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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 H O and Na O , where it is –1). (Oxygen is a +2 when
2 2 2 2
bonded to fluorine only such as in the compound OF )
2
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 H SO ,
2 4
HSO H 2(+1)=+2
2 4
O 4(2)= 8
6
S = ?? + (6) = 0 overall charge
= +6
Find the oxidation state of each of the following
13. B in NaCaBO _____________
3
1. Se in H SeO _____________
2 3
14. Sb in Sb O _____________
2 3
2. N in Al(NO ) _____________
3 3
15. P in H PO _____________
3 4
3. H in BaH _____________
2
16. O in OF _____________
2
4. Si in Na SiO _____________
4 4
17. Mn in MnO _____________
2
5. I in NaIO _____________
4
18. P in Ca (PO ) _____________
3 4 2
6. O in Na O _____________
2 2
19. Cr in K CrO _____________
2 4
7. Br in HBrO _____________
20. As in Na AsO _____________
3 3
8. N in N O _____________
2 3
21. Mn in NaMnO _____________
4
9. C in (NH ) CO _____________
4 2 3
22. S in CaS _____________
10. Si in NH AlSiO _____________
4 4
23. P in H(NH ) PO _____________
4 2 4
11. Cr in K Cr O
2 2 7 ___________________
24. S in KHSO _____________
3
12. Cl in Mg(ClO ) _____________
4 2
25. Mn in MnBr _____________
2
Chemistry Chapter 7 Worksheets—Chemical Formulas and Nomenclature page 1
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:
+1 +2
CuNO and Cu(NO ) (Cu ) Copper I and (Cu ) Copper II
3 3 2
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:
+2 +4
CO (Carbon ) and CO (Carbon )
2
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(SO )__________________ 20. PbO____________________ 39. Ag(CO )_________________
4 3
2. ZnN _____________________ 21. (NH )(SO )________________ 40. BaCl____________________
4 3
3. Cd(ClO )__________________ 22. KF _____________________ 41. MgO____________________
4
4. Li (CrO )__________________ 23. AgS_____________________ 42. (NH )S__________________
4 4
5. Ca(PO )___________________ 24. Zn(BrO )_________________ 43. LiN_____________________
4 3
6. AlF______________________ 25. CaCO __________________ 44. CsCl____________________
3
7. NaNO ___________________ 26. Cs(Cr O )________________ 45. HO_____________________
2 2 7
8. Ba(ClO )__________________ 27. Li(SO )__________________ 46. H(SO )__________________
3 3 3
9. Ca(CN)___________________ 28. Zn(ClO )_________________ 47. HgI _____________________
3 2
10. Cd(NO )_________________ 29. BaN_____________________ 48. CaO____________________
3
11. MgBr____________________ 30. HI _____________________ 49. Al(OH)__________________
12. PbCl____________________ 31. AlO_____________________ 50. Al(SO )__________________
4
13. Al(C H O )_______________ 32. CO_____________________ 51. Mn(NO )_________________
2 3 2 3
14. Fe(SO ) _________________ 33. Cd(C H O )_______________ 52. SiCl_____________________
4 3 2 3 2
15. SiF_____________________ 34. Na(PO )_________________ 53. (NH )(OH)________________
4 4
16. NH I_____________________ 35. Zn(CN)__________________ 54. Mg(BrO )_________________
4 3
17. CuBr____________________ 36. K(CO )__________________ 55. (NH )Br__________________
3 4
18 CS _____________________ 37. Li(MnO )_________________ 56. Ag(SO )_________________
4 4
19. CaF_____________________ 38. CdI_____________________
Chemistry Chapter 7 Worksheets—Chemical Formulas and Nomenclature page 2
WORKSHEET 3: Naming Compounds and Nomenclature
Rules to apply:
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 CaCl = Calcium chloride
2
CaS = Calcium sulfide CaH = Calcium hydride
2
+ —
3. The ammonium ion, NH , the hydroxide ion, OH ; and the cyanide ion, CN retain their –ide suffix.
4
NHOH = Ammonium hydroxide NaCN = Sodium cyanide
4
4. Transition metal capable of more than one oxidation state use roman numerals in their name to indicate their
oxidation state. Place in ( ) .
FeCl = Iron (III) chloride CuO = Copper (II) oxide
3
FeCl = Iron (II) chloride Cu O – Copper (I) oxide
2 2
+2 +2
5. Mercury I is a diatomic ion; therefore, it is found in the Hg form only. Mercury II is Hg .
2
Apply the above rules as you name the following compounds:
1. Ca(OH) ________________________________ 11. K(CN) ________________________________
2
2. AlCl ________________________________ 12. MgO ________________________________
3
3. FeI ________________________________ 13. PbCl ________________________________
2 2
4. Hg Cl ________________________________ 14. Fe(OH) ________________________________
2 2 3
5. NaH ________________________________ 15. Ag O ________________________________
2
6. MgCl ________________________________ 16. HgO ________________________________
2
7. ZnBr ________________________________ 17. (NH )I ________________________________
2 4
8. MnCl ________________________________ 18. Cu O ________________________________
2 2
9. NH Cl ________________________________ 19. Cs N ________________________________
4 3
10. PbS ________________________________ 20. CuS ________________________________
Chemistry Chapter 7 Worksheets—Chemical Formulas and Nomenclature page 3
(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:
NO = Dinitrogen monoxide NO = Nitrogen dioxide
2 2
NO = Nitrogen monoxide NO = Dinitrogen tetraoxide
2 4
NO = Dinitrogen trioxide NO = Dinitrogen pentoxide
2 3 2 5
Apply all rules as you name the following compounds
1. CO ________________________________ 12. SiO ________________________________
2
2. PBr ________________________________ 13. Cl O ________________________________
3 2 7
3. CCl ________________________________ 14. SO ________________________________
4 2
4. NCl ________________________________ 15. N O ________________________________
3 2 3
5. SeO 16. N P ________________________________
2 _________________________________________________ 3 2
6. P O ________________________________ 17. SCl ________________________________
2 3 2
7. SO ________________________________ 18. SeF ________________________________
3 6
8. P O ________________________________ 19. N O ________________________________
2 5 2 4
9. CO ________________________________ 20. CS ________________________________
2 2
10. PI ________________________________ 21. H S ________________________________
5 2
11. SeO ________________________________ 22. CF ________________________________
3 4
Chemistry Chapter 7 Worksheets—Chemical Formulas and Nomenclature page 4
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