Fluoride Ion Properties and Structure

The video tutorial explains how to write the Lewis structure for the fluoride ion (F-). It begins by detailing the Lewis structure for neutral fluorine, which has seven valence electrons. The tutorial then transitions to the fluoride ion, which has an extra electron, giving it a total of eight valence electrons, forming a stable octet. The video concludes by showing the complete Lewis structure for the fluoride ion, emphasizing the addition of brackets to indicate its ionic nature.

What is the first step in writing the Lewis structure for the fluoride ion?

• Identify the number of protons in fluorine.

• Write the Lewis structure for neutral fluorine.

• Determine the molecular geometry of fluorine.

• Calculate the atomic mass of fluorine.

Which group on the periodic table does fluorine belong to?

• Group 1

• Group 18

• Group 14

• Group 17

How many valence electrons does neutral fluorine have?

• 5

• 6

• 7

• 8

What change occurs when fluorine becomes a fluoride ion?

• It loses a neutron.

• It loses an electron.

• It gains an electron.

• It gains a proton.

What is the charge of the fluoride ion?

• Positive

• Double negative

• Neutral

• Negative

Why is the fluoride ion considered stable?

• It has a high atomic mass.

• It has more protons than electrons.

• It has a full outer shell of electrons.

• It has an odd number of electrons.

What is the significance of the brackets in the Lewis structure of the fluoride ion?

• They indicate the ion's charge.

• They show the number of protons.

• They represent the atomic mass.

• They highlight the electron configuration.

What is the total number of valence electrons in the fluoride ion?

• 6

• 9

• 7

• 8