Covalent Bonding Part 2
Presentation
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Science
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9th - 12th Grade
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Practice Problem
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Medium
BRIAN TAYAG
Used 1+ times
FREE Resource
57 Slides • 28 Questions
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Open Ended
Why is understanding molecular structure, shape, and polarity important in chemistry?
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Multiple Choice
Which of the following statements about Lewis Structures is correct?
Lewis Structures use elemental symbols and bonds to show the relative position of the atoms.
Lewis Structures use numbers to represent electrons.
Lewis Structures do not show nonbonding electrons.
Lewis Structures only use dashes to represent electrons.
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Multiple Choice
What is the first step in drawing Lewis structures for molecules or ions?
Sum the valence electrons from all atoms
Decide which atom is the central atom
Complete the octet of all atoms
Count the number of electrons surrounding the central atom
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Multiple Choice
According to the rules for drawing Lewis structures, which atom is NEVER the central atom?
Hydrogen
Carbon
Oxygen
Chlorine
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Open Ended
Explain why hydrogen follows the duet rule instead of the octet rule when drawing Lewis structures.
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Multiple Choice
When drawing Lewis structures, what should you do if the central atom does not have an octet after all electrons have been placed?
Form multiple bonds using nonbonding electron pairs
Remove electrons from the central atom
Add more atoms to the molecule
Ignore the octet rule
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Fill in the Blanks
Type answer...
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Open Ended
Based on the example of CH2O, describe the process for determining the central atom and connecting the atoms with single bonds in a Lewis structure.
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Multiple Choice
Which atom in the CH2O molecule is the central atom when drawing its Lewis structure?
Carbon
Oxygen
Hydrogen
Nitrogen
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Multiple Select
Which of the following statements are true about the octet rule as applied in the CH2O Lewis structure process?
Hydrogen can only have two electrons.
The central atom must satisfy the octet rule.
Lone pairs are added to all atoms except the central atom.
Leftover electrons are placed on the central atom.
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Open Ended
Explain why it is sometimes necessary to form double or triple bonds in a Lewis structure, using CH2O as an example.
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Fill in the Blanks
Type answer...
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Multiple Choice
What information does the Lewis structure of a molecule provide that the molecular formula does not?
The number of atoms involved
The types of atoms present
The connectivity and arrangement of atoms
The molecular mass
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Multiple Choice
How many valence electrons are present in a C2H2 molecule?
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Multiple Choice
Which of the following statements best describes resonance structures?
They differ only in the position of the electron pairs and multiple bonds, never the position of the atoms.
They differ in the number of atoms present in the molecule.
They differ in the types of atoms present in the molecule.
They differ in the total number of electrons in the molecule.
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Open Ended
Explain why the carbonate ion (CO3 2-) has more than one resonance structure. What does this indicate about the bonding in the ion?
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Multiple Choice
Which molecule is used as an example of a molecule with less than an octet in the lesson?
BF3
SF6
NO
CO3 2-
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Multiple Select
Which of the following molecules are exceptions to the octet rule?
BF3
NO
SF6
CH4
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Multiple Choice
What is the main limitation of Lewis structures as described in the lesson?
They do not indicate the shapes of molecules.
They cannot show the number of bonds.
They cannot show the types of atoms.
They do not show electron pairs.
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Fill in the Blanks
Type answer...
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Multiple Choice
According to the VSEPR model, what determines the geometric arrangement of atoms in a molecule?
The repulsions between electron pairs around a central atom
The atomic mass of the central atom
The number of protons in the nucleus
The temperature of the environment
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Fill in the Blanks
Type answer...
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Multiple Choice
How does the VSEPR model help predict the shape of a molecule?
By considering the electrostatic repulsions between bonding and nonbonding electron pairs
By measuring the atomic radius of the central atom
By counting the number of atoms in the molecule
By analyzing the color of the atoms
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Open Ended
Compare the molecular geometries and bond angles of beryllium chloride and boron trifluoride as shown in the images.
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Multiple Choice
Which of the following molecules has a tetrahedral molecular geometry?
Methane
Beryllium chloride
Boron trifluoride
Phosphorus pentachloride
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Multiple Select
Select all the correct bond angles present in phosphorus pentachloride according to the VSEPR model.
90°
109.5°
120°
180°
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Open Ended
How do you think understanding molecular structure and Lewis dot structures can help you predict the properties of a molecule?
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Multiple Choice
What is the purpose of using dots and dashes in Lewis structures?
Dots represent bonding electrons, dashes represent nonbonding electrons.
Dots represent nonbonding electrons, dashes represent a pair of bonding electrons.
Dots represent atoms, dashes represent molecules.
Dots represent protons, dashes represent neutrons.
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