What is the Latin system name for $CuCl_2$?

$CuCl_2$ is an ionic compound composed of the metal cation $Cu^(2+)$ and 2 $Cl^(_)$ anions. The best way to identify the charge is to to use the Periodic table ....

Chlorine has a high electro negativity of 3.0. Copper like most metals has a low electro negativity, So the is ionic making the compound an ionic salt.

$Al rarr Al^(3+) + 3e^-$; oxidation. $CuCl_2(aq) +2e^(-) rarr Cu(s)darr + 2Cl^-$; reduction. We cross-mulitply to remove the electrons. $3CuCl_2(aq) +2Al(s) rarr 2AlCl_3(aq) + 3Cu(s)darr$ A sheet of aluminum place...

Really, if you examine each molecule and atom as a unit, then almost everything is balanced already. We see one equivalent of $"Cu"^(2+)$ (copper(II)) on each side, and one equivalent...

Aluminum is oxidized to $Al^(3+)$. $Al(s) rarr Al^(3+) + 3e^(-)$ $(i)$ And cupric ion is reduced to zerovalent copper.... $Cu^(2+) + 2e^(-) rarr Cu(s)$ $(ii)$ We cross multiply to remove...

I'd start by looking at what is the most complicated and unbalanced, as we can see there is only 1 $Cu$ on the left hand side but there is two...

Aqueous sodium chloride, $"NaCl"$, will not react with aqueous copper(II) sulfate, $"CuSO"_4$, because the two potential products are soluble in aqueous solution. The chemical equation given to you is...

Zinc metal is oxidized to $Zn^(2+)$, whereas $Cu^(2+)$ (as cupric chloride) is reduced to copper metal. We can write the individual redox equations: $ Cu^(2+) + 2e^(-)rarrCu(s) $ $Zn(s) rarr...

Convert the given formula units of $"CuCl"_2"$ to moles by dividing by $6.022xx10^23$ formula units/mol, then determine the mass of $"CuCl"_2"$ by multiplying the moles of $"CuCl"_2"$ by its molar...

According to this law a reactant will produce same no of equivalent of product/s as its reacting mass has. here the equivalent mass of $CuCl_2$ = Formula wt /total valency...