Write formulas for the following compounds. A. Zinc chloride B. Lead(IV)oxide C. Silver bromide D. Sodium phosphate E. Magnesium sulfide F. Cobalt(II)flouride G. Barium oxide H. Calcium phosphide I. Copper(II)cyanide J. Hydrogen selenide K. Copper(I)nitride L. Nickel(II)acetate M. Potassium arsenate N. Nickel(II) oxalate O. Gallium(III)acetate P. Ammonium chloride. Tht is all of them they hav to hav the formula for the compounds can some plz help me with this please
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@Michael6fantorres Think about what ions the different metals would create. Sometimes it is even stated if it can take multiple charges. Lets take a look for example at A:
Zinc only exists are a divalent cation meaning it will have +2. The halides are monovalent anions so chloride has -1. Therefore the formula for zinc chloride must be \(\sf ZnCl_2\)
Follow that procedure and you are safe most of the time. You just need to figure out the oxidation states which is the hardest part.
I can also help with B: Lead(IV)oxide
We are being told that Lead is in it's +4 oxidation state (IV = 4 roman numbers).
Oxygen is in main group 16 and we can therefore deduct it would create a divalent anion (-2). With that information we can write the formula as:
\(\large \sf PbO_2\)