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Electrons test 2009

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					        Electrons Test                                                   Name: __________________
        November 5, 2009                                                 Williamson Chemistry

        I. Vocabulary Matching – see definitions below (1.5 pts each)              (___ / 19.5 pts)

        ____ valence electron ___ kernel electron                        ___ noble gases

        ___ aufbau principle     ___ Pauli Exclusion Principle            ____ Hund’s Rule

                                           ____ c              ____ h

        ____ Meters              ___ joule                               ____ Hertz

        A – the units for energy
        B – the units for frequency
        C – the units for wavelength

        D – electrons found in the highest energy level of an atom
        E – electrons that are not in the highest energy level of an atom.
        F – the family of elements that are inert

        G – this variable is the number of waves that pass a point in space in one second
        H – this variable the distance between two peaks or two troughs of a wave
        I – this constant relates energy to frequency.
        J – this constant is the speed of light

        K – electrons fill the lowest available energy level
        L – There can only be 2 electrons in an orbital and any pair of electrons in the same
        orbital must have opposing spin. Each electron needs to be unique.
        M – states that this is correct                   while this is not
                                         1s   2s 2px 2py 2pz                      1s   2s 2px 2py 2pz




        II. Multiple Choice Answers: (1.5 points each)                             (___ / 25.5)
        Questions are on the last few pages of the test

1____       2 ____     3 _____

4 _____     5 _____    6 _____       7 ____          8 _____       9 _____         10 _____

11 ____    12 _____ 13 _____         14 ____        15 _____       16 _____        17 ____
III. Given the following information, solve for the unknown term.
E = h       c         h = 6.62 x10-34J.s    c = 3.00 x 108 m/s      1 m = 1x109 nm

18) Pick two (2) of the next three(3)                                 (3 points each)

a. What is the frequency of a wave if its wavelength is 2.5meters?




b. What is the energy of a wave if its frequency is 4.78 x 1014 Hz?




c. What is the wavelength of a wave if its frequency is 5.21 x 1019 Hz?




19) Pick one (1) of the next two (2)         (4 points – multiple steps per question)

a. What is the energy of a wave if its wavelength is 534 nm?




b. What is the wavelength of a wave if it has 2.44 x 10-19 J of energy?
IV. The Mercury Spectrum                                                   (____ / 10 pts)
The following lines were seen through a diffraction grating when an electric current was
run through a sample of mercury vapor.

                                                      a    b




                 400nm 430nm       540 nm                 700 nm 740 nm
                   violet indigo    green                 red    dark red



   20) What color line has the lowest frequency? __________


   21) Give the color for each frequency. It is not necessary to do any calculations if you
        can match the longest wavelength with the corresponding frequency, and the
        shortest wavelength with its corresponding frequency…
        Also note that there are two red lines, red a and red b.
Frequency
(Hertz)       4.05 x 1014   7.50 x 1014    4.35 x 1014   6.97 x 1014     5.55 x 1014   4.25 x 1014
Color


   22) What color line has the highest energy? Explain.

________________________________________________________________________

________________________________________________________________________

________________________________________________________________________

   23) The emission spectrum above is from mercury. Explain how these seven spectral
       lines were created by the mercury atoms.

________________________________________________________________________

________________________________________________________________________

________________________________________________________________________

________________________________________________________________________

________________________________________________________________________

________________________________________________________________________

________________________________________________________________________
V. Give the element described by the following: (2 pts each)                                         (___ / 16 pts)

24)_________ = has the electron configuration of 1s22s22p5

25) _________ = has the electron configuration of [Ar] 4s23d7

26) _________ = has the orbital diagram of
                                                              1s        2s     2px 2py 2pz

27) _________ = has 3 valence electrons – its highest energy level is the 3rd

28) _________ = has one less electron than a noble gas (there are a few you may choose from)

29)_________ = has similar chemical properties as Ar, but has twice as many electrons

30)_________ = has the electron configuration of 1s2 2s2 2p6 3s2 3p6 4s1 3d5

31)_________ = has the electron configuration of [He]2s22p6

VI. Complete the Orbital Diagram and Electron Configuration for each of these elements.
                                                     2 pts each                 (___/ 10)
32. boron #e:____    electron configuration:___________________________________



1s    2s       2px 2py       2pz     3s      3px 3py    3pz        4s   3d1   3d2    3d3   3d4 3d5     4px   4py   4pz



33. argon   #e:____           electron configuration:_____________________________



1s    2s       2px 2py       2pz     3s      3px 3py    3pz        4s   3d1   3d2    3d3   3d4 3d5     4px   4py   4pz



34. copper   #e:____          electron configuration:___________________________________



1s    2s       2px 2py       2pz     3s      3px 3py    3pz        4s   3d1   3d2    3d3   3d4 3d5     4px   4py   4pz



35. oxygen    #e:____         electron configuration:_____________________________



1s    2s       2px 2py       2pz     3s      3px 3py    3pz        4s   3d1   3d2    3d3   3d4 3d5     4px   4py   4pz



36. manganese         #e:____ electron configuration:____________________________



1s    2s       2px 2py       2pz     3s      3px 3py    3pz        4s   3d1   3d2    3d3   3d4 3d5     4px   4py   4pz
VII. Compare sulfur (S) and selenium (Se):                        (1 pt each)          (___/9)

36. How many electrons are in sulfur? _____

37. Complete the orbital diagram for sulfur:

1s     2s    2px 2py   2pz   3s   3px 3py   3pz      4s    3d1   3d2   3d3   3d4 3d5     4px   4py   4pz



38: How many valence electrons are in sulfur? ____


39. How many electrons are in selenium? _____

40. Complete the orbital diagram for selenium:

1s     2s    2px 2py   2pz   3s   3px 3py   3pz      4s    3d1   3d2   3d3   3d4 3d5     4px   4py   4pz



41: How many valence electrons are in selenium? ____


42. Write a statement comparing sulfur and selenium, their valence electrons and their
location on the periodic table. (3 pts)




Multiple Choice Questions
  Use this first statement for the first three multiple choice questions (1-3)

The energy of wave A is greater than the energy of wave B.                   (E of A > E of B)

     1) Which of the following is true?
          a.  of A >  of B                      c.  of A <  of B
          b.  of A =  of B                      d. Can’t be determined

     2) Which of the following is true?
          a.  of A >  of B                      c.  of A <  of B
          b.  of A =  of B                      d. Can’t be determined

     3) Which of the following is true?
          a. speed of A > speed of B                      c. speed of A < speed of B
          b. speed of A = speed of B                      d. Can’t be determined
4) This word describes the reactivity of the noble gases.
      a. Explosive               b. Inert        c. Lethargic           d. Critical


5) The fact that electrons can be described by specific, discrete energy locations
   called orbitals is a theory in…
       a. Molecular Dynamics                     c. Simple Mechanics
       b. Nuclear Dynamics                       d. Quantum Mechanics


6) The most useful piece of information that orbital diagrams provide that electron
   configurations do not provide is…
      a. the direction of spin and orbital location of each electron.
      b. the number of electrons in an s orbital.
      c. the energy level that electrons are in.
      d. the number of electrons in a sublevel.

7) How many total electrons can enter the “p” sub-level?
     a. 2               b. 3            c. 6          d. 10             e. 14

8) What are valence electrons?
     a. electrons in the highest energy level
     b. electrons that have been emitted as beta particles from the nucleus
     c. non-bonding electrons
     d. electrons in the lower energy levels of an atom


9) Which of the following types of electromagnetic radiation has the longest
   wavelength?
      a. Microwaves                     d. Red Light waves
      b. Blue Light Waves               e. X-rays
      c. Ultraviolet rays

10) Which order is correct for highest energy to lowest energy for these three types of
    electromagnetic radiation?
        a. Infrared Light >Visible Light > Ultraviolet Light
        b. Visible Light > Ultraviolet Light > Infrared Light,
        c. Visible Light > Infrared Light > Ultraviolet Light
        d. Ultraviolet Light > Visible Light > Infrared Light


11) What is the Heisenberg Uncertainty Principle?
      a. We can’t know the charge or mass of an electron, ever.
      b. We can’t know both the position and speed of an electron simultaneously.
      c. We can’t know what an atom looks like because it is always in motion.
      d. We can’t find an electron in the cathode ray tube.
     12) This is the word that means “to build” in German. It explains how electrons fill
         an atom’s orbitals to form the most stable configuration.
             a. Aufbau          b. Owfbow         c. Achtung        d. Lufthansa


     13) What is wrong with this electron configuration for sodium: Na = 1s2, 2s2, 2p5, 3s2
           a. It doesn’t have the correct number of total electrons
           b. There are not enough protons
           c. There are too many total electrons
           d. The 2p sublevel needs to be filled before the 3s is filled


     14) Which one of these electron configurations is correct for the fluoride anion, F-1?
           a. 1s2, 2s2, 2p6           c. 1s2, 2s2, 2p5
                 2    2   4
           b. 1s , 2s , 2p            d. 1s2


     15) What is wrong with this orbital diagram for manganese, Mn?


1s     2s    2px 2py 2pz     3s    3px 3py 3pz     4s    3d1 3d2 3d3 3d4 3d5 4px 4py 4pz

            a.   Nothing
            b.   There are too many total electrons
            c.   All the electrons need to spin in the same direction
            d.   The 5 electrons in the d sub-level electrons need to spread out into their
                 own orbitals.


     16) What is wrong with this orbital diagram for argon?


1s     2s    2px 2py 2pz     3s    3px 3py 3pz     4s    3d1 3d2 3d3 3d4 3d5 4px 4py 4pz

            a. Nothing
            b. There are too few total electrons
            c. The 3 pairs of electrons in the p sub-level need to spin in opposite
               directions
            d. All the electrons need to spin up


     17) Where are the electrons found in an atom?
           a. Inside the nucleus, with the protons
           b. In orbits going around the nucleus like the moon orbits the earth
           c. Inside the nucleus, with the neutrons
           d. In orbitals that surround the nucleus

				
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