Chapter 7

What is the main difference between a dipole-dipole induced interaction and a dipole-induced dipole interaction?

A. both are similar, but one involves a temporary dipole created by a permanent dipole

If you need 3.01 x 10^23 molecules of sucrose, how many liters of a 4.00 molar solution would you need? a. 0.125 L b. 0.250 L c. 4.00 L d. 1.00 L

a. 0.125 L

Which of the following solutions is the most dilute? a. 1 L water with 1 gram sugar b. 1 L water with 2 grams sugar c. 1 L water with 5 grams sugar 1 L water with 10 grams sugar

a. 1 L water with 1 gram sugar

If you need 10 moles of sucrose, how many of liters of a 4.0 molar solution would you need? a. 2.5 L b. 0.25 L c. 25 L d. 10 L

a. 2.5 L

How many molecules of sucrose are in a 0.500 L of a 1.00 molar solution of sucrose?

a. 3.01 x 10^23 molecules of sucrose

If the solubility of a compound is 72 grams per liter at a given temp, how many grams of the compound with dissolve in 0.50 L at the same temp ? a. 36 g b. 72 g c. 144 g d. 30 g

a. 36 g

Which of the following is most likely to show a dipole-dipole interaction? a. CH3OH b. CH3SH c. CH4 d. H-C-C-H e. A and B

a. CH3OH

Which would you expect to be most strongly attracted to a Cl- ion? a. H-F b. H3CCH3 c. Cl-Cl d. F-F e. CCl4

a. H-F

Hydrogen chloride, HCL is a gas at room temp. would you expect it to be very soluble or not very soluble in water? a. HCL is very soluble in water because of the dipole-dipole attractions b. it is not very solubility because it is a gas c. HCL very soluble because it is so small d. it is not very soluble because it has low density and it floats to the surface and then into the atmosphere

a. HCL is very soluble in water because of the dipole-dipole attractions

The separation of charges within a polar molecule is called a. dipole b. dipole-dipole c. ionic bond d. strong attraction

a. dipole

If you were to increase the pressure of gas above a liquid what happens? a. gas is forced into solution increasing solubility b. solution is compressed and gas is forced out of the solvent c. pressure goes down and gas moves out of solvent d. pressure goes down and gas goes into solvent e. amount of gas in solution stays the same

a. gas is forced into solution and the solubility increases

If an ionic bond is stronger than a dipole-dipole interaction, how can water dissolve an ionic compound? a. ion-dipole interactions of a bunch of water molecules gang up on the bond and pull it into the solution b. ionic bond is weakened by the ion-dipole interactions c. ion-dipole interaction causes ions to heat up and vibrate free d. ions never overcome their interatomic attraction and are not soluble

a. ion-dipole interactions of a bunch of water molecules gang up on the bond and pull it into the solution

Why are the melting temps of most ionic compounds far greater than the melting temps of most covalent compounds? a. ionic bonds are much stronger than the intermolecular attractions between covalently bonded compounds b. covalent bonds are not as strong c. as a solid, salts have a crystalline structure that is hard to break apart d. most covalent compounds have at least one weak bond in their structure that is easily broken when heated

a. ionic bonds are much stronger than the intermolecular attractions between covalently bonded compounds

What property determines the effect of temperature on the solubility of gas molecules? a. kinetic energy of gas b. polarity of gas c. molecular weight of gas d. ionic strength of gas

a. kinetic energy

Red blood cells have a high concentration of dissolved ions. When placed into pure water, they rupture. Why? a. osmosis draws water back into cell until it pops b. water dissolves the cell membrane c. osmosis draws water out of the cell until it tears d. cells aren't stable outside of their biological host

a. osmosis draws water into the cell until it pops

dipole is a a. separation of charges b. molecule with parallel bonds c. nonpolar entity d. form of electronegativity

a. separation of charges

How are intermolecular forces of solubility related?

a. solubility depends on the solvent's ability to overcome the intermolecular forces in a solid

What is a hydrogen bond? a. special dipole-dipole attraction with a hydrogen bound to a highly electronegative atom b. special dipole-dipole with hydrogen bound to another atom c. special dipole-dipole attraction involving hydrogen bound to another hydrogen d. special type of attraction involving any molecules that contain hydrogens

a. special dipole-dipole attraction with a hydrogen bound to a highly electronegative atom

Which of the following accurately describes osmosis?

a. the more concentrated solution absorbs water from the less concentrated solution

What happens if you were to place a dilute solution that is in a bag made of semipermeable membrane and were to then suspend it in a very concentrated solution?

a. the size of the suspended bag would decrease

During osmosis

a. the water moves into the concentration solution faster then it leaves

A solid has a solubility at room temp of 78 g per liter. If 1.0 L of a heated solution containing 100 g of solute is cooled to room temp, how much solid is formed? a. 100 g b. 22 g c. 78 g d. 1 L

b. 22 g

what is the molarity when water is added to 2 moles of NaCL to make a 0.5L solution?

b. 4 M

How many molecules of sucrose are in o.500L of a 2.00 molar solution of sucrose? a. 3.01 X10^23 b. 6.02 x 10^23 c. 12.04 x 10^23 1 gram

b. 6.02 x 10^23 molecules of sucrose

Which of the following would you expect to be lease attracted to the Na+ ion? a. H-F b. H3CCH3 c. Cl2CH2 d. F- e. HO-

b. H3CCH3

What happens if you were to place a concentrated solution into a bag made of a semipermeable membrane and were to then suspend it in a very dilute solution?

b. Size of the suspended bag would increase

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? a. No, greater concentration means its not soluble b. Yes, X is more soluble because a greater concentration in water can be attained c. No, concentration of a solution is not correlated to solubility in water d. since both are saturated, it can't be determined

b. Yes, X is more soluble because a greater concentration in water can be attained

Chlorine is a gas at room temp, but bromine is a liquid. Explain. a. Cl atoms are larger and it forms dipole-induced-dipole attractions b. bromine atoms are larger and this makes the formation of dipole-induced dipole attractions more favorable c. smaller Cl molecules are able to pack together in a tighter physical orientation d. bromine ions are held together by ionic bonds

b. bromine atoms are larger and this makes the formation of dipole-induced dipole attractions more favorable

Hard water contains excessive amounts of a. chlorine ions b. calcium ions c. hydrogen ions d. hydroxide ions

b. calcium ions

Treating water with chlorine or ozone during water purification is an example of a. physical change b. chemical reaction c. ion exchange d. solid dissolving in a liquid

b. chemical reaction

An inventor claims to have developed a new perfume that lasts a long time because it doesn't evaporate. Comment on this claim. a. perfume that doesn't evaporate could be toxic b. in order to smell, molecules must evaporate and reach your nose. this perfume wouldn't have an odor c. this would be impossible to make since you'd have to pressurize it d. this product is sure to sweep the market

b. in order to smell, molecules must evaporate and reach your nose. this perfume wouldn't have an odor

Which of the following is the strongest form of interatomic attraction? a. chemical bond b. ion-dipole c. dipole-dipole d. dipole-induced dipole e. an induced dipole-induced interatcion

b. ion-dipole

which of the following describes the term concentration?

b. it is the amount of solute in a given amount of solution

under which of the following conditions would you expect the highest solubility of a oxygen gas in water?

b. low temp and high pressure above the solution

Is a solution of 77% nitrogen iand 23% oxygen, which is the solvent? a. oxygen b. nitrogen c. both d. neither e. gases cannot form solutions

b. nitrogen

why are ion-dipole attractions stronger than dipole-dipole attractions?

b. the magnitude of the electric charge associated with an ion is much greater

Cells at the top of a tree have a higher concentration of sugars than cells at the bottom. How might this fact assist a tree in moving water upward from its roots? a. cells with high sugar are more dense. the cells migrate downwards and cells with fresh water move up b. water is pushed up by osmotic pressure c. it doesnt. water makes it to the top because thats where the molecules evaporate d. fresh water is drawn up to the sugar cells through dipole-dipole attractions

b. water is pushed up by osmotic pressure

Which of the following is the most concentrated? a. 0.1 L water 1 gram sugar b. 2 L water 0.2 gram sugar c. 0.5 L water with 50 grams sugar d. 3 L water with 30 grams sugar e. all have the same concentration

c. 0.5 L water with 50 grams sugar

How many moles of sugar C12H22O11 are there in 200 grams? a. 1.00 moles b. 68,400 moles c. 0.585 moles d. 0.684 moles

c. 0.585 moles

How many grams of sugar are there in 5.0 liters of sugar water that has a concentration of 0.50 grams per liter of solution? a. 50 g b. 25 g c. 2.5 g d. 1.5 g

c. 2.5 g

Which of the following would have the lowest melting point? a. CCl4 b. CBr4 c. CF4 d. Cl4 e. not enough info given

c. CF4

Which of the following is the most likely to have the weakest induced dipole-induced interaction? a. Cl2 b. Br2 c. F2 d. I2 e. all have the same

c. F2

A student is told to use 10 g of NaCl to make an aqueous solution that has a concentration of 1.00 grams NaCl per liter. How much water will she use in making this solution? a. much more than 10 L b. exactly 10 L c. slightly less than 10 L d. 1 L

c. slightly less than 10 L

Fluroine is relatively a. large b. soft c. small d. greenish

c. small

Why is the surface are of a gecko's foot so extensive?

c. the greater the surface area the greater the number of induced dipole-induced forces of attraction that can occur between the gecko's foot and the surface

What is happening at the molecular level when a polar molecule like water interacts with a typical sodium ion?

c. the water molecule aligns such that the oxygen interacts with the sodium

If the solubility of a compound is 30 g/ L, how much solid is left undissolved if you mix 30 g of the compound in 0.33 L of solution? a. 5 g b. 10 g c. 20 g d. 30 g

d. 20 g

How many grams of sodium chloride are needed to make 15 L of a solution that has a concentration of 3.0 g per liter of solution? a. 30 g b. 141 g c. 5 g d. 45 g

d. 45 g

How many moles of water are there in 100 g of water? a. 1800 b. 100 c. 0.018 d. 5.55

d. 5.55

How can you tell if a sugar solution is saturated?

d. Add more sugar. If it does not dissolve after mixing, the solution is saturated.

Which of the following would have the highest boiling poing? a. C6H14 b. C8H18 c. C10H22 d. C12H26

d. C12H26

which of the following might have the lowest solubility in water? a. CH3OH b. Cl2 c. O2 d. CH3CH3 e. none of the above

d. CH3CH3

which of the following would have the highest boiling point? a. Cl2 b. Br2 c. F2 d. I2 e. not enough info

d. I2

What statement best describes a mole? a. a little furry animal in the ground b. very small number chemists use to count atoms c. amount of molecules or atoms in 1 gram of something d. a very large number chemists use to count atoms

d. a very large number chemists use to count atoms

Which has the most atoms? a. mole of gold b. mole of helium c. mole of lead d. all have the same number of atoms

d. all have the same number of atoms

In which of the following molecules will water induce a temporary dipole? a. CO2 b. O2 c. N2 d. all of them e. none of them

d. all of them

How is the solubility of a gas affected by temperature? a. depends on the gas b. as temp down, solubility down c. as temp up, solubility up d. as temp down, solubility up

d. as temp down, solubility up

Account for the observation that ethyl alcohol, C2H5OH, dissolves readily in water but dimethyl ether C2H5O, which has the same number and kinds of atoms, does not.

d. because dimethyl ether lacks an OH group, it is much less polar than ethyl alcohol and is not readily soluble in water

Fish don't live very long in water that has just been boiled and brought down to room tamp. Suggest why. a. now more Co2 b. nutrients destroyed c. since some water evaporated, salt is more concentrated and negatively affects fish d. boiling process removes the air that was dissolved in the water. Upon cooling, water is void of its usual air content and fish drown

d. boiling process removes the air that was dissolved in the water. Upon cooling, water is void of its usual air content and fish drown

What is molarity? a. number of grams of solute per liter of solution b. number of moles of solute per liter of solvent c. number of liters of solute per mole of solution d. number of moles of solute per liter of solution

d. number of moles of solute per liter of solution

What is the difference between a dipole-dipole interaction and an ion-dipole interaction? a. one involves hydrogen bonding b. one involves salts and water and the other has no water c. one involves ionic molecules and the other has polar d. one has dipole attraction between molecules while the other involves dipole interactions between molecules and ions

d. one has dipole attraction between molecules while the other involves dipole interactions between molecules and ions

Would you expect to find more dissolved oxygen in polar or tropical ocean waters? Why?

d. there would be more dissolved oxygen in the polar oceans because the solubility of oxygen in water decreases with increasing temperature

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.

d. these initial bubbles are gases that were dissolved in the water coming out of solution. The solubility of gases in water decreases with increasing temperature

How is the solubility of a solid affected by temperature? a. as temperature goes up, solubility goes up b. as temperature goes down, solubility goes down c. as temperature goes up, solubility goes down d. as temperature goes down, solubility goes up e. depends on the solid

e. depends on the solid

Which is the most dilute? a. 0.1 L of water with 1 gram sugar b. 0.2 L water with 2 gram sugar c. 0.5 L with 5 gram sugar d. 1 L water with 10 grams sugar e. all the same concentration

e. they all have the same concentration