Ionization Energy Concepts and Trends

The video tutorial by M sjcam explores trends in ionization energy, starting with a definition of first ionization energy as the energy needed to remove one mole of electrons from gaseous atoms. It explains the ionization of sodium and discusses how ionization energies are endothermic. The tutorial examines trends across the periodic table, noting that ionization energy decreases down a group and increases across a period, with exceptions like beryllium to boron and nitrogen to oxygen. The reasons for these trends include changes in nuclear charge, atomic radius, and electron shielding.

What is the first ionization energy?

• The energy required to add one mole of electrons to one mole of gaseous atoms

• The energy required to remove one mole of electrons from one mole of gaseous atoms

• The energy released when one mole of electrons is added to one mole of gaseous atoms

• The energy released when one mole of electrons is removed from one mole of gaseous atoms

What does the equation for the first ionization of sodium show?

• One mole of gaseous sodium atoms gaining one mole of electrons

• One mole of gaseous sodium ions losing one mole of electrons

• One mole of gaseous sodium ions gaining one mole of electrons

• One mole of gaseous sodium atoms losing one mole of electrons

Why do ionization energies have positive values?

• Because the process is exothermic

• Because electrons are attracted to the nucleus

• Because energy is required to overcome the attraction between the nucleus and electrons

• Because energy is released when electrons are removed

Which elements have the highest ionization energies?

• Lithium, Sodium, and Potassium

• Helium, Neon, and Argon

• Beryllium, Boron, and Carbon

• Nitrogen, Oxygen, and Fluorine

What is the trend in ionization energy down Group 18?

• It remains constant

• It decreases

• It fluctuates

• It increases

What is the trend in ionization energy down Group 1?

• It remains constant

• It increases

• It fluctuates

• It decreases

What is the general trend in ionization energy across a period?

• It remains constant

• It increases

• It decreases

• It fluctuates

Which of the following pairs show an exception to the general trend in ionization energy?

• Beryllium and Boron

• Fluorine and Neon

• Lithium and Beryllium

• Carbon and Nitrogen

Why does ionization energy increase across a period?

• Because the nuclear charge decreases and atomic radius increases

• Because the nuclear charge remains constant and atomic radius increases

• Because the nuclear charge decreases and atomic radius remains constant

• Because the nuclear charge increases and atomic radius decreases

Why does ionization energy decrease down a group?

• Because the number of occupied energy levels decreases and electron shielding increases

• Because the number of occupied energy levels increases and electron shielding increases

• Because the number of occupied energy levels increases and electron shielding decreases

• Because the number of occupied energy levels decreases and electron shielding decreases