How do you write the formula of an ionic compound?

Question

Natalie Anton · Accepted Answer

It is your goal to neutralize the compound.

Consider the following instance:

#Na^(+)# + #SO_4^(2-)#

We need to balance the charges, the easiest way to balance this charge is by looking at the overall charge of the ions involved. The #Na# ion has a #+1# charge and the #SO_4# ion has a #-2# charge. In order to give balance, we must have two Na ions to give an overall #+2# with regards to Na: this, thus, neutralises the compound. Therefore, the formula is:

#Na_2SO_4#

If you're asked to balance an ionic compound such as Iron(III) Hydroxide, write down the formula. We know that Fe (Iron) has a #3+# charge and the hydroxide ion (OH) has a #1-# charge - as a result, the compounds in their individualised forms are:

#Fe^(3+)# and #OH^(-)#

We must add brackets around the hydroxide ion to give the following in order to balance this:

#Fe(OH)_3#

As a result, the charges are balanced, and an accurate ionic formula is provided.

Luna Chen · Answer

undefined Once the charges are balanced to produce a neutral compound, write the symbols for the cation and anion in that order, representing the corresponding charges.