Lewis structure of H2Se

The information on this page is ✔ fact-checked.

Lewis structure of H2Se
Lewis structure of H2Se | Image: Root Memory

The Lewis structure of H2Se contains two single bonds, with selenium in the center, and two hydrogens on either side. There are two lone pairs on the selenium atom, and the hydrogen atom does not have any lone pair.

Steps

By using the following steps, you can easily draw the Lewis structure of H2Se.

#1 Draw skeleton
#2 Show chemical bond
#3 Mark lone pairs
#4 Calculate formal charge and check stability (if octet is already completed on central atom)

Let’s one by one discuss each step in detail.

#1 Draw skeleton

In this step, first calculate the total number of valence electrons. And then, decide the central atom.

  • Let’s calculate the total number of valence electrons

We know that… hydrogen is a group 1 element and selenium is a group 16 element. Hence, hydrogen has one valence electron and selenium has six valence electrons.

Now H2Se has two hydrogen atoms and one selenium atom.

So the total number of valence electrons = (valence electrons of hydrogen atom × 2) + valence electrons of selenium atom

Therefore, the total number of valence electrons = 2 + 6 = 8

  • Now decide the central atom

We can not assume hydrogen as 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, assume that selenium is the central atom.

So now, put selenium in the center and hydrogens on either side. And draw the rough skeleton structure for the Lewis structure of H2Se something like this:

Skeleton structure for Lewis structure of H2Se | Image: Root Memory

#2 Show chemical bond

Place two electrons between the atoms to show a chemical bond. Since selenium is surrounded by two hydrogens, use four electrons to show two chemical bonds as follows:

Two chemical bonds shown between atoms | Image: Root Memory

#3 Mark lone pairs

As calculated earlier, we have a total of 8 valence electrons. And in the above structure, we have already used four valence electrons. Hence, four valence electrons are remaining.

Two valence electrons represent one lone pair. So four valence electrons = two lone pairs.

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

Also, make sure that you start marking these lone pairs on outside atoms first. And then, on the central atom.

The outside atoms are hydrogens. But hydrogen can not keep more than 2 electrons in its last shell. Hence, don’t mark the lone pairs on hydrogen.

So the central atom (selenium) will get two lone pairs.

Now draw the Lewis structure of H2Se something like this:

Lone pairs marked on Lewis structure of H2Se | Image: Root Memory

In the above structure, you can see that the octet is completed on the central atom (selenium), and also on the outside atoms. Therefore, the octet rule is satisfied.

After completing the octet, one last thing we need to do is, calculate the formal charge and check the stability of the above structure.

#4 Calculate formal charge and check stability

The following formula is used to calculate the formal charges on atoms:

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

Collect the data from the above structure and then, write it down below as follows:

  • For each hydrogen atom

Valence electrons = 1
Nonbonding electrons = 0
Bonding electrons = 2

Formal charge = 1 – 0 – ½ (2) = 0

  • For selenium atom

Valence electrons = 6
Nonbonding electrons = 4
Bonding electrons = 4

Formal charge = 6 – 4 – ½ (4) = 0

Mention the formal charges of atoms on the structure. So the Lewis structure of H2Se looks something like this:

Formal charges are calculated, and got the stable Lewis structure of H2Se | Image: Root Memory

In the above structure, you can see that the formal charges of both (hydrogen and selenium) are zero. Therefore, this is the stable Lewis structure of H2Se.

And each horizontal line drawn in the above structure represents a pair of bonding valence electrons.

Related

External links

Deep

Rootmemory.com was founded by Deep Rana, who is a mechanical engineer by profession and a blogger by passion. He has a good conceptual knowledge on different educational topics and he provides the same on this website. He loves to learn something new everyday and believes that the best utilization of free time is developing a new skill.

Leave a Comment