In this worksheet, we will practice classifying the bond and electron pair arrangements and identifying the ideal angles of common molecular geometries.

**Q1: **

Nitrogen and phosphorus atoms can both form bonds with three fluorine atoms. However, only phosphorus atoms can form bonds with five fluorine atoms.

Which term best describes the bonding geometry in and ?

- ABent
- BTetrahedral
- CTrigonal bipyramidal
- DTrigonal pyramidal
- ET-shaped

Which term best describes the bonding geometry in ?

- ATrigonal bipyramidal
- BOctahedral
- CPentagonal planar
- DSquare pyramidal
- ETetrahedral

Why is it not possible for to form?

- AThe lone pair in is more stable than two additional bonds.
- BThere is insufficient space around the atom for five bonds to form.
- COnly the atom possesses valence d orbitals.
- DOnly the atom contains d electrons in its valence shell.
- EThe high electronegativity of the atom prevents sharing of electron density in five bonds.

**Q2: **

The bonding geometry is the same in all but one of the following molecules. In which molecule is the geometry different?

- A
- B
- C
- D
- E

**Q3: **

The bonding geometry is the same in all but one of the following molecules and ions. In which species is the geometry different?

- A
- B
- C
- D
- E

**Q4: **

What is the geometry of the complex, and how many unpaired electrons does it contain?

- ATetrahedral, two unpaired electrons
- BSquare planar, two unpaired electrons
- COctahedral, two unpaired electrons
- DSquare planar, no unpaired electrons
- ETetrahedral, no unpaired electrons

**Q5: **

Which of the following has T-shaped molecular geometry?

- A
- B
- C
- D
- E

**Q6: **

What is the molecular geometry of ?

- AOctahedral
- BSquare planar
- CTetrahedral
- DTrigonal planar
- ETrigonal pyramidal

**Q7: **

Consider the Lewis structure of water shown.

What is the electron pair geometry?

- ATrigonal pyramidal
- BTrigonal planar
- CSquare planar
- DTetrahedral
- EBent

What is the molecular geometry?

- ABent
- BTrigonal pyramidal
- CLinear
- DTetrahedral
- ESquare planar

**Q8: **

Sulfur tetrafluoride, , is extremely valuable for the preparation of fluorine-containing compounds used as herbicides (i.e., is used as a fluorinating agent).

What is its electron pair geometry?

- ASquare pyramidal
- BTetrahedral
- CSquare planar
- DTrigonal bipyramidal
- EOctahedral

What is its molecular geometry?

- ASeesaw
- BTrigonal bipyramidal
- CSquare planar
- DTetrahedral
- EOctahedral

**Q9: **

What is the electron pair geometry of each of the following molecules or ions?

- ASquare pyramidal
- BHexagonal planar
- CSquare bipyramidal
- DOctahedral
- EIcosahedral

- ATrigonal bipyramidal
- BOctahedral
- CPentagonal planar
- DSquare pyramidal
- ETetrahedral

- ATetrahedral
- BBent
- CLinear
- D
- ETrigonal

- ATrigonal planar
- BTetrahedral
- CTrigonal pyramidal
- DBent
- ET-shaped

**Q10: **

What is the difference between electron pair geometry and molecular geometry?

- AElectron pair geometry accounts for outer-shell electrons as well as atoms, while molecular geometry is concerned with inner-shell electrons.
- BMolecular geometry accounts for lone pairs as well as atoms, while electron pair geometry is concerned only with the atoms.
- CMolecular geometry is concerned with the rough shape of the entire molecule, while electron pair geometry is concerned with the geometry around a single atom.
- DElectron pair geometry accounts for lone pairs as well as atoms, while molecular geometry is concerned only with the atoms.
- EElectron pair geometry accounts for inner-shell electrons as well as outer-shell electrons, while molecular geometry is concerned only with the atoms.