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BIO 112 - I GOT THIS!!! > Chapter 2 - Chemistry > Flashcards

Chapter 2 - Chemistry Flashcards

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Biology 101 flashcards
1
Q

Matter

A

Anything that takes up space and has mass.
Matter is composed of elements. Solids, liquids, and
gases are matter

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2
Q

Mass

A

Amount of matter present

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3
Q

Weight

A

Heaviness due to gravitational pull on mass

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4
Q

Chemistry

A

Studies composition, properties, interaction
of matter

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5
Q

Biochemistry

A

Biological chemistry, which studies
physiological process and disease

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6
Q

Elements

A

Simplest types of matter with certain chemical
properties. There are 92 naturally occurring elements

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7
Q

Compounds

A

Chemical combinations of different elements

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8
Q

Atoms

A

Smallest particles of an element that have properties
of that element

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9
Q

Bulk elements:

A

Required by the body in large amounts
(C,O,H,N,S,P)

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10
Q

Trace elements:

A

Required by the body in small amounts
(Fe,I)

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11
Q

Ultratrace elements:

A

Required by the body in very minute
amounts (As)

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12
Q

Atoms

A

composed of subatomic particles

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13
Q

Protons

A

large particles
carry a single positive charge

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14
Q

Neutrons

A

Large particles
carry NO electrical charge

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15
Q

Electrons

A

Small particles
carry a single negative charge

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16
Q

Atoms consists of a ______ _______ (protons + Neutrons) and _______ in constant motion around the nucleus

A

Central Nucleus

Electrons

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17
Q

Number of _____ equals number of ______ in a atom; therefore, atoms are electrically _____

A

Protons

Electrons

Neutral

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18
Q

Atomic Number:

A

Number of protons in the nucleus of an atom of a specific
element

Each element has a unique atomic number

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19
Q

Mass Number:

A

The number of protons plus the number of neutrons in one
atom

Electrons do not contribute to the mass of the atom
because they are so light

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20
Q

Molecule

A

Particle formed when two or more atoms
chemically combine

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21
Q

Compound

A

Particle formed when two or more atoms of
different elements chemically combine

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22
Q

Molecular formulas:

A

Depict the elements present and the
number of each atom present in the molecule

H2 = a molecule of hydrogen

C6H12O6 = a molecule of glucose

H2O = a molecule of water

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23
Q

Chemical bonds

A

form when atoms
combine with other atoms. They result
from interactions between the electrons
of the atoms.

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24
Q

Electrons of an atom occupy regions of
space called

A

electron shells - these encircle the nucleus

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25
Q

For atoms with atomic numbers of 18 or
less, the following rules apply:

A
  • The first shell can hold up to 2
    electrons.
  • The second shell can hold up to 8
    electrons.
  • The third shell can hold up to 8
    electrons
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26
Q

Electrons in outermost shell determine

A

whether atom will react with other atoms
to form chemical bonds

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27
Q

Ion

A

An electrically charged atom that gains or loses
electrons to become stable

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28
Q

Cation

A

A positively charged ion, formed when an atom
loses electrons

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29
Q

Anion

A

A negatively charged ion, formed when an atom
gains electrons

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30
Q

Ionic Bonds:

A

Strong chemical bonds formed when ions of
opposite charge attract

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31
Q

Covalent Bonds

A

Strong chemical bonds, formed between
atoms that share electrons

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32
Q

Two atoms of hydrogen (H) can combine to form

A

a
hydrogen molecule (H2). Both atoms in the molecule
become stable

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33
Q

Hydrogen molecules (H2) often combine with oxygen (O2)
molecules to form

A

water molecules (H2O)

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34
Q

Nonpolar covalent bonds:

A

Covalent bonds in which electrons are shared equally

Found between atoms with same electronegativity

Atoms of same element have same number of protons, and
pull shared electrons equally

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35
Q

Polar covalent bonds:

A

Covalent bonds in which electrons are not shared equally

Found between atoms with different electronegativities

Forms polar molecules with unequal charge distribution

Atoms with larger number of protons have higher
electronegativity, and pull shared electrons closer to their
nucleus

Water is a polar molecule

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36
Q

Hydrogen bonds:

A
  • Relatively weak attraction
    of slightly positive (H) end
    of one polar molecule to
    slightly negative (N or O)
    end of a nearby polar
    molecule
  • Form between adjacent
    water molecules
  • Important for protein and
    nucleic acid structure
37
Q

Chemical reactions

A

occur when chemical bonds form or
break between atoms, ions, or molecules

38
Q

Reactants

A

are the starting materials of a chemical
reaction: the atoms, ions, or molecules

39
Q

Products

A

are substances formed at the end of the
chemical reaction

40
Q

Synthesis Reaction

A

more complex chemical structure is
formed

A + B => AB

41
Q

Decomposition Reaction

A

chemical bonds are broken to
form a simpler chemical structure

AB => A + B

42
Q

Exchange Reaction

A

chemical bonds are broken and new
bonds are formed

AB + CD => AD + CB

43
Q

Reversible Reaction

A

: the products can change back to the reaction

A + B = AB

44
Q

Electrolytes

A

Substances that release ions in water. The
solution can conduct an electric current, so it is called an
electrolyte

NaCl => Na plus + Cl negative

45
Q

Acids

A

Electrolytes that dissociate to release hydrogen ions
in water

46
Q

Bases

A

Substances that release ions that can combine with
hydrogen ions

47
Q

Salts

A

Electrolytes formed by the reaction between an acid
and a base

48
Q

pH Scale

A

Indicates the concentration of hydrogen ions in a
solution

49
Q

Neutral

A

A pH of 7 indicates equal concentrations of
This is the pH of water.

50
Q

Acidic

A

A p H of <7 indicates a greater concentration of

51
Q

Basic (alkaline)

A

A pH >7 indicates a higher concentration of

52
Q

What is the normal range of blood?

A

7.35 through 7.45

53
Q

Acidemia occurs when blood pH drops to what?

A

7.0 through 7.3

54
Q

Acidosis makes a person feel?

A

disoriented and fatigued

Caused by vomiting of alkaline intestinal contents, diabetes, lung
disease with impaired CO2 exhalation

55
Q

Alkalemia occurs when blood pH rises to

A

7.5 through 7.8

56
Q

Alkalosis makes a person feel

A

Dizzy and agitated

Caused by high altitude breathing, vomiting of acidic stomach
contents, high fever, taking excess antacids.

Homeostatic mechanisms help regulate pH

57
Q

Organic molecules:

A
  • Contain C and H
  • Depending on the type, they will dissolve in either water or organic
    liquids
  • Water-soluble organic compounds do not release ions, and are non-
    electrolytes
  • Carbohydrates, proteins, lipids, and nucleic acids
58
Q

Inorganic molecules

A
  • Generally do not contain C and H
  • Usually dissolve in water and dissociate, forming ions, and are
    electrolytes
  • Water, oxygen, carbon dioxide, and inorganic salts
59
Q

Water

A
  • Most abundant compound in living material
  • Two-thirds of the weight of an adult human
  • Major component of all body fluids
  • Medium for most metabolic reactions
  • Important role in transporting chemicals in the body
  • Absorbs and transports heat
  • Water balance exists when gains equal losses
  • Water is a solvent that many solutes dissolve in
60
Q

Oxygen

A
  • Used by organelles to release energy from nutrients in order to
    drive cell’s metabolic activities.
  • Necessary for survival
61
Q

Carbon dioxide (CO2)

A
  • Waste product released during metabolic reactions
  • Must be removed from the body through exhaling
62
Q

Inorganic salts:

A
  • Abundant in body fluids
  • Sources of necessary ions
  • Play important roles in metabolism
  • Help control H2O concentration, pH, blood clotting, nerve
    and muscle processes
  • Electrolyte balance exists when gains equal losses
63
Q

Main source of cellular energy:

A
  • Supply materials to build cell structures
  • Water-soluble
  • Contain C, H, and O
  • Ratio of H to O close to 2:1 (C6H12O6 = glucose)
64
Q

Size classification of carbohydrates:

A

Monosaccharides

Disaccharides

Polysaccharides

65
Q

Monosaccharides are…?

A

(single sugars): glucose, fructose

66
Q

Disaccharides

A

(double sugars): sucrose, lactose

67
Q

Polysaccharides

A

(complex carbohydrates): starch,
glycogen, cellulose

68
Q

Lipids

A
  • Insoluble in water, but soluble in organic solvents
  • Include triglycerides (fats), phospholipids, steroids
  • Important component of cell membranes, and have several
    functions in cell
69
Q

Most abundant lipids are triglycerides (fats)

A
  • Used for cellular energy
  • Contain more energy per gram than carbohydrates
  • Contain C, H, and O, but less O than carbohydrates
  • Consist of 1 molecule of glycerol and 3 fatty acids
70
Q

Phospholipids

A

are similar to triglycerides, except that they
have glycerol, 2 fatty acids, and a phosphate group

71
Q

Saturated fatty acids

A

Have only single carbon-carbon bonds
* Most are solid at room temperature
* Most are of animal origin

72
Q

Unsaturated fatty acids

A

Have one or more carbon-carbon double bond
* Most are liquid at room temperature
* Most are of plant origin

73
Q

Phospholipids

A

Similar to triglycerides, except that they have glycerol, 2
fatty acids, and a phosphate group
* Main structural component of cell membranes

74
Q

Steroids

A
  • 4 connected rings of carbon
  • Widely distributed in the body, various functions
  • Component of cell membranes
  • Used to synthesize adrenal and sex hormones
  • Cholesterol is the main steroid in the body
75
Q

Proteins

A
  • Used as structural materials, energy source, hormones,
    receptors, enzymes, antibodies
  • Consist of building blocks called amino acids
  • An amino acid contains an amino (–NH2) group, a carboxyl
  • (COOH) group, and a unique R (side chain) group
  • Amino acids are bound to each other by peptide bonds
76
Q

Peptide bonds

A

form between the amino group of one
amino acid, and the carboxyl group of the adjacent amino
acid

77
Q

4 Levels of Protein Structure:

A

Primary
Secondary
Tertiary
Quaternary

78
Q

Primary

A

Amino acid sequence

79
Q

Secondary

A

Pleated or twisted structure formed by hydrogen bonding
between nonadjacent amino acids

80
Q

Tertiary

A

Unique 3-dimensional folded shape, or conformation, of the
protein, which determines its function

81
Q

Quaternary

A

Structure formed by some proteins, when 2 or more
polypeptide chains are connected to become 1 protein

82
Q

Denaturation

A
  • A change in the secondary and tertiary structure of a protein
  • Caused by heat, radiation, pH changes, chemicals
  • Sometimes reversible, and other times irreversible
  • In case of enzymes, irreversible denaturation stops it from functioning
83
Q

Nucleic acids:

A
  • Carry genetic code (DNA) or aid in protein synthesis (RNA)
  • Nucleic acids encode amino acid sequences of proteins
  • Building blocks are called nucleotides, which consist of a
    sugar (S), a phosphate group (P), and an organic base (B)
84
Q

DNA

A

(Deoxyribonucleic acid): a double chain of nucleotides

85
Q

RNA

A

(Ribonucleic acid): a single chain of nucleotides

86
Q

What are two major types of Nucleic Acids

A

DNA and RNA

87
Q

DNA

A
  • Stores the genetic code
  • Contains the sugar deoxyribose
  • Structure—double helix
  • Composed of nucleotides
88
Q

RNA

A
  • Interacts with DNA to conduct protein synthesis
  • Contains the sugar ribose
  • Structure—single stranded
  • Composed of nucleotides

BIO 112 - I GOT THIS!!! (13 decks)

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