Chapter 6 Study Guide
True/False
Indicate whether the statement is true or false.
____
1. Although chemical properties obey the periodic law, it is impossible to predict physical properties of elements
based on their location in the periodic table.
____
2. All of the nonmetals on the periodic table are gases.
____
3. The transition elements consist only of those that are found in block d of the periodic table.
____
4. Elements in the same family tend to have the same number of valence electrons.
____
5. The radius of an atom is defined as half the distance between the nuclei of two adjacent or bonded atoms of
that element.
____
6. The octet rule states that atoms will gain, lose, or share electrons to achieve a complete set of eight valence
electrons.
____
7. Elements in Group 17 are classified as halogens.
____
8. Elements in Group 2 are classified as alkali metals.
____
9. When an atom loses electrons, its radius gets smaller.
____ 10. The electronegativity of elements increases from left to right and from top to bottom on the periodic table.
____ 11. An atom that gains an electron will form a positive ion.
____ 12. The same amount of energy is required to remove each electron sequentially from an atom.
Multiple Choice
Identify the choice that best completes the statement or answers the question.
____ 13. Which scientist classified elements into four categories: gases, metals, nonmetals, and earths?
a. Mendeleev
c. Newlands
b. Lavoisier
d. Mosely
____ 14. Which scientist first arranged elements by atomic number?
a. Mendeleev
c. Newlands
b. Lavoisier
d. Mosely
____ 15. Which scientist characterized the “law of octaves”?
a. Mendeleev
c. Newlands
b. Lavoisier
d. Mosely
____ 16. Which category of elements have the property of being malleable and ductile?
a. gases
c. metalloids
b. metals
d. nonmetals
____ 17. Which category of elements is commonly used to make computer chips and solar cells due to their ability to
conduct electricity only under certain conditions?
a. metals
c. nonmetals
b. metalloids
d. noble gases
____ 18. Which region is referred to as the p-block on the diagram?
a. A
c. C
b. B
d. D
____ 19. Which region is referred to as the f-block on the diagram?
a. A
c. C
b. B
d. D
____ 20. Which region contains the halogen family of elements?
a. A
c. C
b. B
d. D
____ 21. Which region contains the alkaline earth metal family of elements?
a. A
c. C
b. B
d. D
____ 22. Which region contains elements with two valence electrons?
a. A
c. C
b. B
d. D
____ 23. Which region contains elements with an electron configuration that ends with p3?
a. A
c. C
b. B
d. D
____ 24. Which block on the periodic table contains the actinide series of elements?
a. s-block
c. d-block
b. p-block
d. f-block
____ 25. Which diagram correctly depicts the trend in electronegativity?
a. a
c. c
b. b
d. d
____ 26. Which diagram correctly depicts the general trend in first ionization energy?
a. a
c. c
b. b
d. d
____ 27. Which element has an electron configuration that ends in the fourth energy level?
a. A
c. C
b. B
d. D
____ 28. Which element is the most metallic?
a. A
b. B
c. C
d. D
____ 29. Which block is element Y most likely found in?
Element Block Characteristics
X
s
Soft, shiny grey metal; highly
reactive, lightweight
Y
?
Liquid at room temperature; has the
highest electronegativity in its period
Z
p
Used as a semiconductor due to its
electricity-conducting properties
a. s
b. p
c. d
d. f
____ 30. Which is defined as the energy required to remove an electron from an atom of an element in the gaseous
state?
a. ionization energy
c. ionic radius
b. electronegativity
d. law of octets
____ 31. In which pair is the one on the left larger than the one on the right?
a. Na, Rb
c. Br, Brb. S, Mg
d. K, K+
____ 32. Identify the period and group numbers of the element with the electron configuration. [Ne]3s23p4
a. Period 2, Group 4
c. Period 3, Group 16
b. Period 3, Group 4
d. Period 2, Group 16
____ 33. Which is the energy level that is being filled by electrons in the transition elements of period 5?
a. third
c. fifth
b. fourth
d. sixth
____ 34. Which correctly describes elements in the same group?
a. They have the same number of valence electrons.
b. They have electrons in the same outermost energy level.
c. They have the same atomic radius.
d. They must be in the same state of matter.
____ 35. Which is the halogen that is in Period 5?
a. Bromine (Br)
b. Strontium (Sr)
c. Iodine (I)
d. Xenon (Xe)
____ 36. Which metalloid is in the fourth period and the same group as Carbon?
a. Silicon
c. Tin
b. Germanium
d. Boron
____ 37. Which is a transition element with five d-block electrons in energy level 4?
a. Niobium (Nb)
c. Manganese (Mn)
b. Renium (Re)
d. Technicium (Tc)
____ 38. Which is the most important characteristic in detemining an element’s chemical properties?
a. the number of protons and neutrons in its nucleus
b. which period it is found in
c. the number of valence electrons it contains
d. its outermost energy level
____ 39. Which block contains 5 orbitals?
a. s
b. p
c. d
d. f
____ 40. Which group will have an electron configuration that ends in ns2?
a. Alkali metals
c. Halogens
b. Alkaline Earth metals
d. Actinides
____ 41. Which property describes how much energy must be added to an atom to remove an outermost electron?
a. atomic radius
c. electronegativity
b. ionic radius
d. ionization energy
____ 42. Which of the following elements is a metal?
a. Boron
b. Nitrogen
c. Magnesium
d. Carbon
____ 43. According to ____ periodic table, the physical and chemical properties of elements are periodic functions of
their atomic weights.
a. Dmitri Mendeleev’s
c. Henry Moseley’s
b. John Newlands’
d. Lothar Meyer’s
____ 44. What is another name for the representative elements?
a. Group A elements
c. Group C elements
b. Group B elements
d. transition elements
____ 45. What is another name for the transition metals?
a. noble gases
c. Group B elements
b. Group A elements
d. Group C elements
____ 46. Which of the following elements is in the same period as phosphorus?
a. carbon
c. nitrogen
b. magnesium
d. oxygen
____ 47. Who arranged the elements according to atomic mass and used the arrangement to predict the properties of
missing elements?
a. Henry Moseley
c. John Dalton
b. Antoine Lavoisier
d. Dmitri Mendeleev
____ 48. Which of the following categories includes the majority of the elements?
a. metalloids
c. metals
b. liquids
d. nonmetals
____ 49. Of the elements Pt, V, Li, and Kr, which is a nonmetal?
a. Pt
c. Li
b. V
d. Kr
____ 50. In which of the following sets is the symbol of the element, the number of protons, and the number of
electrons given correctly?
a. In, 49 protons, 49 electrons
c. Cs, 55 protons, 132.9 electrons
b. Zn, 30 protons, 60 electrons
d. F, 19 protons, 19 electrons
____ 51. The atomic number of an element is the total number of which particles in the nucleus?
a. neutrons
c. electrons
b. protons
d. protons and electrons
____ 52. What element has the electron configuration 1s 2s 2p 3s 3p ?
a. nitrogen
c. silicon
b. selenium
d. silver
____ 53. Which of the following is true about the electron configurations of the noble gases?
a. The highest occupied s and p sublevels are completely filled.
b. The highest occupied s and p sublevels are partially filled.
c. The electrons with the highest energy are in a d sublevel.
d. The electrons with the highest energy are in an f sublevel.
____ 54. Which of the following electron configurations is most likely to result in an element that is relatively
inactive?
a. a half-filled energy sublevel
b. a filled energy sublevel
c. one empty and one filled energy sublevel
d. a filled highest occupied principal energy level
____ 55. Which subatomic particle plays the greatest part in determining the properties of an element?
a. proton
c. neutron
b. electron
d. none of the above
____ 56. Which of the following elements is a transition metal?
a. cesium
c. tellurium
b. copper
d. tin
____ 57. Which of the following groupings contains only representative elements?
a. Cu, Co, Cd
c. Al, Mg, Li
b. Ni, Fe, Zn
d. Hg, Cr, Ag
____ 58. Which of the following is true about the electron configurations of the representative elements?
a. The highest occupied s and p sublevels are completely filled.
b. The highest occupied s and p sublevels are partially filled.
c. The electrons with the highest energy are in a d sublevel.
d. The electrons with the highest energy are in an f sublevel.
____ 59. What are the Group 1A and Group 7A elements examples of?
a. representative elements
c. noble gases
b. transition elements
d. nonmetallic elements
____ 60. Of the elements Fe, Hg, U, and Te, which is a representative element?
a. Fe
c. U
b. Hg
d. Te
____ 61. How does atomic radius change from top to bottom in a group in the periodic table?
a. It tends to decrease.
c. It first increases, then decreases.
b. It tends to increase.
d. It first decreases, then increases.
____ 62. How does atomic radius change from left to right across a period in the periodic table?
a. It tends to decrease.
c. It first increases, then decreases.
b. It tends to increase.
d. It first decreases, then increases.
____ 63. What causes the shielding effect to remain constant across a period?
a. Electrons are added to the same principal energy level.
b. Electrons are added to different principal energy levels.
c. The charge on the nucleus is constant.
d. The atomic radius increases.
____ 64. Atomic size generally ____.
a. increases as you move from left to right across a period
b. decreases as you move from top to bottom within a group
c. remains constant within a period
d. decreases as you move from left to right across a period
____ 65. What element in the second period has the largest atomic radius?
a. carbon
c. potassium
b. lithium
d. neon
____ 66. Which of the following factors contributes to the increase in atomic size within a group in the periodic table
as the atomic number increases?
a. more shielding of the electrons by the highest occupied energy level
b. an increase in size of the nucleus
c. an increase in number of protons
d. fewer electrons in the highest occupied energy level
____ 67. Which of the following elements has the smallest atomic radius?
a. sulfur
c. selenium
b. chlorine
d. bromine
____ 68. What is the charge of a cation?
a. a positive charge
b. no charge
c. a negative charge
d. The charge depends on the size of the nucleus.
____ 69. Which of the following statements is true about ions?
a. Cations form when an atom gains electrons.
b. Cations form when an atom loses electrons.
c. Anions form when an atom gains protons.
d. Anions form when an atom loses protons.
____ 70. The metals in Groups 1A, 2A, and 3A ____.
a. gain electrons when they form ions
b. all form ions with a negative charge
c. all have ions with a 1 charge
d. lose electrons when they form ions
____ 71. Which of the following statements is NOT true about ions?
a. Cations are positively charged ions.
b. Anions are common among nonmetals.
c. Charges for ions are written as numbers followed by a plus or minus sign.
d. When a cation forms, more electrons are transferred to it.
____ 72. Why is the second ionization energy greater than the first ionization energy?
a. It is more difficult to remove a second electron from an atom.
b. The size of atoms increases down a group.
c. The size of anions decreases across a period.
d. The nuclear attraction from protons in the nucleus decreases.
____ 73. In which of the following sets are the charges given correctly for all the ions?
a. Na , Mg , Al
c. Rb , Ba , P
b. K , Sr , O
d. N , O , F
____ 74. In which of the following groups of ions are the charges all shown correctly?
a. Li , O , S
c. K , F , Mg
b. Ca , Al , Br
d. Na , I , Rb
____ 75. What is the element with the lowest electronegativity value?
a. cesium
c. calcium
b. helium
d. fluorine
____ 76. What is the element with the highest electronegativity value?
a. cesium
c. calcium
b. helium
d. fluorine
____ 77. Which of the following elements has the smallest ionic radius?
a. Li
c. O
b. K
d. S
____ 78. What is the energy required to remove an electron from an atom in the gaseous state called?
a. nuclear energy
c. shielding energy
b. ionization energy
d. electronegative energy
____ 79. For Group 2A metals, which electron is the most difficult to remove?
a. the first
b. the second
c. the third
d. All the electrons are equally difficult to remove.
____ 80. Which of the following factors contributes to the decrease in ionization energy within a group in the periodic
table as the atomic number increases?
a. increase in atomic size
b. increase in size of the nucleus
c. increase in number of protons
d. fewer electrons in the highest occupied energy level
____ 81. Which of the following elements has the smallest first ionization energy?
a. sodium
c. potassium
b. calcium
d. magnesium
____ 82. Which of the following elements has the lowest electronegativity?
a. lithium
c. bromine
b. carbon
d. fluorine
____ 83. Which statement is true about electronegativity?
a. Electronegativity is the ability of an anion to attract another anion.
b. Electronegativity generally increases as you move from top to bottom within a group.
c. Electronegativity generally is higher for metals than for nonmetals.
d. Electronegativity generally increases from left to right across a period.
____ 84. Which of the following decreases with increasing atomic number in Group 2A?
a. shielding effect
c. ionization energy
b. ionic size
d. number of electrons
____ 85. Which of the following statements correctly compares the relative size of an ion to its neutral atom?
a. The radius of an anion is greater than the radius of its neutral atom.
b. The radius of an anion is identical to the radius of its neutral atom.
c. The radius of a cation is greater than the radius of its neutral atom.
d. The radius of a cation is identical to the radius of its neutral atom.
____ 86. Which of the following factors contributes to the increase in ionization energy from left to right across a
period?
a. an increase in the shielding effect
b. an increase in the size of the nucleus
c. an increase in the number of protons
d. fewer electrons in the highest occupied energy level
____ 87. As you move from left to right across the second period of the periodic table ____.
a. ionization energy increases
c. electronegativity decreases
b. atomic radii increase
d. atomic mass decreases
____ 88. Of the following elements, which one has the smallest first ionization energy?
a. boron
c. aluminum
b. carbon
d. silicon
Matching
Match each item with the correct statement below.
a. electronegativity
f.
b. ionization energy
g.
c. atomic radius
h.
d. metal
i.
e. transition metal
j.
periodic law
cation
period
group
electrons
____ 89. horizontal row in the periodic table
____ 90. vertical column in the periodic table
____ 91. A repetition of properties occurs when elements are arranged in order of increasing atomic number.
____ 92. type of element that is a good conductor of heat and electric current
____ 93. type of element characterized by the presence of electrons in the d orbital
____ 94. one-half the distance between the nuclei of two atoms when the atoms are joined
____ 95. type of ion formed by Group 2A elements
____ 96. subatomic particles that are transferred to form positive and negative ions
____ 97. ability of an atom to attract electrons when the atom is in a compound
____ 98. energy required to remove an electron from an atom