6. Ionization Energy

What is ionization energy?

• The amount of energy required to remove an electron from a gaseous atom.

• The energy released when an electron is added to a gaseous atom.

• The energy required to add a neutron to a nucleus.

• The energy needed to split a molecule into atoms.

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Describe the ionization energy trend from the Periodic Table.

• I.E. decreases down a group and increases across a period.

• I.E. increases down a group and decreases across a period.

• I.E. remains constant down a group and increases across a period.

• I.E. decreases down a group and remains constant across a period.

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Explain why it requires more energy to remove each subsequent electron after the first. It always requires more energy to remove a 2nd or 3rd electron because they are more attracted to a positive ion than a neutral atom.

• Because the electrons are more attracted to a positive ion than a neutral atom.

• Because the electrons are less attracted to a positive ion than a neutral atom.

• Because the electrons are equally attracted to a positive ion and a neutral atom.

• Because the electrons are not attracted to a positive ion at all.

There is a very large increase of ionization energy whenever an electron is removed from an atom/ion that is ____.

• iso electronic with a noble gas.

• in a high energy state.

• part of a covalent bond.

• in a metallic state.

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If an atom loses electrons, it becomes a negative ion.

(a)  

• True
• False

Which of the following factors does not directly influence the ionization energy of an atom?

• Atomic radii

• Nuclear charge

• Shielding effect

• Neutrons

As you move across the periodic table atoms tend to get smaller because, ______________.

• the atoms have more mass.
• the atoms have less mass
• the atoms have more protons.
• the atoms have less electrons.

Which element has the greatest ionization energy: Aluminum (Al)    or    Chlorine (Cl)?

• Aluminum (Al)

• Chlorine (Cl)

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As you move down the periodic table atoms get bigger.  This is because ____________.

• The atoms have more mass.
• The atoms have more protons.
• The atoms have more energy levels
• The atoms have more nuetrons

Which of these elements has the lowest ionization energy?

• Oxygen (O)
• Boron (B)
• Carbon (C)
• Fluorine (F)

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