A student is drawing the Lewis structure for SO3 and calculates the total valence electrons as 18. However, the correct number is 24. What mistake did the student most likely make?

The student only counted the valence electrons of one oxygen atom instead of all three

The student forgot to count the valence electrons of sulfur

The student added extra electrons for the bonds

The student used the atomic number instead of the group number to determine valence electrons for oxygen

When drawing the Lewis structure for PCl5, a student insists that phosphorus cannot form this molecule because it violates the octet rule. Evaluate this reasoning and determine the correct explanation.

The student is incorrect; phosphorus can expand its octet because it has available d-orbitals in the third period

The student is correct; PCl5 cannot exist because phosphorus must follow the octet rule

The student is incorrect; phosphorus follows the duet rule, not the octet rule

The student is correct; PCl5 violates the octet rule and is therefore unstable

A student draws the Lewis structure for CO2 with two single bonds and places all remaining electrons as lone pairs on carbon. Identify the error and explain the correct approach.

The student should form two double bonds between carbon and each oxygen atom to satisfy the octet rule for all atoms

The student should place all lone pairs on oxygen and form a triple bond between carbon and one oxygen

The student should form one double bond and one single bond, placing extra electrons on carbon

The student's structure is correct because carbon does not need to follow the octet rule

When drawing the Lewis structure for a polyatomic ion such as NO3-, how should the negative charge be accounted for in the valence electron count, and why?

Add 1 electron to the total because the negative charge indicates the ion has gained an extra electron

Subtract 1 electron from the total because the ion has lost an electron to become negative

Ignore the charge because it does not affect the number of valence electrons

Divide the total valence electrons by the charge to get the correct count

A student draws the Lewis structure for HCN and places hydrogen as the central atom. Evaluate whether this is correct and explain the reasoning.

This is incorrect; carbon should be the central atom because hydrogen can only form one bond and cannot be a central atom

This is correct because hydrogen always goes in the center of a molecule

This is correct because hydrogen has the fewest valence electrons

This is incorrect; nitrogen should be the central atom because it has the most valence electrons

In drawing the Lewis structure for O3 (ozone), a student finds that a single structure does not adequately represent the molecule. What concept best explains this situation, and how should the student represent the structure?

The student should draw resonance structures to show the delocalization of electrons across the molecule

The student should use an expanded octet for the central oxygen atom

The student should place all electrons as lone pairs on the terminal oxygen atoms

The student should form a triple bond between the two oxygen atoms to satisfy the octet rule

A student is asked to draw the Lewis structure for SF6. They argue that this molecule cannot exist because sulfur would need 12 electrons around it, violating the octet rule. Analyze this argument and provide the correct reasoning.

The student is incorrect; sulfur is in the third period and can accommodate more than 8 electrons by using its available d-orbitals

The student is correct; SF6 cannot exist because no atom can have more than 8 electrons

The student is incorrect; sulfur follows the duet rule and only needs 2 electrons

The student is correct; SF6 is a theoretical molecule that does not exist in nature

When drawing the Lewis structure for N2, a student draws a single bond between the two nitrogen atoms and places three lone pairs on each nitrogen. Evaluate this structure and determine the correct Lewis structure.

The student's structure is incorrect; nitrogen should form a triple bond with the other nitrogen atom, with one lone pair remaining on each nitrogen

The student's structure is correct because nitrogen only needs 5 electrons around it

The student's structure is incorrect; nitrogen should form a double bond, with two lone pairs on each nitrogen

The student's structure is correct because each nitrogen has 8 electrons around it

A student is drawing the Lewis structure for BF3 and insists on adding an extra lone pair to boron to satisfy the octet rule. Analyze this reasoning and determine the correct approach.

The student is incorrect; boron is an exception to the octet rule and can have fewer than 8 electrons, making BF3 an electron-deficient molecule

The student is correct; boron must always satisfy the octet rule in Lewis structures

The student is incorrect; the extra lone pair should be placed on fluorine, not boron

The student is correct; without the extra lone pair, the structure of BF3 would be unstable

In drawing the Lewis structure for ClO4- (perchlorate ion), a student calculates the total valence electrons as 31. Identify the error and determine the correct total number of valence electrons.

The student forgot to add the extra electron for the negative charge; the correct total is 32

The student added an extra electron; the correct total is 30

The student miscounted the valence electrons of chlorine; the correct total is 28

The student is correct; the total number of valence electrons is 31

A student draws the Lewis structure for CO and places a double bond between carbon and oxygen. Evaluate this structure and determine whether it correctly satisfies the octet rule for both atoms.

The structure is incorrect; carbon monoxide has a triple bond between carbon and oxygen, which satisfies the octet rule for both atoms

The structure is correct; a double bond satisfies the octet rule for both carbon and oxygen

The structure is correct; carbon only needs 6 electrons to be stable

The structure is incorrect; carbon monoxide should have a single bond with lone pairs on both atoms

When drawing the Lewis structure for H2SO4, a student places hydrogen atoms directly bonded to sulfur. Identify the error and explain the correct bonding arrangement.

The student is incorrect; the hydrogen atoms in H2SO4 are bonded to oxygen atoms, not directly to sulfur

The student is correct; hydrogen atoms bond directly to sulfur in H2SO4

The student is incorrect; hydrogen atoms should be placed as lone pairs on sulfur

The student is correct; sulfur is the central atom and all other atoms bond directly to it

A student is comparing the Lewis structures of O2 and F2. They claim both molecules should have the same number of lone pairs since oxygen and fluorine are in the same period. Analyze this claim and determine the correct number of lone pairs in each molecule.

The student is incorrect; O2 has 2 lone pairs per oxygen atom (4 total), while F2 has 3 lone pairs per fluorine atom (6 total), because fluorine has one more valence electron than oxygen

The student is correct; both O2 and F2 have the same number of lone pairs

The student is incorrect; O2 has 3 lone pairs per oxygen

Why is this Lewis Structure incorrect? Choose all that apply.

There are too many bonds around the Si atom.

The structure only required two double bonds to fulfill the octet.

The Structure is missing a triple bond.

Each chlorine only has 6 electrons surrounding it.

Mastering Lewis Structures Quiz

Authored by Nicki Graziano

Chemistry

10th Grade

NGSS covered

Used 1+ times

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33 questions

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MULTIPLE CHOICE QUESTION

30 sec • 1 pt

How many valence electrons does a carbon atom have?

What is the total number of valence electrons in a hydrogen atom?

MULTIPLE CHOICE QUESTION

30 sec • 1 pt

How many valence electrons does an oxygen atom have?

What is the maximum number of electrons that can be placed in the first electron shell?

MULTIPLE CHOICE QUESTION

30 sec • 1 pt

In a Lewis structure, what does a single line between two atoms represent?

A lone pair of electrons

A single covalent bond (2 electrons)

A double covalent bond (4 electrons)

An ionic bond

MULTIPLE CHOICE QUESTION

30 sec • 1 pt

How many valence electrons does a nitrogen atom have?

What is the octet rule in the context of Lewis structures?

Atoms tend to gain, lose, or share electrons to have 2 electrons in their outer shell

Atoms tend to gain, lose, or share electrons to have 8 electrons in their outer shell

Atoms always form exactly 4 bonds

Atoms must always have an equal number of protons and electrons

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Mastering Lewis Structures Quiz

How many valence electrons does a carbon atom have?

What is the total number of valence electrons in a hydrogen atom?

How many valence electrons does an oxygen atom have?

What is the maximum number of electrons that can be placed in the first electron shell?

In a Lewis structure, what does a single line between two atoms represent?

How many valence electrons does a nitrogen atom have?

What is the octet rule in the context of Lewis structures?

How many valence electrons does a chlorine atom have?

What is the total number of valence electrons in a molecule of H2O?

In a Lewis structure, what are the dots surrounding an atomic symbol used to represent?

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