1. Which of the following statements are true about covalent bonds, according to the Valence Bond...

1. Which of the following statements are true about covalent bonds, according to the Valence Bond Theory? (select all that apply.)

End-to-end orbital overlaps are more stable than edge-to-edge orbital overlaps.
A triple bond contains one sigma bond and two pi bonds.
A triple bond is longer than a double bond.
Valence p orbitals that are not used in hybridization can be used to form pi bonds.
A double bond contains two pi bonds.
A sigma bond is stronger than a pi bond.
Sigma bonds are formed by edge-to-edge orbital overlaps.
A single bond can be either a sigma or a pi bond
2. Which of the following statements are true about molecular polarity? (Select all that apply.)
A polar molecule must have at least one polar bond.
If a molecule is polar then it has a dipole.
It is not possible for a perfectly linear molecule to be polar.
Molecular polarity is the same as bond polarity.
A polar molecule must be asymmetrical.
3. Assuming all bonds in the molecule are polar and identical, which of the following molecular geometries result in a polar molecule?
Linear
Bent
Trigonal Planar
Trigonal Pyramid
Tetrahedral
Trigonal Bipyramid
See-Saw
T-shape
Square Pyramid
Square Planar
Octahedral

Expert Solution

1)Answer:

End-to-end orbital overlaps are more stable than edge-to-edge orbital overlaps.
A triple bond contains one sigma bond and two pi bonds.
Valence p orbitals that are not used in hybridization can be used to form pi bonds.
A sigma bond is stronger than a pi bond.

(2)

A polar molecule must have at least one polar bond.

If a molecule is polar then it has dipole
Molecular polarity is the same as bond polarity.

Note: polar molecule mIght be symmetrical or asymmetrical like in case of HCl

(3)

Bent
Trigonal Pyramid
See-Saw
T-shape
Square Pyramid

queen_honey_blossom answered 2 years ago

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