Chapter 5 Key Concepts Flashcards
What was the basic new proposal in the Bohr model of the atom?
That an electron is found only in the specific circular paths, or orbits, around the nucleus
Why did Rutherford’s atomic model need to be replaced?
It could not explain the chemical properties of elements
What does the quantum mechanical model determine about electrons in atoms?
The allowed energies an electron can have and how likely it is to find the electron in various locations around the nucleus
How do 2 sublevels of the same principal energy level differ from each other?
Each energy sublevel corresponds to an orbital of a different shape, which describes where the electron is likely to be found
What are the three rules for writing the electron configuration of elements?
The aufbau principle, the Pauli principle, and Hund’s rule
Explain why the actual electron configurations for some elements differ from those assigned using the aufbau principle.
Because half-filled sublevels are not as stable as filled sublevels, but they are more stable than other configurations
How are wavelength and frequency of light related?
They are inversely proportional to each other
Describe the cause of atomic emission spectrum of an element.
When atoms absorb energy, electrons move into higher energy levels, and these electrons lose energy by emitting light when they return to lower energy levels
How is the change in electron energy related to the frequency of light emitted in atomic transitions?
The light emitted by an electron moving from a higher to a lower energy level has a frequency directly proportional to the energy change of the electron
How does quantum mechanics differ from classical mechanics?
Classical mechanics adequately describes the motions of bodies much larger than atoms, while quantum mechanics describes the motions of subatomic particles and atoms as waves
