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Mrs. Unger's AP Biology > Biochemistry Part I > Flashcards

Biochemistry Part I Flashcards

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1
Q

Define

Matter

A

Any substance that occupies space and has mass

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2
Q

Define

Elements

A

A form of matter with specific chemical and physical properties

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3
Q

How many elements are there?

A

98 naturally occurring

118 known / stable

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4
Q

List

Most common elements in the body (6)

A

Carbon

Hydrogen

Oxygen

Nitrogen

Phosphorus*

Sulfur*

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5
Q

List

Subatomic particles

A

Proton

Neutron

Electron

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6
Q

Properties of

Protons

A

Positive

Mass = 1 amu

In nucleus

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7
Q

Properties of

Neutrons

A

Neutral

Mass = 1 amu

In nucleus

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8
Q

Properties of

Electrons

A

Negative

Negligible mass

Surrounding nucleus

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9
Q

Adding or removing protons changes…

A

the element and the atomic number

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10
Q

Adding or removing neutrons changes…

A

mass of an atom;

creates different isotopes (forms) of an element

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11
Q

Adding or removing electrons changes…

A

the charge of the atom

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12
Q

Define

Atomic mass

A

Average mass of one mole of an element, which takes isotopes (which have different mass numbers) into account

FYI: You will NOT need to memorize atomic mass v. mass number

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13
Q

Define

Isotope

A

Different forms of an element with the same number of protons but different numbers of neutrons

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14
Q

Define

Electron orbital

A

“Shells” around a nucleus where electrons are likely to be found

2 in first

8 in second and third

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15
Q

Define

Valence shell

A

Outermost electron orbital in an atom

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16
Q

Define

Molecule

A

Chemical joining of two or more atoms

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17
Q

Define

Covalent bond

A

Sharing of electrons between atomic nuclei

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18
Q

Define

Polar covalent

A

A covalent bond where electrons are more likely to be found around one atom (which is more electronegative)

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19
Q

Define

Nonpolar covalent

A

A covalent bond where electrons are equally shared

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20
Q

What leads to the formation of an cation?

A

Cation (cat-eye-on) = positive ion

Occurs when an atom loses electrons

Most common in first two groups (columns) of periodic table

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21
Q

What leads to the formation of an anion?

A

Anion = Negative ion

Occurs when atoms take electrons to become stable

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22
Q

Why is water polar

A

Oxygen is electronegative, leading to the formation of polar covalent bonds between oxygen and two hydrogens. The bent shape means more electrons (negative) are at the oxygen end

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23
Q

Define

Polarity

A

Unequal distribution of charge in a molecule

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24
Q

Define

Polar molecules

A

Molecules with partial positive and negative regions Ex: Water

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25
Q

Define

Nonpolar molecules

A

Molecules with no partial positive and negative regions

Ex: Hydrocarbons

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26
Q

Define

Hydrophobic

A

“Water fearing”

Nonpolar; avoids water

27
Q

Define

Hydrophilic

A

“Water loving”

Polar; dissolves in or attracts to water

28
Q

Density of water

A

Liquid: Most dense due to hydrogen bonds pulling molecules closer together than in solid form

Solid: Less dense than liquid

29
Q

Importance of water’s density as a solid

A

Ice floats

  • Good for insulating bodies of water
  • Prevents freezing / sinking of ice in bodies of water so that Earth is not a giant icecube
30
Q

Define

Specific heat capacity

A

Energy needed to increase the temperature of a substance

31
Q

Water’s specific heat capacity

A

Very high, which helps regulate temperature within organisms and near large bodies of water

32
Q

Define

Heat of vaporization

A

Energy required to convert substance from liquid to gas

33
Q

Water’s heat of vaporization

A

Very high, leading to evaporative cooling

34
Q

Define

Solvent

A

A substance that dissolves other substances

35
Q

Define

Solute

A

A substance that dissolves in another substance

36
Q

Define

Universal solvent

A

Water can cause dissociation of all polar molecules

37
Q

Define

Cohesion

A

Attraction of like molecules (ex: water attracted to water)

38
Q

Define

Adhesion

A

Attraction of different molecules (ex: water attracted to glass)

39
Q

Define

Surface tension

A

Water’s cohesion pulls molecules together with enough force to overcome droplets being flattened by gravity; some objects remain on the top of water

40
Q

Define

pH

A

Measure of acidity or alkalinity (basicity)

41
Q

Define

Acid

A

A substance that increases [H+] in solution pH < 7

42
Q

Define

Base

A

A substance that increases [OH-] and/or decreases [H+] in solution pH > 7

43
Q

Describe the

pH scale

A

14 - strongest base

>7 - base

7 - neutral

<7 - acid

1 - strongest acid*

44
Q

Define

Buffer

A

A substance that prevents rapid change of pH in a solution

45
Q

Define

Hydrocarbons

A

Chains of carbons and hydrogens

46
Q

Define

Isomer

A

Any molecules with the same chemical formula but different arrangement of atoms

47
Q

Define

Structural isomer

A

An isomer where the bonds are placed differently (ex: butane and isobutane)

48
Q

Define

Geometric isomer

A

An isomer where the arrangement of atoms around double bonds differ

49
Q

cis

A

Having functional groups and/or carbons that reside on the same side of a double bond

50
Q

trans

A

Having functional groups and/or carbons that reside on opposite sides of a double bond

51
Q

Define

Enantiomers

A

Mirror image isomers

52
Q

Draw

Hydroxyl

A
53
Q

Draw

Methyl

A
54
Q

Draw

Carbonyl

A
55
Q

Draw

Carboxyl

A
56
Q

Draw

Amino

A
57
Q

Draw

Phosphate

A
58
Q

Draw

Sulfhydryl

A
59
Q

List

Four types of macromolecules

A

Carbohydrates

Proteins

Lipids

Nucleic acids

60
Q

Single units of macromolecules are called

A

monomers

61
Q

Define

Polymer

A

Many connected monomers

62
Q

What reactions make and break polymers?

A

Dehydration synthesis makes polymers

Hydrolysis breaks polymers

63
Q

Energy in metabolic reactions

A

Making new bonds (forming polymers) requires energy

Breaking bonds (breaking down polymers) releases energy

Mrs. Unger's AP Biology (16 decks)

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