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A&P I > Chapter 2 PPT > Flashcards

Chapter 2 PPT 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

Elements

A

Simplest types of matter with certain chemical properties. There are 98 naturally occurring elements.

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3
Q

Atoms

A

Smallest particles of an element that have properties of that element.

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4
Q

Bulk Elements

A

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

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5
Q

Trace Elements

A

required by the body in small amounts (F e, I)

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6
Q

Ultratrace Elements

A

Required by the body in very minute amounts (As)

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7
Q

Atoms

A

Composed of subatomic particles

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8
Q

Proton

A

Carries a single positive charge

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9
Q

Neurton

A

Carries no electrical charge

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10
Q

Electron

A

Carries a single negative charge

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11
Q

nucleus

A

Central part of atom. Composed of protons and neutrons. Electrons move around the nucleus

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12
Q

Atom Characteristic

A

Smallest particle of an element that has the properties of that element

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13
Q

Electron Characteristic

A

Extremely small particle within an atom; almost no weight; carries a negative electrical charge and is in constant motion around an atomic nucleus

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14
Q

Proton Characteristic

A

Relatively large particle within an atom; carries a positive electrical charge and is found within an atomic nucleus

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15
Q

Neutron Characteristic

A

Relatively large particle within an atom; about the same weight as a proton; uncharged and thus electrically neutral; found within an atomic nucleus

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16
Q

Ion Characteristic

A

Particle, formed from an atom, that is electrically charged because it has gained or lost one or more electrons

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17
Q

Molecule Characteristic

A

Particle formed by the chemical union of two or more atoms

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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

Atomic Weight

A

Number of protons plus the number of neutrons in one atom. Electrons do not contribute to the weight of the atom because they are so light

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20
Q

Isotops

A

Atoms with the same atomic numbers but with different atomic weights. Contain different number of neutrons.

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21
Q

Radioactive Isotopes

A

Are unstable, releasing energy or atomic fragments (atomic radiation) until they gain stability, some are used to detect and treat disease

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22
Q

Radioactive Iodine-131

A

Can be used to destroy cancerous thyroid gland tissue. Only part of the body that transports and metabolizes iodine.

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23
Q

Radioactive Isotope Medical Uses

A

Detecting coronary blood vessel disorders, evalualting kidney function, measuring hormone concentration in body fluids and assessing changes in bone density.

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24
Q

Ionizing Radiation

A

Radiation (Alpha, Beta, Gamma) called this because energy can remove electrons from atoms, resulting in the formation of ions. The free electrons can damage nearby atoms.

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25
Molecule
Particle formed when two or more atoms chemically combine
26
Compound
Particle formed when two or more atoms of different elements chemically combine
27
Molecular Formulas
Depict the elements present and the number of each atom present in the molecule
28
For atoms with atomic number 18 or less
the first shell can hold 2 electrons and the second and third shell can hold up to 8 electrons
29
Ion
An atom that gains or loses electrons to become stable. An electrically charged atom
30
Cation
A positively charged ion. Formed when an atom loses electrons
31
Anion
A negatively charged ion. Formed when an atom gains electrons
32
Ionic Bonds
Formed when electrons are transferred from one atom to another atom. Attraction between a cation and an anion forms a very strong bond between the ions, called an ionic bond
33
Covalent Bond
Strong chemical bonds, formed between atoms that share electrons.
34
Polar Molecules
Molecules with a slightly negative end and a slightly positive end. REsults from unequal sharing of electrons in covalent bonds. WAter is the most important one
35
Hydrogen Bond
A weak attraction ebtween a slightly positive H end of one polar molecule and a slightly negative (N or O) end of another polar molecule. Formed between adjacent water molecules. Important for protein and nucleic acid structure
36
Chemical Reactions occur
when chemical bonds form or break between atoms, ions, or molecules
37
Reactants are
the starting material of a chemical reaction: the atoms ions, or molecules
38
PRoducts are
substances formed at the end of the chemical reaction
39
Synthesis REaction
More complex chemical structure is formed A + B --> AB
40
Decomposition Reaction
Chemical bonds are broken to form a simpler chemical structure AB --> A + B
41
Exchange Reaction
Chemical bonds are broken and new bonds are formed AB + CD --> AD + CB
42
Reversible REaction
The products can change back to the reactants A + B AB
43
Electrolytes
Susbtances that release ions in water. The solution can conduct an electric current, so its called an electroylte NaCl --> Na + Cl
44
Acids
Electroyltes that dissociate to release hydrogen ions in water HCl --> Na + OH
45
Bases
Substances that relase ions that can combine with hydrogen ions NaOH --> Na + OH
46
Salts
Electrolytes formed by the reaction between an acid and a base HCl + NaOH --> H2O + NaCl
47
When an ionically bonded substance is put into water,
the charged ions are attracted to the slightly charged ends of the polar water molecules. Substance dissociates, and the ions become surrounded by water molecules.
48
The pH scale is used as shorthand for
H+ ion concentration, it is based on the number of decimal places in the concentration.
49
The higher the H+ concentration,
the lower the pH, and the higher the acidity
50
The lower the H+ concentration,
the higher the pH and the lower the acidity
51
pH Scale
indicates teh concentration of hydrogen ions in a solution
52
Neutral pH
A pH of 7 indicates equal concentrations of H+ and OH-. pH of water,
53
Acidic pH
A pH of <7 indicates a greater concentration H+ than OH-
54
Basic (Alkaline) pH
A pH >& indicates a higher concentration of OH- than H+
55
Normal range of blood pH?
7.35 - 7.45
56
Acidosis occures when
blood pH drops to 7.0-7.3 Person feels disoriented, fatigued. Caused by vomiting of alkaline intestinal contents
57
Alkalosis occurs when
blood pH rises to 7.5 - 7.8 Makes person feel dizzy and agitated. Caused by high altitude breathing
58
What mechanisms help regulate pH?
Homeeostatic
59
Buffers are
chemicals which act to resist pH changes, bind and release H+ ions to regulate pH
60
ORganic Molecules contain
C and H
61
Orgain Molecules can
dissolve in either water or organic liquids
62
Water-soluble organic compounds do not
release ions, and are non-electrolytes
63
Organic Molecules include
Carbohydrates, Proteins, Lipids, and Nucleic Acids
64
Inorganic Molecules generally do not
contain C and H
65
Inorganic molecules usually
dissolve inw ater and dissociate, forming ions and are electroytes
66
Inorganic molecules include
water, oxygen, CO2 and inorganic salts
67
Water has an important role in
transporting chemicals in the body
68
CO2 ; waste product released during
metabolic reactions
69
Inorganic salts help control
H2O concentration, pH, blood clotting, nerve and muscle processes
70
Carbohydrates are a main
source of cellular energy. Supply materials to build cell structures
71
Carbohydrates solubility
Water-soluble
72
Carbohydrates contain
C, H, and O
73
Ratio of H to O for Carbohydrates
2:1
74
Size classification of carbohydrates
Monosaccharides(Single Sugars) Disaccharides (Double Sugars) Polysaccharides (Complex Carbohydrates)
75
Monosaccharides include
glucose and fructose
76
Disaccharides include
sucrose and lactose
77
Polysaccharides include
starch, glycogen, and cellulose
78
Lipid solubility
insoluble in water, but soluble in organic solvents
79
Lipids include
triglycerides (fats), phospholipids, steroids
80
Lipids important component of
cell membranes, and have several functions in cells
81
Most abundant lipids are
triglycerides (Fats)
82
TRiglycerides used for
Cellular energy Contain more energy per gram than carbohydrates Contain C, H , but less O than Carbs
83
Triglycerides consist of
1 molecule of glycerol and 3 fatty acids
84
Saturated Fatty Acids have
only single carbon-carbon bonds. Most are solid at room temperature, and of animal origin
85
Unsaturated fatty acids have
one or more carbon-carbon double bond. Most are liquid at room temperature, and are of plant origin
86
Phospholipids consist of
1 glycerol, 2 faty acids, and 1 phosphate
87
Phospholipids have
hydrophillic glycerol portion, and hydrophobic fatty acid ends
88
Phospholipids major component of
cell membranes
89
Steroids are
4 connected rings of carbon and widely distributed in the body, various functions
90
Steroids are a component of
cell membranes
91
steroids used to synthesize
adrenal and sex hormones
92
Main steroid in the body?
Cholesterol
93
Proteins are used as
structual materials, energy source, hormones, receptors, enzymes, and antibodies
94
Proteins consist of
building blocks called amino acids
95
Amino Acid contains
an amino group carboxyl group and a unique r (side chain) group
96
Amino acids are bound to each other by
peptide bonds
97
Peptide bonds form between
the amino group of one amino acid, and the carboxyl group of the adjacent amino acid
98
Primary Structure
Amio acid sequene
99
Secondary structure
Pleated or twisted structure form by hydrogen bonding between nonadjacent amino acids
100
Tertiary Structure
Unique 3D folded shape of the protein
101
Quaternary Structure
Structure formed by some proteins, when 2 or more polypepetide chains are conencted to become 1 protein
102
Nucleic cids can
carry genetic code (DNA) or aid in protein synthesis (RNA)
103
Nuclueic acids encode
amino acid sequences of proteins
104
Building blocks are called
nucleotides, which consist of a sugar (S), a phosphate group (P) and an organic base (B)
105
DNA structure
Double chain of nucleotides
106
RNA structure
single chain of nucleotides
107
DNA function?
Store the geneteic code
108
DNA contains
the sugar deoxyribose
109
DNA structure
Double helix
110
DNA composed of
nucleotides
111
RNA function?
interacts with DNA to conduct protein synthesis
112
RNA contains
the sugar ribose
113
RNA structure
single strand
114
RNA composed of
nucleotides
115
CT Imaging
Used to visualize internal antaomy. Used xray imitting decide to create 3D image Differentiates tissuese with slightly different densities, tumors
116
PET Imaging
Uses radioactive isotopes that emit positrons (unusual positively charge electrons) to detect biochemical activity
117
PET used to
detect various brain disroders, blood flow, normal brain physiology

A&P I (33 decks)

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