1. Chapter 5 Review

2. Vocabulary Discrete bundle of energy Energy needed to move an electron from one energy level to another Separation of light into different wavelengths

3. Vocabulary Number of wave cycles passing a point per unit of time Distance between wave crests Frequencies of light emitted by an element

4. Vocabulary Region of high probability of finding an electron Lowest energy level Arrangement of electrons around atomic nucleus

5. Vocabulary States the impossibility of knowing both velocity and position of a moving particle at the same time Tendency of electrons to enter orbitals of lowest energy first Each orbital has at most two electrons

6. The principal quantum number indicates the _____ ______ of an electron. In the Bohr model, an electron in an orbit has a fixed ______. In Bohr’s model, the ______ move around the _______ which are at the center of the atom. How many energy sublevels are in the each principal energy level?

7. How many s, p, d, and f orbitals are there in each energy level? What is the maximum number of electrons in each energy level? What types of orbitals are in each energy level? The sublevel letter indicates the orbital ______.

8. If the spin of one electron in an orbital is clockwise, then the spin of the other electron is ________. If three electrons are available to fill a p sublevel, how will they be distributed? Stable electron configurations contain ______ energy sublevels.

9. Which electromagnetic waves have the highest frequency? Lowest frequency? How are wavelength and frequency related? What is directly proportional to frequency? When does emission of light occur?

10. Write electron configurations and tell number of electrons in the highest energy level: Germanium Sulfur Lithium Calcium Boron Chromium

11. Calculations Determine the energy of a photon having a frequency of 7.3 x 10 6 Hz. Calculate the frequency when the wavelength is 4.92 x 10 -8 m.