Name ____________________________
Chemistry I-H
Midterm Study Guide
1. ______ The element curium (Z = 242, A = 96) can be produced by positive-ion bombardment when an alpha particle
collides with which of the following nuclei? Recall that a neutron is also a product of this bombardment.
a) 249
b) 241
c) 241
d) 239
e) 239
92 U
98 Cf
94 Pu
94 Pu
95 Am
2. ______ The cesium-131 nuclide has a half-life of 30 years. After 90 years, about 6 g remains. The original mass of the
cesium-131 sample is closest to
a) 30 g
b) 40 g
c) 50 g
d) 60 g
e) 70 g
3. ______ The atomic particle having a mass of 0 amu and a charge of -1 is
a) an electron
b) a neutron
c) an alpha particle
d) a proton
4. ______ True or false? Nuclear fusion uses heavy nuclides such as
a) True
b) False
235
92
e) none of these
U as fuel.
5. ______ Which of the following statements is/are true?
I.
John Dalton provided the first experimental support for the atom.
II.
Ernest Rutherford proved the existence of a nucleus by shooting positively charged particles at a thin
gold-foil sheet.
III.
J. J. Thompson proved that electrons travel in elliptical orbits around the nucleus.
IV.
Energy in an atom is quantized, so when electrons fall to their ground state, white light can be observed.
a) I, II
b) I, III
c) I, II, III
d) II, IV
e) All of the above statements (I – IV) are correct.
6. ______ Which atomic particle determines the chemical behavior of an atom?
a) proton
b) electron
c) neutron
d) nucleus
e) none of these
7. ______ An element's most stable ion forms an ionic compound with chlorine having the formula XCl2. If the ion of
element X has a mass of 89 and 36 electrons, what is the identity of the element, and what is the neutron count?
a) Kr, 53 neutrons
b) Kr, 55 neutrons
c) Se, 55 neutrons d) Sr, 51 neutrons e) Rb, 52 neutrons
8. Identify an element for each of the following situations:
a. The heaviest noble gas
b. The transition metal that has 24 electrons as a +3 ion
c. The halogen in the third period
d. The alkaline earth metal that has 18 electrons as a stable ion
9. ______ How many electrons are present in a tin atom with a mass number of 120?
a) 50
b) 120
c) 170
d) 70
e) 6.02  1023
10. ______ The number of protons in the nucleus of an atom is called its
a) mass number
b) valence
c) isotope number
d) atomic number
e) none of these
11. ______ Which of the following elements is an alkali metal?
a) Ca
b) Cu
c) Fe
d) Na
e) Sc
12. ______ Which of the following elements is most similar to chlorine?
a) H
b) He
c) Na
d) Hg
e) Br
13. ______ The form of EMR that has more energy per photon than ultraviolet rays but less energy per photon than gamma
rays is
a) microwaves
b) radio waves
c) X rays
d) infrared rays
e) none of these
-214. ______ Which color of visible light has the most energy per photon?
a) violet
b) blue
c) green
d) yellow
e) red
15. ______When an electron in the ground state absorbs energy, it goes to a(n) ______________ state.
a) excited
b) lower
c) frenetic
d) ionic
e) stable
16. ______The probability map for an electron is called
a) an orbit
b) a photon
c) an orbital
d) an electron configuration
e) none of these
17. ______As the principal energy level increases in an atom's orbitals, the average distance of an electron energy level from
the nucleus ______________.
a) increases
b) decreases
c) stays the same
d) varies
e) none of these
18. ______A given set of f orbitals consists of ______________ orbital(s).
a) 1
b) 3
c) 5
d) 7
e) 9
19. ______The maximum number of electrons allowed in the p sublevel of the third principal level is
a) 1
b) 2
c) 3
d) 6
e) 8
20. ______The maximum number of electrons allowed in the fourth energy level is
a) 2
b) 4
c) 8
d) 18
e) 32
21. ______Phosphorus has how many electrons in its outermost principal energy level?
a) 1
b) 2
c) 3
d) 5
e) 15
22. ______The number of unpaired electrons in a nitrogen atom is
a) 1
b) 2
c) 3
d) 4
e) 5
23. ______When moving down a group (family) in the periodic table, the number of valence electrons
a) remains constant;
b) increases by 2 then 8 then 18 then 32;
c) doubles with each move
d) decreases regularly;
e) changes in an unpredictable manner
24. ______1s22s22p63s23p64s23d7 is the electron configuration for which of the following atoms?
a) Ca
b) Fe
c) Cr
d) Ar
e) Co
25. ______The electron configuration for manganese is
a) [Ar] 3d7
b) 1s22s22p63s13d6
c) [Ar] 4s23d5
d) 1s22s22p63s23d4
26. ______The element with the electron configuration [Kr] 5s24d105p3 is
a) As
b) Sb
c) Nb
d) Pr
e) none of these
27. ______Which of the following is ranked in order of largest to smallest atomic radius?
a) Rb > Mn > S > Ge > F
b) F > S > Ge > Mn > Rb
c) Mn > Rb > F > S > Ge
d) Rb > Ge > Mn > F > S
e) Rb > Mn > Ge > S > F
28. ______Which of the following atoms has the highest ionization energy?
a) Na
b) Mg
c) Si
d) P
e) Cl
29. ______Which of the following has the smallest atomic radius?
a) N
b) F
c) Br
d) Cl
e) S
e) [Ar] 4s24p5
-330. ______Order the elements S, Cl, and F in terms of increasing ionization energy.
a) S, Cl, F
b) Cl, F, S
c) F, S, Cl
d) F, Cl, S
e) S, F, Cl
31. ______Which of the following bonds does not have a dipole moment?
a) N-H
b) O-H
c) F-H
d) H-H
e) S-H
32. ______How many lone pairs of electrons are in the Lewis structure for ammonia, NH3?
a) 0
b) 1
c) 2
d) 3
e) 4
33. Draw the Lewis structure for NI3.
34. ______Which of the following molecules are polar? (Check all that apply.)
a) CH3OH
b) CH4
c) H2O
d) C2H6
35. ______Which of the following species exhibit hydrogen bonding? (Check all that apply.)
a) HBr
b) NO3–
c) H2O
d) SF4
e) KrCl4
f) I3–
Consider the following compounds:
CO
NH3
CO2
CH4
H2
36. ______Which compound has the highest boiling point?
a) CO
b) NH3
c) CO2
d) CH4
e) At least two of the above compounds have equally high
boiling points.
37. ______Which of the following has the highest melting temperature?
a) H2O
b) CO2
c) S8
d) MgF2
e) P4
38. ______The most electronegative element of those listed is
a) Rb
b) Cs
c) Fr
d) K
e) Li
39. ______Which of the following statements about the periodic table is false?
a) Elements in the same column have similar reactivities because their valence electrons tend to be located in
the same types of orbitals.
b) A series of ions that are isoelectronic must have the same electron configuration.
c) The atomic size of the elements increases going across a period from left to right because the number of
electrons increases, so they are located further from the nucleus.
d) It takes more energy to remove an electron from lithium than from cesium because the valence electrons in
lithium are located closer to the nucleus.
e) Fluorine is the most electronegative element due to its size and nuclear charge.
40. ______The correct name for LiCl is
a) lithium monochloride
b) lithium(I) chloride
c) monolithium chloride
41. ______The correct name for FeO is
a) iron oxide
b) iron(II) oxide
d) lithium chloride
e) monolithium monochloride
c) iron(III) oxide
d) iron monoxide
e) iron(I) oxide
-442. ______What is the formula for sulfur trioxide?
a) SO
b) SO2
c) SO3
d) S3O
43. ______The correct name for P2O5 is
a) phosphorus(II) oxide
d) diphosphorus pentoxide
e) S3O3
b) phosphorus(V) oxide
e) phosphorus pentoxide
44. ______Titanium(IV) oxide has the formula
a) Ti4O
b) TiO4
c) Ti(IV)O
d) TiO2
c) diphosphorus oxide
e) Ti4O2
45. ______The correct name for an aqueous solution of H2SO4 is
a) sulfurous acid
b) hydrosulfurous acid
c) sulfuric acid
e) none of these
d) hydrosulfuric acid
46. ______The correct name for an aqueous solution of H3PO4 is
a)hydrophosphoric acid
d)
hydrophosphorus acid
b)phosphorous acid
e)
phosphoric acid
c)phosphate acid
47. ______ The correct name for an aqueous solution of HCl is
a) chloric acid
b) hydrochloric acid
c) hypochloric acid
perchloric acid
d) hypochlorous acid
e)
48. ______The formula for the compound formed from ammonium and sulfate ions is
a) NH4SO4
b) (NH4)2SO4
c) NH4(SO4)2
d) (NH4)3SO4
e) none of these
49. ______The name for the acid HNO2 is
a) nitrous acid
b) nitric acid
acid
50. ______The name for Al(OH)3 is
a) aluminum(III) hydroxide
b) aluminum trihydroxide
c) aluminum hydroxide
c) hydronitrous acid
d) hydronitric acid
e) hydrogen nitrite
d) monaluminum trihydroxide
e) aluminum(I) hydroxide
51. ______The name for Ba(NO3)2 is
a) barium dinitrate
b) barium(II) nitrate
d) barium(I) nitrate
e) barium nitrate
c) barium nitrite
52. ______True or false? The greater the difference in electronegativity between two bonded atoms, the more polar the
bond.
a) True
b) False
53. ______Rank the following bonds from least polar to most polar:
Si-Cl
a)
b)
c)
S-Cl, P-Cl, Mg-Cl, Si-Cl
P-Cl, S-Cl, Si-Cl, Mg-Cl
Mg-Cl, Si-Cl, P-Cl, S-Cl
P-Cl
Mg-Cl S-Cl
d)
e)
Mg-Cl, S-Cl, P-Cl, Si-Cl
S-Cl, P-Cl, Si-Cl, Mg-Cl
54. ______Which of the following bonds would be the most polar without being considered ionic?
a) Mg-O
b) C-O
c) O-O
d) Si-O
e) N-O
-555. ______ A sample of platinum is found to have 3.42% Pt-193, 0.70% Pt-197 and 95.88% Pt-195. Calculate the
average atomic mass of this element.
a) 193.44
b) 195.08
c) 195.00
d) 194.95
56. ______Which type of electromagnetic energy has the shortest wave length?
a. Visible light
b. Radio waves
c. Ultraviolet (UV) radiation
d. Gamma radiation
57. ______ The mathematical equation c= λf means that as the wavelength (λ) increases, the frequency (f) decreases.
The equation E = hf means that as frequency increases, energy increases. Using this information and the
reference tables, which color of visible light has the least energy?
a. Red
b. Yellow
c. Green
d. Violet
e. Orange
58. ______ Using the Bohr model diagram, if an electron drops from the shells, n=6 to n=2, what type of electromagnetic
radiation is emitted?
a. Ultraviolet (UV)
b. Visible
c. Infrared (IR)
d. Radiowaves
e. Gamma
59. ______ This equation represents the alpha decay of U-238:
U 
238
92
4
He
+ X
2
What is the mass number of the element represented by X?
A) 88;
B) 228;
C) 90;
D) 242;
E) 234
60. ______ What is the oxidation number (charge) of potassium in K2CrO4?
A) +1;
B) +2;
C) +4;
D) +6;
E) -2
61. ______ Consider these four element – Fe, Ge, Rb, O. Arrange them in order of increasing electronegativity.
A) Rb < Fe < Ge < O;
B)
Ge < Fe < Rb < O;
A) Rb < Ge < O < Fe;
D) O < Ge < Fe < Rb;
E) Rb < O < Fe < Ge
62. ______ Which of the following sets of quantum numbers is NOT valid?
a. (1, 0, 0, +½)
b. (2, 2, 0, -1/2)
c. (3, 2, -1, +1/2)
d. (4, 1, 0, -1/2)
63. ______ Which of the following is the correct set of quantum number for the 21st electron of Xenon?
a. (6, 2, 1, -1/2) b. (4, 2, -2, +1/2)
c. (3, 2, -2. +1/2)
d. (5, 1, 1, -1/2)
64._______________________ How many total atoms are in exactly 1.000 microgram of pure, distilled water?
65. _______________________ How many grams of sodium chloride would you need in order to have the same number of
sodium ions as you have in 43.9 grams of sodium peroxide?
66. _______________________ How many liters of gas do you have if you have 80.0 grams of carbon dioxide?
(Assume STP)
-667. _______________________ If you had the same volume of gas at the same STP, but the gas is changed to helium gas,
how many more moles of gas would you have?
23
68. _______________________ A certain compound is composed of 1.505 x 10 atoms of potassium, 13.0 grams of
chromium, and 0.875 moles of oxygen. What is the simplest whole number mole ratio of
elements in this compound?
69. _______________________ How many ions (total of both cations and anions) are there in 80.5 grams of barium
phosphate?
70. (a) __________________ Calculate the density of: (a) an object that has a mass of 3.9 g and a volume of 7.2
mL and (b) an object with a mass of 250.0 g that when placed in a graduated
cylinder containing 21.6 mL caused the water level to rise to 59.7 mL.
(b) __________________
71. Fill in the chart below.
Element
Electron Configuration
Noble Gas
Configuration
Lewis Dot Structure
# Half-filled
orbitals
Cobalt
1s22s22p63s23p64s23d104p4
[Ne] 3s23p3
72. Which of the following: (circle the correct answer)
A.
B.
C.
D.
Has the greatest electronegativity:
Has the greatest ionization energy:
Has the smallest atomic radius:
Is the most reactive:
Na or Li
Ca or Mg
Ca or Mg
Al or Sr
K or Ca
Rb or Cs
Rb or Cs
K or Mg
F or Ne
P or S
P or S
P or O
C or Si
Cl or F
Cl or F
Ne or Si
Answer Key
1.
2.
3.
4.
5.
6.
7.
8.
9.
10.
11.
12.
13.
14.
15.
16.
17.
18.
19.
20.
21.
22.
23.
24.
25.
26.
27.
28.
29.
30.
31.
32.
33.
e
c
a
b
a
b
d
a. Rn
b. Co
c. Cl
d. Ca
a
d
d
e
c
a
a
c
a
d
d
e
d
c
a
e
c
b
e
e
b
a
d
b
..
.
.
. I .
..
.
. I —
..
34.
35.
36.
37.
38.
39.
40.
41.
42.
43.
44.
45.
..
—
.
N — I .
..
..
a, c
c
b
d
e
c
d
b
c
d
d
c
46.
47.
48.
49.
50.
51.
52.
53.
54.
55.
56.
57.
58.
59.
60.
61.
62.
63.
e
b
b
a
c
e
a
e
d
d
d
a
b
e
a
a
b
c
64. How many total atoms are in exactly 1.000 microgram of pure, distilled water?
1.000 x 10-6 g cpd.(1 mol cpd./18.0 g. cpd.)(3 mol atoms / 1 mol cpd.)(6.02 x 1023 atoms/1 mol atoms)
= 1.00 x 1017 atoms total
65. How many grams of sodium chloride would you need in order to have the same number of sodium ions as you have in
43.9 grams of sodium peroxide?
1 mol Na2O2
2 mol Na
1 mol NaCl
x --------------- x -------------- x -------------- x
78.0 g Na2O2
1 mol Na2O2
1 mol Na
43.9 g Na2O2
58.5 g NaCl
--------------1 mol NaCl
= 65.9 g NaCl
66. How many liters of gas do you have if you have 80.0 grams of carbon dioxide? (Assume STP)
80.0 g CO2 (1 mol CO2 / 44.0 g CO2) (22.4 L CO2 / 1 mol CO2) = 40.7 L
67. If you had the same volume of gas at the same STP, but the gas is changed to helium gas, how many more moles of gas
would you have?
no more moles; 22.4 L per mole is a constant @STP for any gas
23
68. A certain compound is composed of 1.505 x 10 atoms of potassium, 13.0 grams of chromium, and 0.875 moles of
oxygen. What is the simplest whole number mole ratio of elements in this compound?
23
K 1.505 x 10 atoms / 6.02 x 1023 = 0.250 mol K
Cr 13.0 g / 52.0 g/mol = 0.250 mol Cr
K : Cr : O
K2Cr2O7
=>
&
0.875 mol O
0.250 : 0.250 : 0.875 (divide all by 0.250) = 1: 1: 3.5 => 2 : 2 : 7
or potassium dichromate
69. How many ions (total of both cations and anions) are there in 80.5 grams of barium phosphate?
80.5 g cpd
1 mol cpd
5 mols ions
6.02 x 10 23 ions
x --------------- x -------------- x --------------------------601.9 g cpd
1 mol cpd
1 mols ions
= 4.03 x 1023 ions
70. (a)
0.54 g/mL
Calculate the density of: (a) an object that has a mass of 3.9 g and a volume of 7.2
mL and (b) an object with a mass of 250.0 g that when placed in a graduated
cylinder containing 21.6 mL caused the water level to rise to 59.7 mL.
(b)
6.56 g/mL
(a) D = M / V = (3.9 g) / (7.2 mL) = 0.54 g/mL
(b) D = M / V = 250.0 g / (59.7mL – 21.6 mL) = 6.56 g/mL
71. Fill in the chart below.
Element
Electron Configuration
Noble Gas
Configuration
Cobalt
1s22s22p63s23p64s23d7
[Ar] 4s23d7
3
Selenium
1s22s22p63s23p64s23d104p4
[Ne] 3s23p3
2
Phosphorous
1s22s22p63s23p3
[Ne] 3s23p3
3
Lewis Dot Structure
# Half-filled
orbitals
72. Which of the following: correct answer is BOLDED
A. Has the greatest electronegativity:
Na or Li
K or Ca
F or Ne
C or Si
B. Has the greatest ionization energy:
Ca or Mg
Rb or Cs
P or S
Cl or F
C. Has the smallest atomic radius:
Ca or Mg
Rb or Cs
P or S
Cl or F
D. Is the most reactive:
Al or Sr
K or Mg
P or O
Ne or Si