Question 1

A gemstone is an example of a ________.

Accepted Answer

A) pure material 
B) solid solution 
C) suspension 
D) saturated solution 
A) pure material 
B) solid solution 
C) suspension 
D) saturated solution B

Question 2

Account for the observation that ethyl alcohol,     OH, dissolves readily in water but dimethyl ether, C   OC   , which has the same number and kinds of atoms, does not.

Accepted Answer

A) The hydrogens on the dimethyl ether surround the molecule, shielding the inner atoms from interacting with the water. 
B) Because the carbons arrange themselves in a straight line, the ethanol can interact more easily with more water molecules, thus increasing its solubility. 
C) The high electronegativity of the carbon-oxygen-carbon bond on dimethyl ether creates a strong dipole charge on the ends of the molecule, making it highly soluble in water. 
D) Because dimethyl ether lacks an -OH group, it is significantly less polar than is ethyl alcohol and is not readily soluble in water. 
A) The hydrogens on the dimethyl ether surround the molecule, shielding the inner atoms from interacting with the water. 
B) Because the carbons arrange themselves in a straight line, the ethanol can interact more easily with more water molecules, thus increasing its solubility. 
C) The high electronegativity of the carbon-oxygen-carbon bond on dimethyl ether creates a strong dipole charge on the ends of the molecule, making it highly soluble in water. 
D) Because dimethyl ether lacks an -OH group, it is significantly less polar than is ethyl alcohol and is not readily soluble in water. D

Question 3

What is the purpose of adding aluminum salts and a base to water during water treatment?

Accepted Answer

A) The two together gel and trap dirt and bacteria. 
B) The higher pH kills bacteria. 
C) The aluminum removes the rust taste from the water 
D) The base dissolves the dirt. 
E) It improves the taste. 
A) The two together gel and trap dirt and bacteria. 
B) The higher pH kills bacteria. 
C) The aluminum removes the rust taste from the water 
D) The base dissolves the dirt. 
E) It improves the taste. A

Question 4

Which of the following statements about desalinization is untrue?

Accepted Answer

A) You can use osmosis to remove salt from saltwater. 
B) You can use distillation to separate salt from saltwater. 
C) Desalinization is an energy intensive process. 
D) All are untrue. 
E) Only a and b are untrue. 
A) You can use osmosis to remove salt from saltwater. 
B) You can use distillation to separate salt from saltwater. 
C) Desalinization is an energy intensive process. 
D) All are untrue. 
E) Only a and b are untrue.

Question 5

Which of the following would have the highest boiling point?

Accepted Answer

A) C6H14 
B) C8H18 
C) C10H22 
D) C12H26 
E) not enough information given 
A) C6H14 
B) C8H18 
C) C10H22 
D) C12H26 
E) not enough information given

Question 6

What property primarily determines the effect of temperature on the solubility of gas molecules?

Accepted Answer

A) the kinetic energy of the gas 
B) the polarity of the gas 
C) the molecular weight of the gas 
D) the ionic strength of the gas 
E) the dipole strength of the solvent 
A) the kinetic energy of the gas 
B) the polarity of the gas 
C) the molecular weight of the gas 
D) the ionic strength of the gas 
E) the dipole strength of the solvent

Question 7

If the solubility of a compound is 30 grams per liter, how much solid is left undissolved if you mix 30 g of the compound in 0.33 L of solution?

Accepted Answer

A) 20 g 
B) 10 g 
C) 0 g 
D) 30 g 
E) 33 g 
A) 20 g 
B) 10 g 
C) 0 g 
D) 30 g 
E) 33 g

Question 8

What would be a major advantage and a major disadvantage of desalinizing water by freezing?

Accepted Answer

A) The supply of ocean water is vast, but ocean water is too salty to make this method cost efficient. 
B) The supply of ocean water is vast, but this technique is limited to northern coastal regions. 
C) The supply of ocean water is vast, but time and energy is better spent hauling icebergs to coastal regions in need of fresh water. 
D) all of the above 
A) The supply of ocean water is vast, but ocean water is too salty to make this method cost efficient. 
B) The supply of ocean water is vast, but this technique is limited to northern coastal regions. 
C) The supply of ocean water is vast, but time and energy is better spent hauling icebergs to coastal regions in need of fresh water. 
D) all of the above

Question 9

Which of the following intermolecular forces best describes why molecules like CF3CF3 are soluble in liquid CO2?

Accepted Answer

A) dipole-dipole 
B) induced dipole-induced dipole 
C) dipole-induced dipole 
D) ion-dipole 
E) hydrogen bonding 
A) dipole-dipole 
B) induced dipole-induced dipole 
C) dipole-induced dipole 
D) ion-dipole 
E) hydrogen bonding

Question 10

How many moles of sugar, C12H22O11, are there in 200. grams?

Accepted Answer

A) 0.585 moles 
B) 68,400 moles 
C) 1.71 moles 
D) 0.684 moles 
A) 0.585 moles 
B) 68,400 moles 
C) 1.71 moles 
D) 0.684 moles

Question 11

Why aren't solar stills used in more large urban areas?

Accepted Answer

A) They take up too much space. 
B) They do not produce enough water. 
C) They require too much sunlight. 
D) They are not as efficient are reverse osmosis. 
E) all of the above 
A) They take up too much space. 
B) They do not produce enough water. 
C) They require too much sunlight. 
D) They are not as efficient are reverse osmosis. 
E) all of the above

Question 12

Which of the following is most likely to have the weakest induced dipole-induced dipole interaction?

Accepted Answer

A) Cl2 
B) Br2 
C) F2 
D) I2 
E) All of the above have the same interactions. 
A) Cl2 
B) Br2 
C) F2 
D) I2 
E) All of the above have the same interactions.

Question 13

Why are the melting temperatures of most ionic compounds far greater than the melting temperatures of most covalent compounds?

Accepted Answer

A) Ionic bonds are so much stronger than the intermolecular attractions between covalently bonded compounds. 
B) Covalent bonds are not as strong as ionic bonds. 
C) As a solid, salts have a very organized crystalline structure which takes a lot of energy to break apart. 
D) Most covalent compounds have at least one weak bond in their structure that is easily broken when heat is added. 
A) Ionic bonds are so much stronger than the intermolecular attractions between covalently bonded compounds. 
B) Covalent bonds are not as strong as ionic bonds. 
C) As a solid, salts have a very organized crystalline structure which takes a lot of energy to break apart. 
D) Most covalent compounds have at least one weak bond in their structure that is easily broken when heat is added.

Question 14

Which solute graphed above has a solubility in water that does not markedly increase with increasing temperature?

Accepted Answer

A) NaN   
B) LiCl 
C) KCl 
D) NaCl 
A) NaN   
B) LiCl 
C) KCl 
D) NaCl

Question 15

How does the purchase and use of a home beverage carbonator help to minimize carbon dioxide emissions?

Accepted Answer

A) It allows the consumer to avoid using commercial sodas that require much gasoline for shipping. 
B) Home carbonators are more efficient at forcing the carbon dioxide into solution. 
C) Industrial carbonators are driven by mechanical pumps that require large amounts of gasoline in order to operate. 
D) Home carbonators have the net effect of producing more carbon dioxide per liter of carbonate water. 
A) It allows the consumer to avoid using commercial sodas that require much gasoline for shipping. 
B) Home carbonators are more efficient at forcing the carbon dioxide into solution. 
C) Industrial carbonators are driven by mechanical pumps that require large amounts of gasoline in order to operate. 
D) Home carbonators have the net effect of producing more carbon dioxide per liter of carbonate water.

Question 16

Fluorine is a relatively ________.

Accepted Answer

A) large atom 
B) soft atom 
C) small atom 
D) greenish atom 
A) large atom 
B) soft atom 
C) small atom 
D) greenish atom

Question 17

A saturated solution of compound X in water has a greater concentration than does a saturated solution of compound Y. Does it follow that compound X is also more soluble in water?

Accepted Answer

A) No, the greater the concentration of a compound in water, the less soluble it is. 
B) Yes, compound X is more soluble than is compound Y because a greater concentration in water can be obtained. 
C) No, concentration of a solution is not correlated with how soluble that solution is in water. 
D) Since both solutions are saturated, it cannot be determined which compound has a greater solubility. 
A) No, the greater the concentration of a compound in water, the less soluble it is. 
B) Yes, compound X is more soluble than is compound Y because a greater concentration in water can be obtained. 
C) No, concentration of a solution is not correlated with how soluble that solution is in water. 
D) Since both solutions are saturated, it cannot be determined which compound has a greater solubility.

Question 18

Which of the following intermolecular forces best describes why nonpolar molecules like gasoline (C8H18)have only limited solubility in water?

Accepted Answer

A) dipole-dipole 
B) induced dipole-induced dipole 
C) dipole-induced dipole 
D) ion-dipole 
E) Both A and B 
A) dipole-dipole 
B) induced dipole-induced dipole 
C) dipole-induced dipole 
D) ion-dipole 
E) Both A and B

Question 19

Which of the following would have the smallest number of induced dipole-induced dipole interactions?

Accepted Answer

A) C6H14 
B) C8H18 
C) C10H22 
D) C12H26 
E) not enough information given 
A) C6H14 
B) C8H18 
C) C10H22 
D) C12H26 
E) not enough information given

Question 20

When you set a pot of tap water on the stove to boil, you'll often see bubbles start to form well before boiling temperature is ever reached. Explain this observation.

Accepted Answer

A) These are dissolved salts heating up and escaping from the water. 
B) These bubbles are formed as the surrounding gases from the air dissolve into the water as it is heated. 
C) They are very minute pockets of water in the gaseous phase. When they get large enough, the water will boil as this gas escapes. 
D) These initial bubbles are the gases that were dissolved in the water coming out of solution. The solubility of gases in water decreases with increasing temperature. 
A) These are dissolved salts heating up and escaping from the water. 
B) These bubbles are formed as the surrounding gases from the air dissolve into the water as it is heated. 
C) They are very minute pockets of water in the gaseous phase. When they get large enough, the water will boil as this gas escapes. 
D) These initial bubbles are the gases that were dissolved in the water coming out of solution. The solubility of gases in water decreases with increasing temperature.

A gemstone is an example of a ________.

Account for the observation that ethyl alcohol, OH, dissolves readily in water but dimethyl ether, C OC , which has the same number and kinds of atoms, does not.

What is the purpose of adding aluminum salts and a base to water during water treatment?

Which of the following statements about desalinization is untrue?

Which of the following would have the highest boiling point?

What property primarily determines the effect of temperature on the solubility of gas molecules?

If the solubility of a compound is 30 grams per liter, how much solid is left undissolved if you mix 30 g of the compound in 0.33 L of solution?

What would be a major advantage and a major disadvantage of desalinizing water by freezing?

Which of the following intermolecular forces best describes why molecules like CF₃CF₃ are soluble in liquid CO₂?

How many moles of sugar, C₁₂H₂₂O₁₁, are there in 200. grams?

Why aren't solar stills used in more large urban areas?

Which of the following is most likely to have the weakest induced dipole-induced dipole interaction?

Why are the melting temperatures of most ionic compounds far greater than the melting temperatures of most covalent compounds?

Which solute graphed above has a solubility in water that does not markedly increase with increasing temperature?

How does the purchase and use of a home beverage carbonator help to minimize carbon dioxide emissions?

Fluorine is a relatively ________.

A saturated solution of compound X in water has a greater concentration than does a saturated solution of compound Y. Does it follow that compound X is also more soluble in water?

Which of the following intermolecular forces best describes why nonpolar molecules like gasoline (C₈H₁₈)have only limited solubility in water?

Which of the following would have the smallest number of induced dipole-induced dipole interactions?

When you set a pot of tap water on the stove to boil, you'll often see bubbles start to form well before boiling temperature is ever reached. Explain this observation.

About Science

Particles of Matter

Elements of Chemistry

Subatomic Particles

The Atomic Nucleus

How Atoms Bond

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 7: How Molecules Mix

A gemstone is an example of a ________.

Account for the observation that ethyl alcohol, OH, dissolves readily in water but dimethyl ether, C OC , which has the same number and kinds of atoms, does not.

What is the purpose of adding aluminum salts and a base to water during water treatment?

Which of the following statements about desalinization is untrue?

Which of the following would have the highest boiling point?

What property primarily determines the effect of temperature on the solubility of gas molecules?

If the solubility of a compound is 30 grams per liter, how much solid is left undissolved if you mix 30 g of the compound in 0.33 L of solution?

What would be a major advantage and a major disadvantage of desalinizing water by freezing?

Which of the following intermolecular forces best describes why molecules like CF3CF3 are soluble in liquid CO2?

How many moles of sugar, C12H22O11, are there in 200. grams?

Why aren't solar stills used in more large urban areas?

Which of the following is most likely to have the weakest induced dipole-induced dipole interaction?

Why are the melting temperatures of most ionic compounds far greater than the melting temperatures of most covalent compounds?

Which solute graphed above has a solubility in water that does not markedly increase with increasing temperature?

How does the purchase and use of a home beverage carbonator help to minimize carbon dioxide emissions?

Fluorine is a relatively ________.

A saturated solution of compound X in water has a greater concentration than does a saturated solution of compound Y. Does it follow that compound X is also more soluble in water?

Which of the following intermolecular forces best describes why nonpolar molecules like gasoline (C8H18)have only limited solubility in water?

Which of the following would have the smallest number of induced dipole-induced dipole interactions?

When you set a pot of tap water on the stove to boil, you'll often see bubbles start to form well before boiling temperature is ever reached. Explain this observation.

About Science

Particles of Matter

Elements of Chemistry

Subatomic Particles

The Atomic Nucleus

How Atoms Bond

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

Which of the following intermolecular forces best describes why molecules like CF₃CF₃ are soluble in liquid CO₂?

How many moles of sugar, C₁₂H₂₂O₁₁, are there in 200. grams?

Which of the following intermolecular forces best describes why nonpolar molecules like gasoline (C₈H₁₈)have only limited solubility in water?