AP Chemistry                                                                      Unit 7

Chapter 7                                                                  Atomic Structure/Periodicity

Daily

 

1.The frequency of am electromagnetic wave is 15 X 1013 hz. Calculate its wavelength.

a. 2.0 X 10-6 m    b. 6.6 X 10-9 m          c. 5.0 X 105 m            d. 5.0 X 10-5 m

 

2.Calculate the wavelength of an electromagnetic wave with a frequency of 1.7 X 1014 hz

a. 5.9 X 106 m     . b. 0.67 X 10-15 m     c. 0.33 X 108 m         d. 1.8 X 10-6 m

 

3.An electron has an associated wavelength of 1.0 X 10-6 m. Calculate the velocity in m/s

     a. 45 m/s               b. 91.3 m/s                 c. 730 m/s                  d. 458 m/s

 

4. A particle has a velocity equal to 0.25 c and a wavelength of 1.3 X 10-16 m. Calculate the mass of the particle in kilograms. C = 3 X 108 m/s

 

     a. 1.7 X 10-20 kg  b. 6.8 X 10-26 kg  c. 8.5 X 10-19 kg   d. 3.3 X 10-28 kg

 

5. The Heisenberg Uncertainty Principle states that

a.      both position and momentum of a particle cannot be known precisely at the same time

b.      the position or momentum of a particle cannot be precisely at any time

c.       the probability of finding an electron nearby a nucleus is related to the square of its wave function

d.      the probability of finding an electron nearby an atom is at least 90%

 

6. The depiction of an “s” electron orbital as a three dimensional sphere in not completely correct because

a.      the electron orbitals are not spheres, but vary in shape from spheres to octagons

b.      the electron orbitals are not dimensional, rather they are n-dimensional depending on the probability of an electron being nearby a nucleus

c.       the depiction is correct, and is the best fit to experimental data

d.      the electron orbitals are waves, rather than spheres

 

7. How many quantum numbers are required to describe the electrons of any system?

            a. 1                  b. 3                  c. 4                  d. 2

 

8. How many distinct magnetic quantum numbers are possible if the angular momentum quantum number is 6?

            a. 13               b. 7                  c. 12                d. 3

 

9. If the principal quantum number is 3, how many values for the angular quantum number are possible?

            a. 3                  b. 4                  c. 5                  d. 2

 

10. Which of the following quantum number sets is unacceptable

            a. 1,0,0           b. 6,2,0           c. 4,3,3            d. 4,2,3

 

11. The Pauli Exclusion principle says

  1. the position and velocity of an electron can never be known precisely at the same time.
  2. No two electrons in a system can have the same quantum numbers
  3. The spin number must be –1/2 for the first electron in an orbital and +1/2 for the second one
  4. Electrons fill orbital paths by spin

 

12. The Pauli Exclusion principle is violated by one of the following electron systems.

a.      1,0,0,+1/2 and 1,0,0,+1/2

b.      5,4,-2,+1/2 and 5,4,-2,-1/2

c.       4,3,-3,+1/2 and 4,3,-3,-1/2

d.      3,2,-2,+1/2 and 3,2,-2,-1/2

 

13. We first encounter a “d” electron in what row of the periodic table

            a. 3      b. 6      c. 4      d. 2

 

14. Which one of the following elements does the following configuration describe 1s22s22p63s23p5

a. Cl                b. Ar               c. k                  d. S

 

15. Which one of the following elements has a 5s25p5 valence shell configuration?

a. Te               b. I                  c. Sb                d. As

 

16. What elements in the periodic table have the following electron configuration [Noble gas] ns2nd5

a. Fe, Ru, Os, Uno   b. Mn, Tc, Re            c. F, Cl, br, I, At       d. Co, Rh, Ir, Une

 

 

 

 

17. Place the following atoms P, kr, Mg, Li on order of increasing first ionization energy

  1. P<Kr<Mg<Li
  2. P<Mg<Kr<Li
  3. Ar<P<Mg<Li
  4. Li<Mg<P<Kr

 

18. Place the following atoms Cl, F, Na, C in order of decreasing electron affinity

  1. C>Cl>F>Na
  2. Cl>F>C>Na
  3. F>Na>Cl>C
  4. F>Cl>C>Na

 

19. At what step of ionization does astatine exhibit a sudden marked increase in its ionization energy?

a. 7th                b. 5th                c. 4th                d. 2nd

 

20. Place the following elements Br, Kr, C, Se, Te in order of increasing atomic size

  1. Br<Te<Kr<Se<C
  2. C<Kr<Br<Se<Te
  3. Te<Se<Br<Kr<C
  4. Br<Kr<C<Se<Te

 

21. Which of the following elements has the lowest reducing ability

a.       Li               b. Cs                c. Na                d. K

 

22. The visible region of the spectrum ranges from 400 to 700nm. What is the frequency range of the visible spectrum?

 

23. List the regions of the electromagnetic spectrum and the wavelength of radiation associated with each region

 

24. Calculate the frequency of blue light of wavelength 4.5 X 102 nm

 

25. Calcul;ate the wavelength of green light of frequency 5.7 X 1014 hz

 

26. Red light with a wavelength of 670.8 nm is emitted when lithium is heated in a flame

  1. What is the frequency of the radiation
  2. What is the energy of this radiation (per photon and per mole)

 

27. It takes 6.72 X 10-18 J of energy to remove an electron from an unknown atom. What is the maximum wavelength of lightthat can do this?

 

28. Calculate the energy of a photon that is emitted at a wavelength of 5.69 X 103 nm

 

29. Calculate the wavelength of a thoroughbred racehorse, which weighs 600 lbs, moving with a speed of 40 mi/hr

 

30 What are the wavelengths associated with and alpha particle (mass = 6.64 X 10-27 kg) traveling at 3.0 X 106 m/s

 

31. Calculate the wavelength of light that must be absorbed by a hydrogen atom in its ground state to reach the excited state of ΔE = +2.914 X 10-18 J

 

32. Calculate the wavelength of light emitted in the spectral transition of n=4 to n=2 in the Hydrogen atom

 

33. What region of the spectrum would you look in to find the energy associated with the spectral transition of n=4 to n=1 for Hydrogen

 

34. What region of the spectrum would you look in to find the radiation associated with the spectral transitions of n=3 to n=1 in the Helium atom

 

35. Which of the following sets of quantum numbers are allowed

  1. n=7, l=7, ml=0
  2. n=7, l=1, ml=1
  3. n=7, l=5, ml=-3
  4. n=3, l=-1, ml=0
  5. n=0, l=0, ml=0

 

36. What is the maximum number of electrons that can (theoretically) be accommodated in the following

  1. orbits of n=4
  2. 4f orbital
  3. 5g orbital

 

37. What is the electron configuration for Calcium

 

38. How does the electron configuration of barium compare to calcium

 

39. An element X combines with calcium to give the salt CaX2. The element has its highest energy electrons in the 4p level. What is X?

 

40. In which orbital would an electron have a greater likelihood of being near the nucleus 4f or 6s

 

41. Which group in the periodic table contains elements with the highest ionization energies? Which period in the periodic table contains elements with the highest ionization energies?

 

 

42. Order the following groups from smallest to largest radius (approach from isoelectric POV)

  1. Ar, Cl-, K+, S-2
  2. C, Al, F, Si
  3. Na, Mg, Ar, P
  4. I-1, Ba+2, Cs+1, Xe

 

43. Arrange the following atoms in order of increasing Z (atomic number) for the highest energy electron

            Te, In, Mg, Ga, Xe, Ca

 

44. Which of the following will have the most exothermic electron affinity? The least?

            a. Ge, Si, C                                          Cl, Cl-1, Cl+1

 

45. Properties of the alkali metals are discussed in section 7.13. List some properties you would expect for the alkaline earths.