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pochemuha
3 years ago
12

Sodium electron configuration

Chemistry
1 answer:
Helen [10]3 years ago
8 0

Answer:  [Ne] 3s¹ sodium electron configuration

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Explanation:

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The ammonia molecule in the diagram has the observed bond orientation because ...
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Answer:

  • Nitrogen has four pairs of electrons: 3 bonds and 1 lone pair in the valence shell;
  • Electrons repel one another based on the VSEPR theory;
  • Nitrogen has a total of 7 protons (its atomic number is 7) in its nucleus.

Explanation:

The shape and the bond orientation of molecules and ions are both explained by the valences shell electron pair repulsion theory (VSEPR).

Ammonia, NH_3, is a molecule which contains three N-H bonds, as well as one lone pair on nitrogen. According to the VSEPR theory, molecules try to acquire a shape which would minimize the repulsion exhibited by the electron clouds present, that is, between the bonding (shared in a bond) and non-bonding (lone pair) electrons.

In VSEPR, our main step is to calculate the steric number, this is the sum of the number of bonds (ignoring the multiplicity of any bond) and the lone pairs on a central atom. In ammonia, we have 3 bonds and 1 lone pair, totaling to a steric number of 4. A steric number of 4 without any lone pairs on a central atom and just bonds would yield a tetrahedral shape with bond angles of 109.5^o.

Now, in this case, since we have a lone pair instead of a bond, it is repelling stronger decreasing the bond angles to about 107^o.

The greater the number of lone pairs, the lower the angle becomes.

To summarize:

  • Nitrogen has four pairs of electrons: 3 bonds and 1 lone pair in the valence shell;
  • Electrons repel one another based on the VSEPR theory;
  • Nitrogen has a total of 7 protons (its atomic number is 7) in its nucleus.
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Explanation:

All atoms and molecules have London Dispersion Forces between them, but they are usually overshadowed but the much stronger forces. In this scenario the major attractive force in HF molecules are hydrogen bonds. Hydrogen bonds are electrostatic forces of attraction found when Hydrogen is bonded to a more electronegative atom such as Oxygen, Chlorine and Fluorine.

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