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Kobotan [32]
3 years ago
5

What type of bond would form between two atoms of phosphorus?

Chemistry
2 answers:
finlep [7]3 years ago
5 0

Answer: Option (A) is the correct answer.

Explanation:

Non-metals are the substances which tend to gain electrons from a donor atom in order to attain stability.

For example, atomic number of phosphorous is 15 and its electronic distribution is 2, 8, 5.

As it contains 5 valence electrons electrons therefore, it needs 3 more electrons in order to attain stability.

Hence, when one phosphorous atom combines with another phosphorous atom then it results in sharing of electrons. So, there will be formation a triple bond between the two phosphorous atoms.

Also, there will be one lone pair of electron on each phosphorous atom.

Thus, we can conclude that triple covalent bond would form between two atoms of phosphorus.

grin007 [14]3 years ago
4 0
Ans: A. Triple covalent bond.

Hope this helps!
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V = 4/3 x π x 7^3

Exact Form:
1372 π/ 3

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Which type of combination is a mixture?
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C.  physical

Explanation:

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Mixtures have the following properties:

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13. A mixture of MgCO3 and MgCO3.3H2O has a mass of 3.883 g. After heating to drive off all the water the mass is 2.927 g. What
rjkz [21]

Answer:

63.05% of MgCO3.3H2O by mass

Explanation:

<em>of MgCO3.3H2O in the mixture?</em>

The difference in masses after heating the mixture = Mass of water. With the mass of water we can find its moles and the moles and mass of MgCO3.3H2O to find the mass percent as follows:

<em>Mass water:</em>

3.883g - 2.927g = 0.956g water

<em>Moles water -18.01g/mol-</em>

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<em>Moles MgCO3.3H2O:</em>

0.05308 moles H2O * (1mol MgCO3.3H2O / 3mol H2O) =

0.01769 moles MgCO3.3H2O

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0.01769 moles MgCO3.3H2O * (138.3597g/mol) = 2.448g MgCO3.3H2O

<em>Mass percent:</em>

2.448g MgCO3.3H2O / 3.883g Mixture * 100 =

<h3>63.05% of MgCO3.3H2O by mass</h3>
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2 years ago
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