BL Ch 6 Atomic Structure

Open Ended

How do the properties of extremely small particles, such as electrons, challenge our everyday understanding of matter?

Multiple Choice

Why is understanding the electronic structure of atoms important in chemistry?

• It helps explain chemical bonding and reactivity.

• It determines the color of substances only.

• It is only relevant for large molecules.

• It is not important for understanding chemical reactions.

Multiple Choice

What is the distance between corresponding points on adjacent waves called?

• Wavelength

• Frequency

• Amplitude

• Period

Multiple Select

Which of the following statements about waves are correct?

• The number of waves passing a point per unit time is called frequency.

• Longer wavelength means lower frequency for waves at the same velocity.

• Wavelength and frequency are unrelated.

• If two waves have different frequencies, they must have different velocities.

Fill in the Blank

The speed of light (c) is 3.00 × 10^___ m/s.

Open Ended

Explain why the wave nature of light cannot account for the phenomenon of objects glowing at high temperatures.

Multiple Choice

According to Max Planck, energy comes in discrete packets called:

• Quanta

• Photons

• Electrons

• Waves

Multiple Choice

Which equation represents the relationship between the energy of a photon and its frequency, as explained by Einstein?

• E = hν

• E = mc^2

• E = λν

• E = 1/2 mv^2

Open Ended

Explain why each element has a unique line spectrum.

Fill in the Blank

Johann Balmer discovered a simple formula relating the four lines in the hydrogen spectrum to ___.

Multiple Choice

Which of the following is NOT a limitation of the Bohr Model?

• It only works for hydrogen.

• Classical physics would result in an electron falling into the nucleus.

• Circular motion is not wave-like in nature.

• It accurately describes all elements.

Multiple Choice

Which of the following statements is NOT a postulate of the Bohr model as described in the slides?

• Electrons can only occupy certain orbits corresponding to certain energies.

• Electrons in permitted orbits have specific, allowed energies.

• Energy is absorbed or emitted when electrons move between allowed energy states.

• Electrons can exist at any energy level within the atom.

Open Ended

What are two important ideas from the Bohr Model that are incorporated into the current atomic model?

Open Ended

According to the Bohr model, what is the equation used to calculate the energy absorbed or emitted during electron transitions?

Multiple Choice

According to de Broglie, what is the relationship between the mass and wavelength of a particle?

• λ = h/mv

• λ = mv/h

• λ = h + mv

• λ = h - mv

Multiple Select

Select all statements that correctly describe the process of electron promotion or demotion according to the Bohr model.

• The energy absorbed or emitted can be calculated using the Rydberg formula.

• Electrons can move between any two energy levels without restriction.

• The Rydberg constant is used in calculating the energy change.

• The principal quantum numbers of the initial and final states are important in the calculation.

Fill in the Blank

The more precisely the momentum of a particle is known, the less precisely its ___ is known.

Multiple Choice

Which quantum number describes the energy level on which the orbital resides?

• Principal quantum number (n)

• Angular momentum quantum number (l)

• Magnetic quantum number (ml)

• Spin quantum number (ms)

Open Ended

Explain how the concept of electron density is related to Schrödinger's wave equation.

Fill in the Blank

The letter designation for the value l = 2 is ___

Multiple Select

Which statements about quantum mechanics and Schrödinger's contributions are correct?

• Quantum mechanics incorporates both wave and particle nature of matter.

• Schrödinger developed a mathematical treatment for quantum mechanics.

• Quantum mechanics only describes the wave nature of matter.

• Schrödinger's equation cannot predict electron probability.

Open Ended

Explain how the values of the angular momentum quantum number (l) relate to the shape and type of atomic orbitals.

Multiple Select

Which of the following statements about the magnetic quantum number (ml) are correct?

• It describes the three-dimensional orientation of the orbital.

• Its allowed values range from -l to +l.

• It determines the energy level of the orbital.

• It affects the number of orbitals in a subshell.

Open Ended

Describe the relationship among the quantum numbers n, l, and ml in determining the arrangement and number of atomic orbitals within an electron shell.

Multiple Choice

How many p orbitals are present in the n = 2 shell?

• 1

• 2

• 3

• 6

Multiple Choice

What is meant by the term 'electronic structure' in the context of atoms?

• The arrangement and energy of electrons in an atom

• The number of protons in an atom

• The arrangement of neutrons in the nucleus

• The chemical properties of a molecule