Question 1

The separation of charges within a polar molecule is called a(n)________.

Accepted Answer

A) dipole 
B) dipole-dipole 
C) ionic bond 
D) strong attraction 
E) polar bond 
A) dipole 
B) dipole-dipole 
C) ionic bond 
D) strong attraction 
E) polar bond A

Question 2

If the following generic atom were to undergo ionization, what would the most likely product be?

Accepted Answer

A) +1 
B) -2 
C) -3 
D) +4 
E) would probably not ionize 
A) +1 
B) -2 
C) -3 
D) +4 
E) would probably not ionize E

Question 3

Which of the following elements will most likely form an ion with a +2 charge?

Accepted Answer

A) Na 
B) Mg 
C) Ne 
D) Si 
E) Cl 
A) Na 
B) Mg 
C) Ne 
D) Si 
E) Cl B

Question 4

Which of the following elements has six valence electrons?

Accepted Answer

A) Be 
B) B 
C) C 
D) N 
E) O 
A) Be 
B) B 
C) C 
D) N 
E) O

Question 5

Which of the following is the strongest?

Accepted Answer

A) A chemical bond 
B) An ion-dipole attraction 
C) A dipole-dipole attraction 
D) A dipole-induced dipole attraction 
E) An induced dipole-induced dipole attraction 
A) A chemical bond 
B) An ion-dipole attraction 
C) A dipole-dipole attraction 
D) A dipole-induced dipole attraction 
E) An induced dipole-induced dipole attraction

Question 6

Why does an atom with many valence electrons tend to gain electrons rather than lose any?

Accepted Answer

A) Atoms with many valence electrons tend to have relatively weak forces of attraction between the valence electrons and the nucleus. Therefore, the outer electrons are free to attract other electrons. 
B) There is stability in numbers. Atoms with many valence electrons are always attracting new electrons. 
C) The old adage that "he who has, gets" is also true in atomic structure. Atoms with many valence electrons can essentially overpower atoms with few valence electrons and attract additional electrons. 
D) Atoms with many valence electrons tend to have relatively strong forces of attraction between the valence electrons and the nucleus. This makes it easy for them to gain additional electrons. 
A) Atoms with many valence electrons tend to have relatively weak forces of attraction between the valence electrons and the nucleus. Therefore, the outer electrons are free to attract other electrons. 
B) There is stability in numbers. Atoms with many valence electrons are always attracting new electrons. 
C) The old adage that "he who has, gets" is also true in atomic structure. Atoms with many valence electrons can essentially overpower atoms with few valence electrons and attract additional electrons. 
D) Atoms with many valence electrons tend to have relatively strong forces of attraction between the valence electrons and the nucleus. This makes it easy for them to gain additional electrons.

Question 7

The neon atom tends NOT to lose any electrons because

Accepted Answer

A) of its relatively strong effective nuclear charge. 
B) that would result in a negative ion. 
C) its electrons are paired together within the same orbitals. 
D) the ionization energy is so high. 
A) of its relatively strong effective nuclear charge. 
B) that would result in a negative ion. 
C) its electrons are paired together within the same orbitals. 
D) the ionization energy is so high.

Question 8

How many oxide ions (O-2)are needed to balance the positive charge of a titanium ion (Ti+4)?

Accepted Answer

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

Question 9

Which of the following molecules contains a polar bond?

Accepted Answer

A) H-F 
B) Cl-Cl 
C) H-H 
D) F-F 
E) all of the above 
A) H-F 
B) Cl-Cl 
C) H-H 
D) F-F 
E) all of the above

Question 10

Metals are useful for the structural support of buildings because they

Accepted Answer

A) do not conduct heat well 
B) are shiny 
C) conduct electricity 
D) are strong but can be bent 
E) c and d 
A) do not conduct heat well 
B) are shiny 
C) conduct electricity 
D) are strong but can be bent 
E) c and d

Question 11

Which would you expect to have a higher melting point: sodium chloride, NaCl, or aluminum oxide, Al2O3?

Accepted Answer

A) The aluminum oxide has a higher melting point because it is a larger molecule and has a greater number of molecular interactions. 
B) NaCl has a higher melting point because it is a solid at room temperature. 
C) The aluminum oxide has a higher melting point because of the greater charges of the ions, and hence the greater force of attractions between them. 
D) The aluminum oxide has a higher melting point because of the covalent bonds within the molecule. 
A) The aluminum oxide has a higher melting point because it is a larger molecule and has a greater number of molecular interactions. 
B) NaCl has a higher melting point because it is a solid at room temperature. 
C) The aluminum oxide has a higher melting point because of the greater charges of the ions, and hence the greater force of attractions between them. 
D) The aluminum oxide has a higher melting point because of the covalent bonds within the molecule.

Question 12

Which of the following is the correct electron dot structure for carbon (atomic no. = 6)?

Accepted Answer

A) a 
B) b 
C) c 
D) d 
E) e 
A) a 
B) b 
C) c 
D) d 
E) e

Question 13

Consider the boiling points of the following compounds and their solubilities in room-temperature water. Why does the solubilities in water go down as the boiling points of these alcohols go up.

Accepted Answer

A) Larger molecules are less attracted to one another by induced dipole-induced dipole as well as by dipole-dipole and dipole-induced dipole attractions. 
B) As the boiling increases, it is more difficult to keep the alcohol from evaporating out of solution. 
C) As the boiling point increases, the size of the alcohol molecules decreases. 
D) Larger molecules are more attracted to one another by induced dipole-induced dipole as well as by dipole-dipole and dipole-induced dipole attractions. 
A) Larger molecules are less attracted to one another by induced dipole-induced dipole as well as by dipole-dipole and dipole-induced dipole attractions. 
B) As the boiling increases, it is more difficult to keep the alcohol from evaporating out of solution. 
C) As the boiling point increases, the size of the alcohol molecules decreases. 
D) Larger molecules are more attracted to one another by induced dipole-induced dipole as well as by dipole-dipole and dipole-induced dipole attractions.

Question 14

Which of the following molecules has the highest boiling point?

Accepted Answer

A) BH3 
B) NH3 
C) CH4 
D) All of the above should have the same boiling point. 
A) BH3 
B) NH3 
C) CH4 
D) All of the above should have the same boiling point.

Question 15

An atom loses an electron to another atom. Is this an example of a physical or chemical change?

Accepted Answer

A) physical change involving the formation of negative ions 
B) chemical change involving the formation of neutral atoms 
C) physical change involving the formation of positive ions 
D) chemical change involving the formation of ions 
A) physical change involving the formation of negative ions 
B) chemical change involving the formation of neutral atoms 
C) physical change involving the formation of positive ions 
D) chemical change involving the formation of ions

Question 16

Which are closer together: the two nuclei within potassium fluoride, KF, or the two nuclei within molecular fluorine, F2?

Accepted Answer

A) KF 
B) F2 
C) Both are the same. Any atom bonded to F will have the same inter-nuclear separation. 
D) It makes little sense to compare two molecules which exist in different physical states. KF is a solid while F2 is a gas. 
A) KF 
B) F2 
C) Both are the same. Any atom bonded to F will have the same inter-nuclear separation. 
D) It makes little sense to compare two molecules which exist in different physical states. KF is a solid while F2 is a gas.

Question 17

Is an ionic compound an example of a chemical compound, or is a chemical compound an example of an ionic compound?

Accepted Answer

A) An chemical compound is an example of a ionic compound. 
B) Neither is an example of the other. 
C) Each is an example of the other. 
D) An ionic compound is an example of a chemical compound. 
A) An chemical compound is an example of a ionic compound. 
B) Neither is an example of the other. 
C) Each is an example of the other. 
D) An ionic compound is an example of a chemical compound.

Question 18

Atoms of metallic elements can form ionic bonds, but they are not very good at forming covalent bonds. Why?

Accepted Answer

A) These atoms are too large to be able to come in close contact with other atoms. 
B) They have a great tendency to lose electrons. 
C) Their valence shells are already filled with electrons. 
D) They are on the wrong side of the periodic table. 
A) These atoms are too large to be able to come in close contact with other atoms. 
B) They have a great tendency to lose electrons. 
C) Their valence shells are already filled with electrons. 
D) They are on the wrong side of the periodic table.

Question 19

Which should be larger, the potassium atom, K, or the potassium ion, K⁺?

Accepted Answer

A) The potassium ion, K⁺ is larger since charging an atom always makes it larger. 
B) The potassium atom, K, with an additional shell of electrons is larger. 
C) The potassium ion, K⁺ is larger since it has an extra electron which increases its size. 
D) The potassium atom and the potassium ion are exactly the same size and only differ in charge. 
A) The potassium ion, K⁺ is larger since charging an atom always makes it larger. 
B) The potassium atom, K, with an additional shell of electrons is larger. 
C) The potassium ion, K⁺ is larger since it has an extra electron which increases its size. 
D) The potassium atom and the potassium ion are exactly the same size and only differ in charge.

Question 20

Ammonia, NH3, is more polar than is borane, BH3 because it

Accepted Answer

A) has a lone pair of electrons. 
B) is less symmetrical than borane. 
C) its hydrogens are not exactly opposite one another. 
D) all of the above 
A) has a lone pair of electrons. 
B) is less symmetrical than borane. 
C) its hydrogens are not exactly opposite one another. 
D) all of the above

Exam 15: How Atoms Bond and Molecules Attract

The separation of charges within a polar molecule is called a(n)________.

If the following generic atom were to undergo ionization, what would the most likely product be?

Which of the following elements will most likely form an ion with a +2 charge?

Which of the following elements has six valence electrons?

Which of the following is the strongest?

Why does an atom with many valence electrons tend to gain electrons rather than lose any?

The neon atom tends NOT to lose any electrons because

How many oxide ions (O-2)are needed to balance the positive charge of a titanium ion (Ti+4)?

Which of the following molecules contains a polar bond?

Metals are useful for the structural support of buildings because they

Which would you expect to have a higher melting point: sodium chloride, NaCl, or aluminum oxide, Al2O3?

Which of the following is the correct electron dot structure for carbon (atomic no. = 6)?

Consider the boiling points of the following compounds and their solubilities in room-temperature water. Why does the solubilities in water go down as the boiling points of these alcohols go up.

Which of the following molecules has the highest boiling point?

An atom loses an electron to another atom. Is this an example of a physical or chemical change?

Which are closer together: the two nuclei within potassium fluoride, KF, or the two nuclei within molecular fluorine, F2?

Is an ionic compound an example of a chemical compound, or is a chemical compound an example of an ionic compound?

Atoms of metallic elements can form ionic bonds, but they are not very good at forming covalent bonds. Why?

Which should be larger, the potassium atom, K, or the potassium ion, K⁺?

Ammonia, NH3, is more polar than is borane, BH3 because it

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Prologue: the Nature of Science

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How many oxide ions (O^-2)are needed to balance the positive charge of a titanium ion (Ti⁺⁴)?

Which would you expect to have a higher melting point: sodium chloride, NaCl, or aluminum oxide, Al₂O₃?

Which are closer together: the two nuclei within potassium fluoride, KF, or the two nuclei within molecular fluorine, F₂?

Ammonia, NH₃, is more polar than is borane, BH₃ because it