Ionization Energy and Periodic Trends Quiz

What is ionization energy?

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

• The energy released when an atom gains an electron

• The energy required to split an atom into ions

• The energy required to add an electron to an atom

When a sodium atom loses an electron, what type of ion is formed?

• Neutral atom

• Isotope

• Cation

• Anion

In the sodium atom, which electron is removed during ionization?

• The innermost electron

• The electron in the second energy level

• The electron closest to the nucleus

• The valence electron

How does ionization energy change across a period from left to right?

• It decreases

• It fluctuates randomly

• It remains constant

• It increases

Which region of the periodic table has the highest ionization energies?

• Upper left

• Lower right

• Upper right

• Lower left

What happens to ionization energy as you move down a group in the periodic table?

• It doubles

• It remains the same

• It decreases

• It increases

Why do smaller atoms have higher ionization energies?

• Their electrons are closer to the nucleus

• They have more electrons

• Their electrons are farther from the nucleus

• They have fewer protons

Which type of elements tend to form cations due to low ionization energy?

• Noble gases

• Metals

• Metalloids

• Non-metals

What is the relationship between atomic radius and ionization energy?

• Smaller atomic radius means lower ionization energy

• Larger atomic radius means higher ionization energy

• Atomic radius does not affect ionization energy

• Larger atomic radius means lower ionization energy

Which of the following is true about non-metals in terms of ionization energy?

• They tend to gain electrons

• They have low ionization energies

• They form cations easily

• They tend to lose electrons easily