Molecular Geometry and Valence Electrons

This video tutorial explains how to write the Lewis structure for SnF3-. It begins by counting the valence electrons of tin and fluorine, considering the extra electron due to the negative charge. The tutorial then guides viewers through constructing the Lewis structure, ensuring all atoms achieve an octet. Finally, it discusses the molecular geometry of SnF3-, identifying it as trigonal pyramidal using the AXE notation and explaining the bond angles involved.

How many valence electrons does tin contribute in the SnF3- ion?

• 2

• 4

• 8

• 6

What is the total number of valence electrons in SnF3-?

• 27

• 25

• 26

• 24

Which atom is placed at the center of the Lewis structure for SnF3-?

• Nitrogen

• Fluorine

• Oxygen

• Tin

How many electrons are used to form bonds between tin and fluorine atoms initially?

• 6

• 4

• 10

• 8

After forming initial bonds, how many electrons are left to complete the octets?

• 18

• 20

• 22

• 24

Why are brackets used in the Lewis structure of SnF3-?

• To highlight the central atom

• To denote an ion

• To show the structure is incomplete

• To indicate a molecule

What is the steric number for the central tin atom in SnF3-?

• 3

• 6

• 5

• 4

What is the molecular geometry of SnF3- according to the AXE notation?

• Trigonal pyramidal

• Linear

• Tetrahedral

• Trigonal planar

What is the bond angle approximately in the SnF3- ion?

• 109.5 degrees

• 120 degrees

• 180 degrees

• 90 degrees

In AXE notation, what does 'E' represent in the context of SnF3-?

• Central atom

• Bonded atoms

• Lone pairs

• Electrons in bonds