Molecular/Electronic Geometries and Hybridization

Question 1

What is the molecular/electronic geometry for the following molecule: H₂C=O

What are the hybridization states for each atom? (besides H)

Also, note the bond angles around the central atom

Answer 1

The molecular and electronic geometries of this molecule are trigonal planar due to the sp² hybridization of the carbon atom, giving bond angles of 120 degrees.

Question 2

What are the bond angles of around the groups of an sp² carbon?

Answer 2

120 degrees.

Question 3

What is the molecular/electronic geometry for the following molecule: H₃O⁺

What are the hybridization states of the atoms? (Besides H)

Also, notes the bond angles of the central atom

Answer 3

The molecular geometry is trigonal pyramidal. The electronic geometry is tetrahedral. The oxygen is sp³ hybridized giving bond angles of 109.5 degrees

Question 4

What is the molecular/electronic geometry for the following molecule: HCN

What are the hybridization states of the atoms? (Besides H)

Also, notes the bond angles of the central atom

Answer 4

The molecular and eletronic geometry of this molecule is linear. The carbon and nitrogen have an sp hybridization state, giving 180 degree bond angles around the central carbon.

Question 5

What are the bond angles around an sp hybridize atom?

Answer 5

180 degrees

Question 6

What is the molecular/electronic geometry for the following molecule: C(CH₃)₄

What are the hybridization states of the atoms? (Besides H)

Also, note the bond angles of the central atom

Answer 6

The molecular and electronic geometries of this molecular are tetrahedral. This is due to the sp³ hybridization state of the central carbon atom, giving bond angles of 109.5 degrees. All of the carbon atoms in this molecule are sp³ hybridized and give bond angles of ~109.5 degrees.

Question 7

What is the molecular/electronic geometry for the following molecule: CH₃⁺

What are the hybridization states of the atoms? (Besides H)

Also, note the bond angles of the central atom

Answer 7

The molecular and electronic geometries of this molecular are trigonal planar. This is due to the sp² hybridization state (remember that + charges DO NOT count as a group when determining the hybridization state) of the central carbon atom, giving bond angles of 120 degrees.

Question 8

What is the molecular/electronic geometry for the following molecule: CH₃^-

What are the hybridization states of the atoms? (Besides H)

Also, note the bond angles of the central atom

Answer 8

The molecular geometry is trigonal pyramidal and the electronic geometry is tetrahedral. This is due to the sp³ hybridization state of the central carbon (remember that lone pairs count as one group), giving bond angles of 109.5 degress around the central carbon atom.

Question 9

What is the molecular/electronic geometry for the following molecule: NH₄⁺

What are the hybridization states of the atoms? (Besides H)

Also, note the bond angles of the central atom

Answer 9

The molecular and electronic geometries are tetrahedral. This is due to the sp³ hybridization state of the central nitrogen (remember that + charges **DO NOT **count as a group), giving bond angles of 109.5 degress around the central nitrogen atom.

Question 10

What is the molecular/electronic geometry for the following molecule: NH₃

What are the hybridization states of the atoms? (Besides H)

Also, note the bond angles of the central atom

Answer 10

The molecular geometry is trigonal pyramidal and the electronic geometry is tetrahedral. This is due to the sp³ hybridization state of the central nitrogen atom (remember that lone pairs count as a group when determining the hybridization state), giving bond angles of 109.5 degress around the central nitrogen.

Question 11

What is the molecular/electronic geometry for the following molecule: BH₃

What are the hybridization states of the atoms? (Besides H)

Also, note the bond angles of the central atom

Answer 11

The molecular and electronic geometries are trigonal planar. This is due to the sp² hybridization state of the central boron atom (boron is an example of an element that can violate the octet rule), giving bond angles of 120 degress around the central boron.

Question 12

What is the molecular/electronic geometry for the following molecule: .CH₃

What are the hybridization states of the atoms? (Besides H)

Also, note the bond angles of the central atom

Answer 12

The molecular geometry is trigonal planar. This is due to the sp² hybridization state of the central carbon atom (if the radical is on a highly electronegative atom, like O, it will be sp³ instead), giving bond angles of 120 degress around the central carbon.

Question 13

What are the bond angles around an sp³ hybridized carbon?

Answer 13

~109.5 degrees

Question 14

What is the Lewis structure for the following molecule: CO₃^2-

Answer 14

Question 15

What is the Lewis structure for the following molecule: CO₂

Answer 15