Formal Charges and Lewis Structures

The video tutorial explains how to calculate the formal charge for each atom in xenon hexafluoride (XCF6). It begins with an overview of the Lewis structure, highlighting the expanded octet of xenon. The tutorial then details the calculation of formal charges for fluorine and xenon atoms, emphasizing that the best Lewis structure has formal charges closest to zero. In XCF6, all atoms have a formal charge of zero, confirming the correctness of the structure.

What is the first step in calculating the formal charge for an atom in a molecule?

• Determine the number of protons in the atom.

• Find the number of neutrons in the atom.

• Identify the number of valence electrons in the atom.

• Calculate the atomic mass of the atom.

Why is it acceptable for xenon to have more than eight valence electrons in its Lewis structure?

• Xenon is a metal and can lose electrons easily.

• Xenon is in period two and can hold more electrons.

• Xenon is in period three or below, allowing for an expanded octet.

• Xenon is a non-metal and does not follow the octet rule.

How many unbonded valence electrons does a fluorine atom have in xenon hexafluoride?

• Eight

• Two

• Six

• Four

What is the formal charge of a fluorine atom in xenon hexafluoride?

• +2

• +1

• -1

• 0

Which group does xenon belong to in the periodic table?

• Group 18

• Group 16

• Group 15

• Group 17

How many unbonded valence electrons does xenon have in xenon hexafluoride?

• Six

• Four

• Eight

• Two

What is the formal charge of the xenon atom in xenon hexafluoride?

• +1

• -1

• 0

• +2

What is the significance of having formal charges closest to zero in a Lewis structure?

• It means the structure has too many electrons.

• It indicates the structure is unstable.

• It suggests the structure is incorrect.

• It shows the structure is most likely correct.

What is the formal charge of each atom in xenon hexafluoride?

• +1

• -1

• +2

• 0

What does the presence of zero formal charges in xenon hexafluoride indicate about its Lewis structure?

• The structure is correct.

• The structure is unstable.

• The structure is incorrect.

• The structure has too many electrons.