Question

Ag+ and SO42−
What's the name of the ionic compound?

Answer 1

@MrMudd183

Answer 2

is it Silver (II) sulfate?

Answer 3

\(\color{#0cbb34}{\text{Originally Posted by}}\) @iuytyuioiuytyuiop
is it Silver (II) sulfate?
\(\color{#0cbb34}{\text{End of Quote}}\)
I think so

Answer 4

sulfate

Answer 5

That's correct!

Answer 6

thank you guys

Answer 7

\(\color{#0cbb34}{\text{Originally Posted by}}\) @iuytyuioiuytyuiop
thank you guys
\(\color{#0cbb34}{\text{End of Quote}}\)
Np

Answer 8

Actually, I didn't see that you used two II

Our silver atom has a 1+ charge

Answer 9

so its not the correct option?

Answer 10

Alternatively, you can just call it silver sulfate

Answer 11

the options are silver sulfate and another option is silver (ii) sulfate

Answer 12

Silver (ii) would have a +2 charge and so with sulfate \( (\text{SO}_4)^{-2}\) you would end up with \(\text{AgSO}_4\) to balance the charge

Answer 13

However, with \(\text{Ag}^{+}\) and \((\text{SO}_4)^{-2}\) to make a neutral polyatomic ion, we would need two silver (i) to balance the -2 from sulfate. That would get us \(\text{Ag}_2 \text{SO}_4\)

Answer 14

a
Silver sulfate
b
Silver (II) sulfite
c
Silver (II) sulfate
d
Silver (I) sulfite

Answer 15

but its Ag2SO4

Answer 16

Exactly, which would make it silver sulfate

Answer 17

so its A

Answer 18

Yes

Answer 19

I thought the formula is Ag+SO42-

Answer 20

You have to balance the polyatomic ions so that the compound can be neutral.


\(\text{Ag}^{+}\) has a +1 charge
\((\text{SO}_4)^{-2}\) has a -2 charge

That means we need \( 2~(\text{Ag}^{+})\) for \(1~(\text{SO}_4)^{-2}\)
This will make it \( 2\text{Ag}^{+2}\) and \((\text{SO}_4)^{-2}\)

The +2 and -2 can cancel each other out and we have ourselves the neutral silver sulfate compound. Also we have to move that 2 from the coefficient to a subscript so we get
\(\text{Ag}_2 \text{SO}_4\)

Answer 21

i see

Answer 22

okay

Answer 23

It makes sense thank you

Answer 24

My pleasure!