Atomic Structure and Electron Behavior

The video tutorial explores how atomic size changes with ions, comparing atomic sizes, and understanding effective nuclear charge. It discusses trends in ionization energy, exceptions in these trends, and delves into electron affinity and electronegativity, providing a comprehensive overview of these key chemistry concepts.

How does the size of a magnesium ion compare to an oxygen ion?

• Magnesium ion and oxygen ion are the same size.

• Magnesium ion size cannot be compared to oxygen ion.

• Magnesium ion is smaller than oxygen ion.

• Magnesium ion is larger than oxygen ion.

Which factor primarily determines the effective nuclear charge?

• Number of electrons

• Number of protons

• Number of neutrons

• Number of shells

Why do larger atoms generally require less energy to remove an electron?

• Electrons are closer to the nucleus.

• Electrons are farther from the nucleus.

• Larger atoms have fewer electrons.

• Larger atoms have more protons.

What is a key reason for the exceptions in ionization energy trends?

• Presence of paired electrons

• Presence of empty sub-shells

• Presence of half-filled sub-shells

• Presence of full sub-shells

Which element would have a lower ionization energy due to a new sub-shell?

• Carbon

• Boron

• Nitrogen

• Oxygen

Which atom is likely to have the most exothermic electron affinity?

• Chlorine

• Iodine

• Bromine

• Selenium

What does a higher electronegativity indicate about an atom?

• It has a larger atomic size.

• It has more neutrons.

• It has a lower ionization energy.

• It has a stronger attraction for electrons.

Which of the following atoms would require more energy to remove an electron: sodium or chlorine?

• Chlorine, because it has a higher effective nuclear charge.

• Chlorine, because it has fewer electrons.

• Sodium, because it has more shells.

• Sodium, because it has fewer protons.

Why is it easier to remove an electron from a half-filled sub-shell?

• Electrons in half-filled sub-shells are farther from the nucleus.

• Electrons in half-filled sub-shells are closer to the nucleus.

• Half-filled sub-shells are more stable.

• Half-filled sub-shells are less stable.

What is the relationship between atomic size and electronegativity?

• Atomic size does not affect electronegativity.

• Smaller atoms have higher electronegativity.

• Electronegativity is only affected by the number of protons.

• Larger atoms have higher electronegativity.