# Question 4.8: Name the following binary ionic compounds, each of which con......

Name the following binary ionic compounds, each of which contains a metal whose ionic charge can vary.

a.  AuCl          b.  $Fe_{2}O_{3}$

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We will need to indicate the magnitude of the charge on the metal ion in the name of each of these compounds by means of a Roman numeral.
a. To calculate the metal ion charge, use the fact that total ionic charge (both positive and negative) must add to zero.
$\quad\quad\quad\quad$(Gold charge) + (chlorine charge) = 0
The chloride ion has a – 1 charge (Section 4.5). Therefore,
$\quad\quad\quad\quad$(Gold charge) + (-1) = 0
Thus,
$\quad\quad\quad\quad$Gold charge = +1
Therefore, the gold ion present is $Au^{+}$, and the name of the compound is gold(I) chloride.
b. For charge balance in this compound we have the equation
$\quad\quad\quad\quad$2(iron charge) + 3(oxygen charge) = 0
Note that we have to take into account the number of each kind of ion present (2 and 3 in this case). Oxide ions carry a -2 charge (Section 4.5). Therefore,
$\quad\quad\quad\quad$ 2(iron charge) + 3(-2) = 0
$\quad\quad\quad\quad\quad\quad\quad$2(iron charge) = +6
$\quad\quad\quad\quad\quad\quad\quad\quad$Iron charge = +3
Here, we are interested in the charge on a single iron ion (+3) and not in the total positive charge present (+6). The compound is named iron(III) oxide because $Fe^{3+}$ ions are present. As is the case for all ionic compounds, the name does not contain any reference to the numerical subscripts in the compound’s formula.

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