Deck 2: Atoms and Elements

Question 1

The mass number is equal to

A)the sum of the number of the electrons and protons.
B)the sum of the number of the neutrons and electrons.
C)the sum of the number of protons, neutrons, and electrons.
D)the sum of the number of protons and neutrons.

Answer 1

the sum of the number of protons and neutrons.

Question 2

If 26.0 g of water, H₂O, is found to contain 2.9 g of hydrogen and 23.1 g of oxygen, how much hydrogen and oxygen, in grams, is contained in 32.0 g of water?

A)3.6 g hydrogen and 28.4 g oxygen
B)28.4 g hydrogen and 3.6 g oxygen
C)26.0 g hydrogen and 28.4 g oxygen
D)3.6 g hydrogen and 2.9 g oxygen
E)2.9 g hydrogen and 28.4 g oxygen

Answer 2

3.6 g hydrogen and 28.4 g oxygen

Question 3

What does "X" represent in the following symbol? X

A)mercury
B)chlorine
C)scandium
D)bromine
E)selenium

Answer 3

bromine

Question 4

Identify the charges of protons, neutrons, and electrons.

A)protons +1, neutrons 0, electrons -1
B)protons 0, neutrons -1, electrons +1
C)protons -1, neutrons 0, electrons +1
D)protons 0, neutrons +1, electrons -1
E)protons +1, neutrons -1, electrons 0

Question 5

In a chemical reaction, matter is neither created nor destroyed. Which law does this refer to?

A)Law of definite proportions
B)Law of the conservation of mass
C)Law of modern atomic theory
D)Law of multiple proportions
E)First law of thermodynamics

Question 6

All samples of a given compound, regardless of their source or how they were prepared, have the same proportions of their constituent elements. Which law does this refer to?

A)Law of definite proportions
B)Law of the conservation of mass
C)Law of modern atomic theory
D)Law of multiple proportions
E)First law of thermodynamics

Question 7

Which of the following is an example of the law of multiple proportions?

A)A sample of chlorine is found to contain three times as much Cl-35 as Cl-37.
B)Two different compounds formed from carbon and oxygen have the following mass ratios: 1.33 g O:1 g C and 2.66 g O:1 g C
C)Two different samples of table salt are found to have the same ratio of sodium to chlorine.
D)The atomic mass of bromine is found to be 79.90 amu.
E)Nitrogen dioxide always has a mass ratio of 2.28 g O:1 g N.

Question 8

Determine the number of protons, neutrons, and electrons in the following: X

A)p⁺ = 18 n° = 18 e^- = 22
B)p⁺ = 18 n° = 22 e^- = 18
C)p⁺ = 22 n° = 18 e^- = 18
D)p⁺ = 18 n° = 22 e^- = 40
E)p⁺ = 40 n° = 22 e^- = 18

Question 9

Determine the number of protons, neutrons, and electrons in the following: X

A)p⁺ = 12 n° = 25 e^- = 12
B)p⁺ = 12 n° = 12 e^- = 13
C)p⁺ = 12 n° = 13 e^- = 12
D)p⁺ = 25 n° = 12 e^- = 13
E)p⁺ = 12 n° = 13 e^- = 25

Question 10

If 6.0 g of carbon combines with 16.0 g of oxygen to form 22.0 g of carbon dioxide, how much carbon and oxygen, in grams, is in 28.7 g carbon dioxide?

A)20.9 g carbon and 7.8 g oxygen
B)20.9 g carbon and 10.5 g oxygen
C)7.8 g carbon and 20.9 g oxygen
D)7.8 g carbon and 10.5 g oxygen
E)3.9 g carbon and 20.9 g oxygen

Question 11

What does "X" represent in the following symbol? X

A)silicon
B)sulfur
C)zinc
D)ruthenium
E)nickel

Question 12

When two elements, A and B, form two different compounds, the masses of element B that combine with 1 g of element A can be expressed as a ratio of small whole numbers. Which law does this refer to?

A)Law of definite proportions
B)Law of the conservation of mass
C)Law of modern atomic theory
D)Law of multiple proportions
E)First law of thermodynamics

Question 13

Dalton's atomic theory states

A)that all elements have several isotopes.
B)that matter is composed of small indestructible particles.
C)that the properties of matter are determined by the properties of atoms.
D)that energy is neither created nor destroyed during a chemical reaction.
E)that an atom is predominantly empty space.

Question 14

Identify the element that has an atomic number of 40.

A)neon
B)calcium
C)zirconium
D)bromine

Question 15

Isotopes differ in the number of what particle?

A)beta particles
B)protons
C)electrons
D)neutrons
E)gamma particles

Question 16

Which of the following statements is TRUE according to Dalton's atomic theory?

A)Atoms combine in simple fraction ratios to form compounds.
B)All atoms of chlorine have identical properties to other elements with similar mass.
C)Atoms of carbon can be changed into atoms of oxygen when creating carbon dioxide.
D)Atoms of carbon do not change into another element during a chemical reaction with chlorine.
E)An atom of nitrogen can be broken down into smaller particles that will still have the unique properties of nitrogen.

Question 17

If 3.6 g of chlorine combines with sodium to make 6.0 g of sodium chloride, what mass of sodium is required?

A)3.6 g
B)2.4 g
C)6.0 g
D)9.6 g
E)1.2 g

Question 18

What mass of calcium is required to produce 4.2 g of calcium bromide, starting with 3.4 g of bromine?

A)0.4 g
B)3.4 g
C)4.2 g
D)1.6 g
E)0.8 g

Question 19

What does "X" represent in the following symbol? X

A)tin
B)copper
C)palladium
D)niobium
E)uranium

Question 20

Identify the description of an atom.

A)neutrons and electrons in nucleus; protons in orbitals
B)neutrons in nucleus; protons and electrons in orbitals
C)protons and neutrons in nucleus; electrons in orbitals
D)protons and electrons in nucleus; neutrons in orbitals
E)electrons in nucleus; protons and neutrons in orbitals

Question 21

Predict the charge that an ion formed from bromine would have.

A)1-
B)2+
C)1+
D)4+
E)2-

Question 22

Predict the charge that an ion formed from sulfur would have.

A)1-
B)6+
C)3-
D)4+
E)2-

Question 23

How many electrons are in arsenic?

A)33
B)41
C)42
D)41.9
E)75

Question 24

What element is defined by the following information? p⁺ = 20 n° = 20 e^- = 20

A)zirconium
B)calcium
C)potassium
D)neon
E)argon

Question 25

What element is defined by the following information? p⁺ = 17 n° = 20 e^- = 17

A)calcium
B)rubidium
C)chlorine
D)neon
E)oxygen

Question 26

What species is represented by the following information? p⁺ = 12 n° = 14 e^- = 10

A)Si⁴⁺
B)Mg
C)Ne
D)Si
E)Mg²⁺

Question 27

What species is represented by the following information? p⁺ = 47 n° = 62 e^- = 46

A)Ag⁺
B)Nd
C)Pd
D)Ag
E)Pd⁺

Question 28

Identify a cation.

A)An atom that has lost (an)electron(s).
B)An atom that has gained (an)electron(s).
C)An atom that has lost (a)proton(s).
D)An atom that has gained (a)proton(s).

Question 29

Isotopes differ in the number of

A)protons.
B)neutrons.
C)electrons.
D)none of the above
E)all of the above

Question 30

What species is represented by the following information? p⁺ = 17 n° = 18 e^- = 18

A)Cl
B)Cl^-
C)Ar
D)Ar⁺
E)Kr

Question 31

How many neutrons are in arsenic-42?

A)33
B)41
C)42
D)41.9
E)75

Question 32

What element is defined by the following information? p⁺ = 11 n° = 12 e^- = 11

A)sodium
B)vanadium
C)magnesium
D)titanium

Question 33

Which of the following statements about isotopes is TRUE?

A)Isotopes of the same element differ only in the number of electrons they contain.
B)An isotope of an atom with a larger number of neutrons is larger than an isotope of the same atom that contains fewer neutrons.
C)Isotopes of the same element have the same mass.
D)Isotopes of the same element don't usually have the same properties.
E)Some elements have three or more naturally occurring isotopes.

Question 34

Predict the charge that an aluminum ion would have.

A)5-
B)1+
C)1-
D)2+
E)3+

Question 35

Identify the symbol for fluorine.

A)F
B)Fl
C)Fo
D)Fu
E)Fr

Question 36

Which of the following statements about subatomic particles is TRUE?

A)A neutral atom contains the same number of protons and electrons.
B)Protons have about the same mass as electrons.
C)Electrons make up most of the mass of an atom.
D)Protons and neutrons have opposite, but equal in magnitude, charges.
E)Neutrons and electrons are found in the nucleus of an atom.

Question 37

How many protons are in arsenic?

A)33
B)41
C)42
D)41.9
E)75

Question 38

Determine the number of protons, neutrons, and electrons in the following: X

A)p⁺ = 36 n° = 29 e^- = 36
B)p⁺ = 29 n° = 29 e^- = 36
C)p⁺ = 36 n° = 36 e^- = 29
D)p⁺ = 29 n° = 36 e^- = 29
E)p⁺ = 29 n° = 36 e^- = 36

Question 39

Identify the symbol for silver.

A)S
B)Si
C)Ar
D)Ag
E)Sl

Question 40

Predict the charge that a calcium ion would have.

A)6-
B)2-
C)3+
D)2+
E)1+

Question 41

The atomic mass of tungsten is 183.84 amu. Given the following information for the mass and abundance of the other common isotopes, calculate the atomic mass of tungsten-186. W-180 179.9467 amu 0.12%
W-182 181.9482 amu 26.50%
W-183 182.9502 amu 14.31%
W-184 183.9509 amu 30.64%
W-186 28.43%

A)185.75 amu
B)186.48 amu
C)186.98 amu
D)184.41 amu
E)185.95 amu

Question 42

Carbon has two naturally occurring isotopes, carbon-12 and carbon-13. The more common isotope of carbon is carbon-12 with an abundance of 98.93% while carbon-13 has an atomic mass of 13.00335 amu. Calculate the atomic mass of carbon-12 if the atomic mass of carbon is 12.0107 amu.

A)13.1 amu
B)13.0 amu
C)12.0 amu
D)12.8 amu
E)12.4 amu

Question 43

Bromine has two naturally occurring isotopes, Br-79 and Br-81. The mass of Br-79 is 78.92 amu with a percent abundance of 50.69%. If the atomic mass of bromine is 79.904 amu, calculate the mass and percent abundance of Br-81.

A)80.916 amu and 50.69%
B)78.921 amu and 49.31%
C)79.904 amu and 49.31%
D)80.913 amu and 49.31%
E)80.028 amu and 50.31%

Question 44

Calculate the atomic mass of gallium if gallium has four naturally occurring isotopes with the following masses and natural abundances: Ga-69 68.9256 amu 60.11%
Ga-71 70.9247 amu 39.89%

A)69.72 amu
B)69.93 amu
C)70.00 amu
D)69.80 amu
E)70.68 amu

Question 45

Calculate the atomic mass of element "X" if it has two naturally occurring isotopes with the following masses and natural abundances: X-45 44.8776 amu 32.88%
X-47 46.9443 amu 67.12%

A)46.26 amu
B)45.91 amu
C)46.34 amu
D)46.84 amu
E)44.99 amu

Question 46

Calculate the atomic mass of silver if silver has two naturally occurring isotopes with the following masses and natural abundances: Ag-107 106.90509 amu 51.84%
Ag-109 108.90476 amu 48.46%

A)107.90 amu
B)108.00 amu
C)107.79 amu
D)108.32 amu
E)108.19 amu

Question 47

What is the atomic mass for cadmium?

A)48
B)112.41
C)40.08
D)20

Question 48

Calculate the atomic mass of chromium if chromium has four naturally occurring isotopes with the following masses and natural abundances: Cr-50 49.9461 amu 4.35%
Cr-52 51.9405 amu 83.79%
Cr-53 52.9407 amu 9.50%
Cr-54 53.9389 amu 2.36%

A)51.941 amu
B)51.699 amu
C)208.766 amu
D)53.214 amu
E)51.996 amu

Question 49

What is the atomic number for tin?

A)47.87
B)50
C)118.71
D)22

Question 50

Identify the largest atom or ion of carbon.

A)p⁺ = 6 n° = 6 e^- = 6
B)p⁺ = 6 n° = 7 e^- = 6
C)p⁺ = 6 n° = 6 e^- = 7
D)p⁺ = 6 n° = 6 e^- = 5

Question 51

Identify the number of neutrons in P^-3. Phosphorus has one stable isotope, phosphorus-31.

A)18
B)12
C)19
D)15
E)16

Question 52

What is the atomic mass for tin?

A)47.87
B)50
C)118.71
D)22

Question 53

Bromine has two naturally occurring isotopes, Br-79 and Br-81. The atomic mass of Br-79 is 78.9183 amu with a percent abundance of 50.69% and the atomic mass of Br-81 is 80.9163 amu. Calculate the atomic mass of bromine.

A)80.91 amu
B)78.92 amu
C)79.90 amu
D)80.92 amu
E)80.03 amu

Question 54

Gallium has an atomic mass of 69.723 amu. The abundance of Ga-69 (68.926 amu)is 60.11%. What is the atomic mass, in amu, of the other isotope?

A)70.924 amu
B)70.928 amu
C)70.932 amu
D)70.920 amu
E)70.930 amu

Question 55

Silver has an atomic mass of 107.868 amu. The Ag-109 isotope (108.905 amu)has an abundance of 48.161%. What is the atomic mass, in amu, of the other isotope?

A)106.905 amu
B)106.908 amu
C)106.903 amu
D)106.911 amu

Question 56

Identify the number of electrons in P^-3.

A)18
B)12
C)19
D)15
E)16

Question 57

Calculate the atomic mass of tungsten given the atomic mass and percent abundance for the following isotopes: W-180 179.9467 amu 0.12%
W-182 181.9482 amu 26.50%
W-183 182.9502 amu 14.31%
W-184 183.9509 amu 30.64%
W-186 185.9544 amu 28.43%

A)183.75 amu
B)183.84 amu
C)182.98 amu
D)184.41 amu
E)183.92 amu

Question 58

Identify the number of protons in P^-3.

A)18
B)12
C)19
D)15
E)16

Question 59

Zinc has five naturally occurring isotopes, Zn-64, Zn-66, Zn-67, Zn-68 and Zn-70. Calculate the atomic mass of zinc given the following abundances and atomic masses for the isotopes: Zn-64 63.9291 amu 48.61%
Zn-66 65.9260 amu 27.9%
Zn-67 66.9271 amu 4.1%
Zn-68 67.9248 amu 18.75%
Zn-70 69.9253 amu 0.62%

A)65.34 amu
B)65.38 amu
C)65.65 amu
D)65.19 amu
E)65.85 amu

Question 60

Cerium has four stable isotopes listed below. If the weighted average atomic mass of cerium is 140.116 amu, calculate the atomic mass of cerium-142. Ce-136 135.90714 amu 0.19%
Ce-138 137.90599 amu 0.25%
Ce-140 139.90543 amu 88.43%
Ce-142 11.13%

A)141.911 amu
B)142.341 amu
C)142.000 amu
D)141.556 amu
E)142.911 amu

Question 61

How many argon atoms are contained in 7.66 × 10⁵ mmol of argon?

A)4.61 × 10²⁶ Ar atoms
B)1.84 × 10²⁸ Ar atoms
C)1.15 × 10²⁸ Ar atoms
D)7.86 × 10²⁰ Ar atoms
E)3.24 × 10²⁶ Ar atoms

Question 62

How many moles are in 2.16 × 10²⁴ atoms of lead?

A)35.9 moles
B)3.59 moles
C)0.359 moles
D)6.08 moles
E)1.79 moles

Question 63

Which of the following contains the FEWEST atoms? You shouldn't need to do a calculation here.

A)4.0 g Li
B)4.0 g Na
C)4.0 g Rb
D)4.0 g K
E)4.0 g Ca

Question 64

How many xenon atoms are contained in 2.36 moles of xenon?

A)3.92 × 10²⁴ xenon atoms
B)2.55 × 10²³ xenon atoms
C)1.42 × 10²⁴ xenon atoms
D)7.91 × 10²⁵ xenon atoms
E)1.87 × 10²⁶ xenon atoms

Question 65

How many moles are in one dozen?

A)12 mol
B)6.0 × 10²³mol
C)2.0 × 10^-23 mol
D)5.0 × 10²² mol
E)2.0 × 10²³ mol

Question 66

What mass (in g)does 3.99 moles of Kr have?

A)334 g
B)476 g
C)211 g
D)240 g
E)144 g

Question 67

How many dozen are in one mole?

A)12 dozen
B)6.0 × 10²³ dozen
C)2.0 × 10^-23 dozen
D)5.0 × 10²² dozen
E)2.0 × 10²³ dozen

Question 68

What is the average mass, in grams, of one atom of carbon?

A)5.01 × 10^-22 g
B)5.01 × 10²² g
C)1.38 × 10^-25 g
D)1.99 × 10^-23 g
E)1.99 × 10²³ g

Question 69

How many silver atoms are contained in 3.75 moles of silver?

A)6.23 × 10²⁴ silver atoms
B)2.26 × 10²⁴ silver atoms
C)1.61 × 10²³ silver atoms
D)2.44 × 10²⁶ silver atoms
E)6.50 × 10²⁵ silver atoms

Question 70

If 102.7 g of tin is mixed with 10.9 g of copper to create the alloy pewter, how many metal atoms total are present in the pewter?

A)5.81 × 10²³ metal atoms
B)5.22 × 10²³ metal atoms
C)3.75 × 10²³ metal atoms
D)9.66 × 10²³ metal atoms
E)6.24 × 10²³ metal atoms

Question 71

How many moles of potassium are contained in 449 g of potassium?

A)11.5 moles
B)17.6 moles
C)69.2 moles
D)23.9 moles
E)41.5 moles

Question 72

If 102.7 g of tin is mixed with 10.9 g of copper to create the alloy pewter, how many moles of metal are present in the pewter?

A)0.9643 mol total
B)1.037 mol total
C)0.6233 mol total
D)1.604 mol total
E)0.8675 mol total

Question 73

In a 41.5 g sample of carbon, how many atoms have a mass of 12.0107?

A)2.08 × 10²⁴
B)3.00 × 10²⁶
C)12
D)1.2 × 10²¹
E)0

Question 74

How many atoms of chlorine are in 354.53 g of chlorine?

A)6.02214 × 10^-23
B)6.02214 × 10²³
C)6.02214 × 10²⁴
D)6.02214 × 10²⁵
E)6.02214 × 10^-24

Question 75

How many moles of fructose are in a sample containing 1.43 × 10²⁴ molecules of fructose?

A)1.16 × 10^-48mol
B)0.420 mol
C)8.61 × 10⁴⁷ mol
D)2.38 mol
E)2.38 × 10^-1 mol

Question 76

How many atoms are in 2.50 moles of CO₂?

A)4.52 × 10²⁴ atoms
B)1.52 × 10²⁴ atoms
C)5.02 × 10²³ atoms
D)3.01 × 10²⁴ atoms
E)7.53 × 10²³ atoms

Question 77

How many atoms are in 2.50 moles of CO₂?

A)4.52 × 10²⁴ atoms
B)1.51 × 10²⁴ atoms
C)5.02 × 10²³ atoms
D)3.01 × 10²⁴ atoms
E)7.53 × 10²³ atoms

Question 78

How many atoms are in 1.00 kg of copper?

A)3.83 × 10²⁹ atoms
B)3.83 × 10²² atoms
C)15.74 atoms
D)2.61 × 10^-23 atoms
E)9.48 × 10²⁴ atoms

Question 79

If 8.32 g of copper is mixed with 5.2372 × 10^-2 mol of zinc to create the alloy brass, how many metal atoms total are present in the brass?

A)7.88 × 10²² metal atoms
B)3.04 × 10^-25 metal atoms
C)1.10 × 10²³ metal atoms
D)3.15 × 10²² metal atoms
E)3.15 × 10^-22 metal atoms

Question 80

Which of the following contains the MOST atoms? You shouldn't need to do a calculation here.

A)10.0 g Ne
B)10.0 g He
C)10.0 g Ar
D)10.0 g Kr
E)10.0 g Mg