Deck 2: Atoms, Ions, and Molecules: Matter Starts Here

Question 1

Which statement is not correct?

A) Electrons have a negative electrical charge.
B) Protons have a positive electrical charge.
C) Neutrons do not have an electrical charge.
D) In an atom, the interaction between electrons and protons is attractive.
E) In an atom, the interaction between electrons and neutrons is repulsive.

Answer 1

In an atom, the interaction between electrons and neutrons is repulsive.

Question 2

Which statement best describes isotopes?

A) They have the same atomic mass.
B) They have the same total number of protons and neutrons.
C) They have the same number of neutrons but a different number of protons.
D) They have the same number of protons but a different number of neutrons.
E) They have very different chemical reactivity.

Answer 2

They have the same total number of protons and neutrons.

Question 3

Which statement about isotopes of the same element is not correct?

A) They have the same number of protons.
B) They have different numbers of neutrons.
C) They have essentially the same chemical properties.
D) They have the same atomic mass.
E) They have the same number of electrons.

Answer 3

They have the same atomic mass.

Question 4

Which particle-level diagram is the best representation of a ${ } _ { 7 } ^ { 14 } \mathrm {~N} ^ { 3 - }$ ion?

A)
B)
C)
D)

Question 5

If an atom had a radius of 100 m, it would be approximately the size of a football stadium. On this scale, what would be the radius of the atomic nucleus? The radius of the nucleus is approximately 10,000 times smaller than the radius of an atom.

A) 1 mm, like a very dull pencil point
B) 1 cm, like a dime
C) 10 cm, like your longest finger
D) 10 $\mu$ m, like a red blood cell
E) 100 pm, like a real atom

Question 6

Which statement is not correct? In atomic mass units (amu or u), __________

A) the mass of an electron, proton, or neutron is approximately 1 u.
B) the mass of a proton or neutron is approximately 1 u, and the mass of an electron is approximately 0 u.
C) the mass of an atom is approximately equal to the number of protons and neutrons in the nucleus of the atom.
D) the mass of a carbon-12 atom is exactly 12 u.
E) the mass of an oxygen-16 atom is approximately 16 u.

Question 7

Which particle-level diagram is the best representation for a atom?

A)
B)
C)
D)

Question 8

Which statement is correct?

A) Electrons, protons, and neutrons have about the same mass.
B) Electrons have a much smaller mass than that of protons and neutrons.
C) Neutrons are much more massive than protons.
D) Protons are much more massive than neutrons.
E) Electrons have a much larger mass than that of protons and neutrons.

Question 9

Who discovered electrons?

A) Robert Boyle
B) Robert Millikan
C) Joseph John Thomson
D) John Dalton
E) Albert Einstein

Question 10

What is the correct symbol for a proton?

A) ${ } _ { - 1 } ^ { 0 } \mathrm { p }$
B) ${ } _ { 1 } ^ { 0 } \mathrm { p }$
C) ${ } _ { 1 } ^ { 1 } p$
D) ${ } _ { 0 } ^ { 1 } P$
E) ${ } _ { 0 } ^ { 0 } \mathrm { p }$

Question 11

What is the correct symbol for a neutron?

A) ${ } _ { 0 } ^ { 1 } \mathrm { n }$
B) ${ } _ { 1 } ^ { 1 } \mathrm { n }$
C) ${ } _ { 1 } ^ { 0 } \mathrm { n }$
D) ${ } _ {-1 } ^ { 1 } \mathrm { n }$
E) ${ } _ { 0 } ^ { 0 } \mathrm { n }$

Question 12

What is the correct symbol for an electron?

A) ${ } _ { - 1 } ^ { 0 } \mathrm { e }$
B) ${ } _ {1 } ^ { 1 } \mathrm { e }$
C) ${ } _ { 1 } ^ { 0 } \mathrm { e }$
D) ${ } _ { - 1 } ^ { 1 } \mathrm { e }$
E) ${ } _ { 0 } ^ { 0 } \mathrm { e }$

Question 13

Rutherford, Geiger, and Marsden's experiment demonstrated that the volume of the nucleus is roughly what fraction of the volume occupied by the electrons?

A) 1/10
B) 1/100
C) 1/1,000
D) 1/10,000
E) 1/100,000

Question 14

Protons and neutrons are examples of __________

A) nuclei.
B) nuclides.
C) nucleons.
D) isotopes.
E) charged particles.

Question 15

Who was the first scientist to determine the charge of an electron?

A) Robert Boyle
B) Robert Millikan
C) Joseph John Thomson
D) John Dalton
E) Albert Einstein

Question 16

When cosmic rays strike atoms in the upper atmosphere, energetic neutrons are produced. These neutrons collide with nitrogen-14 atoms, producing carbon-14 atoms and hydrogen atoms. Which diagram represents the carbon-14 product?

A)
B)
C)
D)

Question 17

The ⁴He nucleus is an example of __________

A) a nuclide.
B) an element.
C) a proton.
D) a neutron.
E) a nucleon.

Question 18

Which one of the following experiments provided evidence that atoms contained small massive nuclei with positive charges?

A) Bunsen and Kirchoff's flame test
B) Fraunhofer lines
C) the Rutherford-Geiger-Marsden experiment
D) Thomson's experiments with cathode ray tubes
E) Millikan's oil-drop experiment

Question 19

In the atoms in the Rutherford-Geiger-Marsden experiment, the alpha particles were repelled by __________

A) electrons.
B) protons.
C) neutrons.
D) nuclei.
E) gravity.

Question 20

In the Rutherford-Geiger-Marsden experiment, alpha particles were projected at a thin film of __________

A) gold.
B) silver.
C) platinum.
D) sodium.
E) aluminum.

Question 21

Enriched weapons-grade uranium consists of 80% uranium-235 (235.044 amu) and 20% uranium-238 (238.051 amu). What is the average atomic mass of weapons-grade uranium, assuming the percentages are exact?

A) 235.044 amu
B) 236.547 amu
C) 238.051 amu
D) 235.645 amu
E) 235.754 amu

Question 22

A ${ } _ { 17 } ^ { 15 } \mathrm { Cl }$ atom has __________ protons, __________ neutrons, and __________ electrons.

A) 17, 18, 19
B) 17, 20, 17
C) 17, 17, 20
D) 17, 18, 17
E) 18, 17, 18

Question 23

What is the symbol for magnesium?

A) M
B) Mg
C) Mn
D) Mo
E) Ma

Question 24

An unknown element is found to contain isotopes with the following masses and natural abundances: 38.9637 amu (93.08%), 39.9640 amu (0.012%), and 40.9618 amu (6.91%). Using these data, identify the element.

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

Question 25

The Curiosity rover now on Mars analyzed rocks and found magnesium to have the following isotopic composition. What is the average atomic mass of magnesium in these rocks? $$\begin{array} { | c | c | } \hline \text { Mass (u) } & \text { \% Abundance } \\\hline 23.9872 & 79.70 \\\hline 24.9886 & 10.13 \\\hline 25.9846 & 10.17 \\\hline\end{array}$$

A) 24.31 u
B) 24.29 u
C) 24.33 u
D) 24.99 u
E) 33.33 u

Question 26

Technetium often is used to image areas of bone growth because it is a radioisotope with a half-life of 6 hours that emits gamma rays. A ${ } _ { 43 } ^ { 9 } T c ^ { + }$ ion has __________ protons, __________ neutrons, and __________electrons.

A) 99, 43, 98
B) 43, 99, 42
C) 43, 56, 42
D) 56, 43, 43
E) 43, 99, 43

Question 27

Tellurium and iodine appear next to each other in the periodic table with tellurium in group 16 and iodine in group 17. Mendeleev's early periodic table had this order reversed because __________

A) the mass number is larger for iodine.
B) tellurium has one more proton than iodine.
C) iodine has one more proton than tellurium.
D) Te comes after I in the alphabet.
E) in total tellurium has more protons and neutrons than iodine.

Question 28

Which statement regarding the organization of the periodic table is not correct?

A) Mendeleev arranged known elements with similar chemical properties in columns.
B) Mendeleev's predictions of the chemical properties of unknown elements facilitated their discovery.
C) Mendeleev arranged the elements in order of increasing atomic mass.
D) The modern periodic table arranges elements in order of increasing atomic number.
E) The elements go from gases to liquids to solids in order down the columns in Mendeleev's periodic table.

Question 29

What is the symbol for sulfur?

A) Si
B) Sc
C) Su
D) S
E) Sf

Question 30

A ${ } _ { 8 } ^ { 16 } \mathrm { O } ^ { 2 - }$ ion has __________ protons, __________ neutrons, and __________ electrons.

A) 8, 8, 6
B) 8, 10, 10
C) 8, 8, 10
D) 8, 8, 8
E) 8, 16, 8

Question 31

A hypothetical element has two stable isotopes: one isotope has a mass of 106.9051 amu with an abundance of 48.183%, the other isotope has a mass of 108.9048 amu with an abundance of 51.825%. What is the average atomic mass of this element?

A) 107.980 amu
B) 107.970 amu
C) 107.960 amu
D) 107.950 amu
E) 107.940 amu

Question 32

Zinc has five naturally occurring isotopes with an average mass of 65.39 amu. Three isotopes, in roughly equal amounts, account for 95% of zinc. Which isotope is most abundant?

A) (⁶⁴Zn, 63.9291 amu)
B) (⁶⁶Zn, 65.9260 amu)
C) (⁶⁷Zn, 66.9271 amu)
D)(⁶⁸Zn, 67.9249 amu)
E) (⁷⁰Zn, 69.9253 amu)

Question 33

The average atomic mass of lithium is 6.941 amu. Lithium has two naturally occurring isotopes, ⁶Li (7.52%) and ⁷Li (92.48%). The mass of ⁶Li is 6.0151 amu. What is the mass of ⁷Li?

A) 7.016 amu
B) 0.926 amu
C) 6.001 amu
D) 7.000 amu
E) 6.941 amu

Question 34

What is the symbol of the ion having 12 protons and 10 electrons?

A) Mg²⁺
B) Al³⁺
C) Mg^2-
D) Na²⁺
E) Mg

Question 35

For each of the elements below, there are only two naturally occurring isotopes. Using information in your periodic table, identify the pair in which the heavier isotope is the more abundant one.

A) (⁶³Cu and ⁶⁵Cu)
B) (⁸⁵Rb and ⁸⁷Rb)
C) (¹⁰B and ¹¹B)
D) (⁷⁹Br and ⁸¹Br)
E) (¹⁴N and ¹⁵N)

Question 36

Tellurium and iodine appear next to each other in the periodic table. Tellurium is in group 16 and iodine is in group 17 because __________.

A) the mass number is larger for iodine.
B) tellurium has one more proton than iodine.
C) iodine has one more proton than tellurium.
D) the mass number is larger for tellurium.
E) Mendeleev identified that this order is the correct one.

Question 37

The mass of thallium (Tl) on the periodic table is given as 204.3833 without any units. There are 47 isotopes of thallium, but only two are stable and abundant, thallium-203, with a mass of 202.9723 amu, and thallium-205, with a mass of 204.9744 amu. What is the percentage of each of these isotopes in naturally occurring thallium?

A) 29.5% ²⁰³Tl and 70.5% ²⁰⁵Tl
B) 70.5% ²⁰³Tl and 29.5% ²⁰⁵Tl
C) 25.5% ²⁰³Tl and 74.5% ²⁰⁵Tl
D) 74.5% ²⁰³Tl and 25.5% ²⁰⁵Tl
E) 32.5% ²⁰³Tl and 67.5% ²⁰⁵Tl

Question 38

The average atomic mass of zinc is 65.39 amu. Given the data in the following table, what is the natural abundance of ⁶⁶Zn? $$\begin{array} { c c c } \text { Isotope } & \text { Mass (amu) } & \text { Natural Abundance (\%) } \\{ } ^ { 64 } \mathrm { Zn } & 63.9291 & 48.89 \\{ } ^ { 66 } \mathrm { Zn } & 65.9260 & ? \\{ } ^ { 67 } \mathrm { Zn } & 66.9271 & 4.11 \\{ } ^ { 68 } \mathrm { Zn } & 67.9249 & 18.56 \\{ } ^ { 70 } \mathrm { Zn } & 69.9253 & 0.62\end{array}$$

A) 27.83%
B) 0.2783%
C) 50.00%
D) 2.783%
E) 28.73%

Question 39

The average atomic mass of calcium is 40.078 amu. Which is likely to be the most abundant isotope of calcium?

A) (⁴⁰Ca)
B) (⁴²Ca)
C) (⁴³Ca)
D) (⁴⁴Ca)
E) (⁴⁸Ca)

Question 40

For each of the elements below, there are only two naturally occurring isotopes. Using information in your periodic table, identify the pair in which the lighter isotope is the more abundant one.

A) (⁶Li and ⁷Li)
B) (⁷⁹Br and ⁸¹Br)
C) (¹⁰B and ¹¹B)
D) (¹⁹¹Ir and ¹⁹³Ir)
E) (⁵⁰V and ⁵¹V)

Question 41

He is the symbol for __________

A) hydrogen.
B) hafnium.
C) mercury.
D) helium.
E) holmium.

Question 42

Silicon is best described as a __________

A) metalloid.
B) metal.
C) transition metal.
D) noble gas.
E) nonmetal.

Question 43

Which of the following is an alkali metal?

A) K
B) Mg
C) Al
D) Cu
E) Ca

Question 44

Identify the statement regarding O₂, NO, and H₂O that is correct.

A) Only O₂ is a chemical element.
B) Only NO is a chemical element.
C) Only H₂O is a chemical compound.
D) All are chemical elements.
E) All are chemical compounds.

Question 45

Potassium is best described as a __________

A) metalloid.
B) metal.
C) transition metal.
D) noble gas.
E) nonmetal.

Question 46

Oxygen is best described as a __________

A) metalloid.
B) metal.
C) transition metal.
D) noble gas.
E) nonmetal.

Question 47

Which statement below is not correct?

A) Oxygen is a chalcogen.
B) Calcium is an alkaline earth metal.
C) Silicon is a nonmetal.
D) Sodium is an alkali metal.
E) Bromine is a halogen.

Question 48

Iron can form two sulfides: FeS and Fe₂S₃. Use Dalton's law of multiple proportions to predict the ratio of the two masses of sulfur that combine with 100 g of iron in each case to form these compounds.

A) 1:1
B) 1:3
C) 1:2
D) 2:3
E) 3:4

Question 49

Cobalt is best described as a(n) __________

A) metalloid.
B) transition metal.
C) chalcogen.
D) alkaline earth metal.
E) nonmetal.

Question 50

Elements in group 18 (VIIIA) are called __________

A) alkali metals.
B) noble gases.
C) alkaline earth metals.
D) halogens.
E) chalcogens.

Question 51

Nitrogen and oxygen combine to form several different nitrogen oxides. In one case, 8.4 g of nitrogen reacted completely with 4.8 g of oxygen. In another case, 4.2 g of nitrogen reacted with 9.6 g of oxygen. Which pair of nitrogen oxides is consistent with these data?

A) NO and N₂O
B) NO and NO₂
C) N₂O and N₂O₅
D) NO and N₂O₄
E) N₂O and N₂O₄

Question 52

When 10.0 g of sulfur is combined with 10.0 g of oxygen, 20.0 g of sulfur dioxide is formed. What mass of oxygen would be required to convert 10.0 g of sulfur into sulfur trioxide?

A) 5.0 g
B) 10 g
C) 15 g
D) 30 g
E) 20 g

Question 53

Dalton's law of multiple proportions can be applied to __________

A) H₂O and CO₂.
B) CO and NO.
C) PF₃ and PF₅.
D) SO₂ and CO.
E) O₂ and O₃.

Question 54

Which one of the following statements is not consistent with Dalton's atomic view of matter?

A) Atoms of one element can be converted into atoms of another element.
B) Each element is composed of atoms that are identical in size, mass, and chemical properties.
C) Compounds are formed from different atoms in simple whole number ratios.
D) Atoms of different elements can combine in several different proportions to make different compounds.
E) Matter is discrete, as proposed by Democritus.

Question 55

The elements below are used in fireworks. Which one is not classified correctly according to its position in the periodic table?

A) Sodium is an alkali metal.
B) Strontium is an alkaline earth metal.
C) Iron is a transition metal.
D) Phosphorus is a nonmetal.
E) Sulfur is a metalloid.

Question 56

Calcium is an example of __________

A) an alkali metal.
B) a transition metal.
C) an alkaline earth metal.
D) a halogen.
E) a chalcogen.

Question 57

Dalton's law of multiple proportions deals with __________

A) the proportions of reacting chemicals that maximize the reaction rate.
B) the total number of different compounds that can be made from two elements.
C) the volumes of two elements that can combine to form two or more compounds.
D) the relative masses of two elements that can combine to form two or more compounds.
E) reactions that involve multiple steps.

Question 58

Elements in group 17 (VIIA) are called __________

A) alkali metals.
B) pnictogens.
C) alkaline earth metal.
D) halogens.
E) chalcogens.

Question 59

The sixth period of the periodic table contains __________ elements.

A) 18
B) 32
C) 24
D) 16
E) 8

Question 60

Elements 21-30 are known as __________

A) alkaline earths.
B) chalcogens.
C) halides.
D) transition metals.
E) rare earths.

Question 61

Which one of the following is a cation?

A) NO₃^-
B) SO₂
C) Ca²⁺
D) Na
E) O₂

Question 62

Identify the binary compound that has ionic bonding.

A) H₂O
B) NO
C) LiF
D) CH₄
E) CF₄

Question 63

What is the correct formula for the compound formed between sodium and iodine based on their positions in the periodic table?

A) Na₂I
B) NaI₂
C) NaI
D) Na₂I₂
E) Na₃I

Question 64

Which element labeled A-E in the periodic table below will have an ionic charge of -1?

A) A
B) B
C) C
D) D
E) E

Question 65

What is the empirical formula for benzene, C₆H₆?

A) CH
B) C₆H₆
C) C₂H₂
D) CH₃
E) C₆H

Question 66

How many atoms of each element are there in the compound (NH₄)₂(S₂O₃)·5H₂O?

A) nitrogen 2, hydrogen 18, sulfur 2, oxygen 8
B) nitrogen 1, hydrogen 6, sulfur 2, oxygen 4
C) nitrogen 2, hydrogen 10, sulfur 2, oxygen 4
D) nitrogen 1, hydrogen 6, sulfur 2, oxygen 8
E) nitrogen 2, hydrogen 8, sulfur 2, oxygen 3

Question 67

Which element labeled A-E in the periodic table below will have an ionic charge of +1?

A) A
B) B
C) C
D) D
E) E

Question 68

Which of the following is most likely to exhibit covalent bonding?

A) NaF
B) CaCl₂
C) Cs₂O
D) CO₂
E) NaCl

Question 69

Which element labeled A-E in the periodic table below will have an ionic charge of -2?

A) A
B) B
C) C
D) D
E) E

Question 70

How many atoms of each element are there in the compound Na₃(PO₄)₃?

A) sodium 3, phosphorus 3, oxygen 12
B) sodium 9, phosphorus 3, oxygen 12
C) sodium 3, phosphorus 1, oxygen 4
D) sodium 3, potassium 1, oxygen 4
E) sodium 9, potassium 3, oxygen 12

Question 71

Locate each element in the periodic table and identify which statement is not correct. The common ion of __________ has __________ electrons and a charge of __________.

A) Cs, 55, +1
B) Ca, 18, +2
C) Ba, 54, +2
D) S, 18, -2
E) Cl, 18, -1

Question 72

Locate each element in the periodic table and identify which statement is not correct. The common ion of __________ has __________ electrons and a charge of __________.

A) Na, 10, +1
B) K, 18, +1
C) Mg, 10, +2
D) O, 10, -2
E) F, 10, -2

Question 73

Which element labeled A-E in the periodic table below will have an ionic charge of +3?

A) A
B) B
C) C
D) D
E) E

Question 74

Based on the element's position in the periodic table, which statement below is not correct?

A) The charge on an ion of sodium is 1+.
B) The charge on an ion of magnesium is 2+.
C) The charge on an ion of oxygen is 2-.
D) The charge on an ion of chlorine is 1-.
E) Ca²⁺ has more electrons than Ar.

Question 75

Based on its position in the periodic table, which atom would you predict to form an ionic compound with two bromine atoms?

A) sodium
B) aluminum
C) lithium
D) calcium
E) carbon

Question 76

Based on its position in the periodic table, which atom would you predict to form a compound with one chlorine atom?

A) boron
B) aluminum
C) lithium
D) calcium
E) carbon

Question 77

Which one of the following is a molecular compound? Molecular compounds also are known as covalent compounds.

A) Na₂O
B) CaO
C) FeO
D) CCl₄
E) Fe₂O₃

Question 78

Which one of the following is an ionic compound?

A) SO₂
B) ClO₂
C) H₂O
D) TiO₂
E) CO₂

Question 79

Which element labeled A-E in the periodic table below will have an ionic charge of +2?

A) A
B) B
C) C
D) D
E) E

Question 80

Which one of the following is an anion?

A) Na⁺
B) CO₂
C) Cl^-
D) Na
E) O₃