AP Chemistry                                                               Unit 7

Chapter 7                                                                     Atomic Structure         

Takehome Test 7

Directions:The test is divided into 2 parts multiple guess and free response. Answer any 10 multiple guess (3 points each) and any 2 free response (15 pts each). It is suggested you do the free response first. Answer on the provided answer blank at the appropriate location. Remember: ”It is quality not quantity that matters” Seneca 65AD

 

Multiple Guess

Electromagnetic Radiation

1. Which pair of electromagnetic radiations has the relation of lower and higher in energy

  1. UV, IR
  2. Visible light, IR
  3. Radar, Radio
  4. X Ray, Gamma Ray
  5. none of these

 

2. Red light has a wavelength of 650 nm. What is the frequency of this light

     a. 3.64 X 10-38 J

     b. 2.17 X 10-5 J

     c. 3.61 X 10-19 /sec

    d. 4.61 X 1014 /sec

    e. none of these

 

The Nature of Matter

3. The frequency of blue light is about 4.5 X 1014 /sec. What is the energy of this radiation?

  1. 6.66 X 10-34 J
  2. 6.66 X 1014 /sec
  3. 4.41 X 10-19 J
  4. 4.41 X 10-27 /sec
  5. None of these

 

4. The energy associated with the characteristic yellow of sodium  is 3.37 X 10-19 J. What is the wavelength of this wave?

  1. 4.22 X 1034 J
  2. 5.09 X 1014 /sec
  3. 744 nm
  4. 5890 Ǻ
  5. none of these

 

 

 

5. According to deBroglie, many objects can be assigned wave characteristics. What is the wavelength of an electron (9.11 X 10-31 kg) orbiting a nucleus at the rate of 5.00 X 106 m/sec?

     a. 3.26 X 10-7 m

     b. 4.43 X 1014 hz

     c. 0.146 nm

    d. 735 Ǻ

     e. none of these

 

 

The Bohr Model

6. Calculate the amount of energy released when a Hydrogen electron falls from the second energy level (n=2) to the 1nd energy level (n=1).

  1. -2.178 X 10-18 J
  2. -1.56 X 10-18 J
  3. -1.09 X 10-18 J
  4. -5.45 X 10-19 J
  5. none of these

 

7. Calculate the energy involved if a Helium (atomic number Z=2) electron moves from the 2nd to the 3rd level

  1. -2.43 X 10-18 J
  2. +1.77 X 10-18 J
  3. -1.21 X 10-18 J
  4. +1.05 X 10-18 J
  5. none of these

 

Quantum Mechanical Model of the Atom

8. The configuration endings for La, Ce, and Pr are

     a. d1,d2,d3

     b. f1,f2,f3

     c. s1,p2,d3

     d. d1,d1f1,f3

     e. none of these

 

9. To relate electron behaviors we use the Schroedinger Wave Equation which describes

                       

     a. probability of electron position

     b. possibility of chemical bonding

     c. types of chemical bonds in molecules

     d. atomic size vs. atomic number

     e. none of these

 

Quantum Numbers

10. The quantum number description for the last electron in Na is (…according to your authors definitions of mℓ = +ℓ to -ℓ, and ms  are +1/2, -1/2…)

  1. 1,0,0,-1/2
  2. 2,0,0,-1/2
  3. 2,1,0,-1/2
  4. 2,1,1, 1/2
  5. none of these

 

11. The ending configuration piece for Br is

     a. 2s2

     b. 3p5

     c. 4d9

     d. 5f13

     e. none of these

 

 

 

 

 

12. In a d orbital, there are how many electron density plots (or possible routes)

a. 1

b. 3

c. 5

d. 7

e none of these

 

 

13. The final part of the spin diagram (Aufbau diagram) for Ce would be

a. O

 

b. OOO

 

c. OOOOO

 

d. OOOOOOO

 

e. None of these

 

Periodic Trends

14. Arrange the following in terms of decreasing atomic size

a.       Ca>Ga>Ge

b.       Ca<Ga<Ge

c.       Ca<Ga>Ge

d.       Ca>Ga<Ge

e.       none of these

 

15. Arrange in terms of increasing ionization energy

a.       Al>P>S

b.       Al<P<S

c.       Al>P<S

d.       Al<P>S

e.       none of these

 

Free Response

 

16. Associate the description with the principle

 

1. Pauli Exclusion Principle

2. Aufbau Principle

3. Hunds Rule

4. Rule of Octets

 

a. as protons are added to the nucleus, electrons would also be added hydrogenlike to orbitals (work outward from the nucleus)

b. there are never more than 8 electrons in the outer layer

c. in a given atom no two electrons can have the same 4 quantum numbers

d. the lowest energy configuration is the one with the maximum number of unpaired electrons (electrons fill by spin first)

 

 

 

 

 

 

17. Given the Ionization table below…:

a)       explain what the first ionization energy values do (table expressed in Kj/mole) as one moves across a period (justify any deviations in behavior)

b)       explain why there is a big jump in ionization energy for Z=13 between I3 and I4

c)       discuss what column from the periodic chart the following energies belong

      I1=690, I2=1510, I3=2850, I4=4200, I5=15900, I6=18500, I7=21000

d)       why I1 for Z=16 is less than I1 for Z=15

e)       give the approximate I1 value for Z=19 and justify

Atomic #

I1

I2

I3

I4

I5

I6

I7

11

495

4560

 

 

 

 

 

12

735

1445

7730

 

 

 

 

13

580

1815

2740

11160

 

 

 

14

780

1575

3220

4350

16100

 

 

15

1060

1890

2905

4950

6270

21200

 

16

980

1750

2801

4759

6120

8733

9622

17

1255

2295

3850

5160

6560

9360

11000

18

1527

2665

3945

5770

7230

8780

12000

 

 

 

18. Write    a) the 4 quantum numbers, b) the complete configuration(NOT OK to abbreviate with noble gases), and c) the spin notation(show energy positions) for plutonium (Pu)