Name ________________________________________________ Pd _________ Date ______
AP Chemistry Review Questions
Use these answers for questions 1 - 3.
(A) O
(B) La
(C) Rb
(D) Mg
(E) N
1. What is the most electronegative element of the above?
2. Which element exhibits the greatest number of different oxidation states?
3. Which of the elements above has the smallest ionic radius for its most commonly found ion?
Use these answers for questions 4 - 7.
(A) 1s2 2s22p5 3s2 3p5
(B) 1s2 2s22p6 3s23p6
(C) 1s2 2s22p62d10 3s23p6
(D) 1s2 2s22p6 3s23p63d5
(E) 1s2 2s22p6 3s23p63d3 4s2
4. An impossible electronic configuration
5. The ground-state configuration for the atoms of a transition element
6. The ground-state configuration of a negative ion of a halogen
7. The ground-state configuration of a common ion of an alkaline earth element
8. Pi bonding occurs in each of the following species EXCEPT
(A) CO2
(B) C2H4
(C) CN¯
(D) C6H6
(E) CH4
9. All of the following statements concerning the characteristics of the halogens are true
EXCEPT:
(A) The first ionization energies (potentials) decrease as the atomic numbers of the halogens
increase.
(B) Fluorine is the best oxidizing agent.
(C) Fluorine atoms have the smallest radii.
(D) Iodine liberates free bromine from a solution of bromide ion.
(E) Fluorine is the most electronegative of the halogens.
Question 10-13 refer to atoms for which the
occupied atomic orbitals shown to the right.
10. Represents an atom that is chemically unreactive
11. Represents an atom in an excited state
12. Represents an atom that has four valence
electrons.
13. Represents an atom of a transition metal.
14. In the periodic table, as the atomic number increases from 11 to 17, what happens to the atomic
radius?
(A) It remains constant.
(B) It increases only.
(C) It increases, then decreases.
(D) It decreases only.
(E) It decreases, then increases.
15. The ionization energies for element X are listed in the table below.
On the basis of the data, element X is most likely to be
Ionization Energies for element X (kJ mol-1)
(A) Na
First
Second Third
Fourth Five
(B) Mg
580
1815
2740
11600 14800
(C) AI
(D) Si
(E) P
16. Which of the following molecules has the shortest bond length?
(A) N2
(B) O2
(C) Cl2
(D) Br2
(E) I2
17. For which of the following molecules are resonance structures necessary to describe the
bonding satisfactorily?
(A) H2S
(B) SO2
(C) CO2
(D) OF2
(E) PF3
18. When writing electron configurations, which sublevel comes before the others?
a. 2s
b. 2p
c. 3p
d. 4p
e. 4s
19. How many electrons can the d sublevel hold?
a. 2
b. 6
c. 2n2
d. 10
e. 3
20. The Lewis dot structure of which of the following molecules shows only one unshared pair
of valence electrons?
(A) Cl2
(B) N2
(C) NH3
(D) CCl4
(E) H2O2
21. The electron-dot structure (Lewis structure) for which of the following molecules would have
two unshared pairs of electrons on the central atom?
(A) H2S
(B) NH3
(C) CH4
(D) HCN
(E) CO2
22. When writing that an electron is in 3p, the 3 stands for
a. the level
b. the sublevel
c. the orbital
d. the electron spin
23. Molecules that have 120° bond angles include which of the following?
I. BCl3
II. CHCl3
(A) I only
(B) III only
(C) I and II only
(D) II and III only
(E) I, II, and III
III. NCl3
24. Which of the following molecules is an exception to the octet rule?
a. PF3
b. CCl4
c. CO2
d. SF6
e. H2O
25. How many valence electrons are in PO43-?
a. 28
b. 64
e. 2
c. 32
d. 30
26. Write the electron configuration for neon.
27. State the charge for the following elements. (Make sure that you include both a number and
a sign.)
______________A.
oxygen
______________B.
sodium
______________C.
magnesium
______________D.
aluminum
______________E.
fluorine
28. Using electron configurations and the periodic table, write a paragraph to explain why
nitrogen has an oxidation number of 3-.
29. What is the difference between ionic, nonpolar covalent, and polar covalent bonds?
30. What type of bonding would occur between:
A. Sulfur (S) and Bromine (Br) ________________________
B. Sodium (Na) and Chlorine (Cl) _____________________
31. Explain the relationship between bond energy and number of bonds.
32. Explain the relationship between bond length and number of bonds.
33. Draw the resonance structures for O3.
34. An FM radio station broadcasts at 99.7 MHz. Calculate the wavelength of the
corresponding radio waves.
35. A photon of ultraviolet light possesses enough energy to mutate a strand of human DNA.
For this reason, it is used to sterilize chemical goggles. What is the energy of a single photon and
a mole of UV photons that have a wavelength of 250 nm?
35 ½. Match the scientist with his important contribution.
____Mendeleev
A. Cannot know both location and speed of electron at same time
____Einstein
B. Equation gives probability distribution of an electron
____De Broglie
C. Objects radiate energy in packets called quanta
____Schrodinger
D. Model of atom works only for hydrogen
____Bohr
E. Father of modern periodic table
____Planck
F. Photons gave way to acceptance of particle behavior of light
____Heisenberg
G. Mathematically showed that matter can have wave nature
36. Draw Lewis structures that obey the octet rule for each of the following:
HCN
POCl3
SCl2
XeO3
ONF
37. Calculate the formal charge of the central atom in each structure drawn for 36. If needed,
write Lewis structures that involve minimizing the formal charge.