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ONLINE PHYSIOLOGY > Chapter 2: Chemical Composition of the Body > Flashcards

Chapter 2: Chemical Composition of the Body Flashcards

1
Q

Matter

A
  • Anything that takes up space and has mass (solid, liquid, gas)
  • composed of elements
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2
Q

Element

A
  • substance that can’t be chemically broken down into any simpler substance (i.e. oxygen, carbon, gold, helium)
  • elements are composed of atoms
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3
Q

Subatomic particles

A
  • protons: positive charge and in atoms nucleus
  • neutrons: electrically neutral/no charge and in nucleus
  • electrons: negative charge and orbit around nucleus
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4
Q

Atomic symbol

A
  • letters of the atom
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5
Q

Atomic Number

A
  • # of protons (bottom number in symbol)
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6
Q

Atomic Mass

A
  • equals # of protons and neutrons

- top number in symbol

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7
Q

Isotopes

A
  • different forms of an atom with same number protons, but different number neutrons (i.e. carbon-12, carbon-13, carbon-14)
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8
Q

Major elements of body

A
  • 99.3%
  • hydrogen 63%
  • oxygen 26%
  • carbon 9%
  • nitrogen 1%
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9
Q

Remaining 0.7% of total atoms

A
  • calcium
  • phosphorus
  • potassium
  • sulfur
  • sodium
  • chlorine
  • magnesium
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10
Q

Trace Elements

A
  • less than 0.01% total atoms in body
  • iron
  • iodine
  • copper
  • zinc
  • maganese
  • cobalt
  • chromium
  • selenium
  • molybdenum
  • flourine
  • tin
  • silicon
  • vanadium
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11
Q

Molecule

A

group of 2 or more atoms held together by energy

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12
Q

Compound

A
  • molecule composed of 2+ elements (i.e. O2 or H2O)

- electrons contain energy and atoms always seek out their lowest energy state meaning a full outer shell of electrons

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13
Q

Energy shell levels

A
  • 1st energy level = max 2 electrons
  • 2nd energy level = max 8 electrons
  • 3rd level = max 8 electrons
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14
Q

Lowest energy state

A
  • outermost level needs to be completely filled in order to be a stable atom
  • unstable elements seek out other unstable elements
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15
Q

Chemical Bond

A
  • force holding 2 atoms together
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16
Q

Covalent Bonds

A

form when 2 atoms share a pair of electrons

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17
Q

Double Covalent Bond

A

form when 2 atoms share 2 pairs of electrons

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18
Q

Polar v Nonpolar

A
  • atoms have different degrees of electronegativity (the power to attract electrons)
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19
Q

Polar covalent molecule

A
  • unequal sharing of the electron pair between atoms

- unequal charge distribution of the molecule

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20
Q

Nonpolar covalent molecules

A
  • equal sharing of electron pair

- equal charge distribution across the molecule

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21
Q

Ionic Bonds

A
  • occurs as result of an electrical attraction between 2 ions
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22
Q

Ion

A
  • a charged atom

- an atom in which the number or protons does not equal the number of electrons

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23
Q

Cations

A

positively charged ions

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24
Q

anions

A

negatively charged ions

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25
Q

electrolytes

A

the ionic forms of mineral elements because give electrical charge to solution

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26
Q

Hydrogen Bond

A
  • form between polar molecules as a result of an electrical attraction between the positive end of one molecule and the negative end of another (i.e. H2O)
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27
Q

Strength of Chemical bonds (highest to lowest)

A
  • covalent (share e-)
  • ionic (opposite charge attraction)
  • hydrogen (attraction of H to O or N)
  • hydrophobic interactions/VanDerWaals ( attraction between nonpolar molecules when close together - NOT AN ACTUAL BOND)
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28
Q

Molecular shape

A
  • contributes to ability of different molecules to form chemical bonds
  • rotations of bonds can rearrange molecules 3-D shape and therefore its molecular function
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29
Q

free radicals

A

atom containing an unpaired (single) electron in its outermost orbital

  • highly reactive
  • oxidize other atoms
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30
Q

Formation of free radcal

A
  • produced in certain cell types ~ used by certain leukocytes to destroy pathogens
  • produced as a consequence of exposure to radiation or toxins
  • -> cause DNA damage and are harmful to cells ~ associated with age-related disorders including cardiovascular, neural and eye diseases
  • -> antioxidants are protective (i.e. vitamins C and E)
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31
Q

Aqueous solution

A
  • chemical reactions in cells occur within an aqueous environment
  • aqueous solution = water is solvent
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32
Q

Important Properties of water

A
  • excellent solvent
  • water has great capacity to absorb, store, and release heat
  • water is adhesive and cohesive
  • water molecules take part in many chemical reactions in the body
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33
Q

Excellent Solvent Property of Water

A
  • dissolves more compounds in greater amounts than any other liquid
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34
Q

Solution

A

homogeneous mixture of 2+ kinds of molecules, atoms, or ions

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35
Q

Solute

A

dissolved substance

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36
Q

solvent

A

substance in which the solute dissolves

37
Q

solute concentration

A

amount of the solute present in a unit volume of solution (g/L), (moles/L) –> 1M of solute per solution

38
Q

like dissolves likes

A
  • nonpolar solutes will be soluble in nonpolar solvents

- polar solutes will be solutes in polar solutes

39
Q

hydrophilic substances

A
  • dissolve in and interact with water (ions, and polar covalent molecules)
40
Q

hydrophobic substances

A
  • do not interact with water

- are poorly soluble or completely insoluble in water (nonpolar covalent molecules)

41
Q

Water has a great capactiy to absorb, sore and release heat property

A
  • high heat capacity and high heat of vaporization
  • high specific heat (amount of energy required to raise the temperature of a substance by 1 degrees celcius
  • water serves as a heat “buffer” = keeps internal temperature relatively stable
42
Q

Water is adhesive and cohesive

A
  • cohesion: water molecules cling together
  • adhesion: water molecules adhere to surfaces
  • facilitate flow of blood to blood vessels
43
Q

Water molecules take part in many chemical reactions in the body property

A
  • hydrolysis reaction
  • dehydration reaction
  • reactions are good for creating or breaking large organic molecules
44
Q

hydrolysis reaction

A

covalent bond is broken when water is added to system

45
Q

dehydration reaction

A

covalent bond is formed when water is removed between molecules

46
Q

Acid

A
  • molecule that dissociates in an aqueous solution releasing hydrogen ions (i.e. HCL –> H+ and Cl-)
  • increase in H+ in solution = more acidic
47
Q

Strong Acid

A

Completely Ionize in solution

48
Q

Weak Acid

A

Incompletely ionize in solution

49
Q

Base

A

a molecule that takes up hydrogen ions, or releases hydroxide ions (OH-) in an aqueous solution
- basic solution = alkaline solution

50
Q

pH sclae

A
  • based on -log[H+] of solution
  • lower ph = more acidic, higher ph = more basic
  • neutral solution = pH 7.0
  • acidic solution = pH 7.0
  • up to 14
51
Q

pH importance

A
  • cells function in a limited pH range (7.25-7.45) is normal range in human blood
  • enzyme activity is affected by pH
  • pH changes can cause protein and enzyme denaturation
  • buffering systems in body function to keep pH in normal limits
52
Q

Buffer

A
  • chemical that takes up excess H+ or OH- from solution (or donates H+ to solution) to minimize changes in pH
53
Q

Organic Molecules

A
  • life is carbon-based
  • organic molecules contain carbon and hydrogen
  • each carbon atom can covalently bond to 4 other atoms
  • hydrocarbons contain only carbon and hydrogen
54
Q

Macromolecules

A
  • polymers

- structure depends on monomer structure, number, 3-D organization or subunits

55
Q

Polymers

A
  • composed of smaller subunits called monomers

- synthesized by dehydration reactions, broken down by hydrolysis reactions

56
Q

Function Group

A
  • group of atoms attached to an organic molecule that gives it unique chemical properties
  • specific combinations of atoms, always reacts the same way chemically
  • often provide an electrical charge or polarity to the molecule, make a molecule hydrophobic or hydrophilic
57
Q

4 classes of organic molecules in organisms

A
  • carbohydrates
  • lipids
  • proteins
  • nucleic acids
58
Q

Carbohydrates

A
  • simple and complex sugars; important to energy production and storage
59
Q

Simple Sugars

A
  • monosaccharides (monomer) –> most are pentoses or hexoses (i.e. glucose, fructose)
  • disaccharides: 2 bonded monosaccharides –> i.e. lactose, maltose, sugar
60
Q

Complex Sugars

A
  • polysaccharides: many joined monosaccharides
  • starch & glycogen: store energy. composed of thousands of glucose molecules linked together and differ in degree of branching
  • cellulose & chitin: structural components
61
Q

Lipids

A
  • composed mostly of hydrogen and carbon atoms
  • nonpolar and hydrophobic
  • subclasses: triglycerides (fats&oils), phospholipids, steroids
62
Q

Fats

A
  • long-term energy storage and insulation in animals
63
Q

Oils

A
  • long-term energy storage in plants and their seeds
64
Q

Phospholipids

A
  • component of plasma membrane
65
Q

Steroids

A
  • component of plasma membrane (cholesterol) and sex hormones
66
Q

Triglycerides and fats

A
  • composed of 3 fatty acid molecules and 1 glycerol molecule

- 1 fat molecule = triglyceride

67
Q

Saturated Fatty Acid

A
  • all carbons are linked by single covalent bonds
68
Q

Unsaturated fatty acid

A
  • contain 1+ double bonds between carbon atoms
69
Q

Monounsaturated

A

one double bond

70
Q

polyunsaturated

A

more than one double bond

71
Q

Cis fatty acid

A

both hydrogens are on the same side of the double-bonded carbons (most naturally occurring)

72
Q

Trans fatty acid

A

hydrogens are opposite sides of the double bonded carbons

73
Q

Eicosanoids

A

altered fatty acids derived from arachidonic acid that regulate certain cell functions

74
Q

phospholipids

A

glycerol
2 fatty acids
phosphate group
nitrogen containing group

75
Q

Amphipathic

A

important for phospholipid membrane

76
Q

Steroids

A
  • structure includes 4 interconnected rings of carbon atoms

- i.e. cholesterol, cortisol, testosterone, estrogen

77
Q

Polypeptide

A
  • polymers formed from amino acids joined by peptide bonds
  • carbon, hydrogen, oxygen, nitrogen
  • peptide has 50 amino acids
78
Q

Amino Acids

A
  • all have an amino group, a carboxyl group, and a varying side chain (R)
  • 20 different naturally occurring amino acids
  • proteins creating by dehydration reaction of amino acids
79
Q

glycoproteins

A

one or more monosaccharides covalently attached to the side chains of specific amino acids

80
Q

levels of protein structure

A
  • primary, secondary, tertiary, quaternary
81
Q

Primary structure

A
  • amino acid sequence

- determines 2nd and 3rd structures

82
Q

Secondary structure

A
  • alpha helix

- beta pleated sheet

83
Q

Tertiary structure

A
  • conformation= 3D shape of molecule
  • how folds in space
  • critical to protein function!
84
Q

Quaternary structure

A

only in proteins with one or more polypeptide subunits

85
Q

Nucleic Acids

A

composed of chains of nucleotides

86
Q

DNA

A
  • deoxyribonucleic acid
  • contains the sugar deoxyribose
  • double-stranded (double-helix)
  • genetic material
  • nucleotides covalently bind to make DNA
  • sugars&phosphates are the backbone
  • adenine&thymine = 2H bonds
  • cytosine&guanine = 3H bonds
87
Q

RNA

A
  • ribonucleic acid
  • ribose
  • single-stranded
  • involved in converting the info in DNA to proteins
88
Q

ATP

A
  • adenosine triphosphate = energy currency of the cell
  • receives energy from breakdown of carbs, proteins, and fats
  • releases energy upon hydrolysis
  • energy transfer
  • *energy currency of cell**
89
Q

Cells use ATP for:

A
  • production and force movement
  • active transport
  • synthesis of organic molecules

ONLINE PHYSIOLOGY (13 decks)

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