Lecture 5 - EMR, Bohr model

What are the specific, allowed energy levels that electrons occupy in atoms called?

Atomic orbitals.

What is the lowest energy state of an electron in an atom referred to as?

Ground state.

What is the relationship between energy and wavelength in electromagnetic radiation?

Wavelength and energy are inversely related.

What is the equation that relates wavelength (λ), frequency (ν), and the speed of light (c)?

λν = c.

How do electrons move between energy levels in an atom?

By absorbing or emitting light energy (electromagnetic radiation).

What is the significance of the Bohr model's ground state?

It indicates the lowest energy level, with the electron closest to the nucleus.

How does the photon energy relate to frequency and wavelength according to the equations presented?

Ephoton = hν and Ephoton = hc/λ.

Which electromagnetic radiation has the highest frequency: gamma rays, visible light, or radio waves?

Gamma rays.

What is considered a 'clicker question' in the context of this lecture?

A question used to engage students and assess their understanding of key concepts.

What major restriction does the Bohr model have regarding the elements it can accurately describe?

It only works for hydrogen or any ion that contains just one electron.

Define ionization energy in the context of the Bohr model.

The energy required to remove an electron from the atom, taking it to the n = ∞ energy level.

What type of model is currently used instead of the Bohr model?

The quantum mechanical model.

What are the units for frequency (ν) in electromagnetic waves?

Hertz (Hz) or waves per second (s⁻¹).

What is a major issue with the Bohr model when applied to elements other than hydrogen?

It does not accurately describe multi-electron atoms.

In terms of electron transitions, what does a positive ΔE signify?

Electrons are being absorbed to move to a higher energy level (endothermic process).