VSEPR Theory Practice

Which of the following molecular shapes would have a bond angle of 180 Degrees?

• Bent

• Trigonal Planar

• Tetrahedral

• Linear

Lone pairs of electron ​ (a)   other electron pairs ​​ (b)   strongly than bonded pairs. This ​ (c)   the bond angle.​

• repel

• more

• reduces

• attract

• less

• increases

How many lone pairs of electrons are on the P atom in PF3?

• 1

• 2

• 3

• 0

How many unshared pairs of electrons will a bent molecule have? 

• 1

• 2

• 3

• 4

What shape would PH₃ have?

• Trigonal Planar

• Trigonal Bipyramidal

• Bent

• Linear

Why is the bond angle in NH₃ molecule is smaller than that in CH₄ molecule?

• Among the four electron pairs around the central atom N in NH₃

  molecule, there are two lone pairs which require more space than bonding pairs and tend to compress the angles between the bonding pairs.

• Among the four electron pairs around the central atom N in NH₃

  molecule, there is one lone pair which requires more space than a bonding pair and tends to compress the angles between the bonding pairs.

• Among the four electron pairs around the central atom N in NH₃

  molecule, there is one lone pair which requires less space than bonding pairs and tend to increase the angles between the bonding pairs.

• In reality, bond angle in NH₃ molecule is larger than that in CH₄ molecule.

How many lone pairs are on S in SH₂? What shape is the molecule?

• none/linear

• one/trigonal planar

• two/bent

• two/tetrahedral

How many lone pairs are in this molecule's structure? (Hint: the green atoms are fluorine.)

• 6

• 2

• 0

• 4

What is the molecular shape of a silicon dioxide (SiO2) molecule?

• linear

• trigonal planar

• bent

• tetrahedral

Who could this be? 

• CO₂

• NH₃

• H₂S

• CH₄

Tags

NGSS.MS-PS1-1