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Exam 2 with Solution Key - General Chemistry I | CHEM 1110, Exams of Chemistry

Middle Tennessee State University (MTSU)Chemistry
Prof. William Ilsley

Material Type: Exam; Professor: Ilsley; Class: General Chemistry I; Subject: Chemistry; University: Middle Tennessee State University; Term: Fall Term 2015;

Typology: Exams

2014/2015

Uploaded on 12/02/2015

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Exam 2 Name: ____________________
October 15, 2015 Chemistry 1110 I.D.#: ____________________
1. Which one of the following electron configurations would have the smallest atomic radius?
A. [Kr]5s1B. [Ne]3s23p5C. [Ar]4s23d104p4D. [Ne]3s2
E. [Ar]4s1
2. Which quantum number represents the number of sublevels in a principal energy level?
A. magnetic spin B. magnetic orbital C. principal
D. angular momentum
3. What is/are the possible value(s) of the ml quantum number of the l quantum number is 2?
A. -1, 0, +1 B. -2, -1, 0, +1, +2 C. 0, 1, 2
D. 1, 2, 3 E. 0, 1
4. Which of the following is the correct Lewis structure for SF4?
A.
S
F
F
F
F
B.
S
F
F
F
F
C.
S
F
F
F
F
D.
S
F
F
F
F
5. What are the possible values of the l quantum number if the n quantum number is 3?
A. 1, 2, 3 B. 0, 1, 2 C. 0, 1, 2, 3
D. -1, 0, +1 E. -3, -2, -1, 0, +1, +2, +3
6. Of the following elements, _______ has the most negative (i.s. largest) electron affinity?
A. C B. B C. Be D. O
7. Which of the following scientists performed the famous oil-drop experiment?
A. J.J. Thompson B. R.A. Millikan C. Louis de Broglie
D. Earnest Rutherford E. Neisl Bohr
8. The electron configuration of the Al2- anion is ______.
A. [Ne]3s2B. [Ne]3s23p1C. [Ne]3s23p3D. [Ne]3p2E. [Ne]3s23p6
9. Which of the following ground state orbital diagrams violates the Pauli Principal?
A.
1s 2s 2p
B.
2p
C.
1s 2s 2p
D.
1s 2s 2p
pf3
pf4
pf5

Partial preview of the text

Download Exam 2 with Solution Key - General Chemistry I | CHEM 1110 and more Exams Chemistry in PDF only on Docsity!

Exam 2 Name: ____________________ October 15, 2015 Chemistry 1110 I.D.#: ____________________

  1. Which one of the following electron configurations would have the smallest atomic radius? A. [Kr]5s 1 B. [Ne]3s 2 3p 5 C. [Ar]4s 2 3d 10 4p 4 D. [Ne]3s 2 E. [Ar]4s 1
  2. Which quantum number represents the number of sublevels in a principal energy level? A. magnetic spin B. magnetic orbital C. principal D. angular momentum
  3. What is/are the possible value(s) of the ml quantum number of the l quantum number is 2? A. -1, 0, +1 B. -2, -1, 0, +1, +2 C. 0, 1, 2 D. 1, 2, 3 E. 0, 1
  4. Which of the following is the correct Lewis structure for SF 4? A.

S

F

F

F

F

B.

S

F

F

F

F

C.

S

F

F

F

F

D.

S

F

F

F

F

  1. What are the possible values of the l quantum number if the n quantum number is 3? A. 1, 2, 3 B. 0, 1, 2 C. 0, 1, 2, 3 D. -1, 0, +1 E. -3, -2, -1, 0, +1, +2, +
  2. Of the following elements, _______ has the most negative (i.s. largest) electron affinity? A. C B. B C. Be D. O
  3. Which of the following scientists performed the famous oil-drop experiment? A. J.J. Thompson B. R.A. Millikan C. Louis de Broglie D. Earnest Rutherford E. Neisl Bohr
  4. The electron configuration of the Al2-^ anion is ______. A. [Ne]3s 2 B. [Ne]3s 2 3p 1 C. [Ne]3s 2 3p 3 D. [Ne]3p 2 E. [Ne]3s 2 3p 6
  5. Which of the following ground state orbital diagrams violates the Pauli Principal? A.

1s 2s 2p

B.

2p C.

1s 2s 2p

D.

1s 2s 2p

  1. What is the energy, in Joules, of an electron in the n=2 orbit of the Bohr hydrogen atom? [R (^) H = 2.18x10 -18^ J] A. -2.42x10 -19^ J B. -2.18x10 -18^ J C. -5.45x10 -19^ J D. -1.36x10 -19^ J E. -5.45x10 -20^ J
  2. The chemical formula for Tin(IV) sulfite is A. Sn(SO 3 ) 2 B. SnSO 4 C. SnS 2 D. Sn(SO 4 ) 2 E. SnSO (^4)
  3. What is the formula weight of K 2 CO 3?

A. 122.21 amu B. 183.21 amu C. 136.21 amu D. 99.21 amu E. 138.21 amu

  1. How many grams of chromium are there in 85.60 grams of barium dichromate, BaCr 2 O 7? [FW(BaCr 2 O 7 ) = 353.27 amu] A. 58.3 g B. 37.4 g C. 25.2 g D. 22.5 g E. 52.2 g
  2. The electron configuration of the phosphide ion ( P3-^ ) is ______. Note: [Ne]=1s^2 2s^2 2p^6

A. [Ne]3s 2 B. [Ne]3s 2 3p 1 C. [Ne]3s 2 3p 3 D. [Ne]3p 2 E. [Ne]3s 2 3p 6

  1. Which one of the following ground state orbital diagrams violates Hund's Rule? A.

1s 2s 2p

B.

2s 2p C.

1s 2s 2p

D.

1s 2s 2p

  1. What are the formal charges on the atoms 1,2, and 3 below, respectively

N N O

A. +1, +1, 0 B. -1, -1, 0 C. 0, -1, +1 D. -1, 0, +1 E. -1, +1, 0

  1. Which of the following sets of quantum numbers refers to a 3d orbital? A. n =3, l = 3, ml = -1 B. n =4, l = 3, ml = -2 C. n =3, l = 2, ml = - D. n =4, l = 3, ml = -4 E. n =4, l = 1, ml = -
  2. The n = 5 to n = 3 transition in the Bohr hydrogen atom corresponds to the ________ of a photon with a wavelength of ______ nm. [R (^) H = 2.18x10-18^ J, h=6.626x10 -34J .s, c=3.0x10 8 m/s, 1m=10 9 nm] A. absorption, 657 B. absorption, 1282 C. emission, 657 D. emission, 1282 E. emission, 389
  1. Which of the following is the correct orbital diagram for sodium. A.

1s (^) 2s 2p (^) 3s 3p 4s B.

1s (^) 2s 2p (^) 3s 3p 4s C.

1s (^) 2s 2p (^) 3s 3p 4s D.

1s (^) 2s 2p 3s 3p 4s E.

1s (^) 2s 2p (^) 3s 3p 4s

  1. The Pauli exclusion principle states that A. Electrons can have either positive or negative spins B. No two electrons in an atom can have the same 4 quantum numbers C. Two electrons can share the same orbital if they have the same spin D. No two electrons in an atom can have the same spin E. Atoms with one or more unpaired electrons are paramagnetic
  2. Which of the following is the correct orbital diagram for Iron? A.

1s 2s 2p 3s 3p 4s 3d

B.

1s 2s 2p 3s 3p 4s 3d

C.

1s 2s 2p 3s 3p 4s 3d

D.

1s 2s 2p 3s 3p 4s 3d

E.

1s (^) 2s 2p 3s 3p 4s (^) 3d

  1. Which of the following is the correct Lewis structure for ClF 3?

A.

Cl

F

F

F

B.

Cl

F

F

F

C.

Cl

F

F

F

D.

Cl

F

F

F

E.

Cl

F

F

F

  1. What is the correct IUPAC name, using the Stock System, for Hg 2 SO 4?

A. Mercury(II) sulfide B. Mercury(II) sulfate C. Mercury (I) sulfite D. Mercury(I) sulfate E. Mercury(II) sulfite

  1. Which of the following is the correct Lewis electron-dot formula for the element indicated? A.

B

B.

O

C.

Mg

D.

S

E.

P

  1. What is the maximum number of electrons that can occupy the n = 4 shell? A. 6 B. 18 C. 8 D. 50 E. 32
  2. The electronic configuration of calcium is given by

A. 1s 2 2s 2 3s 2 3p 6 3d 6 B. 1s 2 2s 2 2p 6 3s 2 3p 6 3d 6 4s 2 C. 1s 2 2s 2 2p 6 3s 2 3p 6 4s 2 D. 1s 2 2s 2 2p 6 3s 2 3p 6 4s 2 4d 6

  1. What is the maximim number of electrons that can occupy an f sublevel? A. 2 B. 6 C. 10 D. 14 E. 18
  2. Using the trend learned in class, which of the following would you expect to have the smallest ionization energy? A. Ca B. K C. Ga D. Ge E. Se
  3. Arrange the following atoms in order of increasing radius. Mg, Ca, Ti, N

A. Mg < Ca < Ti < N B. N < Mg < Ti < Ca C. Ca < N < Ti < Mg D. Ti < N < Ca < Mg E. Mg < Ti < N < Ca

  1. Ammonia can be made by reaction of water with magnesium nitride. __ Mg 3 N 2 (s) + __ H 2 O(l) __ Mg(OH) 2 (s) + __ NH 3 (g) When the equation is properly balanced, the sum of the coefficients is A. 6 B. 8 C. 9 D. 12 E. 14
  1. In order to draw a Lewis structure of a species you must determine the total number of valence electrons in the species. How many valence electrons are there in ICl 4 -^? A. 34 B. 35 C. 36 D. 28 E. 8
  2. The first ionization energies of the elements _______ as you go from left to right across a period of the periodic table, and ________ as you go from the bottom to the top of a group in the table. A. increase, increase B. increase, decrease C. decrease, increase D. decrease, decrease