Boron and BBr3 Molecular Geometry

The video tutorial explains the molecular geometry of BBr3 by examining its Lewis structure. Boron in BBr3 has six valence electrons, which is sufficient for its stability. The geometry is described as trigonal planar, with bromine atoms spreading out evenly around the boron. The AXN notation is used to confirm this geometry, with A representing boron, X representing the three bromine atoms, and N representing non-bonding electron pairs, which are absent. The bond angles in this geometry are 120 degrees. The video concludes with a summary of these concepts.

What is the number of valence electrons boron has in the Lewis structure of BBr3?

• Ten

• Four

• Eight

• Six

Why is it acceptable for boron to have only six valence electrons in BBr3?

• Boron is stable with six electrons.

• Boron shares electrons with other atoms.

• Boron can expand its octet.

• Boron forms ionic bonds.

What is the molecular geometry of BBr3?

• Trigonal Planar

• Linear

• Tetrahedral

• Bent

How do the bromine atoms arrange themselves around the boron atom in BBr3?

• In a zigzag pattern

• In a square

• In a triangular shape

• In a straight line

In the AXN notation for BBr3, what does 'X' represent?

• The central atom

• The number of lone pairs

• The number of atoms bonded to the central atom

• The total number of valence electrons

What is the value of 'A' in the AXN notation for BBr3?

• Zero

• Boron

• Bromine

• Three

What is the bond angle in a trigonal planar molecular geometry?

• 120 degrees

• 180 degrees

• 90 degrees

• 109.5 degrees

How many non-bonding electron pairs are around the boron atom in BBr3?

• Zero

• One

• Three

• Two

Which of the following is true about the bond angles in BBr3?

• They vary between 90 and 120 degrees.

• They are all 180 degrees.

• They are all 120 degrees.

• They are all 90 degrees.

What is the significance of the AX3 notation in determining the geometry of BBr3?

• It indicates a linear geometry.

• It confirms a trigonal planar geometry.

• It implies a bent geometry.

• It suggests a tetrahedral geometry.