Download Study Guide: Chapter 4 - the Arrangement of Electrons in Atoms

Study Guide: Chapter 4 - the Arrangement of Electrons in Atoms
1. Understand the relationship between a light wave’s frequency and wavelength; Know how to calculate
wavelength given frequency and frequency given wavelength (MEMORIZE FORMULA) – work a few practice
problems
2. Understand the relationship between energy of light and its frequency; Know how to calculate the energy of light
given its frequency, and the frequency given its energy (MEMORIZE FORMULA; Planck’s constant will be given on
the test) – work a few practice problems
3. Know what a line emission spectrum is and how it’s produced
4. Understand that an electron must gain energy in order to move (temporarily) to a higher energy level – excited
state; it emits the same amount of energy (in the form of light) when it falls back to its ground state
5. Understand how the line emission spectrum of hydrogen led to Bohr’s idea that electrons travel around the
nucleus in specific, allowed orbits in which the e- has specific energy and is a specific distance from the nucleus
6. Understand how the Heisenberg uncertainty principle led to the quantum model of the atom
7. Know how the quantum model of the atom is different from Bohr’s model of the atom
8. Understand the 4 quantum numbers:
a. The principle quantum number (n) = main energy level; indicates the energy of an electron and the
distance from the nucleus; n2 = total number of orbitals in that main energy level; 2n2 = total number of
electrons in that main energy level
b. The angular momentum quantum number (l) = the number of sublevels in the main energy level and the
shapes of the orbitals in each sublevel; s=sphere; p=dumbbell; d=double dumbbell; f=complex
c. The magnetic quantum number (m) = the number of orbitals in each sublevel (s=1; p=3; d=5; f=7)
d. The spin quantum number = +½ or –½; indicates the direction in which the electron is spinning; two
electrons in the same orbital must have opposite spins
9. Know the Aufbau principle, the Pauli exclusion principle, and Hund’s rule
10. Memorize the orbital filling diagram
11. Know how to write orbital notations, electron configurations, and noble gas notations
12. Know how to identify an element given any of the above electron notations
Study Guide: Chapter 4 - the Arrangement of Electrons in Atoms
1. Understand the relationship between a light wave’s frequency and wavelength; Know how to calculate
wavelength given frequency and frequency given wavelength (MEMORIZE FORMULA) – work practice problems
2. Understand the relationship between energy of light and its frequency; Know how to calculate the energy given
frequency, and the frequency given energy (MEMORIZE FORMULA; Planck’s constant will be given) – work a few
practice problems
3. Know what a line emission spectrum is and how it’s produced
4. Understand that an electron must gain energy in order to move (temporarily) to a higher energy level – excited
state; it emits the same amount of energy (in the form of light) when it falls back to its ground state
5. Understand how the line emission spectrum of hydrogen led to Bohr’s idea that electrons travel around the
nucleus in specific, allowed orbits in which the e- has specific energy and is a specific distance from the nucleus
6. Understand how the Heisenberg uncertainty principle led to the quantum model of the atom
7. Know how the quantum model of the atom is different from Bohr’s model of the atom
8. Understand the 4 quantum numbers:
a. The principle quantum number (n) = main energy level; indicates the energy of an electron and the
distance from the nucleus; n2 = total number of orbitals in that main energy level; 2n2 = total number of
electrons in that main energy level
b. The angular momentum quantum number (l) = the number of sublevels in the main energy level and the
shapes of the orbitals in each sublevel; s=sphere; p=dumbbell; d=double dumbbell; f=complex
c. The magnetic quantum number (m) = the number of orbitals in each sublevel (s=1; p=3; d=5; f=7)
d. The spin quantum number = +½ or –½; indicates the direction in which the electron is spinning; two
electrons in the same orbital must have opposite spins
9. Know the Aufbau principle, the Pauli exclusion principle, and Hund’s rule
10. Memorize the orbital filling diagram
11. Know how to write orbital notations, electron configurations, and noble gas notations
12. Know how to identify an element given any of the above electron notations