Deck 2: Atoms and Elements

Question 1

Which of the following statements is FALSE according to John Dalton's reformulated atomic theory?

A) Each element is composed of destructible particles called atoms.
B) All atoms of a given element have the same mass as well as other properties.
C) Compounds are formed when atoms combine in simple, whole-number ratios.
D) Atoms composing one element cannot change into atoms of another element during a chemical reaction.
E) All atoms of a given element have the same physical and chemical properties.

Answer 1

Each element is composed of destructible particles called atoms.

Question 2

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.

Answer 2

Atoms of carbon do not change into another element during a chemical reaction with chlorine.

Question 3

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

Answer 3

Law of the conservation of mass

Question 4

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

Question 5

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 6

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 7

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 8

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 9

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

Question 10

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 11

What are isotopes?

A) Atoms with the same number of neutrons but different numbers of protons.
B) Atoms with the same number of protons but different numbers of neutrons.
C) Atoms with the same number of protons but different numbers of electrons.
D) Atoms with the same number of electrons but different numbers of protons.
E) Atoms with the same number of neutrons but different numbers of electrons.

Question 12

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 13

Identify the element that has an atomic number of 40.

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

Question 14

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

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

Question 15

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

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

Question 16

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

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

Question 17

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 18

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 19

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 20

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 21

How many neutrons are in arsenic-42?

A) 33
B) 41
C) 9
D) 41.9
E) 75

Question 22

Identify the symbol for fluorine.

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

Question 23

Which of the following statements is FALSE?

A) Atoms are composed of protons, neutrons, and electrons.
B) The number of protons in the nucleus of an atom is equal to its atomic number.
C) Atoms that have lost or gained electrons form ions.
D) Cations are negatively charged.
E) Atomic mass number is equal to the sum of the number of protons and neutrons.

Question 24

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

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

Question 25

Isotopes differ in the number of ________.

A) protons
B) neutrons
C) electrons
D) neutrons and electrons
E) protons and electrons

Question 26

How many electrons are in arsenic?

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

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

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 29

Identify the symbol for silver.

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

Question 30

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 31

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 32

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 33

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 34

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 35

Predict the charge that a calcium ion would have.

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

Question 36

How many protons are in arsenic?

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

Question 37

Predict the charge that an aluminum ion would have.

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

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

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 40

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 41

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

A) 70.92 u
B) 70.93 u
C) 70.94 u
D) 70.91 u
E) 70.930 u

Question 42

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

A) 141.911 u
B) 142.617 u
C) 140.334 u
D) 142.501 u
E) 139.886 u

Question 43

What is the atomic number for tin?

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

Question 44

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 45

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

A) 51.94 u
B) 51.69 u
C) 208.7 u
D) 53.21 u
E) 52.00 u

Question 46

Identify the largest by size 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 47

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 u. Calculate the atomic mass of carbon-12 if the atomic mass of carbon is 12.0107 u.

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

Question 48

What is the atomic mass for cadmium?

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

Question 49

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

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

Question 50

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

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

Question 51

What is the atomic mass for tin?

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

Question 52

Identify the number of electrons in P^-3.

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

Question 53

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

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

Question 54

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

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

Question 55

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

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

Question 56

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

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

Question 57

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

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

Question 58

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 u 48.61%
Zn-66 65.9260 u 27.9%
Zn-67 66.9271 u 4.1%
Zn-68 67.9248 u 18.75%
Zn-70 69.9253 u 0.62%

A) 66.3 u
B) 65.4 u
C) 66.7 u
D) 65.1 u
E) 64.8 u

Question 59

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

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

Question 60

Identify the number of protons in P^-3.

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

Question 61

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 62

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 63

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 64

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 65

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 66

The atomic mass of tungsten is 183.84 u. 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 u 0.12%
W-182 181.9482 u 26.50%
W-183 182.9502 u 14.31%
W-184 183.9509 u 30.64%
W-186 28.43%

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

Question 67

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 68

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 69

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 70

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 71

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 72

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 73

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

A) 1.16 × 10^-48 mol
B) 0.420 mol
C) 8.61 × 10⁴⁷ mol
D) 2.37 mol
E) 2.38 × 10^-1 mol

Question 74

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 u 32.88%
X-47 46.9443 u 67.12%

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

Question 75

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

Question 76

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 77

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 78

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 79

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

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

Question 80

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