Module 2 Flashcards
To mater the terms and concepts in Module 2. Study guide and test review hand out.
1
Q
Element
A
A substance which cannot be split into simpler substances by chemical means
2
Q
Atoms
A
The smallest unit of matter which retains the properties and characteristics of the element
3
Q
Oxygen (O)
A
65% of total body mass
Part of water and many organic molecules
4
Q
Organic molecules
A
Carbon containing molecules
5
Q
Carbon (C)
A
18.5% of total body mass
Forms backbone chains and rings of all organic molecules, carbohydrates,lipids, proteins,nucleic acids
6
Q
Hydrogen (H)
A
9.5% of body mass
Constituent of water and most organic molecules
ionized form (H+) makes body fluids more acidic
7
Q
Nitrogen (N)
A
3.2% of total body mass
Component of all proteins and nucleic acids
8
Q
Blood Urea
A
The product of protein breakdown in the blood
9
Q
Macroelements
A
O 65%
C 18.5%
H 9.5%
N 3.2%
10
Q
Calcium (Ca)
A
Contributes to the hardness of bones and teeth
The ionized form (Ca2+) is needed for blood clotting,the release of some hormones.and the contraction of muscles
11
Q
Phosphorous (P)
A
component of nucleic acids and ATP
Required for normal bone/tooth structure
12
Q
Potassium (K)
A
ionized form (K+) is the most plentiful cation inside the cell
Needed for nerve activity
13
Q
ATP
A
Adenosine Triphosphate
Molecule needed to store chemical energy for the cell
14
Q
Cation
A
Positively charged particle (ion)
15
Q
Sulfur (S)
A
Component of some vitamins and many proteins
16
Q
Sodium (Na)
A
ionized form (Na+) is the most plentiful cation in the extracellular fluid
17
Q
Chlorine (Cl)
A
Ionized form (Cl-) is the most plentiful anion in the extracellular fluid
Essentil for maintaining water balance
18
Q
Anion
A
Negatively charged particle (ion)
19
Q
Magnesium (Mg)
A
ionized form (Mg2+) needed for many enzymes
20
Q
Enzymes
A
molecules that increase the rate of chemical reactions in organisms
21
Q
Iron (Fe)
A
ionized forms (Fe2+and Fe3+) are part of hemoglobin and some enzymes
22
Q
Hemoglobin
A
oxygen carrying proteins in red blood cells (RBC)
23
Q
Microelements
A
Calcium (Ca) Phosphorus (P) Potassium (K) Sulfur (S) Sodium (Na) Chlorine (Cl) Magnesium (Mg) Iron (Fe)
24
Q
Trace Elements
A
Elements needed in "trace" amounts Aluminum (Al) Boron (B) Chromium (Cr) Cobalt (Co) Copper (Cu) Flourine (F) Iodine (I) Manganese (Mn) Molybendum (Mo) Selenium (Se) Silicon (Si) Tin (Sn) Vanadium (V) Zinc (Zn)
25
Molecule
two or more atoms sharing electrons joined by a chemical bond
Can be the same or different elements
26
Compound
A molecule that contains atoms of different elements
H2O, NaCl, CaCl2
27
States of matter (3)
Solid, Liquid, Gas
28
Solid
Shape: definite
Volume: definite
Compressibility: very slight
Particles: Rigidly clinging,tightly packed
29
Liquid
Shape: indefinite
Volume: definite
Compressibility: slight
Particles: mobile, adhering
30
Gas
Shape: indefinite
Volume: indefinite
Compressibility: high
Particles: Independent of each other and relatively far apart
31
Changes in physical states (4)
Freezing
Melting
Condensation
Vaporization
32
Potential Energy
Stored energy
33
Kinetic Energy
Energy of motion
34
Endergonic Reactions
Reaction requires energy to be added to happen
Anabolic reaction
35
Exergonic Reactions
Reaction that releases energy
Catabolic reaction
36
Anabolism
Energy stored in chemical bonds
37
Catabolism
Energy released from chemical bonds. This energy can be turned into work
38
Entropy
The measure of disorder
39
Diffusion
The movement of substances from areas of high concentration to areas of low concentration
A kind of entropy
40
Specific Heat
The amount of energy that is needed to raise 1g (gram) os substance 1 degree of temperature
41
Matter is made up of these: (3)
Electrons, Neutrons, Protons
42
These form the nucleus of an atom:
Protons and neutrons
43
Electrons
```
the negatively charged part of the atom
is the reactive part of the atom
gives an atom it's chemical properties
very light 0.0005 Daltons
Do NOT contribute to the mass of an atom
```
44
Protons
Positively charged particles
Part of the nucleus
Large. heavy 1.007 Daltons (rounded to 1)
Contribute to the mass of an atom
45
Neutrons
No charge (neutral)
part of the nucleus
large, heavy 1.009 Daltons (rounded to 1)
Do contribute to the mass of the atom
46
Atomic Mass
The combined mass of all particles in an atom
47
Isotopes
Atoms which vary in their number of neutrons
48
Atomic number
The number of protons
49
Mass number
sum of the protons and neutrons
50
Atomic mass (atomic weight)
the average miss of all naturally occuring isotopes of an element
51
47Ca (Calcium 47)
Used to study bone in nuclear medicine
20 protons
27 neutrons
52
131I (Iodine 131)
Used to destroy Thyroid tissue
53 protons
78 neutrons
53
133Xe (Xenon 133)
Used for respiratory studies
54 protons
79 neutrons
54
Name an important element required for muscle contraction and bone integrity
Calcium (Ca)
55
Name an element that is vital for the formation of carbohydrates, lipids and proteins
Carbon (C)
56
Name an element that is responsible for the activity of many enzymes
Magnesium (Mg)
57
And abundance of hydrogen ions in solution is referred to a/an:
Acid
58
Which element is a compound of many vitamins and proteins?
Sulfur (S)
59
Which element is a constituent of proteins and nucleic acids?
Nitrogen (N)
60
Atoms are the smallest unit of matter that retains the properties and ______ of an element.
Characteristics
61
This element is vital for the storage of energy (ATP)
Phosphorus (P)
62
T/F: Iodine is an anion.
False
63
Identify the constituent atoms of H2O
Hydrogen (H) - 2
| Oxygen (O)- 1
64
Substances with two or more different elements are________.
Compounds
65
Matter that has a definite shape with tightly packed atoms/molecules is called _______.
Solid
66
Matter that has an indefinite shape and definite volume with mobile molecules is called a _______.
Liquid
67
Matter that has indefinite volume with independent, widely spaced atoms/molecules is called a ______.
Gas
68
A body at rest with the ability to move has ______ energy.
Potential
69
A body in motion is an example of _________ energy.
Kinetic
70
Building through chemical bonds is called______.
Anabolic
Hint: anabolic steroids build muscles
71
Deconstruction of chemical bonds is called _________.
Catabolic
72
Endergonic chemical reactions require _______ input.
Energy
73
__________ reactions release more energy than they consume
Exergonic
74
Measurement of disorder in a system is called________.
Entropy
75
1.000cal/gC (gram degree C) is also known as the ___________.
Specific Heat
76
H, O, ____, and C are the four most abundant elements of the body's mass.
N (Nitrogen)
77
Name the elements for Fe, Na, K, Au, Ag, and Cu
Iron, Sodium, Potassium, Gold, Silver, Copper
78
The neutral subatomic particle of the nucleus of an atom is called a________.
Neutron
79
Electrons have a _______ charge.
Negative
80
Protons have a _________ charge.
Positive
81
Changing the number of this subatomic particle will result in an isotope.
Neutrons
82
The atomic number is equal to the number of ______ in the atom.
Protons
83
Adding the number of protons and neutrons together will provide this number
Atomic Mass Number
84
Giving, taking and/or sharing of which subatomic particle is responsible for chemical reactions.
Electrons
85
Define and ion
An electrically charged atom/molecule
86
Define cation
A positively charged ion
87
What is the most acidic of the following pH values? 3, 4, 5, 6, 7
The pH of 3 is the most acidic
88
Buffers maintain __________ balances in the body.
Acid/Base
89
A solution without H+ or OH- is considered to be a _______.
Salt
90
An __________ is a mixture of fats and proteins and water,all mixed together, with microscopic droplets of fat suspended in a protein and water solution.
Emulsion
91
if someone gave you a 15% NaCl solution, how many grams of NaCl are in 100 mL of this solution?
15g
92
Define a solute.
A solid dissolved in a solvent. NaCl dissolved in water.
93
A substance called _________ reduces surface tension.
Surfactant
94
H and O2 atoms are bound together inside cells as _______ and are used in most _______ reactions.
ions, chemical
95
The hydrogen atom in a water molecule has a partial positive charge. Why?
Because it is a polar covalent bond where the O is more electronegative than the H and it "hogs" the electrons.
96
A polar covalent bond is the _______ sharing of electrons between two non-metals.
Uneven
97
Name the following polyatomic ions:
OH-
HCO3-
NH4+
Hydroxyl
Bicarbonate
Ammonia
98
Superoxide,hydroxyl, and peroxynitrite are examples of ________
free radicals
99
An atom or a molecule containing an unpaired electron is called a __________.
Free Radical
100
High energy photons are associated with _______ and ________.
Light and energy
101
Beta particles are __________ expelled at high energy from radioactive atoms.
Electrons
102
An alpha particle is a ___________.
Helium nucleus
103
Radio isotopes occur when there are more _______ in the nucleus than can be supported.
Neutrons
104
Identify the constituent atoms of H2O
Hydrogen- 2
| Oxygen- 1
