Write the empirical formula of at least four binary ionic compounds that could be formed from the following ions: Mg2+, V5+, Br-, S2-

, , and are four binary ionic compounds that could be formed.

Explanation:

For formation of a neutral ionic compound, the charges on cation and anion must be balanced. The cation is formed by loss of electrons by metals and anions are formed by gain of electrons by non metals.

Mg is having an oxidation state of +2 called as cation and is an anion with oxidation state of -2. Thus they combine and their oxidation states are exchanged and written in simplest whole number ratios to give neutral . Also cation and can combine and their oxidation states are exchanged and written in simplest whole number ratios to give neutral .

Also Vanadium is having an oxidation state of +5 called as cation and is an anion with oxidation state of -2. Thus they combine and their oxidation states are exchanged and written in simplest whole number ratios to give neutral . Also cation and anion can combine and their oxidation states are exchanged and written in simplest whole number ratios to give neutral .

since electrons are negative the answer is neagtaive

as given the equation is

2al + 6 hcl > 2 alcl3 + 3 h2(g)

as per equation two moles of aluminum reacts with six moles of hcl to give two moles of alcl3 and three moles of hydrogen gas

given: three moles of al are present and 7 moles of hcl

for three moles of aluminum nine moles of hcl will be required

however as 7 moles of hcl are present so the limiting reagent is hcl

hcl is going to decide the number of moles of product formed

when six moles of hcl are present = 3 moles of h2 are formed

when one mole of hcl is present == 3/6 mole sof h2 will be formed

when 7 moles of hcl are present = 3 x 7/ 6 moles of h2 will be formed = 3.5 moles of h2