chemistry: ions in chemical compounds\nname: micah carter\nhour: 7 date: 9/20/25\ncomplete the following…
chemistry: ions in chemical compounds\nname: micah carter\nhour: 7 date: 9/20/25\ncomplete the following table, being sure that the total charge on the resulting compound is zero.\n| ions | chloride cl⁻ | hydroxide oh⁻ | nitrate no₃⁻ | sulfate so₄²⁻ | sulfide s²⁻ | carbonate co₃²⁻ | phosphate po₄³⁻ |\n| ---- | ---- | ---- | ---- | ---- | ---- | ---- | ---- |\n| hydrogen h⁺ | hcl | hoh | hno₃ | | | | |\n| sodium na⁺ | nacl | naoh | nano₃ | | | | |\n| ammonium nh₄⁺ | nh₄cl | nh₄oh | nh₄no₃ | | | | |\n| potassium k⁺ | kcl | koh | kno₃ | | | | |\n| calcium ca²⁺ | cacl₂ | ca(oh)₂ | ca(no₃)₂ | | | | |\n| magnesium mg²⁺ | mgcl₂ | mg(oh)₂ | mg(no₃)₂ | | | | |\n| aluminum al³⁺ | alcl₃ | al(oh)₃ | al(no₃)₃ | | | | |\n| iron (ii) fe²⁺ | | | | | | | |\n| iron (iii) fe³⁺ | fecl₃ | fe(oh)₃ | | | | | |\n| copper (i) cu⁺ | cucl | cuoh | | | | | |
Answer
Explanation:
Step1: Determine compound formulas
For each pair of cations and anions, balance the charges to form a neutral - charge compound. For example, when a calcium ion ($Ca^{2 + }$) combines with a sulfate ion ($SO_{4}^{2 - }$), the formula is $CaSO_{4}$ because the + 2 charge of calcium balances the - 2 charge of sulfate.
Step2: Write formulas systematically
Go through each row (cation) and column (anion) combination. For a hydrogen ion ($H^{+}$) and a carbonate ion ($CO_{3}^{2 - }$), two hydrogen ions are needed to balance the - 2 charge of the carbonate ion, so the formula is $H_{2}CO_{3}$.
Answer:
| Ions | Chloride $Cl^{-}$ | Hydroxide $OH^{-}$ | Nitrate $NO_{3}^{-}$ | Sulfate $SO_{4}^{2 - }$ | Sulfide $S^{2 - }$ | Carbonate $CO_{3}^{2 - }$ | Phosphate $PO_{4}^{3 - }$ |
|---|---|---|---|---|---|---|---|
| Hydrogen $H^{+}$ | $HCl$ | $H_{2}O$ (Note: $HOH$ is incorrect, it's $H_{2}O$) | $HNO_{3}$ | $H_{2}SO_{4}$ | $H_{2}S$ | $H_{2}CO_{3}$ | $H_{3}PO_{4}$ |
| Sodium $Na^{+}$ | $NaCl$ | $NaOH$ | $NaNO_{3}$ | $Na_{2}SO_{4}$ | $Na_{2}S$ | $Na_{2}CO_{3}$ | $Na_{3}PO_{4}$ |
| Ammonium $NH_{4}^{+}$ | $NH_{4}Cl$ | $NH_{4}OH$ (usually written as $NH_{3}\cdot H_{2}O$) | $NH_{4}NO_{3}$ | $(NH_{4}){2}SO{4}$ | $(NH_{4})_{2}S$ | $(NH_{4}){2}CO{3}$ | $(NH_{4}){3}PO{4}$ |
| Potassium $K^{+}$ | $KCl$ | $KOH$ | $KNO_{3}$ | $K_{2}SO_{4}$ | $K_{2}S$ | $K_{2}CO_{3}$ | $K_{3}PO_{4}$ |
| Calcium $Ca^{2 + }$ | $CaCl_{2}$ | $Ca(OH)_{2}$ | $Ca(NO_{3})_{2}$ | $CaSO_{4}$ | $CaS$ | $CaCO_{3}$ | $Ca_{3}(PO_{4})_{2}$ |
| Magnesium $Mg^{2 + }$ | $MgCl_{2}$ | $Mg(OH)_{2}$ | $Mg(NO_{3})_{2}$ | $MgSO_{4}$ | $MgS$ | $MgCO_{3}$ | $Mg_{3}(PO_{4})_{2}$ |
| Aluminum $Al^{3 + }$ | $AlCl_{3}$ | $Al(OH)_{3}$ | $Al(NO_{3})_{3}$ | $Al_{2}(SO_{4})_{3}$ | $Al_{2}S_{3}$ | $Al_{2}(CO_{3})_{3}$ | $AlPO_{4}$ |
| Iron (II) $Fe^{2 + }$ | $FeCl_{2}$ | $Fe(OH)_{2}$ | $Fe(NO_{3})_{2}$ | $FeSO_{4}$ | $FeS$ | $FeCO_{3}$ | $Fe_{3}(PO_{4})_{2}$ |
| Iron (III) $Fe^{3 + }$ | $FeCl_{3}$ | $Fe(OH)_{3}$ | $Fe(NO_{3})_{3}$ | $Fe_{2}(SO_{4})_{3}$ | $Fe_{2}S_{3}$ | $Fe_{2}(CO_{3})_{3}$ | $FePO_{4}$ |
| Copper (I) $Cu^{+}$ | $CuCl$ | $CuOH$ (unstable, usually forms $Cu_{2}O$ and $H_{2}O$ in solution) | $CuNO_{3}$ | $Cu_{2}SO_{4}$ | $Cu_{2}S$ | $Cu_{2}CO_{3}$ | $Cu_{3}PO_{4}$ |