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Virty [35]
2 years ago
5

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

Chemistry
1 answer:
lidiya [134]2 years ago
3 0

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

<h3>Mole calculation</h3>

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

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If you want to stop the reaction at Ketone stage then you are required to use another mild reactive organometallic compound. In our case we will use Organocuprates. Organocuprates are also known as Gilman Reagents. These reagents does not add to ketones, aldehydes and esters but they can add to acid halides to produce Ketones.

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