Deck 1: A Very Brief History of Chemistry

Question 1

Which of the following is the logical progression of elements formed in a star?

A)Hydrogen $\rarr$ Helium $\rarr$ Argon $\rarr$ Carbon
B)Hydrogen $\rarr$ Helium $\rarr$ Carbon $\rarr$ Argon
C)Helium $\rarr$ Hydrogen $\rarr$ Argon $\rarr$ Carbon
D)Helium $\rarr$ Hydrogen $\rarr$ Carbon $\rarr$ Argon
E)Argon $\rarr$ Carbon $\rarr$ Helium $\rarr$ Hydrogen

Answer 1

Hydrogen $\rarr$ Helium $\rarr$ Carbon $\rarr$ Argon

Question 2

Why is iron the heaviest element formed in a star prior to the formation of a supernova?

A)The formation of iron in a star starts a cooling process of the star, ending nucleosynthesis.
B)Iron reacts with the hydrogen in stars to cause a violet explosion that leads to a super nova.
C)Iron is the heaviest element that is stable at high temperatures; all others are radioactive.
D)The formation of iron in a star causes a reaction with helium that causes nucleosynthesis to end.
E)When iron is formed in the outer layers of a star, the iron has enough kinetic energy to leave the gravity of the star.

Answer 2

The formation of iron in a star starts a cooling process of the star, ending nucleosynthesis.

Question 3

One would expect a fairly even distribution of elements on the earth; instead, the distribution is uneven. Which of the following best describes why we observe this?

A)The nebula that formed the earth had elements that were not evenly distributed.
B)Winds on the surface of the earth have moved the heavy and light elements into bands.
C)The early earth liquefied, resulting in heavier elements migrating toward the core and lighter elements moving toward the surface. This migration to the surface was largely by lava flows, which were inconsistent.
D)Some water-soluble elements were washed by water into pockets on the surface.
E)The magnetic properties of the core caused the metals to pool into certain areas between the poles on the earth.

Answer 3

The early earth liquefied, resulting in heavier elements migrating toward the core and lighter elements moving toward the surface. This migration to the surface was largely by lava flows, which were inconsistent.

Question 4

The relative number of atoms of each element in a particular compound

A)is always l:l.
B)is the same as the density ratio.
C)is the same as the weight ratio.
D)is definite and constant.
E)cannot be determined experimentally.

Question 5

Which of the following postulates from Dalton's atomic theory are now considered incorrect?
I. All atoms of a given element are identical.
II. Matter consists of very small particles known as atoms.
III. Atoms are indestructible and indivisible.

A)III only
B)II only
C)I only
D)I and II
E)I and III

Question 6

Which of the following statements is/are consistent with Dalton's atomic theory?
I. The atoms in a given sample of an element do not share any common properties.
II. Matter consists of particles called atoms.
III. In chemical reactions, atoms merely rearrange and do not disintegrate.

A)III only
B)II only
C)I only
D)II and III
E)I and III

Question 7

Which of the following statements is/are NOT consistent with Dalton's atomic theory?
I. The atoms in a given sample of an element do not share any common properties.
II. Matter consists of tiny particles called molecular substances.
III. In chemical reactions, atoms merely rearrange and do not disintegrate.

A)III only
B)II only
C)I only
D)II and III
E)I and II

Question 8

Which of the following postulates from Dalton's atomic theory is incorrectly stated?

A)The atoms in a given sample of an element are identical.
B)Matter consists of tiny particles called atoms.
C)In chemical reactions, atoms merely rearrange and do not disintegrate.
D)In a given chemical compound, the atoms can be present in various numerical ratios.
E)The atoms of different elements differ in mass and other properties.

Question 9

Which of the following is consistent with the postulates from Dalton's atomic theory?

A)The atoms in a given sample of an element are not necessarily identical.
B)Matter consists of tiny particles called ions.
C)In chemical reactions, atoms both rearrange and disintegrate in smaller subatomic particles.
D)The atoms of different elements can be identical in mass and other properties.
E)In a given chemical compound, the atoms are always present in the same fixed numerical ratio.

Question 10

Which one of the statements below is true?

A)When two atoms combine to form a chemical compound, they do so in many different proportions by mass.
B)When two different compounds combine to form an element, they do so in definite proportions by mass.
C)When two different elements combine to form a chemical compound, they do so in definite proportions by mass.
D)When two molecules combine in a chemical reaction, a number of different elements can be generated depending on the masses used.
E)When two different elements combine to form a mixture, they do so in definite proportions by atomic number.

Question 11

Which one of the statements below is false?

A)In chemical reactions, atoms are rearranged.
B)In a given compound, the atoms are always present in the same fixed numerical ratio.
C)Matter is made up of tiny particles called atoms.
D)In a sealed reaction flask, the total mass after the reaction is over, is the same as before the reaction started.
E)When hydrogen and oxygen react to form water, the mass of oxygen atoms is equal to the mass of hydrogen atoms.

Question 12

Which of the following examples is consistent with the postulates from Dalton's atomic theory? Hint: Be sure to keep the definitions of atoms and molecules straight!

A)The atoms in a sample of chlorine are similar to the atoms in a sample of elemental sulfur.
B)Matter consists of extremely tiny particles that are always either positively or negatively charged.
C)When water is formed from oxygen and hydrogen molecules, the atoms in water are grouped differently compared to the atoms in molecules of hydrogen and oxygen.
D)A sample of water contains hydrogen and oxygen atoms combined in two different ratios by mass.
E)There are eight different types of sulfur atoms in any naturally occurring sample of elemental sulfur.

Question 13

To form hydrogen sulfide, H₂S, 4.03 g of molecular hydrogen (H₂)are reacted with 62.13 g of sulfur (S). If all of the hydrogen and sulfur completely react to form hydrogen sulfide, how many grams of hydrogen sulfide should be formed?

A)66.16 g
B)58.10 g
C)4.03 g
D)70.19 g
E)33.03 g

Question 14

Which of these scientists developed the atomic theory?

A)John Dalton
B)J. J. Thomson
C)Robert Millikan
D)Henry Moseley
E)Ernest Rutherford

Question 15

Which one of the following contributes to the charge of an atom, but does NOT contribute significantly to the mass of an atom?

A)electrons
B)nuclei
C)photons
D)neutrons
E)protons

Question 16

Which of the following have roughly the same mass?

A)a proton and an electron
B)a neutron and an electron
C)a neutron and a proton
D)an electron and an alpha particle
E)none of these options

Question 17

Which of the following have opposite electric charges?

A)a proton and an electron
B)a neutron and an electron
C)a neutron and a proton
D)an electron and an alpha particle
E)none of these options

Question 18

Consider the atoms of ⁶⁵Cu and ⁶⁵Zn. Both of these atoms have the same

A)number of electrons.
B)atomic mass.
C)number of neutrons.
D)mass number.
E)number of protons.

Question 19

Which of the following particles will not be deflected by charged plates?

A)hydrogen atoms
B)cathode rays
C)alpha particles
D)protons
E)These are all deflected by charged plates.

Question 20

Uranium exists in nature in the form of several isotopes and the different isotopes have different

A)atomic numbers.
B)charges.
C)numbers of electrons.
D)numbers of neutrons.
E)numbers of protons.

Question 21

Which answer below best describes all atoms of a given isotope of a particular element?

A)They possess the same mass but their other properties differ.
B)They possess similar chemical properties and the same mass but have nothing else in common.
C)They possess the same atomic number but have nothing else in common.
D)They possess the same number of electrons, the same atomic number, and similar chemical properties but differ in their masses.
E)They possess the same number of electrons, the same atomic number, the same mass, and the same chemical properties.

Question 22

Which answer below best describes all atoms of a particular element?

A)They possess the same number of electrons, the same atomic number, and the same mass, but have nothing else in common.
B)They possess the same mass and the same chemical properties but have nothing else in common.
C)They possess the same number of electrons and the same atomic number but may differ in mass.
D)They possess the same number of electrons, chemical properties, and mass but have nothing else in common.
E)They possess the same atomic number and the same mass but have nothing else in common.

Question 23

The species shown below that has 24 neutrons is

A) Cr
B) Mn
C) Mg
D) Sc
E) V

Question 24

The species shown below that has 24 electrons is

A) Cr
B) Mn
C) Mg
D) Sc
E) V

Question 25

The species V has the same number of neutrons as

A) V
B) Sc
C) Mn
D) Cr
E) Co

Question 26

Consider the atoms of Mg and Al. Both of these species have the same

A)number of neutrons and electrons.
B)number of ions.
C)number of neutrons.
D)number of neutrons and mass number.
E)number of protons and electrons.

Question 27

Consider the atoms of ⁵⁹Co and ⁶⁰Co. Both of these atoms have the same

A)number of neutrons and electrons.
B)number of neutrons and ions.
C)mass number.
D)number of photons.
E)number of protons and electrons.

Question 28

An atom of the isotope sulfur-33 consists of how many protons, neutrons, and electrons? (p = proton, n = neutron, e = electron)

A)15 p, 18 n, 15 e
B)16 p, 17 n, 16 e
C)33 p, 16 n, 33 e
D)16 p, 16 n, 33 e
E)16 p, 33 n, 16 e

Question 29

An ion of the isotope chlorine-35 has an ionic charge of 1-. How many protons, neutrons, and electrons does it contain? (p = proton, n = neutron, e = electron)Hint: Consider how changes in the number of electrons versus the number of protons affects the ionic charge of an ion.

A)17 p, 35 n, 17 e
B)17 p, 17 n, 35 e
C)18 p, 17 n, 18 e
D)17 p, 18 n, 18 e
E)35 p, 17 n, 18 e

Question 30

Compare Mg and Al. In what respect do these species differ? I. number of neutrons and number of electrons
II. number of protons, and number of neutrons
III. mass number and number of protons

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

Question 31

A neutral iodine atom has an atomic mass number = 131. Which description below fits this atom?

A)39 protons, 78 neutrons, 39 electrons
B)53 protons, 78 neutrons, 53 electrons
C)52 protons, 79 neutrons, 54 electrons
D)53 protons, 131 neutrons, 53 electrons
E)54 protons, 131 neutrons, 54 electrons

Question 32

Which description below fits the atom?Hint: Remember how charge alters the number of electrons.

A)29 protons, 65 neutrons, 29 electrons
B)29 protons, 36 neutrons, 65 electrons
C)29 protons, 36 neutrons, 31 electrons
D)29 protons, 36 neutrons, 27 electrons
E)31 protons, 34 neutrons, 29 electrons

Question 33

Which description below fits the ¹¹²Cd atom?

A)48 protons, 64 neutrons, 48 electrons
B)48 protons, 62 neutrons, 48 electrons
C)48 protons, 64 neutrons, 46 electrons
D)48 protons, 62 neutrons, 46 electrons
E)50 protons, 64 neutrons, 48 electrons

Question 34

The atomic mass of naturally occurring iron, which is a mixture of isotopes, is listed as . This means that the average mass of iron is

A)55.847 times as great as that of a ¹²C atom.
B)55.847 times as great as that of a ¹H atom.
C)55.847/1.0079 times as great as that of a ¹H atom.
D)55.847/12.000 times as great as that of a ¹²C atom.
E)55.847/12.011 times as great as that of a ¹²C atom.

Question 35

The atomic mass of naturally occurring nickel, which is a mixture of isotopes, is listed as 58.6934 u. This means that the average mass of nickel is

A)58.6934 times as great as that of a ¹²C atom.
B)58.6934 times as great as that of a ¹H atom.
C)58.6934/1.0079 times as great as that of a ¹H atom.
D)58.6934/12.000 times as great as that of a ¹²C atom.
E)58.6934/12.011 times as great as that of a ¹²C atom.

Question 36

The atomic mass of naturally occurring silver, which is a mixture of two isotopes, is listed as 107.868 u. This means that ,Hint: Individual atoms have a mass number that is the sum of the protons and neutrons.

A)all silver atoms found in nature have a mass that is 107.868/12.000 times as great as that of a ¹²C atom.
B)all silver atoms found in nature have a mass that is 107.868/1.0079 times as great as that of a ¹H atom.
C)some silver atoms found in nature have a mass that is 107.868/12.000 times as great as that of a ¹²C atom.
D)some silver atoms found in nature have a mass that is 107.868/1.0079 times as great as that of a ¹H atom.
E)no silver atoms found in nature has a mass that is 107.868/12.000 times as great as that of a ¹²C atom.

Question 37

The atomic mass of naturally occurring copper, which is a mixture of two isotopes, is listed as 63.546 u. This means that ,Hint: Individual atoms have a mass number which is the sum of the protons and neutrons.

A)all copper atoms found in nature have a mass that is 63.546/12.000 times as great as that of a ¹²C atom.
B)all copper atoms found in nature have a mass that is 63.546/1.0079 times as great as that of a ¹H atom.
C)some copper atoms found in nature have a mass that is 63.546/12.000 times as great as that of a ¹²C atom.
D)some copper atoms found in nature have a mass that is 63.546/1.0079 times as great as that of a ¹H atom.
E)no copper atoms found in nature has a mass that is 63.546/12.000 times as great as that of a ¹²C atom.

Question 38

The atomic mass of naturally occurring gallium, which is a mixture of two isotopes, is listed as 69.723 u. This means that ,Hint: Individual atoms have a mass number that is the sum of the protons and neutrons.

A)all gallium atoms found in nature have a mass that is 69.723/12.000 times as great as that of a ¹²C atom.
B)all gallium atoms found in nature have a mass that is 69.723/1.0079 times as great as that of a ¹H atom.
C)some gallium atoms found in nature have a mass that is 69.723/12.000 times as great as that of a ¹²C atom.
D)some gallium atoms found in nature have a mass that is 69.723/1.0079 times as great as that of a ¹H atom.
E)no gallium atoms found in nature has a mass that is 69.723/12.000 times as great as that of a ¹²C atom.

Question 39

The atomic mass of naturally occurring fluorine, which exists in nature as a single isotope, is listed as 18.9984 u. This means that

A)all fluorine atoms found in nature have a mass that is 18.9984/12.000 times as great as that of a ¹²C atom.
B)all fluorine atoms found in nature have a mass that is 18.9984/1.0079 times as great as that of a ¹H atom.
C)some fluorine atoms found in nature have a mass that is 18.9984/12.000 times as great as that of a ¹²C atom.
D)some fluorine atoms found in nature have a mass that is 18.9984/1.0079 times as great as that of a ¹H atom.
E)no fluorine atom found in nature has a mass that is 18.9984/12.000 times as great as that of a ¹²C atom.

Question 40

The atomic mass of naturally occurring cobalt, which exists in nature as a single isotope, is listed as 58.9332 u. This means that

A)all cobalt atoms found in nature have a mass that is 58.9332/12.000 times as great as that of a ¹²C atom.
B)all cobalt atoms found in nature have a mass that is 58.9332/1.0079 times as great as that of a ¹H atom.
C)some cobalt atoms found in nature have a mass that is 58.9332/12.000 times as great as that of a ¹²C atom.
D)some cobalt atoms found in nature have a mass that is 58.9332/1.0079 times as great as that of a ¹H atom.
E)no cobalt atom found in nature has a mass that is 58.9332/12.000 times as great as that of a ¹²C atom.

Question 41

A naturally occurring element consists of three isotopes. The data for the isotopes are:
Isotope 1: 46.972 u, 69.472%
Isotope 2: 48.961 u, 21.667%
Isotope 3: 49.954 u, 8.8610% What is the average atomic mass of this naturally occurring element?

A)47.667 u
B)47.699 u
C)48.629 u
D)48.667 u
E)48.961 u

Question 42

A naturally occurring element consists of three isotopes. The data for the isotopes are:
Isotope 1: 146.9672 u, 64.792%
Isotope 2: 148.9638 u, 26.117%
Isotope 3: 149.9592 u, 9.0910% What is the average atomic mass of this naturally occurring element?

A)49.254 u
B)147.76 u
C)148.63 u
D)148.67 u
E)147.88 u

Question 43

A naturally occurring element consists of three isotopes. The data for the isotopes are:
Isotope 1: 187.9122 u., 10.861%
Isotope 2: 190.9047 u, ------%
Isotope 3: 192.8938 u, 76.711% What is the average atomic mass of this naturally occurring element? Hint: Percentages should always add up to 100% then find the weighted average.

A)64.035 u
B)190.57 u
C)190.67 u
D)192.08 u
E)192.11 u

Question 44

A naturally occurring element consists of three isotopes. The data for the isotopes are:
Isotope 1: 147.9554 u, 10.563%
Isotope 2: 150.9496 u, 70.811%
Isotope 3: 152.9461 u, 18.626% What is the average atomic mass of this naturally occurring element?

A)50.335 u
B)150.62 u
C)150.67 u
D)151.01 u
E)151.08 u

Question 45

A naturally occurring element consists of two isotopes. The data for the isotopes are:
Isotope 1 68.5257 u 60.226 %
Isotope 2 70.9429 u ------ % Calculate the average atomic mass of this element. Hint: Percentages should always add up to 100% then find the weighted average.

A)69.728 u
B)69.743 u
C)69.934 u
D)69.972 u
E)70.141 u

Question 46

Chemistry has four main ideas that were given in chapter 0. List them.

Question 47

Planets are formed after supernovas from ________ left over from the formation of a new star.

Question 48

What two factors determine the final chemical makeup of a planet?

Question 49

Molecules are made of tiny particles called ________.

Question 50

According to the Law ________, there is no gain or loss of mass in chemical reactions.

Question 51

In a chemical compound, the elements are always combined in the same proportions by ________.

Question 52

A compound is made of nitrogen and hydrogen in a ratio of 5.65 grams nitrogen to 1.22 grams of hydrogen. There are ________ grams of nitrogen in a sample of this compound containing 4.00 grams of hydrogen. Hint: Consider the ratio of the masses to determine the mass of nitrogen.

Question 53

A compound is made of nitrogen and hydrogen in a ratio of 22.6 grams nitrogen to 4.88 grams of hydrogen. There are ________ grams of hydrogen in a sample of the compound containing 12.6 grams of nitrogen. Hint: Consider the ratio of the masses to determine the mass of hydrogen.

Question 54

A compound of phosphorus and chlorine contains 3.00 grams of phosphorus and 10.3 grams of chlorine. There are ________ grams of phosphorus in a sample of the compound containing 17.2 grams of chlorine. Hint: Consider the ratio of the masses to determine the mass of phosphorous.

Question 55

A compound of phosphorus and chlorine contains 3.00 grams of phosphorus and 10.3 grams of chlorine. There are ________ total grams of the compound in a sample that contains 4.00 grams of chlorine. Hint: Consider the ratio of the masses to determine the mass of compound.

Question 56

If 2.00 grams of molecular hydrogen react with 16.00 grams of oxygen to form water, how many grams of water must be formed if all of the hydrogen and oxygen react? Hint: Consider the ratio of the masses to determine the mass of compound.

Question 57

The particles found in nuclei, the protons and neutrons, are collectively called ________.

Question 58

Which subatomic particle has a positive charge?

Question 59

How many electrons are in an atom of ³⁵Cl?

Question 60

How many nucleons are in an atom of ⁴⁰K?

Question 61

The element chlorine has two main isotopes that result in almost all chlorine on Earth. The two are listed below with their atomic masses. The average atomic mass of chlorine is listed as 35.453 u. Using this information what is the relative abundances of the two chlorine isotopes?
Chlorine-35: 34.969 u
Chlorine-37: 36.966 u ,Hint: Set up a weighted average calculation where one percentage is x and the other percentage is (100 - x).

Question 62

The element bromine has two main isotopes that result in almost all bromine on Earth. The two are listed below with their atomic masses. The average atomic mass of bromine is listed as 79.904 u. Using this information what is the relative abundances of the two chlorine isotopes?
Bromine-79: 78.918 u
Bromine-81: 80.916 u ,Hint: Set up a weighted average calculation where one percentage is x and the other percentage is (100 - x).

Question 63

Microwave radiation observed by Penzias and Wilson in 1964 helps to support the big-bang theory because it observed microwave radiation that was characteristic of a temperature that matched the predicted temperature of the universe after heating up for 14 billion years.

Question 64

Stars that are classified as red giants are formed after the outer layer of hydrogen in a star cools and is no longer white hot.

Question 65

In stars the heaviest elements migrate to the outer layers of the star due to centrifugal forces.

Question 66

Atoms are made of tiny particles called molecules.

Question 67

In any given chemical compound, elements are be combined in various non-fixed amounts by mass.

Question 68

When a piece of paper burns in a closed container, the combined masses of the products is less than the mass of the original piece of paper.

Question 69

Atoms must be broken apart into their subatomic particles and then rearranged in order for chemical reactions to occur. Hint: What happens in a chemical reaction between reactants and products?

Question 70

The hydrogen atom minus an electron is known as the proton.

Question 71

Almost the entire mass of an atom is concentrated in a very large volume outside the center of the atom.

Question 72

In a neutral atom, the number of protons must equal the number of neutrons.

Question 73

At the nanoscale level, the structures under investigation usually have dimensions of tens to hundreds of atoms.

Question 74

Molecular self-assembly occurs when two atoms can spontaneously arrange themselves into creating a diatomic molecular structure.

Question 75

The atomic force microscope that is used with electrically nonconducting samples makes it possible to obtain an image of individual atoms.

Question 76

When an electrical spark is passed through hydrogen gas molecules, positive ions can be generated through the interaction.

Question 77

When positive ions are formed in a mass spectrometer, they are attracted to a positively charged metal plate that has a small hole in its center.

Question 78

In a mass spectrometer, a beam of ions is sorted by the magnet into a number of beams based on the same charges that they have.

Question 79

In a mass spectrometer, a beam of ions emerge from between the poles of the magnet after being sorted into an array of beams based on their masses.

Question 80

According to recent IUPAC recommendations, a range of atomic masses should be used instead a single value.