Question 1

What is the atomic number for tin?

Accepted Answer

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

Question 2

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?

Accepted Answer

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 
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 3

An atom of 131Xe contains ________ electrons.

Accepted Answer

A) 131 
B) 185 
C) 77 
D) 123 
E) 54 
A) 131 
B) 185 
C) 77 
D) 123 
E) 54

Question 4

Predict the charge of the most stable ion of bromine.

Accepted Answer

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

Question 5

Match the following.

-potassium

Accepted Answer

A) Si 
B) Fe 
C) Mg 
D) C 
E) K 
A) Si 
B) Fe 
C) Mg 
D) C 
E) K

Question 6

Isotopes differ in the number of what particle?

Accepted Answer

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

Question 7

Predict the charge that a calcium ion would have.

Accepted Answer

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

Question 8

How many Li atoms are contained in 97.9 g of Li?

Accepted Answer

A) 5.90 × 1025 Li atoms 
B) 7.09 × 1021 Li atoms 
C) 8.49 × 1024 Li atoms 
D) 4.27 × 1022 Li atoms 
E) 4.18 × 1024 Li atoms 
A) 5.90 × 1025 Li atoms 
B) 7.09 × 1021 Li atoms 
C) 8.49 × 1024 Li atoms 
D) 4.27 × 1022 Li atoms 
E) 4.18 × 1024 Li atoms

Question 9

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

Accepted Answer

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 
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 10

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

Accepted Answer

A) Si4+ 
B) Mg 
C) Ne 
D) Si 
E) Mg2+ 
A) Si4+ 
B) Mg 
C) Ne 
D) Si 
E) Mg2+

Question 11

Which of the following elements is an alkali metal?

Accepted Answer

A) Zn 
B) Xe 
C) F 
D) Li 
E) Ca 
A) Zn 
B) Xe 
C) F 
D) Li 
E) Ca

Question 12

Iodine belongs to the ________ group of the periodic table.

Accepted Answer

A) alkali metal 
B) alkaline earth metal 
C) halogen 
D) noble gas 
A) alkali metal 
B) alkaline earth metal 
C) halogen 
D) noble gas

Question 13

Argon belongs to the ________ group of the periodic table.

Accepted Answer

A) alkali metal 
B) alkaline earth metal 
C) halogen 
D) noble gas 
A) alkali metal 
B) alkaline earth metal 
C) halogen 
D) noble gas

Question 14

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

Accepted Answer

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. 
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 15

An atom that has an atomic number of 20 and a mass number of 42 is an isotope of an atom that has

Accepted Answer

A) an atomic number of 21 and a mass number of 42. 
B) an atomic number of 20 and a mass number of 40. 
C) 22 neutrons and 20 protons. 
D) 22 protons and 20 neutrons. 
A) an atomic number of 21 and a mass number of 42. 
B) an atomic number of 20 and a mass number of 40. 
C) 22 neutrons and 20 protons. 
D) 22 protons and 20 neutrons.

Question 16

Give the name of the instrument that is used to measure masses of atoms and the percent abundance of isotopes.

Accepted Answer

The answer of Give the name of the instrument that...

Question 17

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

Accepted Answer

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

Question 18

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

Accepted Answer

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 
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

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

Accepted Answer

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 
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 20

Which of the following statements about isotopes is TRUE?

Accepted Answer

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. 
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.

Exam 2: Atoms and Elements

What is the atomic number for tin?

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?

An atom of 131Xe contains ________ electrons.

Predict the charge of the most stable ion of bromine.

Match the following. -potassium

Isotopes differ in the number of what particle?

Predict the charge that a calcium ion would have.

How many Li atoms are contained in 97.9 g of Li?

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

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

Which of the following elements is an alkali metal?

Iodine belongs to the ________ group of the periodic table.

Argon belongs to the ________ group of the periodic table.

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

An atom that has an atomic number of 20 and a mass number of 42 is an isotope of an atom that has

Give the name of the instrument that is used to measure masses of atoms and the percent abundance of isotopes.

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

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

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

Which of the following statements about isotopes is TRUE?

Units of Measurement for Physical and Chemical Change

Molecules, Compounds, and Nomenclature

Chemical Reactions and Stoichiometry

Gases

Thermochemistry

The Quantum-Mechanical Model of the Atom

Periodic Properties of the Elements

Chemical Bonding I: Lewis Theory

Chemical Bonding Ii: Molecular Shapes, Valence Bond Theory, and Molecular Orbital Theory

Liquids, Solids, and Intermolecular Forces

Solutions

Chemical Kinetics

Chemical Equilibrium

Acids and Bases

Aqueous Ionic Equilibrium

Gibbs Energy and Thermodynamics

Electrochemistry

Radioactivity and Nuclear Chemistry

Organic Chemistry I: Structures

Organic Chemistry II: Reactions

Biochemistry

Chemistry of the Nonmetals

Metals and Metallury

Transition Metals and Coordination Compounds

Filters

An atom of 131_Xe contains ________ electrons.

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

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

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