Question

Consider the compound Cu(NO3)2 and answer the following questions.
a.What is the name of this compound?
b.What is the molar mass of this compound? Explain how you calculated this value.

Answer 1

a) Copper (II) Nitrate
b) 187.56 g

Answer 2

How do you solve it? @redsox389

Answer 3

for b) you add up the individual masses of the atoms in the correct proportions.

for a) you have to use rules for transition metals

First you have to know the oxidation state of Cu, this is inferred from what it's bound to - the ligands.

The nitrate (\(NO_3^-\)) anion has a -1 charge (polyatomic ions is something you should already know). So we know that Cu must be 2+ (in order to balance the charges).

so we have \(Cu^{2+}\) and \(NO_3^-\) twice.

We name the metal: Copper
the charge in roman numerals: II
and the ligands: nitrate

So we have Copper(II)nitrate

The reason why we use the roman numerals to specify the oxidation state is because transition metals easily lose d electrons and their oxidation states wildly vary.

Answer 4

@iPwnBunnies

Answer 5

Yeah that's CCl4

Answer 6

Yay. :3