Lewis Structure and Valence Electrons

This video tutorial explains how to write the Lewis structure for the hydrosulfide ion (HS-). It begins by counting the valence electrons of hydrogen and sulfur, considering the additional electron due to the negative charge. The tutorial then demonstrates how to draw the Lewis structure by placing electrons between hydrogen and sulfur to form a bond, ensuring hydrogen's outer shell is full. The remaining electrons are placed around sulfur to complete its octet. The video concludes by showing the final Lewis structure with brackets and a negative sign to indicate the ion's charge.

What is the main focus of this video tutorial?

• Understanding molecular geometry

• Discussing chemical reactions

• Explaining the periodic table

• Drawing the Lewis structure for HS- ion

How many valence electrons does sulfur have?

• 1

• 6

• 8

• 16

What does the negative charge on the HS- ion indicate?

• Gain of an electron

• Loss of a proton

• Loss of an electron

• Gain of a proton

How many electrons are shared between hydrogen and sulfur in the HS- ion?

• Four

• Three

• Two

• One

Why does hydrogen only need two electrons in its outer shell?

• It has a full d-orbital

• It is highly electronegative

• It follows the duet rule

• It is a noble gas

What is the total number of valence electrons used in the HS- ion structure?

• 6

• 7

• 8

• 9

Why are brackets used around the Lewis structure of HS-?

• To show it is an ion

• To indicate it is a molecule

• To highlight the central atom

• To denote resonance