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Virty [35]
1 year ago
5

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

Chemistry
1 answer:
lidiya [134]1 year 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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The halogens mostly form single bond with the other elements by gaining one electron and -1 charge. These are most reactive non-metals.

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Fluorine:

1. It is yellow in color.

2. It is flammable gas.

3. It is highly corrosive.

4. Fluorine has pungent smell.

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1. It is greenish-yellow irritating gas.

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1. It is present in solid form.

2. It is crystalline in nature.

3. It is very corrosive and has pungent odor.

4. It can not react with oxygen and nitrogen.

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