Question

A Group 2 metal with an electron configuration of [Ne]3s2 combines with fluorine (F2) to

Answer 1

The molar mass of the product is equal to 62g/mol.

Mole calculation

To calculate the molar mass of a compound it is necessary to have knowledge of the atomic mass of all the elements involved.

In the case of the question, we have the reaction between flourine and magnesium, which represents the element of group 2 with the presented electronic configuration.

Thus, we have the following reaction:

                                   $Mg^{+2} + 2F^{-1} = MgF_2$

So, just add the molar masses, having:

$MM_Mg = 24.3g/mol\\MM_F = 19g/mol$

                                               $24.3 + 19 + 19 = 62.3g$

So, the molar mass of the product, round to the nearest tenth, is equal to 62g/mol.

Learn more about mole calculation in: brainly.com/question/2845237