Chemistry in Focus A Molecular View of Our World 5th Edition by Nivaldo J. Tro

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Sample Test

Chapter 3—Atoms and Elements

MULTIPLE CHOICE

1. The most abundant element in the earth’s crust by mass is:

a.	Hydrogen
b.	Carbon
c.	Oxygen
d.	Silicon
e.	Nitrogen

ANS: C PTS: 1

2. Which of these statements about atoms is incorrect?

a.	Atoms are the smallest visible amount of an element.
b.	Atoms are composed of protons, neutrons, and electrons.
c.	Atoms are the building blocks of all matter.
d.	Atoms are the smallest identifiable unit of an element.
e.	There are 90 different naturally occurring atoms.

ANS: A PTS: 1

3. The number of protons in a neutral atom is equal to the ____ of the atom.

a.	Mass
b.	atomic weight
c.	atomic number
d.	mass number
e.	valence electron number

ANS: C PTS: 1

4. Which of these particles has a negative charge?

a.	Proton
b.	Neutron
c.	Electron
d.	Nucleus
e.	an atom

ANS: C PTS: 1

5. Which of these statements about an atom is incorrect?

a.	The number protons equals the number of electrons.
b.	The number of protons equals the atomic number.
c.	The number of protons equals the number of neutrons.
d.	The mass number is the sum of protons and neutrons in the atom.
e.	The mass number minus the atomic number equals the number of neutrons in the atom.

ANS: C PTS: 1

6. Which of these is the correct chemical symbol for carbon?

a.	C
b.	Ca
c.	Cl
d.	Cb
e.	Co

ANS: A PTS: 1

7. Which of these is the correct chemical symbol for cobalt?

a.	C
b.	Cl
c.	Co
d.	Ca
e.	Ce

ANS: C PTS: 1

8. Which of these is the correct chemical symbol for potassium?

a.	K
b.	Po
c.	P
d.	Pd
e.	Pt

ANS: A PTS: 1

9. Which of the following is not true for an atom that has an atomic number of 19 and a mass number of 41?

a.	The atom contains 22 neutrons.
b.	The atom is potassium.
c.	The atom contains 19 neutrons.
d.	The atom contains 19 electrons.
e.	The atom contains 19 protons.

ANS: C PTS: 1

10. Which statement about electrons is incorrect?

a.	Electrons are negatively charged.
b.	Electrons have a negligible mass compared to the rest of the atom.
c.	Electrons exist in the nucleus of the atom..
d.	The number of electrons equals the atomic number in a neutral atom.
e.	Both B and D are incorrect statements.

ANS: C PTS: 1

11. Nonmetals tend to _____ electrons to form ions of ________ charge.

a.	lose, negative
b.	lose, positive
c.	gain, positive
d.	gain, negative

ANS: D PTS: 1

12. Metals tend to __________ electrons to form ions of _______ charge.

a.	lose, negative
b.	lose, positive
c.	gain, positive
d.	gain, negative

ANS: B PTS: 1

13. Determine the correct number of protons and electrons in P^3– ?

a.	3 protons, 6 electrons
b.	15 protons, 18 electrons
c.	15 protons, 12 electrons
d.	31 protons, 28 electrons
e.	31 protons, 34 electrons

ANS: B PTS: 1

14. Determine the correct number of protons and electrons in F^–?

a.	9 protons, 10 electrons
b.	9 protons, 11 electrons
c.	10 protons, 9 electrons
d.	11 protons, 10 electrons
e.	19 protons, 20 electrons

ANS: A PTS: 1

15. A certain ion contains 47 protons and 46 electrons. The ion is:

a.	Pd⁺
b.	Pd^–
c.	Ag⁺
d.	Ag^–
e.	Can’t tell from the given information

ANS: C PTS: 1

16. What is the charge on an ion that contains 16 protons and 18 electrons?

a.	0
b.	+2
c.	-2
d.	It depends on the number of neutrons.
e.	None of these.

ANS: C PTS: 1

17. How many electrons are there in ¹⁵N^3–?

a.	15
b.	18
c.	12
d.	4
e.	10

ANS: E PTS: 1

18. Which of these particles has the smallest mass?

a.	a proton
b.	a neutron
c.	an electron
d.	a hydrogen atom
e.	a hydrogen nucleus

ANS: C PTS: 1

19. When an oxygen atom gains two electrons, it becomes (a)n ____ with a charge of ____.

a.	anion, 2⁺
b.	anion, 2^–
c.	cation, 2^–
d.	cation, 2⁺
e.	cation, 0

ANS: B PTS: 1

20. When a strontium atom loses two electrons, it becomes (a)n ____ with a charge of ____.

a.	anion, 2⁺
b.	anion, 2^–
c.	cation, 2^–
d.	cation, 2⁺
e.	cation, 0

ANS: D PTS: 1

21. Metals tend to form ions with a positive charge. The most likely way to form a positively charged ion from an atom is by doing which of the following?

a.	Gaining electron(s).
b.	Gaining proton(s).
c.	Losing electron(s).
d.	Losing proton(s).
e.	Losing neutron(s).

ANS: C PTS: 1

22. Which of these statements best describes the formation of an anion?

a.	An atom loses one or more electrons and becomes positively charged.
b.	An atom loses one or more electrons and becomes negatively charged.
c.	An atom gains one or more electrons and becomes positively charged.
d.	An atom gains one or more electrons and becomes negatively charged.
e.	None of these are correct.

ANS: D PTS: 1

23. Which of these statements best describes the formation of a cation?

a.	An atom loses one or more electrons and becomes positively charged.
b.	An atom loses one or more electrons and becomes negatively charged.
c.	An atom gains one or more electrons and becomes positively charged.
d.	An atom gains one or more electrons and becomes negatively charged.
e.	None of these are correct.

ANS: A PTS: 1

24. The Ca²⁺ ion contains ____ protons and ____ electrons.

a.	20, 20
b.	20, 22
c.	22, 20
d.	18, 20
e.	20, 18

ANS: E PTS: 1

25. The Cl^– ion contains ____ protons and ____ electrons.

a.	17, 17
b.	17, 18
c.	18, 16
d.	18, 18
e.	16, 17

ANS: B PTS: 1

26. How many protons, neutrons and electrons are in an ²⁵Mg⁺² ion?.

a.	12 protons, 12 electrons, 13 neutrons
b.	12 protons, 10 electrons, 12 neutrons
c.	13 protons, 10 electrons, 12 neutrons
d.	12 protons, 10 electrons, 13 neutrons
e.	12 protons, 14 electrons, 13 neutrons

ANS: D PTS: 1

27. Which of these is the correct representation for the ion with Z=27, A=60, and C=2⁺ ?

a.
b.
c.
d.
e.

ANS: A PTS: 1

28. What are the Z and A values for an atom of silicon which contains 15 neutrons?

a.	Z=14, A=15
b.	Z=15, A=14
c.	Z=29, A=14
d.	Z=14, A=29
e.	Z=15, A=29

ANS: D PTS: 1

29. Isotopes of an element have the same number of ____ but a different number of ____.

a.	neutrons, protons
b.	electrons, protons
c.	protons, neutrons
d.	neutrons, electrons
e.	protons, electrons

ANS: C PTS: 1

30. What are the Z and A values for an atom of krypton which contains 46 neutrons?

a.	Z=36, A=46
b.	Z=46, A=36
c.	Z=36, A=82
d.	Z=82, A=36
e.	Z=82, A=46

ANS: C PTS: 1

31. Radon -222 has ____ protons, ____ neutrons, and ____ electrons.

a.	86, 86, 86
b.	86, 222, 86
c.	86, 136, 86
d.	86, 136, 222
e.	86, 222, 308

ANS: C PTS: 1

32. How many protons (p), neutrons (n), and electrons (e) are in an atom of ²³⁵U?

a.	92 p, 146 n, 92 e
b.	92 p, 143 n, 92 e
c.	92 p, 92 n, 146 e
d.	92 p, 92 n, 92 e
e.	92 p, 51 n, 92 e

ANS: B PTS: 1

33. Carbon has three isotopes: ¹²C, ¹³C, and ¹⁴C. These isotopes each have ____ protons, ____ electrons and ____, ____, and ____ neutrons respectively.

a.	6, 6 and 6, 7, 8
b.	12, 12, and 6, 7, 8
c.	12, 12, and 12, 13, 14
d.	6, 6 and 12, 13, 14
e.	12, 12, and 24, 25, 26

ANS: A PTS: 1

34. An element has two naturally occurring isotopes. One has an abundance of 37.4% and an isotopic mass of 184.953 amu. The other has an abundance of 62.6% and a mass of 186.956 amu. What is the atomic weight of the element?

a.	185.702 amu
b.	185.954 amu
c.	186.207 amu
d.	186.956 amu
e.	190.234 amu

ANS: C PTS: 1

35. Chlorine has two isotopes, 35Cl and 37Cl that have the respective percent abundance’s of 75.77% and 24.23% and masses of 34.9688 amu and 36.9659 amu. Calculate the atomic weight of chlorine.

a.	37.54 amu
b.	36.65 amu
c.	35.45 amu
d.	34.97 amu
e.	36.97 amu

ANS: C PTS: 1

36. Rubidium consists of two naturally occurring isotopes rubidium-85 and rubidium-87. Rubidium-85 (⁸⁵Rb) has an isotopic mass of 84.9117 amu and a 72.15% abundance. Rubidium-87(⁸⁷Rb) has a 27.85% abundance. The atomic weight of rubidium is 85.4768 amu. Determine the isotopic mass of ⁸⁷Rb?

a.	86.72371 amu
b.	86.8013 amu
c.	86.8220 amu
d.	86.8621 amu
e.	86.9085 amu

ANS: E PTS: 1

37. Copper has two naturally occuring isotopes. Cu-63 has a mass of 62.939 amu and Cu-65 has a mass of 64.928 amu. Based on the atomic mass of copper, which isotope has a higher fractional abundance?

a.	Cu-63
b.	Cu-65
c.	Both have the same fractional abundance.
d.	Not enough information to tell.

ANS: A PTS: 1

38. There are three isotopes of neon. Assuming the mass of each isotope is very close to its mass number, which isotope is most abundant based on the atomic mass of neon (Ne)?

a.	Ne-20
b.	Ne-21
c.	Ne-22
d.	Can’t tell from the given information.

ANS: A PTS: 1

39. Mendeleev organized the elements of the periodic table

a.	by increasing atomic number and similar properties.
b.	by increasing atomic weight and similar properties.
c.	by increasing number of electrons.
d.	by increasing number of isotopes.
e.	alphabetically.

ANS: B PTS: 1

40. Which scientist is responsible for the organization of the modern Periodic Table?

a.	Bohr
b.	Galileo
c.	Dalton
d.	Avogadro
e.	Mendeleev

ANS: E PTS: 1

41. Which of these elements is a metal?

a.	Mg
b.	Br.
c.	Ar
d.	Ge
e.	B

ANS: A PTS: 1

42. Which of these statements concerning atomic mass is correct?

a.	Atomic mass is the same as the mass number of the most common isotope.
b.	Atomic mass is derived from the weight of the most common isotope of the element.
c.	Atomic mass is determined by adding the masses of the protons, electrons, and neutrons in the atom.
d.	Atomic mass is calculated from the atomic mass of the two most common isotopes.
e.	Atomic mass is a weighted average of the masses of the naturally occurring isotopes.

ANS: E PTS: 1

43. Which of these elements is a metalloid?

a.	Ge
b.	Br
c.	Ar
d.	Ca
e.	Fe

ANS: A PTS: 1

44. Which of these is a nonmetal?

a.	Mg
b.	Br
c.	Cu
d.	Ge
e.	Li

ANS: B PTS: 1

45. Which element is not a non-metal?

a.	P
b.	I
c.	N
d.	K
e.	Cl

ANS: D PTS: 1

46. Which scientist is responsible for the theory which explains why properties of elements recur in a periodic fashion?

a.	Bohr
b.	Galileo
c.	Dalton
d.	Avogadro
e.	Mendeleev

ANS: A PTS: 1

47. Which of the following elements is generally not found in diatomic form in nature?

a.	C
b.	N
c.	O
d.	F

ANS: A PTS: 1

48. What is the maximum number of electrons which can occupy the orbit n=2?

a.	2
b.	6
c.	8
d.	10
e.	18

ANS: C PTS: 1

49. What is the total number of electrons which can occupy the first and second principal energy levels (n=1, n=2)?

a.	2
b.	6
c.	8
d.	10
e.	18

ANS: D PTS: 1

50. Which of these statements about Bohr’s model of the atom is incorrect?

a.	Electrons fill lower energy orbits first.
b.	The greater the quantum number the higher the energy of an orbit.
c.	Electrons occupy orbits with certain radii corresponding to discrete energies.
d.	Elements with the same number of electrons in their outer orbit have similar properties.
e.	All of these statements are correct.

ANS: E PTS: 1

51. He has the same number of valence electrons as ______.

a.	H
b.	Ne
c.	Be
d.	F

ANS: C PTS: 1

52. Elements in the same group have the same ____.

a.	Mass number
b.	atomic number
c.	number of protons
d.	number of electrons
e.	number of valence electrons

ANS: E PTS: 1

53. The elements of group IA will all form ions. These ions will be ____ and will have a charge of ____.

a.	cations, 2+
b.	anions, 2-
c.	cations, 3+
d.	anions, 1-
e.	cations, 1+

ANS: E PTS: 1

54. The elements of group VIIA will all form ions. These ions will be ____ and will have a charge of ____.

a.	cations, 2+
b.	anions, 2-
c.	cations, 3+
d.	anions, 1-
e.	cations, 1+

ANS: D PTS: 1

55. Which of these elements has two valence electrons?

a.	Mg
b.	Li
c.	Al
d.	S
e.	Cl

ANS: A PTS: 1

56. Which of these elements has three valence electrons?

a.	Mg
b.	Li
c.	Al
d.	S
e.	Cl

ANS: C PTS: 1

57. Which of these elements has seven valence electrons?

a.	Mg
b.	Li
c.	Al
d.	S
e.	Cl

ANS: E PTS: 1

58. Which of the following is true.

a.	Argon and chlorine have the same number of electrons.
b.	Argon and chlorine have the same number of valence electrons.
c.	Argon and neon have the same number of electrons.
d.	Argon and neon have the same number of valence electrons.
e.	There is more than one correct statement.

ANS: D PTS: 1

59. Which of the following is true.

a.	Argon and chlorine have a different number of electrons.
b.	Argon and chlorine have a different number of valence electrons.
c.	Argon and neon have a different number of electrons.
d.	Argon and neon have a different number of valence electrons.
e.	There is more than one correct statement.

ANS: E PTS: 1

60. These elements Li, Na, K, Rb and Cs are members of what group/family?

a.	halogen
b.	noble gas
c.	alkali metal
d.	transition metal
e.	alkaline earth metals

ANS: C PTS: 1

61. Strontium is a member of what group/family?

a.	halogen
b.	noble gas
c.	alkali metal
d.	transition metal
e.	alkaline earth metals

ANS: E PTS: 1

62. Bromine is a member of what group/family?

a.	halogen
b.	noble gas
c.	alkali metal
d.	transition metal
e.	alkaline earth metals

ANS: A PTS: 1

63. Which of these elements is not a transition metal?

a.	Cu
b.	Fe
c.	Na
d.	Ag
e.	Hg

ANS: C PTS: 1

64. Which family/group is largely unreactive?

a.	halogen
b.	noble gas
c.	alkali metal
d.	transition metal
e.	alkaline earth metals

ANS: B PTS: 1

65. Which of the following is true.

a.	Oxygen and sulfur are in the same group.
b.	Oxygen and sulfur are in different groups.
c.	Oxygen and sulfur are in the same period.
d.	Oxygen and sulfur are in different periods.
e.	Both A + D are correct.

ANS: E PTS: 1

66. Which of these groups is incorrectly matched with its group/family name?

	Group	Name
I.	2A	alkaline earth metals
II.	3A	alkali metals
III.	7A	halogens
IV.	8A	noble gases
V.	2B – 3B	transition metals

a.	I
b.	II
c.	III
d.	IV
e.	V

ANS: B PTS: 1

67. The atomic mass of fluorine (F) is 19.00. Which of the following is not true?

a.	An atom of F has a mass of 19.00 amu.
b.	One mole of F has a mass of 19.00 g.
c.	6.02 x 10²³ atoms of F has a mass of 19.00 g.
d.	6.02 x 10²³ atoms of F has a mass of 19.00 amu.

ANS: D PTS: 1

68. What is the correct number of atoms in one mole of aluminum?

a.	12
b.	26.98
c.	6.022 ´ 10²³
d.	13
e.	14

ANS: C PTS: 1

69. What is the correct number of atoms in one mole of neon?

a.	10
b.	11
c.	6.022 ´ 10²³
d.	20
e.	12

ANS: C PTS: 1

70. One mole of nickel (Ni) has a mass of _________.

a.	28 amu
b.	28 g
c.	58.71 amu
d.	58.71 g

ANS: D PTS: 1

71. Determine the mass of one mole of silver.

a.	107.87 amu
b.	107.87 g
c.	47 amu
d.	47 g
e.	6.022 ´ 10²³ amu

ANS: B PTS: 1

72. Calculate the number of moles in a 2.98 g sample of aluminum.

a.	0.0124 moles
b.	0.110 moles
c.	80.4 moles
d.	1.79 ´ 10²⁴ moles
e.	1.62 ´ 10²⁵ moles

ANS: B PTS: 1

73. Calculate the number of moles in a 233 gram sample of barium.

a.	0.589 moles
b.	1.70 moles
c.	3.20 ´ 10⁴
d.	6.022 ´ 10²³ moles
e.	1.02 ´ 10²⁴ moles

ANS: B PTS: 1

74. Calculate the number of moles of lead in a 442 gram lead anvil.

a.	0.468 moles
b.	2.13 moles
c.	96.97 moles
d.	6.022 ´ 10²³ moles
e.	1.28 ´ 10²⁴ moles

ANS: B PTS: 1

75. Calculate the number of moles in a 25.0 g sample of carbon.

a.	2.08 moles
b.	13.0 moles
c.	300 moles
d.	1.51 ´ 10²⁵ moles
e.	3.33 ´ 10^–3 moles

ANS: A PTS: 1

76. Determine the number of atoms in a copper strip that has a mass of 35.0 grams.

a.	3.33 ´ 10²⁵ atoms
b.	2.11 ´ 10²⁵ atoms
c.	2.71 ´ 10²⁰ atoms
d.	3.32 ´ 10²³ atoms
e.	0.551 atoms

ANS: D PTS: 1

77. Determine the number of atoms in a piece of ultrapure silicon that has amass of 15.0 grams.

a.	1.13 ´ 10²⁴ atoms
b.	1.69 ´ 10²⁵ atoms
c.	2.54 ´ 10²⁰ atoms
d.	3.21 ´ 10²³ atoms
e.	9.03 ´ 10²⁴ atoms

ANS: D PTS: 1

78. Determine the mass in grams of 1.15 ´ 10²³ atoms of cobalt.

a.	0.191 grams
b.	5.23 grams
c.	11.2 grams
d.	12.4 grams
e.	308 grams

ANS: C PTS: 1

79. Determine the mass in grams of 3.45 ´ 10²⁵ molecules of oxygen, O₂?

a.	0.556 grams
b.	57.2 grams
c.	458 grams
d.	916 grams
e.	1.83 ´ 10³ grams

ANS: E PTS: 1

80. Determine the mass in grams of one molecule of water, H₂O?

a.	2.99 ´ 10^–23 g
b.	1.08 ´ 10²⁵ g.
c.	10 grams
d.	18 grams
e.	None of the above.

ANS: A PTS: 1

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