Ch. 5 Electrons in Atoms

Multiple Choice

Define wavelength?

• Wavelength is the distance between equal points of a wave (crest to crest or trough to trough).

• Wavelength is the frequency of a wave.
• Wavelength is the amplitude of a wave.
• Wavelength is the speed of a wave.

Multiple Choice

Define frequency of a wave.

• The frequency of a wave is its amplitude.
• The frequency of a wave is the distance between two peaks.
• The frequency of a wave is the speed of the wave divided by its wavelength.
• The frequency of a wave is the number of cycles per second.

Multiple Choice

Describe the relationship between wavelength and frequency.

• Wavelength and frequency are unrelated.
• Wavelength increases as frequency increases.
• Wavelength and frequency are directly related.
• Wavelength and frequency are inversely related.

Multiple Choice

Describe the relationship between energy and frequency.

• Energy is directly proportional to frequency.
• Energy is inversely proportional to frequency.
• Energy is unrelated to frequency.
• Energy decreases as frequency increases.

Multiple Choice

What are photons?

• Photons are particles that have mass and are found in atoms.
• Photons are massless particles that carry energy in the form of electromagnetic radiation.

• Photons are heavy particles that carry sound waves.
• Photons are electromagnetic waves that do not exist in particle form.

Multiple Choice

Describe the Bohr model.

• The Bohr model describes the atom as a solid sphere with no internal structure.
• The Bohr model shows electrons moving in random paths around the nucleus.
• The Bohr model suggests that electrons can exist anywhere in the atom without specific energy levels.
• The Bohr model depicts the atom with electrons in fixed orbits around a nucleus, with quantized energy levels.

Multiple Choice

Describe the quantum mechanical model.

• Electrons are depicted as particles in fixed orbits around the nucleus.
• The model states that electrons have definite positions and velocities at all times.
• It describes atoms as solid spheres with no internal structure.
• The quantum mechanical model describes electrons as wave functions in orbitals, emphasizing probability and quantization.

Multiple Choice

What are the 4 types of orbitals?

• g, h, i, j
• x, y, z, w
• s, p, d, f
• 1s, 2p, 3d, 4f

Multiple Choice

Describe the Aufbau Principle.

• The Aufbau Principle states that electrons can occupy any orbital regardless of energy level.
• The Aufbau Principle describes the behavior of protons in an atom.
• The Aufbau Principle is a theory about the chemical bonding of molecules.
• The Aufbau Principle describes the order in which electrons fill atomic orbitals, starting from the lowest energy level to higher ones.

Multiple Choice

Describe Pauli Exclusion Principle.

• A maximum electrons can occupy the same atomic orbital, but they must have opposite spins.

• The Pauli Exclusion Principle applies only to bosons.
• All particles can occupy the same quantum state without restriction.
• Electrons can occupy the same quantum state if they are in different energy levels

Multiple Choice

Describe Hund's Rule.

• Hund's Rule describes the distribution of electrons in orbitals, emphasizing that electrons fill like orbitals singly before pairing.

• Electrons are distributed randomly across all orbitals without any specific order.
• Hund's Rule states that electrons must always pair up in the same orbital first.
• Electrons fill all orbitals completely before any pairing occurs.

Multiple Choice

What are valence electrons?

• Valence electrons are the electrons that do not participate in chemical reactions.
• Valence electrons are the electrons that are always in the inner shells of an atom.
• Valence electrons are the electrons in the outermost shell of an atom that are involved in chemical bonding.
• Valence electrons are the protons in the nucleus of an atom.