Name: _______________________________ Period: _______ Date: ___________________

Chemistry Practice Test Unit 03: Periodic Table and Periodic Properties

For the following electron configuration notation indicate all four quantum numbers for the two electrons indicated.

1. 2.

^{1s 2s 2p 3s 3p 3d 4s}

__ __ __ __ __ __ __ __ __ __ __ __ __ __ __

1. n = ___ l = ___ m_l = ___ m_s = ___

2. n = ___ l = ___ m_l = ___ m_s = ___

In each of the element pairs listed below, circle the one that has the largest atomic radius.

3. Calcium Titanium 4. Barium Radium 5. Mercury Arsenic

Classify the following elements as metals, nonmetals or metalloids.

6. Carbon ______________________ 7. Aluminum ______________________

8. Calcium ______________________ 9. Radon ______________________

In the following pairs of elements circle the element with the highest ionization energy.

10. Rubidium Lithium 11. Calcium Titanium 12. Mercury Arsenic

Write the proper orbital notation for each of the following.

1s 2s 2p 3s 3p 4s 3d 4p 5s

13. Copper ___________________________________________________________________________________

14. Rubidium _________________________________________________________________________________

Completion: Give the condensed electron configuration for each of the following elements.

Draw the dot diagram on the right.

Atom/Ion condensed electron configuration dot diagram

15. Se ^-2

16. Co

17. Cr

Complete problems 18, 19, and 20 by first circling one of the two elements and then give the reason(s) why for the element you circled.

18. Phosphorus, Sulfur and Oxygen are located near each other on the periodic table.

a. Phosphorus or Oxygen has a higher ionization energy because _______________________________

_____________________________________________________________________________

b. Sulfur or Oxygen has a lower ionization energy because ____________________________________

_____________________________________________________________________________

19. Sodium, Magnesium and Calcium are located near each other on the periodic table.

a. Sodium or Magnesium is a larger atom because ___________________________________________

_____________________________________________________________________________

b. Magnesium or Calcium is a smaller atom because _________________________________________

_____________________________________________________________________________

20. Tin, Antimony and Bismuth are located near each other on the periodic table.

a. Antimony or Tin has a larger electronegativity because _____________________________________

______________________________________________________________________________

b. Bismuth or Antimony has a smaller electronegativity because ________________________________

______________________________________________________________________________

Fill in the missing information for each atom or ion.

Symbol	Protons	Mass #	Charge	Electrons	Neutrons
21. 22. K				19	21
Pb		207	+2

Indicate the ion that will be formed for each atom. Some of the ions have been provided. Also provide the ion formation equation for each atom. If an ion will not be formed, write “NO ION FORMED”

23. 24. 25. Atom	Ion	Ion Formation Equation
He
Sc	Sc^+3
I

26. For the ion ¹³⁷Ba⁺², answer the following questions.

a) How many protons, electrons, and neutrons? _____ p⁺ _____ e^- _____ n⁰

4f __ __ __ __ __ __ __

6s ___

5p ___ ___ ___

4d ___ ___ ___ ___ ___

5s ___

4p ___ ___ ___

3d ___ ___ ___ ___ ___

4s ___

3p ___ ___ ___

3s ___

2p ___ ___ ___

2s ___

1s ___

b) Complete the Aufbau Diagram:

c) Write the condensed electron configuration: _________________________

d) The four quantum numbers of the last electron:

n = ___ l = ___ m_l = ___ m_s = ___

e) The dot diagram:

f) The ion formation equation:

27. The neutron-to-proton ratio for an atom of ¹⁸⁶Re is ____________________. Show your work to receive credit.

28. Write the alpha decay reaction for ²⁵¹Cf.

29. Write the beta decay reaction for ²⁵⁰Bk.

30. The half-life of ²⁵⁷Fm is 100.5 days. If you start with 32.50 g, it will be __________ days before only

8.125 g remains. Show your work to receive credit.

31. The half-life of ²⁵⁹No is 58 minutes. If you start with 354 mg of ²⁵⁹No, __________ mg will remain

after 116 minutes. Show your work to receive credit.

32. For a principle quantum number,n, equal to 6 ,what is the total electron capacity of that level? __________

33. For a principle quantum number,n, equal to 5 ,is it possible for l to be equal to 1 (Y or N)? __________

34. For a principle quantum number,n, equal to 5 ,what is largest allowed value of l? __________

35. For the quantum number, l, equal to 2 is an m_l value of -2 permitted (Y or N)? __________

36. Is the 5h orbital permitted (Y or N)? __________

37. For the quantum number, l, equal to 5, how many orbitals of that type are permitted? __________

38. What is the l quantum number for an f orbital? __________

39. For a principle quantum number, n, equal to 8, what is the total number of orbitals permitted? __________

40. What is the correct representation for an orbital which has an n value of 7 and an l value of 6? __________

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