ionic bonds
name the following ionic compounds (rule 1 and 2):
1. nabr
2. cao
3. li₂o
4. mgbr₂
5. mgbr₂
6. be(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!!
11. potassium iodine
12. magnesium oxide
13. aluminum chloride
14. sodium nitrate
15. calcium carbonate
16. lithium sulfate
17. beryllium phosphide
18. magnesium hydroxide
19. cobalt (ii) nitride
20. chromium (ii) fluoride
21. sodium phosphate
22. aluminum carbonate

Question

Accepted Answer

# Explanation:
## Step1: Identify ions
For each compound, identify the cation and anion. For example, in potassium iodide, the cation is $K^{+}$ (potassium ion) and the anion is $I^{-}$ (iodide ion).
## Step2: Apply charge balance
The formula of an ionic compound is determined by balancing the charges of the cations and anions. The overall charge of the compound should be zero.
   - For potassium iodide ($K^{+}$ and $I^{-}$): Since the charges are $+ 1$ and $-1$ respectively, the formula is $KI$ (1:1 ratio).
   - For magnesium oxide ($Mg^{2+}$ and $O^{2 -}$): The charges are $+2$ and $-2$, so the formula is $MgO$ (1:1 ratio).
   - For aluminum chloride ($Al^{3+}$ and $Cl^{-}$): To balance $+3$ and $-1$ charges, we need 3 $Cl^{-}$ ions for 1 $Al^{3+}$ ion. So the formula is $AlCl_{3}$.
   - For sodium nitrate ($Na^{+}$ and $NO_{3}^{-}$): Charges are $+1$ and $-1$, formula is $NaNO_{3}$.
   - For calcium carbonate ($Ca^{2+}$ and $CO_{3}^{2-}$): Charges $+2$ and $-2$, formula $CaCO_{3}$.
   - For lithium sulfate ($Li^{+}$ and $SO_{4}^{2-}$): To balance $+1$ and $-2$, 2 $Li^{+}$ ions are needed. Formula $Li_{2}SO_{4}$.
   - For beryllium phosphide ($Be^{2+}$ and $P^{3-}$): Using the cross - multiply method (charges as sub - scripts), we get $Be_{3}P_{2}$ ($2\times3 = 3\times2$ to balance charges).
   - For magnesium hydroxide ($Mg^{2+}$ and $OH^{-}$): 2 $OH^{-}$ ions are needed for 1 $Mg^{2+}$ ion. Formula $Mg(OH)_{2}$.
   - For cobalt (II) nitride ($Co^{2+}$ and $N^{3-}$): Cross - multiply charges ($2$ and $3$), formula $Co_{3}N_{2}$.
   - For chromium (II) fluoride ($Cr^{2+}$ and $F^{-}$): 2 $F^{-}$ ions for 1 $Cr^{2+}$ ion. Formula $CrF_{2}$.
   - For sodium phosphate ($Na^{+}$ and $PO_{4}^{3-}$): 3 $Na^{+}$ ions for 1 $PO_{4}^{3-}$ ion. Formula $Na_{3}PO_{4}$.
   - For aluminum carbonate ($Al^{3+}$ and $CO_{3}^{2-}$): Cross - multiply charges ($3$ and $2$), formula $Al_{2}(CO_{3})_{3}$.

# Answer:
11. $KI$
12. $MgO$
13. $AlCl_{3}$
14. $NaNO_{3}$
15. $CaCO_{3}$
16. $Li_{2}SO_{4}$
17. $Be_{3}P_{2}$
18. $Mg(OH)_{2}$
19. $Co_{3}N_{2}$
20. $CrF_{2}$
21. $Na_{3}PO_{4}$
22. $Al_{2}(CO_{3})_{3}$

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QUESTION IMAGE

Question

Explanation:

Step1: Identify ions

Step2: Apply charge balance

Answer: