CH2 Flashcards
(100 cards)
1
Q
Matter
A
Physical substance; occupies space and has mass
2
Q
Mass
A
- Amount of matter it contains
- Mass is the same when gravity is changed
3
Q
Weight
A
An object’s weight is its mass as affected by the pull of gravity
4
Q
Elements
A
Substances that cannot be created/broken down by ordinary chemical means;
118 fundamental substances
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Q
Chemical Symbol
A
Each element designated by 1 or 2 letters
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Q
Compounds
A
Two or more elements joined by chemical bonds
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Q
Minor Elements
A
Calcium, phosphorous, potassium, sulfur, sodium, chlorine, magnesium
8
Q
Atoms
A
Smallest unit of an element that retains the unique properties of that element
9
Q
Subatomic Particles
A
Proton, neutrons and electrons
- The # of protons and electrons within a neutral atom are equal, thus, the atom’s overall charge is balanced
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Q
Protons
A
- Largest particle in atom’s nucleus
- Heavy subatomic particle having a +
charge
(p+)
11
Q
Neutrons
A
Heavy subatomic particle having (n)o electrical charge
- In atom’s nucelus
12
Q
Electrons
A
- orbits around nucleus
- Subatomic particle having a - charge
- Nearly no mass
(e-)
13
Q
Electron Shell
A
Layer of electrons that encircles the nucleus at a distinct energy level; electron cloud
- Holds 8 electrons except the first shell, which can only hold 2
14
Q
Valence shell
A
Atom’s outermost shell layer
- Depends on number of electrons in an atom for them to have more than one electron shell
15
Q
Octet Rule
A
Atoms are most stable when there are 8 electrons in their valence shell (except hydrogen and helium)
- An atom will give up/gain/share electrons with other atom(s) to have 8 electrons in its own valence shell
16
Q
Atomic Number
A
- # of protons in nucleus of an atom
- # above element that is representative of both the number of protons and electrons
17
Q
Mass Numbers
A
- # of protons and neutrons in nucleus of atom
- Doesn’t always contain same number of protons and neutrons
18
Q
Periodic Table of Elements
A
- A chart identifying elements discovered or synthesized
- Organizes elements according tot heir tendency to react with other elements
19
Q
Common elements in the human body
A
- 4 most abundant elements = 96%
1) Oxygen
2) Carbon
3) Hydrogen
4) Nitrogen
20
Q
Isotopes
A
Atoms of same element, different # of neutrons
some have same chemical properties but different mass numbers b/c of # of neutrons
21
Q
Radioactive isotopes
A
- Elements w/ unstable nuclei or have more than the usual # of neutrons
- Emit radiation from extra energy
-Weak radioisotopes are used in medical diagnostic and treatment procedures
ex: PET scanner - radioactive glucose is injected to detect metabolically active tissues, such as cancerous masses
22
Q
Molecules
A
Stable grouping of 2+ atoms held together by chemical bonds
ex: H2(hydrogen gas) or H2O
23
Q
Compound
A
When a molecule is made up of 2+ atoms of different elements
24
Q
Free Radicals
A
Highly chemically active molecules and ions with an odd # of electrons in their valence shells
- They can form in our body from metabolism of oxygen, food, and/or environmental sources (smoke, sunlight)
- They react with biological molecules like DNA/proteins, and cause cell damage or “oxidative stress”
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Acids
Compound that releases hydrogen ions (H+) in solution
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Antioxidants
Protects cell membranes from free radical damage
- Sources from food or chemically made in our body (turmeric, avocados, sweet potatoes)
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Chemical Bonds
When electrons in atoms valence shell interact with another atom; typically more stable
1) Ionic bonds
2) Covalent bonds
3) Hydrogen bonds
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Ion
Atom with overall + or - charge
- An atom can give away or receive one or more electrons
- Loss of (-) electrons = positive charge
- Gain of electrons = negative charge
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Cation
Ion with + charge - PAWsitive (cat)
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Anion
Ion with - charge - A-Negative
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Ionic Bond
- Creates an ionic compound which holds groups of ion's together by attraction between oppositely charge ions
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Ionic Compound
Dissolves in water because water molecules disrupt ionic bonds and release ions = electrolytes
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Electrolytes
Minerals in our blood/body fluids that carry electric charge
- Affect amount of water in your body, pH of blood, and nerve and muscle function
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Covalent Bonds
These atoms share electrons (do not lose/gain electrons)
- Stronger bond than ionic due to sharing -> does not break in water and can form with the same or different element
Carbon, hydrogen, oxygen atoms are major elements and linked by covalent bonds
35
Non-polar Covalent Bonds
Type of bond that occurs when two atoms share a pair of electrons with each other
- Single covalent bond: single electron pair (2 electrons) shared b/w 2 atoms
- Double covalent bond: two electron pairs shared b/w 2 atoms
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Polar Covalent Bond
Unequal sharing of electrons and hydrogen bonds
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Hydrogen Bonds
Bond between two atoms that are involved in other chemical bonds.
- Bond forms b/w partially positive hydrogen atom of a polar molecule and a partially negative atoms (Oz, nitrogen)
- Holds 2 strands of DNA molecule together
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Polar Molecule
- Molecules with opposing charges at each end "polar opposites"
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Oxidation-Reduction Reactions
One reactant loses electrons (oxidized) while other reactant gains electrons (reduced)
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Oxidation
Loss of electrons (OIL)
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Reduction
Gain of electrons (RIG)
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Catalyst
A substance that increases the rate of a chemical reaction w/o itself undergoing any change
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Enzyme
Biological catalyst that speeds up chemical reactions in a cell or body
+ Composed of protein
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Inorganic Compounds
A substance that does not contain both carbon and hydrogen
ex: H2O, CO2, sodium NaCl
- Water, salts, acids and bases essential to life
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Organic Compound
Contains carbon and hydrogen
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Water
Human body made up of 60% of water
- Help us function:
+ Lubrication and cushion
+ Absorbs or dissipates heat for thermoregulation
+ Universal solvent (liquid capable of dissolving another substance
+ Reactant or product of chemical reaction
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Acids and Bases
Bother compounds can dissociate in water into charged ions or electrolytes
- Inorganic compounds essential to life
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Acids
Release hydrogen ions(H+) in a solution
+ Strong acids dissociate completely, while weak acids do not release all available hydrogen ions
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Bases
Releases hydroxyl ions (OH-) in solution or takes up hydrogen ion H+ present in solution
50
pH
Potential of hydrogen
- Measurement of the concentration of hydrogen ions in solution
- Indicates acidity/alkalinity of a solution
0 = most acidic, 7= neutral, 14= most basic/alkaline
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pH scale examples
0= battery acid, hydrochloric acid
2= lemon juice, vinegar
3= grapefruit juice, soda, tomato juice
5= black coffee
6= milk, urine, saliva
7= blood, water
8= sea water
9= baking soda
11= ammonia solution
13= bleach
14= liquid drain cleaner
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Buffers
- a solution of a weak acid and its conjugate base that can neutralize small amounts of acids or bases in body fluids.
In our blood, helps to maintain pH levels
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Organic compounds in the body
1) Carbohydrates
2) Lipids
3) Proteins
4) Nucleic acids
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Carbohydrates
Sugars and starches
- Composed of carbon, hydrogen and oxygen atoms
- Stored in the form of glycogen in liver and muscles
1) Monosaccharides
2) Disaccharides
3) Polysaccharides
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Monosaccharides
Building blocks (monomers) of carbohydrates, simplest form
+ mono- = one, saccharide = sugar
+ Glucose, fructose and galactose
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Disaccharides
Made by connecting two Monosaccharides
+ Sucrose (table sugar), lactose (milk) and maltose
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Polysaccharides
Polymers of monosaccharides; hundreds or thousands of monosaccharides
+ Starches, glycogen, and cellulose - important in body
+ Starch is broken down into glucose (rice, wheat, potatoes)
+ Cellulose is found in the cell wall of plant cells and is a component of fiber
- Our cells use glucose as fuel
- Glucose is broken down to produce adenosine triphosphate (ATP)
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Lipids
Mostly composed of carbon and hydrogens, a few oxygen atoms
- B/c they're rich in carbon and hydrogens, these molecules are non-polar and hydrophobic (does not mix with water)
- Triglycerides, phospholipids, steroids, prostaglandins, fatty acids
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Triglycerides
Most abundant lipids in our body and diet (fats and oils)
+ Helps protect, insulate, and provide energy
+ Composed of glycerol and 3 fatty acid chains (via dehydration synthesis)
+ Stored as adipose tissue, highly concentrated fat source
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Prostaglandins
- prevents stomach ulcers
- help with inflammation
- dilates airways to lungs
- regulate body temperature
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Fatty Acids
Saturated and unsaturated
- fat soluble vitamins: Vitamins D E K
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Saturated fatty acids
Doesn't have double carbon bonds in the carbon chain, solid, or semi-solid at room temp
- butter, lard
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Unsaturated fatty acids
Has one or more double carbon bonds, chain shape is kinked
+ Liquid at room temp (olive oil)
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Phospholipids
lipid compound in which a phosphate group is combined with a diglyceride.
Important plasma membrane component.
- It's an amphipathic molecule: has a hydrophobic tail and hydrophilic head
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Amphipathic molecules
Chemical compound that has both hydrophilic and hydrophobic parts
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Steroids
Has 4 hydrocarbon rings bonded to a variety of other atoms and molecules
- Steroids include sex hormones and cholestorol
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Cholestrol
An important steroid and the major component of bile acids
+ Modified to make various steroid hormones in our body
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Prastaglandins
Type of of signaling molecules in the body
+ Derived from unsaturated fatty acids, such as omega 3 fatty acids
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Proteins
Polymers of amino acids
+ Amino acids are linked by a covalent bond called the peptide bond to form a peptide (short chain of amino acids) or polypeptide (longer chain)
+ Contains nitrogen, carbon, hydrogen and oxygen and frequently contains sulfur
70
Function of protein in the body
Major components of our cells, tissues, and organs
+ Support - structural proteins (keratin, collagen)
+ Movement - contractile proteins (actin, myosin)
+ Transport - carrier proteins (hemoglobin)
+ Buffering - regulation of pH
+ Metabolism - enzymes
+ Horomones
+ Defense - antibodies
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Protein Shape
Primary, secondary, and teritary structures
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Primary Structure
Sequence of amino acids in the chain determines overall shape of a protein
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Secondary Structures
Alpha-helix and beta-sheet
+ Local structures created by chemical interaction b/w nearby amino acids in a polypeptide chain
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Teritary Structure
3D structure of an entire polypeptide chain containing several secondary structures
+ Some protein, such as hemoglobin are formed by multiple polypeptide subunits coming together
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Structure/function of protein
Changing protein shapes disrupts functions
ex: heat, pH (denature) --> like cooking an egg
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Enzymes
Proteins that catalyze a chemical reaction
+ The reactants in a chemical reaction called substrates, must bind to a specific site called the active site of an enzyme for chemical reaction to take place
+ Shape of active site specifies what substrate can bind to the enzyme
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Nucleic Acids
Polymers of nucleotides
- Contain nitrogen, carbon, hydrogen, oxygen and phosphate
- DNA and RNA are examples of nucleic acids
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Nucleotides
Adjacent nucleotides are bonded together by phsphodiester bonds to form a chain
Composed of :
- Pentose sugar - either deoxyribose or ribose
- Nitrogen - containing base essential for the replication of genetic material, protein synthesis, and cellular metabolism
+ Either pyrimidine (cystosine, thymine or uracil) OR Purine (adenine or guanine)
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Phosphodiester Bonds
A covalent bond that forms the backbone of DNA and RNA
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DNA
Deoxyribonucleic Acid
- Genetic material in nucleus of a cell
- Is a polymer of deoxynucleotides which contains deoxyribose, one phosphate group and nitrogenous base (A, C, G or T)
- Double helix formed by two chains (strands) of nucleotides held together by hydrogen bonds between nitrogenous bases of opposite strands
- Hydrogen bonds form between base pairs
+ Adenine-Thymine
+ Cytosine-Guanine
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RNA
Ribonucleic acid
- Single strand of ribonucleotides containing ribose, one phosphate group, and one nitrogenous base (A, C, G or U)
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Types of RNA
Messanger mRNA
Transfer tRNA
Ribosomal rRNA
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ATP
Adenosine triphosphate
- energy carrying molecule found in cells; breakdown of glucose for energy
- releases free energy when its phosphate bonds are broken, and thus supplies ready energy to the cell to do work.
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Chemical reactions of physiology
Kinetic, potential, chemical
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Kinetic energy
energy of motion, form of energy powers any type of matter in motions, like swimming or running
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Potential Energy
energy of position or the energy that matter holds because of the position or structure of its components
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Chemical Energy
Chemical bonds between atoms and molecules
- Released by chemical bonds
- When bonds are formed -> chemical energy is invested
- When bonds break -> chemical energy is released
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Exergonic Reactions
chemical reactions that release more energy than they absorb; energy EXITs
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Endergonic Reactions
chemical reactions that absorb more energy than they release
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Mechanical energy
sum of kinetic and potential energy
EX: lifting a brick, muscles provide the mechanical energy to move the brick
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Radiant Energy
Energy emitted and transmitted as waves rather than matter
- Varies in length from long radio waves and microwaves to short gamma waves emitted from radioisotopes
- Electromagnetic spectrum
EX: Body uses UV rays from sunlight that’s converted to vitamin D compounded by skin cells
EX: human eye ability to see wavelengths (colors); visible light
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Electrical Energy
supplied by electrolytes in cells and body fluids
EX: helps transmit impulses in nerve and muscle cells
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Synthesis Reaction
chemical reaction that results in the synthesis (joining) of formerly separate components. (A + B→AB)
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Decomposition Reaction
chemical reaction that breaks down or “decomposes” something larger into its constituent part (AB→A+B)
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Exchange Reaction
synthesis and decomposition; chemical bonds are both formed and broken, and chemical energy is absorbed, stored, and released (A+BC→AB+C) into chemical bonds
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Reactants
one or more substances that enter into the reaction
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Products
one or more substances produced by chemical reaction
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Factors that influence chemical reactions
Temperature, concentration, pressure (volume of space) *diffusion
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Monomers
molecules bond with identical molecules (covalnet bond) to form polymers
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Polymers
large molecules made up of many monomers joined together
