worksheet- formulas name - Free Printable

To solve the problem of writing the chemical formulas for each compound listed in the worksheet, we need to understand the rules for naming and writing chemical formulas. Here's a step-by-step explanation of how to approach this task:

Key Rules for Writing Chemical Formulas:

1. Ionic Compounds:
- The formula is written by balancing the charges of the cation (positive ion) and anion (negative ion).
- Use subscripts to indicate the number of atoms or ions needed to balance the charge.

2. Covalent Compounds:
- Prefixes are used to indicate the number of atoms of each element in the molecule.
- Common prefixes include mono-, di-, tri-, tetra-, etc.

3. Acids:
- Binary acids: "hydro-" prefix + root name of nonmetal + "-ic acid."
- Oxoacids: Root name of central atom + suffix (-ic or -ous) + "acid."

4. Hydrates:
- Include the number of water molecules using a prefix (e.g., monohydrate, dihydrate).

5. Polyatomic Ions:
- Memorize common polyatomic ions and their charges (e.g., sulfate \( \text{SO}_4^{2-} \), nitrate \( \text{NO}_3^- \)).

Solution Approach:

We will go through each compound and write its chemical formula based on the above rules.

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1. Barium sulfide

- Barium (\( \text{Ba} \)) has a charge of \( +2 \).
- Sulfide (\( \text{S}^{2-} \)) has a charge of \( -2 \).
- Formula: \( \text{BaS} \)

2. Manganese (III) iodide

- Manganese (III) has a charge of \( +3 \).
- Iodide (\( \text{I}^- \)) has a charge of \( -1 \).
- To balance the charges: \( \text{MnI}_3 \)

3. Ammonium hydrogen phosphate

- Ammonium (\( \text{NH}_4^+ \)) has a charge of \( +1 \).
- Hydrogen phosphate (\( \text{HPO}_4^{2-} \)) has a charge of \( -2 \).
- Formula: \( \text{(NH}_4\text{)}_2\text{HPO}_4 \)

4. Carbon disulfide

- Covalent compound.
- One carbon atom and two sulfur atoms.
- Formula: \( \text{CS}_2 \)

5. Lead (II) sulfate

- Lead (II) has a charge of \( +2 \).
- Sulfate (\( \text{SO}_4^{2-} \)) has a charge of \( -2 \).
- Formula: \( \text{PbSO}_4 \)

6. Magnesium carbonate

- Magnesium (\( \text{Mg} \)) has a charge of \( +2 \).
- Carbonate (\( \text{CO}_3^{2-} \)) has a charge of \( -2 \).
- Formula: \( \text{MgCO}_3 \)

7. Potassium permanganate

- Potassium (\( \text{K}^+ \)) has a charge of \( +1 \).
- Permanganate (\( \text{MnO}_4^- \)) has a charge of \( -1 \).
- Formula: \( \text{KMnO}_4 \)

8. Silver bicarbonate

- Silver (\( \text{Ag}^+ \)) has a charge of \( +1 \).
- Bicarbonate (\( \text{HCO}_3^- \)) has a charge of \( -1 \).
- Formula: \( \text{AgHCO}_3 \)

9. Bismuth (III) bromide

- Bismuth (III) has a charge of \( +3 \).
- Bromide (\( \text{Br}^- \)) has a charge of \( -1 \).
- To balance the charges: \( \text{BiBr}_3 \)

10. Tetranitrogen tetrasulfide

- Covalent compound.
- Four nitrogen atoms and four sulfur atoms.
- Formula: \( \text{N}_4\text{S}_4 \)

11. Ferric perchlorate

- Ferric (\( \text{Fe}^{3+} \)) has a charge of \( +3 \).
- Perchlorate (\( \text{ClO}_4^- \)) has a charge of \( -1 \).
- To balance the charges: \( \text{Fe(ClO}_4\text{)}_3 \)

12. Chromium (III) chloride

- Chromium (III) has a charge of \( +3 \).
- Chloride (\( \text{Cl}^- \)) has a charge of \( -1 \).
- To balance the charges: \( \text{CrCl}_3 \)

13. Tin (III) thiosulfate

- Tin (III) has a charge of \( +3 \).
- Thiosulfate (\( \text{S}_2\text{O}_3^{2-} \)) has a charge of \( -2 \).
- To balance the charges: \( \text{Sn}_2(\text{S}_2\text{O}_3)_3 \)

14. Cuprous bisulfate

- Cuprous (\( \text{Cu}^+ \)) has a charge of \( +1 \).
- Bisulfate (\( \text{HSO}_4^- \)) has a charge of \( -1 \).
- Formula: \( \text{CuHSO}_4 \)

15. Sodium bisulfite

- Sodium (\( \text{Na}^+ \)) has a charge of \( +1 \).
- Bisulfite (\( \text{HSO}_3^- \)) has a charge of \( -1 \).
- Formula: \( \text{NaHSO}_3 \)

16. Carbon tetrachloride

- Covalent compound.
- One carbon atom and four chlorine atoms.
- Formula: \( \text{CCl}_4 \)

17. Sodium acetate

- Sodium (\( \text{Na}^+ \)) has a charge of \( +1 \).
- Acetate (\( \text{CH}_3\text{COO}^- \)) has a charge of \( -1 \).
- Formula: \( \text{NaCH}_3\text{COO} \) or \( \text{CH}_3\text{COONa} \)

18. Ferric difluorophosphate

- Ferric (\( \text{Fe}^{3+} \)) has a charge of \( +3 \).
- Difluorophosphate (\( \text{F}_2\text{PO}_4^{3-} \)) has a charge of \( -3 \).
- Formula: \( \text{FeF}_2\text{PO}_4 \)

19. Chromium (II) phosphate

- Chromium (II) has a charge of \( +2 \).
- Phosphate (\( \text{PO}_4^{3-} \)) has a charge of \( -3 \).
- To balance the charges: \( \text{Cr}_3(\text{PO}_4)_2 \)

20. Mercuric perchlorate

- Mercuric (\( \text{Hg}^{2+} \)) has a charge of \( +2 \).
- Perchlorate (\( \text{ClO}_4^- \)) has a charge of \( -1 \).
- To balance the charges: \( \text{Hg(ClO}_4\text{)}_2 \)

21. Nickel (II) borate

- Nickel (II) has a charge of \( +2 \).
- Borate (\( \text{BO}_3^{3-} \)) has a charge of \( -3 \).
- To balance the charges: \( \text{Ni}_3(\text{BO}_3)_2 \)

22. Cadmium thiocyanate

- Cadmium (\( \text{Cd}^{2+} \)) has a charge of \( +2 \).
- Thiocyanate (\( \text{SCN}^- \)) has a charge of \( -1 \).
- To balance the charges: \( \text{Cd(SCN)}_2 \)

23. Ammonium sulfide

- Ammonium (\( \text{NH}_4^+ \)) has a charge of \( +1 \).
- Sulfide (\( \text{S}^{2-} \)) has a charge of \( -2 \).
- To balance the charges: \( (\text{NH}_4)_2\text{S} \)

24. Bismuth (III) bisulfite

- Bismuth (III) has a charge of \( +3 \).
- Bisulfite (\( \text{HSO}_3^- \)) has a charge of \( -1 \).
- To balance the charges: \( \text{Bi(HSO}_3\text{)}_3 \)

25. Strontium chlorate

- Strontium (\( \text{Sr}^{2+} \)) has a charge of \( +2 \).
- Chlorate (\( \text{ClO}_3^- \)) has a charge of \( -1 \).
- To balance the charges: \( \text{Sr(ClO}_3\text{)}_2 \)

26. Aluminum bisulfide

- Aluminum (\( \text{Al}^{3+} \)) has a charge of \( +3 \).
- Bisulfide (\( \text{HS}^- \)) has a charge of \( -1 \).
- To balance the charges: \( \text{Al}_2(\text{HS})_3 \)

27. Diphosphorus trioxide

- Covalent compound.
- Two phosphorus atoms and three oxygen atoms.
- Formula: \( \text{P}_2\text{O}_3 \)

28. Zinc hydroxide

- Zinc (\( \text{Zn}^{2+} \)) has a charge of \( +2 \).
- Hydroxide (\( \text{OH}^- \)) has a charge of \( -1 \).
- To balance the charges: \( \text{Zn(OH)}_2 \)

29. Silver chromate

- Silver (\( \text{Ag}^+ \)) has a charge of \( +1 \).
- Chromate (\( \text{CrO}_4^{2-} \)) has a charge of \( -2 \).
- To balance the charges: \( \text{Ag}_2\text{CrO}_4 \)

30. Copper (II) acetate

- Copper (II) has a charge of \( +2 \).
- Acetate (\( \text{CH}_3\text{COO}^- \)) has a charge of \( -1 \).
- Formula: \( \text{Cu(CH}_3\text{COO)}_2 \)

31. Cobaltous iodide

- Cobaltous (\( \text{Co}^{2+} \)) has a charge of \( +2 \).
- Iodide (\( \text{I}^- \)) has a charge of \( -1 \).
- To balance the charges: \( \text{CoI}_2 \)

32. Cupric dichromate

- Cupric (\( \text{Cu}^{2+} \)) has a charge of \( +2 \).
- Dichromate (\( \text{Cr}_2\text{O}_7^{2-} \)) has a charge of \( -2 \).
- Formula: \( \text{Cu(Cr}_2\text{O}_7) \)

33. Sodium peroxide

- Sodium (\( \text{Na}^+ \)) has a charge of \( +1 \).
- Peroxide (\( \text{O}_2^{2-} \)) has a charge of \( -2 \).
- To balance the charges: \( \text{Na}_2\text{O}_2 \)

34. Dinitrogen trioxide

- Covalent compound.
- Two nitrogen atoms and three oxygen atoms.
- Formula: \( \text{N}_2\text{O}_3 \)

35. Dichlorine hexoxide

- Covalent compound.
- Two chlorine atoms and six oxygen atoms.
- Formula: \( \text{Cl}_2\text{O}_6 \)

36. Cobaltic nitrite

- Cobaltic (\( \text{Co}^{3+} \)) has a charge of \( +3 \).
- Nitrite (\( \text{NO}_2^- \)) has a charge of \( -1 \).
- To balance the charges: \( \text{Co(NO}_2\text{)}_3 \)

37. Barium cyanide

- Barium (\( \text{Ba}^{2+} \)) has a charge of \( +2 \).
- Cyanide (\( \text{CN}^- \)) has a charge of \( -1 \).
- To balance the charges: \( \text{Ba(CN)}_2 \)

38. Hypochlorous acid

- Formula: \( \text{HClO} \)

39. Sulfurous acid

- Formula: \( \text{H}_2\text{SO}_3 \)

40. Hydrosulfuric acid

- Formula: \( \text{H}_2\text{S} \)

41. Nitric acid

- Formula: \( \text{HNO}_3 \)

42. Bromic acid

- Formula: \( \text{HBrO}_3 \)

43. Bromous acid

- Formula: \( \text{HBrO}_2 \)

44. Iodic acid

- Formula: \( \text{HIO}_3 \)

45. Hydrosulfuric acid

- Formula: \( \text{H}_2\text{S} \)

46. Periodic acid

- Formula: \( \text{HIO}_4 \)

47. Hydrofluoric acid

- Formula: \( \text{HF} \)

48. Hypobromous acid

- Formula: \( \text{HBrO} \)

49. Mercurous chloride

- Formula: \( \text{Hg}_2\text{Cl}_2 \)

50. Ferric cyanate

- Formula: \( \text{Fe(CN)}_3 \)

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Final Answer:

\[
\boxed{
\begin{array}{ll}
1. \text{BaS} & 26. \text{Al}_2(\text{HS})_3 \\
2. \text{MnI}_3 & 27. \text{P}_2\text{O}_3 \\
3. \text{(NH}_4\text{)}_2\text{HPO}_4 & 28. \text{Zn(OH)}_2 \\
4. \text{CS}_2 & 29. \text{Ag}_2\text{CrO}_4 \\
5. \text{PbSO}_4 & 30. \text{Cu(CH}_3\text{COO)}_2 \\
6. \text{MgCO}_3 & 31. \text{CoI}_2 \\
7. \text{KMnO}_4 & 32. \text{Cu(Cr}_2\text{O}_7) \\
8. \text{AgHCO}_3 & 33. \text{Na}_2\text{O}_2 \\
9. \text{BiBr}_3 & 34. \text{N}_2\text{O}_3 \\
10. \text{N}_4\text{S}_4 & 35. \text{Cl}_2\text{O}_6 \\
11. \text{Fe(ClO}_4\text{)}_3 & 36. \text{Co(NO}_2\text{)}_3 \\
12. \text{CrCl}_3 & 37. \text{Ba(CN)}_2 \\
13. \text{Sn}_2(\text{S}_2\text{O}_3)_3 & 38. \text{HClO} \\
14. \text{CuHSO}_4 & 39. \text{H}_2\text{SO}_3 \\
15. \text{NaHSO}_3 & 40. \text{H}_2\text{S} \\
16. \text{CCl}_4 & 41. \text{HNO}_3 \\
17. \text{NaCH}_3\text{COO} & 42. \text{HBrO}_3 \\
18. \text{FeF}_2\text{PO}_4 & 43. \text{HBrO}_2 \\
19. \text{Cr}_3(\text{PO}_4)_2 & 44. \text{HIO}_3 \\
20. \text{Hg(ClO}_4\text{)}_2 & 45. \text{H}_2\text{S} \\
21. \text{Ni}_3(\text{BO}_3)_2 & 46. \text{HIO}_4 \\
22. \text{Cd(SCN)}_2 & 47. \text{HF} \\
23. (\text{NH}_4)_2\text{S} & 48. \text{HBrO} \\
24. \text{Bi(HSO}_3\text{)}_3 & 49. \text{Hg}_2\text{Cl}_2 \\
25. \text{Sr(ClO}_3\text{)}_2 & 50. \text{Fe(CN)}_3 \\
\end{array}
}
\]