H2Se Lewis structure

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H₂Se (hydrogen selenide) has two hydrogen atoms and one selenium atom.

In the H₂Se Lewis structure, there are two single bonds around the selenium atom, with two hydrogen atoms attached to it, and on the selenium atom, there are two lone pairs.

Steps

Here’s how you can easily draw the H₂Se Lewis structure step by step:

#1 Draw a rough skeleton structure
#2 Mention lone pairs on the atoms
#3 If needed, mention formal charges on the atoms

Now, let’s take a closer look at each step mentioned above.

#1 Draw a rough skeleton structure

• First, determine the total number of valence electrons

In the periodic table, hydrogen lies in group 1, and selenium lies in group 16.

Hence, hydrogen has one valence electron and selenium has six valence electrons.

Since H₂Se has two hydrogen atoms and one selenium atom, so…

Valence electrons of two hydrogen atoms = 1 × 2 = 2
Valence electrons of one selenium atom = 6 × 1 = 6

And the total valence electrons = 2 + 6 = 8

Learn how to find: Hydrogen valence electrons and Selenium valence electrons

• Second, find the total electron pairs

We have a total of 8 valence electrons. And when we divide this value by two, we get the value of total electron pairs.

Total electron pairs = total valence electrons ÷ 2

So the total electron pairs = 8 ÷ 2 = 4

• Third, determine the central atom

Here hydrogen can not be the central atom. Because the central atom is bonded with at least two other atoms, and hydrogen has only one electron in its last shell, so it can not make more than one bond.

Hence, here we have to assume that the central atom is selenium.

Therefore, place selenium in the center and hydrogens on either side.

• And finally, draw the rough sketch

#2 Mention lone pairs on the atoms

Here, we have a total of 4 electron pairs. And two Se — H bonds are already marked. So we have to only mark the remaining two electron pairs as lone pairs on the sketch.

Also remember that hydrogen is a period 1 element, so it can not keep more than 2 electrons in its last shell. And selenium is a period 4 element, so it can keep more than 8 electrons in its last shell.

Always start to mark the lone pairs from outside atoms. Here, the outside atoms are hydrogens. But no need to mark on hydrogen, because each hydrogen has already two electrons.

So for selenium, there are two lone pairs.

Mark the lone pairs on the sketch as follows:

#3 If needed, mention formal charges on the atoms

Use the following formula to calculate the formal charges on atoms:

Formal charge = valence electrons – nonbonding electrons – ½ bonding electrons

For each hydrogen atom, formal charge = 1 – 0 – ½ (2) = 0

For selenium atom, formal charge = 6 – 4 – ½ (4) = 0

Here, both hydrogen and selenium atoms do not have charges, so no need to mark the charges.

In the above structure, you can see that the central atom (selenium) forms an octet. And the outside atoms (hydrogens) also form a duet. Hence, the octet rule and duet rule are satisfied.

Therefore, this structure is the stable Lewis structure of H₂Se.

Next: H₃O⁺ Lewis structure

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External links

• https://techiescientist.com/h2se-lewis-structure/
• https://topblogtenz.com/h2se-lewis-structure-molecular-geometry-polar-or-nonpolar-bond-angle/
• https://www.thegeoexchange.org/chemistry/bonding/Lewis-Structures/H2Se-lewis-structure.html
• https://sciedutut.com/h2se-lewis-structure/