Slide 1 / 42 1 In a single molecule of water, the two hydrogen atoms are bonded to a single oxygen atom by A hydrogen bonds. B nonpolar covalent bonds. C polar covalent bonds. D ionic bonds. E van der Waals interactions.
Slide 2 / 42 2 The slight negative charge at one end of one water molecule is attracted to the slight positive charge of another water molecule. What is this attraction called? A a covalent bond B a hydrogen bond C an ionic bond D a hydrophilic bond E a hydrophobic bond
Slide 3 / 42 3 An example of a hydrogen bond is the bond between A C and H in methane (CH 4 ). the H of one water molecule and the B O of another water molecule. Na + and Cl - in salt. C the two hydrogen atoms in a molecule D of hydrogen gas (H 2 ). Mg + and Cl - in MgCl 2 . E
Slide 4 / 42 4 Water is able to form hydrogen bonds because A oxygen has a valence of 2. the water molecule is shaped like a B tetrahedron. the bonds that hold together the C atoms in a water molecule are polar covalent bonds. the oxygen atom in a water molecule D has a weak positive charge. each of the hydrogen atoms in a E water molecule is weakly negative in charge.
Slide 5 / 42 5 What determines the cohesiveness of water molecules? A hydrophobic interactions B nonpolar covalent bonds C ionic bonds D hydrogen bonds E both A and C
Slide 6 / 42 6 What do cohesion, surface tension, and adhesion have in common with reference to water? All increase when temperature A increases. B All are produced by ionic bonding. All are properties related to C hydrogen bonding. All have to do with nonpolar covalent D bonds. E C and D only
Slide 7 / 42 7 Which of the following is possible due to the high surface tension of water? Lakes don't freeze solid in winter, A despite low temperatures. A water strider can walk across the B surface of a small pond. Organisms resist temperature C changes, although they give off heat due to chemical reactions. D Water can act as a solvent. The pH of water remains exactly E neutral.
Slide 8 / 42 8 Which of the following is true when an ice cube cools a drink? Molecule collisions in the drink A increase. Kinetic energy in the drink B decreases. A calorie of heat energy is C transferred from the ice to the water of the drink. The specific heat of the water in the D drink decreases. Evaporation of the water in the drink E increases.
Slide 9 / 42 9 Water's high specific heat is mainly a consequence of the A small size of the water molecules. high specific heat of oxygen and B hydrogen atoms. absorption and release of heat when C hydrogen bonds break and form. fact that water is a poor heat D conductor. inability of water to dissipate heat E into dry air.
Slide 10 / 42 10 Which bonds must be broken for water to vaporize? A ionic bonds B nonpolar covalent bonds C polar covalent bonds D hydrogen bonds E covalent bonds
Slide 11 / 42 11 Ice is lighter and floats in water because it is a crystalline structure in which each water molecule is bonded to a maximum of four other water molecules by which kind of bond? A ionic B hydrogen C covalent D A and C only E A, B, and C
Slide 12 / 42 12 Why does ice float in liquid water? The liquid water molecules have A more kinetic energy and thus support the ice. The ionic bonds between the B molecules in ice prevent the ice from sinking. Ice always has air bubbles that keep C it afloat. Hydrogen bonds stabilize and keep the molecules of ice farther apart D than the water molecules of liquid water. The crystalline lattice of ice causes it E to be denser than liquid water.
Slide 13 / 42 13 Based on your knowledge of the polarity of water molecules, the solute molecule in the center of the diagram is most likely A positively charged. negatively charged. B C without charge. D hydrophobic. E nonpolar.
Slide 14 / 42 14 Hydrophobic substances such as vegetable oil are nonpolar substances that repel water A molecules. nonpolar substances that have an B attraction for water molecules. polar substances that repel water C molecules. polar substances that have an affinity D for water. charged molecules that hydrogen- E bond with water molecules.
Slide 15 / 42 15 One mole (mol) of a substance is 6.02 × 10 23 molecules of the A substance. 1 g of the substance dissolved in 1 L B of solution. t he largest amount of the substance C that can be dissolved in 1 L of solution. the molecular mass of the substance D expressed in grams. E A and D only
Slide 16 / 42 16 How many molecules of glucose (C 6 H 12 O 6 molecular mass =180 amu) would be present in one mole of glucose? A 24 B 342 23 × 10 14 C 180 × 10 14 D 6.02 × 10 23 E
Slide 17 / 42 17 How many molecules of glycerol (C 3 H 8 O 3 ) would be present in 1 L of a 1 M glycerol solution? A 1 B 14 C 92 D 1 × 10 7 6.02 × 10 23 E
Slide 18 / 42 18 Recall that when sodium chloride (NaCl) is placed in water the component atoms of the NaCl crystal dissociate into individual sodium ions (Na+) and chloride ions (Cl - ). In contrast, the atoms of covalently bonded molecules (e.g., glucose, sucrose, glycerol) do not generally dissociate when placed in aqueous solution. Which of the following solutions would be expected to contain the greatest concentration of particles (molecules or ions)? 0.5 M NaCl A 0.5 M glucose B 1.0 M NaCl C 1.0 M glucose D 1.0 M MgCl 2 E
Slide 19 / 42 19 When sodium chloride (NaCl) is placed in water the component atoms of the NaCl crystal dissociate into individual sodium ions (Na + ) and chloride ions (Cl - ). In contrast, the atoms of covalently bonded molecules (e.g., glucose, sucrose, glycerol) do not generally dissociate when placed in aqueous solution. Which of the following solutions would be expected to contain the greatest number of particles (molecules or ions)? A 1 L of 0.5 M NaCl B 1 L 0.5 M glucose C 1 L of 1.0 M NaCl D 1 L of 1.0 M glucose E C and D only
Slide 20 / 42 20 How many grams of the molecule in the figure would be equal to 1 mol of the molecule? (Carbon = 12, Oxygen = 16, Hydrogen = 1) A 29 B 30 C 60 D 150 E 342
Slide 21 / 42 21 Which of the following ionizes completely in solution and is considered to be a strong acid? A NaOH B HCl C NH 3 D H 2 CO 3 E CH 3 COOH
Slide 22 / 42 22 Which of the following ionizes completely in solution and is considered to be a strong base? A NaCl B HCl C NH 3 H 2 CO 3 D E NaOH
Slide 23 / 42 23 A given solution contains 0.0001(10 -4 ) moles of hydrogen ions [H + ] per liter. Which of the following best describes this solution? acidic: H + acceptor A basic: H + acceptor B acidic: H + donor C basic: H + donor D E neutral
Slide 24 / 42 24 A solution contains 0.0000001(10 -7 ) moles of hydroxide ions [OH - ] per liter. Which of the following best describes this solution? acidic: H + acceptor A basic: H + acceptor B acidic: H + donor C basic: H + donor D E neutral
Slide 25 / 42 25 What would be the pH of a solution with a hydroxide ion [OH - ] concentration of 10 -12 M? A pH 2 B pH 4 C pH 10 D pH 12 E pH 14
Slide 26 / 42 26 What would be the pH of a solution with a hydrogen ion [H + ] concentration of 10 -8 M? A pH 2 B pH 4 C pH 6 D pH 8 E pH 10
Slide 27 / 42 27 Which of the following solutions has the greatest concentration of hydrogen ions [H + ]? A gastric juice at pH 2 B vinegar at pH 3 C tomato juice at pH 4 D black coffee at pH 5 E household bleach at pH 12
Slide 28 / 42 28 Which of the following solutions has the greatest concentration of hydroxide ions [OH - ]? A lemon juice at pH 2 B vinegar at pH 3 C tomato juice at pH 4 D urine at pH 6 E seawater at pH 8
Slide 29 / 42 29 If the pH of a solution is decreased from 9 to 8, it means that the concentration of H + has decreased A 10 times what it was at pH 9. concentration of H + has increased 10 B times what it was at pH 9. concentration of OH - has increased C 10 times what it was at pH 9. concentration of OH - has decreased D 10 times what it was at pH 9. E B and D are correct.
Slide 30 / 42 30 If the pH of a solution is increased from pH 5 to pH 7, it means that the concentration of H + is 2 times greater A than what it was at pH 5. concentration of H + is 2 times less B than what it was at pH 5. concentration of OH - is 100 times C greater than what it was at pH 5. concentration of OH - is 100 times less D than what it was at pH 5. concentration of H + is 100 times greater and the concentration of OH- E is 100 times less than what they were at pH 5.
Slide 31 / 42 31 One liter of a solution of pH 2 has how many more hydrogen ions (H + ) than 1 L of a solution of pH 6? A 4 times more B 400 times more C 4,000 times more D 10,000 times more E 100,000 times more
Slide 32 / 42 32 One liter of a solution pH 9 has how many more hydroxide ions (OH - ) than 1 L of a solution of pH 4? A 5 times more B 100 times more C 1,000 times more D 10,000 times more E 100,000 times more
Recommend
More recommend
