Question

ionic bonds
name the following ionic compounds (rule 1 and 2):

1. nabr
2. cao
3. li₂o
4. mgbr₂
5. mgbr₂
6. ba(oh)₂
7. fecl₃
8. pbo
9. (nh₄)so₄
10. cos

write the formulas for the following ionic compounds (rule 1 and 2). must show all work!!

1. potassium iodine
2. magnesium oxide
3. aluminum chloride
4. sodium nitrate
5. calcium carbonate
6. lithium sulfate
7. beryllium phosphide
8. magnesium hydroxide
9. cobalt (ii) nitride
10. chromium (ii) fluoride
11. sodium phosphate
12. aluminum carbonate

Explanation:

Step1: Determine the ions

For each compound, identify the cation (positive ion) and anion (negative ion). For example, in \(NaBr\), \(Na^{+}\) is the cation and \(Br^{-}\) is the anion.

Step2: Name the compound

Name the cation first, then the anion. For monatomic anions, change the ending to -ide. For polyatomic anions, use their specific names.

• \(NaBr\): Sodium (from \(Na^{+}\)) and bromide (from \(Br^{-}\)) → Sodium bromide
• \(CaO\): Calcium (\(Ca^{2+}\)) and oxide (\(O^{2 -}\)) → Calcium oxide
• \(Li_{2}O\): Lithium (\(Li^{+}\)) and oxide (\(O^{2 -}\)) → Lithium oxide
• \(MgBr_{2}\): Magnesium (\(Mg^{2+}\)) and bromide (\(Br^{-}\)) → Magnesium bromide
• \(Be(OH)_{2}\): Beryllium (\(Be^{2+}\)) and hydroxide (\(OH^{-}\)) → Beryllium hydroxide
• \(FeCl_{3}\): Iron (\(Fe^{3+}\)) and chloride (\(Cl^{-}\)) → Iron(III) chloride (since iron has a +3 charge)
• \(PbO\): Lead (\(Pb^{2+}\)) and oxide (\(O^{2 -}\)) → Lead(II) oxide
• \((NH_{4})_{2}SO_{4}\): Ammonium (\(NH_{4}^{+}\)) and sulfate (\(SO_{4}^{2 -}\)) → Ammonium sulfate
• \(CoS\): Cobalt (\(Co^{2+}\)) and sulfide (\(S^{2 -}\)) → Cobalt(II) sulfide

For writing formulas:

Step1: Determine the ions

Identify the cation and anion with their charges.

• Potassium iodide: \(K^{+}\) (potassium) and \(I^{-}\) (iodide). The charges balance (\(1 + (- 1)=0\)) → \(KI\)
• Magnesium oxide: \(Mg^{2+}\) and \(O^{2 -}\). Charges balance (\(2+(-2) = 0\)) → \(MgO\)
• Aluminum chloride: \(Al^{3+}\) and \(Cl^{-}\). To balance (\(3+3\times(-1)=0\)) → \(AlCl_{3}\)
• Sodium nitrate: \(Na^{+}\) and \(NO_{3}^{-}\). Charges balance (\(1+(-1) = 0\)) → \(NaNO_{3}\)
• Calcium carbonate: \(Ca^{2+}\) and \(CO_{3}^{2 -}\). Charges balance (\(2+(-2)=0\)) → \(CaCO_{3}\)
• Lithium sulfate: \(Li^{+}\) and \(SO_{4}^{2 -}\). To balance (\(2\times1+(-2)=0\)) → \(Li_{2}SO_{4}\)
• Beryllium phosphide: \(Be^{2+}\) and \(P^{3 -}\). To balance (\(3\times2 + 2\times(-3)=0\)) → \(Be_{3}P_{2}\)
• Magnesium hydroxide: \(Mg^{2+}\) and \(OH^{-}\). To balance (\(2+2\times(-1)=0\)) → \(Mg(OH)_{2}\)
• Cobalt(II) nitride: \(Co^{2+}\) and \(N^{3 -}\). To balance (\(3\times2+2\times(-3)=0\)) → \(Co_{3}N_{2}\)
• Chromium(II) fluoride: \(Cr^{2+}\) and \(F^{-}\). To balance (\(2 + 2\times(-1)=0\)) → \(CrF_{2}\)
• Sodium phosphate: \(Na^{+}\) and \(PO_{4}^{3 -}\). To balance (\(3\times1+(-3)=0\)) → \(Na_{3}PO_{4}\)
• Aluminum carbonate: \(Al^{3+}\) and \(CO_{3}^{2 -}\). To balance (\(2\times3+3\times(-2)=0\)) → \(Al_{2}(CO_{3})_{3}\)

Answer:

1. Sodium bromide
2. Calcium oxide
3. Lithium oxide
4. Magnesium bromide
5. Beryllium hydroxide
6. Iron(III) chloride
7. Lead(II) oxide
8. Ammonium sulfate
9. Cobalt(II) sulfide
10. \(KI\)
11. \(MgO\)
12. \(AlCl_{3}\)
13. \(NaNO_{3}\)
14. \(CaCO_{3}\)
15. \(Li_{2}SO_{4}\)
16. \(Be_{3}P_{2}\)
17. \(Mg(OH)_{2}\)
18. \(Co_{3}N_{2}\)
19. \(CrF_{2}\)
20. \(Na_{3}PO_{4}\)
21. \(Al_{2}(CO_{3})_{3}\)