Name ______

AP Chemistry

Date______Block ______

Periodic Review

1. Give full and abbreviated (noble gas core) electronic configurations for the following.

a)  Br FULL ______

NOBLE GAS CORE ______

b)  Cr FULL ______

NOBLE GAS CORE ______

c)  Fe FULL ______

NOBLE GAS CORE ______

d)  S2- FULL ______

NOBLE GAS CORE ______

2. For each of the following sets of orbitals, indicate which orbital is higher in energy.

a)  1s, 2s ______

b)  2p, 3p ______

c)  4s, 3d ______

d)  3px, 3py, 3pz ______

3. Indicate the block (s, p or d) in which each of the following elements found.

BLOCK

a)  Sc ______

b)  P ______

c)  Fr ______

d)  Ni ______

e)  As ______

4. An atom has two electrons with principal quantum number (n) = 1, eight electrons with principal quantum number (n) = 2 and seven electrons with principal quantum number (n) = 3. From these data, supply the following values (if insufficient information is given, say so)

a) the mass number. ______

b) the atomic number. ______

c) the electron configuration. ______

5. Identify the element from the electron configurations of atoms shown below.

a) [Ne] 3s2 3p2 ______

b) [Ar] 4s2 3d7 ______

c) [Xe] 6s2 ______

6. State which atom or ion is represented by the following sets of atomic numbers and electronic configurations.

Atomic # Electronic Configuration

a) 8 1s2 2s2 2p4 ______

b) 11 1s2 2s2 2p6 ______

c) 14 1s2 2s2 2p6 3s2 3p2 ______

d) 22 1s2 2s2 2p6 3s2 3p6 3d2 ______

8. Consider the element Scandium, atomic # 21.

a) If the electronic configuration of the element were constructed into which orbital (and into which shell) would the final electron be placed? ______

10. Identify the element that is composed of atoms whose last electron;

a) enters and fills the 4s sub-shell ______

b) enters but does not fill the 4s sub-shell ______

c) is the first to enter the 2p sub-shell ______

d) is the next to the last to enter the 4p sub-shell ______

e) is the second to enter the 4d sub-shell ______

11. Write the full electronic configuration for argon.

______

12. Identify two positive and two negative ions that are isoelectronic (same number of electrons) with argon.

Two Positive ions ______

Two Negative ions ______

13. Using orbital diagrams complete the electronic configurations of the following elements.

4s 3d 4p Element

V

4s 3d 4p Element

Ar

4s 3d 4p Element

Zn

14. State the number of unpaired electrons in each of the electronic configurations in question 13.

# of unpaired electrons

V ______

Ar ______

Zn ______

15. Write three possible sets of quantum numbers for the highest energy electrons in the aluminum atom.

n / l / ml / ms

Electron # 11

Electron # 12
Electron # 13

16. Calculate the wavelength of the energy released when an electron in a hydrogen atom falls back to the first shell after being promoted to the fifth shell.

h = 6.626 x 10-34 J sec, c = 3.00 x 108 m sec-1

17. How would you expect the magnitude of the energy released in a similar process (5th shell è 1st shell transition) in question 16 to vary for a He+ ion? Explain your answer.

______

______

______

18. Which atomic theory is violated by the following sets of quantum numbers representing beryllium’s outer shell electrons? Explain your answer.

n / l / ml / ms
2 / 0 / 0 / + ½
2 / 0 / 0 / + ½

______

______

______

______

19. Identify the following atoms as either paramagnetic or diamagnetic.

Ga ______

Cr ______

Ni ______

1.  Complete the table. (5)

Element / Predicted charge on its ion
Rb
Cs
Ga
At
Se

2.  Define Ionization Energy. (2)

______

______

3.  Using the metal magnesium as an example, write two separate equations to show the first and second ionization energy of magnesium. (Remember state symbols are important as they from part of the definition). (4)

First Ionization ______

Second Ionization ______

4.  Which of the following elements (one from each pair) would you expect to have the highest first ionization energy? Explain your answers. (4)

Ca and Be ______

______

Na and Ar ______

______

5.  Consider the table of the first four ionization energies for element A shown below.

Ionization Energy in kJ/mol / 1st / 2nd / 3rd / 4th
578 / 1817 / 2745 / 11580

(i)  In which group does A appear on the periodic table? (1) ______

(ii)  Predict the formula of the compound A forms with chlorine. (1) ______

(iii)  What is the minimum number of electrons that A must have? (1) ______

6.  Are there any atoms for which the second ionization energy is greater than the first? Explain your answer. (2)

______

______

______

7.  Define electron affinity. (2)

______

______

8.  Write an equation to summarize the process of second electron affinity of oxygen. (2)

______

9.  Consider the table of ionization energies for element X shown below.

Ionization Energy in kJ/mol / 1st / 2nd / 3rd / 4th / 5th / 6th
737 / 1450 / 7732 / 10540 / 13360 / 17995

(i)  In which group will X be found? (1) ______

(ii)  Explain your answer to 9(i). (2)

______

______

______

(iii)  Predict the formula of X’s bromide. (1) ______

10.  Explain carefully why elements in the same group react in similar ways? (1)

______

______

______

11.  Explain carefully, the factor, when moving up and down groups I & II, that determines the pattern of reactivity that is observed? (2)

______

______

______

12. From the data below predict the boiling point of Radon. (1) ______

Noble Gas / Boiling Point/K
Helium / 4.21
Neon / 27.1
Argon / 87.3
Krypton / 120
Xenon / 165

13. Arrange the following atoms into order of increasing first ionization energy. Sr, Cs, S, F and As. (1)

LOWEST HIGHEST

______

14. What do you understand by the term, shielding? (2)

______

______

______

______