The electronic configuration of two elements X and Y are given below:
where p = proton, n = neutron, e = electron.

When these two elements combine together to form a compound, give the mass (in grams) of one mole of this compound.

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Solution

$X = L i$ (lithium) and $Y = O$ (oxygen)

$∵$ Number of protons = Atomic number

Lithium and oxygen combine to form $L i_{2} O$ (lithium oxide).

Mass of 1 mole of $L i_{2} O$ = ( 2 $\times$ Molar mass of lithium )+ (Molar mass of oxygen )

= $2 \times (7) + 16 = 30 g$

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The electronic configuration of two elements X and Y are given below:where p = proton, n = neutron, e = electron. When these two elements combine together to form a compound, give the mass (in grams) of one mole of this compound.

X=Li (lithium) and Y=O (oxygen)∵ Number of protons = Atomic numberLithium and oxygen combine to form Li2O (lithium oxide).Mass of 1 mole of Li2O = ( 2×Molar mass of lithium )+ (Molar mass of oxygen ) = 2×(7)+16=30g

The electronic configuration of two elements X and Y are given below:
where p = proton, n = neutron, e = electron.

When these two elements combine together to form a compound, give the mass (in grams) of one mole of this compound.

$X = L i$ (lithium) and $Y = O$ (oxygen)

$∵$ Number of protons = Atomic number

Lithium and oxygen combine to form $L i_{2} O$ (lithium oxide).

Mass of 1 mole of $L i_{2} O$ = ( 2 $\times$ Molar mass of lithium )+ (Molar mass of oxygen )

= $2 \times (7) + 16 = 30 g$