Electrons and Atoms

Presentation

•

Chemistry

•

9th - 12th Grade

•

Hard

Joseph Anderson

FREE Resource

57 Slides • 12 Questions

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.

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