Deck 2: Atoms

Question 1

Molecules can be described as

A) mixtures of two or more pure substances.
B) mixtures of two or more elements that has a specific ratio between components.
C) two or more atoms chemically joined together.
D) heterogeneous mixtures.
E) homogeneous mixtures.

Answer 1

two or more atoms chemically joined together.

Question 2

All of the following will lead to a homogeneous mixture EXCEPT

A) sugar and coffee.
B) mud and water.
C) salt and water.
D) ice tea and lemonade.
E) vinegar and water.

Answer 2

mud and water.

Question 3

How are gases different from solids and liquids?

A) Gases can only be made up of atoms.
B) The particles in a gas attract each other much more strongly than in solids and liquids.
C) Gases are compressible.
D) Only gases can take the shape of their container.
E) Gases are colorless.

Answer 3

Gases are compressible.

Question 4

All statements about scientific theories are true EXCEPT

A) they explain why nature behaves the way it does.
B) they must have the ability to make predictions on future behavior.
C) they should use observations to test the theory.
D) they are derived from hypothesis.
E) they are speculation.

Question 5

an atom that has lost an electron is

A) a cation.
B) unlikely to be found in homogeneous mixtures.
C) electrically neutral.
D) likely to behave exactly like the parent atom.
E) an anion.

Question 6

Give the composition of water.

A) two hydrogen atoms and two oxygen atoms
B) one hydrogen atom and one oxygen atom
C) two hydrogen atoms and one oxygen atom
D) one hydrogen atom and two oxygen atoms

Question 7

Rank in the order of increasing mass.

A) proton, neutron, electron
B) neutron, proton, electron
C) electron, proton, neutron
D) electron, neutron, proton
E) proton, electron, neutron

Question 8

A new compound was recently discovered and found to have an atomic weight of 342.38 amu.This element has two isotopes,the lighter of which has a mass of 340.91 amu and an abundance of 68.322%.What is the mass of the heavier isotope?

A) 350.21
B) 345.55
C) 342.38
D) 348.67
E) 343.29

Question 9

Identify the characteristics of a solid.

A) definite volume and definite shape
B) definite volume and no definite shape
C) no definite shape and definite volume
D) no definite shape and no definite volume

Question 10

A sample of a compound containing only carbon and oxygen decomposes and produces 24.50g of carbon and 32.59g of oxygen.What is the sample?

A) CO
B) CO₂
C) CO₃
D) C₃O₂
E) C₂O

Question 11

A scientific law

A) is a brief statement that summarizes past observations and makes predictions.
B) is subject to change via legal action.
C) contains an explanation of observations.
D) must have a mathematical formula.
E) cannot be modified.

Question 12

The atomic number (Z)is the number of ________ found in the nucleus of an atom.

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

Question 13

Identify the characteristics of a gas.

A) definite volume and definite shape
B) definite volume and no definite shape
C) no definite shape and definite volume
D) no definite shape and no definite volume

Question 14

Which of the following statements about the phases of matter is TRUE?

A) In both solids and liquids, the atoms or molecules pack closely to one another.
B) Solids are highly compressible.
C) Gaseous substances have long-range repeating order.
D) There is only one type of geometric arrangement that the atoms or molecules in any solid can adopt.
E) Liquids have a large portion of empty volume between molecules.

Question 15

An element has three stable isotopes with masses of 27.977 amu,28.976 amu,and 29.973 amu.The heavier two isotopes have an abundance of 4.68% and 3.09%,respectively.What is the mass of the element?

A) 27.684 amu
B) 29.251 amu
C) 28.085 amu
D) 30.107 amu
E) 28.991 amu

Question 16

A substance composed of two or more elements in a fixed,definite proportion is

A) a homogeneous mixture.
B) a heterogeneous mixture.
C) a compound.
D) a solution.
E) an alloy.

Question 17

Give the composition of hydrogen peroxide.

A) two hydrogen atoms and two oxygen atoms
B) one hydrogen atom and one oxygen atom
C) two hydrogen atoms and one oxygen atom
D) one hydrogen atom and two oxygen atoms

Question 18

Rutherford's Gold Foil Experiment helped prove

A) the diameter of a gold atom.
B) the exact charge of an electrons.
C) the exact mass of a gold atom.
D) that the mass of an atom is concentrated in a very small space.
E) the mass to charge ratio of an electron.

Question 19

Identify the characteristics of a liquid.

A) definite volume and definite shape
B) definite volume and no definite shape
C) no definite shape and definite volume
D) no definite shape and no definite volume

Question 20

A substance that can't be chemically broken down into simpler substances is

A) a homogeneous mixture.
B) an element.
C) a heterogeneous mixture.
D) a compound.
E) a gas.

Question 21

Which of the following represents a hypothesis?

A) Sodium reacts with water to form sodium hydroxide and hydrogen gas.
B) Nitrogen gas is a fairly inert substance.
C) Nickel has a silvery sheen.
D) When a substance combusts, it combines with air.
E) When wood burns, heat is given off.

Question 22

When two elements 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 23

Which of the following statements is FALSE according to Dalton's Atomic Theory?

A) Atoms combine in simple whole number ratios to form compounds.
B) All atoms of chlorine have identical properties that distinguish them from other elements.
C) One carbon atom will combine with one oxygen atom to form a molecule of carbon monoxide.
D) Atoms of sodium do not change into another element during 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 24

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

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

Question 25

Identify the charges of the 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 26

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 27

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 28

The Scientific Method

A) is just a theory.
B) is a strict set of rules and procedures that lead to inarguable fact.
C) isn't used much in modern chemistry.
D) is based on continued observation and experiment.
E) is a framework for proving an argument you know to be true.

Question 29

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 30

Which of the following represents a valid hypothesis?

A) Neon does not react with oxygen.
B) Sodium metal reacts violently with water.
C) Lead is soft and malleable.
D) Oxygen is a gas at room temperature.
E) Metals tend to lose electrons.

Question 31

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 32

Two or more substances in variable proportions,where the composition is constant throughout are

A) a compound.
B) an element.
C) a heterogeneous mixture.
D) a homogeneous mixture.
E) a crystalline solid.

Question 33

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 34

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 35

Two or more substances in variable proportions,where the composition is variable throughout are

A) a solution.
B) a homogeneous mixture.
C) a compound.
D) an amorphous solid.
E) a heterogeneous mixture.

Question 36

Which of the following statements is TRUE?

A) A scientific law is fact.
B) Once a theory is constructed, it is considered fact.
C) A hypothesis is speculation that is difficult to test.
D) An observation explains why nature does something.
E) A scientific law summarizes a series of related observations.

Question 37

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 38

The statement,"In a chemical reaction,matter is neither created nor destroyed" is called

A) the Law of Conservation of Mass.
B) Dalton's Atomic Theory.
C) the Scientific Method.
D) the Law of Multiple Proportions.
E) the Law of Definite Proportions.

Question 39

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

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

Question 40

All of the following are SI base units of measurement,EXCEPT

A) meter.
B) gram.
C) second.
D) kelvin.
E) mole.

Question 41

The atomic mass for cadmium is

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

Question 42

Identify the instrument that is used to determine the mass of a molecule.

A) mass spectrometer
B) nuclear magnetic resonance spectrometer
C) infrared spectrometer
D) gas chromatograph
E) ultraviolet spectrophotometer

Question 43

Calculate the atomic mass of gallium if gallium has 2 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 44

Calculate the atomic mass of element "X," if it has 2 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 45

Calculate the atomic mass of element "X," if it has 2 naturally occurring isotopes with the following masses and natural abundances. X-107 106.90509 amu 51.84%
X-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 46

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 47

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 3 or more naturally occurring isotopes.

Question 48

Silver has an atomic mass of 107.868 amu.The Ag-109 isotope (108.91 amu)is 48.16%.What is the mass,in amu,of the other isotope?

A) 106.91 amu
B) 105.87 amu
C) 108.47 amu
D) 106.12 amu

Question 49

Gallium has an atomic mass of 69.723 amu.The Ga-69 (68.926 amu)is 60.111%.What is the amu of the other isotope?

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

Question 50

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 51

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 52

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 53

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

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

Question 54

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 55

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

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

Question 56

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 57

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 58

Ions differ from atoms in their number of

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

Question 59

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 60

Give the symbol for silver.

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

Question 61

Calculate the mass (in ng)of 2.33 × 10²⁰ atoms of oxygen.

A) 6.19 × 10⁶ ng
B) 1.62 × 10⁷ ng
C) 2.25 × 10³ ng
D) 3.73 × 10⁶ ng
E) 4.69 × 10⁷ ng

Question 62

How many iron atoms are contained in 354 g of iron?

A) 2.62 × 10²⁵ Fe atoms
B) 2.13 × 10²⁶ Fe atoms
C) 4.69 × 10²⁴ Fe atoms
D) 3.82 × 10²⁴ Fe atoms
E) 9.50 × 10²² Fe atoms

Question 63

Iodine is an example of

A) a compound.
B) an element.
C) a heterogeneous mixture.
D) a homogeneous mixture.

Question 64

What mass (in mg)does 2.63 moles of nickel have?

A) 44.8 mg
B) 2.23 × 10⁴ mg
C) 129 mg
D) 3.56 × 10⁵ mg
E) 1.54 × 10⁵ mg

Question 65

Calculate the atomic mass of magnesium if magnesium has 3 naturally occurring stable isotopes with the following masses and natural abundances. Mg-24 23.9996 amu 78.99%
Mg-25 24.9858 amu 10.00%
Mg-26 25.9826 amu 11.01%

A) 22.53 amu
B) 24.32 amu
C) 24.86 amu
D) 25.41 amu
E) 23.92 amu

Question 66

Calculate the mass (in mg)of 4.82 × 10²² atoms of sodium.

A) 3.48 mg
B) 287 × 10³ mg
C) 287 mg
D) 1.84 × 10³ mg
E) 1.84 mg

Question 67

Choose the pure substance from the list below.

A) coffee
B) a casserole
C) carbon dioxide
D) salt water
E) pomegranate juice

Question 68

Identify the crystalline solid.

A) plastic
B) glass
C) table salt
D) water
E) bleach

Question 69

How many phosphorus atoms are contained in 158 kg of phosphorus?

A) 3.07 × 10²⁷ phosphorus atoms
B) 2.95 × 10²⁷ phosphorus atoms
C) 3.25 × 10²⁸ phosphorus atoms
D) 1.18 × 10²⁴ phosphorus atoms
E) 8.47 × 10²⁴ phosphorus atoms

Question 70

Natural gas is an example of

A) a compound.
B) an element.
C) a heterogeneous mixture.
D) a homogeneous mixture.

Question 71

Water is an example of

A) a compound.
B) an element.
C) a heterogeneous mixture.
D) a homogeneous mixture.

Question 72

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

A) protactinium
B) zirconium
C) mangesium
D) xenon
E) titanium

Question 73

How many nitrogen atoms are contained in 485 cmol of atomic nitrogen?

A) 4.25 × 10²² N atoms
B) 7.87 × 10²⁵ N atoms
C) 2.60 × 10²³ N atoms
D) 2.92 × 1024 N atoms
E) 5.37 × 10²⁶ N atoms

Question 74

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 75

Calculate the mass (in kg)of 4.87 × 10²⁵ atoms of Zn.

A) 5.29 kg
B) 1.89 kg
C) 8.09 kg
D) 1.24 kg
E) 1.09 kg

Question 76

What species is represented by the following information?
P⁺ = 53 n° = 76 e^- = 54

A) Os
B) Os^-
C) I⁺
D) I
E) I^-

Question 77

How many moles of Cs are contained in 595 kg of Cs?

A) 2.23 × 10² moles Cs
B) 4.48 × 10³ moles Cs
C) 7.91 × 10⁴ moles Cs
D) 1.26 × 10³ moles Cs
E) 5.39 × 10² moles Cs

Question 78

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 79

A wooden baseball bat is an example of

A) a compound.
B) an element.
C) a heterogeneous mixture.
D) a homogeneous mixture.

Question 80

How many moles of Kr are contained in 398 mg of Kr?

A) 4.75 × 10^-3 moles Kr
B) 33.4 moles Kr
C) 2.11 × 10^-4 moles Kr
D) 2.99 × 10^-3 moles Kr
E) 1.19 × 10^-4 moles Kr