Electron Configurations and Energy Levels

The video tutorial explains electron movement, focusing on electronic excitation within atoms. It covers principal energy levels, electron capacity, and how electrons become excited and change states. Using sodium as an example, the tutorial demonstrates electron configuration changes. It concludes with an explanation of atomic emission spectra, highlighting how energy is absorbed and released as light.

What is electronic excitation?

• Electrons moving to a different atom

• Electrons being lost from an atom

• Electrons moving within the same atom

• Electrons being gained by an atom

What is the relationship between principal energy levels and the nucleus?

• Closer PELs have higher energy

• Further PELs have lower energy

• Closer PELs have lower energy

• PEL size is unrelated to the nucleus

How can you determine the maximum number of electrons in a principal energy level?

• By memorizing a formula

• By observing electron behavior

• By using the periodic table

• By counting the electrons in an atom

What happens when an electron absorbs energy?

• It is ejected from the atom

• It moves to a lower energy level

• It moves to a higher energy level

• It stays in the same energy level

What is the ground state of an atom?

• The highest energy configuration

• The lowest energy configuration

• A state with no electrons

• A state with maximum electrons

In the context of electron configurations, what does an excited state mean?

• Electrons are at their lowest energy

• Electrons have absorbed energy and moved to a higher level

• Electrons are in a stable configuration

• Electrons have been lost from the atom

What is the significance of atomic emission spectra?

• They demonstrate electron loss

• They show how electrons are absorbed

• They indicate the energy levels of electrons

• They reveal the color of an atom

What causes the light we see in atomic emission spectra?

• Electrons falling back to lower energy levels

• Electrons moving to higher energy levels

• Electrons absorbing energy

• Electrons being ejected from the atom

How do fireworks utilize the concept of atomic emission spectra?

• By releasing energy as light when electrons fall

• By losing electrons to the environment

• By absorbing energy from the air

• By gaining electrons from other atoms

What is the role of energy in changing electron configurations?

• Energy is not involved

• Energy is absorbed to move electrons to higher levels

• Energy is released to move electrons to higher levels

• Energy is absorbed to keep electrons in the same level