Understanding Sulfide Ion Properties

The video tutorial explains how to draw the Lewis structure for the sulfide ion (S2-). It begins by illustrating the Lewis structure for neutral sulfur, which has six valence electrons. The tutorial then transitions to the sulfide ion, which has a 2- charge, indicating two additional electrons. This results in a stable octet configuration. The video concludes by showing the correct notation for the sulfide ion's Lewis structure, including the use of brackets.

What is the initial step in drawing the Lewis structure for the sulfide ion?

• Identify the number of protons in sulfur.

• Draw the Lewis structure for sulfur as a neutral element.

• Determine the molecular geometry of sulfur.

• Calculate the atomic mass of sulfur.

In which group is sulfur found on the periodic table?

• Group 14

• Group 15

• Group 16

• Group 17

How many valence electrons does a neutral sulfur atom have?

• Four

• Six

• Eight

• Two

What change occurs when sulfur becomes a sulfide ion?

• It gains two valence electrons.

• It loses two protons.

• It gains two protons.

• It loses two valence electrons.

What is the charge of the sulfide ion?

• Negative one

• Positive one

• Positive two

• Negative two

What is the term used to describe the stable arrangement of eight electrons around sulfur?

• Sextet

• Quartet

• Octet

• Duet

Why are brackets used in the Lewis structure of the sulfide ion?

• To highlight the central atom.

• To indicate the presence of a covalent bond.

• To show the ion's charge and complete structure.

• To separate different molecules.

What is the significance of the two additional electrons in the sulfide ion?

• They complete the octet, stabilizing the ion.

• They increase the ion's atomic number.

• They decrease the ion's atomic mass.

• They make the ion positively charged.