Question 1

Which of the following best describes what is happening in the image above?

Accepted Answer

Two fluorine atoms are sharing a pair of electrons to form a covalent bond.

Question 2

Based on the electron configurations shown in the image, how many valence electrons does each fluorine atom have before bonding?

Accepted Answer

$$7$$

Question 3

After the covalent bond forms between the two fluorine atoms, how many electrons are in the valence shell of each atom?

Accepted Answer

$$8$$

Question 4

What type of bond is represented by the shared pair of electrons between the two fluorine atoms?

Accepted Answer

Single covalent bond

Question 5

Why do the two fluorine atoms share electrons instead of transferring them?

Accepted Answer

Both atoms have high electronegativity and neither wants to lose electrons.

Question 6

Which of the following is the correct Lewis dot structure for a fluorine molecule ($$\mathrm{F_2$}$$)?

Accepted Answer

$$\cdot\cdot F : F \cdot\cdot$$ with a shared pair of electrons between the two F atoms

Question 7

What is the electron configuration of fluorine after it forms a covalent bond in $$\mathrm{F_2$}$$?

Accepted Answer

$$1s^2$$ $$2s^2$$ $$2p^6$$

Question 8

Which statement best explains why fluorine forms only one single covalent bond?

Accepted Answer

Fluorine has only one unpaired electron in its valence shell.

Question 9

If a fluorine atom were to form an ionic bond with sodium, what would be the resulting formula?

Accepted Answer

$$\mathrm{NaF}$$

Question 10

Which of the following best describes the octet rule as it applies to the fluorine molecule?

Accepted Answer

Each fluorine atom shares electrons to achieve eight electrons in its valence shell.

Covalent Bonding and Naming Covalent Compounds: Guided Study

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