Chemistry 1310
Exam 1
February 10, 2023
A
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limited to the use of unauthorized materials and knowingly providing or obtaining unauthorized
assistance from another student. Any form of academic dishonesty will result in a zero on the
exam and possible expulsion from the course.
***You may remove the periodic table and scrap paper from the back of the exam***
!!!All materials must be turned in at the conclusion of the exam!!!
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1. (3 pts) How many protons does an electrically neutral mercury – 202 atom have?
a) 80 protons
e) 282 protons
b) 122 protons
c) 200.59 protons
d) 202 protons
2. (3 pts) How many electrons does an electrically neutral mercury – 202 atom have?
a) 80 electrons
d) 202 electrons
b) 122 electrons
e) 282 electrons
c) 200.59 electrons
3. (3 pts) How many electrons does a silver ion have?
a) 45 electrons
d) 48 electrons
b) 46 electrons
e) 49 electrons
4. (3 pts) How many neutrons does an
a) 21 neutrons
e) 53 neutrons
b) 24 neutrons
c) 47 electrons
53
Cr 3+ atom have?
c) 29 neutrons
d) 50 neutrons
5. (3 pts) How many electrons does an 53Cr 3+ atom have?
a) 21 electrons
e) 53 electrons
b) 24 electrons
c) 29 electrons
d) 50 electrons
6. (3 pts) How many orbitals are contained in the third principal level (n = 3) of a given atom?
a) 10
b) 12
c) 1
d) 9
e)6
7. (3 pts) How many subshells are there in the shell with n = 5?
a) 4
b)5
c) 10
d) 35
e) 25
8. (3 pts) How many valence electrons does an atom of In possess?
a) 1
b) 2
c) 3
d) 11
e) 13
9. (3 pts) What are four possible quantum numbers for one of the valence electrons in tin?
a) n = 5, l = 0, ml = 0, ms = -½
c) n = 4, l = 2, ml = 0, ms = +½
e) n = 5, l = 1, ml = -2, ms = +½
b) n = 5, l =2, ml = -1, ms = +½
d) n = 4, l = 3, ml = +1, ms = -½
10. (3 pts) The electron configuration of copper, using core notation, is…
a) [Ar] 4s2 3d9
d) [Kr] 4s2 4p6 3d9
b) [Ar] 4s1 3d10
e) [Kr] 4s2 3d9
c) [Kr] 4s1 3d10
11. (3 pts) Choose the ground state electron configuration for Rf2 +.
a) [Rn] 7s2 6d2
d) [Rn] 5f14 6d2
b) [Rn] 7s2
e) [Rn] 7s2 6d4
c) [Rn] 6f14 7d2
12. (3 pts) Of the following, which element has the highest first ionization energy?
a) Br
b) Sr
c) Te
d) K
e) Ba
13. (3 pts) Which of the following is isoelectronic with Sr2+?
a) Ca2+
b) Zr2+
c) Kr
d) Sr
e) Zr2-
14. (3 pts) Predict which species has the largest atomic/ionic radius…
a) P3-
b) S2-
c) Cl-
d) Ar
e) K+
15. (3 pts) Of the following elements, which is most metallic in character?
a) Sn
b) Ra
c) In
d) Cl
e) Ba
16. (3 pts) Calculate the number of atoms in 91.690 g of Sn.
a) 7.724×10-7 atoms
d) 4.651×1020 atoms
b) 7.724×107 atoms
e) 4.651×1017 atoms
c) 4.651×1023 atoms
17. (3 pts) Calculate the mass percent composition of oxygen for FeCO3 (siderite).
a) 48.20 %
e) 21.55 %
b) 13.81 %
c) 51.80 %
d) 41.43 %
18. (3 pts) Determine the number of moles of oxygen atoms in 2.20×10-2 mol H2CO3.
a) 2.20×10-2 mol
d) 22 mol
b) 7.33×10-3 mol
e) 1.10×10-2 mol
c) 6.60×10-2 mol
Please name the following species;
19. (3 pts) NiSO3
a) nickel I sulfate
d) nickel I sulfite
b) nickel II sulfate
e) nickel II sulfite
c) nickel sulfite
20. (3 pts) C4H10
a) tetrane
d) propane
b) ethane
e) methane
c) butane
21. (3 pts) Cd(ClO2)2
a) cadmium hypochlorite
d) cadmium perchlorate
b) cadmium chlorite
e) cadmium chloride
c) cadmium chlorate
b) phosphorous acid
e) perphosphoric acid
c) phosphitic acid
22. (3 pts) H3PO3(aq)
a) phosphoric acid
d) hypophosphoric acid
23. (3 pts) HgI2
a) mercury II iodide
d) mercury diodide
b) mercury iodide
e) mercuous iodide
c) mercury I iodide
b) chromium nitride
e) chromium III nitride
c) chromium II nitride
b) nitrogen pentoxide
e) nitrogen V oxide
c) nitrogen V pentoxide
24. (3 pts) CrN
a) chromium II nitrogen
d) chromium III nitrogen
25. (3 pts) N2O5
a) nitrogen oxide
d) dinitrogen pentoxide
26. (3 pts) C7H15CO2H
a) octanol
d) heptyl amine
b) heptanol
e) octanoic acid
c) heptanoic acid
27. (3 pts) P4O10
a) tetraphosphorus decoxide
d) tetraphosphorus oxide
b) phosphorus decoxide
e) phosphoric oxide
c) phosphorus oxide
28. (3 pts) AgNO3
a) silver I nitrate
d) silver II nitrite
b) silver nitrate
e) silver nitrite
c) silver I nitrite
b) dichromitic acid
e) chromium oxide
c) hydrogen chromate
b) carbonic acid
e) acetic acid
c) ethanol
b) hypoiodous acid
e) periodous acid
c) iodous acid
29. (3 pts) H2Cr2O7(aq)
a) chromic acid
d) dichromic acid
30. (3 pts) HC2H3O2(aq)
a) methanoic acid
d) formic acid
31. (3 pts) HIO3(aq)
a) iodic acid
d) periodic acid
Please provide the correct molecular formulae for the following species;
32. (3 pts) Manganese II nitrite
a) MnNO2
d) Mn2NO
b) Mn(NO2)2
e) Mn(NO)2
c) Mn2(NO2)2
b) HBrO2(aq)
e) HBrO5(aq)
c) HBrO3(aq)
33. (3 pts) Bromous acid
a) HBrO(aq)
d) HBrO4(aq)
34. (3 pts) Hydrogen phosphate ion
a) HPO32ˉ
d) H2PO4ˉ
b) H2PO3ˉ
e) H2PO42ˉ
c) HPO42ˉ
b) H2SO3(aq)
e) HSO3(aq)
c) H2SO4(aq)
35. (3 pts) Hydrosulfuric acid
a) H2S(aq)
d) HSO4(aq)
Useful Constants and Relationships
𝐸 = ℎ𝜈
𝐾𝐸 = 𝐸𝑙𝑖𝑔ℎ𝑡 − 𝛷
NA = 6.022 x 1023 mol-1
R = 0.08206 (L•atm)/(mol•K)
R = 8.314 J/(mol•K)
1 L•atm = 101.3 J
8
c = 2.998 x 10 m/s
h = 6.626 x 10-34 J•s
1 W = 1 J/s
ℛ = 1.097 × 107 𝑚−1
𝑃𝑎 = 𝜒𝑎 𝑃𝑡𝑜𝑡𝑎𝑙
𝑢𝑟𝑚𝑠 = √
3𝑅𝑇
𝑀
𝐶𝑖 𝑉𝑖 = 𝐶𝑓 𝑉𝑓
𝑃𝑠𝑜𝑙𝑢𝑡𝑖𝑜𝑛 =
𝑛𝑠𝑜𝑙𝑣𝑒𝑛𝑡
𝑃°
𝑛𝑠𝑜𝑙𝑣𝑒𝑛𝑡 + 𝑖 ∙ 𝑛𝑠𝑜𝑙𝑢𝑡𝑒 𝑠𝑜𝑙𝑣𝑒𝑛𝑡
𝑃𝑡𝑜𝑡𝑎𝑙 = 𝑋𝐴 𝑃°𝐴 + 𝑋𝐵 𝑃°𝐵
𝛱 = 𝑖 ∙ 𝑀𝑜𝑙𝑎𝑟𝑖𝑡𝑦 × 𝑅𝑇
∆𝑇 = 𝑖 ∙ 𝑚𝑜𝑙𝑎𝑙𝑖𝑡𝑦 ∙ 𝐾
(𝑃 +
𝑎𝑛2
) (𝑉
𝑉2
− 𝑛𝑏) = 𝑛𝑅𝑇
𝑞 = 𝐶∆𝑇
∆𝐸 = 𝑞 + 𝑤
𝑤 = −𝑃∆𝑉
𝐻 = 𝐸 + 𝑃𝑉
𝑞 = 𝑛∆𝐻
𝑙𝑛
𝑃2 −∆𝐻𝑣𝑎𝑝 1
1
( − )
=
𝑃1
𝑅
𝑇2 𝑇1
c = λν
𝜆𝑑𝑒 =
ℎ
𝑚v
𝛥𝑥 × 𝑚∆v ≥
ℎ
4𝜋
1
1
1
= −ℛ ( 2 − 2 )
𝜆
𝑛𝑓
𝑛𝑖