Free Printable U2E2 OnRamps Chemistry

Free Printable Worksheets

Worksheets

U2E2 OnRamps Chemistry

Total questions: 99

Worksheet time: 2hrs 51mins

Name

Class

Date

1.

Carbon dioxide

a)

C₂O₂

b)

C₂0

c)

CO

d)

CO₂

2.

Phosphorous trichloride

a)

PCl₃

b)

P₃Cl

c)

P₃Cl₃

d)

PCL

3.

Disulfur trioxide

a)

S₃O₂

b)

SO

c)

S₂O₃

d)

S₂O

4.

P₃F₄

a)

Phosphorous fluoride

b)

Triphosphorous tetrafluoride

c)

Phosphate Fluoride

d)

Trifluoride hexafluoride

5.

Give the name of this compound...

C₃H₈

a)

ethane

b)

octane

c)

Butene

d)

Propane

6.

Name this compound.

a)

hexane

b)

pentane

c)

butane

d)

heptane

7.

Name this alkyne.

a)

propyne

b)

butyne

c)

It has no name.

d)

ethyne

8.

How many carbon atoms are in butane?

a)

1

b)

2

c)

3

d)

4

9.

How many carbon atoms are in propane?

a)

1

b)

2

c)

3

d)

4

10.

How many carbon atoms are in ethane?

a)

1

b)

2

c)

3

d)

4

11.

How many carbon atoms are in methane?

a)

1

b)

2

c)

3

d)

4

12.

Electrons occupy orbitals of lowest energy first is part of what electron configuration rule?

a)

Hund’s Rule

b)

Aufbau Principle

c)

Pauli Exclusion Principle

13.

Electrons are paired based on their spin directions, clockwise and counterclockwise, is what electron configuration rule?

a)

Hund’s Rule

b)

Aufbau Principle

c)

Pauli Exclusion Principle

14.

Which guideline, Hund’s rule or the Pauli exclusion principle, is violated in the following orbital diagrams?

a)

Aufbau's

b)

Hund's

c)

Pauli exclusive

15.

Which guideline, Hund’s rule or the Pauli exclusion principle, is violated in the following orbital diagrams?

a)

Hund's

b)

Aufbau's

c)

Pauli's Exclusive

16.

All orbitals of equal energy are occupied by one electron before any single orbital is occupied by a second electron.

a)

Aufbau principle

b)

Pauli exclusion principle

c)

Hund’s rule

d)

Core Notation

17.

Which orbital shows a violation of Hund's Rule?

a)

A

b)

B

c)

C

d)

D

18.

Which orbital shows a violation of the Pauli's Rule

a)

A

b)

B

c)

C

d)

D

19.

Which orbital shows a violation of the Pauli Exclusion Principle?

a)

A

b)

B

c)

C

d)

D

20.

The correct electron configuration for Chlorine is

a)

1s²2s²2p⁵

b)

1s²2s²2p⁶3s²

c)

1s²2s²2p⁶3s²3p⁴

d)

1s²2s²2p⁶3s²3p⁵

21.

What is the correct diagram for Nitrogen (N)?

a)

b)

c)

d)

22.

What atom matches this electron configuration?
1s²2s²2p⁶3s²

a)

Neon

b)

Magnesium

c)

Aluminum

d)

Potassium

23.

Which is the electron configuration for an oxygen atom?

a)

1s²2s²2p⁶3s²3p⁶4s²

b)

1s²2s²2p⁴

c)

1s²2s²2p⁶

d)

1s²2s²2p⁶3s²3p⁶

24.

Which of the following is the correct Lewis structure for water?

a)

A

b)

B

c)

C

25.

Bond angle for trigonal planar

a)

120^o

b)

109.5^o

c)

104.5^o

d)

107^o

26.

Bond angle for tetrahedral

a)

120^o

b)

109.5^o

c)

104.5^o

d)

107^o

27.

Bond angle for bent

a)

120^o

b)

109.5^o

c)

104.5^o

d)

107^o

28.

Bond angle for trigonal pyramidal

a)

120^o

b)

109.5^o

c)

104.5^o

d)

107^o

29.

Bond angle for linear

a)

120^o

b)

109.5^o

c)

180^o

d)

107^o

30.

This molecule is...

a)

polar

b)

nonpolar

31.

This molecule is...

a)

trigonal planar

b)

trigonal pyramidal

c)

bent

d)

tetrahedral

32.

The molecular geometry for this molecule is...

a)

trigonal planar

b)

trigonal pyramidal

c)

bent

d)

tetrahedral

33.

When you have Be-F, what is the polarity?

a)

nonpolar

b)

polar

c)

ionic

34.

When you have Li-O, what is the polarity?

a)

nonpolar

b)

polar

c)

ionic

35.

When you have F-F, what is the polarity?

a)

nonpolar

b)

polar

c)

ionic

36.

When you have C-H, what is the polarity?

a)

nonpolar

b)

polar

c)

ionic

37.

Is this molecule polar or non-polar?

a)

Polar

b)

Non-polar

38.

Is this molecule polar or non-polar?

a)

Polar

b)

Non-polar

39.

Is this molecule polar or non-polar?

a)

Non-polar

b)

Polar

40.

Is this molecule polar or non-polar?

a)

Non-polar

b)

Polar

41.

Is this molecule polar or non-polar?

a)

Polar

b)

Non-polar

42.

Define the term resonance structure

a)

Delocalization of electrons in an atom

b)

Delocalization of π electrons within a molecule

c)

Spread of π electrons in an atom

d)

Spread of π electrons within a molecule

43.

For carbonate ions, how many resonance structures can be drawn ?

a)

2

b)

3

c)

4

d)

5

44.

How many resonance structures for NO₃^- ion?

a)

1

b)

2

c)

3

d)

4

45.

How many resonance structure for SO₂ ?

a)

1

b)

2

c)

3

d)

4

46.

How many resonance structures for CH₃COO^- ion?

a)

1

b)

2

c)

3

d)

4

47.

How many resonance structure can you draw for benzene?

a)

1

b)

2

c)

3

d)

4

48.

This Lewis structure is...

a)

Impossible

b)

A resonance structure

c)

Hypervalent

d)

Ionized

49.

What is the correct Lewis Dot Structure for ammonia NH3

a)

b)

c)

d)

50.

Which is the correct lewis structure for carbon dioxide?

a)

b)

c)

d)

51.

Sulfur hexafluoride is an example of a molecule where the central atom violates the octet rule. This is also known as being_____________.

a)

hypervalent

b)

hypovalent

c)

hyperoctet

d)

hypoctet

52.

In the resonance form of ozone shown, the formal charge of the oxygen atom on the left is _______.

a)

0

b)

+1

c)

-1

d)

+2

e)

-2

53.

In the resonance form of ozone shown, the formal charge on the central oxygen atom is _______.

a)

0

b)

+1

c)

-1

d)

+2

e)

-2

54.

What is the formal charge of each fluorine atom in this structure?

a)

0

b)

-1

c)

+1

d)

-7

55.

Boron trifluoride violates the octet rule because it only has 6 electrons around boron atom. This is because boron is known as ....

a)

Hypovalent

b)

Hypervalent

c)

Isovalent

d)

Ionic

56.

In the resonance form of ozone shown, the formal charge of the oxygen atom on the right is _______.

a)

0

b)

+1

c)

-1

d)

+2

e)

-2

57.

What is the correct structure for BF₃?

a)

Option A.

b)

Option B.

c)

Option C.

d)

Option D.

58.

A lone pair is defined as

a)

A pair of bonding electrons

b)

One non-bonding electron

c)

A pair of non-bonding electrons

d)

A pair of electrons on the central atom

59.

Which of the following molecular geometries has an unshared pairs of electrons on the central atom?

a)

Trigonal Bipyramidal

b)

Bent

c)

Trigonal Planar

d)

Tetrahedral

60.

What molecule could this be?

a)

H₂O

b)

CCl₄

c)

PCl₅

d)

NaCl

61.

Who could this be?

a)

CO₂

b)

NH₃

c)

H₂S

d)

CH₄

62.

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

a)

1

b)

2

c)

3

d)

0

63.

Determine the electron geometry (eg) and molecular geometry (mg) of XeF4 (Lewis structure is shown) .

a)

eg = tetrahedral, mg = tetrahedral

b)

eg = linear, mg = linear

c)

eg = octahedral, mg = square planar

d)

eg = trigonal bipyramidal, mg = tetrahedral

64.

Consider the molecule below. Determine the molecular geometry at each of the 2 labeled carbons.

a)

C1 = tetrahedral, C2 = linear

b)

C1 = trigonal planar, C2 = bent

c)

C1 = bent, C2 = trigonal planar

d)

C1 = trigonal planar, C2 = tetrahedral

65.

What is the shape of H₂O?

a)

linear

b)

tetrahedral

c)

bent

d)

trigonal pyramidal

66.

Which statement is TRUE, based on the diagram provided?

a)

atomic orbital overlap to produce sigma bond

b)

s orbital overlap to produce π bond

c)

s orbital overlap with s orbital to produce sigma bond

d)

p orbital overlap to produce π bond

67.

Diagram below shows

a)

formation of hybrid orbital

b)

atomic orbital overlap to produce hybrid orbital

c)

atomic orbital overlap to form sp hybrid orbital

d)

s orbital overlap with p orbital to form sp hybrid orbital

68.

Which of the statement is TRUE?

a)

s orbital overlap with p orbitals to form sp hybrid orbital

b)

s orbital with two p orbitals to form one sp² hybrid orbital

c)

s orbital with two p orbitals to form two sp² hybrid orbital

d)

s orbital with two p orbitals to form three sp² hybrid orbital

69.

Which molecule will undergo sp³ hybridization?

a)

CO₂

b)

NH₃

c)

SO₃

d)

NO₂

70.

Carbon atom undergo

a)

sp hybridization

b)

sp² hybridization

c)

sp³ hybridization

d)

dsp³ hybridization

71.

Sulfur atom undergo

a)

sp hybridization

b)

sp² hybridization

c)

sp³ hybridization

d)

dsp³ hybridization

72.

Nitrogen atom undergo

a)

sp hybridization

b)

sp² hybridization

c)

sp³ hybridization

d)

dsp³ hybridization

73.

Carbon atom undergo

a)

sp hybridization

b)

sp² hybridization

c)

sp³ hybridization

d)

dsp³ hybridization

74.

What is the geometry of sp³ hybrid orbital?

a)

trigonal planar

b)

tetrahedral

c)

trigonal bipyramidal

75.

Which of the following is POSSIBLE for the geometry of sp³d hybrid orbital? (CHOOSE 3)

a)

see-saw

b)

square planar

c)

T-shape

d)

linear

76.

How many sigma bonds does this have?

a)

1

b)

2

c)

3

d)

4

77.

How many pi bonds does this have?

a)

1

b)

2

c)

3

d)

4

78.

How many sigma bonds does this have?

a)

1

b)

2

c)

3

d)

4

79.

Pi bonds are formed by

a)

side to side overlap of s orbitals

b)

end to end overlap of s orbitals

c)

side to side overlap of p orbitals

d)

end to end overlap of p orbitals

80.

How many sigma and pi bonds does this have?

a)

1 sigma and 1 pi

b)

2 sigma and 1 pi

c)

1 sigma and 2 pi

d)

2 sigma and 2 pi

81.

How many sigma and pi bonds does this have?

a)

3 sigma and 2 pi

b)

5 sigma and 5 pi

c)

5 sigma and 0 pi

d)

0 sigma and 5 pi

82.

How many pi bonds are there in a double bond?

a)

0

b)

1

c)

2

d)

3

83.

How many pi bonds are there in a single bond?

a)

0

b)

1

c)

2

d)

3

84.

How many pi bonds are there in a single bond?

a)

0

b)

1

c)

2

d)

3

85.

How many sigma bonds are there in a triple bond?

a)

0

b)

1

c)

2

d)

3

86.

How many sigma bonds are in the following molecule?

a)

0

b)

1

c)

2

d)

5

e)

6

87.

How many sigma bonds are in the following molecule?

a)

0

b)

4

c)

8

d)

12

e)

16

88.

What can be said about this molecule?

a)

Non-polar molecule with polar bonds

b)

Polar molecule with polar bonds

c)

ionic molecule with polar bonds

d)

Non polar molecule with non-polar bonds

89.

Which bonds are arranged in order of increasing polarity?

a)

H–F < H–Cl < H–Br < H–I

b)

H–I < H–Br < H–F < H–Cl

c)

H–I < H–Br < H–Cl < H–F

d)

H–Br < H–I < H–Cl < H–F

90.

How many sigma and pi bonds are present in a molecule of propyne, CH₃CCH?

a)

sigma: 5

pi: 3

b)

sigma: 6

pi: 2

c)

sigma: 7

pi: 1

d)

sigma: 8

pi: 0

91.

What type of bond has a ΔE between 0.4 and 1.5 ?

a)

non-polar

b)

polar

c)

ionic

d)

I don't know

e)

teacher-student bond

92.

What type of hybridization is present in the C atoms of a molecule of propyne, CH₃CCH? Starting from left to the right, you have C1, C2 and C3.

a)

C1 = sp², C2 = sp², C3=sp³

b)

C1 = sp, C2 = sp, C3=sp³

c)

C1 = sp³, C2 = sp³, C3=sp²

d)

C1 = sp, C2 = sp, C3=sp²

e)

C1 = sp², C2 = sp², C3=sp²

93.

Which of the following geometries could be nonpolar?

a)

bent

b)

tetrahedral

c)

trigonal pyrimidal

d)

none of the above

94.

The hybridization of the central atom in XeF₅⁺ is:

a)

sp

b)

sp²

c)

sp³

d)

dsp³

e)

d²sp³

95.

how many unbonded electron pairs are in an O₂ molecule?

a)

1

b)

3

c)

4

d)

0

96.

s-s overlap is a _______

a)

σBond

b)

πBond

97.

The hybridization of the central atom in XeF₅⁺ is:

a)

sp

b)

sp²

c)

sp³

d)

dsp³

e)

d²sp³

98.

The hybridization of the central atom in ClF₂⁺ is:

a)

sp

b)

sp²

c)

sp³

d)

dsp³

e)

d²sp³

99.

The hybridization of the central atom in O₃ is:

a)

sp

b)

sp²

c)

sp³

d)

dsp³

e)

d²sp³

100 %

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