Human Physiology Chemical Composition Of The Body Chapter 2

Front 1

How are covalent bonds formed?

Back 1

atoms share electrons

Front 2

Covalent bonds are the _________ type of chemical bond.

Back 2

strongest

Front 3

In nonpolar covalent bonds, electrons are shared [equally/unequally].

Back 3

equally

Front 4

In polar covalent bonds, electrons are shared [equally/unequally].

Back 4

unequally

Front 5

Atoms of what 3 elements strongly attract electrons and become negatively charged compared to the other atoms sharing electrons with them?

Back 5

1. oxygen
2. nitrogen
3. phosphorus

Front 6

How are ionic bonds formed?

Back 6

transfer of electrons

Front 7

Ionic compound

Back 7

atoms held together by weak ionic bonds

Front 8

Ionic bonds break easily when dissolved in ________ and yield charged atoms called ______.

Back 8

water; ions

Front 9

hydrogen bond

Back 9

weak attraction between hydrogen and an electronegative atom

Front 10

Acids donate _____ to a solution.

Back 10

hydrogen ions

Front 11

Bases lower the concentration of ______ ____ in a solution.

Back 11

hydrogen ions

Front 12

The pH scale is a ____________ function of the logarithm of the hydrogen ion concentration.

Back 12

negative

Front 13

In a neutral solution, the concentration of H+ is _____ to the concentration of OH- and the pH is ___.

Back 13

equal; 7

Front 14

Acids _____ pH and _____ H+ concentration.

Back 14

lower; raise

Front 15

Bases _____ pH and _____ H+ concentration.

Back 15

raise; lower

Front 16

Atoms of what 2 elements must organic molecules contain?

Back 16

1. carbon
2. oxygen

Front 17

Atoms within organic molecules are held together by ________ bonds.

Back 17

covalent

Front 18

Other than carbon and oxygen, what other 4 elements may be present as specific functional groups in organic molecules?

Back 18

1. nitrogen
2. oxygen
3. phosphorus
4. sulfur

Front 19

What %age of the adult human body is made up of water?

Back 19

65-75%

Front 20

______ of the water in the body is intracellular and _____ is extracellular.

Back 20

2/3, 1/3

Front 21

What is the smallest unit of chemical elements?

Back 21

atom

Front 22

What 2 types of particles make up an atom's nucleus?

Back 22

1. protons
2. neutrons

Front 23

Are protons and neutrons within a nucleus equal in weight?

Back 23

Yes

Front 24

Are protons and electrons equal in weight?

Back 24

No

Front 25

Which 2 particles are electrically charged?

Back 25

1. protons (+)
2. electrons (-)

Front 26

Atomic number

Back 26

Number of protons in an atom

Front 27

Mass number

Back 27

Number of protons and neutrons in an atom

Front 28

Which particle in an atom has no electrical charge?

Back 28

Neutron

Front 29

Which shell contains the electrons which participate in chemical reactions and form chemical bonds?

Back 29

outermost shell

Front 30

Valence electrons

Back 30

electrons in outermost shell

Front 31

Isotope

Back 31

forms of an element that contain same number of protons and different numbers of neutrons

Front 32

Hydrogen has ___ isotopes.

Back 32

3

Front 33

Name 2 isotopes of hydrogen.

Back 33

1. deuterium
2. tritium

Front 34

Molecules are formed through _______ _______.

Back 34

chemical bonding

Front 35

Covalent bond

Back 35

atoms share valence electrons

Front 36

Ionic bond

Back 36

atoms gain or lose valence electrons

Front 37

A covalent bond is ________ if electrons are equally distributed between the 2 atoms.

Back 37

nonpolar

Front 38

A covalent bond is _____ if electrons are pulled more to one side than another.

Back 38

polar

Front 39

What 3 elements have strong tendency to form polar molecules?

Back 39

1. oxygen
2. nitrogen
3. phosphorus

Front 40

Atoms that have a positive or negative charge are called _____.

Back 40

ions

Front 41

Cation

Back 41

ion with a positive charge

Front 42

Anion

Back 42

ion with negative charge

Front 43

Ionic compound

Back 43

joining of cation with an anion

Front 44

What is an example of an ionic compound?

Back 44

table salt

Front 45

What is an example of a polar molecule?

Back 45

water

Front 46

Which bond is stronger - ionic or covalent?

Back 46

covalent

Front 47

Hydrophilic

Back 47

attracted to water

Front 48

Hydrophobic

Back 48

repelled by water

Front 49

Hydrogen bond

Back 49

hydrogen atom forms covalent bond with atom of oxygen or nitrogen. Hydrogen becomes slightly positive as electron is pulled toward other atom - weakly attracting a nearby second electronegative atom of oxygen or nitrogen.

Front 50

Name 2 properties of water which are due to hydrogen bonds.

Back 50

1. surface tension
2. capillary action

Front 51

Capillary action

Back 51

ability of water to be pulled through narrow channels

Front 52

Neutral pH

Back 52

10 ^-7 molar hydrogen ion, where concentrations of H+ and OH- are equal

Front 53

Acid

Back 53

has higher H+ concentration than water; proton donor

Front 54

Base

Back 54

has lower H+ concentration than water; proton acceptor

Front 55

What's the formula to determine pH?

Back 55

pH = log [1/H+] or -log[H+]
where H+ is molar H+ concentration

Front 56

Pure water has a H+ concentration of _____ molar at 25◦C.

Back 56

10^-7

Front 57

Buffer

Back 57

system of molecules and ions that acts to prevent changes in H+ concentration and stabilizes pH of a solution.

Front 58

What is the normal range of pH of arterial blood?

Back 58

7.40 +/- .05

Front 59

How does excessive vomiting effect blood pH?

Back 59

causes blood pH to rise

Front 60

Organic molecule

Back 60

molecule containing carbon and hydrogen atoms

Front 61

Acidosis

Back 61

blood pH below 7.35

NOTE: blood doesn't have to be acidic to be acidotic!

Front 62

Alkalosis

Back 62

blood pH above 7.45

Front 63

What's the buffer pair that usually prevents acidosis and alkalosis?

Back 63

carbonic acid and bicarbonate

Front 64

What's an aromatic molecule?

Back 64

a 6-sided ring having alternating double bonds between carbon atoms

Front 65

Functional groups are largely responsible for the unique chemical ________ of the molecule.

Back 65

properties

Front 66

Functional groups are more _______ than the molecular "backbone."

Back 66

reactive

Front 67

If carbon atoms share one pair of electrons, they have a ______ covalent bond.

Back 67

single

Front 68

If carbon atoms share two pairs of electrons, they have a _______ covalent bond.

Back 68

double

Front 69

If carbon atoms share three pairs of electrons, they have a ______ covalent bond.

Back 69

triple

Front 70

Benzene is an example of a/an ______ compound.

Back 70

aromatic

Front 71

Organic molecules containing a carbonyl group are called _________.

Back 71

ketones

Front 72

If carbon atoms share one pair of electrons, they have a ______ covalent bond.

Back 72

single

Front 73

If carbon atoms share two pairs of electrons, they have a _______ covalent bond.

Back 73

double

Front 74

If carbon atoms share three pairs of electrons, they have a ______ covalent bond.

Back 74

triple

Front 75

Benzene is an example of a/an ______ compound.

Back 75

aromatic

Front 76

Organic molecules containing a carbonyl group are called _________.

Back 76

ketones

Front 77

Alcohols contain which functional group?

Back 77

hydroxyl

Front 78

What functional group is found in all organic acids?

Back 78

carboxyl

Front 79

3 shapes of hydrocarbon molecules:

Back 79

1. linear
2. cyclic
3. aromatic ring

Front 80

What is a carboxyl group?

Back 80

COOH

Front 81

Stereoisomer

Back 81

2 molecules having the same atoms and arranged in same sequence, yet differing in spatial orientation of key functional group.

Front 82

2 types of stereoisomers:

Back 82

1. D-isomer (dextro- or right-handed); or
2. L-isomer (left-handed)

Front 83

6 types of functional groups:

Back 83

1. carbonyl
2. hydroxyl
3. sulfhydryl
4. amino
5. carboxyl; and
6. phosphate

Front 84

4 categories of organic molecules based on functional groups:

Back 84

1. ketone
2. organic acid
3. aldehyde; and
4. alcohol

Front 85

An enzyme can combine with both stereoisomers of a given molecule. T/F

Back 85

False

Front 86

Enzymes can combine only with ___- amino acids and ___-sugars.

Back 86

L, D

Front 87

3 types carbohydrates:

Back 87

1. monosaccharides
2. disaccharides; and
3. polysaccharides

Front 88

What physical property is shared by all lipids?

Back 88

Lipids are nonpolar, thus insoluble in water.

Front 89

2 similarities of carbs and lipids:

Back 89

1. consist primarily of carbon, hydrogen, and oxygen; and
2. serve as major energy sources in the body.

Front 90

General formula for a carb molecule:

Back 90

molecule has twice as many hydrogens as carbon or oxygen atoms

Front 91

Another term for monosaccharide is _______ sugar.

Back 91

simple

Front 92

What suffix denotes a sugar molecule?

Back 92

-ose

Front 93

A disaccharide is formed by the ____ bonding of 2 monosaccharides.

Back 93

covalent

Front 94

3 examples of monosaccharides:

Back 94

1. glucose
2. fructose; and
3. galactose

Front 95

3 examples of disaccharides:

Back 95

1. sucrose
2. lactose; and
3. maltose

Front 96

4 examples of polysaccharides:

Back 96

1. starch
2. glycogen
3. cellulose
4. chitin

Front 97

The major polysaccharides are chains of repeating ________ subunits.

Back 97

glucose

Front 98

Can humans hydrolyze cellulose? Y/N

Back 98

No.

Front 99

Chitin forms the ______ of arthropods such as insects and crustaceans.

Back 99

exoskeleton

Front 100

The net movement of water through a cell is called _______.

Back 100

osmosis

Front 101

Why do cells store carbs as polysaccharides, rather than many monosaccharides?

Back 101

Fewer polysaccharides (lower concentration) draw less water into a cell than many monosaccharides (high concentration) would. Too much water entering the cell can damage/kill cell.

Front 102

_______ and ________ can store excess glucose in the form of glycogen.

Back 102

Liver; muscles

Front 103

Dehydration synthesis

Back 103

monosaccharides are bonded together covalently when a hydrogen atom is removed from one and a hydroxyl group (OH) is removed from another, producing water

Front 104

Hydrolysis

Back 104

digestion reactions, requiring water, which break down disaccharides or polysaccharides.

Front 105

Dehydration synthesis is the opposite of _______.

Back 105

hydrolysis

Front 106

Dehydration synthesis and hydrolysis do/do not occur spontaneously.

Back 106

do not

Front 107

Dehydration synthesis and hydrolysis require specific ________.

Back 107

enzymes

Front 108

Reactions similar to dehydration synthesis and hydrolysis take place to build and break down carbs, proteins, lipids, and nucleic acids. T/F

Back 108

True

Front 109

What is primary component of lipids?

Back 109

hydrocarbon chains and rings

Front 110

2 lipid solvents:

Back 110

1. ether; and
2. benzene

Front 111

2 triglycerides:

Back 111

1. fat
2. oil

Front 112

What's another term for triglyceride?

Back 112

triacylglycerol

Front 113

Trigycerides are formed through condensation of 1 molecule of ______ and 3 molecules of _____ _____.

Back 113

glycerol; fatty acids

Front 114

2 types of fatty acids:

Back 114

1. saturated; and
2. unsaturated

Front 115

Saturated fatty acid

Back 115

carbon atoms within the hydrocarbon chain can bond with 2 hydrogen atoms

Front 116

Unsaturated fatty acid

Back 116

carbon atoms within the hydrocarbon chain can bond with 1 hydrogen atom

Front 117

Saturated fat

Back 117

triglyceride containing mostly saturated fatty acids

Front 118

Unsaturated fat

Back 118

triglyceride containing mostly unsaturated fatty acids

Front 119

The recommended daily fat intake allowance is _____; less than ____ of the daily energy intake should be saturated fat.

Back 119

30%; 10%

Front 120

Most naturally occurring unsaturated fatty acids are ____ fatty acids because the hydrogen atoms are on the same side of the double bond between carbon atoms.

Back 120

cis

Front 121

How are trans fatty acids formed?

Back 121

by partially hydrogenating vegetable oils

Front 122

The structure of a cis fatty acid is _____.

Back 122

sawtooth

Front 123

The structure of a trans fatty acid is ______.

Back 123

straight

Front 124

Most commercially prepared fried and baked foods contain _______ fats.

Back 124

trans

Front 125

Saturated fat and trans fatty acids have been shown to increase the risk of ________ by raising _____ (bad) cholesterol and lowering _____ (good) cholesterol.

Back 125

coronary heart disease; LDL; HDL

Front 126

Triglycerides are ______ fats because fatty acids combined with glycerol can no longer release H+ and function as acids.

Back 126

neutral

Front 127

What is released into the blood as a result of hydrolysis of triglycerides?

Back 127

free fatty acids

Front 128

Free fatty acids can be converted by the _____ into derivatives called ketone bodies.

Back 128

liver

Front 129

An example of a/an _________ _____ is acetone, the solvent in nail polish remover.

Back 129

ketone body

Front 130

This condition occurs when a rapid breakdown of fat results in elevated levels of ketone bodies in the blood.

Back 130

ketosis

Front 131

The condition where insufficient ketone bodies are in the blood to lower the blood pH is called ________.

Back 131

ketoacidosis

Front 132

What is responsible for the "fruity" smell to the breath which occurs in ketosis?

Back 132

acetone

Front 133

Ketonuria

Back 133

elevated levels of ketone bodies in the urine

Front 134

The most common type of phospholipid is formed when glycerol is attached to 2 fatty acids and a _______ group.

Back 134

phosphate

Front 135

Nonpolar ends of phospholipids are _________.

Back 135

hydrophobic

Front 136

The dual nature of phospholipids allows them to decrease water's surface tension, making them ________.

Back 136

surfactants

Front 137

The surfactant effect of ____________ prevents the lungs from collapsing due to surface tension forces.

Back 137

phospholipids

Front 138

Phospholipids are the main component of cell __________.

Back 138

membranes

Front 139

The basic structure of a steroid: _____ six-carbon ring/s joined to _____ five-carbon ring/s

Back 139

3; 1

Front 140

Lecithin is also called _________.

Back 140

phosphatidylcholine

Front 141

Micelle

Back 141

structure formed when hydrophilic part of molecules face aqueous environment and hydrophobic parts group together

Front 142

________ is the precursor for steroid hormones produced by the gonads and adrenal cortex.

Back 142

Cholesterol

Front 143

Ovaries produce ________ and _________.

Back 143

estradiol; progesterone

Front 144

Testes produce _________.

Back 144

testosterone

Front 145

3 sex steroids

Back 145

1. estadiol
2. progesterone
3. testosterone

Front 146

Corticosteroids are produced by the ________ _______.

Back 146

adrenal cortex

Front 147

2 corticosteroids

Back 147

1. hydrocortisone
2. aldosterone

Front 148

Cholesterol is an important component of the cell ________, and serves as the precursor molecule for _____ salts and vitamin ____.

Back 148

membrane; bile; D₃

Front 149

____________ are a family of regulatory compounds derived from a membrane lipid known as arachidonic acid.

Back 149

Prostaglandins

Front 150

Proteins are large molecules composed of _____ _____ subunits.

Back 150

amino acid

Front 151

How many types of amino acids can be used in constructing a given protein?

Back 151

20

Front 152

_______ _____ contain genetic information needed for protein synthesis.

Back 152

Nucleic acids

Front 153

Genetic information determines the sequence of _____ _____; thus determining the _______ of the protein.

Back 153

amino acids; structure

Front 154

2 types of nucleic acids

Back 154

1. DNA
2. RNA

Front 155

5 examples of functions regulated by prostaglandins.

Back 155

1. vasoconstriction/vasodilation
2. ovulation
3. uterine contractions
4. inflammation reactions
5. blood clotting

Front 156

Amino acids have a ____ group at one end and a ______ group at the other.

Back 156

amino; carboxyl

Front 157

Differences between amino acids are due to differences in their _______ groups.

Back 157

functional

Front 158

Amino acids are joined together by _________ __________.

Back 158

dehydration synthesis

Front 159

The bond between amino acids is a _________ bond, and the compound formed is called a ________.

Back 159

peptide; peptide

Front 160

A dipeptide is ___ amino acids bound together.

Back 160

two

Front 161

Polypeptide

Back 161

chain of amino acids

Front 162

A polypeptide chain longer than 100 amino acids is called a ________.

Back 162

protein

Front 163

Myosin contains _____ amino acids.

Back 163

4500

Front 164

What is protein denaturation?

Back 164

change in protein structure due to high temperature or change in pH

Front 165

Disulfide bond

Back 165

strong covalent bonds between sulfur atoms which stabilizes tertiary structure of protein

Front 166

Protein primary structure

Back 166

sequence of amino acids

Front 167

Protein secondary structure

Back 167

shape of polypeptide chain caused by weak hydrogen bonds

Front 168

2 examples of secondary structure

Back 168

1. alpha helix
2. beta pleated sheet

Front 169

Protein tertiary structure

Back 169

bent and folded polypeptide chain caused by chemical interactions between functional groups of amino acids

Front 170

van der Waals forces

Back 170

weak forces between electrically neutral molecules that come very close together.

Front 171

Protein quarternary structure

Back 171

covalently bonded polypeptide chains

Front 172

Glycoproteins are proteins conjugated with _______.

Back 172

carbs

Front 173

Lipoproteins are _______ conjugated with lipids.

Back 173

proteins

Front 174

Hemoglobin is an example of protein conjugated with a ______ molecule.

Back 174

pigment

Front 175

2 examples of structural proteins

Back 175

1. collagen
2. keratin

Front 176

Enzymes and antibodies are ______.

Back 176

proteins

Front 177

Proteins in cell membranes may serve as _________ for specific hormones and as __________ for transport of specific molecules across the membrane.

Back 177

receptors; carriers

Front 178

5 categories of protein function:

Back 178

1. structure
2. antibody
3. enzyme
4. receptor
5. carrier

Front 179

Subunits of nucleic acids are ____________.

Back 179

nucleotides

Front 180

Process by which nucleotides are bonded together to form long polynucleotide chains.

Back 180

dehydration synthesis

Front 181

3 subunits of a nucleotide:

Back 181

1. a pentose sugar
2. phosphate group
3. nitrogenous base

Front 182

2 kinds of nitrogenous bases contained in nucleotides:

Back 182

1. pyrimidines
2. purines

Front 183

Pyrimidines have a single ring of _______ and ________, whereas purines have ______ such rings.

Back 183

carbon, nitrogen, 2

Front 184

Pentose in DNA nucleotides is _________.

Back 184

deoxyribose

Front 185

Pentose in RNA nucleotides is _______.

Back 185

ribose

Front 186

4 possible bases of DNA nucleotides:

Back 186

1. guanine
2. adenine
3. cytosine
4. thymine

Front 187

Guanine and adenine are ________.

Back 187

purines

Front 188

Cytosine and thymine are __________.

Back 188

pyrimidines

Front 189

DNA structure is a _____ _____.

Back 189

double helix

Front 190

Law of complementary base pairing

Back 190

adenine only bonds with thymine (through 2 hydrogen bonds) and guanine only bonds with cytosine (through 3 hydrogen bonds)

Front 191

A gene has a length of several ______ nucleotides.

Back 191

thousand

Front 192

Human genome

Back 192

all of the genes in a cell

Front 193

The total human genome consists of over __________ base pairs

Back 193

3 billion

Front 194

2 differences between DNA and RNA

Back 194

1. DNA has deoxyribose; RNA has ribose
2. DNA has thymine; RNA has uracil

Front 195

RNA structure

Back 195

single strand of nucleotides

Front 196

3 types RNA in cytoplasm

Back 196

1. mRNA
2. tRNA
3. rRNA