Name: KEY
Chemistry: Fall Semester Review 2015
Multiple Choice: Identify the letter of the choice that best completes the statement or answers the question.
____
1. Most of the mass of an atom is found
a. in the electron cloud.
c. in the number of protons.
b. in the nucleus.
d. in the outer region of an atom.
____ 2. A spherical electron cloud surrounding an atomic nucleus would best represent
a. an s orbital.
c. a combination of px and py orbitals.
b. a px orbital.
d. a combination of an s and a px orbital.
____ 3. For an electron in an atom to change from the ground state to an excited state,
a. energy must be released.
b. energy must be absorbed.
c. radiation must be emitted.
d. the electron must make a transition from a higher to a lower energy level.
____ 4. The number of atoms in 1 mole of hydrogen is
a. 6.022 x 1022.
b. 6.022 x 1023.
c. 5.022 x 1022.
d. 5.022 x 1023.
____ 5. Among the d-block elements, as atomic radii decrease, electronegativity values
a. remain constant. b. increase.
c. decrease.
d. drop to zero.
____ 6. The elements that border the zigzag line in the periodic table are
a. inactive.
b. metals.
c. metalloids.
d. nonmetals.
____ 7. The liter is defined as
a. 1000 m3.
b. 1000 cm3.
c. 1000 g3.
d. 1000 c3.
____ 8. What one number identifies an element?
a. mass number
c. number of protons
b. number of neutrons
d. number of nucleons
_C (b)_ 9. Which two compounds are examples of the law of multiple proportions?
a. FeCl3 and Fe2(SO4)3
c. CO and CO2
b. O2 and O3
d. FeCl2 and Fe(NO3)2
____ 10. The energy of a photon, or quantum, is related to its
a. mass.
b. speed.
c. frequency.
d. size.
____ 11. In a row in the periodic table, as the atomic number increases, the atomic radius generally
a. decreases.
c. increases.
b. remains constant.
d. becomes unmeasurable.
____ 12. Within a group of elements, as the atomic number increases, the atomic radius
a. increases.
c. decreases regularly.
b. remains approximately constant.
d. decreases, but not regularly.
____ 13. Argon (atomic number 18 and mass number 40) has ____ protons in its nucleus.
a. 22
b. 9
c. 40
d. 18
____ 14. Written in scientific notation, the measurement 0.000 065 cm is
a. 65 x 10–4 cm.
c. 6.5 x 10–6 cm.
b. 6.5 x 10–5 cm.
d. 6.5 x 10–4 cm.
____ 15. Atoms of the same element that have different masses are called
a. moles.
b. isotopes.
c. nuclides.
d. neutrons.
____ 16. To calculate the density of an object,
a. multiply its mass and its volume.
c. divide its volume by its mass.
b. divide its mass by its volume.
d. divide its mass by its area.
____ 17. A vertical column of blocks in the periodic table is called a(n)
a. group.
b. period.
c. property.
d. octet.
M/C Answers:
If A = 1
B=2
C=3
D=4
then questions
totals for:
1 thru 8 = 17
10 thru 16 = 15
17 thru 26 = 23
.
____ 18. A nuclear particle that has about the same mass as a proton, but with no electrical charge, is called a(n)
a. nuclide.
b. neutron.
c. electron.
d. isotope.
____ 19. Which orbitals are characteristic of the lanthanide elements?
a. d orbitals
b. s orbitals
c. f orbitals
d. p orbitals
____ 20. Which of the following observations is quantitative?
a. The liquid turns blue litmus paper red.
c. The liquid tastes bitter.
b. The liquid boils at 100ºC.
d. The liquid is cloudy.
____ 21. A horizontal row of blocks in the periodic table is called a(n)
a. group.
c. family.
b. period.
d. octet.
____ 22. A line spectrum is produced when an electron moves from one energy level
a. to a higher energy level.
b. to a lower energy level.
c. into the nucleus.
d. to another position in the same sublevel.
____ 23. Elements to the "top side" of the stairs on the periodic table (p-block elements) have properties most
associated with
a. gases.
c. metals.
b. nonmetals.
d. metalloids.
____ 24. Cesium, atomic number 55, has the electron configuration [Xe] 6s1. In what period is cesium?
a. Period 2
b. Period 6
c. Period 1
d. Period 20
____ 25. The ionization energies for removing successive electrons from sodium are 496 kJ/mol, 4562 kJ/mol, 6912
kJ/mol, and 9544 kJ/mol. The great jump in ionization energy after the first electron is removed indicates
that
a. sodium has four or five electrons.
b. the atomic radius has increased.
c. a d-electron has been removed.
d. the noble gas configuration has been reached.
____ 26. Zirconium, atomic number 40, has the configuration [Kr]5s24d2 . To what group does zirconium belong?
a. Group 2
b. Group 3
c. Group 4
d. Group 5
Short Answer
27. a) Which has a longer wavelength, green or yellow light?
b) Which has a higher frequency an X ray or microwave?
YELLOW
X-RAY
c) Which travels at a greater speed, ultraviolet or infrared light? SAME
28. Describe the differences between qualitative and quantitative observations.
29. a) What are the valence electrons?
30. Distinguish between precision and accuracy.
b) Where are valence electrons located?
31. What is the relationship between isotopes, mass number, and neutrons?
Isotopes have different mass numbers depending upon the amount of neutrons.
32. Which elements are most likely to undergo the same kinds of reactions, those in a group or a period?
Explain.
Groups (family) – same number of valence electrons
Problem
33. What is the percent error for a mass measurement of 0.63 grams, given the correct value is 0.70 grams?
10%
34. A student measures the mass of a beaker filled with corn oil. The mass reading averages 215.6 g. The mass
of the beaker is 110.4 g.
a) What is the mass of the corn oil?
b) What is the density of the corn oil if its volume is 114 cm3?
0.922 g/cm3
35. How many significant figures are there in each of the following measured values?
a) 6.002 cm
__________
b) 0.0020 m
__________
c) 10.0500 g
__________
d) 7000 kg
__________
e) 250. kg
__________
Total = 16
36. Given calculations with the calculator answer, write the answer to the appropriate number of significant
figures.
a) 13.0 + 46.1 = 59.1
The answer should be 59.1
b) 460 x 120 = 55200
The answer should be
55 000
c) 56.1 - 35 = 21.1
The answer should be
21
d) 32 / 2 = 16
The answer should be
20
37. Complete the following conversions - SHOW ALL WORK!!!!
a) 525 nanograms =
5.25 x 10-10
b) 0.25 megaliters =
2.5 x 105
kilograms
liters
38. Complete and balance the following nuclear equations
a)
Es + B → 2
n+
260
Rf
104
b)
Po → He +
205
Pb
82
39. Determine the mass in grams of each of the following
a) 3.00 mole Al
80.94 grams Al
b) 2.56 x 1024 atoms Li
29.5 grams Li
40. The half-life of polonium-210 is 138.4 days. How many milligrams of polonium-210 remains after 415.2 days,
if you start with 2.0 mg of the isotope?
0.25 mg
41. a) Which element has the following electron configuration: [Ar] 4s2 3d10 4p3? _____________
a) What are the quantum numbers for this element?
4, 1, 1 , + ½
b) How many electrons are in each atom of this element? ________
c) Write the orbital notation for this atom? ARROWS
d) How many unpaired electrons does this atom have?
e) What is the highest occupied energy level?
3
4
f) How many outer-shell electrons (valence electrons) does the atom contain?
5
28
g) How many inner-shell electrons (core electrons) does the atom contain?
42. List the following atoms in order of increasing electron affinity: Al, Ca, Ne, O
Ne < Ca < Al < O
43. Explain why within a family such as the halogens, the ionic radius increases as the atomic number increases.
Within a family, ionic radius increases as atomic number increase due to
INCREASE SHIELDING.
44. Choose the element with the greatest first ionization energy:
Nitrogen or aluminum
Beryllium or Magnesium
Lithium or Helium
Xenon or Iodine
Sulfur or Oxygen
Oxygen or Fluorine
45. What are the two factors that will affect periodicity? (Hint: Coulombic Attraction)
1)
Effective Nuclear Charge (ENC) – strength (amount) of charge
2)
Shielding Effect – distance between the +/- charges
46. What is the formula mass of tetrethyl lead, Pb(C2H5)4?
323.48 g/mole
47. Complete the following chart
Element
or Ion
24
Atomic
Number
Mg
Mass
Number
Charge
24
12
Cl -1
17
0
17
Ca +2
-1
18
14
20
18
P -3
Au
Electrons
6
27
13 Al
40
Neutrons
12
12
C
6
35
Protons
15
79
0
118
31
-3
15P
Neutrons: ______
48. How many protons, electron and neutrons are in the following ion?
Protons: ________
Electrons: ________
TOTAL = 49
49. Fill in the missing information in the table below. Uranium-238
Nuclear
Notation
Hyphen
Notation
Atomic
Number
Proton
Number
Mass
Number
Electron
Number
92
238
92
Neutron
Number
4.3 x 10 22 atoms NaCl
50. How many atoms are there in 4.2 grams of NaCl?
14.98 gram CH4
51. How many grams are there in 5.62 x 1023 atoms of CH 4?
52. A) What are diatomic molecules? _____________________________________________
b) List the seven diatomic molecules: __________________________________________
53. Almost all commercially available microwave ovens employ radiation with a frequency of
2.45 x 10 9 /sec. Calculate the wavelength of this radiation.
 = 0.122 meters
54. What are the quantum numbers for the following elements
a) Ca:
4, 0, 0, - ½
b) Br:
4, 1, 0, - ½
55. a) Write the electron configuration for Nitrogen: ___________________________________________
b) How many valence electrons does Nitrogen have? ______
56. A compound contains 13.5 g Ca, 10.8 g O and 0.675 g H. What is the empirical formula?
Ca(OH)2 = CaO2H2
57. Calculate the percent water if 6 grams of the hydrate and 5.2 grams of the anhydrate are present?
13.3 % H2O
58. Write the proper name for : Fe3(PO4)2 • 7H2O :
Iron (II) phosphate heptahydrate
59. Write the formula for diboron tetrabromide: B2Br4
60. Write the formula for: copper (II) chloride:
61. Write the proper chemical name: SnBr2:
CuCl2
Tin (II) bromide