Lewis Structures and Valence Electrons

This video tutorial explains how to write the Lewis structure for the SF3+ ion. It begins by counting the valence electrons of sulfur and fluorine, considering the positive charge of the ion. The tutorial then guides the viewer through placing sulfur at the center and arranging fluorine atoms around it. It details forming chemical bonds and ensuring each fluorine atom has a complete octet. Finally, it discusses placing the remaining electrons on sulfur and finalizing the structure with brackets and a positive sign.

What is the first step in writing the Lewis structure for SF3+?

• Determine the molecular geometry.

• Identify the hybridization.

• Count the valence electrons.

• Calculate the formal charge.

How many valence electrons does sulfur contribute in SF3+?

• 8

• 2

• 4

• 6

What is the total number of valence electrons for SF3+?

• 30

• 26

• 28

• 24

Which element is placed at the center of the SF3+ Lewis structure?

• Fluorine

• Nitrogen

• Sulfur

• Oxygen

How many fluorine atoms are bonded to sulfur in SF3+?

• 2

• 3

• 4

• 1

What is the purpose of placing electron pairs between atoms in the Lewis structure?

• To represent hybrid orbitals.

• To show resonance structures.

• To form chemical bonds.

• To indicate lone pairs.

How many valence electrons are used to complete the octets of the fluorine atoms?

• 18

• 22

• 20

• 24

What is done to the sulfur atom after completing the octets of fluorine atoms?

• Remove a bond from sulfur.

• Add two electrons to sulfur.

• Remove two electrons from sulfur.

• Add a double bond to sulfur.

Why are brackets used in the Lewis structure of SF3+?

• To highlight the central atom.

• To denote it is an ion.

• To show the molecular geometry.

• To indicate resonance.

What charge is written outside the brackets in the SF3+ Lewis structure?

• Neutral

• Negative

• Positive

• Double positive