sa 3 writing chemical formulas\nwrite the chemical formulas for the following compounds:\n1. sodium…

Explanation:

Step1: Determine ion charges

Use common - ion charges and oxidation states to write chemical formulas. For example, sodium has a + 1 charge ($Na^+$) and hydride has a - 1 charge ($H^-$).

Step2: Balance charges

Combine ions in ratios to balance the overall charge of the compound.

1. Sodium hydride: $Na^+$ and $H^-$ combine to give $NaH$.
2. Gallium (III) has a + 3 charge ($Ga^{3 + }$) and hydrogen sulfide ion ($HS^-$), so the formula is $Ga(HS)_3$.
3. Potassium has a + 1 charge ($K^+$) and arsenide has a - 3 charge ($As^{3 - }$), the formula is $K_3As$.
4. Gold (I) has a + 1 charge ($Au^+$) and carbonate has a - 2 charge ($CO_3^{2 - }$), the formula is $Au_2CO_3$.
5. Krypton hexabromide: Krypton is a noble - gas, but here it forms a compound with bromine. Krypton has an oxidation state of + 6 and bromine has a - 1 charge ($Br^-$), the formula is $KrBr_6$.
6. Manganese (II) has a + 2 charge ($Mn^{2+}$) and nitride has a - 3 charge ($N^{3 - }$), the formula is $Mn_3N_2$.
7. Mercury (II) has a + 2 charge ($Hg^{2+}$) and sulfide has a - 2 charge ($S^{2 - }$), the formula is $HgS$.
8. Zinc has a + 2 charge ($Zn^{2+}$) and phosphide has a - 3 charge ($P^{3 - }$), the formula is $Zn_3P_2$.
9. Nickel (II) has a + 2 charge ($Ni^{2+}$) and borate ($BO_3^{3 - }$), the formula is $Ni_3(BO_3)_2$.
10. Ammonium has a + 1 charge ($NH_4^+$) and oxalate has a - 2 charge ($C_2O_4^{2 - }$), the formula is $(NH_4)_2C_2O_4$.
11. Titanium (IV) has a + 4 charge ($Ti^{4+}$) and carbide has a - 4 charge ($C^{4 - }$), the formula is $TiC$.
12. Barium has a + 2 charge ($Ba^{2+}$) and arsenide has a - 3 charge ($As^{3 - }$), the formula is $Ba_3As_2$.
13. Tetraarsenic trisulfide: Arsenic and sulfur combine. The prefixes indicate the number of atoms. The formula is $As_4S_3$.
14. Tantalum (V) has a + 5 charge ($Ta^{5+}$) and hydrogen sulfite ($HSO_3^-$), the formula is $Ta(HSO_3)_5$.
15. Aluminum has a + 3 charge ($Al^{3+}$) and iodide has a - 1 charge ($I^-$), the formula is $AlI_3$.
16. Hydrogen has a + 1 charge ($H^+$) and telluride has a - 2 charge ($Te^{2 - }$), the formula is $H_2Te$.
17. Cadmium has a + 2 charge ($Cd^{2+}$) and chloride has a - 1 charge ($Cl^-$), the formula is $CdCl_2$.
18. Cesium has a + 1 charge ($Cs^+$) and phosphate has a - 3 charge ($PO_4^{3 - }$), the formula is $Cs_3PO_4$.
19. Germanium (IV) has a + 4 charge ($Ge^{4+}$) and selenide has a - 2 charge ($Se^{2 - }$), the formula is $GeSe_2$.
20. Disulfur dinitride: The prefixes indicate 2 sulfur and 2 nitrogen atoms, the formula is $S_2N_2$.
21. Heptasulfur dioxide: The prefixes indicate 7 sulfur and 2 oxygen atoms, the formula is $S_7O_2$.
22. Silver has a + 1 charge ($Ag^+$) and citrate ($C_6H_5O_7^{3 - }$), the formula is $Ag_3C_6H_5O_7$.
23. Rhenium (VII) has a + 7 charge ($Re^{7+}$) and carbonate ($CO_3^{2 - }$), the formula is $Re_2(CO_3)_7$.
24. Magnesium has a + 2 charge ($Mg^{2+}$) and thiosulfate has a - 2 charge ($S_2O_3^{2 - }$), the formula is $MgS_2O_3$.

Answer:

1. $NaH$
2. $Ga(HS)_3$
3. $K_3As$
4. $Au_2CO_3$
5. $KrBr_6$
6. $Mn_3N_2$
7. $HgS$
8. $Zn_3P_2$
9. $Ni_3(BO_3)_2$
10. $(NH_4)_2C_2O_4$
11. $TiC$
12. $Ba_3As_2$
13. $As_4S_3$
14. $Ta(HSO_3)_5$
15. $AlI_3$
16. $H_2Te$
17. $CdCl_2$
18. $Cs_3PO_4$
19. $GeSe_2$
20. $S_2N_2$
21. $S_7O_2$
22. $Ag_3C_6H_5O_7$
23. $Re_2(CO_3)_7$
24. $MgS_2O_3$