Question

1. sodium nitrate _ 2. calcium carbonate _ 3. magnesium oxide _ 4. ammonium sulfite _ 5. lead (ii) sulfate _ 6. sodium cyanide _ 7. potassium hydroxide _ 8. silver chloride _ 9. iron (iii) hydroxide _ 10. potassium hydroxide _ 11. tin (iv) perchlorate _ 12. potassium carbonate _ 13. silver nitrate _ 14. sodium iodide _ 15. ammonium hydroxide _ 16. potassium iodate _ 17. lead (iv) oxide _ 26. aluminum chloride _ 27. iron (iii) hydroxide _ 28. sodium acetate _ 29. calcium hydroxide _ 30. sodium iodate _ 31. nickel (ii) nitrate _ 32. iron (ii) chloride _ 33. magnesium bromide _ 34. ammonium nitrate _ 35. silver bromide _ 36. al(oh)3 _ 37. nh4i _ 38. li2co3 _ 39. cuso4 _ 40. kcn _ 41. pb(clo)2 _ 42. bas _

Explanation:

Step1: Recall chemical - naming rules

For ionic compounds, write the symbol of the cation first followed by the symbol of the anion. For poly - atomic ions, use their standard symbols.

Step2: Write formulas for remaining compounds

1. Sodium iodide: Sodium has a + 1 charge ($Na^+$) and iodide has a - 1 charge ($I^-$), so the formula is $NaI$.
2. Ammonium hydroxide: Ammonium ion is $NH_4^+$ and hydroxide ion is $OH^-$, so the formula is $NH_4OH$.
3. Potassium iodate: Potassium has a + 1 charge ($K^+$) and iodate ion is $IO_3^-$, so the formula is $KIO_3$.
4. Lead (IV) oxide: Lead (IV) has a + 4 charge ($Pb^{4 + }$) and oxide has a - 2 charge ($O^{2 - }$). To balance the charges, we need 2 oxygen atoms for 1 lead (IV) atom, so the formula is $PbO_2$.
5. Aluminum chloride: Aluminum has a + 3 charge ($Al^{3+}$) and chloride has a - 1 charge ($Cl^-$), so the formula is $AlCl_3$.
6. Iron (III) hydroxide: Iron (III) has a + 3 charge ($Fe^{3+}$) and hydroxide has a - 1 charge ($OH^-$), so the formula is $Fe(OH)_3$.
7. Sodium acetate: Sodium has a + 1 charge ($Na^+$) and acetate ion is $C_2H_3O_2^-$, so the formula is $NaC_2H_3O_2$.
8. Calcium hydroxide: Calcium has a + 2 charge ($Ca^{2+}$) and hydroxide has a - 1 charge ($OH^-$), so the formula is $Ca(OH)_2$.
9. Sodium iodate: Sodium has a + 1 charge ($Na^+$) and iodate ion is $IO_3^-$, so the formula is $NaIO_3$.
10. Nickel (II) nitrate: Nickel (II) has a + 2 charge ($Ni^{2+}$) and nitrate ion is $NO_3^-$. To balance the charges, we need 2 nitrate ions for 1 nickel (II) ion, so the formula is $Ni(NO_3)_2$.
11. Iron (II) chloride: Iron (II) has a + 2 charge ($Fe^{2+}$) and chloride has a - 1 charge ($Cl^-$), so the formula is $FeCl_2$.
12. Magnesium bromide: Magnesium has a + 2 charge ($Mg^{2+}$) and bromide has a - 1 charge ($Br^-$), so the formula is $MgBr_2$.
13. Ammonium nitrate: Ammonium ion is $NH_4^+$ and nitrate ion is $NO_3^-$, so the formula is $NH_4NO_3$.
14. Silver bromide: Silver has a + 1 charge ($Ag^+$) and bromide has a - 1 charge ($Br^-$), so the formula is $AgBr$.
15. $Al(OH)_3$ is aluminum hydroxide.
16. $NH_4I$ is ammonium iodide.
17. $Li_2CO_3$ is lithium carbonate.
18. $CuSO_4$ is copper (II) sulfate.
19. $KCN$ is potassium cyanide.
20. $Pb(ClO)_2$ is lead (II) hypochlorite.
21. $BaS$ is barium sulfide.

Answer:

1. $NaI$
2. $NH_4OH$
3. $KIO_3$
4. $PbO_2$
5. $AlCl_3$
6. $Fe(OH)_3$
7. $NaC_2H_3O_2$
8. $Ca(OH)_2$
9. $NaIO_3$
10. $Ni(NO_3)_2$
11. $FeCl_2$
12. $MgBr_2$
13. $NH_4NO_3$
14. $AgBr$
15. Aluminum hydroxide
16. Ammonium iodide
17. Lithium carbonate
18. Copper (II) sulfate
19. Potassium cyanide
20. Lead (II) hypochlorite
21. Barium sulfide