7.4 and 7.5 Questions

What is one of the objectives of this lesson regarding ionization energy?

• Predict the product of chemical reactions

• Describe the trend in ionization energy across a period and down a group

• Calculate the exact ionization energy for elements

• Compare ionization energy between only two specific elements

What else does this lesson aim to explain about ionization energy?

• How to measure ionization energy in a laboratory

• The history of the discovery of ionization energy

• Why the trends in ionization energy exist

• The impact of ionization energy on the human body

What is ionization energy?

• Energy required to add an electron to an atom

• Energy required to remove the most loosely bound electron in the valence shell

• Energy released when an electron is added to an atom

• Energy required to break a chemical bond

What happens to ionization energy as you move across a period in the periodic table?

• It decreases

• It remains constant

• It increases

• It fluctuates unpredictably

Why does ionization energy increase across a period?

• Due to increased electron shielding

• Because of a decrease in atomic radius

• Because of a stronger proton (nuclear) pull

• Due to a decrease in nuclear charge

Which element has a greater nuclear charge, Al or Cl?

• Al

• Cl

• Both have the same nuclear charge

• Cannot be determined from the image

Based on the image, what is the trend in nuclear charge from Al to Cl?

• It decreases from Al to Cl

• It increases from Al to Cl

• It remains constant from Al to Cl

• The trend is not shown in the image

Refer to the diagrams in the image. What do the characters inside the atomic orbitals represent?

• The size of the atom

• The nuclear charge of the atom

• The number of electrons in the atom

• The number of protons in the nucleus

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

• It increases

• It stays the same

• It decreases

• It fluctuates unpredictably

Why does ionization energy decrease as you move down a group in the periodic table?

• Smaller atomic radius means more nuclear pull on outer electrons

• Larger atomic radius means more nuclear pull on outer electrons

• Smaller atomic radius means less nuclear pull on outer electrons

• Larger atomic radius means less nuclear pull on outer electrons