Lewis Structures and Valence Electrons

The video tutorial explains how to draw the Lewis structure for tin(II) fluoride (SNF2) in its gaseous form. It begins by counting the valence electrons of tin and fluorine, totaling 18 electrons. The tutorial then guides viewers through placing tin in the center and arranging fluorine atoms on either side, forming chemical bonds and completing the octets for fluorine. Tin is noted as an exception to the octet rule. The video concludes with a discussion on the molecular geometry of SNF2, identifying it as bent due to the presence of a lone pair on tin, with an approximate bond angle of 120 degrees.

What is the first step in writing the Lewis structure for SnF2?

• Determine the hybridization

• Draw the skeletal structure

• Identify the molecular geometry

• Count the valence electrons

How many valence electrons does tin contribute in SnF2?

• 2

• 8

• 4

• 6

What is the total number of valence electrons in SnF2?

• 22

• 20

• 18

• 16

In the Lewis structure of SnF2, where is the tin atom placed?

• At the top

• In the center

• On the left

• On the right

How many valence electrons are used to form bonds between tin and fluorine in SnF2?

• 4

• 6

• 8

• 10

Why does tin in SnF2 not need to follow the octet rule?

• It is a noble gas

• It is an exception to the octet rule

• It forms ionic bonds

• It has a full d-orbital

What is the molecular geometry of SnF2 in the gaseous phase?

• Bent

• Tetrahedral

• Trigonal planar

• Linear

How many steric groups are attached to the tin atom in SnF2?

• 2

• 3

• 4

• 5

What is the approximate bond angle in the bent geometry of SnF2?

• 150 degrees

• 120 degrees

• 180 degrees

• 90 degrees

What effect does the lone pair on tin have on the molecular geometry of SnF2?

• It makes the molecule linear

• It causes a bent shape

• It increases the bond angle

• It has no effect