Free Printable Practice Problems Unit 4 Lesson 2

Free Printable Worksheets

Worksheets

Practice Problems Unit 4 Lesson 2

Total questions: 35

Worksheet time: 2hrs 15mins

Name

Class

Date

1.

Draw the Lewis Dot structure for SF₄ and determine how many lone pair electrons it has?

a)

0

b)

1

c)

2

d)

3

2.

Using the Lewis Structure you drew for SF₄, which best describes it's polarity?

a)

polar bonds but a nonpolar molecule

b)

Polar bonds and a polar molecule

c)

nonpolar bonds but a polar molecule

d)

nonpolar bonds and a nonpolar molecule

3.

Using the Lewis Structure you drew for ICl₂^-, which best describes it's polarity?

a)

polar bonds but a nonpolar molecule

b)

Polar bonds and a polar molecule

c)

nonpolar bonds but a polar molecule

d)

nonpolar bonds and a nonpolar molecule

4.

Using the Lewis Structure you drew for BrF₃^, which best describes it's polarity?

a)

polar bonds but a nonpolar molecule

b)

Polar bonds and a polar molecule

c)

nonpolar bonds but a polar molecule

d)

nonpolar bonds and a nonpolar molecule

5.

Using the Lewis Structure you drew for PCl₅^, which best describes it's polarity?

a)

polar bonds but a nonpolar molecule

b)

Polar bonds and a polar molecule

c)

nonpolar bonds but a polar molecule

d)

nonpolar bonds and a nonpolar molecule

6.

Using the Lewis Structure you drew for BrF₅^, which best describes it's polarity?

a)

polar bonds but a nonpolar molecule

b)

Polar bonds and a polar molecule

c)

nonpolar bonds but a polar molecule

d)

nonpolar bonds and a nonpolar molecule

7.

Draw the Lewis Dot structure for SF₄ and determine how many bonding pair electrons it has?

a)

2

b)

3

c)

4

d)

5

8.

Draw the Lewis Dot structure for SF₄ and determine its predicted molecular geometry.

a)

square planar

b)

trigonal bipyramidal

c)

see-saw

d)

tetrahedral

9.

Draw the Lewis Dot structure for ICl₂^- and determine its number of bonding pair electrons.

a)

3

b)

1

c)

2

d)

4

10.

Draw the Lewis Dot structure for ICl₂^- and determine its number of lone pair electrons.

a)

3

b)

1

c)

2

d)

4

11.

Draw the Lewis Dot structure for ICl₂^- and determine its predicted molecular geometry.

a)

see-saw

b)

trigonal bipyramidal

c)

linear

d)

bent

12.

Draw the Lewis Dot structure for BrF₃ and determine its number of lone pair electrons.

a)

3

b)

1

c)

2

d)

4

13.

Draw the Lewis Dot structure for BrF₃ and determine its number of bonding pair electrons.

a)

3

b)

1

c)

2

d)

4

14.

Draw the Lewis Dot structure for BrF₃ and determine its predicted molecular geometry

a)

t-shaped

b)

trigonal bipyramidal

c)

tetrahedral

d)

square planar

15.

Draw the Lewis Dot structure for PCl₅ and determine how many lone pair electrons it has?

a)

0

b)

1

c)

2

d)

3

16.

Draw the Lewis Dot structure for PCl₅ and determine how many bonding pair electrons it has?

a)

6

b)

3

c)

4

d)

5

17.

Draw the Lewis Dot structure for PCl₅ and determine the predicted molecular geometry

a)

octahedral

b)

trigonal pyramidal

c)

seesaw

d)

trigonal bipyramidal

18.

Draw the Lewis Dot structure for BrF₅ and determine how many lone pair electrons it has?

a)

0

b)

1

c)

2

d)

3

19.

Draw the Lewis Dot structure for BrF₅ and determine how many bonding pair electrons it has?

a)

0

b)

4

c)

6

d)

5

20.

Draw the Lewis Dot structure for BrF₅ and determine the predicted molecular geometry

a)

octahedral

b)

trigonal pyramidal

c)

square pyramidal

d)

trigonal bipyramidal

21.

What is the electron geometry for Xenon tetrafluoride?

a)

square pyramidal

b)

t-shaped

c)

octahedral

d)

square planar

22.

What is the Molecular Geometry of the molecule?

a)

Linear

b)

Trigonal Pyramidal

c)

Bent

d)

Trigonal Planar

23.

What is the Molecular Geometry of the molecule?

a)

Linear

b)

Bent, 120^o

c)

Bent, 109.5^o

d)

Trigonal Planar

24.

What is the molecular shape of a molecule with 3 bonded atoms and 2 lone pairs?

a)

T-Shape

b)

Trigonal Bipyramid

c)

See-Saw

d)

Square Planar

25.

What is the molecular shape of a molecule with 5 bonded atoms and 1 lone pair?

a)

Octahedral

b)

Pentagon

c)

Square Pyramidal

d)

Square Planar

26.

What is the formal charge on the phosphorus atom in this Lewis dot structure?

a)

0

b)

-1

c)

+1

d)

-3

27.

What is the picture showing?

a)

All of the resonance structures for carbonate.

b)

The formal charge on each atom in carbonate.

c)

The electronegativity for carbonate.

d)

The ionization energy for carbonate.

28.

What is the formal charge on the bromine atom in this Lewis dot structure?

a)

-1

b)

+1

c)

-2

d)

+2

29.

Draw the Lewis Dot structure for BrF₃ and determine its predicted electron geometry

a)

t-shaped

b)

trigonal bipyramidal

c)

tetrahedral

d)

square planar

30.

Draw the Lewis Dot structure for SF₄ and determine its predicted electron geometry.

a)

square planar

b)

trigonal bipyramidal

c)

see-saw

d)

tetrahedral

31.

What is the Electron Geometry of the molecule?

a)

Linear

b)

Tetrahedral

c)

Bent

d)

Trigonal Planar

32.

Which shape will always result in a polar molecule?

a)

bent

b)

trigonal planar

c)

linear

d)

tetrahedral

33.

Select all of the polar molecules in this picture.

a)

SeH₂

b)

SiF₄

c)

NO₃⁻¹

d)

CS₂

e)

None of these are polar?

34.

In the picture which element would be the negative dipole moment of the molecule?

a)

H1

b)

H2

c)

O

d)

C

e)

There isn't one the molecule is nonpolar

35.

Which of the statements is true based on the VSEPR model provided?

a)

The Carbon atom would experience the dipole moment in the center of the molecule.

b)

The Chlorine atoms would experience the negative dipole moment on every end.

c)

All atoms would experience a negative dipole moment equally.

d)

There would not be a negative dipole moment and the molecule is nonpolar

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