Big Idea 1: “Atomic Theory and Structure” AP LEVEL ASSESSMENT
_____ / 15 pts
Name:_______________________________________________________
DUE: Wed 2/18
Section I Notes:
•Remember, this is practice in the end- Do NOT cheat yourself of finding out
what you are capable of doing.
• DO NOT USE A CALCULATOR. The College Board does not allow the use of
a calculator for Section I (the MC part of the exam, so it is time to start
practicing without one. You may use ONLY a periodic table and the
equations.
• While you should practice working as fast as possible, it is more important
at this point in the course that you practice without a calculator, even if it
slows you down. Look for the “easy math” − common factors and rough
estimation – do not do “long division” to try to get exact values.
Remember it is a MC test, use the answers to guide you.
Section I: Section I of this assessment contains multiple-choice questions. Clearly circle the response that best satisfies the prompt giving only one answer to each
question. The use of the College Board provided periodic table and equations and constants sheet is advised. You may use the assessment or a separate sheet of paper that you
need not attach for notes or scratch work. Use your time effectively, working as quickly as you can without losing accuracy. Do not spend too much time on any one question. Go
on to other questions and come back to the ones you have not answered if you have time. It is not expected that everyone will know the answers to all of the multiple-choice
questions. Your total score on Section I is based only on the number of questions answered correctly. Points are not deducted for incorrect answers or unanswered questions.
Use the PES spectra below to answer questions 1-4,
7. Which element will have a higher electronegativity value: chlorine or bromine? Why?
(A) Chlorine, because it has less Coulombic repulsion among its electrons
(B) Bromine, because it has more protons
(C) Chlorine, because it is smaller
(D) Bromine, because it is larger
8. Which of the following elements has its highest energy subshell completely full?
(A) Sodium
(B) Aluminum
(C) Chlorine
(D) Zinc
9. Which of the following isoelectric species has the smallest radius?
(A) S2−
(B) Cl −
(C) Ar
(D) K+
10. What is the most likely electron configuration for a sodium ion in its ground state?
(A) 1s2 2s2 2p5
(B) 1s2 2s2 2p6
(C) 1s2 2s2 2p6 3s1
(D) 1s2 2s2 2p5 3s2
1. What element does this spectra represent?
(A) Boron
(B) Nitrogen
(C) Aluminum
(D) Phosphorous
2. What peak represents the 2s subshell?
(A) The peak at 104 MJ/mol
(B) The peak at 6.84 MJ/mol
(C) The peak at 2.29 MJ/mol
(D) The peak at 1.76 MJ/mol
3. An electron from which peak would have the greatest velocity after ejection?
(A) The peak at 104 MJ/mol
(B) The peak at 4.98 MJ/mol
(C) The peak at 2.29 MJ/mol
(D) The peak at 1.76 MJ/mol
4. What element does this spectra represent?
(A) 2
(B) 3
(C) 4
(D) 5
5. Why does an ion of phosphorous, P3-, have a larger radius than a neutral atom of
phosphorous?
(A) There is a greater Coulombic attraction between attraction between the
nucleus and the electrons in P3-.
(B) The core electrons in P3- exert a weaker shielding force than those of a
neutral atom.
(C) The nuclear charge is weaker in P3- than it is in P.
(D) The electrons in P3- have a greater Coulombic repulsion than those in the
neutral atom.
6. Which neutral atom of the following elements would have the most unpaired
electrons?
(A) Titanium
(B) Manganese
(C) Nickel
(D) Zinc
11. Which of the following statements is true regarding sodium and chlorine?
(A) Sodium has a greater electronegativity and a larger first ionization energy.
(B) Sodium has a larger first ionization energy and a larger atomic radius
(C) Chlorine has a larger atomic radius and a greater electronegativity.
(D) Chlorine has greater electronegativity and a larger first ionization energy.
12. An atom of silicon in its ground state is subjected to a frequency of light that is high
enough to cause electron ejection. An electron from which subshell of silicon would
have the highest kinetic energy after ejection?
(A) 1s
(B) 2p
(C) 3p
(D) 4s
13. The wavelength range for infrared radiation is 10 – 5 m, while that of ultraviolet
radiation is 10 – 8 m. Which type of radiation has more energy, and why?
(A) Ultraviolet has more energy because it has a higher frequency.
(B) Ultraviolet has more energy because it has a longer wavelength.
(C) Infrared has more energy because it has a lower frequency.
(D) Infrared has more energy because it has a shorter wavelength.
14. Which of the following nuclei has 3 more neutron than protons?
(A) 11B
(B) 37Cl
24
(C) Mg
(D) 70Ga
15. Which of the following is true of the halogens when comparing them to other
elements in the same period?
(A) Halogens have larger atomic radii than other elements within their period.
(B) Halogens have less ionization energy than other elements within their
period.
(C) Halogens have fewer peaks on a PES than other elements within their
period.
(D) The electronegativity of halogens is higher than other elements within their
period.
Big Idea 1: “Atomic Theory and Structure” AP LEVEL ASSESSMENT
16. In general, do metals or nonmetals from the same period have higher ionization
energies? Why?
(A) Metals have higher ionization energies because they usually have more
protons than nonmetals.
(B) Nonmetals have higher ionization energies because they are larger than
metals and harder to ionize.
(C) Metals have higher ionization energies because there is less electron
shielding than there is in nonmetals.
(D) Nonmetals have higher ionization energies because they are closer to
having filled a complete energy level.
17. The ionization energies for an element are listed in the table below:
First
Second Third
Fourth
Fifth
8 eV
15 eV
80 eV
109 eV 141 eV
(A) Sodium
(B) Magnesium
(C) Aluminum
(D) Silicon
Use the following information to answer questions 18-20.
The outermost electron of an atom has a binding energy of 2.5 eV. The atom is
exposed to light of a high enough frequency to cause exactly one electron to be
ejected. The ejected electron is found to have a KE of 2.0 eV.
Section II Notes:
•Again, remember that this is practice in the end- Do NOT cheat yourself of
finding out what you are capable of doing.
• YOU MAY NOW USE A CALCULATOR in addition to a periodic table and
the equations.
DUE: Wed. 2/18
18. How much energy did photons of the incoming light contain?
(A) 0.50 eV
(B) 0.80 eV
(C) 4.5 eV
(D) 5.0 eV
19. If the wavelength of the light were to be shortened, how would that effect the kinetic
energy of the ejected electron?
(A) A shorter wavelength would increase the kinetic energy.
(B) A shorter wavelength would decrease the kinetic energy.
(C) A shorter wavelength would stop all electron emissions completely.
(D) A shorter wavelength would have no effect on the kinetic energy of the
ejected electrons.
20. If the intensity of the light were to decreased, how would that affect the kinetic
energy of the ejected electron?
(A) The decreased intensity would increase the kinetic energy.
(B) The decreased intensity would decrease the kinetic energy.
(C) The decreased intensity would stop all electron emissions completely.
(D) The decreased intensity would have no effect.
• Remember, you might be asked to use the result of a pervious part of a
problem in a later part. If you previous response is incorrect the grader
will still give you full credit for your later responses as long as they are
based on that original incorrect response.
Section II: Section II of this assessment contains free response questions. You may use separate sheets of paper or the assessment to organize your answers or for scratch
work, but you must write your answers on a separate sheet of blank paper in order for each response. Only material written in such a fashion will be scored. Examples and
equations may be included in your responses where appropriate. For calculations, clearly show the method used and the steps involved in arriving at your answers. You must
show your work to receive credit for your answer. Pay attention to significant figures. Write clearly and legibly. Cross out any errors you make; erased or crossed-out work will not
be scored. Manage your time carefully. You may proceed freely from one question to the next but your work responses must be written in order.
21. (SFR) Explain each of the following in terms of atomic and molecular structures
and/or forces.
23. (LFR) The table below gives data on four different elements, in no particular order:
Carbon, Oxygen, Phosphorus, and Chlorine
(a) The first ionization energy for magnesium is greater than the first ionization
energy for calcium.
Atomic radius
(pm)
First Ionization energy
( kJ/mol )
Element 1
170
1086.5
(c) There are three peaks of equal height in the PES of carbon, but on the PES of
oxygen the last peak has a height twice as high as all the others.
Element 2
180
1011.8
(d) The first ionization energy for aluminum is lower than the first ionization
energy for magnesium.
Element 3
175
1251.2
Element 4
152
1313.9
(b) The first and second ionization energies for calcium are comparable, but the
third ionization energy is much larger.
(a) Which element is element number 3? Justify your answer using both
properties.
(b) What is the outermost energy level that has electrons in element 2? How
many valence electrons does element 2 have?
(c) Which element would you expect to have the highest electronegativity? Why?
22. (SFR) Use your knowledge of thee periodic table of the elements to answer the
following questions.
(a) Explain the trend in electronegativity from P to S to Cl.
(b) Explain the trend in electronegativity from Cl to Br to I.
(c) Explain the trend in atomic radius from Li to Na to K.
(d) Explain the trend in atomic radius from Al to Mg to Na.
(d) How many peaks would the PES for element 4 have and what would the
relative heights of these peaks be to each other.