Practice Questions

ch2Student: ___________________________________________________________________________

1. List the three primary particles found in an atom.

2. What is the value of the mass number in the isotope ?

3. What is the term for atoms of the same element having different masses due to a different number of

neutrons?

4. What is the process by which certain isotopes emit particles and release large amounts of energy?

5. What do we call electrically charged particles that result from the gain of one or more electrons by a

parent atom?

6. Dalton proposed that all atoms of an element have identical properties. Briefly, explain why this proposal is invalid.

7. J. J. Thomson in 1897, announced that cathode rays consisted of a stream of _______.

8. In one sentence, state Rutherford's important contribution to our knowledge of atomic structure.

9. What instrument is used to study the wavelengths of light emitted and absorbed by atoms?

10. In Bohr's model of the hydrogen atom, what is an "orbit"?

11. In Bohr's theory of the atom, what is the number n (n = 1, 2, 3, ...) called?

12. In one sentence, explain the meaning/consequences of Heisenberg's Uncertainty Principle.

13. In modern atomic theory, Bohr's orbits are replaced by atomic orbitals. What is an atomic orbital?

14. Which two scientists in 1869 arranged the elements in order of increasing atomic masses to form a

precursor of the modern periodic table of elements?

15. Who stated that the elements, when arranged according to their atomic masses, showed a distinct

periodicity of their properties?

16. In the modern periodic table, how are the elements arranged?

17. The modern periodic law states that the physical and chemical properties of the elements are periodic

functions of what property?

18. What do we call the horizontal row of elements on the periodic table?

19. How many periods are found on the periodic table?

20. Which period contains the element sodium?

21. What do we call the columns of elements on the periodic table?

22. For an atom, what number gives the number of electrons and protons found in that atom?

23. What is the general name given to the elements of Group IA (1)?

24. What term is used for the elements straddling the "staircase" boundary between the metals and nonmetals?

25. For a representative element, how can we deduce the number of valence electrons in a neutral atom from

the position of the element in the periodic table?

26. In what way(s) are the three orbitals in the 2p sublevel similar? In what way(s) are they different?

27. What requirement must be met in order for two electrons to coexist in the same orbital?

28. State the Aufbau Principle.

29. Give the electronic configuration in an atom of neon, element number 18.

30. Give the electronic arrangement in an atom of strontium, element number 38.

31. How many valence electrons are present in a chloride ion?

32. State the Octet Rule.

33. Give the name of a Group VIIA (17) ion that has the following electronic arrangement:

1s22s22p63s23p6

34. Give the complete electronic arrangement of a sulfide ion, S2-.

35. Atoms with the biggest radii occur in the _______ _______ region of the periodic table.

36. How would you expect an Al3+ ion to compare in size with an Al atom? Explain why.

37. Which group of elements has the highest ionization energies? Which group has the lowest?

38. Explain what is meant by electron affinity.

39. _________ is the ion responsible for the regulation of blood pressure and involved in the transmission of

neural impulses.

40. What does the mass number minus the atomic number represent?

A. Number of protonsB. Number of electronsC. Number of neutronsD. Number of protons - number of neutronsE. Number of neutrons - number of protons

41. In a neutral atom, what number equals the number of electrons?

A. Atomic numberB. Mass numberC. Mass number minus the atomic numberD. Both A and CE. None of the above

42. Given that helium has an isotope , predict the number of electrons in a helium atom.

A. 1B. 2C. 4D. 6E. 0

43. How many neutrons are present in an atom of the isotope ? A. 3B. 4C. 7D. 10E. none of the above

44. Microwaves, light and X-rays are all forms of ____________.

A. ElectricityB. High energy electronsC. Electron repulsionD. Electromagnetic radiationE. Radioactivity

45. Where are the alkaline earth metals located on the periodic table?

A. IA (1)B. IIA (2)C. IIIA (3)D. VIIA (17)E. VIIIA (18)

46. How many orbitals are in an s sublevel? How many in a p sublevel?

A. S: 1, p: 2B. S: 2, p: 3C. S: 1, p: 3D. S: 2, p: 6E. S: 3, p: 3

47. How many electrons are present in an atom of silicon?

A. 14B. 16C. 18D. 24E. 26

48. Give the name of a Group IA (1) ion that has the following electronic arrangement: 1s22s22p6

A. Lithium ionB. Sodium ionC. Potassium ionD. Magnesium ionE. Calcium ion

49. What ion carries two negative charges and is isoelectronic with K+?

A. O2-

B. S2-

C. F2-

D. Cl2-

E. Ar2-

50. What kind(s) of particles can be found outside the nucleus of an atom?

A. ProtonsB. NeutronsC. ElectronsD. Protons and electronsE. Protons and neutrons

51. The total mass of the protons in any neutral atom is about _______ times the total mass of electrons in the atom. A. 0.0005B. 0.3C. 1D. 2E. 2000

52. What is the quantity represented by the mass number minus the atomic number?

A. Number of atomsB. Number of neutronsC. Number of electronsD. Number of protonsE. Number of particles in the nucleus

53. Which isotope of hydrogen has two neutrons?

A. Hydrogen-1B. Hydrogen-2C. Hydrogen-3D. DeuteriumE. H2

54. Which of the following accounts for the fact that chlorine has an atomic mass of 35.45 amu rather than a

whole number? A. IsotopesB. ElectronsC. ProtonsD. RadioactivityE. Isomers

55. Who discovered that cathode rays consist of a stream of negative particles, electrons?

A. CrookesB. ThomsonC. GeigerD. RutherfordE. Bohr

56. Who discovered the existence of the atomic nucleus?

A. CrookesB. ThomsonC. GeigerD. RutherfordE. Bohr

57. In Rutherford's experiment, which led to the discovery of the atomic nucleus, what type of particle or ray

was fired at the gold foil target? A. AlphaB. BetaC. GammaD. NeutronsE. Cathode rays

58. In Mendeleev's table of the elements, they were arranged according to ______________.

A. Atomic numberB. Mass numberC. Atomic massD. Neutron numberE. Density

59. The modern periodic table is arranged according to what property? A. Atomic numberB. Mass numberC. Atomic massD. Neutron numberE. Density

60. What do we call a complete horizontal row of elements on the periodic table?

A. GroupB. PeriodC. FamilyD. Representative elementsE. Transition elements

61. What are all the elements in the A-groups often called?

A. Transition elementsB. LanthanidesC. MetalsD. Non-metalsE. Representative elements

62. Which of the following elements is a metalloid?

A. CB. GeC. PbD. NE. P

63. Where are the halogens located on the periodic table?

A. Representative elementsB. Transition metalsC. Group VIIA (17)D. Group IIA (2)E. Group IIIA (3)

64. How many valence electrons are in an atom of carbon?

A. 8B. 6C. 4D. 1E. 0

65. What is the lowest energy sublevel of a principal level?

A. dB. eC. fD. sE. p

66. How many sublevels are there in the third principal energy level?

A. 3B. 2C. 1D. 0E. 4

67. How many orbitals are there in the second principal energy level? A. 2B. 3C. 1D. 0E. 4

68. Which of the following correctly gives the electron capacity of a principal energy level in terms of the

number n? A. nB. 2nC. 2n +

2D. N2

E. 2n2

69. What is the electron configuration of sulfur, atomic number 16?

A. 1s21p62s22p6

B. 1s22s22p62d6

C. 1s22s22p63s23p4

D. 1s22s22p63s23d4

E. 1s22s22p63s22d4

70. Which one of the following electron configurations is appropriate for a normal atom?

A. 1s12s1

B. 1s22s1

C. 1s22s22p8

D. 1s22s22p43s1

E. 1s22s22p63d1

71. Which of the following elements is most likely to form a 2+ ion?

A. LiB. KC. AlD. NE. Cu

72. Give the complete electronic configuration of a sodium ion.

A. 1s22s22p5

B. 1s22s22p6

C. 1s22s22p63s1

D. 1s22s22p63s2

E. 1s22s22p63s23p64s1

73. Which of the following ions does not follow the octet rule?

A. Na+

B. Ca2+

C. Al3+

D. N3-

E. Cl2-

74. Which of the following atoms has the biggest size (radius)?

A. NaB. AlC. ClD. RbE. I

75. Which of the following elements has the highest ionization energy? A. LiB. BC. OD. FE. He

76. Which of the following elements has the lowest ionization energy?

A. LiB. BC. OD. FE. Ne

77. The electron affinity is _________________.

A. The energy required to remove an electron from an isolated atomB. The force between two electrons in the same orbitalC. The force between two ions of opposite chargeD. The energy released when an isolated atom gains an electronE. The attraction of an atom for an electron in a chemical bond

78. Which one of the following elements has the highest electron affinity?

A. LiB. KC. KrD. OE. Cl

79. Which of the following statements relating to Bohr's model of the hydrogen atom is incorrect?

A. The lowest energy orbit has quantum number n = 1B. The highest energy orbits are farthest from the nucleusC. In a transition from the n = 3 to the n = 1 level, light is emittedD.

Energy differences between energy levels can be calculated from the wavelengths of the light absorbed or emitted

E. The Bohr model consists of energy levels that are evenly spaced, like the rungs of a ladder 80. Who proposed that electrons could behave like waves, as well as like particles?

A. ThomsonB. RutherfordC. BohrD. De BroglieE. Heisenberg

81. In the calcium atom represented by the symbol , there are 20 protons, 20 neutrons and 20

electrons. True False

82. All atoms of a particular element have identical chemical properties.

True False 83. An atom cannot be created, divided, destroyed or converted to any other type of atom.

True False 84. The atomic number of an ion tells us the number of protons that are present.

True False 85. If an atom gains one electron, it becomes an anion.

True False

86. The first experimentally based theory of atomic structure was proposed by John Dalton. True False

87. J. J. Thomson was the first to state that an atom is mostly empty space.

True False 88. Short wavelengths of electromagnetic radiation have more energy than long wavelengths.

True False 89. Bohr was the first to use the term "orbit" to explain the fixed energy levels of electrons.

True False 90. Niels Bohr developed a theory which accounted for the lines in the visible region of the hydrogen

spectrum. True False

91. In Mendeleev's table, the elements were arranged according to their atomic mass.

True False 92. There are nine periods on the periodic table.

True False 93. Sulfur (S) is one of the representative elements.

True False 94. Europium (Eu) is a lanthanide element.

True False 95. Arsenic (As) is a metalloid.

True False 96. Valence electrons are involved when atoms form bonds.

True False 97. There are a maximum of 50 electrons in principal energy level number five.

True False 98. Atoms of the noble gas elements, Group VIII A (18), do not form bonds with any other elements.

True False 99. There are eight valence electrons in a chloride ion.

True False 100.The ions formed from Group IIA (2) atoms have charges of 2+.

True False 101.Cations tend to be formed from metal atoms, while anions are formed from non-metal atoms.

True False 102.The atoms of smallest radius are those of elements in top left hand part of the periodic table.

True False 103.The halogens, Group VII A (17) have the lowest ionization energies of any group in the periodic

table. True False

104.The last period in the periodic table is incomplete.

True False

ch2 Key 1. List the three primary particles found in an atom.

proton, electron and neutron

Denniston - Chapter 02 #1

2. What is the value of the mass number in the isotope ?

131


3. What is the term for atoms of the same element having different masses due to a different number of neutrons?

isotopes


4. What is the process by which certain isotopes emit particles and release large amounts of energy?

radioactive decay


5. What do we call electrically charged particles that result from the gain of one or more electrons by a parent atom?

anions


6. Dalton proposed that all atoms of an element have identical properties. Briefly, explain why this proposal is invalid.

Isotopes of an element have different properties, particularly their mass.


7. J. J. Thomson in 1897, announced that cathode rays consisted of a stream of _______.

electrons


8. In one sentence, state Rutherford's important contribution to our knowledge of atomic structure.

He concluded that atoms have a small, heavy, positively charged nucleus surrounded largely by empty space, occupied by electrons.


9. What instrument is used to study the wavelengths of light emitted and absorbed by atoms?

a spectrophotometer


10. In Bohr's model of the hydrogen atom, what is an "orbit"?

An orbit is a circular path followed by the electron.


11. In Bohr's theory of the atom, what is the number n (n = 1, 2, 3, ...) called?

quantum number


12. In one sentence, explain the meaning/consequences of Heisenberg's Uncertainty Principle.

It is impossible to know the exact position and momentum of a particle, such as an electron in an atom.


13. In modern atomic theory, Bohr's orbits are replaced by atomic orbitals. What is an atomic orbital?

It is a region of space where an electron is likely to be found; or, an electron "cloud".


14. Which two scientists in 1869 arranged the elements in order of increasing atomic masses to form a precursor of the modern periodic table of elements?

Mendeleev and Meyer


15. Who stated that the elements, when arranged according to their atomic masses, showed a distinct periodicity of their properties?

Dimitri Mendeleev


16. In the modern periodic table, how are the elements arranged?

by increasing atomic number


17. The modern periodic law states that the physical and chemical properties of the elements are periodic functions of what property?

atomic number


18. What do we call the horizontal row of elements on the periodic table?

periods


19. How many periods are found on the periodic table?

seven


20. Which period contains the element sodium?

period three


21. What do we call the columns of elements on the periodic table?

groups


22. For an atom, what number gives the number of electrons and protons found in that atom?

atomic number


23. What is the general name given to the elements of Group IA (1)?

alkali metals


24. What term is used for the elements straddling the "staircase" boundary between the metals and nonmetals?

metalloids


25. For a representative element, how can we deduce the number of valence electrons in a neutral atom from the position of the element in the periodic table?

the group number is also the number of valence electrons


26. In what way(s) are the three orbitals in the 2p sublevel similar? In what way(s) are they different?

They have the same shape and the same energy. They are oriented differently in space.


27. What requirement must be met in order for two electrons to coexist in the same orbital?

they must have opposite spins


28. State the Aufbau Principle.

Electrons occupy the available orbital of lowest energy first.


29. Give the electronic configuration in an atom of neon, element number 18.

1s22s22p6


30. Give the electronic arrangement in an atom of strontium, element number 38.

1s22s22p63s23p64s23d104p65s2


31. How many valence electrons are present in a chloride ion?

eight


32. State the Octet Rule.

Elements tend to react in such a way as to attain the electron configuration of the atoms of the noble gas nearest to them in the periodic table.


33. Give the name of a Group VIIA (17) ion that has the following electronic arrangement: 1s22s22p63s23p6

chloride


34. Give the complete electronic arrangement of a sulfide ion, S2-.

1s22s22p63s23p6


35. Atoms with the biggest radii occur in the _______ _______ region of the periodic table.

bottom left


36. How would you expect an Al3+ ion to compare in size with an Al atom? Explain why.

The ion will be much smaller. In forming the ion, the atom loses all its outermost electrons. The net positive charge on the ion ensures that all the electrons in the ion are strongly attracted to the nucleus, keeping the ion small.


37. Which group of elements has the highest ionization energies? Which group has the lowest?

Group VIIIA (18) are the highest; Group IA (1) are the lowest.


38. Explain what is meant by electron affinity.

It is the energy released when a neutral atom gains an electron to form an anion.


39. _________ is the ion responsible for the regulation of blood pressure and involved in the transmission of neural impulses.

Ca2+


40. What does the mass number minus the atomic number represent? A. Number of protonsB. Number of electronsC. Number of neutronsD. Number of protons - number of neutronsE. Number of neutrons - number of protons


41. In a neutral atom, what number equals the number of electrons? A. Atomic numberB. Mass numberC. Mass number minus the atomic numberD. Both A and CE. None of the above


42. Given that helium has an isotope , predict the number of electrons in a helium atom. A. 1B. 2C. 4D. 6E. 0


43. How many neutrons are present in an atom of the isotope ? A. 3B. 4C. 7D. 10E. none of the above


44. Microwaves, light and X-rays are all forms of ____________. A. ElectricityB. High energy electronsC. Electron repulsionD. Electromagnetic radiationE. Radioactivity


45. Where are the alkaline earth metals located on the periodic table? A. IA (1)B. IIA (2)C. IIIA (3)D. VIIA (17)E. VIIIA (18)


46. How many orbitals are in an s sublevel? How many in a p sublevel? A. S: 1, p: 2B. S: 2, p: 3C. S: 1, p: 3D. S: 2, p: 6E. S: 3, p: 3


47. How many electrons are present in an atom of silicon? A. 14B. 16C. 18D. 24E. 26


48. Give the name of a Group IA (1) ion that has the following electronic arrangement: 1s22s22p6 A. Lithium ionB. Sodium ionC. Potassium ionD. Magnesium ionE. Calcium ion


49. What ion carries two negative charges and is isoelectronic with K+? A. O2-

B. S2-

C. F2-

D. Cl2-

E. Ar2-


50. What kind(s) of particles can be found outside the nucleus of an atom? A. ProtonsB. NeutronsC. ElectronsD. Protons and electronsE. Protons and neutrons


51. The total mass of the protons in any neutral atom is about _______ times the total mass of electrons in the atom. A. 0.0005B. 0.3C. 1D. 2E. 2000


52. What is the quantity represented by the mass number minus the atomic number? A. Number of atomsB. Number of neutronsC. Number of electronsD. Number of protonsE. Number of particles in the nucleus


53. Which isotope of hydrogen has two neutrons? A. Hydrogen-1B. Hydrogen-2C. Hydrogen-3D. DeuteriumE. H2


54. Which of the following accounts for the fact that chlorine has an atomic mass of 35.45 amu rather than a whole number? A. IsotopesB. ElectronsC. ProtonsD. RadioactivityE. Isomers


55. Who discovered that cathode rays consist of a stream of negative particles, electrons? A. CrookesB. ThomsonC. GeigerD. RutherfordE. Bohr


56. Who discovered the existence of the atomic nucleus? A. CrookesB. ThomsonC. GeigerD. RutherfordE. Bohr


57. In Rutherford's experiment, which led to the discovery of the atomic nucleus, what type of particle or ray was fired at the gold foil target? A. AlphaB. BetaC. GammaD. NeutronsE. Cathode rays


58. In Mendeleev's table of the elements, they were arranged according to ______________. A. Atomic numberB. Mass numberC. Atomic massD. Neutron numberE. Density


59. The modern periodic table is arranged according to what property? A. Atomic numberB. Mass numberC. Atomic massD. Neutron numberE. Density


60. What do we call a complete horizontal row of elements on the periodic table? A. GroupB. PeriodC. FamilyD. Representative elementsE. Transition elements


61. What are all the elements in the A-groups often called? A. Transition elementsB. LanthanidesC. MetalsD. Non-metalsE. Representative elements


62. Which of the following elements is a metalloid? A. CB. GeC. PbD. NE. P


63. Where are the halogens located on the periodic table? A. Representative elementsB. Transition metalsC. Group VIIA (17)D. Group IIA (2)E. Group IIIA (3)


64. How many valence electrons are in an atom of carbon? A. 8B. 6C. 4D. 1E. 0


65. What is the lowest energy sublevel of a principal level? A. dB. eC. fD. sE. p


66. How many sublevels are there in the third principal energy level? A. 3B. 2C. 1D. 0E. 4


67. How many orbitals are there in the second principal energy level? A. 2B. 3C. 1D. 0E. 4


68. Which of the following correctly gives the electron capacity of a principal energy level in terms of the number n? A. nB. 2nC. 2n +

2D. N2

E. 2n2


69. What is the electron configuration of sulfur, atomic number 16? A. 1s21p62s22p6

B. 1s22s22p62d6

C. 1s22s22p63s23p4

D. 1s22s22p63s23d4

E. 1s22s22p63s22d4


70. Which one of the following electron configurations is appropriate for a normal atom? A. 1s12s1

B. 1s22s1

C. 1s22s22p8

D. 1s22s22p43s1

E. 1s22s22p63d1


71. Which of the following elements is most likely to form a 2+ ion? A. LiB. KC. AlD. NE. Cu


72. Give the complete electronic configuration of a sodium ion. A. 1s22s22p5

B. 1s22s22p6

C. 1s22s22p63s1

D. 1s22s22p63s2

E. 1s22s22p63s23p64s1


73. Which of the following ions does not follow the octet rule? A. Na+

B. Ca2+

C. Al3+

D. N3-

E. Cl2-


74. Which of the following atoms has the biggest size (radius)? A. NaB. AlC. ClD. RbE. I


75. Which of the following elements has the highest ionization energy? A. LiB. BC. OD. FE. He


76. Which of the following elements has the lowest ionization energy? A. LiB. BC. OD. FE. Ne


77. The electron affinity is _________________. A. The energy required to remove an electron from an isolated atomB. The force between two electrons in the same orbitalC. The force between two ions of opposite chargeD. The energy released when an isolated atom gains an electronE. The attraction of an atom for an electron in a chemical bond


78. Which one of the following elements has the highest electron affinity? A. LiB. KC. KrD. OE. Cl


79. Which of the following statements relating to Bohr's model of the hydrogen atom is incorrect? A. The lowest energy orbit has quantum number n = 1B. The highest energy orbits are farthest from the nucleusC. In a transition from the n = 3 to the n = 1 level, light is emittedD.

Energy differences between energy levels can be calculated from the wavelengths of the light absorbed or emitted

E. The Bohr model consists of energy levels that are evenly spaced, like the rungs of a ladder


80. Who proposed that electrons could behave like waves, as well as like particles? A. ThomsonB. RutherfordC. BohrD. De BroglieE. Heisenberg


81. In the calcium atom represented by the symbol , there are 20 protons, 20 neutrons and 20 electrons. TRUE


82. All atoms of a particular element have identical chemical properties. TRUE


83. An atom cannot be created, divided, destroyed or converted to any other type of atom. FALSE


84. The atomic number of an ion tells us the number of protons that are present. TRUE


85. If an atom gains one electron, it becomes an anion. TRUE


86. The first experimentally based theory of atomic structure was proposed by John Dalton. TRUE


87. J. J. Thomson was the first to state that an atom is mostly empty space. FALSE


88. Short wavelengths of electromagnetic radiation have more energy than long wavelengths. TRUE


89. Bohr was the first to use the term "orbit" to explain the fixed energy levels of electrons. TRUE


90. Niels Bohr developed a theory which accounted for the lines in the visible region of the hydrogen spectrum. TRUE


91. In Mendeleev's table, the elements were arranged according to their atomic mass. TRUE


92. There are nine periods on the periodic table. FALSE


93. Sulfur (S) is one of the representative elements. TRUE


94. Europium (Eu) is a lanthanide element. TRUE


95. Arsenic (As) is a metalloid. TRUE


96. Valence electrons are involved when atoms form bonds. TRUE


97. There are a maximum of 50 electrons in principal energy level number five. TRUE


98. Atoms of the noble gas elements, Group VIII A (18), do not form bonds with any other elements. FALSE


99. There are eight valence electrons in a chloride ion. TRUE


100. The ions formed from Group IIA (2) atoms have charges of 2+. TRUE


101. Cations tend to be formed from metal atoms, while anions are formed from non-metal atoms. TRUE


102. The atoms of smallest radius are those of elements in top left hand part of the periodic table. FALSE


103. The halogens, Group VII A (17) have the lowest ionization energies of any group in the periodic table. FALSE


104. The last period in the periodic table is incomplete. TRUE


ch2 Summary Category # of Questions

Denniston - Chapter 02 104

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