Formal Charges and Valence Electrons

Formal Charges and Valence Electrons

Assessment

Interactive Video

Chemistry

9th - 10th Grade

Practice Problem

Hard

Created by

Amelia Wright

FREE Resource

The video tutorial explains how to calculate the formal charge for each element in hydrofluoric acid (HF) using the Lewis structure. It details the process for hydrogen and fluorine, showing that both have a formal charge of zero. The tutorial concludes that when formal charges are zero or close to zero, it indicates the most favorable Lewis structure. This is demonstrated as the best structure for HF.

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8 questions

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1.

MULTIPLE CHOICE QUESTION

30 sec • 1 pt

What is the first step in calculating formal charges using the Lewis structure?

Count the total number of electrons in the molecule.

Identify the number of protons in the atom.

Calculate the molecular weight of the compound.

Determine the number of valence electrons for each atom.

2.

MULTIPLE CHOICE QUESTION

30 sec • 1 pt

How many valence electrons does hydrogen have in HF?

Two

One

Three

Four

3.

MULTIPLE CHOICE QUESTION

30 sec • 1 pt

What is the formal charge on hydrogen in HF after calculation?

-1

+1

+2

0

4.

MULTIPLE CHOICE QUESTION

30 sec • 1 pt

In which group is fluorine found on the periodic table?

Group 1

Group 17

Group 2

Group 18

5.

MULTIPLE CHOICE QUESTION

30 sec • 1 pt

How many unbonded valence electrons does fluorine have in HF?

Four

Eight

Two

Six

6.

MULTIPLE CHOICE QUESTION

30 sec • 1 pt

What is the formal charge on fluorine in HF after calculation?

+1

-1

0

+2

7.

MULTIPLE CHOICE QUESTION

30 sec • 1 pt

What does a formal charge of zero indicate about a Lewis structure?

It is unstable.

It is the most likely or favorable structure.

It is incorrect.

It has too many electrons.

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