Download Practice Test 2

Practice Test: Unit 2
Provided:
Electromagnetic
Spectrum
Periodic Table
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Practice?
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Memorized:
Frequency/ Wavelength & Energy/ Frequency Calculations
Speed of Light, Planck’s Constant
Quantum Numbers & Periodic Table
Filling Order for Subshell Configurations
Exceptions to filling order
Metric Prefixes & Meanings…particularly nanometers
Weighted Atomic Mass Formula
1. Which of the following is the correct outer electron configuration for zinc?
A) 5s24d10
B) 2s21d10
C) 4s21d10
D) 4s23d10
Coverage:
Unit 2, Lessons 1-6
Unit 3, Lesson 1
Lecture Demonstrations:
Colored Fire
Emission Spectrum Tubes
Flame Test Lab
Dimensional Analysis (not a
lot, but some equations require)
E) 3s23d10
2. Which of the following atoms has the ground state electron configuration of 1s22s22p63s23p64s13d10?
A) Cr
B) Zn
C) Ag
D) Cu
E) none
3. Which of the following sets of four quantum numbers n, l, ml, ms, describes one of the outermost
electrons in a ground-state As atom?
A) 4, 1, 2, +1/2
B) 4, 1, 1, +1/2
C) 4, 2, 1, -1/2
D) 4, 0, 1, -1/2
E) 3, 1, 1, +1/2
4. Which of the following is a possible excited electron configuration for sodium?
A) 1s22s22p63s2
B) 1s22s22p63s1
2 2
5 2
C) 1s 2s 2p 3s
D) 1s22s22p63s13p2
E) none
5. What is the maximum number of electrons that can be in the energy level n= 4?
A) 8
B) 18
C) 32
D) 50
E) 100
6. Which of the following has a completely filled set of d orbitals in its neutral atoms?
A) potassium
B) iron
C) phosphorus
D) bromine
E) none
7. Elements in a given period have the same
A) atomic weight
C) maximum principal quantum number
B) maximum azimuthal quantum number
D) valence electron structure
E) atomic number
8. If the principal quantum number of a shell is equal to 2, what shapes of orbitals will be present?
A) spheres, only
B) spheres and dumbbells
C) spheres, dumbbells, clovers
D) spheres, dumbbells, clovers, and further complicated shapes
E) dumbbells, only
9. When going from 1s22s22p63s23p64s1 to 1s22s22p63s23p54s2, an electron would
A) absorb energy
B) emit energy
C) relax to the ground state
D) bind to another atom
E) undergo no change in energy
10. The properties of light can best be explained by assuming that light is composed of:
I. Particles
II. Waves
III. Atoms
A)
I only
B) II only
C) I and II
D) II and III
11. An electron with the quantum numbers n=5 and l=3 would be in which of the following?
A) 5d
B) 3d
C) 5f
D) 3f
E) I, II, and III
E) none
12. Which of the following combinations represents an element with a net charge of +1 and a mass number of 75?
A) 35 neutrons, 35 protons, 34 electrons
B) 40 neutrons, 40 protons, 39 electrons
C) 40 neutrons, 35 protons, 34 electrons
D) 37 neutrons, 38 protons, 39 electrons
E) 40 neutrons, 35 protons, 35 electrons
13. Two electrons with the same n, l, and ml values
A) must be in different atoms
B) are in different orbitals of the same subshell
C) are indistinguishable from each other
D) could never occur
E) are in the same orbital of the same subshell with opposite spins
14. What is the mass number of an atom of nitrogen that has 8 neutrons?
A) 8
B) 7
C) 14
D) 15
E) none
15. Atoms of which two elements have the same number of unpaired electrons?
A) Na and S
B) Si and S
C) Mg and S
D) Al and S
16. In a single atom, how many electrons can be held in the second shell?
A) 6
B) 8
C) 18
D) 32
E) none
E) none
17. Which of the following sets of four quantum numbers n, l, ml, ms, describes one of the outermost valence electrons in
a ground-state As atom?
A) 4, 1, 2, +1/2
C) 4, 1, -1, +1/2
B) 4, 2, 1, -1/2
D) 4, 0, 1, -1/2
E) none
18. What is the mass number of an atom of rubidium, Rb, that has 48 neutrons?
A) 112
B) 96
C) 79
D) 85
E) none
19. In a far galaxy, the average atomic mass of an oxygen atom is 16.5 amu. Based upon the assumption of the existence
of only two oxygen isotopes 16O and 18O (with atomic masses corresponding to their mass numbers), the natural
abundance of the 18O isotope is
A) 15%
C) 75%
B) 25%
D) 85%
E) none
20. Which conclusion was a direct result of the gold foil experiment?
A) An atom is mostly empty space with a dense, positively charged nucleus.
B) An atom is composed of at least three types of subatomic particles.
C) An electron has a positive charge and is located inside the nucleus.
D) An electron has properties of both waves and particles.
E) none
21. Which pair of elements have chemical properties that are the most similar?
A) Be and B
B) Al and Ga
C) Co and Cu
22. Which one of the following is a transition element?
A) F
B) Fe
23. The Periodic Table is arranged in order of
A) atomic mass
B) the alphabet
C) Ge
D) As
C) atomic number
24. Which element is a solid at room temperature and conducts electricity?
A) mercury
B) iodine
C) sulfur
D) discovery
D) none
25. Magnesium and calcium have similar chemical properties they have the same total number of
A) electron shells
B) neutrons
C) valence electrons
D) protons
26. The noble gases are
A) highly reactive with many elements
C) nonreactive with many elements
E) highly acidic in water
D) F and Ne
B) He, Li, Ar, Na, Kr, Xe, and Rn
D) He, Ne, Ar, Br, Kr, and Rn
E) none
27. How many miles is 1.42 lightyears? (A lightyear is defined as the distance light travels in 365 days). Hint:
You will need to use the speed of light in your calculation.
28. Every three times I clean my bedroom, my mother makes me an apple pie. I cleaned my bedroom 9 times. How many
apple pies does she owe me?
29. A High School senior was applying to college and wondered how many applications she needed to send. Her
counselor explained that with the excellent grade she received in chemistry she would probably be accepted to one
school out of every three to which she applied. She immediately realized that for each application she would have to
write 3 essays, and each essay would require 2 hours work. Of course writing essays is no simple matter. For each
hour of serious essay writing, she would need to expend 500 calories which she could derive from her mother's apple
pies [1 pie = 1000 calories]. How many times would she have to clean her room in order to gain acceptance to 10
colleges? (You’ll need to refer back to #23)
30. A type of radiation produces a frequency of 5.6 x 10-14 Hz. What is the wavelength in nanometers?
31. It takes 4.56 x 10-24J of energy to emit electrons from a certain type of metal. If the 5.67 x 10-12J is applied
to the metal, how many electrons are emitted. Calculate the wavelength in nanometers.
32. An x ray is used at the dentist office to gather more information about a patient’s dental health. Using the
electromagnetic spectrum, determine the energy given off by an x-ray.
33. A certain type of radiation has a frequency of 4.28 x 10-24s-1. Calculate its wavelength and energy.
34. A new element is discovered to have three isotopes. Isotope #1 has a mass of 45.2 amu and an abundance
of 35.0%; Isotope #2 has a mass of 40.0 amu and an abundance of 55.0%; Isotope #3 has a mass of 44.9
amu and an abundance of 10.0%. Calculate the average atomic mass of the element.
35. Hydrogen comes in two stable isotopes, Hydrogen-1 and Hydrogen-2. The molar mass of Hydrogen-1 is 1.007825
g/mol. The molar mass of Hydrogen-2 is 2.014108 g/mol. Determine the percent abundance of each isotope.
36. A compound containing sodium is placed in a flame and yellow/orange color is produced. Explain how
and why this occurs.
37. Electromagnetic radiation can be discussed in terms of both particles and waves. Explain the experimental
verification for each of these views.
38. Summarize the development of the atomic model, including the scientists involved, their experiments, and
resulting atomic models. Be brief, but do not leave out the important details!
39. Explain Hund’s Rule. In your explanation, provide an example of a violation of Hund’s Rule.
40. Copper and Chromium have electron configurations that are exceptions to the Aufbau rule. Write each
element’s electron configuration and explain what is exceptional about them.
41. Consider O and Fe.
a. Write the ground state electronic configuration for each atom in Bohr configuration, condensed subshell
configuration, and orbital box notation.
b. Determine the number of unpaired electrons present for each atom.
42. Define the Aufbau Rule and the Pauli Exclusion Principle. Show examples of violations of the rules.
43. Write the four quantum numbers associated with each of the last electron of each of the following elements:
As
W
Li
U
O
Rn
V
44. What is the maximum number of electrons that can be described by the following quantum numbers?
a. n=3
b. ml= -1, ms = -1/2
c. n=4, l=2
d. l= 2, ml = 0
45. Write the electron configurations of the following elements in Bohr notation, condensed subshell
configuration, and condensed orbital box notation.
a. phosphorus
b. nickel
c. osmium
d. radon
46. Write the number of valence electrons for an element that belongs to the following group (8 points):
A. This group contains gases, a liquid, and solids. Elements are reactive due to their high electron affinity. ____
B. This group contains all metals that can form many different charged ions. ______
C. This group of gases was to be considered inert, until it was determined that some elements form bonds. _____
D. This group contains metals that react violently with water. ______
47. Consider the Periodic Table below.
A. Label the alkali metals, the transition metals, the halogens, and the noble gases. (4 points)
B. Draw arrows to indicate the trends for Ionization Energy across a period and within a group. (4 points)
C. Star the groups that do not follow the Ionization Energy trend. (2 points)