Exploring the Periodic Table and Its Trends

The video tutorial covers the electron configuration of atoms and ions, focusing on the energy changes when filling D orbitals. It explains the periodic table's structure, highlighting trends in ionization energy and electron affinity. The tutorial also discusses the historical development of the periodic table and its significance in chemistry. Additionally, it provides insights into the measurement of ionization energies using photoelectron spectroscopy.

What happens to the energy levels of 4s and 3d orbitals when they start filling?

• There is no change in their energy levels.

• 4s and 3d switch in energy levels.

• 3d remains lower in energy than 4s.

• 4s remains lower in energy than 3d.

Why are some elements in the periodic table grouped together?

• They are discovered at the same time.

• They have the same number of protons.

• They have similar electron configurations.

• They have similar atomic masses.

What is ionization energy?

• The energy released when an atom gains an electron.

• The energy required to remove an electron from an atom.

• The energy required to add an electron to an atom.

• The energy released when an atom loses an electron.

Which orbital is the highest occupied atomic orbital in boron?

• 1s

• 2s

• 3s

• 2p

Why is the ionization energy of boron plus different from that of neutral boron?

• Boron plus has more electrons.

• Boron plus has less shielding.

• Boron plus has a lower Z effective.

• Boron plus has more protons.

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

• It increases.

• It decreases.

• It remains the same.

• It fluctuates randomly.

What is the trend in ionization energy as you move down a group in the periodic table?

• It increases.

• It remains the same.

• It decreases.

• It fluctuates randomly.

What is electron affinity?

• The energy released when an atom loses an electron.

• The energy released when an atom gains an electron.

• The energy required to remove an electron from an atom.

• The energy required to add an electron to an atom.

Which group of elements has the highest electron affinity?

• Transition metals

• Halogens

• Alkali metals

• Noble gases

Why do noble gases have negative electron affinities?

• They are highly reactive.

• They have a high Z effective.

• They have low ionization energies.

• They have a full valence shell and do not want to gain electrons.