A2.241-g sample of nickel reacts with oxygen to form 2.852 g of the metal oxide.
calculate the empirical formula for oxide.

The empirical formula is =

Explanation:

Given that:- Mass of nickel = 2.241 g

Mass of the oxide formed = 2.852 g

Mass of the oxygen reacted = Mass of the oxide formed - Mass of nickel  = 2.852 g - 2.241 g = 0.611 g

Molar mass of nickel  = 58.6934 g/mol

Moles of nickel = = 0.03818 mol

Molar mass of oxygen  = 15.999 g/mol

Moles of nickel = = 0.03818 mol

Taking the simplest ratio for Ni and O as:

0.03818 : 0.03818 = 1 : 1

The empirical formula is =

you need to take a look at the periodic system in order to sort these elements into pairs that would most likely exhibit similar chemical properties. first, you need to find elements that are found in the same group (groups are vertical in the periodic system), and then to see whether they have the same valence number. if they meet these criteria, they will have similar properties.

the first pair: ne (neon) and kr (krypton), are noble gases found in group 8

the second pair: li (lithium) and k (potassium), found in group 1

the third pair: s (sulfur) and te (tellurium), found in group 6