Question 1

Which of the following describes the reason for the following application of metals? designer jewelry

Accepted Answer

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

Question 2

Take money away from your bank account and the bank will show a negative credit. Take an electron away from an atom, however, and the atom shows up positive. Explain.

Accepted Answer

A) Electrons are already negative. Therefore, we know from basic math that subtracting a negative (number)from a neutral (atom), will make the result positive. 
B) Neutral atoms contain identically charged but oppositely signed protons and electrons. Removing one of the negative electrons results in an excess of positively charged protons. 
C) Removing an electron from an atom does not have the atom show up positive. It simply leaves the atom short one electron. 
D) Atoms are constantly exchanging electrons. Having an atom "show up positive" is only an expression indicating that it has taken its turn in the game of electron exchange. 
A) Electrons are already negative. Therefore, we know from basic math that subtracting a negative (number)from a neutral (atom), will make the result positive. 
B) Neutral atoms contain identically charged but oppositely signed protons and electrons. Removing one of the negative electrons results in an excess of positively charged protons. 
C) Removing an electron from an atom does not have the atom show up positive. It simply leaves the atom short one electron. 
D) Atoms are constantly exchanging electrons. Having an atom "show up positive" is only an expression indicating that it has taken its turn in the game of electron exchange.

Question 3

How do the electron-dot structures of elements in the same group in the periodic table compare with one another?

Accepted Answer

A) The structures differ by exactly two electrons between vertically consecutive elements. 
B) The number of valence shell electrons increases by one for each element from the top to the bottom of the group. 
C) Elements of the same group have the same number of valence electrons. 
D) The number of electrons in the electron-dot-structure will equal the group number for each element of the group. 
A) The structures differ by exactly two electrons between vertically consecutive elements. 
B) The number of valence shell electrons increases by one for each element from the top to the bottom of the group. 
C) Elements of the same group have the same number of valence electrons. 
D) The number of electrons in the electron-dot-structure will equal the group number for each element of the group.

Question 4

Which of the following compounds has polar covalent bonds?

Accepted Answer

A) H2O 
B) CsF2 
C) S8 
D) Ne 
E) CH4 
A) H2O 
B) CsF2 
C) S8 
D) Ne 
E) CH4

Question 5

Which of the above substances would have the largest dipole?

Accepted Answer

A) a 
B) b 
C) c 
D) Each has the same size dipole. 
E) None of the molecules has a dipole. 
A) a 
B) b 
C) c 
D) Each has the same size dipole. 
E) None of the molecules has a dipole.

Question 6

When is the geometry of a molecule not the same as its molecular shape?

Accepted Answer

A) when one or more of the substituents is a lone pair of electrons 
B) when there are an odd number of electron pairs as substituents 
C) when there are an odd number of electrons surrounding the central atom 
D) The geometry of a molecule is always the same as its shape. 
A) when one or more of the substituents is a lone pair of electrons 
B) when there are an odd number of electron pairs as substituents 
C) when there are an odd number of electrons surrounding the central atom 
D) The geometry of a molecule is always the same as its shape.

Question 7

A hydrogen atom does not form more than one covalent bond because it ________.

Accepted Answer

A) has only one shell of electrons 
B) has only one electron to share 
C) loses its valence electron so readily 
D) has such a strong electronegativity 
A) has only one shell of electrons 
B) has only one electron to share 
C) loses its valence electron so readily 
D) has such a strong electronegativity

Question 8

What is one role of unpaired valance electrons?

Accepted Answer

A) They take part in the formation of different types of bonds. 
B) They keep the paired electrons separated to minimize interaction. 
C) They are the nonbonding electrons. 
D) They provide the number of Lewis dots. 
E) They tell us which Lewis dot structure is correct. 
A) They take part in the formation of different types of bonds. 
B) They keep the paired electrons separated to minimize interaction. 
C) They are the nonbonding electrons. 
D) They provide the number of Lewis dots. 
E) They tell us which Lewis dot structure is correct.

Question 9

Atoms of nonmetallic elements form covalent bonds, but they can also form ionic bonds. How is this possible?

Accepted Answer

A) This happens when one of the bonded nonmetallic elements has a strong electronegativity. 
B) It happens when one of the nonmetallic elements loses an electron to become a positive ion. 
C) An ionic bond results when a nonmetallic elements loses an electron to a metallic element. 
D) An ionic bond results when a nonmetallic elements gains an electron from a metallic element. 
A) This happens when one of the bonded nonmetallic elements has a strong electronegativity. 
B) It happens when one of the nonmetallic elements loses an electron to become a positive ion. 
C) An ionic bond results when a nonmetallic elements loses an electron to a metallic element. 
D) An ionic bond results when a nonmetallic elements gains an electron from a metallic element.

Question 10

Which of the following molecules contains an ionic bond?

Accepted Answer

A) MgCl2 
B) Cl2 
C) SF3 
D) Cl2O7 
E) none of the above 
A) MgCl2 
B) Cl2 
C) SF3 
D) Cl2O7 
E) none of the above

Question 11

What is the molecular shape of the following molecule?

Accepted Answer

A) pyramidal 
B) bent 
C) tetrahedral 
D) T-shaped 
E) linear 
A) pyramidal 
B) bent 
C) tetrahedral 
D) T-shaped 
E) linear

Question 12

Does an ionic bond have a dipole?

Accepted Answer

A) No, dipoles are only found in covalent compounds. 
B) No, but the electrical charges are relatively strong. 
C) Yes, the ionic bond is an example of a very strong dipole. 
D) Yes, but for ionic compounds they are referred to as monopoles. 
A) No, dipoles are only found in covalent compounds. 
B) No, but the electrical charges are relatively strong. 
C) Yes, the ionic bond is an example of a very strong dipole. 
D) Yes, but for ionic compounds they are referred to as monopoles.

Question 13

What molecule loses a proton to form the hydroxide ion, OH⁻?

Accepted Answer

A) The oxygen molecule,   
B) The water molecule,   O 
C) The hydrogen peroxide molecule,     
D) The hydrogen molecule,   
A) The oxygen molecule,   
B) The water molecule,   O 
C) The hydrogen peroxide molecule,     
D) The hydrogen molecule,

Question 14

If you mix a typical aluminum ion (Al, atomic no. = 13)with a typical oxygen ion (O, atomic no. = 8), what compound is formed?

Accepted Answer

A) Al2O3 
B) Al3O2 
C) Al13O8 
D) Al3O 
E) Al2O2 
A) Al2O3 
B) Al3O2 
C) Al13O8 
D) Al3O 
E) Al2O2

Question 15

Which of the following substances contains   ions?

Accepted Answer

A)    
B)    
C)    
D)    
E) all of the above 
A)    
B)    
C)    
D)    
E) all of the above

Question 16

Germanium chloride, Ge   , has only two atoms surrounding the central germanium atom. Why then is the germanium chloride molecule bent?

Accepted Answer

A) There is a covalent bond between the two chlorine atoms. 
B) A lone pair of electrons on germanium pushes it to this orientation. 
C) Lone pairs of electrons on the chlorine atoms push it to this orientation. 
D) It is bent only periodically as it swings between both bent and linear shapes. 
A) There is a covalent bond between the two chlorine atoms. 
B) A lone pair of electrons on germanium pushes it to this orientation. 
C) Lone pairs of electrons on the chlorine atoms push it to this orientation. 
D) It is bent only periodically as it swings between both bent and linear shapes.

Question 17

Electron dot structures are not so important for understanding ________.

Accepted Answer

A) ionic bonds 
B) metallic bonds 
C) covalent bonds 
D) polar covalent bonds 
A) ionic bonds 
B) metallic bonds 
C) covalent bonds 
D) polar covalent bonds

Question 18

How many valence electrons does gallium (Ga, atomic no. = 31)have?

Accepted Answer

A) 1 
B) 6 
C) 3 
D) 31 
E) 70 
A) 1 
B) 6 
C) 3 
D) 31 
E) 70

Question 19

Calcium fluoride, CaF2, is an example of ________.

Accepted Answer

A) an ionic compound 
B) a metallic compound 
C) a covalent compound 
D) a polar covalent compound 
A) an ionic compound 
B) a metallic compound 
C) a covalent compound 
D) a polar covalent compound

Question 20

How many covalent bonds would the following generic atom usually form?

Accepted Answer

A) 1 
B) 2 
C) 4 
D) 8 
E) would usually not form any covalent bonds 
A) 1 
B) 2 
C) 4 
D) 8 
E) would usually not form any covalent bonds

Which of the following describes the reason for the following application of metals? designer jewelry

Take money away from your bank account and the bank will show a negative credit. Take an electron away from an atom, however, and the atom shows up positive. Explain.

How do the electron-dot structures of elements in the same group in the periodic table compare with one another?

Which of the following compounds has polar covalent bonds?

Which of the above substances would have the largest dipole?

When is the geometry of a molecule not the same as its molecular shape?

A hydrogen atom does not form more than one covalent bond because it ________.

What is one role of unpaired valance electrons?

Atoms of nonmetallic elements form covalent bonds, but they can also form ionic bonds. How is this possible?

Which of the following molecules contains an ionic bond?

What is the molecular shape of the following molecule?

Does an ionic bond have a dipole?

What molecule loses a proton to form the hydroxide ion, OH⁻?

If you mix a typical aluminum ion (Al, atomic no. = 13)with a typical oxygen ion (O, atomic no. = 8), what compound is formed?

Which of the following substances contains ions?

Germanium chloride, Ge , has only two atoms surrounding the central germanium atom. Why then is the germanium chloride molecule bent?

Electron dot structures are not so important for understanding ________.

How many valence electrons does gallium (Ga, atomic no. = 31)have?

Calcium fluoride, CaF₂, is an example of ________.

How many covalent bonds would the following generic atom usually form?

About Science

Particles of Matter

Elements of Chemistry

Subatomic Particles

The Atomic Nucleus

How Molecules Mix

How Water Behaves

How Chemicals React

Acids and Bases in Our Environment

Oxidations and Reductions Charge the World

Organic Compounds

Nutrients of Life

Medicinal Chemistry

Optimizing Food Production

Protection Water and Air Resources

Capturing Energy

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Exam 6: How Atoms Bond

Which of the following describes the reason for the following application of metals? designer jewelry

Take money away from your bank account and the bank will show a negative credit. Take an electron away from an atom, however, and the atom shows up positive. Explain.

How do the electron-dot structures of elements in the same group in the periodic table compare with one another?

Which of the following compounds has polar covalent bonds?

Which of the above substances would have the largest dipole?

When is the geometry of a molecule not the same as its molecular shape?

A hydrogen atom does not form more than one covalent bond because it ________.

What is one role of unpaired valance electrons?

Atoms of nonmetallic elements form covalent bonds, but they can also form ionic bonds. How is this possible?

Which of the following molecules contains an ionic bond?

What is the molecular shape of the following molecule?

Does an ionic bond have a dipole?

What molecule loses a proton to form the hydroxide ion, OH⁻?

If you mix a typical aluminum ion (Al, atomic no. = 13)with a typical oxygen ion (O, atomic no. = 8), what compound is formed?

Which of the following substances contains ions?

Germanium chloride, Ge , has only two atoms surrounding the central germanium atom. Why then is the germanium chloride molecule bent?

Electron dot structures are not so important for understanding ________.

How many valence electrons does gallium (Ga, atomic no. = 31)have?

Calcium fluoride, CaF2, is an example of ________.

How many covalent bonds would the following generic atom usually form?

About Science

Particles of Matter

Elements of Chemistry

Subatomic Particles

The Atomic Nucleus

How Molecules Mix

How Water Behaves

How Chemicals React

Acids and Bases in Our Environment

Oxidations and Reductions Charge the World

Organic Compounds

Nutrients of Life

Medicinal Chemistry

Optimizing Food Production

Protection Water and Air Resources

Capturing Energy

Filters

Calcium fluoride, CaF₂, is an example of ________.