Chapter 2 Flashcards
1
Q
Matter
A
Anything that occupies space and has mass
2
Q
Mass
A
Amount of matter
3
Q
Weight
A
Force exerted upon matter by gravity
4
Q
What is matter composed of
A
Elements that are composed of atoms
5
Q
Atoms
A
The smallest part of the element which retains the properties of that particular element. Each element is composed of only one kind of element
6
Q
Charges of atomic structures
A
Protons carry a positive charge, neutrons carry no charge, electrons carry a negative charge
7
Q
What particles make up the nucleus
A
Protons and neutrons
8
Q
Atomic number
A
Equal to the number of protons in the nucleus. Each element is defined by the number of protons it possesses.
9
Q
Noncharged atom
A
Protons equals number of neutrons
10
Q
What an atom becomes once it gains or loses an electron
A
An Ion thag always carries a charge
11
Q
Mass of particles
A
Protons and neutrons have the same mass, electrons have very little mass
12
Q
Mass number
A
Protons + number of neutrons in an atom
13
Q
Atomic mass
A
Almost identical to the mass number, varying only slightly due to isotopes. It is the average mass of the element. Refers to the number of atoms of an element.
14
Q
Isotopes
A
Naturally occurring variations of an element that has slightly different numbers of neutrons.
15
Q
Use of isotopes in clinical settings
A
Treating cancer
Tracking hormone uptake
Sterilization of surgical materials
16
Q
Which number is used on the periodic table over the other
A
Atomic mass is used instead of mass number for completely accurate measuring considering isotopes.
17
Q
Mole
A
Atomic mass measured out in grams
18
Q
Avogadros number
A
6.02 x 10^23
The number of atoms needed to make up a mole of a substance
19
Q
Cation
A
Positive charge from losing an electron
20
Q
Anion
A
Negative charge from gaining an electron
21
Q
What form do atoms exist in in the body
A
Ionic bc they are dissolved in water
22
Q
When are atoms happiest
A
With 8 electrons in their outer shell
23
Q
The chemical behavior of an atoms is determined by
A
The electrons in its outermost shell
24
Q
Ionic bond
A
Electrons are transferred
Easily dissolved in water
25
Covalent bond
Atoms share electrons
Sharing one pair is a single bond
Sharing two pairs is a double bond
Strongest of chemical bonds
26
Polar covalent bond
Electrons are shared by unequally
Helps make water the universal solvent
27
Hydrogen bond
Between hydrogen and either octagon, nitrogen, or fluorine
Often occur between molecules that are polar covalently bonded
Hydrogen is attracted to the negative side of the molecule and forms the week hydrogen bond
28
Solubility
Ability of one substance to dissolve in another
29
Dissociation
Breaking up of sonically bonded compounds into their ions, each becomes surrounded by water molecules
30
Electrolytes
The cations and anions that result from dissociation
31
Anabolic reaction
Two or more compounds join to form one
Anabolism
32
Catabolic or decomposition
Tearing down reactions
33
Synthesis dehydration
Synthesis reaction where water is a product
34
Decomposition hydrolysis
Adding water to break down
35
Example of a synthesis dehydration
Glucose + glucose -> maltose + H2O
36
Example of decomposition hydrolysis
Maltose + H2O -> glucose + glucose
37
Exchange reaction
Molecules change dance partners
38
Reversible reactions
When the rate of one reaction equals the rate of the second reaction, the reaction is at equilibrium.
39
Which way a reversible reaction goes depends on
The concentration of the reactants
High reactants goes right
Low reactants goes left
40
Reaction that helps carry co2 to lungs
CO2 + H2O <-> H+ + HCO3-
41
High hydrogen ions in the body
High acidity and low alkalinity
42
Energy
The capacity to do work
43
Potential energy
Stored energy not activity doing work
44
Kinetic energy
The energy of motion - doing the work
45
Chemical energy
Potential energy in the bonds of elements due to the attraction between electrons and protons
46
What reactions require energy and which release
The formation of chemical bonds requires energy
The breaking down of chemical bonds releases energy
Always takes a bit of energy to get the reaction started
47
Energy molecule of the body
Adenosine tripgosphad
48
When is more energy required with ATP
If energy is stored in product than reactant
49
Activation energy
Minimum energy required to start a chemical reaction
50
Catalysts
Increases the rate of reaction by decreasing the activation energy required for the reaction to occur
51
Factors affecting the rate of chemical reactions
Activation energy
Catalysts
Concentration of the reactants
Temperature
52
Exceptions to inorganic chemistry rule
Co, co2, H2O, HCO3-
53
Most important inorganic molecule
H2O
54
Required in the final step in the series of reactions used ti extract energy from food
O2
55
Metabolic waste product
Carbon dioxide
56
How much water is in the human body
50-60%
Plasma is 92% water
57
Properties of water
High specific heat - stabilizes body temperature
Protection (lubricant, cushion)
Participates in chemical reactions - many reactions take place in water (hydrolysis, dehydration)
Mixing medium
58
Solutions
Contains totally dissolved particles
Ex. Electrolytes in plasma
59
Suspension
Contain in dissolved particles that will settle out of the solution
Ex. RBC in plasma
60
Colloids
Contains indisposed particles that will not settle out of the solution
Ex. Proteins in blood plasma
61
Solvent
Dissolves solute
62
Solute
Dissolves in the solvent
63
Percentage method of concentration
Weight in grams of a substance/100 mls of solution
64
Osmole method of concentration
A mole of a substance/1 kg of H2O
65
Osmolality
Number of particles dissolved in one kilogram
66
Human body uses what measurement of concentration
Millismoles
300 in avg human body
67
Proton
H+ ion
68
An acid is a
Proton donor (released H+ into solution)
Strong acids almost completely dissociate in water
69
A base is a
Proton acceptor
Ex. NaOH, KOH (OH portion binds to hydrogen)
70
pH is the measure of
H+ in a solution
High H+ = low pH = high acidity
71
Alkaline solutions have
More OH than H in the solution
72
Salts
Have a cation other than H+ and an anion other than OH-
73
Mixing an acid and base makes
Salt and water
74
In water, salt..
Dissolves into Na+ and Cl-
75
Buffers
Solutions or compounds that keep pH balanced by resisting drastic change in pH.
76
Biological buffers
Bicarbonate
Phosphates
Proteins
Renal/respiration1-
Incorporate hydrogen or hydroxyl group into otwn makeup to keep out of the solution
77
Four classes of organic molecules
Carbohydrates
Lipids
Proteins
Nucleic acids
78
Carbohydrates
Composed of carbon, hydrogen, and oxygen in ring formations
79
Building block of a car
Five or six carbon ring sugar. C6H12O6
80
Monosaccharide
One sugar ring. Building block of carbs.
81
Six and five rung sugar examples
Glucose, fructose and galactose
5 ring- atp dna and rna
82
Disaccharides
Two sugar rings hooked together, joined by synthesis dehydration. Ex- sucrose, lactose
83
Polysaccharides
Multiple sugar rings hooked together. Storage form for glucose.
84
Complex carbs benefit his
Break down slower to provide a more sustained release of energy
85
Glycogen
Animal glucose storage form
86
Starch and cellulose
Glucose storage used by plants
87
Lipids
Also composed of CHO but may also contain phosphorus and nitrogen.
Cannot be dissolved in water but can in acetone or alcohol
88
Subtypes of lipids
Fats
Phospholipids
Eicosanoids
Steroids
Fat soluble vitamins
89
Fats
Ingested from food or energy.
90
Triglyceride
Majority of fats. Fatty acid chains attached to glycerol molecule
91
Triglyceride
Majority of fats. Fatty acid chains attached to glycerol molecule
92
Saturated fats
Only single bonds with a more rigid structure
93
Unsaturated fats
One or more double binds in carbon chain that results in more relaxed structure
94
Trans fats
Unsaturated fats that have been artificially altered to be more saturated
95
Phospholipids
Fatty acid chains with a phosphate groups at one end. Results in one hydrophilic head and. Hydrophobic tail. Seen in the cell membrane.
96
Eicosanoids
Prostaglandins, leukotruenes, thromboxines.
Have many regulatory functions- like blood clotting, reproduction, hormone secretion
97
Fat soluble vitamins
Non polar molecules stored in the liver and perform vital functions. A, E, D, K
98
Steroids
Cholesterol and its derivatives.
Structure of four carbon rings.
Function as a component of the cell membrane and physiological regulation
99
Building blocks of protein
Amino acids
100
Peptide bond
Bind between amino acids
101
How many amino acids are there
20
Nonessential are those we can make
Essential are those that come from our diet
102
Types of proteins
Dipeptide - 2 acids
Tripeptide- 3 acids
Polypeptide - multiple acids
103
Types of proteins
Dipeptide - 2 acids
Tripeptide- 3 acids
Polypeptide - multiple acids
104
Primary structure of protein
Sequence of amino acids
105
Primary structure of protein
Sequence of amino acids
106
Secondary structure of proteins
Primary structure coils into alpha helix or pleated sheet with hydrogen bonds
107
Tertiary structure
Folding inward if secondary structure, spontaneous, requires no energy. Structure determines the shape of a domain in the protein, where the functions occur.
108
Desaturation
When hydrogen bonds in protein break and cause protein to fall apart
109
Quaternary structure
When two or more proteins associate to form a functional unit.
Like the hemoglobin molecule
110
Quaternary structure
When two or more proteins associate to form a functional unit.
Like the hemoglobin molecule
111
Enzymes
Lower activation energy and increase rate of reaction.
112
Active site
Where reactants (substrates) attach to an enzyme
113
Lock and key method
Things fit
114
Induced fit model
Compound binds to enzyme and changes shape
115
Cofactor
A no protein portion that might activate an enzyme
116
Building block of a nucleic acid
Nucleotide, composed of sugar, a nitrogenous base, and a phosphorous groups
117
DNA nitrogenous bases
Adenine, thymine, guanine, and cytosine in a double helix
118
RNA nitrogenous bases
Adenine, uracil, guanine, and cytosine in a single strand
119
Structure of dna
Double stranded model where bases pair in the middle through a hydrogen bonds
120
Long long chain of dna in nucleus
Chromatin
121
ATP is
A nucleotide with adenosine as a phosphate base, attached to a ribose sugar, and with three phosphate groups
