Chemistry Benchmark 1 Review Completion Complete each statement. 1. Chemistry is the study of _____________________ and the changes that it undergoes. 2. A(n) ______________________ is a set of controlled observations that test the hypothesis. 3. 100.00 meters 50.000 centimeters 1.0000 kilometer = ____________________ meters. 4. A process that involves one or more substances changing into new substances is known as a ____________________ change. 5. Cutting a sheet of paper is an example of a ____________________ change. 6. A ____________________ property enables a substance to combine with or change into one or more substances. 7. Sugar is a ____________________ form of matter with a definite shape and volume. 8. A ____________________ is a subatomic particle that has mass nearly equal to that of a proton, but it carries no electrical charge. 9. Atoms with the same number of protons but different number of neutrons are called ____________________. 10. An alpha particle is _____________________ charged with two protons and neutrons. 11. Democritus believed that matter is made up of tiny individual particles known as a(n) ____________________. 12. The number of protons in an atom is called the ____________________ of the element. 13. The ____________________ principle states that a maximum of two electrons may occupy a single atomic orbital, but only if the electrons have opposite spins. 14. The arrangement of electrons in an atom is called the ____________________ of an atom. 15. The group 2A elements are known as ____________________ metals. 16. Elements that have physical and chemical properties of both metals and nonmetals are known as ____________________. Short Answer 17. Explain the difference between mass and weight. 18. Explain how hypothesis and theory are different. Use the figure below to answer the question. 19. Infer a qualitative measurement that can be made from the scene shown.
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Chemistry Benchmark 1 Review
Completion
Complete each statement.
1. Chemistry is the study of _____________________ and the changes that it undergoes.
2. A(n) ______________________ is a set of controlled observations that test the hypothesis.
3. 100.00 meters 50.000 centimeters 1.0000 kilometer = ____________________ meters.
4. A process that involves one or more substances changing into new substances is known as a
____________________ change.
5. Cutting a sheet of paper is an example of a ____________________ change.
6. A ____________________ property enables a substance to combine with or change into one or more
substances.
7. Sugar is a ____________________ form of matter with a definite shape and volume.
8. A ____________________ is a subatomic particle that has mass nearly equal to that of a proton, but it carries
no electrical charge.
9. Atoms with the same number of protons but different number of neutrons are called ____________________.
10. An alpha particle is _____________________ charged with two protons and neutrons.
11. Democritus believed that matter is made up of tiny individual particles known as a(n)
____________________.
12. The number of protons in an atom is called the ____________________ of the element.
13. The ____________________ principle states that a maximum of two electrons may occupy a single atomic
orbital, but only if the electrons have opposite spins.
14. The arrangement of electrons in an atom is called the ____________________ of an atom.
15. The group 2A elements are known as ____________________ metals.
16. Elements that have physical and chemical properties of both metals and nonmetals are known as
____________________.
Short Answer
17. Explain the difference between mass and weight.
18. Explain how hypothesis and theory are different.
Use the figure below to answer the question.
19. Infer a qualitative measurement that can be made from the scene shown.
20. Infer a quantitative measurement that can be made from the scene shown.
21. What must be immediately done if chemicals come in contact with the eyes or skin while performing an
experiment in the laboratory?
22. Evaluate this dimensional analysis setup. A paperclip is 3.2 cm long. How many paperclips would fit in a
football field (100 yards) if 1 inch = 2.54 cm?
23. What two things does a conversion factor do?
24. The data for two different measurements are shown below. Which experiment was more accurate? Explain
your answer.
Sample Measured value Accepted value
Distance 54,700 m 57,900 m
Mass 61.3 g 65.7 g
A student conducts an experiment to determine the effect of adding salt on the boiling temperature of water.
The results are shown below.
Sample Amount of Salt Boiling Temperature
Sample 1 0 g 100.0° C
Sample 2 2 g 102.3° C
Sample 3 5 g 104.8° C
Sample 4 10 g 107.5° C
25. The student graphs this data using the axes shown. Is this graph correct? Explain your answer.
26. Define a base unit.
27. The distance between the earth and the sun is 90.0 million miles. Calculate this distance in meters up to three
significant digits.
28. Convert 600 mg to grams.
29. How many significant digits are there in 6.023 1023
molecules?
30. Identify both a physical change and a chemical change that could be done to a piece of paper.
31. Distinguish between element and compound.
32. Distinguish between homogeneous and heterogeneous mixtures. Give an example of each one.
33. Compare and contrast mass number and atomic mass.
34. What is the average atomic mass of this element?
Isotope Mass (amu) Percent Abundance
Phosphorus-29 29 5%
Phosphorus-31 31 71%
Phosphorus-32 32 24%
35. What is the average atomic mass of this element?
Isotope Mass (amu) Percent Abundance
Silver-105 105 48%
Silver-108 108 43%
Silver-109 109 9%
36. Write the chemical symbol for the isotope of cobalt with 37 neutrons.
37. Element X has an average atomic mass of 64.32 amu. If this element consists of only two isotopes, X-64 and
X-65, which isotope is present in the greater abundance? Explain how you can tell.
38. Define an atom.
39. What do you understand by the term atomic mass unit (amu)?
40. How are atomic number and mass number denoted in the chemical symbol of the isotope of an element?
Express the shortened notation for an isotope of element X with atomic number 92 and atomic mass 238.
41. Identify the element containing 34 protons.
42. What were the main flaws in Dalton’s atomic theory?
43. Summarize the relationship between wavelength, frequency, and energy of a wave.
44. A student records the following electron configuration for the element Arsenic (As). Evaluate this student’s
answer.
1s22s
22p
63s
23p
64s
24d
104p
3
45. Explain why it is only possible for two electrons to exist in the same orbital.
46. Use the model of the atom shown to identify the correct element. Write the electron configuration and orbital
diagram for this element.
47. Which rule for filling of orbitals by electrons in the element Silicon is being violated in the orbital diagram
shown? Justify your answer.
48. Which rule for the filling of orbitals in the element Phosphorus is being violated in the orbital diagram
shown? Justify your answer.
49. Which rule for the filling of orbitals by electrons in the element Magnesium is being violated? Justify your
answer.
50. Define a photon. What is the formula used to calculate the energy of a photon?
51. Why does a piece of iron appear red when heated sufficiently and blue at a higher temperature?
52. What is the ground state electron configuration of chlorine and the number of valence electrons in it?
53. How many valence electrons are present in cesium? Write the electron configuration of cesium if the atomic
number is 55.
54. Write the noble gas form of the electron configuration and the electron dot structure of sodium and oxygen.
55. Write the noble gas form of the electron configuration and the electron dot structure of selenium and
phosphorus.
56. A student makes the following statement: “It’s easy to tell which energy level an element is in - you just count
down which row it is in, and that’s the energy level.” Is this student correct? Explain how you came to your
conclusion.
57. Explain what is meant by the “octet rule.” Does it hold true for the modern periodic table?
58. Label the blank periodic table with the following terms.
A: metalloids
B: element with the highest electronegativity
C: alkali metals
D: lanthanide series
E: element with the greatest atomic radius
F: noble gases
G: halogens
59. Explain the significance of the stair-step line located near the right-hand side of the periodic table
60. Do the figures in this partial periodic table demonstrate the trend in atomic radius, ionic radius, or neither of
these? Relate your answer to the structure of atoms across the periodic table.
61. Place these five elements in order of electronegativity, with the highest electronegativity first.
62. Identify the representative elements from the list given below.
Na, Ca, Sc, Co, Ni, Si, N, Se, Cl, Ge
63. Why is argon placed before potassium in the modern periodic table?
64. Why do elements in the same group have similar properties?
65. Why is the size of a sodium ion (Na+) less than that of a sodium atom (Na)?
66. List the general electron configuration and location of the s, p, d, and f-block elements in the periodic table.
67. Use the periodic table to write the names of the third alkali metal and the first transition metal.
Problem
68. A vessel contains 30 mL of water. A sample of 5.0 g of copper metal is dropped into this vessel, raising the
level of water in it to 40 mL. What is the density of the copper sample?
69. When a 5.00-g metal piece, A, was immersed in 38.0 mL of water, the water level rose to 50.0 mL. Similarly,
when a 5.00-g metal piece, B, was immersed in 38.0 mL of water, the level of water rose to 60.0 mL.
Compare the density of the metal pieces, A and B.
70. Calculate the area of a rectangular piece of land with a length of 8.0 105 cm and a width of 4.0 10
3 cm.
Express your answer in meters.
71. Complete the following table:
Element Number of
protons
Number of
electrons
Number of
neutrons
Atomic
number
Mass number
Sodium 11 12
Phosphorus 15 31
Cobalt 27 32
Bromine 35 80
Silver 61 47
72. An element X has two naturally occurring isotopes: X-79 (abundance = 50.69%, mass = 78.918 amu) and
X-81 (abundance = 49.31%, mass = 80.917 amu). Calculate the weighted atomic mass of X. Also, identify the
unknown element which exists as a reddish-brown gas and is a liquid at room temperature.
73. An element X has three naturally occurring isotopes: X-24, X-25, and X-26. The atomic mass of X-25 is
24.986 amu and the relative abundance is 10.00 %. The atomic mass of X-26 is 25.982 amu and the relative
abundance is 11.01 %.Given that the weighted atomic mass of the element X is 24.305, calculate the mass
contribution due to the isotope X-24 and identify the element.
74. Calculate the number of protons, electrons, and neutrons in an atom of the element Pb with mass number 207
and atomic number 82.
75. Fluorine (F) contains 9 proton and 10 neutrons. Calculate its mass in amu for 81 atoms. (Given: mass of a
proton = 1.007276 amu, mass of a neutron = 1.008665 amu).
76. Lead contains 82 protons and 125 neutrons. Write the shortened notation of the element with its symbol,
atomic number, and mass number.
77. How many sublevels and orbitals are possible in the third energy level?
78. Write the ground state electron configuration of sulfur and draw its electron-dot structure.
79. Two elements A and B have atomic numbers 8 and 17 respectively. Identify their groups in the periodic table.
80. An element has similar chemical properties as oxygen and selenium. It has an atomic number greater than
krypton but less than iodine. Use the periodic table to identify the element.
81. Identify the element having the largest size and the element having the highest electronegativity from the list
of electron configurations given below:
a. [Ne] 3s23p
3
b. [Ne] 3s23p
4
c. [Ne] 3s23p
5
d. [Ne] 3s23p
34s
23d
3
82. Arrange the elements given below in the increasing order of their atomic size.