Chapters 3 & 4 Flashcards

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1
Q

Water molecules have a polarity, which allows them to be electrically attracted to other water molecules and other polar molecules by weak chemical bonds known as _____.

A

hydrogen bonds

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2
Q

Many of water’s emergent properties, such as its cohesion, its high specific heat, and its high heat of vaporization, result from the fact that water molecules _____.

A

are attracted to each other by partial negative and positive charges on the oxygen and hydrogen atoms, respectively

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3
Q

The amount of energy that must be absorbed or lost to raise or lower the temperature of 1 g of liquid water by 1°C _____.

A

is 1 calorie

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4
Q

Because organisms are made primarily of water, they resist rapid temperature changes. This useful quality is based on water’s _____.

A

high specific heat

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5
Q

Water has a high specific heat, meaning that

A

a relatively large amount of heat must be added or removed in order to get the temperature of the water to change significantly.

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6
Q

The specific heat of liquid water is

A

1 cal/g/°C

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7
Q

The formation of hydrogen bonds between the positive and negative regions of different water molecules accounts for

A

most of water’s unique properties.

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8
Q

The polarity of a water molecule allows the oxygen of one water molecule to

A

bond weakly to the hydrogen of another water molecule.

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9
Q

Sodas typically contain sugar, flavorings, coloring agents, and carbon dioxide dissolved in water. The best term to describe this mixture would be _____.

A

an aqueous solution

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10
Q

If the molecular mass of a carbon atom is 12, the mass of a hydrogen atom is 1, and the mass of an oxygen atom is 16 daltons, how many molecules does one mole of table sugar (sucrose; C12H22O11) contain?

A

6.02 x 10^23

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11
Q

the number of molecules in one mole of any substance is

A

6.02 x 10^23

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12
Q

An acid is a substance that _____.

A

increases the hydrogen ion concentration of an aqueous solution

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13
Q

As an acid dissociates, it

A

donates a hydrogen ion to the solution

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14
Q

A pH of 6 is how many times more acidic than a pH of 9?

A

1,000

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15
Q

A pH of 6 is

A

10 times more acidic than 7, which is 10 times more acidic than 8, which is 10 times more acidic than 9. 10 x 10 x 10 = 1,000.

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16
Q

A buffer

A

resists change in pH by accepting hydrogen ions when acids are added to the solution and donating hydrogen ions when bases are added.

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17
Q

Buffers minimize the change in the _____ of a solution.

A

pH

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18
Q

Most acid precipitation results from the combination of _____ with water in the atmosphere, forming strong acids that fall with rain or snow.

A

sulfur oxides and nitrogen oxides.

These compounds react with water in the atmosphere to form sulfuric acid and nitric acid.

19
Q

Most organic compounds contain carbon and _____.

A

hydrogen

20
Q

The experiments of Wöhler, Kolbe, Miller, and other chemists invalidated the concept of vitalism by demonstrating that _____.

A

organic molecules could be produced apart from living organisms using inorganic materials

21
Q

Vitalism gave way to mechanism, the view that _____.

A

physical and chemical laws govern living systems

Living things are subject to physical and chemical laws. They do not exist outside of them.

22
Q

The large diversity of shapes of biological molecules is possible because of the extensive presence of _____ in the molecules.

A

carbon

With four electrons to share, carbon-based molecules can be multibranching and three-dimensionally variable.

23
Q

Which of the following is a hydrocarbon?

A

C3H8

(This is a typical hydrocarbon with single covalent bonds; the number of hydrogen atoms is equal to two times the number of carbon atoms plus 2.)

24
Q

Molecules that have the same chemical formula (same numbers of each atom) but different three-dimensional shapes are called _____.

A

isomers

Isomers of carbon compounds can arise in several different ways.

25
Q

Cis-trans isomers

A

differ in their spatial arrangement around inflexible double bonds.

(Cis-trans isomers maintain the same covalent partnerships, but the atoms may be arranged differently.)

26
Q

Citric acid makes lemons taste sour. Which of the following is a functional group that would cause a molecule such as citric acid to be acidic?

A

carboxyl

The carboxyl group can release a hydrogen ion when in solution.

27
Q

Variations in the reactive properties of different organic molecules are most closely associated with _____.

A

the presence or absence of functional groups.

28
Q

Functional groups are the most common participants in

A

chemical reactions

29
Q

What functional group is commonly used in cells to transfer energy from one organic molecule to another?

A

phosphate.

(The addition and release of phosphate groups to and from ADP and ATP is how cells store chemical energy and expend it to accomplish work.)

30
Q

Each water molecule is joined to _____ other water molecules by ____ bonds.

A

four … hydrogen

(As can be seen in the illustration on page 1 of the activity titled “The Polarity of Water” a water molecule is joined to four other water molecules by hydrogen bonds.)

31
Q

The unequal sharing of electrons within a water molecule makes the water molecule _____.

A

polar

(The electrons spend more time with the oxygen of the water molecule than with the hydrogens of water. Thus, the oxygen has a net negative charge and the hydrogens have a net positive charge.)

32
Q

The tendency of an atom to pull electrons toward itself is referred to as its _____.

A

electronegativity

33
Q

Hydrogen Bonds are weaker than covalent bonds because

A

they do not involve sharing of electrons, and they are weaker than ionic bonds because they involve the attraction of partial (not full) opposite charges.

34
Q

The high surface tension of water allows

A

the insect to remain on the surface.

35
Q

Many mammals control their body temperature by sweating. Which property of water is most directly responsible for the ability of sweat to lower body temperature?

A

the absorption of heat by the breaking of hydrogen bonds

36
Q

The bonds that are broken when water vaporizes are

A

hydrogen bonds between water molecules

37
Q

Which of the following is a hydrophobic material?

A

wax

38
Q

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

A

number of molecules

39
Q

Measurements show that the pH of a particular lake is 4.0. What is the hydrogen ion concentration of the lake?

A

10^-4 M

40
Q

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.)

A

10 degrees C

41
Q

How many grams of acetic acid (C2H4O2) would you use to make 10 L of a 0.1 M aqueous solution of acetic acid? (Note: The atomic masses, in daltons, are approximately 12 for carbon, 1 for hydrogen, and 16 for oxygen.)

A

60 g

42
Q

Organic chemistry is currently defined as

A

the study of carbon compounds

43
Q

Which chemical group is most likely to be responsible for an organic molecule behaving as a base?

A

amino