Lewis Structure and Molecular Geometry of OF2

The video tutorial explains the Lewis structure of oxygen difluoride (OF2), focusing on the lone and bonding pairs of electrons. It describes how these pairs influence the molecular geometry, resulting in a bent shape due to the repulsion between lone pairs and bonding pairs. The tutorial concludes with a recap of the key points discussed.

What is the first step in analyzing the Lewis structure of OF2?

• Counting the total number of electrons

• Identifying the central atom

• Starting with a valid Lewis structure

• Determining the molecular geometry

How many bonding pairs of electrons are present in OF2?

• Four

• Three

• Two

• One

What type of bond is formed between oxygen and fluorine in OF2?

• Covalent bond

• Double bond

• Metallic bond

• Ionic bond

How many lone pairs of electrons are found on the oxygen atom in OF2?

• Four

• Three

• Two

• One

What is the effect of lone pairs on the molecular geometry of OF2?

• They have no effect

• They make the molecule linear

• They cause the molecule to be bent

• They make the molecule tetrahedral

What is the molecular geometry of OF2?

• Linear

• Bent

• Trigonal planar

• Tetrahedral

Why do the fluorine atoms in OF2 spread out as far as possible?

• To maximize the molecule's size

• To minimize repulsion between bonding pairs

• To maximize bonding

• To minimize repulsion between lone pairs

How many lone pairs and bonding pairs are there in OF2?

• Three lone pairs and one bonding pair

• One lone pair and three bonding pairs

• Four lone pairs and no bonding pairs

• Two lone pairs and two bonding pairs

What is the significance of lone pairs in determining the shape of OF2?

• They determine the bond length

• They have no significance

• They determine the bond angle

• They influence the molecular geometry