Chemistry Comes Alive Flashcards
1
Q
Our body is made up of many _____
A
Chemicals
2
Q
Chemistry underlies all physiological reactions including:
A
Movement
Digestion
Pumping of the Heart
Nervous System
3
Q
Chemistry can be broken down in to:
A
Basic Chemistry
Biochemistry
4
Q
Anything that has mass and occupies space
A
Matter
5
Q
Mass plus the effects of gravity is called ____
A
Weight
6
Q
Definite shape and volume
A
Solid
7
Q
Changeable shape; definite volume
A
Liquid
8
Q
Changeable shape and volume
A
Gas
9
Q
Capacity to do work or put matter into motion
A
Energy
10
Q
Energy in action
A
Kinetic Energy
11
Q
Stored (inactive) energy
A
Potential Energy
12
Q
Energy can be transformed from _____ to _____.
A
Potential
Kinetic
13
Q
Stored in bonds of chemical substances
A
Chemical Energy
14
Q
Results from movement of charged particles
A
Electrical Energy
15
Q
Directly involved in moving matter
A
Mechanical Energy
16
Q
Travels in waves
A
Radiant or Electromagnetic Energy
17
Q
All matter is composed of _____.
A
Elements
18
Q
Substances that cannot be broken down into simpler substances by ordinary chemical methods
A
Elements
19
Q
Four elements make up 96% of the body:
A
Carbon
Oxygen
Hydrogen
Nitrogen
20
Q
- Unique building blocs for each element
- Smallest particles of an element with properties of that element
- What give each element its particular physical and chemical properties
A
Atoms
21
Q
- Carry a positive charge
- Have an arbitrary 1 atomic mass unit
A
Proton
22
Q
- Have no electrical charge
- Have an arbitrary 1 atomic mass unit
A
Neutron
23
Q
- Carry a negative charge
- Are so tiny they have virtually no weight
A
Electron
24
Q
Simplified and outdated because it incorrectly depicts electrons in and “orbit”
A
Planetary Model
25
Current model used that depicts orbitals rather than fixed orbits
Orbital Model
26
Total number of protons AND neutrons in an element
Mass Number
27
- Structural variations of the same element
| - Atoms contain same number of protons but sometimes differ in the number of neutrons they contain
Isotopes
28
Average of mass numbers of all isotope forms of an atom
Atomic Weight
29
Isotopes that decompose to more stable forms
Radioisotopes
30
Sometimes loss of various subatomic particles causes and isotope to become a _____ _____.
Different Element
31
Energy that is released when an isotope's subatomic particles are being decayed
Radioactivity
32
General term for 2 or more atoms bonded together
Molecule
33
Specific molecule that has 2 or more different kinds of atoms bonded together
Compound
34
Two or more components that are physically intermixed
Mixture
35
Homogeneous mixtures, meaning particles are evenly distributed throughout
Solution
36
Substance present in greatest amount (usually a liquid)
Solvent
37
Substance dissolved in solvent and present in smaller amounts
Solute
38
Heterogeneous mixtures, meaning that particles are not evenly distributed throughout the mixture
Colloids (also known as emulsions)
39
Some colloids undergo a "sol-gel" or ___ ___ ___ transformation
Solution to Gel
40
Heterogeneous mixtures that contain large, visible solutes that DO settle out
Suspensions
41
Mixtures do not involve _____ _____ between components, unlike compounds.
Chemical Bonding
42
Mixtures can be separated by ______ _____, such as straining or filtering
Physical Means
43
Compounds can be separated only by breaking their _____ _____/
Chemical Bonds
44
Mixtures can be heterogeneous or homogeneous, compounds can only be ______.
Homogeneous
45
"Energy relationships" between electrons of reacting atoms
Chemical Bonds
46
Electrons are the ______ ______ that are involved in all chemical reactions.
Subatomic Particles
47
Determine whether a chemical reaction will take place and, if so, what type of chemical bond is formed
Electrons
48
Electrons can occupy areas around a nucleus called the _____ _____.
Electron Shell
49
Each electron shell contains electrons that have a certain amount of kinetic and potential energy, so shells are also referred to as ____ _____.
Energy Levels
50
Depending on its size, and atom can have up to ____ electron shells.
7
51
Shells can hold only a specific number of _____.
Electrons
52
The shell closest to the _____ is filled first.
Nucleus
53
Outermost electron shell is called the _____ _____.
Valence Shell
54
- Atoms desire ____ electrons in their valence shell
| - Desire to have ___ electrons is the driving force behind chemical reactions.
8 (Octet Rule)
55
Most atoms do not have full _____ _____.
Valence Shells
56
Atoms that have gained or lost electrons and have become charged
Ions
57
Involve the TRANSFER of valence shell electrons from one atom to another
Ionic Bonds
58
Attraction of ____ charges result in an ionic bond
Opposite
59
Most ionic bonds form _____.
Salts
60
Formed by sharing two or more valence shell electrons between two atoms
Covalent Bonds
61
- Equal sharing of electrons between atoms
| - Results in electrically balanced, nonpolar molecules
Nonpolar Covalent Bonds
62
- Unequal sharing of electrons between 2 atoms
- Results in electrically polar molecule
- Atoms have different electron-attracting abilities, leading to unequal sharing
Polar Covalent Bonds
63
Atoms with a greater electron-attracting ability
Electronegative
64
Atoms with a less electron-attracting ability
Electropositive
65
- Attractive force between electropositive hydrogen of one molecule and an electronegative atom of another molecule
- Not a true bond, more of a weak magnetic attraction
Hydrogen Bonds
66
Occur when chemical bonds are formed, rearranged or broken
Chemical Reactions
67
Chemical reactions can be written in symbolic form called ____ _____.
Chemical Equations
68
Substances entering in to a reaction together
Reactants
69
Resulting chemical end products
Products
70
Involve atoms or molecules combining to form larger, more complex molecule
Synthesis Reactions
71
Involve breakdown of a molecule into smaller molecules or its constituent atoms
Decomposition Reactions
72
Involve both synthesis and decomposition
Exchange (or Displacement) Reactions
73
In living systems, these reactions are also referred to as _____ _____ or _____ reactions.
Reduction-Oxidation
| Redox
74
Atoms are _____ when they gain electrons.
Reduced
75
Atoms are _____ when they lose electrons
Oxidized
76
All chemical reactions are either ______ or ______.
Exergonic
| Endergonic
77
- Result in a net release of energy (give off energy)
- Products have less potential energy than reactants
- Catabolic and oxidative reactions
Exergonic Reactions
78
- Result in a net absorption of energy (use up energy)
- Products have more potential energy than reactants
- Anabolic rections
Endergonic Reactions
79
Increased _____ usually increases the rate of the reaction
Tempera
Concentration
Particle Size (smaller)
Catalysts
80
Substances that increase rxn rate without themselves being changed (enzymes)
Catalysts
81
The study of chemical composition and reactions of living matter
Biochemistry
82
Water, salts, and many acids and bases are____.
| Do not contain carbon
Inorganic Compounds
83
Carbohydrates, fats, proteins, and nucleic acids are____.
| Contain carbon, are usually large, and are covalently bonded
Organic Compounds
84
- Most abundant inorganic compound
- High heat capacity and heat of vaporization
- Polar solvent properties
- Reactivity
- Cushioning
Water
85
Ionic compounds that dissociate into separate ions in water
Salts
86
Salts separate into _____ and _____.
Cations
| Anions
87
Positively charged molecules
Cations
88
Negatively charged molecules
Anions
89
All ions are called _____ because they can conduct electrical currents in solutions
Electrolytes
90
Ionic balance is vital for _______.
Homeostasis
91
_______ play a big role in maintaining proper balance of electrolytes
Kidneys
92
If electrolyte balance is _____, virtually all organ systems cease to function.
Disrupted
93
_____ are proton donors.
Acids
94
Release hydrogen ions and bare protons into a solution
Proton Donors
95
_____ are proton acceptors.
Bases
96
The pick up hydrogen ions in a solution,
Proton Acceptors
97
Measurement of concentration of hydrogen ions in a solution
pH Scale
98
The more hydrogen ions in a solution, the more _____ it is.
Acidic
99
Resist abrupt and large swings in pH
Buffers
100
_____ can convert strong acids or bases into weak ones.
Buffers
101
Organic molecules contain _____
Carbon
102
Carbon is _______
Electroneutral
103
- Shares electrons; never gains or loses them
- Forms four covalent bonds with other elements
- Carbon is unique to living systems
Electronuetral (Carbon)
104
Include sugar and starches
Carbohydrates
105
One single sugar
Monosaccharides
106
Smallest unit of carbohydrate
Monomers
107
Two sugars
Disaccharides
108
Many sugars
Polysaccharides
109
_____ are made up of monomers of monosaccharides
Polymers
110
Simple sugars containing three to seven carbon atoms
Monosaccharides
111
Ribose and deoxyribose
Pentose Sugars
112
Glucose
Hexose Sugars
113
- Double sugars
- Too large to pass through cell membrane
- Formed by dehydration synthesis of two momsaccharides
Disaccharides
114
- Polymers of monosaccharides
- Formed by dehydration synthesis of many monomers
- Not very soluble
Polysaccharides
115
- Contains C, H, O, but less than carbohydrates, and sometimes P
- Insoluble in water
Lipids
116
- Called fats when solid and oils when liquid
- Composed of three fatty acids bonded to a glycerol molecule
- Used for energy storage, insulation, and protection
Triglycerides
117
- Modified triglycerides
- Head is a polar region and is attracted to water
- Tails are nonpolar and are repelled by water
- Important in cell membrane structure
Phospholipids
118
- Consist of four interlocking ring structures
- Most important steroid is cholesterol
- Important in cell plasma membrane structure
Steroids
119
- Many different ones
- Derived from a fatty acid found in cell membranes
- Most important are prostaglandins
- Play a role in blood clotting, control of blood pressure, inflammation, and labor contractions
Eicosanoids
120
- Comprise 20-30% of cell mass
- Have most varied function of any molecule
- Contain C, H, O, N, and sometimes S and P
Proteins
121
All proteins are polymers made from ____ types of amino acids
20
122
Four levels of protein structure determine ____ and _____.
Shape
| Function
123
- Strandlike, water insoluble and stable
- Most have tertiary or quaternary structure
- Provide mechanical support and tensile strength
Fibrous (structural) Proteins
124
- Compact, spherical, water-soluble, and sensitive to environmental changes
- Tertiary or quaternary structure
- Specific functional regions (active sites)
Globular (functional) Proteins
125
- Globular proteins unfold and lose their functional 3-D shape
- Can be caused by decreased pH or increased temperature
- Usually reversible if normal conditions restored
- Irreversible if changes are extreme
Denaturation
126
Globular proteins that act as biological catalysts
Enzymes
127
Regulate and increase speed of chemical reactions without getting used up in the process
Catalysts
128
Most functional enzymes
Holoenzymes
129
Protein part of a holoenzyme
Apoenzyme
130
Metal ion or organic molecule (often a vitamin) part a holoenzyme
Cofactor or Coenzyme
131
Enzymes act on a very specific _____.
Substrate
132
1. Substrate binds to enzyme's active site, temporarily forming ______-_____ complex.
2. Complex undergoes rearrangement of _____, resulting in final product.
3. Product is _____ from the enzyme.
Enzyme-substrate
Substrate
Released
133
Composed of C,H, O, N, and P, are the largest molecules in the body
Nucleic Acids
134
Made up of monomers called nucleotides and are composed of a nitrogen base, a pentose sugar and a phosphate group
Nucleic Acid Polymers
135
Holds the genetic blueprint for the synthesis of all proteins
DNA
136
Links DNA to protein synthesis and is slightly different from DNA
RNA
137
Chemical energy released when glucose is broken down is captured in _____
ATP (adenosine triphosphate)
138
ATP directly powers _____ _____ in cells and offers immediate, reusable energy needed by body cells
Chemical Reactions
