Chapter 2 - Chemistry Flashcards
(88 cards)
1
Q
Matter
A
Anything that takes up space and has mass.
Matter is composed of elements. Solids, liquids, and
gases are matter
2
Q
Mass
A
Amount of matter present
3
Q
Weight
A
Heaviness due to gravitational pull on mass
4
Q
Chemistry
A
Studies composition, properties, interaction
of matter
5
Q
Biochemistry
A
Biological chemistry, which studies
physiological process and disease
6
Q
Elements
A
Simplest types of matter with certain chemical
properties. There are 92 naturally occurring elements
7
Q
Compounds
A
Chemical combinations of different elements
8
Q
Atoms
A
Smallest particles of an element that have properties
of that element
9
Q
Bulk elements:
A
Required by the body in large amounts
(C,O,H,N,S,P)
10
Q
Trace elements:
A
Required by the body in small amounts
(Fe,I)
11
Q
Ultratrace elements:
A
Required by the body in very minute
amounts (As)
12
Q
Atoms
A
composed of subatomic particles
13
Q
Protons
A
large particles
carry a single positive charge
14
Q
Neutrons
A
Large particles
carry NO electrical charge
15
Q
Electrons
A
Small particles
carry a single negative charge
16
Q
Atoms consists of a ______ _______ (protons + Neutrons) and _______ in constant motion around the nucleus
A
Central Nucleus
Electrons
17
Q
Number of _____ equals number of ______ in a atom; therefore, atoms are electrically _____
A
Protons
Electrons
Neutral
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
19
Q
Mass Number:
A
The number of protons plus the number of neutrons in one
atom
Electrons do not contribute to the mass of the atom
because they are so light
20
Q
Molecule
A
Particle formed when two or more atoms
chemically combine
21
Q
Compound
A
Particle formed when two or more atoms of
different elements chemically combine
22
Q
Molecular formulas:
A
Depict the elements present and the
number of each atom present in the molecule
H2 = a molecule of hydrogen
C6H12O6 = a molecule of glucose
H2O = a molecule of water
23
Q
Chemical bonds
A
form when atoms
combine with other atoms. They result
from interactions between the electrons
of the atoms.
24
Q
Electrons of an atom occupy regions of
space called
A
electron shells - these encircle the nucleus
25
For atoms with atomic numbers of 18 or
less, the following rules apply:
* The first shell can hold up to 2
electrons.
* The second shell can hold up to 8
electrons.
* The third shell can hold up to 8
electrons
26
Electrons in outermost shell determine
whether atom will react with other atoms
to form chemical bonds
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Ion
An electrically charged atom that gains or loses
electrons to become stable
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Cation
A positively charged ion, formed when an atom
loses electrons
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Anion
A negatively charged ion, formed when an atom
gains electrons
30
Ionic Bonds:
Strong chemical bonds formed when ions of
opposite charge attract
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Covalent Bonds
Strong chemical bonds, formed between
atoms that share electrons
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Two atoms of hydrogen (H) can combine to form
a
hydrogen molecule (H2). Both atoms in the molecule
become stable
33
Hydrogen molecules (H2) often combine with oxygen (O2)
molecules to form
water molecules (H2O)
34
Nonpolar covalent bonds:
Covalent bonds in which electrons are shared equally
Found between atoms with same electronegativity
Atoms of same element have same number of protons, and
pull shared electrons equally
35
Polar covalent bonds:
Covalent bonds in which electrons are not shared equally
Found between atoms with different electronegativities
Forms polar molecules with unequal charge distribution
Atoms with larger number of protons have higher
electronegativity, and pull shared electrons closer to their
nucleus
Water is a polar molecule
36
Hydrogen bonds:
* Relatively weak attraction
of slightly positive (H) end
of one polar molecule to
slightly negative (N or O)
end of a nearby polar
molecule
* Form between adjacent
water molecules
* Important for protein and
nucleic acid structure
37
Chemical reactions
occur when chemical bonds form or
break between atoms, ions, or molecules
38
Reactants
are the starting materials of a chemical
reaction: the atoms, ions, or molecules
39
Products
are substances formed at the end of the
chemical reaction
40
Synthesis Reaction
more complex chemical structure is
formed
A + B => AB
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Decomposition Reaction
chemical bonds are broken to
form a simpler chemical structure
AB => A + B
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Exchange Reaction
chemical bonds are broken and new
bonds are formed
AB + CD => AD + CB
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Reversible Reaction
: the products can change back to the reaction
A + B = AB
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Electrolytes
Substances that release ions in water. The
solution can conduct an electric current, so it is called an
electrolyte
NaCl => Na plus + Cl negative
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Acids
Electrolytes that dissociate to release hydrogen ions
in water
46
Bases
Substances that release ions that can combine with
hydrogen ions
47
Salts
Electrolytes formed by the reaction between an acid
and a base
48
pH Scale
Indicates the concentration of hydrogen ions in a
solution
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Neutral
A pH of 7 indicates equal concentrations of
This is the pH of water.
50
Acidic
A p H of <7 indicates a greater concentration of
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Basic (alkaline)
A pH >7 indicates a higher concentration of
52
What is the normal range of blood?
7.35 through 7.45
53
Acidemia occurs when blood pH drops to what?
7.0 through 7.3
54
Acidosis makes a person feel?
disoriented and fatigued
Caused by vomiting of alkaline intestinal contents, diabetes, lung
disease with impaired CO2 exhalation
55
Alkalemia occurs when blood pH rises to
7.5 through 7.8
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Alkalosis makes a person feel
Dizzy and agitated
Caused by high altitude breathing, vomiting of acidic stomach
contents, high fever, taking excess antacids.
Homeostatic mechanisms help regulate pH
57
Organic molecules:
* Contain C and H
* Depending on the type, they will dissolve in either water or organic
liquids
* Water-soluble organic compounds do not release ions, and are non-
electrolytes
* Carbohydrates, proteins, lipids, and nucleic acids
58
Inorganic molecules
* Generally do not contain C and H
* Usually dissolve in water and dissociate, forming ions, and are
electrolytes
* Water, oxygen, carbon dioxide, and inorganic salts
59
Water
* Most abundant compound in living material
* Two-thirds of the weight of an adult human
* Major component of all body fluids
* Medium for most metabolic reactions
* Important role in transporting chemicals in the body
* Absorbs and transports heat
* Water balance exists when gains equal losses
* Water is a solvent that many solutes dissolve in
60
Oxygen
* Used by organelles to release energy from nutrients in order to
drive cell’s metabolic activities.
* Necessary for survival
61
Carbon dioxide (CO2)
* Waste product released during metabolic reactions
* Must be removed from the body through exhaling
62
Inorganic salts:
* Abundant in body fluids
* Sources of necessary ions
* Play important roles in metabolism
* Help control H2O concentration, pH, blood clotting, nerve
and muscle processes
* Electrolyte balance exists when gains equal losses
63
Main source of cellular energy:
* Supply materials to build cell structures
* Water-soluble
* Contain C, H, and O
* Ratio of H to O close to 2:1 (C6H12O6 = glucose)
64
Size classification of carbohydrates:
Monosaccharides
Disaccharides
Polysaccharides
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Monosaccharides are...?
(single sugars): glucose, fructose
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Disaccharides
(double sugars): sucrose, lactose
67
Polysaccharides
(complex carbohydrates): starch,
glycogen, cellulose
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Lipids
* Insoluble in water, but soluble in organic solvents
* Include triglycerides (fats), phospholipids, steroids
* Important component of cell membranes, and have several
functions in cell
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Most abundant lipids are triglycerides (fats)
* Used for cellular energy
* Contain more energy per gram than carbohydrates
* Contain C, H, and O, but less O than carbohydrates
* Consist of 1 molecule of glycerol and 3 fatty acids
70
Phospholipids
are similar to triglycerides, except that they
have glycerol, 2 fatty acids, and a phosphate group
71
Saturated fatty acids
Have only single carbon-carbon bonds
* Most are solid at room temperature
* Most are of animal origin
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Unsaturated fatty acids
Have one or more carbon-carbon double bond
* Most are liquid at room temperature
* Most are of plant origin
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Phospholipids
Similar to triglycerides, except that they have glycerol, 2
fatty acids, and a phosphate group
* Main structural component of cell membranes
74
Steroids
* 4 connected rings of carbon
* Widely distributed in the body, various functions
* Component of cell membranes
* Used to synthesize adrenal and sex hormones
* Cholesterol is the main steroid in the body
75
Proteins
* Used as structural materials, energy source, hormones,
receptors, enzymes, antibodies
* Consist of building blocks called amino acids
* An amino acid contains an amino (–NH2) group, a carboxyl
* (COOH) group, and a unique R (side chain) group
* Amino acids are bound to each other by peptide bonds
76
Peptide bonds
form between the amino group of one
amino acid, and the carboxyl group of the adjacent amino
acid
77
4 Levels of Protein Structure:
Primary
Secondary
Tertiary
Quaternary
78
Primary
Amino acid sequence
79
Secondary
Pleated or twisted structure formed by hydrogen bonding
between nonadjacent amino acids
80
Tertiary
Unique 3-dimensional folded shape, or conformation, of the
protein, which determines its function
81
Quaternary
Structure formed by some proteins, when 2 or more
polypeptide chains are connected to become 1 protein
82
Denaturation
* A change in the secondary and tertiary structure of a protein
* Caused by heat, radiation, pH changes, chemicals
* Sometimes reversible, and other times irreversible
* In case of enzymes, irreversible denaturation stops it from functioning
83
Nucleic acids:
* Carry genetic code (DNA) or aid in protein synthesis (RNA)
* Nucleic acids encode amino acid sequences of proteins
* Building blocks are called nucleotides, which consist of a
sugar (S), a phosphate group (P), and an organic base (B)
84
DNA
(Deoxyribonucleic acid): a double chain of nucleotides
85
RNA
(Ribonucleic acid): a single chain of nucleotides
86
What are two major types of Nucleic Acids
DNA and RNA
87
DNA
* Stores the genetic code
* Contains the sugar deoxyribose
* Structure—double helix
* Composed of nucleotides
88
RNA
* Interacts with DNA to conduct protein synthesis
* Contains the sugar ribose
* Structure—single stranded
* Composed of nucleotides
