Download ExamView - Periodic Trends Study Guide.tst

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ID: A
Periodic Trends
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.
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periodic law
atomic mass
period
group
electrons
horizontal row in the periodic table
vertical column in the periodic table
type of element that is a good conductor of heat and electric current
type of element characterized by the presence of electrons in the d orbital
subatomic particles that are transferred to form positive and negative ions
ability of an atom to attract electrons when the atom is in a compound
energy required to remove an electron from an atom
Multiple Choice
Identify the choice that best completes the statement or answers the question.
____
8. What is another name for the representative elements?
a. Group A elements
b. Group B elements
c. Group C elements
d. transition elements
____ 9. Each period in the periodic table corresponds to a(n) ____.
a. principal energy level
b. energy sublevel
c. orbital
d. suborbital
____ 10. The modern periodic table is arranged in order of increasing atomic ____.
a. mass
b. charge
c. number
d. radius
____ 11. Who arranged the elements according to atomic mass and used the arrangement to predict the properties of
missing elements?
a. Henry Moseley
b. Antoine Lavoisier
c. John Dalton
d. Dmitri Mendeleev
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Name: ________________________
ID: A
____ 12. Which of the following categories includes the majority of the elements?
a. metalloids
b. liquids
c. metals
d. nonmetals
____ 13. Of the elements Pt, V, Li, and Kr, which is a nonmetal?
a. Pt
b. V
c. Li
d. Kr
____ 14. To what category of elements does an element belong if it is a poor conductor of electricity? ____
a. transition elements
b. metalloids
c. nonmetals
d. metals
____ 15. 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
b. Zn, 30 protons, 60 electrons
c. Cs, 55 protons, 132.9 electrons
d. F, 19 protons, 19 electrons
____ 16. The atomic number of an element is the total number of which particles in the nucleus?
a. neutrons
b. protons
c. electrons
d. protons and electrons
____ 17. Elements that are characterized by the filling of p orbitals are classified as ____.
a. groups 3A through 8A
b. transition metals
c. inner transition metals
d. groups 1A and 2A
____ 18. 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
____ 19. Which subatomic particle plays the greatest part in determining the properties of an element?
a. proton
b. electron
c. neutron
d. nucleus
____ 20. Which of the following groupings contains only representative elements?
a. Cu, Co, Cd
b. Ni, Fe, Zn
c. Al, Mg, Li
d. Hg, Cr, Ag
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Name: ________________________
ID: A
____ 21. 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.
____ 22. 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.
____ 23. Which of the following elements has the smallest atomic radius?
a. sulfur
b. chlorine
c. selenium
d. bromine
____ 24. 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.
____ 25. 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.
____ 26. By 1700, how many elements had scientists discovered and isolated?
a. 7
b. 13
c. 27
d. 46
____ 27. In which of the following sets are the charges given correctly for all the ions?
a. Na + , Mg + , Al +
b. K + , Sr 2 + , O 2 −
c. Rb − , Ba 2 − , P 3 +
d. N − , O 2 − , F 3 −
____ 28. In which of the following groups of ions are the charges all shown correctly?
a. Li − , O 2 − , S 2 +
b. Ca 2 + , Al 3 + , Br −
c. K 2 − , F − , Mg 2 +
d. Na + , I − , Rb −
____ 29. What is the element with the lowest electronegativity value?
a. cesium
b. helium
c. calcium
d. fluorine
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Name: ________________________
ID: A
____ 30. What is the element with the highest electronegativity value?
a. cesium
b. helium
c. calcium
d. fluorine
____ 31. Which of the following elements has the smallest ionic radius?
a. Li
b. K
c. O
d. S
____ 32. What is the energy required to remove an electron from an atom in the gaseous state called?
a. nuclear energy
b. ionization energy
c. shielding energy
d. electronegative energy
____ 33. By the early 1800’s, chemists started organizing elements into groups because
a. the printing press made it possible to disseminate knowledge faster.
b. universities had a sudden influx of students interested in chemistry.
c. there were so many new elements that had been discovered.
d. more books were being published on the topic.
____ 34. 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
____ 35. Which of the following elements has the smallest first ionization energy?
a. sodium
b. calcium
c. potassium
d. magnesium
____ 36. Which of the following elements has the lowest electronegativity?
a. lithium
b. carbon
c. bromine
d. fluorine
____ 37. 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.
____ 38. Compared with the electronegativities of the elements on the left side of a period, the electronegativities of
the elements on the right side of the same period tend to be ____.
a. lower
b. higher
c. the same
d. unpredictable
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Name: ________________________
ID: A
____ 39. Which of the following decreases with increasing atomic number in Group 2A?
a. shielding effect
b. ionic size
c. ionization energy
d. number of electrons
____ 40. 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.
____ 41. 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
____ 42. As you move from left to right across the second period of the periodic table
a. ionization energy increases.
b. atomic radii increase.
c. electronegativity decreases.
d. atomic mass decreases.
____ 43. Of the following elements, which one has the smallest first ionization energy?
a. boron
b. carbon
c. aluminum
d. silicon
Short Answer
44. Which group of elements in the periodic table is known as the alkali metals?
45. In which group in the periodic table do the elements have the highest electronegativity values?
Numeric Response
46. How many electrons are there in the highest occupied energy level of atoms in Group 5A elements?
47. How many electrons does the ion Ca 2 + contain?
Essay
48. Describe the trends in first ionization energy within groups and across periods in the periodic table. Provide
examples.
49. Positive ions are smaller than the atoms from which they are formed, but negative ions are larger than the
atoms from which they are formed. Explain why this is so.
50. Describe the trends in electronegativity within groups and across periods in the periodic table. Provide
examples.
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Periodic Trends
Answer Section
MATCHING
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MULTIPLE CHOICE
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SHORT ANSWER
44. ANS:
1A
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45. ANS:
7A
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NUMERIC RESPONSE
46. ANS: 5
PTS: 1
47. ANS: 18
PTS: 1
ESSAY
48. ANS:
First ionization energies decrease from top to bottom within a group and increase across a period from left to
right. For example, the first ionization energy of rubidium is less than that of lithium. The first ionization
energy of iodine is much greater than that of lithium.
PTS: 1
49. ANS:
When an electron is added to an atom, the attraction of the nucleus for any one electron decreases and the
size of the ion’s radius increases. When an electron is removed from an atom, there is an increase in the
nuclear attraction experienced by the remaining electrons. Consequently, the remaining electrons are drawn
closer to the nucleus.
PTS: 1
50. ANS:
Electronegativity values decrease from top to bottom within a group, and from right to left across a period.
For example, rubidium is less electronegative than lithium. Lithium is less electronegative than fluorine.
PTS: 1
2