for the following compounds, give the formulas
22) sodium phosphide
23) magnesium nitrate
24) lead (ii) sulfite
25) calcium phosphate
26) ammonium sulfate
27) silver cyanide
28) aluminum sulfide
29) beryllium chloride
30) copper (i) arsenide
31) iron (iii) oxide
32) gallium nitride
33) iron (ii) bromide
34) vanadium (v) phosphate
35) calcium oxide
36) magnesium acetate
37) aluminum sulfate
38) copper (i) carbonate
39) barium oxide
40) ammonium sulfite
41) silver bromide
42) lead (iv) nitrite

Question

Accepted Answer

# Explanation:
## Step1: Determine ion charges
Sodium has a +1 charge ($Na^+$) and phosphide has a -3 charge ($P^{3 -}$), so for sodium phosphide, we need 3 sodium ions to balance the charge of 1 phosphide ion.
## Step2: Write formula
The formula is $Na_3P$.

## Step3: For magnesium nitrate
Magnesium has a +2 charge ($Mg^{2+}$), nitrate ion is $NO_3^-$. We need 2 nitrate ions to balance the +2 charge of magnesium. The formula is $Mg(NO_3)_2$.

## Step4: For lead (II) sulfite
Lead (II) has a +2 charge ($Pb^{2+}$), sulfite ion is $SO_3^{2 -}$. The formula is $PbSO_3$.

## Step5: For calcium phosphate
Calcium has a +2 charge ($Ca^{2+}$), phosphate ion is $PO_4^{3 -}$. To balance the charges, we need 3 calcium ions and 2 phosphate ions. The formula is $Ca_3(PO_4)_2$.

## Step6: For ammonium sulfate
Ammonium ion is $NH_4^+$, sulfate ion is $SO_4^{2 -}$. We need 2 ammonium ions to balance the - 2 charge of sulfate. The formula is $(NH_4)_2SO_4$.

## Step7: For silver cyanide
Silver has a +1 charge ($Ag^+$), cyanide ion is $CN^-$. The formula is $AgCN$.

## Step8: For aluminum sulfide
Aluminum has a +3 charge ($Al^{3+}$), sulfide ion is $S^{2 -}$. We need 2 aluminum ions and 3 sulfide ions to balance the charges. The formula is $Al_2S_3$.

## Step9: For beryllium chloride
Beryllium has a +2 charge ($Be^{2+}$), chloride ion is $Cl^-$. We need 2 chloride ions to balance the +2 charge of beryllium. The formula is $BeCl_2$.

## Step10: For copper (I) arsenide
Copper (I) has a +1 charge ($Cu^+$), arsenide ion is $As^{3 -}$. We need 3 copper ions to balance the -3 charge of arsenide. The formula is $Cu_3As$.

## Step11: For iron (III) oxide
Iron (III) has a +3 charge ($Fe^{3+}$), oxide ion is $O^{2 -}$. We need 2 iron ions and 3 oxide ions to balance the charges. The formula is $Fe_2O_3$.

## Step12: For gallium nitride
Gallium has a +3 charge ($Ga^{3+}$), nitride ion is $N^{3 -}$. The formula is $GaN$.

## Step13: For iron (II) bromide
Iron (II) has a +2 charge ($Fe^{2+}$), bromide ion is $Br^-$. We need 2 bromide ions to balance the +2 charge of iron. The formula is $FeBr_2$.

## Step14: For vanadium (V) phosphate
Vanadium (V) has a +5 charge ($V^{5+}$), phosphate ion is $PO_4^{3 -}$. We need 3 vanadium ions and 5 phosphate ions to balance the charges. The formula is $V_3(PO_4)_5$.

## Step15: For calcium oxide
Calcium has a +2 charge ($Ca^{2+}$), oxide ion is $O^{2 -}$. The formula is $CaO$.

## Step16: For magnesium acetate
Magnesium has a +2 charge ($Mg^{2+}$), acetate ion is $C_2H_3O_2^-$. We need 2 acetate ions to balance the +2 charge of magnesium. The formula is $Mg(C_2H_3O_2)_2$.

## Step17: For aluminum sulfate
Aluminum has a +3 charge ($Al^{3+}$), sulfate ion is $SO_4^{2 -}$. We need 2 aluminum ions and 3 sulfate ions to balance the charges. The formula is $Al_2(SO_4)_3$.

## Step18: For copper (I) carbonate
Copper (I) has a +1 charge ($Cu^+$), carbonate ion is $CO_3^{2 -}$. We need 2 copper ions to balance the -2 charge of carbonate. The formula is $Cu_2CO_3$.

## Step19: For barium oxide
Barium has a +2 charge ($Ba^{2+}$), oxide ion is $O^{2 -}$. The formula is $BaO$.

## Step20: For ammonium sulfite
Ammonium ion is $NH_4^+$, sulfite ion is $SO_3^{2 -}$. We need 2 ammonium ions to balance the -2 charge of sulfite. The formula is $(NH_4)_2SO_3$.

## Step21: For silver bromide
Silver has a +1 charge ($Ag^+$), bromide ion is $Br^-$. The formula is $AgBr$.

## Step22: For lead (IV) nitrite
Lead (IV) has a +4 charge ($Pb^{4+}$), nitrite ion is $NO_2^-$. We need 4 nitrite ions to balance the +4 charge of lead. The formula is $Pb(NO_2)_4$.

# Answer:
22) $Na_3P$
23) $Mg(NO_3)_2$
24) $PbSO_3$
25) $Ca_3(PO_4)_2$
26) $(NH_4)_2SO_4$
27) $AgCN$
28) $Al_2S_3$
29) $BeCl_2$
30) $Cu_3As$
31) $Fe_2O_3$
32) $GaN$
33) $FeBr_2$
34) $V_3(PO_4)_5$
35) $CaO$
36) $Mg(C_2H_3O_2)_2$
37) $Al_2(SO_4)_3$
38) $Cu_2CO_3$
39) $BaO$
40) $(NH_4)_2SO_3$
41) $AgBr$
42) $Pb(NO_2)_4$

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QUESTION IMAGE

Question

Explanation:

Step1: Determine ion charges

Step2: Write formula

Step3: For magnesium nitrate

Step4: For lead (II) sulfite

Step5: For calcium phosphate

Step6: For ammonium sulfate

Step7: For silver cyanide

Step8: For aluminum sulfide

Step9: For beryllium chloride

Step10: For copper (I) arsenide

Step11: For iron (III) oxide

Step12: For gallium nitride

Step13: For iron (II) bromide

Step14: For vanadium (V) phosphate

Step15: For calcium oxide

Step16: For magnesium acetate

Step17: For aluminum sulfate

Step18: For copper (I) carbonate

Step19: For barium oxide

Step20: For ammonium sulfite

Step21: For silver bromide

Step22: For lead (IV) nitrite

Answer: