1. Chapter 5 Review
Electrons in Atoms

2. Electrons are restricted to certain energy levels
What are the similarities and differences between the Bohr model of the atom and the quantum mechanical model of the atom?
Similarities:
Electrons are restricted to certain energy levels
Electrons must gain a minimum amount of energy to change position within the atom
Differences:
In the quantum mechanical model, electrons can be found in regions of space (orbitals) surrounding the nucleus, but the path that they travel is not predictable unlike the electrons in the Bohr model which travel in specified orbits.

3. What is the wavelength of a wave that has a frequency of 3.0x108/s?
1x10-2m
Is this wave part of the continuous spectrum?
No. This wave is not present in the visible range

4. What is the relationship between …
Wavelength and frequency =
Frequency and Energy=
Wavelength and Energy=
indirect (negative slope)
direct(positive slope)
indirect (negative slope)

5. What is the energy of a wave that has a wavelength of 1x 10-8m?
In order to do this problem you first have to solve for frequency using the speed of light equation and then input this frequency in to the energy equation.
E=2x10-17J

6. What particles of light carry a quantum of energy?
Photons

7. What is the electron configuration of lead
What is the electron configuration of lead? How many valence electrons does it have? What is it’s Lewis Dot Structure?
[Xe]4f14 5d10 6s2 6p2 4

8. How does the speed of ultraviolet waves compare to that of visible waves?
The speed of all waves travel at the speed of light, so there is no difference in the speed of ultraviolet waves and visible waves

9. What color light has the longest wavelength?
Red

10. How much energy must an electron gain to transition to a higher energy level within the atom? Is the amount of energy constant for transitions from one level to the next?
Quantum
No. As an electron moves further away from the nucleus, less and less energy is required to transition to the next energy level.

11. Match the rule/principle name to the description below.
A. Hund’s Rule B. Pauli’s Exclusion Principle C. Aufbau’s Principle
___ A maximum of two electrons can occupy a single orbital
___ Electrons occupy the orbitals of lowest energy first
___Electrons enter the orbitals of sublevels that contain multiple orbitals one at a time before electrons are paired in those orbitals B C A

12. How many pairs of electrons exist in the 3d orbitals of Iron (Fe)?1

13. What part of the electromagnetic spectrum contains the continuous spectrum?
The visible spectrum. The continuous spectrum contains all the wavelength and frequencies of visible light (a rainbow)

14. How many electrons are there in the 3rd energy level of Iron?
12 (3s2, 3p6, 3d6)

15. Which transition between energy levels would represent the greatest amount of energy being emitted by an element? A. 1 to 5 B. 2 to 4 C. 5 to 2 C
Electrons absorb energy and move from low energy levels to high energy levels. Energy is emitted in the form of light as electrons return to a lower energy level (ground state)