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

Biochemistry Part I Flashcards

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
*Define* **Nonpolar molecules**
Molecules with no partial positive and negative regions Ex: Hydrocarbons
26
*Define* **Hydrophobic**
"Water fearing" Nonpolar; avoids water
27
*Define* **Hydrophilic**
"Water loving" Polar; dissolves in or attracts to water
28
**Density of water**
Liquid: Most dense due to hydrogen bonds pulling molecules closer together than in solid form Solid: Less dense than liquid
29
**Importance of water's density as a solid**
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
*Define* **Specific heat capacity**
Energy needed to increase the temperature of a substance
31
**Water's specific heat capacity**
Very high, which helps regulate temperature within organisms and near large bodies of water
32
*Define* **Heat of vaporization**
Energy required to convert substance from liquid to gas
33
**Water's heat of vaporization**
Very high, leading to evaporative cooling
34
*Define* **Solvent**
A substance that dissolves other substances
35
*Define* **Solute**
A substance that dissolves in another substance
36
*Define* **Universal solvent**
Water can cause dissociation of all polar molecules
37
*Define* **Cohesion**
Attraction of like molecules (ex: water attracted to water)
38
*Define* **Adhesion**
Attraction of different molecules (ex: water attracted to glass)
39
*Define* **Surface tension**
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
*Define* **pH**
Measure of acidity or alkalinity (basicity)
41
*Define* **Acid**
A substance that increases [H+] in solution pH \< 7
42
*Define* **Base**
A substance that increases [OH-] and/or decreases [H+] in solution pH \> 7
43
*Describe the* **pH scale**
14 - strongest base \>7 - base 7 - neutral \<7 - acid 1 - strongest acid\*
44
*Define* **Buffer**
A substance that prevents rapid change of pH in a solution
45
*Define* **Hydrocarbons**
Chains of carbons and hydrogens
46
*Define* **Isomer**
Any molecules with the same chemical formula but different arrangement of atoms
47
*Define* **Structural isomer**
An isomer where the bonds are placed differently (ex: butane and isobutane)
48
*Define* **Geometric isomer**
An isomer where the arrangement of atoms around double bonds differ
49
**cis**
Having functional groups and/or carbons that reside on the same side of a double bond
50
**trans**
Having functional groups and/or carbons that reside on opposite sides of a double bond
51
*Define* **Enantiomers**
Mirror image isomers
52
*Draw* **Hydroxyl**
53
*Draw* **Methyl**
54
*Draw* **Carbonyl**
55
*Draw* **Carboxyl**
56
*Draw* **Amino**
57
*Draw* **Phosphate**
58
*Draw* **Sulfhydryl**
59
*List* **Four types of macromolecules**
Carbohydrates Proteins Lipids Nucleic acids
60
**Single units of macromolecules are called**
monomers
61
*Define* **Polymer**
Many connected monomers
62
**What reactions make and break polymers?**
Dehydration synthesis makes polymers Hydrolysis breaks polymers
63
**Energy in metabolic reactions**
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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