Chapter 2 Flashcards
1
Q
Matter
A
Has weight and occupies space and forms 3 mixtures;
3 States : SOLID, LIQUID, and GAS
2
Q
Atoms
A
Smallest unit of matter;
Subatomic particles: ELECTRONS, NEUTRONS, and PROTONS
3
Q
Electrons
A
(0-) Negative charge;
OUTSIDE NUCLEUS
4
Q
Neutrons
A
Neutral charge;
* IN NUCLEUS*
5
Q
Protons
A
Positive charge;
* IN NUCLEUS CORE*
6
Q
Electron Shells
A
Region surrounding atomic nucleus-Electrons Exist;
- 1st shell* - 2 electrons
- 2nd shell* - 8 electrons
- 3rd shell* - 18 electrons “satisfied with 8”
7
Q
Atomic Number
A
Number of protons;
Represented by chemical symbols;
8
Q
4 Elements of the Human Body:
A
Hydrogen, Oxygen, Carbon, and Nitrogen;
7 mineral elements and 13 trace elements
9
Q
Mass Number
A
Number of protons and neutrons;
10
Q
Isotopes
A
Atoms that have (SAME ATOMIC NUMBER) but (DIFFERENT ATOMIC WEIGHT);
11
Q
Radioisotopes
A
Radiation therapy (Cancer);
12
Q
Radiotracers
A
Used by camera that shows shape, size, and activity of organs & cells;
13
Q
Suspension
A
Type of mixture
Will settle out (blood);
Unevenly distributed particles;
14
Q
Colloids
A
2nd type of mixture
Small evenly distributed particles;
Will Not settle out;
15
Q
Solutions
A
3rd type of mixture
Small evenly distributed particles;
Will Not settle out;
16
Q
Solute
A
Where substance dissolves;
17
Q
Solvent
A
Substance dissolves in the solute;
18
Q
Chemical Bond
A
Holds atoms of a molecule or compound together;
- Molecule- chemical bond.
- Compound- formed when two or more atoms from different elements combine.
19
Q
Molecular Formula
A
Used by letters and numbers;
20
Q
Duet Rule
A
Atoms with 5 or less electrons;
- hydrogen and helium * -example
21
Q
Ionic Bonds
A
Holds ions together by force (metal to nonmetal);
22
Q
Cation
A
Positive charged; metal loses
23
Q
Anion
A
Negatively charged; nonmetal gains
24
Q
Covalent Bonds
A
Atoms of 2 or more sharing electrons;
25
Electronegativity
Proton attraction;
* Fluorine= most electric element*
* INCREASES FROM BOTTOM left to UPPER RIGHT*
26
Non-polar Covalent Bond
Attraction is an equal force between two nonmetals;
27
Polar Covalent Bonds
Attraction is unequal;
28
Hydrogen Bonds
Weak attraction between one positive end of dipole and one negative end of dipole;
*Key property of WATER*
29
Chemical Reaction
Occurs when bonds form or old ones break;
*Foundation of all Life Processes*
30
Chemical Notation
Symbols and abbreviations;
*Shows what occurs in Chemical Equation*
Two parts:
Reactants - (left) Starting
Product - (right) Result
31
Reversible Reaction
Can go in either direction;
32
Irreversible Reaction
Left to right;
33
Energy
Do work or put matter into motion;
*Two Forms*
Potential - stored, released later.
Kinetic - potential energy, already released so in motion.
34
Energy Forms in the Human Body:
Chemical, Electrical, and Mechanical energy;
Chemical- bonds between atoms; STORAGE
Electrical- generated by movement; NERVE IMPULSE
Mechanical- transferred energy from one object to the other; MUSCLE PULL ON BONES
35
Endergonic Reactions
*IN*
| Absorbs energy;
36
Exergonic Reaction
*OUT*
| Release of energy;
37
3 types of Chemical Reactions:
Catabolic, Exchange, and Anabolic;
Catabolic- decomposition
AB -> A + B
Exchange (*SWAP*) - ph neutralization
AB + CD—> AD + BC
Anabolic (Synthesis) - building of DNA replication
AB—> A+ B =
A +B —> AB
38
Oxidation-Reduction
Redox( exchange) reaction;
*EXERGONIC*
Oxidized- reactant LOSING electrons (+)
Reduced- reactant GAINS electrons (-)
39
Activation Energy
Ea= energy required for chemical reactions;
*TRANSITION STATE*
40
Factors that Increase Reaction Rate by Reduced Activation Energy:
Concentration- how many molecules present (increase collision between reactants)
Temperature- movement (leads to more forceful collisions)
Reactant Properties- characteristic ( size & phase - solid, liquid, gas)
Presence or Absence of Catalyst- helper (lowers activation energy, which increases reaction rate)
41
Catalyst
*Enzyme*
| SPEEDS up chemical reactions by LOWERING activation energy;
42
Induced-fit Mechanism
Enzymes interaction with subtrates;
| Binds subtrates that causes small shape change, which brings subtrate to the transition state;
43
Enzyme deficiency’s
Tay-Sachs
Lack of hexosaminidase;
| Ganglosides accumulate around neurons in the brain
44
Enzyme Deficiency’s
SCIDS
Lack of adenosine deaminase;
45
Enzyme Deficiency’s
Phenylketonuria
Lack of phenylalanine hydroxylase;
Results in seizures or mental retardation
46
Inorganic Compounds
Lack carbon- NO;
Molecules have FEW ATOMS;
Example- water, salts, acids, and bases
Co2, HCO 3 (-), H2CO3
47
Organic Compounds
ALWAYS contains carbon;
| Carbon BONDS to Hydrogen;
48
Water
60-80% mass of the body;
```
*Functions * -
High heat capacity (body temp)
Carries heat when evaporates (sweat)
Cushions body structures (heavy)
Acts as lubricant (serous fluid)
```
49
Universal solvent ?
```
Water;
Only dissolves in a HYDROPHILIC substance;
*Polar Covalent Molecule*
-oxygen pole (-)
-hydrogen pole (+)
```
50
Hydrophilic Solutes
Solute that contains polar covalent bonds- Dissolves In;
51
Hydrophobic Solutes
Mainly non-polar covalent bonds present- Doesn’t dissolve in;
52
Acid
Goes in to one or more H+ ions;
| *PROTON DONOR*
53
Base
Substance mainly dissolves in OH- ions;
Alkali;
If base is added, # of ions DECREASE
54
Acids & Bases of Ph
Ph of 7= NEUTRAL; (hydrogen ions and base ions are equal)
Ph 7 or less=ACIDIC; (hydrogen ions OUT NUMBER base ions)
Ph 7 or greater=BASIC/ALKALINE (base ions OUT NUMBER hydrogen ions)
55
Buffer
Chemical system that resist changes in pH; *
| Blood pH range- 7.35-7.45; *
56
Acidosis
Build up of acid in bloodstream;
CAUSES:
- hypoventilation
- rapid respiration
- pale skin
- drowsiness
- muscle weakness
57
Alkalosis
Excess of base in the blood stream;
CAUSES:
- seizures
- rapid breathing
- low or normal blood pressure range
- confusion
- nausea
- numbness
58
Salt
```
Any METAL (+) cation and NONMETAL (-) anion, HELD BY ionic bonds;
Can dissolve in water to form ELECTROLYTES
```
59
Monomer
Single subunit; Mono=1
| Forms or builds polymers by DEHYDRATION SYNTHESIS;*
60
Hydrolysis
*Catabolic* reaction: break polymers into smaller subunits;
61
Carbohydrates
Composed of carbon, hydrogen, and oxygen;
FUEL FUNCTION;
Monosaccharides *[ ONE sugar] *
Example:
- Glucose
- Fructose
- Galactose
62
Polysaccharides
Many sugars;
POLY=1 or more;
*Glycogen is a storage of glucose*
63
Lipid
Non polar and hydrophobic;
| FATS and OILS
64
Fatty Acid
*Lipid monomers*
65
Saturated Fatty Acid
Solid @ room temperature;
| No double bonds
66
Mono saturated Fatty Acids
Liquid @ room temperature;
| One double bond
67
Polyunsaturated Fatty Acids
Also liquid @ room temperature;
| 2+ double bonds
68
Good Fatty Acid
Flaxseed oil and Fish oils;
69
Bad Fatty Acid
Saturated fats;
*Animal fats*
Can increase cardiac disease!
70
Ugly Fatty Acid
Trans fats;
NOT SAFE for CONSUMPTION;
Hydro generated oils
71
Triglycerides
(Triacylglycerol)
| Building blocks : Single glycerol molecules & 3 fatty acids and molecules;
72
Phospholipid
Backbone=Glycerol
Tails=2 Fatty Acids (non polar)
Head=1 Phosphate (polar)
*Vital to cell membrane structure*
73
Steroids
4 ring structure;
*Forms cholesterol (building block)*
Non polar
74
Proteins
Big molecules (macro)
Functions as an Enzyme;
Involved in Movement and used for Fuel
75
Primary structure of a Protein ?
Amino acid;
*20 different types of amino acids in humans*
Monomer of ALL proteins
1) Linked by PEPTIDE bond, Into a POLYPEPTIDE
76
Peptide
Formed from 2+ amino acids linked by peptide bonds;
| 2+ polypeptide chains folded in different/unique structures
77
Fibrous Proteins
Long, Rope-like structure;
Links things Together;
Adds Strength to Structures;
78
Globular Proteins
Spherical shaped;
Functions as enzymes, hormones, and cell messengers
79
Primary Structure
1st level of polypeptide chain
80
Secondary Structure
One or more segments [folded];
- Alpha [helix]
- Beta Pleated sheet
81
Tertiary Structure
3D shape
82
Quaternary Structure
Final level of polypeptide chain;
Links one or more chain together in a SPECIFIC way;
* Critical to function as protein as a whole *
* Shape determines ability to function*
83
Protein Denaturation
[Destroys] shape by [heat], [pH changes], and [chemical exposure]
84
Nucleotide
*Monomer of nucleic acids* ( genetic material)
STRUCTURE:
- Nitrogenous base (RNA & DNA)
- Pentose Sugar
- Phosphate group
85
Nitrogenous Base
Double-ringed adenine & guanine structure; (Purines)
Single-ringed cytosine, uracil, and thymine structure; (Pyrimidines)
86
ATP
Adenine attached to Ribose and 3 phosphate groups;
| *Main source in ENERGY* (die without)
87
ADP
Synthesized from ATP;
Adenine Diphosphate & Phosphate group;
Energy comes from Oxidation
88
RNA
Single strand of nucleotides;
Making of proteins;
Contains all but Thymine;
* C-G*
* U-A*
89
Transcription
Gene for DNA
90
Translation
RNA exists in the nucleus;
| Making of protein
91
DNA
2 chains forming DOUBLE HELIX; (weak)
Deoxyribose = Backbone
*Contains genes/recipe for protein synthesis*
BASES:
* A-T*
* G-C*
92
Groups found in Amino Acids?
Amino acid & Carboxyl acid
93
Two organ systems that maintain pH balance ?
Respiratory & Urinary system
94
Highest hydrogen Ion concentration ?
PH 1
95
Primary lipid ?
Phospholipid
96
If blood rises above 7.45, body system will suffer from?
Alkalosis
97
Which structure of nucleic acid NOT contain Uracil?
| DNA or RNA
DNA
98
Is fatty acid considered a polymer ?
NO
99
If there are more hydrogen ions present, will the solution be more acidic or basic?
Acidic
100
Is water an organic molecule ?
No
101
What is Hydrolysis ?
Reaction of water breaking down large molecules into small molecules
102
Amino acid are monomers for?
Proteins
103
Which polymer group is responsible for storage and execution for genetic code?
Nucleic acids
104
Why does water allow high density ?
To protect body structure and allow cushion
105
Organic vs Inorganic
Inorganic lacks carbon
