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ANAPHY LEC > WEEK 2 > Flashcards

WEEK 2 Flashcards

1
Q

This state of matter is compact and has a definite shape and volume.

A

Solid

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2
Q

The science of the structure and interactions of matter.

A

Chemistry

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3
Q

The force of gravity acting on matter. Change

A

Weight

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4
Q

All forms of matter are made up of limited number of building blocks called

A

Chemical Elements

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5
Q

The four elements that constitute about 96% of the body’s mass are called

A

Major elements.

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6
Q

Anything that occupies space and has mass

A

Matter

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7
Q

The amount of matter in any object. No change

A

Mass

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8
Q

How many different chemical elements are normally present in Rafael John F Dubria’s body?

A

26

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9
Q

Has a definite shape and volume; takes the shape of their container

A

Liquid

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10
Q

The smallest atoms; diameter less than 0.1 nanometer (0.1 x 10-9m = 0.0000000001 m) Not sure pila ka 0 pero u get the gist

A

Hydrogen Atoms

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11
Q

These 14 elements are present in tiny amounts. Account for 0.4% of the body’s mass; some function as cofactors.

A

Trace Elements

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12
Q

Have neither a definite shape nor volume.

A

Gas

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13
Q

Each named element is designated by one or two letters of the English alphabet, Latin, or another language. What is this designation called?

A

Chemical Symbol

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14
Q

Rest question

A

Rafael John F. Dubria is handsome

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15
Q

The dense central core of an atom is called…………………….

A

Nucleus

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16
Q

These 8 elements contribute about 3.6% of the body’s mass

A

Lesser Elements.

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17
Q

This element is a part of water and many organic (carbon-containing) molecules; used to generate ATP, a molecule used by cells to temporarily store chemical energy. About 65% of the body’s mass

A

Oxygen

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18
Q

This subatomic particle is positively charged ++++++++++++++++++++++++++++++++++++++++++++

A

Protons

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19
Q

A certain region around the nucleus where groups of electrons are most likely to move around in.

A

Electron Shell

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20
Q

This designation of an element is = number of protons

A

Atomic Number

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21
Q

The sum of an element’s protons and neutrons

A

Mass Number

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22
Q

Atoms of an element that have different numbers of neutrons and therefore different mass numbers.

A

Isotopes

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23
Q

Certain Isotopes are unstable. What are these unstable isotopes called hmm?

A

Radioactive Isotopes/Radioisotopes

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24
Q

Some radioisotopes are used to follow the movement of certain substances through the body. What are these radioisotopes called, team?

A

Tracers

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25
Q

The time required for half of the radioactive atoms in a sample of an isotope to decay into a more stable form

A

Half-life

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26
Q

The standard unit for measuring the mass of atoms and their subatomic particles is called?????????????????????????????????????????????????????????????????

A

Dalton

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27
Q

Substance that contains atoms of two or more different elements

A

Compound

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28
Q

An atom or group of atoms with an unpaired electron in the outermost shell

A

Free Radical

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29
Q

The average mass of all naturally occurring isotopes in an element

A

Atomic Mass

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30
Q

An atom that has a positive or negative charge because of its unequal amount of protons and electrons

A

Ions

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31
Q

These subatomic particles are negatively charged ———————-

A

Electrons

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32
Q

Substances that inhibit oxygen-derived free radicals

A

Antioxidants

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33
Q

Under the right conditions, two or more atoms can interact in ways that produce a chemically stable arrangement of eight valence electrons for each atom. What chemical principle is this?

A

Octet Rule

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33
Q

Under the right conditions, two or more atoms can interact in ways that produce a chemically stable arrangement of eight valence electrons for each atom. What chemical principle is this?

A

Octet Rule

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34
Q

The force of attraction that holds together ions with opposite charges.

A

Ionic Bond

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35
Q

The total number of electrons exceed the number of protons; a negatively charged ion

A

Anion

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36
Q

The total number of protons exceeds the number of electrons; a positively charged ion

A

Cation

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37
Q

An ionic compound that breaks apart into positive and negative ions in solutions

A

Electrolyte

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38
Q

Two or more atoms share electrons rather than gaining or losing them.

A

Covalent Bonds

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39
Q

This bond results when two atoms share one electron pair.

A

Single Covalent Bond

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40
Q

This bond results when two atoms share two pairs of electrons.

A

Double Covalent Bond

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41
Q

This bond results when two atoms share three pairs of electrons.

A

Triple Covalent Bond

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42
Q

In some covalent bonds, two atoms share the electrons equally— one atom does not attract the shared electrons more strongly than the other atom

A

Nonpolar Covalent Bond

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43
Q

the sharing of electrons between two atoms is unequal—the nucleus of one atom attracts the shared electrons more strongly than the nucleus of the other atom.

A

Polar Covalent Bond

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44
Q

The power of atoms to attract electrons to themselves.

A

Electronegativity

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45
Q

This type of bond forms when a hydrogen atom with a partial positive charge attracts the partial negative charge of neighboring electronegative atoms.

A

Hydrogen Bond

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46
Q

True or False: Hydrogen bonds occur because hydrogen atoms in one water molecule are attracted to the partial negative charge of the oxygen atom in another water molecule.

A

True

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47
Q

A measure of the difficulty of stretching or breaking the surface of a liquid.

A

Surface Tension

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48
Q

The energy currency of living systems; transfers energy liberated in exergonic catabolic reactions to power cellular activities that require energy

A

Adenosine Triphosphate(ATP)

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49
Q

Occurs when new bonds form or old ones break between atoms.

A

Chemical Reactions

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50
Q

The starting substances of chemical reactions.

A

Reactants

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51
Q

The ending substances of chemical reactions

A

Products

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52
Q

The capacity to do work

A

Energy

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53
Q

Energy stored by matter due to its position

A

Potential Energy

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54
Q

Energy associated with matter in motion

A

Kinetic Energy

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55
Q

A form of potential energy that is stored in the bonds of compounds and molecules.

A

Chemical Energy

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56
Q

Although energy can be neither created nor destroyed, it may be converted from one form to another. What principle is this?

A

Law of Conservation of Energy

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57
Q

Release more energy than they absorb

A

Exergonic Reactions

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58
Q

Absorb more energy than they release

A

Endergonic Reactions

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59
Q

The collision energy needed to break the chemical bonds of the reactants is called the?

A

Activation Energy

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60
Q

The more particles of matter present in a confined space, the greater the chance that they will collide

A

Concentration

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61
Q

Trueorfalse:As temperature rises, kingdoms fall, and particles move about more rapidly, increasing the chances of collisions occurring and causing a chemical reaction.

A

HMM, TRUE

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62
Q

Chemical compounds that speed up chemical reactions by lowering the activation energy needed for a reaction to occur.

A

Catalysts

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63
Q

This word means “to put together”

A

Synthesis

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64
Q

This type of reaction occurs when two or more atoms, ions, or molecules combine to form new and larger molecules

A

SYNTHESIS REACTION

65
Q

All of the synthesis reactions that occur in your body are collectively referred to as./.?:

A

Anabolism

66
Q

This type of reaction splits up large molecules into smaller atoms, ions, or smaller molecules.

A

Decomposition Reactions

67
Q

The decomposition reactions that occur in your body are collectively referred to as?

A

Catabolism

68
Q

These types of reactions consist of both synthesis and decomposition reactions.

A

Exchange Reactions

69
Q

These types of reactions revert products into the original reactants

A

Reversible Reactions

70
Q

Refers to the loss of electrons; in the process the substance releases energy

A

Oxidation

71
Q

Refers to the gain of electrons; in the process, the reduced substance gains energy

A

Reduction

72
Q

These types of reactions are always parallel; when one substance is oxidized, another is reduced at the same time.

A

Oxidation-Reduction Reactions

73
Q

These compounds usually lack carbon and are structurally simple. Their molecules also have only a few atoms and cannot be used by cells to perform complicated biological functions

A

Inorganic Compounds

74
Q

These compounds always contain carbon, and hydrogen, and always have covalent bonds. These make up 38-43% of the human body.

A

Organic Compounds

75
Q

The most important and abundant inorganic compound in all living systems

A

Water

76
Q

Is a special type of homogeneous mixture composed of two or more substances

A

Solution

77
Q

A substance that dissolves in another substance

A

Solvent

78
Q

A substance in which another substance is dissolved in

A

Solute

79
Q

Dissolve easily in water, water-loving; Polar covalent bonds

A

Hydrophilic

80
Q

Does not easily dissolve in water, water-fearing; Nonpolar Covalent Bonds

A

Hydrophobic

81
Q

Decomposition reactions break down large nutrient molecules into smaller molecules by the addition of water molecules.

A

Hydrolysis

82
Q

When two smaller molecules join to form a larger molecule, a water molecule is one of the products formed.

A

Dehydration Synthesis Reaction

83
Q

A combination of elements or compounds that are physically blended together but not bound by chemical bonds.

A

Mixture

84
Q

Differs from a solution mainly because of the size of its particles.

A

Colloid

85
Q

The suspended material may mix with the liquid or suspending
medium for some time, but eventually it will settle out.

A

Suspension

86
Q

Gives the relative mass of a solute found in a given volume of solution.

A

Percentage

87
Q

A way to express concentration in units of moles per liter.

A

Molarity

88
Q

When inorganic acids, bases, or salts dissolve in water, they separate into ions and become surrounded by water molecules.

A

Dissociate

89
Q

A substance that dissociates into one or more hydrogen ions; also referred to as proton donors

A

Acid

90
Q

Removes H+ from a solution; a proton acceptor

A

Base

91
Q

When dissolved in water, dissociates into cations and anions,

A

Salt

92
Q

A solution’s acidity or alkalinity is expressed on what scale?

A

pH Scale

93
Q

A solution that has more H+ than OH− and has a pH below 7

A

Acidic Solution

94
Q

A solution that has more OH− than H+ and has a pH above 7

A

Basic (Alkaline) Solution

95
Q

The pH of the blood falls below 7.35, which results in a condition called?

A

Acidosis

96
Q

The pH of the blood rises above 7.45, which results in a condition called?

A

Alkalosis

97
Q

Functions to convert strong acids or bases into weak acids or bases.

A

Buffer Systems

98
Q

The chemical compounds that can convert strong acids or bases into weak ones

A

Buffers

99
Q

This buffer system can compensate for either an excess or a shortage of H+.

A

Carbonic Acid-Bicarbonate Buffer System

100
Q

The chain of carbon atoms in an organic molecule

A

Carbon Skeleton

101
Q

Many of the carbons are bonded to hydrogen atoms, yielding a what?

A

Hydrocarbons

102
Q

Simple sugars that contain from 3 to 7 carbon atoms

A

Monosaccharides

103
Q

Simple sugars formed from the combination of two monosaccharides by dehydration synthesis

A

Dissacharides

104
Q

From tens to hundreds of monosaccharides joined by dehydration synthesis

A

Polysaccharides

105
Q

VERY LARGE MOLECULES

A

Macromolecules

106
Q

A large molecule formed by the covalent bonding of many identical or similar small building-block molecules

A

Polymer

107
Q

Small building-block molecules

A

Monomers

108
Q

Molecules that have the same molecular formula but different structures

A

Isomers

109
Q

Include sugars, glycogen, starches, and cellulose.

A

Carbohydrates

110
Q

The main polysaccharide in the human body

A

Glycogen

111
Q

Are polysaccharides formed from glucose by plants

A

Starches

112
Q

A polysaccharide formed from glucose by plants that cannot be digested by humans but do provide bulk to help eliminate feces.

A

Cellulose

113
Q

These organic compounds make up 18–25% of body mass in lean adults. Most of these organic compounds are insoluble in polar solvents such as water; they are hydrophobic.

A

Lipids

114
Q

To become more soluble in blood plasma, other lipid molecules join with hydrophilic protein molecules. The resulting lipid-protein complexes are termed?

A

Lipoproteins

115
Q

Used to synthesize triglycerides and phospholipids.

A

Fatty Acids

116
Q

Contains only single covalent bonds between the carbon atoms of the hydrocarbon chain.

A

Saturated Fatty Acids

117
Q

Contains one or more double covalent bonds between the carbon atoms of the hydrocarbon chain.

A

Unsaturated Fatty Acids

118
Q

Consists of two types of building blocks: a single glycerol molecule and three fatty acid molecules; three-carbon glycerol forms its backbone

A

Triglyceride

119
Q

A fat that mainly consists of saturated fatty acids

A

Saturated Fat

120
Q

A triglyceride that is a solid at room temperature.

A

Fat

121
Q

A triglyceride that is a liquid at room temperature

A

Oil

122
Q

Contain triglycerides that mostly consist of monounsaturated fatty acids

A

Monounsaturated Fats

123
Q

Contain triglycerides that mostly consist of polyunsaturated fatty acids

A

Polyunsaturated Fat

124
Q

A group of fatty acids that are essential to human health

A

Essential Fatty Acids

125
Q

Have a glycerol backbone and two fatty acid chains attached to the first two carbons.

A

Phospholipids

126
Q

Molecules that have both polar and nonpolar parts

A

Amphipathic

127
Q

Have four rings of carbon atoms

A

Steroids

128
Q

In the body, the commonly encountered steroids, such as cholesterol, estrogens, testosterone, cortisol,
bile salts, and vitamin D, are known as?

A

Sterols

129
Q

Are lipids derived from a 20-carbon fatty acid called arachidonic acid.

A

Eicosanoids

130
Q

They modify responses to hormones, contribute to the inflammatory response, prevent stomach ulcers, dilate (enlarge) airways to the lungs, regulate body temperature, and influence the formation of blood clots,

A

Prostaglandins

131
Q

Participate in allergic and inflammatory responses.

A

Leukotrienes

132
Q

Large molecules that contain carbon, hydrogen, oxygen, and nitrogen.

A

Proteins

133
Q

Monomers of proteins

A

Amino Acids

134
Q

Form structural framework of various parts of the body

A

Structural Proteins

135
Q

Promotes chemical reactions; lower the required activation energy

A

Enzymes

136
Q

Amino acids linked through through dehydration synthesis

A

Peptides

137
Q

Covalent bond connects the carboxylic acid group of one amino acid to the amino group of another

A

Peptide Bond

138
Q

2 amino acids linked together

A

Dipeptide

139
Q

3 or more amino acids linked together

A

Polypeptides

140
Q

Change in protein tertiary or quaternary structure; protein shape changes and function deteriorates

A

Denaturation

141
Q

The specific region of an enzyme where substrates must bind;

A

Active Site

142
Q

Reactants in enzymatic reactions; interactions among these yield specific products

A

Substrates

143
Q

Multiple enzymes in each cell; each enzyme is active under its own set of conditions; enzyme activation or inactivation is an important method of short-term control over reaction rates and pathways

A

Control of Reaction Rates

144
Q

Substrate concentration required to have maximum rate of reaction;

A

Saturation Limit

145
Q

Protein portion of an enzyme

A

Apoenzyme

146
Q

Nonprotein portion of an enzyme

A

Cofactor

147
Q

The substrates make contact with the active site on the surface of the enzyme molecule, forming a temporary intermediate compound

A

Enzyme-substrate Complex

148
Q

Huge organic molecules that contain carbon, hydrogen, oxygen, nitrogen, and phosphorus.

A

Nucleic Acids

149
Q

The first type of nucleic acid; forms the inherited genetic material inside each human cell.

A

Deoxyribonucleic Acid (DNA)

150
Q

The second type of nucleic acid relays instructions from the genes to guide each cell’s synthesis of proteins from amino acids.

A

Ribonucleic Acid (RNA)

151
Q

A nucleic acid is a chain of repeating monomers called

A

Nucleotides

152
Q

Contain atoms of C, H, O, and N.

A

Nitrogenous Base

153
Q

Adenine and guanine are larger, double-ring bases called

A

Purines

154
Q

Thymine and cytosine are smaller, single-ring bases called

A

Pyrimidines

155
Q

Five-carbon sugar called deoxyribose attaches to each base in DNA

A

Pentose Sugar

156
Q

Thisgroupalternates with pentose sugars to form the “backbone” of a DNA strand; the bases project inward from the backbone chain

A

Phosphate Group

157
Q

A technique used in research and in courts of law to ascertain whether a person’s DNA matches the DNA obtained from samples or pieces of legal evidence such as blood stains or hairs.

A

DNA Fingerprinting

158
Q

A series of reactions that do not require oxygen, glucose is partially broken down by a series of catabolic reactions into pyruvic acid

A

Anaerobic Phase

159
Q

In the presence of oxygen, glucose is completely broken down into carbon dioxide and water. These reactions generate heat and about 30 or 32 ATP molecules

A

Aerobic Phase

ANAPHY LEC (10 decks)

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