1. Electrons & the Periodic Table Review
Chapter 5 – 6.3

2. Given on the Test!!!!!
c = 3.00 x 108 m/s
h = x Js
c = f E = hf

3. Find the energy of an infrared photon whose frequency is 2.0  1012 Hz.
f = 2.0 x /s
h = x Js
E = ?
E = hf
E = (6.626 x Js)(2.0 x /s)
E = 1.3 x J

4. 2. What is the wavelength of a red light wave whose frequency is 4
2. What is the wavelength of a red light wave whose frequency is 4.3  1014 Hz?
c = f   = c/f
7.0 x 10-7 m
3. Calculate the frequency of an X-ray wave that has a wavelength of 9.2 nm.
 = 9.2 x 10-9 m
c = f  f = c/ 
3.3 x 1016 Hz

5. 4. What is the energy of a cosmic ray photon whose wavelength is 2
4. What is the energy of a cosmic ray photon whose wavelength is 2.0 pm?
= 2.0 x m
9.9 X J
5. Find the frequency of a microwave that carries 3.4  J of energy.
E = hf  f = E/h
5.1 x 108 Hz

6. 6. A packet of light energy that carries a quantum of energy.
7. The state when all electrons of an atom are in the lowest possible energy levels.
8. When an electron jumps up to a higher energy level, the atom is in its ___.
9. The scientist who applied Einstein’s particle-wave theory to electrons.
10. The theory that it is impossible to know both the position and speed of an electron simultaneously.
11. The theory that no two electrons in an atom can share the same 4 quantum numbers.
photon
ground state
excited state
Louis de Broglie
Heisenberg uncertainty principle
Pauli exclusion principle

7. 12. The theory that electrons fill the lowest energy orbitals first.
13. The theory that, within a sublevel, electrons prefer to occupy their own orbital.
14. A term describing the outermost electrons in an atom.
15. A positively charged ion is called a(n) ______. A negatively charged ion is called a(n) _______.
16. The lower, left-hand section of the periodic table that includes most of the elements.
17. The upper right-hand section of the periodic table.
Aufbau principle
Hund’s rule
Valence electrons
cation
anion
metals
non-metals

8. 18. The section of the periodic table that includes only the elements in the d-block.
19. The section of the periodic table that includes both the s-block and the p-block.
20. A three-dimensional region in space where an electron is likely to exist.
21. The process by which the core electrons partially block the attraction between the nucleus and the valence electrons.
22. What is the basis for exceptions to the aufbau diagram?
Transition metals
Representative elements
Energy level; sublevel; orbital
shielding
Full and ½ full sublevels are stable (i.e. Cr)

9. One electron in each orbital
33. According to the Heisenberg uncertainty principle, if the position of a moving particle is known, what other quantity CANNOT be known?
34. How many unpaired electrons are in a sulfur atom (Z = 16)?
35. The principal quantum number indicates what property of an electron?
36. What is the maximum number of electrons in the second principal energy level?
37.If three electrons are available to fill three empty 2p atomic orbitals, how will the electrons be distributed?
38. When an electron moves from a lower to a higher energy level, the electron _____.
speed 2
Energy level 8
2n2 & n2
One electron in each orbital
Absorbs energy

10. 39. According to the aufbau principle, electrons enter orbitals of ___ first.
40. What is the maximum number of “f” orbitals in any single energy level of an atom?
41. What is the charge of a cation?
42. Which of these elements has the lowest electronegativity value: a) cesium, or b) calcium?
43.What element in the second period has the largest atomic radius?
43. What is the element with the highest electronegativity value: a) calcium, or b) fluorine?
Lowest energy 7
positive
cesium
Li - Lithium
F - Fluorine

11. 44. Of the following, which one has the smallest first ionization energy: a) aluminum, or b) silicon?
45. Which of the following elements has the smallest ionic radius: a) Li, or b) K
Al - Aluminum
Li - Lithium