Chemistry Final-Multiple Choice

1) No two electrons can have the same four quantum number is known as A) Pauli exclusion principle B) Hund's rule C) Aufbau principle D) Heisenberg uncertainty principle

A

10) Calculate the wavelength (in nm) of a the red light emitted by a neon sign with a frequency of 4.74 × 1014 Hz. A) 633 nm B) 158 nm C) 142 nm D) 704 nm E) 466 nm

A

13) Identify the element that has a ground state electronic configuration of [Kr]5s24d5. A) Tc B) Mn C) Nb D) Ru

A

17) Which of the following occur as the wavelength of a photon increases? A) the frequency decreases B) the energy increases C) the speed decreases D) Planck's constant decreases E) None of the above occur as the wavelength of a photon increases.

A

19) Calculate the energy of the violet light emitted by a hydrogen atom with a wavelength of 410.1 nm. A) 4.85 × 10-19 J B) 2.06 × 10-19 J C) 1.23 × 10-19 J D) 8.13 × 10-19 J E) 5.27 x 10-19 J

A

2) Choose the orbital diagram that represents the ground state of N. A) B) C) D) E)

A

2) Place the following types of electromagnetic radiation in order of increasing frequency. visible light microwaves X-rays A) microwaves < visible light < X-rays B) X-rays < visible light < microwaves C) microwaves < X-rays < visible light D) X-rays < microwaves < visible light E) visible light < X-rays < microwaves

A

23) How many valence electrons does an atom of Ba possess? A) 2 B) 1 C) 8 D) 6 E) 3

A

24) Determine the shortest frequency of light required to remove an electron from a sample of Ti metal if the binding energy of titanium is 3.14 × 103 kJ/mol. A) 7.87 x 1015 Hz B) 4.74 x 1015 Hz C) 2.11 x 1015 Hz D) 1.27 x 1015 Hz E) 6.19 x 1015 Hz

A

24) How many valence electrons does an atom of Ti possess? A) 2 B) 4 C) 6 D) 8 E) 0

A

27) Calculate the wavelength of an electron (m = 9.11 × 10-28 g) moving at 3.66 × 106 m/s. A) 1.99 × 10-10 m B) 5.03 × 10-10 m C) 1.81 × 10-10 m D) 5.52 × 10-9 m E) 2.76 × 10-9 m

A

3) Choose the valence orbital diagram that represents the ground state of Zn. A) B) C) D) E)

A

33) Place the following in order of increasing radius. Ca2+ S2- Cl- A) Ca2+ < Cl- < S2- B) Cl- < Ca2+ < S2- C) S2- < Cl- < Ca2+ D) Ca2+ < S2-< Cl- E) Cl- < S2- < Ca2+

A

33) Which of the following transitions (in a hydrogen atom) represent absorption of the smallest frequency photon? A) n = 5 to n = 6 B) n = 5 to n = 4 C) n = 4 to n = 1 D) n = 1 to n = 3 E) n = 1 to n = 2

A

34) Choose the transition (in a hydrogen atom) below that represents the absorption of the shortest wavelength photon. A) n = 1 to n = 2 B) n = 2 to n = 3 C) n = 4 to n = 5 D) n = 6 to n = 3 E) n = 3 to n = 1

A

37) What are the possible orbitals for n = 3? A) s, p, d B) s, p, d, f C) s D) s, p

A

4) Give the set of four quantum numbers that could represent the last electron added (using the Aufbau principle) to the Cl atom. A) n = 3, l = 1, ml = 1, ms = + B) n = 3, l = 0, ml = 1, ms = - C) n = 3, l = 2, ml =1 , ms = + D) n = 2, l = 1, ml = 1, ms = - E) n = 3, l =2 , ml = 1, ms = -

A

42) How many orbitals are contained in the third principal level (n=3) of a given atom? A) 9 B) 3 C) 18 D) 7 E) 5

A

45) Choose the diamagnetic species from below. A) Sn2+ B) Br C) P D) Cr E) None of the above are diamagnetic.

A

46) Which of the following quantum numbers describes the orientation of an orbital? A) magnetic quantum number B) principal quantum number C) angular momentum quantum number D) spin quantum number E) Schrödinger quantum number

A

49) Give the ground state electron configuration for Br-. A) [Ar]4s23d104p6 B) [Ar]4s23d104p5 C) [Ar]4s24p6 D) [Ar]4s24d104p6 E) [Ar]4s23d104p4

A

5) Give the set of four quantum numbers that could represent the last electron added (using the Aufbau principle) to the Sr atom. A) n = 5, l = 0, ml = 0, ms = - B) n = 4, l = 1, ml = 1, ms = - C) n = 5, l = 1, ml = 0, ms = + D) n = 4, l = 1, ml = -1, ms = + E) n = 5, l = 1, ml =1 , ms = -

A

5) Identify the color that has a wavelength of 460 nm. A) blue B) green C) red D) yellow

A

50) If two electrons in the same atom have the same value of "l", they are A) in the same sublevel, but not necessarily in the same level. B) in the same level, but different sublevel. C) in the same orbital. D) in different levels and in different shaped orbitals. E) None of the above

A

7) Which of the following statements is TRUE? A) An orbital that penetrates into the region occupied by core electrons is less shielded from nuclear charge than an orbital that does not penetrate and therefore has a lower energy. 3 B) An orbital that penetrates into the region occupied by core electrons is more shielded from nuclear charge than an orbital that does not penetrate and therefore has a lower energy. C) It is possible for two electrons in the same atom to have identical values for all four quantum numbers. D) Two electrons in the same orbital can have the same spin. E) None of the above are true.

A

8) Give the ground state electron configuration for Se. A) [Ar]4s23d104p4 B) [Ar]4s24d104p4 C) [Ar]4s23d104p6 D) [Ar]4s23d10 E) [Ar]3d104p4

A

44) Which of the following statements are TRUE? A) We can sometimes know the exact location and speed of an electron at the same time. B) All orbitals in a given atom are roughly the same size. C) Since electrons have mass, we must always consider them to have particle properties and never wavelike properties. D) Atoms are roughly spherical because when all of the different shaped orbitals are overlapped, they take on a spherical shape. E) All of the above are true.

D

48) How many of the following species are diamagnetic? Cs Zr2+ Al3+ Hg2+ A) 1 B) 3 C) 0 D) 2 E) 4

D

49) How many different values of ml are possible in the 3d sublevel? A) 2 B) 1 C) 3 D) 5 E) 7

D

7) Which of the following visible colors of light has the longest wavelength? A) blue B) green C) yellow D) red E) violet

D

1) Place the following types of electromagnetic radiation in order of increasing wavelength. ultraviolet light gamma rays radio waves A) gamma rays < radio waves < ultraviolet light B) radio waves < ultraviolet light < gamma rays C) radio waves < gamma rays < ultraviolet light D) ultraviolet light < gamma rays < radio waves E) gamma rays < ultraviolet light < radio waves

E

12) Give the ground state electron configuration for Cd. A) [Kr]5s25d10 B) [Kr]5s24d105p2 C) [Kr]4d10 D) [Kr]5s24d8 E) [Kr]5s24d10

E

18) Calculate the energy of the red light emitted by a neon atom with a wavelength of 703.2 nm. A) 3.54 × 10-19 J B) 4.27 × 10-19 J C) 2.34 × 10-19 J D) 6.45 × 10-19 J E) 2.83 × 10-19 J

E

22) How many valence electrons does an atom of S have? A) 3 B) 1 C) 2 D) 4 E) 6

E

23) What total energy (in kJ) is contained in 1.0 mol of photons all with a frequency of 2.75 × 1014 Hz? A) 182 kJ B) 219 kJ C) 457 kJ D) 326 kJ E) 110 kJ

E

25) How many valence electrons does an atom of Cu possess? A) 2 B) 9 C) 11 D) 3 E) 1

E

26) Which of the following statements is TRUE? A) The emission spectrum of a particular element is always the same and can be used to identify the element. B) Part of the Bohr model proposed that electrons in the hydrogen atom are located in "stationary states" or particular orbits around the nucleus. C) The uncertainty principle states that we can never know both the exact location and speed of an electron. D) An orbital is the volume in which we are most likely to find an electron. E) All of the above are true.

E

27) How many valence electrons do the halogens possess? A) 5 B) 6 C) 2 D) 1 E) 7

E

32) Place the following in order of increasing atomic radius. As O Br A) As < Br < O B) O < As < Br C) Br < As < O D) As < O < Br E) O < Br < As

E

32) Which of the following transitions (in a hydrogen atom) represent emission of the longest wavelength photon? A) n = 1 to n = 2 B) n = 3 to n = 1 C) n = 3 to n = 4 D) n = 4 to n = 2 E) n = 5 to n = 4

E

38) Which reaction below represents the second ionization of Sr? A) Sr(g) → Sr+ (g) + e- B) Sr2+ (g) + e- → Sr+ (g) C) Sr+ (g) + e-⁻ → Sr(g) D) Sr- (g) + e- → Sr2- (g) E) Sr+ (g) → Sr2+ (g) + e-

E

41) Each of the following sets of quantum numbers is supposed to specify an orbital. Choose the one set of quantum numbers that does not contain an error. A) n = 4, l = 4, ml =0 B) n = 3, l = 2, ml =+3 C) n = 4, l = 0, ml =-1 D) n = 3, l = 1, ml = -2 E) n = 5, l = 3, ml =-3

E

43) Place the following in order of decreasing metallic character. P As K A) P > As > K B) As > P > K C) K > P > As D) As > K > P E) K > As > P

E

44) Choose the paramagnetic species from below. A) Ca B) O2- C) Cd2+ D) Zn E) Nb3+

E

45) Which of the following quantum numbers describes the shape of an orbital? A) principal quantum number B) magnetic quantum number C) spin quantum number D) Schrödinger quantum number E) angular momentum quantum number

E

28) Calculate the wavelength of a baseball (m = 155 g) moving at 32.5 m/s. A) 7.60 × 10-36 m B) 1.32 × 10-34 m C) 2.15 × 10-32 m D) 2.68 × 10-34 m E) 3.57 × 10-32 m

B

28) How many valence electrons do the alkali metals possess? A) 1 B) 2 C) 7 D) 6 E) 8

B

3) Place the following types of electromagnetic radiation in order of decreasing energy. ultraviolet light radio waves microwaves A) radio waves > microwaves > ultraviolet light B) ultraviolet light > microwaves > radio waves C) radio waves > ultraviolet light > microwaves D) ultraviolet light > radio waves > microwaves E) microwaves > radio waves > ultraviolet light

B

31) It is possible to determine the ionization energy for hydrogen using the Bohr equation. Calculate the ionization energy for an atom of hydrogen making the assumption that ionization is the transition from n=1 to n=∞. A) -2.18 × 10-18 J B) +2 .18 × 10-18 J C) +4.59 × 10-18 J D) -4.59 × 10-18 J E) +4.36 x 10-18 J

B

34) Place the following in order of increasing radius. Br- Na+ Rb+ A) Br- < Rb+ < Na+ B) Na+ < Rb+ < Br- C) Rb+ < Br- < Na+ D) Br- < Na+ < Rb+ E) Rb+ < Na+ < Br-

B

35) Which of the following transitions represent the emission of a photon with the largest energy? A) n = 2 to n = 1 B) n = 3 to n = 1 C) n = 6 to n = 3 D) n = 1 to n = 4 E) n = 2 to n = 5

B

36) Choose the statement that is TRUE. A) Outer electrons efficiently shield one another from nuclear charge. B) Core electrons effectively shield outer electrons from nuclear charge. C) Valence electrons are most difficult of all electrons to remove. D) Core electrons are the easiest of all electrons to remove. 8 E) All of the above are true.

B

38) What value of l is represented by a d orbital? A) 1 B) 2 C) 0 D) 3

B

40) Place the following in order of increasing IE1. N F As A) N < As < F B) As < N < F C) F < N < As D) As < F < N E) F < N < As

B

43) How many sublevels are contained in the second shell (n=2) of a given atom? A) 1 B) 2 C) 9 D) 4 E) 3

B

46) Choose the paramagnetic species from below. A) Ti4+ B) O C) Ar D) All of the above are paramagnetic. E) None of the above are paramagnetic.

B

47) How many different values of ml are possible in the 4f sublevel? A) 1 B) 7 C) 3 D) 5 E) 2

B

50) Give the ground state electron configuration for Mg2+. A) 1s22s22p63s2 B) 1s22s22p6 C) 1s22s22p63s23p2 D) 1s22s22p63s23p6 E) 1s22s22p63s1

B

6) Give the set of four quantum numbers that represent the last electron added (using the Aufbau principle) to the Zn atom. A) n = 4, l = 3, ml = 3, ms = - B) n = 3, l = 2, ml = 2, ms = - C) n = 3, l = 1, ml = 1, ms = + D) n = 3, l = 3, ml = 2, ms = - E) n = 4, l = 2, ml = 0, ms = +

B

8) Which of the following types of electromagnetic radiation has the shortest wavelength? A) blue B) violet C) orange D) green E) yellow

B

9) Give the ground state electron configuration for I. A) [Kr]5s24d105p6 B) [Kr]5s24d105p5 C) [Kr]4d105p6 D) [Kr]5s25p6 E) [Kr]5s25d105p6

B

10) Give the ground state electron configuration for Sr. A) [Kr]5s24d2 B) [Kr]5s24d105p2 C) [Kr]5s2 D) [Kr]5s25d105p2 E) [Kr]5s24d10

C

12) Calculate the frequency of the red light emitted by a neon sign with a wavelength of 659.9 nm. A) 2.20 × 1014 s-1 B) 1.98 × 1014 s-1 C) 4.55 × 1014 s-1 D) 5.05 × 1014 s-1 E) 3.32 × 1014 s-1

C

14) Calculate the energy of the orange light emitted per photon, by a neon sign with a frequency of 4.89 × 1014 Hz. A) 3.09 × 10-19 J B) 6.14 × 10-19 J C) 3.24 × 10-19 J D) 1.63 × 10-19 J E) 5.11 × 10-19 J

C

14) Identify the element that has a ground state electronic configuration of [Ar]4s23d104p1. A) Al B) In C) Ga D) B

C

16) How many unpaired electrons are present in the ground state Kr atom? A) 1 B) 2 C) 0 D) 3 E) 5

C

18) Write out the orbital diagram that represents the ground state of As. How many unpaired electrons are there? A) 0 B) 4 C) 3 D) 2 E) 1

C

20) How many of the following elements have 1 unpaired electron in the ground state? B Al S Cl A) 1 B) 2 C) 3 D) 4

C

20) How many photons are contained in a burst of yellow light (589 nm) from a sodium lamp that contains 609 kJ of energy? A) 3.37 × 1019 photons B) 3.06 × 1030 photons C) 1.80 × 1024 photons D) 4.03 × 1028 photons E) 2.48 × 1025 photons

C

29) Determine the velocity of a marble (m = 8.66 g) with a wavelength of 3.46 × 10-33 m. A) 45.2 m/s B) 11.3 m/s C) 22.1 m/s D) 38.8 m/s E) 52.9 m/s

C

29) Give the complete electronic configuration for Mn. A) 1s22s22p63s23p64s24d5 B) 1s22s22p63s23p64s13d6 C) 1s22s22p63s23p64s23d5 D) 1s22s22p63s23p64s24p5

C

30) Place the following elements in order of increasing atomic radius. P Ba Cl A) Ba < P < Cl B) P < Cl < Ba C) Cl < P < Ba D) Cl < Ba < P E) Ba < Cl < P

C

35) Place the following in order of decreasing radius. Te2- F- O2- A) F- > O2- > Te2- B) F- > Te2- > O2- C) Te2- > O2- > F- D) Te2- > F- > O2- E) O2- > F- > Te2-

C

36) For n = 3 what are the possible sublevels? A) 0 B) 0, 1 C) 0, 1, 2 D) 0, 1,2, 3

C

39) Each of the following sets of quantum numbers is supposed to specify an orbital. Which of the following sets of quantum numbers contains an error? A) n = 2, l = 1 , ml = -1 B) n = 4, l = 2, ml =0 C) n = 3, l =3 , ml = -2 D) n = 1, l = 0, ml =0 E) n = 3, l = 0, ml =0

C

39) What period 3 element having the following ionization energies (all in kJ/mol)? IE1 = 1012 IE2 = 1900 IE3= 2910 IE4= 4960 IE5= 6270 IE6 = 22,200 A) Si B) S C) P D) Cl E) Mg

C

4) Identify the color that has a wavelength of 700 nm. A) blue B) green C) red D) yellow

C

41) Place the following in order of decreasing IE1. Cs Mg Ar A) Cs > Mg > Ar B) Mg > Ar > Cs C) Ar > Mg > Cs D) Cs > Ar > Mg E) Mg > Cs > Ar

C

47) How many of the following species are paramagnetic? Sc3+ Br- Mg2+ Se A) 0 B) 2 C) 1 D) 4 E) 3

C

48) How many different values of l are possible in the third principal level? A) 1 B) 2 C) 3 D) 0 E) 4

C

6) Which of the following visible colors of light has the largest frequency? A) green B) red C) blue D) yellow E) orange

C

9) Which of the following types of electromagnetic radiation has the smallest frequency? A) yellow B) blue C) orange D) green E) purple

C

11) Give the ground state electron configuration for Pb. A) [Xe]6s26p2 B) [Xe]6s25d106p2 C) [Xe]6s25f146d106p2 D) [Xe]6s24f145d106p2 E) [Xe]6s25f145d106p2

D

15) Calculate the frequency of the green light emitted by a hydrogen atom with a wavelength of 486.1 nm. A) 1.46 × 1014 s-1 B) 6.86 × 1014 s-1 C) 4.33 × 1014 s-1 D) 6.17 × 1014 s-1 E) 1.62 × 1014 s-1

D

16) Which of the following occur as the energy of a photon increases? A) the frequency decreases. B) the speed increases. C) the wavelength increases D) the wavelength gets shorter. E) None of the above occur as the energy of a photon increases.

D

17) How many unpaired electrons are present in the ground state Ge atom? A) 0 B) 3 C) 1 D) 2 E) 4

D

19) How many of the following elements have 2 unpaired electrons in the ground state? C O Ti Si A) 1 B) 2 C) 3 D) 4

D

21) How many photons are contained in a flash of green light (525 nm) that contains 189 kJ of energy? A) 5.67 × 1023 photons B) 2.01 × 1024 photons C) 1.25 × 1031 photons D) 4.99 × 1023 photons E) 7.99 × 1030 photons

D

21) Identify the number of valence electrons for Mn. A) 8 B) 7 C) 5 D) 2

D

22) How much energy (in kJ) do 3.0 moles of photons all with a wavelength of 655 nm, contain? A) 183 kJ B) 303 kJ C) 394 kJ D) 548 kJ E) 254 kJ

D

26) How many valence electrons does an atom of Al possess? A) 1 B) 2 C) 5 D) 3 E) 8

D

30) Determine the velocity of a medicine ball (m = 10.0 kg) with a wavelength of 1.33 × 10-35 m. A) 8.81 m/s B) 12.3 m/s C) 2.21 m/s D) 4.98 m/s E) 6.44 m/s

D

31) Place the following elements in order of decreasing atomic radius. Xe Rb Ar A) Ar > Xe > Rb B) Xe > Rb > Ar C) Ar > Rb > Xe D) Rb > Xe > Ar E) Rb > Ar > Xe

D

37) Which reaction below represents the first ionization of O? A) O+ (g) + e- → O(g) B) O(g) + e- → O- (g) C) O- (g) → O(g) + e- D) O(g) → O+ (g) + e- E) O- (g) + e- → O2- (g)

D

40) Each of the following sets of quantum numbers is supposed to specify an orbital. Choose the one set of quantum numbers that does not contain an error. A) n = 2, l = 2, ml =-1 B) n = 2, l = 2, ml =0 C) n = 3, l = 2, ml =-3 D) n = 4, l = 3, ml =-2 E) n = 4, l = 2, ml =+4

D

11) Calculate the wavelength (in nm) of the blue light emitted by a mercury lamp with a frequency of 6.88 × 1014 Hz. A) 229 nm B) 436 nm C) 206 nm D) 485 nm E) 675 nm

B

13) Calculate the energy of the green light emitted per photon, by a mercury lamp with a frequency of 5.49 × 1014 Hz. A) 2.75 × 10-19 J B) 3.64 × 10-19 J C) 5.46 × 10-19 J D) 1.83 × 10-19 J E) 4.68 × 10-19 J

B

15) How many unpaired electrons are present in the ground state P atom? A) 0 B) 3 C) 1 D) 2 E) 4

B

25) Determine the longest wavelength of light required to remove an electron from a sample of potassium metal if the binding energy for an electron in K is 1.76 × 103 kJ/mol. A) 147 nm B) 68.0 nm C) 113 nm D) 885 nm E) 387 nm

B

42) Place the following in order of increasing IE1. K Ca Rb A) Ca < K < Rb B) Rb < Ca < K C) Ca < Rb < K D) Rb < K < Ca E) K < Ca < Rb

D