Download CHAPTER 6 PRACTICE TEST Name Relevant Equations E = hν E

CHAPTER 6 PRACTICE TEST
Name
Relevant Equations
E = h






E = energy
speed of light, c = 3.0 x 108 m s-1
c = 






 = frequency
Planck’s constant, h = 6.63 x 10-34 J s
 = wavelength
Avogadro’s number = 6.02 x 1023 mol-1
–2.18 x 10-18
En = ------------------- joule
n2
n = principal quantum number
MULTIPLE CHOICE QUESTIONS (NO CALCULATOR IS ALLOWED)
Questions 1-4 refer to atoms of the following elements:
(A) lithium
(B) rubidium
(C) aluminum
(D) fluorine
(E) iodine
1.
Has the largest atomic radius.
2.
Has exactly one valence electron located in a p sub-shell.
3.
Is a grey solid at room temperature, but undergoes sublimation to produce a violet gas
4.
Forms an oxide that has the formula X2O3
Questions 5-8 refer to the following electron configurations
(A)
(B)
(C)
(D)
(E)
1s22s22p3
1s22s22p4
1s22s22p6
1s22s22p53s1
1s22s22p63s23p1
5.
Represents the ground state electron configuration of a halide anion
6.
Represents an atom that contains exactly three valence electrons
7.
Represents an electron configuration for an atom in an excited state
8.
Represents an element that can have a variety of oxidation states in its compounds, including -3 and +3
9.
An energy value of 6.63 x 10-19 J is needed to break a chemical bond. The wavelength that is
associated with this energy is approximately
(A) 150 nm
(B) 300 nm
(C) 450 nm
(D) 600 nm
(E) 750 nm
10. Which of the following represents the ground state electron configuration for the Mn2+ ion?
(A) [Ar] 3d5
(B) [Ar] 3d44s1
(C) [Ar] 3d34s2
(D) [Ar] 3d54s2
(E) [Ar] 3d74s2
11. Which of the following represents an impossible set of quantum numbers?
(A)
(B)
(C)
(D)
(E)
n
l
ml
ms
1
2
3
4
5
1
1
2
2
3
0
-1
1
2
0
+½
–½
+½
–½
+½
12. As the atomic number of Group 14 elements increases, which of the following properties tend to
decrease?
(A)
(B)
(C)
(D)
(E)
density
atomic radius
1st ionization energy
metallic character
oxidation number
13. Based on the chemical properties of the elements, which if the following reactions should not occur?
(A) I2 + 2 KF  2 KI + F2
(B) Cl2 + 2 NaI  2 NaCl + I2
(C) 2 K + 2 H2O  2 KOH + H2
(D) 2 Al + 3 Br2  2 AlBr3
(E) 4 Li + O2  2 Li2O
14. Which of the following series is listed in order of decreasing radius?
(A)
(B)
(C)
(D)
(E)
Sr, Ba, Ba2+
Na+, Na, Mg
Cl–, Cl, Br
Si, S, S2K, Ca, Ca2+
15. Which of the following statements concerning the Group 2 elements is true?
(A)
(B)
(C)
(D)
(E)
They tend to form molecular compounds in which electrons are shared with other atoms.
Reactivity of these elements tends to decrease as atomic number increases.
These elements tend to be more reactive than the Group 1 elements.
Their 1st ionization energy values are higher than those of the Group 1 elements.
Their atomic radii are larger than those of the Group 1 elements.
FREE RESPONSE QUESTIONS (NO CALCULATOR IS ALLOWED)
1.
The longest wavelength of light with enough energy to break the Br–Br bond in Br2(g) is 620 nm.
(a) Calculate the frequency, in s-1, of the light
(b) Calculate the energy, in J, of a photon of the light.
(c) Calculate the minimum energy, in kJ mol-1, of the Br–Br bond.
(d) Should radiation with a wavelength of 1200 nm have enough energy to break the Br–Br bond? Justify your
answer by discussing the relationship between wavelength and energy.
2.
A certain line in the spectrum of atomic hydrogen is associated with the electronic transition in
the H atom from the first energy level (n = 1) to the sixth energy level (n = 6)
(a) Indicate whether the H atom emits energy or whether it absorbs energy during the transition. Justify your
answer.
2. (continued)
(b) Calculate the energy change, in J, associated with this transition.
(c) Calculate the wavelength, in nm, of the radiation associated with this transition.
(d) Would the radiation associated with the transition from n = 1 to n = 2 have a longer wavelength or a shorter
wavelength than the radiation associated with the transition from n = 1 to n = 6? Justify your answer with a
calculation.
3.
Use the principles of atomic structure to explain each of the following. You must discuss the electron
configurations of both substances that are being compared. If you merely state a general trend without justifying
your answer, you will not receive credit.
(a) The atomic radius of boron is smaller than the atomic radius of aluminum.
3. (continued)
(b) The 1st ionization energy of Na is less than the 1st ionization energy of Mg.
(c) The 2nd ionization energy of Na is greater than the 2nd ionization energy of Mg.
(d) Fluorine has a larger electronegativity value than bromine.
(e) The ionic radius of Ca2+ is smaller than the ionic radius of S2-.
(f)
The 1st ionization energy of B is slightly less than the 1st ionization energy of Be.