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Biology > Chapter Two: Life's Chemistry and the Importance of Water > Flashcards

Chapter Two: Life's Chemistry and the Importance of Water Flashcards

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AP® Biology flashcards Biology 101 flashcards
1
Q

Each element has a unique number of ______

A

protons

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2
Q

Different isotopes have different numbers of ______

A

neutrons

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3
Q

How do radioisotopes behave?

A

They are unstable and spontaneously breakdown, giving off energy

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4
Q

Atoms with _____ outer shells are stable

A

full

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5
Q

What do atoms do to maximize stability?

A

They react (bond) with other atoms to obtain full outer shells

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6
Q

Why are noble/inert gases non-reactive

A

their shell is full

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7
Q

When does a covalent bond form

A

when the electron orbitals of the two atoms overlap in an energetically favorable manner

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8
Q

When does unequal sharing of electrons occur?

A

when the two atoms are different elements and they have differences in electronegativities

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9
Q

What happens to the electrons in a polar bond?

A

electrons are pulled closer to the nucleus of the more electronegative atom; because of this the more electronegative atom will be slightly negatively charged and the other will be slightly positively charged

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10
Q

What is a nonpolar bond?

A

electrons are shared equally

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11
Q

Electronegativity of Oxygen

A

3.5

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12
Q

Electronegativity of Hydrogen

A

2.1

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13
Q

Properties of the covalent bonds of water

A

Both are polar and have a slight negative on the oxygen and slight positive on the hydrogen

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14
Q

When do covalent bonds form and when do ionic bonds form, based on electronegativities?

A

smaller difference in electronegativity: polar covalent bond
larger difference in electronegativity: ionic bond formation

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15
Q

If the electronegativity of atoms differs by 0.4 or less…

A

Covalent with equal sharing forms

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16
Q

If the electronegativity of atoms differs by 0.4 to 2.0…

A

Covalent with unequal sharing forms

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17
Q

If the electronegativity of atoms differs by more than 2.0…

A

Ionic bond forms

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18
Q

What is an ionic bond?

A

The transfer of electron(s) from one atom to another

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19
Q

When can a complete transfer of an electron occur

A

When the electronegativity difference is greater than 2.0

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20
Q

Cations

A

positively charged ions

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21
Q

Anions

A

negatively charged ions

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22
Q

What are ionic bonds formed by?

A

electrical attraction of anions and cations

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23
Q

Ionic compounds tend to form _____ in which there is a regular arrangement of ______ and _____

A

crystals; anions; cations

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24
Q

Where can hydrogen bonds form?

A

Between two water molecules, water and a polar molecule, or two separate parts of a big molecule

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25
Q

Van der Waals interactions

A

Attractions between oppositely charged atoms in nonpolar molecules. Movement of electrons results in small temporary dipoles

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26
Q

When does Van der Waals result in significant force?

A

When there are many interactions

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27
Q

What does Anabolism do?

A

Converts subunits to macromolecules

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28
Q

What does catabolism do?

A

Convert macromolecules to subunits

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29
Q

What is a subunit?

A

sugars, amino acids, fatty acids, nucleotides

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30
Q

What is a macromolecule?

A

carbohydrates, proteins, fats, nucleic acids

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31
Q

What are energy transformations linked to in cells?

A

chemical transformations

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32
Q

Does catabolic or anabolic reactions need energy input? releases energy?

A

Anabolic needs energy input, catabolic releases energy

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33
Q

What is metabolism?

A

The sum total of all chemical reactions occurring in a biological system at a given time

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34
Q

What is energy?

A

The capacity to do work

35
Q

What is potential energy?

A

energy stored as chemical bonds, concentration gradient, charge imbalance, etc.

36
Q

What is kinetic energy?

A

the energy of movement

37
Q

Define 1st Law of Thermodynamics

A

Energy is neither created nor destroyed

38
Q

Define 2nd Law of Thermodynamics

A

When energy is converted from one form to another, some of that energy becomes unavailable to do work

39
Q

What is entropy?

A

Some energy is converted to a nonusable form associated with disorder or randomness

40
Q

Will a change that decreases entropy occur spontaneously?

A

No – only can occur if energy is added to the system

41
Q

In a closed system, the amount of usable` energy _______ with every transformation

A

decreases

42
Q

Equation for enthalpy

A

Enthalpy (H) = free energy (G) + entropy (S)

43
Q

What energy can be used for cellular work?

A

Free Energy (G)

44
Q

∆G Equation

A

∆G = H-TS = Gproducts - Greactants

45
Q

When G is negative, free energy is ________ and the reaction is _____ . When G is positive, free energy is _____ and the reaction is ____.

A

released, exergonic;
consumed, endergonic;

46
Q

Chemical reaction

A

when atoms combine or change their bonding partners

47
Q

What is activation energy (Ea)

A

The additional energy required to initiate the reaction

48
Q

In what type of reactions is Ea required? Why?

A

Both exergonic and endergonic; Covalent bonds in reactants must be broken

49
Q

In exergonic reactions, do reactants or products have higher free energy?

A

reactants

50
Q

In endergonic reactions, do reactants or products have higher free energy?

A

products

51
Q

What is a condensation reaction?

A

glucose + fructose = sucrose + H20

52
Q

What is hydrolysis?

A

complex molecule + h20 = simpler molecules

53
Q

Does a condensation reaction have positive or negative G?

A

positive G, meaning it requires energy

54
Q

Describe exergonic reactions

A

release free energy, the complexity decreases, the disorder is generated and can occur spontaneously

55
Q

Describe endergonic reactions

A

consume free energy, complexity increases, localized decrease in entropy, does not occur spontaneously

56
Q

anabolic reactions are ______ and catabolic reactions are _____

A

Endergonic
Exergonic

57
Q

What is equilibrium?

A

a point where the forward and reverse reactions proceed at the same rate and ∆G=0

58
Q

Heterotrophs

A

start with chemical energy from photosynthetic cohabitants

59
Q

How do photosynthetic organisms get energy?

A

capture solar energy and convert it to chemical energy

60
Q

Is work able to be done at equilibrium?

A

No

61
Q

Why are water molecules polar

A

unequal charge distribution and asymmetric shape

62
Q

What makes water naturally cohesive?

A

H bonds

63
Q

Why does water have a high specific heat?

A

It has a large number of H bonds

64
Q

What molecules are soluble in water

A

hydrophilic molecules (ionic, polar)

65
Q

How do salts dissolve in water

A

Anions are surrounded by the hydrogens on a water molecule and cations are surrounded by oxygens

66
Q

Nonpolar molecules are more attracted to _________ _________ than water

A

one another

67
Q

How do you calculate pH

A

-log(H+)

68
Q

Does water act as a base or acid?

A

Water acts as both a weak base and weak acid

69
Q

What happens when acids dissolve in water?

A

they release hydrogen ions

70
Q

What do bases do?

A

accept H+ ions; decreases proton concentrations

71
Q

What percent of cells are water?

A

70%

72
Q

What is intracellular pH

A

ranges from 7.0 - 7.4

73
Q

What do buffers do?

A

help maintain constant pH by absorbing or releasing H+ ions

74
Q

What are buffers composed of?

A

a weak acid and its corresponding base

75
Q

What is homeostasis

A

the process of living organisms mainting constant internal conditions

76
Q

changes in pH can alter _______

A

cellular structures

77
Q

Hydroxyl Group

A

-OH

78
Q

Aldehyde

A

-C=OH

79
Q

Keto

A

-C=O
I

80
Q

Carboxyl

A

=COOH

81
Q

Amino

A

R-NH2

82
Q

What do functional groups do when they attach to larger molecules?

A

they give their properties to the larger molecules

83
Q

Sulfhydryl

A

-SH

Biology (12 decks)

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