Ionization energy-AP

Ionization energy-AP

Multiple Choice

After the atom is ionised, it then requires more energy to remove a second electron because the second electron experiences less shielding from the nucleus.

• True
• False
• Not sure

Multiple Choice

• a

• b

• c

• d

Multiple Choice

• a

• b

• c

• d

Multiple Choice

Which element could #3 be based on ionization energy?

• Na

• Mg

• Al

• Si

Multiple Choice

What is ionization energy?

• How well an atom attracts electrons in a chemical bond

• The relative size of an atom

• An atom that has gained or lost an electron

• The amount of energy it takes to remove an electron from the valence shell of an atom

Multiple Choice

Which of the following atoms would have the largest second ionization energy?

• Mg

• Cl

• S

• Ca

• Na

Multiple Choice

Which element has the greater ionization energy?

• Lead
• Silicon

Multiple Choice

Which element has the greater ionization energy?

• Strontium
• Boron

Multiple Choice

Which of the following is true about a sulfur atom and a chlorine atom?

• Sulfur is larger and has higher ionization energy.
• Sulfur is larger and has lower ionization energy.
• Sulfur is smaller and has higher ionization energy.
• Sulfur is smaller and has lower ionization energy.

Multiple Choice

Which of the following sequences corresponds to a correct trend in ionization energy?

• Cl > S > P > Al
• Sr > Ca > Mg > Be
• Rb > K > Na > Li
• Rb > Sr > I > Xe

Multiple Choice

Which of the following is true for alkaline earth metals as their atomic number increases?

• The atomic radius decreases.
• Ionization energy decreases.
• The number of valence electrons increases.
• The Coulombic attraction increases.

Multiple Choice

The bar graph above represents four elements and their respective ionization energies. Based on the organization of the modern periodic table, how would these elements be found on the periodic table?

• They are in the same period with W being furthest left.
• They are in the same period with W being furthest right.
• They are in the same group with W being furthest to the bottom.
• They are in a diagonal line with W being at the bottom right.

Multiple Choice

The graph above shows the ionization energy values as the elements are arranged on the periodic table. Which conclusion cannot be drawn from the graph?

• The ionization energy drops significantly as you move down a group because the valence electrons are in a shell further from the nucleus.

• The ionization energy increases gradually as you move right across a period because the valence electrons are in a shell further from the nucleus.

• The ionization energy increases gradually as you move right across a period because you are adding more protons.

• The ionization energy increases when the valence electrons are more attracted to the nucleus.