Question

naming ionic compounds practice worksheet
name the following ionic compounds:
) nh₄cl
) fe(no₃)₃
tibr₃
cu₃p
snse₂
gaas
pb(so₄)₂
be(hco₃)₂
write the formulas for the following compounds:
chromium (vi) phosphate
vanadium (iv) carbonate
cobalt (iii) oxide
titanium (ii) acetate
vanadium (v) sulfide
chromium (iii) hydroxide
thallium iodide
lead (ii) nitride
silver bromide
lots of ionic naming practice problems
name the following ionic compounds:

1. nabr
2. sc(oh)₃
3. v₂(so₄)₃
4. nh₄f
5. caco₃
6. nipo₄

7)

1. zn₃p₂
2. sr(c₂h₃o₂)₂
3. cu₂o
4. ag₃po₄
5. yclo₃
6. sns₂

14)
15)

1. pb₃n₂
2. coco₃

18)
19)

1. fe(hco₃)₂

Explanation:

Step1: Recall naming rules for ionic compounds

For naming ionic compounds, we name the cation first followed by the anion. For poly - atomic anions, we use their specific names. For metals with variable oxidation states, we indicate the oxidation state in Roman numerals in parentheses.

Step2: Name $NH_4Cl$

The cation is ammonium ($NH_4^+$) and the anion is chloride ($Cl^-$), so the name is ammonium chloride.

Step3: Name $Fe(NO_3)_3$

The cation is iron(III) as the oxidation state of iron is + 3 (since nitrate is $NO_3^-$ and there are 3 of them, so iron must have a + 3 charge to balance the - 3 charge from the nitrates). The anion is nitrate. So the name is iron(III) nitrate.

Step4: Name $TiBr_3$

The cation is titanium(III) (as titanium has an oxidation state of + 3 since there are 3 bromide ions, $Br^-$) and the anion is bromide. So the name is titanium(III) bromide.

Step5: Name $Cu_3P$

The cation is copper(I) (as there are 3 copper atoms and 1 phosphide ion $P^{3 - }$, so each copper has a + 1 charge). The anion is phosphide. So the name is copper(I) phosphide.

Step6: Name $SnSe_2$

The cation is tin(IV) (since there are 2 selenide ions $Se^{2 - }$, so tin has a + 4 charge to balance the - 4 charge from the selenides). The anion is selenide. So the name is tin(IV) selenide.

Step7: Name $GaAs$

The cation is gallium and the anion is arsenide. So the name is gallium arsenide.

Step8: Name $Pb(SO_4)_2$

The cation is lead(IV) (as sulfate is $SO_4^{2 - }$ and there are 2 of them, so lead has a + 4 charge to balance the - 4 charge from the sulfates). The anion is sulfate. So the name is lead(IV) sulfate.

Step9: Name $Be(HCO_3)_2$

The cation is beryllium and the anion is bicarbonate. So the name is beryllium bicarbonate.

Step10: Name $NaBr$

The cation is sodium and the anion is bromide. So the name is sodium bromide.

Step11: Name $Sc(OH)_3$

The cation is scandium(III) (as there are 3 hydroxide ions $OH^-$) and the anion is hydroxide. So the name is scandium(III) hydroxide.

Step12: Name $V_2(SO_4)_3$

The cation is vanadium(III) (since sulfate is $SO_4^{2 - }$ and there are 3 of them with a total charge of - 6, and there are 2 vanadium atoms, so each vanadium has a + 3 charge). The anion is sulfate. So the name is vanadium(III) sulfate.

Step13: Name $NH_4F$

The cation is ammonium and the anion is fluoride. So the name is ammonium fluoride.

Step14: Name $CaCO_3$

The cation is calcium and the anion is carbonate. So the name is calcium carbonate.

Step15: Name $NiPO_4$

The cation is nickel(III) (as phosphate is $PO_4^{3 - }$, so nickel has a + 3 charge to balance the - 3 charge from the phosphate). The anion is phosphate. So the name is nickel(III) phosphate.

Step16: Name $Zn_3P_2$

The cation is zinc and the anion is phosphide. So the name is zinc phosphide.

Step17: Name $Sr(C_2H_3O_2)_2$

The cation is strontium and the anion is acetate. So the name is strontium acetate.

Step18: Name $Cu_2O$

The cation is copper(I) (as there are 2 copper atoms and 1 oxide ion $O^{2 - }$, so each copper has a + 1 charge). The anion is oxide. So the name is copper(I) oxide.

Step19: Name $Ag_3PO_4$

The cation is silver and the anion is phosphate. So the name is silver phosphate.

Step20: Name $YClO_3$

The cation is yttrium(III) (as chlorate is $ClO_3^-$ and yttrium has a + 3 charge to balance the - 1 charge from the chlorate in a neutral compound). The anion is chlorate. So the name is yttrium(III) chlorate.

Step21: Name $SnS_2$

The cation is tin(IV) (since there are 2 sulfide ions $S^{2 - }$, so tin has a + 4 charge to balance the - 4 charge from the sulfides). The anion is sulfide. So the name is tin(IV) sulfide.

Step22: Name $Pb_3N_2$

The cation is lead(II) (as there are 3 lead atoms and 2 nitride ions $N^{3 - }$, so each lead has a + 2 charge to balance the - 6 charge from the nitrides). The anion is nitride. So the name is lead(II) nitride.

Step23: Name $CoCO_3$

The cation is cobalt(II) (as carbonate is $CO_3^{2 - }$, so cobalt has a + 2 charge to balance the - 2 charge from the carbonate). The anion is carbonate. So the name is cobalt(II) carbonate.

Step24: Name $Fe(HCO_3)_2$

The cation is iron(II) (as there are 2 bicarbonate ions $HCO_3^-$ and iron has a + 2 charge to balance the - 2 charge from the bicarbonates). The anion is bicarbonate. So the name is iron(II) bicarbonate.

For writing formulas:

Step1: Chromium(VI) phosphate

Chromium has a + 6 charge ($Cr^{6+}$) and phosphate is $PO_4^{3 - }$. To balance the charges, we need 2 phosphate ions for 1 chromium ion. The formula is $Cr(PO_4)_2$.

Step2: Vanadium(IV) carbonate

Vanadium has a + 4 charge ($V^{4+}$) and carbonate is $CO_3^{2 - }$. To balance the charges, we need 2 carbonate ions for 1 vanadium ion. The formula is $V(CO_3)_2$.

Step3: Cobalt(III) oxide

Cobalt has a + 3 charge ($Co^{3+}$) and oxide is $O^{2 - }$. To balance the charges, we need 2 cobalt ions and 3 oxide ions. The formula is $Co_2O_3$.

Step4: Titanium(II) acetate

Titanium has a + 2 charge ($Ti^{2+}$) and acetate is $C_2H_3O_2^-$. To balance the charges, we need 2 acetate ions for 1 titanium ion. The formula is $Ti(C_2H_3O_2)_2$.

Step5: Vanadium(V) sulfide

Vanadium has a + 5 charge ($V^{5+}$) and sulfide is $S^{2 - }$. To balance the charges, we need 2 vanadium ions and 5 sulfide ions. The formula is $V_2S_5$.

Step6: Chromium(III) hydroxide

Chromium has a + 3 charge ($Cr^{3+}$) and hydroxide is $OH^-$. To balance the charges, we need 3 hydroxide ions for 1 chromium ion. The formula is $Cr(OH)_3$.

Step7: Thallium iodide

Assuming thallium in its common + 1 oxidation state ($Tl^+$) and iodide is $I^-$, the formula is $TlI$.

Step8: Lead(II) nitride

Lead has a + 2 charge ($Pb^{2+}$) and nitride is $N^{3 - }$. To balance the charges, we need 3 lead ions and 2 nitride ions. The formula is $Pb_3N_2$.

Step9: Silver bromide

Silver has a + 1 charge ($Ag^+$) and bromide is $Br^-$. The formula is $AgBr$.

Answer:

1. ammonium chloride
2. iron(III) nitrate
3. titanium(III) bromide
4. copper(I) phosphide
5. tin(IV) selenide
6. gallium arsenide
7. lead(IV) sulfate
8. beryllium bicarbonate
9. sodium bromide
10. scandium(III) hydroxide
11. vanadium(III) sulfate
12. ammonium fluoride
13. calcium carbonate
14. nickel(III) phosphate
15. zinc phosphide
16. strontium acetate
17. copper(I) oxide
18. silver phosphate
19. yttrium(III) chlorate
20. tin(IV) sulfide
21. lead(II) nitride
22. cobalt(II) carbonate
23. iron(II) bicarbonate

Formulas:

1. $Cr(PO_4)_2$
2. $V(CO_3)_2$
3. $Co_2O_3$
4. $Ti(C_2H_3O_2)_2$
5. $V_2S_5$
6. $Cr(OH)_3$
7. $TlI$
8. $Pb_3N_2$
9. $AgBr$