Question

give the formulas from the names
1 gold (iii) nitrite
2 gold (i) sulfide
3 gold (iii) hydrogen sulfate
4 gold (iii) dihydrogen phosphate
a. au3no2 b. au(no2)3 c. au3(no2)3 d. au(no3)3 e. au3(h2po4)
f. au(hpo4)3 g. au(h2po3)3 h. au(h2po4)3 i. aus j. au2s k. au2s3
l. au3(hso4) m. au3(hso3) n. au(so3)3 o. au(so4)3 p. au(hso3)3
q. au(hso4)3 r. au3(hso4)3

Explanation:

Step1: Determine charge of gold(III)

Gold(III) has a charge of +3, written as $Au^{3 +}$.

Step2: Find charge of nitrite ion

Nitrite ion is $NO_{2}^{-}$ with a - 1 charge.

Step3: Balance charges for gold(III) nitrite

To balance the +3 charge of $Au^{3+}$, we need 3 $NO_{2}^{-}$ ions. So the formula is $Au(NO_{2})_{3}$.

Step4: Determine charge of gold(I)

Gold(I) has a charge of +1, written as $Au^{+}$.

Step5: Find charge of sulfide ion

Sulfide ion is $S^{2 -}$.

Step6: Balance charges for gold(I) sulfide

To balance the - 2 charge of $S^{2-}$, we need 2 $Au^{+}$ ions. So the formula is $Au_{2}S$.

Step7: Determine charge of gold(III) again

Gold(III) has a charge of +3, $Au^{3 +}$.

Step8: Find charge of hydrogen sulfate ion

Hydrogen sulfate ion is $HSO_{4}^{-}$ with a - 1 charge.

Step9: Balance charges for gold(III) hydrogen sulfate

To balance the +3 charge of $Au^{3+}$, we need 3 $HSO_{4}^{-}$ ions. So the formula is $Au(HSO_{4})_{3}$.

Step10: Determine charge of gold(III) once more

Gold(III) has a charge of +3, $Au^{3 +}$.

Step11: Find charge of dihydrogen phosphate ion

Dihydrogen phosphate ion is $H_{2}PO_{4}^{-}$ with a - 1 charge.

Step12: Balance charges for gold(III) dihydrogen phosphate

To balance the +3 charge of $Au^{3+}$, we need 3 $H_{2}PO_{4}^{-}$ ions. So the formula is $Au(H_{2}PO_{4})_{3}$.

Answer:

1. B. $Au(NO_{2})_{3}$
2. J. $Au_{2}S$
3. Q. $Au(HSO_{4})_{3}$
4. H. $Au(H_{2}PO_{4})_{3}$