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53 Cards in this Set
- Front
- Back
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If you need 10. Moles of sucrose, how many liters of 4.0 molar solution would you need? |
2.5L |
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The separation of charges within a polar molecule is called |
Dipole |
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If an ionic bond is stronger than a dipole-dipole interaction, how can water dissolve an ionic compound? |
The ion-dipole interaction of a bunch of water molecules gang up on the strong ionic bond and pull it into the solution. |
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Account for the observation that ethyl alcohol dissolves readily in water but dimethyl ether, which has the same number and kinds of atoms does not |
Because dimethyl ether lacks -OH group, it is significantly less polar than is ethyl alcohol and is not readily soluble in water. |
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If you were to increase the pressure of gas above a liquid (such as by pressing a piston above a liquid) what happens? |
The gas is forced into solution and solubility increases. |
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Which of the following would have the weakest indices dipole-indices dipole interactions? |
C6H14 |
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Under which of the following conditions would you expect the highest solubility of oxygen? |
Low temperature and high pressure above the solution |
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A student is told to use 10 grams of sodium chloride to make an aqueous solution that has a concentration of 1 grams of sodium chloride per liter of solution. How much water will she use in making this solution? |
Slightly less than 10 L |
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How many molecules of sucrose are in 0.500L of a 1.00 molar solution of sucrose? |
3.01 x 10 to the 23 |
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Which of the following is the strongest form of intermolecular attraction? |
An ion-dipole interaction |
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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. |
These initial bubbles are the gases that were dissolved in the water coming out of solution. The solubility of gasses decreases with increasing temperature. |
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A solid has a solubility at room temperature of 78 grams per liter. If 1.0 L of heated solution containing 100. g of solute is cooled to room temperature, how much solid is formed? |
22g |
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Why are the melting temperatures of most ionic compounds far greater than the melting temperatures of most covalent compounds? |
Ionic bonds are so much stronger than the intermolecular attractions between covalently bonded compounds. |
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What is a hydrogen bond? |
A special type of dipole-dipole attraction involving hydrogen bound to a highly electronegative atom. |
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How many molecules of sucrose are in 0.500 moles of sucrose? |
3.01 x 10 to the 23rd molecules of sucrose |
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Fish don't live very love in water that has been boiled and brought back to room temperature. Suggest why. |
The boiling process removes most of the air that was dissolved in the water. Upon cooling, the water is void of its usual air content, hence, the fish drown. |
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Fluorine is a relatively........... |
Small atom |
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What is the molarity of 0.50 liters of a solution with five moles of sucrose in it? |
10 molar |
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How is the solubility of a gas affected by temperature? |
As temperature goes down, the solubility goes up |
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Which of the following is mostly likely to show a dipole-dipole interaction? |
SO2 |
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How are intermolecular forces and solubility related? |
Solubility depend on the solvent's ability to overcome the intermolecular forces in a solid. |
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Which of the following is most likely to show a hydrogen bonding interaction? |
A |
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Chlorine is a gas at room temperature, but bromine is a liquid. Explain. |
Bromine atoms are larger and this makes formation of induced dipole-induced dipole attractions more favorable. |
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A dipole is a..... |
A separation of charges |
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A soap molecule is.... |
A molecule with both polar and non polar parts |
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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? |
The size of the suspended bag would decrease. |
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Why might a solvent like turpentine be better for neocolonial grease and grime than water? |
All of the above |
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How is the solubility of a solid affected by temperature? |
It depends on the solid. |
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Describe what usually happens to a hot solution that is saturated with a solid as it cools. |
Some of the solid comes out of the solution |
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How many moles of water are there in 100 grams of water? |
0.018 moles |
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Which of the following wound have the highest boiling point? |
Last answer |
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Which is the following molecules is most likely to show a dipole-dipole interaction? |
CH4 |
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Which of the following would you expect to be the least attracted to a NA+ ion? |
H3C-CH3 |
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Which of the following would you expect to be the least attracted to a NA+ ion? |
H3C-CH3 |
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A sample of steel is composed of 5 percent carbon and 95% iron. Which is the solvent? |
Iron |
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What is the different between a dipole-dipole interaction and an ion-dipole interaction? |
One involved dipole attraction between molecules while the other involves dipole interaction between molecules and ions. |
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Which of the following molecules would you expect to be most strongly attracted to a Cl- ion? |
H-F |
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If the solubility of a compound is 30 grams per liter, how much solid is left undissolved if you mix 30g of the compound in 0.33 L of solution? |
20 g |
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Does a plastic bottle of fresh water sink or float in the ocean? Why? |
Floats; the bottle filled with fresh water floats in ocean water because it is less dense than ocean water. |
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Which of the following might have the lowest solubility in water? |
CH3CH3 |
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What is the main difference between a dipole-dipole interaction and a dipole-induced dipole interaction? |
Both are similar but one involves a temporary dipole created by a permanent dipole. |
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Which of the following would have the lowest melting point? |
CF4 |
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Which of the following accurately describes osmosis? |
The more concentrated solution absorbs water from the less concentrated solution |
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Which of the following describes an aqueous solution? |
A mixture of some compound dissolved in water |
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How many grams of sugar are there in 5.0 liters of sugar water that has a concentration of .50 grams per liter of solution? |
2.5 g |
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What is the formula to figure out the molarity of a solution? |
Number of moles of solute divided by liters of solution |
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A mole of something is how many? |
6.02x10 to the 23 |
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What is the formula to figure out the concentration of something? |
Amount of solute divided by the amount of solution. |
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What is the formula to figure out the amount of solute? |
Concentration of solution x volume of solution |
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What is the formula to figure out the amount of solute? |
Concentration of solution x volume of solution |
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What is the formula to figure out the volume of a solution? |
Amount of solute divided by the concentration of solution |
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What is the formula to figure out the amount of solute? |
Concentration of solution x volume of solution |
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What is the formula to figure out the volume of a solution? |
Amount of solute divided by the concentration of solution |
