Deck 2: Atoms and the Atomic Theory

Question 1

A 25 g sample of sugar is found to contain 51.4% oxygen by mass. Another 250 g sample of the same sugar is also 51.4% oxygen by mass. This is consistent with the:

A) law of conservation of mass
B) law of constant composition
C) law of multiple proportions
D) first assumption of Dalton's atomic theory
E) second assumption of Dalton's theory

Answer 1

law of constant composition

Question 2

Isotopes have different atomic number (Z) but the same mass number (A).

Answer 2

False

Question 3

Choose the INCORRECT statement.

A) The Law of Constant Composition is the Law of Definite Proportions.
B) Objects of like charge repel each other.
C) Electrons were once known as cathode rays.
D) Alpha particles are the same mass as a helium nucleus.
E) Gamma rays are the same as electrons.

Answer 3

Gamma rays are the same as electrons.

Question 4

Dalton's atomic theory is based on several assumptions, which are listed below. Which of these assumptions is strictly correct? I) All atoms of the same element are identical.
II) Atoms are indivisible and unchangeable.
III) Chemical changes are the result of the combination, separation, and rearrangement of atoms.

A) I, II, and III are correct.
B) I and III are correct.
C) II and III are correct.
D) I and II are correct.
E) III is correct.

Question 5

Choose the INCORRECT statement from those given below.

A) Atoms retain their identity during a chemical reaction.
B) All matter is composed of atoms.
C) Atoms combine in small, whole-numbered ratios.
D) All atoms of a given element are identical.
E) Different ratios of atoms produce different compounds.

Question 6

All atoms of a given element are identical.

Question 7

Atoms combine in small, whole-numbered ratios.

Question 8

All matter is composed of atoms.

Question 9

Which of the following statements is FALSE?

A) Michael Faraday discovered cathode rays.
B) J .J. Thomson suggested the "plum pudding" model of the atom.
C) Robert Millikan determined the charge on an electron.
D) J. J. Thomson determined the charge-to-mass ratio for electrons.
E) Michael Faraday determined that cathode rays were the fundamental negatively charged particles and called them electrons.

Question 10

Choose the correct statement.

A) Neutrons have no charge and no mass.
B) An electron has 1/1837 the mass of a proton.
C) The atomic number is the total number of protons and neutrons in the nucleus.
D) The charge of a proton is 1837 times the charge of an electron.
E) Electrons and protons have about the same mass.

Question 11

A 0.920-gram sample of magnesium is allowed to burn in 0.321 g of oxygen gas. The sole product is magnesium oxide. After the reaction, no oxygen remains and 0.809 g of magnesium oxide has been formed. What mass of magnesium is left unreacted?

A) 0.210 g
B) 0.432 g
C) 1.408 g
D) 0.111 g
E) 0.488 g

Question 12

Robert Millikan determined the charge on an electron.

Question 13

Which of the following would be unaffected by an electric field?

A) alpha particles
B) beta particles
C) gamma rays
D) protons
E) electrons

Question 14

Different ratios of atoms produce different compounds.

Question 15

Atoms retain their identity during a chemical reaction.

Question 16

The vertical columns in the periodic table of the elements are called groups.

Question 17

J. J. Thomson suggested the "plum pudding" model of the atom.

Question 18

The number of protons and neutrons in the nucleus of a given atom is called the atomic number.

Question 19

When a chemical reaction is carried out in a sealed container, the substances may change in color, temperature, or state, but no change in mass is detected. This is evidence of the:

A) law of conservation of mass
B) law of constant composition
C) law of definite proportions
D) existence of electrons
E) existence of protons

Question 20

When decomposed chemically, 73.0 grams of a sample of HCl produce 71.0 g of Cl2 and 2.0 g of H2, while 34.0 g of a sample of H2S produce 32.0 g of S and 2.0 g of H2. This is an example of the Law:

A) of Conservation of Mass
B) of Multiple Proportions
C) of Definite Proportions
D) E = mc2
E) of Simple Whole Numbers

Question 21

Which statement below is true?

A) Metals gain electrons to have a positive charge.
B) Metals gain electrons to have a negative charge.
C) Metals lose electrons to have a positive charge.
D) Nonmetals lose electrons.
E) Transition metals can gain 2 or more electrons to become metal ions.

Question 22

What is the mass in grams of 1 atom of sulfur (atomic mass = 32.066)?

A) 1.661 × 10-24 g
B) 1.931 × 10-25 g
C) 5.325 × 10-23 g
D) 5.179 × 10-26 g
E) 5.989 × 10-23 g

Question 23

How many arsenic atoms are in 5.21 g of arsenic?

A) 0.0695 atoms
B) 9.51 × 1022 atoms
C) 3.14 × 1024 atoms
D) 2.10 × 1022 atoms
E) 4.19 × 1022 atoms

Question 24

The atomic weight of chlorine is very close to 35.5. This means that:

A) chlorine occurs with a variable number of protons
B) a variable number of electrons gives the fractional weight
C) on the average, an atom of chlorine weighs almost 3 times as much as carbon
D) the actual weight of a chlorine atom is not known very precisely
E) chlorine atoms contain half of a proton

Question 25

Beta particles:

A) have a mass of 4 and a charge of +2
B) are like X-rays
C) are repelled by a positively charged plate
D) are electrons
E) have the same mass as a neutron

Question 26

Which of the following is a correct feature of the nuclear atom proposed by Rutherford?

A) All atoms of an element have the same mass.
B) The atom is mostly empty space.
C) The number of neutrons and electrons in the atom are equal.
D) The majority of alpha particles to strike the foil "bounced back."
E) It is like the "plum pudding" model.

Question 27

Ernest Rutherford is credited with: I) the nuclear model of the atom
II) the identification of alpha and beta particles
III) the discovery of protons
IV) the prediction of a third, neutral, subatomic particle

A) I and II
B) I and III
C) I, II, III
D) II, III, IV
E) I, II, III, IV

Question 28

Which of the following statements is true concerning the masses of individual Cl atoms?

A) All atoms have a mass of 35.45 u.
B) Most of the atoms have a mass of 35.45 u.
C) Some of the atoms have a mass of 35.45 u.
D) None of the atoms have a mass of 35.45 u.
E) All atoms have a mass of 17 u.

Question 29

Choose the information a mass spectrometer is unable to provide.

A) the relative abundance of two isotopes of potassium
B) the number of protons in potassium
C) the atomic mass of a single isotope of potassium
D) the mass of a proton
E) the number of stable isotopes of potassium

Question 30

A hypothetical element, E, has two stable isotopes: E-46 = 46.046 u 64.08% E-51 = 50.826 u 35.92%
What is the average atom weight of the element?

A) 47.76 u
B) 48.44 u
C) 49.11 u
D) 48.50 u
E) 47.44 u

Question 31

Which of these atoms has the greatest number of neutrons in its nucleus?

A)
B)
C)
D)
E)

Question 32

Choose the INCORRECT statement.

A) Gamma rays are bent by magnetic fields as a ray of positive charges.
B) Protons and neutrons are found in the nucleus.
C) Protons and neutrons are close to the same mass.
D) The atomic number is the proton number.
E) The mass number is the number of protons plus neutrons.

Question 33

A hypothetical element, E, has two stable isotopes. E-38 = 38.012 u 75.68%
E-46 = 45.981 u 24.32%
The element's atomic mass would be closest to which of the elements?

A) K
B) Ar
C) Ca
D) Sc
E) Cl

Question 34

31.0 grams of the element phosphorus contain:

A) 6.02 × 1023 P4 molecules
B) 31.0 × (6.02 × 1023) P atoms
C) 6.02 × 1023 P atoms
D) 31.0 P atoms
E) 31.0 moles of P

Question 35

Which of the following is a metalloid?

A) mercury
B) selenium
C) bismuth
D) radium
E) calcium

Question 36

A species that differs in charge from another atom of the same element:
I. is called an isotope
II. has more or less neutrons
III. has lost or gained electrons
IV. is called an ion
V. has the same number of protons

A) I and II
B) I and III
C) II and IV
D) III and IV
E) III, IV, V

Question 37

An element has 5 stable isotopes. The mass and percentage of each are: 89.9043 51.46%
90)9053 11.23%
91)9046 17.11%
93)9061 17.40%
95)9082 2.80%
The element is which of the following?

A) Nb
B) Y
C) Sr
D) Zr
E) Rb

Question 38

An element has 5 stable isotopes. The mass and percentage of each are: 69.9243 20.52%
71)9217 27.43%
72)9234 7.76%
73)9219 36.54%
75)9214 7.76%
The element is which of the following?

A) As
B) Se
C) Ge
D) Ga
E) Zn

Question 39

What is the mass number of the most abundant form of oxygen atom?

A) 15.9994
B) 8
C) 16
D) 24
E) 32

Question 40

Groups, or families, on the periodic table are:

A) vertical columns of elements with similar properties
B) horizontal rows of elements with increasing atomic numbers
C) named for the first elements in the series; such as "actinides"
D) extremely reactive with each other
E) elements that all occur naturally in the same state

Question 41

The total number of neutrons in an 192Ir2+ cation is ________.

A) 115
B) 77
C) 192
D) 75
E) 269

Question 42

How many atoms of sulfur are in 280 g of a 50% by mass H2SO4 solution?

A) 8.6 × 1025 atoms
B) 8.6 × 1023 atoms
C) 8.0 × 1025 atoms
D) 8.0 × 1023 atoms
E) 2.8 × 1029 atoms

Question 43

How many atoms of silicon are contained in 8.50 × 10-5 grams?

A) 1.44 × 1023 atoms
B) 1.82 × 1018 atoms
C) 5.02 × 1030 atoms
D) 5.02 × 1018 atoms
E) 1.82 × 1020 atoms

Question 44

A cubic centimeter of lead weighs 11.35 g. How many atoms are in the block?

A) 6.8 × 1024 atoms
B) 2.4 × 1023 atoms
C) 3.3 × 1022 atoms
D) 5.3 × 1022 atoms
E) 1.1 × 1025 atoms

Question 45

How many atoms of rubidium-85 are in 87.2 g of rubidium? Rubidium-85 is 72.2 % abundant.

A) 5.16 × 1046 atoms
B) 4.44 × 1023 atoms
C) 8.51 × 1023 atoms
D) 6.14 × 1022 atoms
E) 1.02 × 1024 atoms

Question 46

A certain mass of nickel reacts with sulphur to produce 2.83 g of NiS. The same mass of nickel reacts completely with 0.5 g of oxygen to produce 2.33 g of NiO. How many grams of sulfur reacted in the first reaction?

A) 0.5 g
B) 1 g
C) 1.5 g
D) 10-1 g
E) 1.25 g

Question 47

A 1.4 g sample of calcium is reacted with 3.2 g of oxygen. The only product after the reaction is 1.96 g of CaO. How many grams of oxygen remains unreacted?

A) 0.56 g
B) 0.224 g
C) 2.64 g
D) 0.264 g
E) 0.203 g

Question 48

Which is the proper chemical symbol for tungsten?

A) Te
B) Ti
C) Tm
D) W
E) Tc

Question 49

What mass of magnesium is necessary to make 10.5 g of magnesium bromide if 1.04 g of magnesium makes 7.88 g of magnesium bromide?

A) 1.39 g
B) 79.9 g
C) 1.58 g
D) 3.66 g
E) 7.89 g

Question 50

How many Cu atoms are present in a 75.0 cm length of 20-gauge copper wire? A 20-gauge wire has a diameter of 0.03196 in. Copper's density is 8.92 g/cm3.

A) 1.31 × 1021
B) 3.28 × 1022
C) 8.08 × 1021
D) 1.04 × 1022
E) 2.08 × 1022

Question 51

A sample of pure carbon weighing 1.48 g was burned in an excess of air. The mass of carbon dioxide, the sole product, was 5.42 g. In a second experiment, 11.62 g of carbon dioxide was obtained. What mass of carbon was burned in the second experiment?

A) 42.6 g
B) 3.17 g
C) 3.54 g
D) 0.866 g
E) 11.6 g

Question 52

If the density of lead is 11.34 g/cm3, how many atoms are in a piece of lead that is 2.00 cm wide, 1.00 m long, and 2.00 mm thick?

A) 1.32 × 1024 atoms
B) 1.16 × 1023 atoms
C) 1.32 × 1023 atoms
D) 1.16 × 1022 atoms
E) 6.60 × 1023 atoms

Question 53

How many atoms of lead are required to cover a 33.0 cm by 45.0 cm area with a sheet of lead that is 0.140 mm thick? The density of lead is 11.35 g/cm3.

A) 6.86 × 1023
B) 2.29 × 1026
C) 2.29 × 1025
D) 6.86 × 1022
E) 1.42 × 1026

Question 54

With mass spectral data the ratio of the mass of 14N/12C was found to be 1.167. What is the mass of the 14N atom?

A) 14.017 u
B) 10.292 u
C) 14.004 u
D) 17.000 u
E) 14.007 u

Question 55

A 3.214 g sample of magnesium reacts with 8.416 g of bromine. The only product is magnesium bromide. If 1.934 g of magnesium is left unreacted, how much magnesium bromide is formed?

A) 1.280 g
B) 5.202 g
C) 9.696 g
D) 7.136 g
E) 3.268 g

Question 56

How many moles are represented by 2.5 × 1015 Na atoms?

A) 3.8 × 10-10 mol
B) 1.8 × 10-10 mol
C) 1.5 × 1039 mol
D) 4.2 × 10-9 mol
E) 1.1 × 1014 mol

Question 57

57.7 g Ni contains how many atoms?

A) 6.13 × 1023 atoms
B) 3.47 × 1023 atoms
C) 5.92 × 1023 atoms
D) 1.24 × 1024 atoms
E) 0.983 atoms

Question 58

The natural abundance of calcium in the earth's crust is 3.4% by mass. How many calcium atoms are present in a 1.50 g sample of the earth's crust?

A) 6.6 × 1023 atoms
B) 3.1 × 1022 atoms
C) 7.7 × 1020 atoms
D) 7.7 × 1022 atoms
E) 5.1 × 1020 atoms

Question 59

How many atoms of hydrogen are present in 1.5 lb of hydrogen peroxide, which is 5.93% hydrogen? (1 lb = 454 grams)

A) 2.4 × 1025 atoms
B) 1.21 × 1025 atoms
C) 1.2 × 1025 atoms
D) 2.41 × 1025 atoms
E) 1.2 × 1020 atoms

Question 60

Write the symbol for the radioactive isotope phosphorus-32.

A)
B)
C)
D)
E)

Question 61

Write the symbol for the most common ion formed by sulfur.

A) S-1
B) S-2
C) S+1
D) S+2
E) requires experimental data

Question 62

The average atomic mass of B is 10.80 u. Boron has only two stable forms (10.00 u) and (11.00 u). What is the natural percent abundance of ?

A) 80%
B) 20%
C) 1.0%
D) 3.8%
E) 75%

Question 63

Copper occurs in an isotopic mixture of 69.09% 63Cu (mass = 62.93 u per atom) and 30.91% 65Cu (mass = 64.93 u per atom). What is the average atomic mass of copper?

A) 64.00 u
B) 63.55 u
C) 63.45 u
D) 64.31 u
E) 29.00 u

Question 64

Rubidium possesses two stable forms and has an average mass of 85.5. 85Rb has a mass of 84.9 and a percent abundance of 72.2%. What is the mass of the other form of Rb?

A) 86.1 u
B) 85.7 u
C) 88.3 u
D) 87.1 u
E) 89.4 u

Question 65

How many protons, neutrons, and electrons are in ?

A) 12 protons, 10 electrons, 12 neutrons
B) 12 protons, 12 electrons, 12 neutrons
C) 12 protons, 12 electrons, 24 neutrons
D) 24 protons, 10 electrons, 12 neutrons
E) 10 protons, 12 electrons, 24 neutrons

Question 66

The total numbers of neutrons, protons, and electrons in 35Cl- are ________.

A) 17 neutrons, 35 protons, 36 electrons
B) 35 neutrons, 17 protons, 18 electrons
C) 18 neutrons, 17 protons, 16 electrons
D) 18 neutrons, 17 protons, 18 electrons
E) 17 neutrons, 17 protons, 17 electrons

Question 67

The total numbers of neutrons, protons, and electrons in 31P3- are:

A) 15 neutrons, 31 protons, 15 electrons
B) 16 neutrons, 15 protons, 18 electrons
C) 31 neutrons, 15 protons, 18 electrons
D) 15 neutrons, 16 protons, 12 electrons
E) 16 neutrons, 16 protons, 18 electrons

Question 68

The three naturally occurring isotopes of magnesium are 24Mg (23.985042 u, 78.99%), 25Mg (24.985837, 10.00%), and 26Mg. What is the atomic mass of 26Mg?

A) 25.98 u
B) 48.67 u
C) 23.94 u
D) 26.43 u
E) 24.31 u

Question 69

A new element is discovered. It has two isotopes. The relative abundance of the isotopes and their masses are 18% isotope 1, mass 350.0 u and 82% isotope 2, mass 352.0 u. What is the atomic mass of the element?

A) 351.6
B) 351.0
C) 350.4
D) 352.0
E) 350.0

Question 70

Which is the more abundant isotope, Cl-35 or Cl-37?

A) The two isotopes are equal in abundance.
B) Cl-37
C) Cl-35
D) A third unstable isotope is more abundant.
E) Cl-17

Question 71

An isotope with mass number 81 has eleven more neutrons than protons. This is an isotope of what element?

A) Tl
B) Yb
C) Zr
D) Br
E) Nb

Question 72

A cation has 13 neutrons and 10 electrons. If it has a charge of +1, what is its correct symbol?

A)
B)
C)
D)
E)

Question 73

Silver possesses two stable isotopes: 107Ag (106.90 u) and 109Ag (108.90 u). If the average atomic mass of Ag is 107.87 u, what is the percent abundance of 107Ag?

A) 48.5%
B) 50.0%
C) 51.5%
D) 46.3%
E) 53.8%

Question 74

There are two stable isotopes of supposium (Su). Su-191 = 190.9609 u (27.30%) Su-194 = 193.9633 u (72.70%)
Compute the atomic mass of supposium.

A) 190.9 u
B) 194.0 u
C) 191.8 u
D) 192.5 u
E) 193.1 u

Question 75

An anion has 45 neutrons and 36 electrons. If it has a -1 charge, what is its correct symbol?

A)
B)
C)
D)
E)

Question 76

Write the appropriate symbol for the species containing 18 neutrons, 17 protons, and 16 electrons.

A)
B)
C)
D)
E)

Question 77

The total numbers of neutrons, protons, and electrons in 138Ba2+ are ________.

A) 138 neutrons, 56 protons, 54 electrons
B) 82 neutrons, 56 protons, 54 electrons
C) 56 neutrons, 82 protons, 80 electrons
D) 82 neutrons, 56 protons, 58 electrons
E) 82 neutrons, 82 protons, 82 electrons

Question 78

A cation has 28 neutrons and 21 electrons. If it has a +3 charge, what is its correct symbol?

A)
B)
C)
D)
E)

Question 79

What is the proper notation for an ion having 35 protons, 36 electrons and 45 neutrons?

A)
B)
C)
D)

Question 80

The following ratios of masses were obtained with a mass spectrometer: / = 1.8406, / = 1.5832 What is the mass of a atom in atomic mass units?

A) 35.45 u
B) 36.36 u
C) 13.95 u
D) 35.00 u
E) 34.97 u