________

7. ZnBr2

________________________________

17. (NH4)I ________________________________

8. MnCl2

________________________________

18. Cu2O

________________________________

9. NH4Cl

________________________________

19. Cs3N

________________________________

10. PbS

________________________________

20. CuS

________________________________

Chemistry

Chapter 7 Worksheets--Chemical Formulas and Nomenclature

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(continued) WORKSHEET 3: Naming Compounds and Nomenclature

B. Binary Compounds ? Nonmetal + Nonmetal 1. Compounds formed by two nonmetals sharing electrons named by using the prefixes mono, di, tri, tetra, penta, hexa, hepta, and octa, non, and deca to indicate the number of atoms involved.

2. The least electronegative is named first. a. if MORE THAN ONE ATOM, give it a prefix b. If only one atom, it is not given a prefix. c. element name is not changed d. use above prefixes

3. The more electronegative is named second ? drop ending and add ?ide. Second element always has prefix.

Examples:

N2O = Dinitrogen monoxide NO = Nitrogen monoxide N2O3 = Dinitrogen trioxide

NO2 = Nitrogen dioxide N2O4 = Dinitrogen tetraoxide N2O5 = Dinitrogen pentoxide

Apply all rules as you name the following compounds

1. CO ________________________________ 2. PBr3 ________________________________ 3. CCl4 ________________________________ 4. NCl3 ________________________________ 5. SeO2 _________________________________________________ 6. P2O3 ________________________________ 7. SO3 ________________________________ 8. P2O5 ________________________________ 9. CO2 ________________________________ 10. PI5 ________________________________ 11. SeO3 ________________________________

12. SiO2 ________________________________ 13. Cl2O7 ________________________________ 14. SO2 ________________________________ 15. N2O3 ________________________________ 16. N3P2 ________________________________ 17. SCl2 ________________________________ 18. SeF6 ________________________________ 19. N2O4 ________________________________ 20. CS2 ________________________________ 21. H2S ________________________________ 22. CF4 ________________________________

Chemistry

Chapter 7 Worksheets--Chemical Formulas and Nomenclature

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(continued) WORKSHEET 3: Naming Compounds and Nomenclature

C. Tertiary Compounds:

1. Compounds containing polyatomic ions (more than 2 elements) 2. Polyatomic ion retains its name whether it is positive or negative. 3. Metals and nonmetals are names the same as before.

1. Pb(SO4)____________________________________ 2. Cd(ClO4)2__________________________________ 3. Li2(CrO4)___________________________________ 4. Ca3(PO4)2___________________________________ 5. NaNO2_____________________________________ 6. Ba(ClO3)2___________________________________ 7. Ca(CN)2____________________________________ 8. Cd(NO3)2___________________________________ 9. Al(C2H3O2)3_________________________________ 10. Fe2(SO4)3_________________________________ 11. (NH4)2(SO3)________________________________ 12. Zn(BrO3)2__________________________________ 13. CaCO3____________________________________

14. Cs2(Cr2O7)_________________________________ 15. Li2(SO3)___________________________________ 16. Zn(ClO3)2__________________________________ 17. Cd(C2H3O2)2_______________________________ 18. Na3(PO4)__________________________________ 19. Zn(CN)2___________________________________ 20. K2(CO3)___________________________________ 21. Li(MnO4)__________________________________ 22. Ag2(CO3)__________________________________ 23. (NH4)2S___________________________________ 24. H2(SO3)___________________________________ 25. Sn(CO3)2____________________________________________________

Chemistry

Chapter 7 Worksheets--Chemical Formulas and Nomenclature

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(continued) WORKSHEET 3: Naming Compounds and Nomenclature

D. Variations of Polyatomic Ions:

1. Polyatomic ions with oxygen included have multiple variations. The number of oxygen atoms included determines the naming scheme.

2. The charge of the ion is always the same as the main version no matter the number of oxygen atoms.

3. Main versions of ion always have: base root of ion and end with ?ate examples: SO42 (sulfate) NO31 (nitrate)

4. One more oxygen than the main version always has: per base root of ion ?ate examples: SO52 (persulfate) NO41 (pernitrate)

5. One less oxygen than the main version always have: base root of ion and end with ?ite examples: SO32 (sulfite) NO21 (nitrite)

6. Two less oxygens than the main version always has: hypo base root of ion ?ite examples: SO22 (hyposulfite) NO1 (hyponitrite)

7. How to determine what is a main version of a polyatomic ion:

Outside of chart always has three (3) oxygen atoms for the main version.

B4O72 CO32 NO31 C2O42 FO31

Notice the patterns of charges.

SiO44 PO43 SO42 ClO31

AsO43 Inside of chart always has four (4) oxygen atoms for the main version. Notice charges.

SeO42 TeO42

BrO31 IO31 AtO31

Main Versions of Polyatomic Ions

1. PbSO2_______________________________________ 2. Cd(ClO2)2_____________________________________ 3. Ca3(PO5)2_____________________________________ 4. Na3AsO3_____________________________________ 5. Ba(ClO)2_____________________________________ 6. Cd(NO)2_____________________________________ 7. Al(IO3)3______________________________________ 8. Fe(SO2)3_____________________________________ 9. (NH4)2SO4____________________________________ 10 Zn(BrO)2____________________________________ 11. Sn(CO4)________________________________________________________

12. CaCO2_____________________________________ 13.Ni2(SO4)3_____________________________________ 14. Zn(ClO4)2____________________________________ 15. Cd(C2H3O2)2__________________________________ 16. AuPO2______________________________________ 17. Hg2SeO5_____________________________________ 18. Pb2SiO3____________________________________ 19. Ti(AtO3)3_____________________________________ 20. Sn(NO4)2________________________________________________________

Chemistry

Chapter 7 Worksheets--Chemical Formulas and Nomenclature

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WORKSHEET 4: Total Nomenclature (Binary, Tertiary, Modified Tertiary)

Instructions: If the formula given is correct, write "correct" in the first blank and if there is more than one compound write out all the correct formulae. Name all the possible compounds in the second blank.

1. ZnCN______________________________________ 2. AlN_________________________________________ 3. BaOH______________________________________ 4. RaBr________________________________________ 5. AgO_________________________________________ 6. AlS_________________________________________ 7. NH4S_______________________________________ 8. CuI2_________________________________________ 9. CdOH______________________________________ 10. NH4Cl_______________________________________ 11. MgN________________________________________ 12. CsH________________________________________ 13. CaCN______________________________________ 14. AgS________________________________________ 15. SnCl2_______________________________________ 16. PI5________________________________________ 17. AsBr________________________________________ 18. AlCl________________________________________ 19. SiO_________________________________________ 20. FeI_________________________________________ 21. SrOH______________________________________ 22. AlBr3________________________________________ 23. BN_________________________________________ 24. Cr(PO2)2_____________________________________ 25. SiBr________________________________________

26. Cadmium Acetate_____________________________ 27. Barium Iodide______________________________ 28. Copper (II) Sulfide_____________________________ 29. Potassium Monohydride________________________ 30. Cadmium Dichloride___________________________ 31. Berylium bromide____________________________ 32. Boron Phosphide______________________________ 33. Trinitrogen Dioxide_____________________________ 34. Platinum (IV) Iodide____________________________ 35. Nitrogen Triiodide____________________________ 36. Germanium Tetrachloride______________________ 37. Sodium Percarbonate_______________________ 38. Diphosphorus Triiodide_________________________ 39. Potassium Sulfide____________________________ 40. Lithium Nitride________________________________ 41. Sulfur Diflouride______________________________ 42. Arsenic Sulfide________________________________ 43. Ammonium Hydroxide__________________________ 44. Strontium Carbide_____________________________ 45. Sodium Hypophosphite________________________ 46. Aluminum Carbonite___________________________ 47. Berylium Perbromate_________________________ 48. Calcium Hypofluorite___________________________ 49. Copper (II) Sulfite_____________________________ 50. Mercury (I) Perchlorate_________________________

Chemistry

Chapter 7 Worksheets--Chemical Formulas and Nomenclature

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Rules to apply:

WORKSHEET 5: Acids and Nomenclature

I. Acids Traditional inorganic acids contain hydrogen combined with a negative ion.

A. Binary acids (acids with hydrogen and a single anion or pseudosingle anion CN--or OH ). Binary acids may be named as binary compounds or by the following rules:

1. Use the full name of the nonmetallic element. 2. Add the prefix hydro. 3. Add the suffix ic.

Examples : H2S = Hydrosulfuric acid

HCl = Hydrochloric acid

B. Oxyacids/Ternary (acid with three elements hydrogen and a polyatomic ion) also have a molecular name and an acid name.

Follow these rules:

1. Determine the name of the polyatomic ion. 2. Eliminate the hydrogen and change ?ate endings to ?ic and ?ite ending to ?ous. 3. Keep hypo and per prefixes.

Examples: Formula

Molecular name

Acid name

HClO4

Hydrogen perchlorate

Perchloric acid

HClO3

Hydrogen chlorate

Chloric acid

HClO2

Hydrogen chlorite

Chlorous acid

HClO

Hydrogen hypochlorite

Hypochlorous acid

Chemistry

Chapter 7 Worksheets--Chemical Formulas and Nomenclature

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