QUESTION IMAGE
Question
an ionic compound has the formula au₂se₃. complete the table to determine the charge of the transition metal ion in this compound. enter a negative sign before negative numbers. positive numbers do not need a positive sign. in one formula unit what is the name of this ionic compound? table with rows: element (gold, selenium), charge of one ion, total charge of ion(s) in compound, number of ion(s) in compound* (yellow boxes for input in table and name dropdowns)
For Gold (Au) and Selenium (Se) in $\boldsymbol{Au_2Se_3}$:
Step 1: Determine charge of Selenium ion
Selenium is in group 16, so its ion is $Se^{2-}$ (charge = $-2$).
Step 2: Total charge of Selenium ions
Number of $Se^{2-}$ ions = 3.
Total charge = $3 \times (-2) = -6$.
Step 3: Charge of Gold ion
Let charge of $Au$ ion be $x$. Number of $Au$ ions = 2.
Total charge of $Au$ ions + Total charge of $Se$ ions = 0 (neutral compound).
$2x + (-6) = 0$
$2x = 6$
$x = +3$. So $Au$ has charge $+3$.
Step 4: Total charge of Gold ions
Total charge = $2 \times (+3) = +6$.
Step 5: Number of ions
From formula $Au_2Se_3$:
- Number of $Au^{3+}$ ions = 2.
- Number of $Se^{2-}$ ions = 3.
Filling the table:
| Element | Charge of One Ion | Total Charge of Ion(s) in Compound | Number of Ion(s) in Compound |
|---|---|---|---|
| Selenium (Se) | $-2$ | $-6$ | 3 |
Name of the ionic compound:
Gold(III) selenide (since Au has a +3 charge, we use Roman numerals for transition metal charge).
Final Answers for the Table:
- Gold: Charge = $\boldsymbol{+3}$, Total Charge = $\boldsymbol{+6}$, Number of Ions = $\boldsymbol{2}$
- Selenium: Charge = $\boldsymbol{-2}$, Total Charge = $\boldsymbol{-6}$, Number of Ions = $\boldsymbol{3}$
Name of the compound:
$\boldsymbol{\text{Gold(III) selenide}}$
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For Gold (Au) and Selenium (Se) in $\boldsymbol{Au_2Se_3}$:
Step 1: Determine charge of Selenium ion
Selenium is in group 16, so its ion is $Se^{2-}$ (charge = $-2$).
Step 2: Total charge of Selenium ions
Number of $Se^{2-}$ ions = 3.
Total charge = $3 \times (-2) = -6$.
Step 3: Charge of Gold ion
Let charge of $Au$ ion be $x$. Number of $Au$ ions = 2.
Total charge of $Au$ ions + Total charge of $Se$ ions = 0 (neutral compound).
$2x + (-6) = 0$
$2x = 6$
$x = +3$. So $Au$ has charge $+3$.
Step 4: Total charge of Gold ions
Total charge = $2 \times (+3) = +6$.
Step 5: Number of ions
From formula $Au_2Se_3$:
- Number of $Au^{3+}$ ions = 2.
- Number of $Se^{2-}$ ions = 3.
Filling the table:
| Element | Charge of One Ion | Total Charge of Ion(s) in Compound | Number of Ion(s) in Compound |
|---|---|---|---|
| Selenium (Se) | $-2$ | $-6$ | 3 |
Name of the ionic compound:
Gold(III) selenide (since Au has a +3 charge, we use Roman numerals for transition metal charge).
Final Answers for the Table:
- Gold: Charge = $\boldsymbol{+3}$, Total Charge = $\boldsymbol{+6}$, Number of Ions = $\boldsymbol{2}$
- Selenium: Charge = $\boldsymbol{-2}$, Total Charge = $\boldsymbol{-6}$, Number of Ions = $\boldsymbol{3}$
Name of the compound:
$\boldsymbol{\text{Gold(III) selenide}}$