Question 1

How are the hydrogen bonds formed between water molecules?

Accepted Answer

A)  by the attraction between the positive end of one water molecule with the negative end of the other 
B)  by sharing of electrons between two water molecules 
C)  by the transfer of electrons from one water molecule to the other 
D)  by sharing protons between two water molecules 
A)  by the attraction between the positive end of one water molecule with the negative end of the other 
B)  by sharing of electrons between two water molecules 
C)  by the transfer of electrons from one water molecule to the other 
D)  by sharing protons between two water molecules

Question 2

Sulfur is in the same column of the periodic table as oxygen but it is less electronegative than oxygen. Compared to water molecules, how will the H2S molecules behave?

Accepted Answer

A)  have greater cohesion to other H2S molecules 
B)  have a greater tendency to form hydrogen bonds with each other 
C)  have a higher capacity to absorb heat for the same change in temperature 
D)  not be able to form hydrogen bonds with each other 
A)  have greater cohesion to other H2S molecules 
B)  have a greater tendency to form hydrogen bonds with each other 
C)  have a higher capacity to absorb heat for the same change in temperature 
D)  not be able to form hydrogen bonds with each other

Question 3

When carbon dioxide in the atmosphere dissolves with the raindrops, what is the expected change in pH of the raindrops?

Accepted Answer

A)  slightly acidic 
B)  slightly basic 
C)  same as pure water 
D)  depends on the altitude where rain drops are formed 
A)  slightly acidic 
B)  slightly basic 
C)  same as pure water 
D)  depends on the altitude where rain drops are formed

Question 4

A solution of pH 7 is ________ than a solution of pH 8.

Accepted Answer

A)  100% less acidic 
B)  100% more acidic 
C)  twice as acidic 
D)  ten times as acidic 
A)  100% less acidic 
B)  100% more acidic 
C)  twice as acidic 
D)  ten times as acidic

Question 5

Dilution of a buffer solution with a small amount of water will ________ the pH of the solution.

Accepted Answer

A)  raise 
B)  lower 
C)  not bring major change in 
D)  immediately raise then lower 
A)  raise 
B)  lower 
C)  not bring major change in 
D)  immediately raise then lower

Question 6

What kind of bond is formed between the two hydrogen atoms and the single oxygen atom?

Accepted Answer

A)  hydrogen bonds 
B)  nonpolar covalent bonds 
C)  polar covalent bonds 
D)  ionic bonds 
A)  hydrogen bonds 
B)  nonpolar covalent bonds 
C)  polar covalent bonds 
D)  ionic bonds

Question 7

Which of the following is NOT impacted by the acidification of ocean water?

Accepted Answer

A)  Mollusk shells 
B)  Coral reef 
C)  Tiger shark teeth 
D)  Diatom shells 
A)  Mollusk shells 
B)  Coral reef 
C)  Tiger shark teeth 
D)  Diatom shells

Question 8

On a hot day, temperature of land rises more quickly than that of sea. Which of the following statements best describe the process?

Accepted Answer

A)  specific heat of soil is less than water 
B)  specific heat of soil is more than water 
C)  It rains more over the sea. 
D)  Dry soil soaks more water. 
A)  specific heat of soil is less than water 
B)  specific heat of soil is more than water 
C)  It rains more over the sea. 
D)  Dry soil soaks more water.

Question 9

Which of the following is a hydrophobic material?

Accepted Answer

A)  paper 
B)  table salt 
C)  wax 
D)  sugar 
A)  paper 
B)  table salt 
C)  wax 
D)  sugar

Question 10

What is the hydroxide ion concentration of the lake described in question 3?

Accepted Answer

A)  10-10M 
B)  10-4M 
C)  10-7M 
D)  10.0M 
A)  10-10M 
B)  10-4M 
C)  10-7M 
D)  10.0M

Question 11

A slice of pizza has 500 kcal. If we could burn the pizza and use all the heat to warm a 50-L container of cold water, what would be the approximate increase in the temperature of the water? (Note: A liter of cold water weighs about 1 kg.)

Accepted Answer

A)  50°C 
B)  5°C 
C)  100°C 
D)  10°C 
A)  50°C 
B)  5°C 
C)  100°C 
D)  10°C

Question 12

Rank, from low to high, the pH of blood, stomach acid, and urine.

Accepted Answer

A)  blood, urine, and stomach acid 
B)  stomach acid, blood, and urine 
C)  urine, blood, stomach acid 
D)  stomach acid, urine, blood 
A)  blood, urine, and stomach acid 
B)  stomach acid, blood, and urine 
C)  urine, blood, stomach acid 
D)  stomach acid, urine, blood

Question 13

0.660 moles of NaCl are dissolved in 95.0 mL of water. Calculate the molarity of the NaCl solution.

Accepted Answer

A)  62.7 M 
B)  0.069 M 
C)  0.0069 M 
D)  6.95 M 
A)  62.7 M 
B)  0.069 M 
C)  0.0069 M 
D)  6.95 M

Question 14

How many grams of the compound in the figure are required to make 1 liter of a 0.5 M solution? (Note: The atomic masses, in daltons, are approximately 12 for carbon, 1 for hydrogen.)

Accepted Answer

A)  39 
B)  72 
C)  78 
D)  156 
A)  39 
B)  72 
C)  78 
D)  156

Question 15

We can be sure that a mole of table sugar and a mole of vitamin C are equal in their ________.

Accepted Answer

A)  mass 
B)  volume 
C)  number of atoms 
D)  number of molecules 
A)  mass 
B)  volume 
C)  number of atoms 
D)  number of molecules

Question 16

When an ionic compound such as 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 solute particles (molecules or ions)?

Accepted Answer

A)  1 liter of 0.5 M NaCl 
B)  1 liter of 1.0 M NaCl 
C)  1 liter of 1.0 M glucose 
D)  1 liter of 1.0 M NaCl and 1 liter of 1.0 M glucose will contain equal numbers of solute particles. 
A)  1 liter of 0.5 M NaCl 
B)  1 liter of 1.0 M NaCl 
C)  1 liter of 1.0 M glucose 
D)  1 liter of 1.0 M NaCl and 1 liter of 1.0 M glucose will contain equal numbers of solute particles.

Question 17

Identical heat lamps are arranged to shine on two identical containers, one containing water and one methanol (wood alcohol), so that each liquid absorbs the same amount of energy minute by minute. The covalent bonds of methanol molecules are nonpolar, so there are no hydrogen bonds among methanol molecules. Which of the following graphs correctly describes what will happen to the temperature of the water and the methanol?

Accepted Answer

A) 
  
B) 
  
C) 
  
D) 
  
A) 
  
B) 
  
C) 
  
D)

Question 18

Rubbing alcohol swab on the skin feels cool because ________.

Accepted Answer

A)  liquid alcohol transfers cold temperature to the skin 
B)  the density of alcohol is less than water 
C)  alcohol destroys skin microorganisms and they give off cold heat as they die 
D)  skin transfers heat to the liquid alcohol and the alcohol evaporates 
A)  liquid alcohol transfers cold temperature to the skin 
B)  the density of alcohol is less than water 
C)  alcohol destroys skin microorganisms and they give off cold heat as they die 
D)  skin transfers heat to the liquid alcohol and the alcohol evaporates

Question 19

What kind of bonds are responsible for the unique cohesion, surface tension, and adhesion properties of water molecules?

Accepted Answer

A)  hydrophobic bonding 
B)  ionic bonding 
C)  hydrogen bonding 
D)  polar covalent bonding 
A)  hydrophobic bonding 
B)  ionic bonding 
C)  hydrogen bonding 
D)  polar covalent bonding

Question 20

What is the concentration of hydroxide ions in a solution of pH 5?

Accepted Answer

A)  10-9 M 
B)  10-5 M 
C)  10-12 M 
D)  10-10 M 
A)  10-9 M 
B)  10-5 M 
C)  10-12 M 
D)  10-10 M

Exam 3: The Chemistry of Water

How are the hydrogen bonds formed between water molecules?

Sulfur is in the same column of the periodic table as oxygen but it is less electronegative than oxygen. Compared to water molecules, how will the H2S molecules behave?

When carbon dioxide in the atmosphere dissolves with the raindrops, what is the expected change in pH of the raindrops?

A solution of pH 7 is ________ than a solution of pH 8.

Dilution of a buffer solution with a small amount of water will ________ the pH of the solution.

What kind of bond is formed between the two hydrogen atoms and the single oxygen atom?

Which of the following is NOT impacted by the acidification of ocean water?

On a hot day, temperature of land rises more quickly than that of sea. Which of the following statements best describe the process?

Which of the following is a hydrophobic material?

What is the hydroxide ion concentration of the lake described in question 3?

A slice of pizza has 500 kcal. If we could burn the pizza and use all the heat to warm a 50-L container of cold water, what would be the approximate increase in the temperature of the water? (Note: A liter of cold water weighs about 1 kg.)

Rank, from low to high, the pH of blood, stomach acid, and urine.

0.660 moles of NaCl are dissolved in 95.0 mL of water. Calculate the molarity of the NaCl solution.

How many grams of the compound in the figure are required to make 1 liter of a 0.5 M solution? (Note: The atomic masses, in daltons, are approximately 12 for carbon, 1 for hydrogen.)

We can be sure that a mole of table sugar and a mole of vitamin C are equal in their ________.

Rubbing alcohol swab on the skin feels cool because ________.

What kind of bonds are responsible for the unique cohesion, surface tension, and adhesion properties of water molecules?

What is the concentration of hydroxide ions in a solution of pH 5?

Biology and Its Themes

Atoms and Molecules

Carbon: the Basis of Molecular Diversity

Biological Macromolecules and Lipids

Energy and Life

Cell Structure and Function

Cell Membranes

Cellular Signaling

Cell Respiration

Photosynthetic Processes

Mitosis

Sexual Life Cycles and Meiosis

Mendelian Genetics

Linkage and Chromosomes

Nucleic Acids and Inheritance

Expression of Genes

Control of Gene Expression

Dna Technology

The Evolution of Genomes

How Evolution Works

Phylogenetic Reconstruction

Microevolution

Species and Speciation

Macroevolution

Introduction to Viruses

Prokaryotes

The Origin and Evolution of Eukaryotes

Nonvascular and Seedless Vascular Plants

Seed Plants

Introduction to Fungi

An Introduction to Animal Diversity

Invertebrates

Vertebrates

Plant Structure and Growth

Transport in Vascular Plants

Plant Nutrition

Reproduction of Flowering Plants

Plant Signals and Behavior

The Animal Body

Chemical Signals in Animals

Animal Digestive Systems

Animal Transport Systems

Animal Excretory Systems

Animal Reproductive Systems

Development in Animals

Animal Defenses Against Infection

Electrical Signals in Animals

Neural Regulation in Animals

Sensation and Movement in Animals

An Overview of Ecology

Behavioral Ecology

Populations and Life History Traits

Biodiversity and Communities

Energy Flow and Chemical Cycling in Ecosystems

Conservation and Global Ecology

Filters

Sulfur is in the same column of the periodic table as oxygen but it is less electronegative than oxygen. Compared to water molecules, how will the H₂S molecules behave?