NAME __________________________________ PERIOD _____ CE CHAPTER 3 TEST REVIEW #2
3.1 Periodic Law & Table
1. List 2 elements that are in the same period as Antimony, Sb.
2. Which element is the 1st one in group VIIA (17)?
3. What is the symbol of the element in period 7 group IA (1)?
4. Gold, Au, belongs to what period?
5. If the formula for phosphoric acid is H3PO4, what would be the expected formula for the compound
containing hydrogen, oxygen and arsenic (As)?
3.2 Electron Arrangements in Atoms
6. What is the maximum number of electrons in the s subshell? The p subshell? The d subshell? The f subshell?
7. How many orbitals are in an s subshell? A p subshell? A d subshell? An f subshell?
8. List the subshells in order of increasing energy. 4d, 5d, 5f, 5p, 5s
9. What makes an electron change energy levels (both moving to higher level & to lower energy level)?
10.
What is the maximum number of electrons that can occupy a 4p orbital (NOT subshell)?
11. What is the maximum number of electrons
12. How many electrons are in the outer shell of the
that can occupy each shell?
following elements?
Shell
Maximum number of electrons
Element Element Name
# of electrons in
the outer shell
1
#13
2
#2
3
#34
4
5
3.3 The Shell Model & Chemical Properties
13. List 2 elements that have similar properties of oxygen, O.
14. What is the shell number for the outer electrons in Iodine, I?
15. In the Alkali Metal family, which metal Li, Na, K or Rb will react fastest? Why?
3.4 Electron Configurations
16. Which is a transition element? Iron (Fe) Strontium (Sr) Cerium (Ce)
17. Describe the Aufbau Principle.
18. Describe the Pauli Principle
19. Describe Hund’s Rule.
20. Do elements in the same group or the same period have the same number of electrons in the outermost
shell? Give an example.
21. Write the electron configuration, expanded and noble gas notation for: a. Cl b. Ba c. Cu
22. Which of the following elements contains a total of 6 “s” electrons? (Circle all that work) Sc Cl Na Cs Mg
23. How many unpaired electrons are in each of the following? A. Si
b. Cl
c. Ba
3.5 Another Look at the Periodic Table
24. What type of electron is the distinguishing electron in Be? s p d f
25. List an element that has the distinguishing electron configuration 3d6?
26. Which groups are representative elements?
27. On the periodic table describe where the non-metals are located?
28. List at least 2 elements that are gases at room temperature.
29. Where are the Noble Gases located on the periodic table?
30. Where are the inner-transition elements located on the periodic table?
31. Why is the periodic table arranged with elements in specific families?
32. Define valence shell.
3.6 Property Trends within the Periodic Table
33. Put the following elements in order of increasing atomic radii: Cl, I, Na, Rb
34. Why does the atomic radii decrease across a period (left to right)?
35. The melting point of oxygen is _____________________ than selenium.
36. Elements from which group number would require the least amount of energy in the following reaction?
E → E+ + e- (E stands for the element)
37. How many unpaired electrons are in Carbon?
38. How is the modern day periodic table organized?
ANSWERS: 1. Rubidium, Strontium, Yttrium, zirconium, niobium, molybdenum, technetium, ruthenium, rhodium,
palladium, silver, cadmium, indium, tin, tellurium, iodine, xenon 2. Fluorine 3. Fr 4. 6 5. H3AsO4 6. 2, 6, 10, 14
7. 1, 3, 5, 7
8. 5s, 4d, 5p, 5d, 5f
9. Electrons absorb energy to move to higher energy levels and they release
energy to move to lower energy levels. 10. 2 11. 2, 8, 18, 32, 32
12. Aluminum, 3; helium, 2; selenium, 6
13. Sulfur, selenium or tellurium
14. 5
15. Rubidium will react the fastest because it has more energy levels
which makes the outer electrons further away from the protons than in the other elements 16. Iron
17. Electrons fill the lowest energy levels first
18. Only electrons spinning in opposite directions can fill the same
orbital.
19. Electrons will not occupy orbitals of the same energy until there is an electron in each orbital of that
energy.
20. Same group, example Lithium & potassium both have 1 valence electron
21. a. 1s22s22p63s23p5 ;
2
5
2 2
6 2
6
2
10
6 2
10
6
2
2
2 2
6 2
6 2
[Ne] 3s 3p
21b. 1s 2s 2p 3s 3p 4s 3d 4p 5s 4d 5p 6s [Xe]6s
21c. 1s 2s 2p 3s 3p 4s 3d9 (really one of the
electrons in the 4s orbital gets bumped up to fill in the d orbital so it’s really 1s22s22p63s23p64s13d10) [Ar]4s23d9
22. Mg, Cl
23. A. Si: 2 B. Cl: 1 C. Ba: 0
24. S 25. Fe 26. 1,2,13-17 27. Right hand side above the
staircase
28. N, O, F, Cl, He, Ne, Ar, Kr, Xe, Rn 29. Group 18 or 8A
30. F-block or the two rows that are
underneath the table. 31. Families of elements have similar properties because they have the same number of
valence electrons. 32. Valence shell is the outer electron energy level 33. Cl, Na, I, Rb 34. The atomic radus
decreases across a period because more protons and electrons are being added to the atom which causes a stronger
attraction and pulls in the energy levels tighter that having fewer energy levels. 35. Lower 36. Alkali metals
(group 1)-this is showing an electron being removed from the element. 37. 2
38. Today the periodic table is
organized according to increasing atomic number (# of protons).