Chem Ch 5 Review Sheet

atomic orbital
ground state
aufbau principle
Pauli exclusion principle
electron configuration
Heisenberg uncertainty principle

atomic emission spectrum
photon
frequency
quantum
wavelength
spectrum

1.	In Bohr's model of the atom, where are the electrons and protons located?
2.	How does the energy of an electron change when the electron moves closer to the nucleus?
3.	The principal quantum number indicates what property of an electron?
4.	What is the shape of the 3p atomic orbital?
5.	How many energy sublevels are in the second principal energy level?
6.	What is the maximum number of f orbitals in any single energy level in an atom?
7.	What is the maximum number of orbitals in the p sublevel?
8.	What is the maximum number of electrons in the second principal energy level?
9.	When an electron moves from a lower to a higher energy level, the electron ____.
10.	If the spin of one electron in an orbital is clockwise, what is the spin of the other electron in that orbital?
11.	What types of atomic orbitals are in the third principal energy level?
12.	What is the next atomic orbital in the series 1s, 2s, 2p, 3s, 3p?
13.	According to the aufbau principle, ____.
14.	What is the number of electrons in the outermost energy level of an oxygen atom?
15.	What is the electron configuration of potassium?
16.	If three electrons are available to fill three empty 2p atomic orbitals, how will the electrons be distributed in the three orbitals?
17.	How many unpaired electrons are in a sulfur atom (atomic number 16)?
18.	How many half-filled orbitals are in a bromine atom?
19.	Stable electron configurations are likely to contain ____.
20.	What is the basis for exceptions to the aufbau diagram?
21.	Which electron configuration of the 4f energy sublevel is the most stable?
22.	Which color of visible light has the shortest wavelength?
23.	How are the frequency and wavelength of light related?
24.	What is the wavelength of an electromagnetic wave that travels at 3  10 m/s and has a frequency of 60 MHz? (1 MHz = 1,000,000 Hz)
25.	As changes in energy levels of electrons increase, the frequencies of atomic line spectra they emit ____.
26.	The atomic emission spectra of a sodium atom on Earth and of a sodium atom in the sun would be ____.
27.	What is the approximate energy of a photon having a frequency of 4  10 Hz? (h = 6.6  10 Js)
28.	What is the approximate frequency of a photon having an energy 5  10 J? (h = 6.6  10 Js)
29.	Which variable is directly proportional to frequency?
30.	What are quanta of light called?
31.	Which scientist developed the quantum mechanical model of the atom?
32.	Bohr's model could only explain the spectra of which type of atoms?
33.	Who predicted that all matter can behave as waves as well as particles?
34.	According to the Heisenberg uncertainty principle, if the position of a moving particle is known, what other quantity CANNOT be known?
35.	How can the position of a particle be determined?
36.	The wavelike properties of electrons are useful in ____.
37.	In an s orbital, the probability of finding an electron a particular distance from the nucleus does NOT depend on ____.
38.	Give the electron configuration for a neutral atom of chlorine.
39.	Give the electron configuration for a neutral atom of selenium.
40.	What is the wavelength of gamma ray electromagnetic radiation with a frequency of 2.73  10 Hz? (c = 3.00  10 m/s)
41.	What is the frequency of a radar photon with energy 6.80  10 J? (h = 6.63  10 Js)
42.	What is the energy of a microwave photon that has a frequency of 1.12  10 Hz? (h = 6.63  10 Js)