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148 Cards in this Set
- Front
- Back
Matter Consists of
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Mass and Volume
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Mass
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is Weight
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Volume
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Takes up Space
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Properties of Matter
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Solid, Liquid, Gas. They Consist of Atoms
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Smallest unit of an element that can exist alone
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Atom
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Subatomic Particles of an Atom
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Protons (p)
Neutrons (n) Electrons (e) |
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Non Subatomic Particle
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Nucleus
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Positive Charge
in the Nucleus |
Protons
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Neutral Charge (0)
In the nucleus |
Neutrons
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Negative Charge
Not in Nucleus Moves at Speed of Light Spec of Sand Compared to Protons and Neutrons |
Electrons
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Diagram of an Atom
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Substances that consists of atoms with unique properties
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Element
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Calculating Protons Neutrons and Electrons
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Protons = Atomic Number
Electrons = Atomic Number Neutrons = Atomic Mass - Atomic Number |
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Calculating Protons Neutrons and Electrons of Sodium
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How Many Electrons in First Electron Shell
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2
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How Many Electrons in Second Electron Shell
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8
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How Many Electrons in Third and Beyond Electron Shell
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18
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How Many
Protons Electrons Neutrons |
Protons = 8
Neutrons = 8 Electrons = 8 |
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How Many
Protons Neutrons Electrons |
Protons = 1
Neutrons = 0 Electrons = 0 |
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What is Electron Configuration of Argon
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Atoms of the same element of with different Atomic Masses
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Isotopes
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What causes an Isotope
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Different Number of Neutrons in Nucleus
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Sharing of a pair of Electrons between 2 Atoms
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Covalent Bond
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Types of Covalent Bonds
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Polar Covalent Bond
Non Polar Covalent Bond |
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Polar Covalent Bond
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The Electron Between 2 Atoms are Shared UNEqually
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Non Polar Covalent Bond
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Electrons are shared equally between atoms
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Substance made up of atoms with 2 or more elements (in a fixed ratio)
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Compounds
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Only Consists of Covalent Bonds (smallest unit is a Molecule)
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Molecular Bond
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Structural Formula of Water
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Most Common Elements
(CHNOPS) + Ca |
Carbon
Hydrogen Nitrogen Oxygen Phosphorus Sulfur Calcium |
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Most abundant Element in the universe
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Hydrogen
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Electrons that are Shared unequally and generates partial electron charges on the surface of the molecule
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Polar Covalent Bond
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Most Electronegative Element
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Oxygen
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Least Electronegative Element
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Hydrogen
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Diatomic Molecules (Not Compounds)
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Elements of Same Type Bonded Together:
O2 N2 H2 |
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Ionic Bonds made up of oppositely charged ions
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Ionic Compounds
Example Na+ Cl- |
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Attractive force between oppositely charged ions
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Ionic Bond
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Atom or group of atoms tat have lost or gained an Electron
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Ion
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Positively Charged Ion
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Cat Ion
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Negatively Charged Ion
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Anion
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Single Atom Ion
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Monoatomic Ion
Na+ Cl- |
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Example of Ion
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4 Polyatomic Ions
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Phosphate
Hydroxyl Bicarbonate Ammonium |
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Polyatomic Ion
Phosphate Ion |
PO4 -3
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Polyatomic Ion
Hydroxyl Ion |
OH -
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Polyatomic Ion
Bicarbonate |
NCO -3
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Polyatomic Ion
Ammonium |
NH4
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Sodium Atom to Sodium Ion
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Loses An electron to Become an Sodium Ion
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Chlorine atom to Chloride Ion
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Chlorine Atom gains an electron to become an Chlorine Ion
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Absence of Water
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Dehydration
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Describe how Salts breakup in H2O
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H2O breaks the ionic bond and surrounds the ions with hydration spores which prevents the ions from rebinding
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Weak Attraction Bonds between Polar Covalent Bonds
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Hydrogen Bonds (H-Bond)
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Up to how many bonds per water molecule
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4
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How does water become slippery and wet
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H-Bonds rapidly break and rebind
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How do you make h-bonds harder to break
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drop the temperature
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Sticking together of like molecules (H2O)
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Cohesion
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Sticking together of different molecules (water on wall)
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Adhesion
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Substance that increases the Hydrogen Ion Concentration [H+] of a water base solution
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Acids
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How Do water Molecules Link together
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Through an H-bond
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How do you make Hydrogen Concentration
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Remove the electron from the Hydrogen Atom to make it a Hydrogen Ion
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Substance that releases Hydrogen Ions into a Solution and increases [H+] of an aqueous
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Acid
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Decreases the pH of a solution and makes it more Acidic
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Proton Donors
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How does adding HCl make a beaker of Water more Acidic
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H+ unbinds from the HCl making the solution more acidic
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Substance when added to water will decrease [H+] of that solution
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Base (alkaline)
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Value along the pH scale that measures the [H+] of a solution
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pH (Power of Hydrogen)
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Calculating pH
pH = log10([H+] mole/L) pH = log10(1x10-3 mole/L) |
3
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How to Make a Base by adding NaOH
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OH- combines with H+ from H20 and removes H+ from Solution
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Chemical Added to solution so that the solution will resist changes in pH
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Buffer
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Buffer in an Acid
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Binds to H+
Acids have High H+ |
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Buffer in a Base
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Releases H+
Bases has low H+ |
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Acidic Solution on pH scale
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0-6
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Base (alkaline) on a pH scale
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7.01-14
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Water on a pH scale
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7
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pH is inversely proportional to [H+]
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pH goes up, [H+] goes down
pH goes down, [H+] goes up |
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Calculating Scientific Notation
10 -6 10 +5 |
10 -6 = .000001
10 +5 = 100000 |
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Compound that DOESNOT contain Carbon
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Inorganic Compound
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Carbon Containing Compound
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Organic Compound
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Exception in Inorganic Compound
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CO2
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Inorganic Compounds
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NaCl
H2O O2 MgSO4 |
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3 Solutions of Water
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Cytoplasm
Interstitial Fluid Blood Plasma |
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Cytoplasm
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Water in Cells
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Interstitial Fluid
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Water Between Cells
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Blood Plasma
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Water that circulates in blood vessels
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Solvent
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Always Water
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Solute
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Mix into a solvent
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Ease at which it can be mixed into water
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Solubility
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Easy to dissolve
(Salt, glucose) |
Hydrophilic
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Difficult to Dissolve
(Fat, oil, wax) |
Hydrophobic
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Organic Compounds
4 |
Carbohydrates
Lipids (fats, oils) Proteins Nucleic Acids (DNA, RNA) |
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3 Carbon Skeletons
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Straight Chain
Branched Chain Ring Chain (Contains O or N) |
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Straight Chain Carbon
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Branched Chain Carbon Skeleton
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Ring Chain Carbon Skeleton
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Groups of atoms that attached to carbon chain. They have chemical properties of organic compounds
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Functional Groups
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List 6 Functional Groups
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Hydroxyl -OH
Carboxyl -COOH Amine -NH2 Carbonyl -C=O Phosphate -PO4 Methyl - CH3 |
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Hydroxyl Group Functional Group
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Carbynol
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Carboxyl Group
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Amine Group
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Phosphate Group
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Methyl Group
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Includes sugars and large complex molecules like starch and glycogen
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Carbohydrates
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List 4 Types of Carbohydrates
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Monosaccharides
Disaccharides Oligosaccharides Polysaccharides |
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Building block unites that are used to make other carbohydrates
Contains 3-7 Carbons |
Monosaccharides
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Monosaccharides
5 in carbon Skeleton |
Pentose
Ribose, Deoxyribose |
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Monosaccharides
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Hexose
*Glucose*, Fructose |
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Drawing of Glucose
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Glucose
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To make ATP (dextrose)
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2 Monosaccharides bonded together
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Disaccharides
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Bond between 2 Disaccharides (Glucose and Fructose)
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Covalent Bond called
Glycosidic Bond |
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When a H and OH are removed form the reactants and end up as a water molecule as a covalent bond forms
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Dehydration Synthesis
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Example of Dehydration Synthesis
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Glucose + Fructrose Form Sucrose + H20 molecule
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7-10 Monosaccharides linked together to make glucose
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Polysaccharides
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Animal Cells are made up of
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7-10 Glycogen liked by Glycocidic Bonds
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Plant cells are made up of
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Starch
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Types of Lipids
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Fats
Oils Steroids Phospholipds |
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Fatty Acids
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Saturated Fats
Unsaturated Fats |
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Saturated Fats
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DOESNOT contain a double bond (C=C) in the hydrocarbon chain between 2 Carbons
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Unsaturated Fats
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Contains at least 1 double bond (C=C) between 2 carbons in the hydrocarbon chain **Fewer Hydrogen**
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Saturated Fatty Acid Drawing
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Drawing of Unsaturated Fatty Acids
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Triglycerides
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Fats and Oils
3 Carbon glycerol + 3 Fatty Acids Forms and Estrobond when joins a Saturated Fatty Acid |
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Lipids
3 |
Fats
Oils Phospholipids |
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Fats
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Saturated Fats found in Animals
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Oils
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Unsaturated Fats found in Plants
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Phosopholipid
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Drawn as Clothes Pin
3 Carbon Clycerol +FA + P |
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Phospholipid Drawing
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Linked by peptide bonds and has a Biological function
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Proteins
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Speeds of the rate of chemical reaction in Proteins
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Catalyst
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Protein Hormones
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Insulin
Growth Hormone |
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Alter Structure of Protein by exposing it to hard conditions (becomes not functional)
Boiling Strong Acids |
Denaturation
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Nucleic Acids
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DNA
RNA |
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3 Carbons in Nucleatides
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Pentosugar (5 Carbons)
N-Base Phosphate Group |
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Bond between DNA
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Phosdyester Bond
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Bonds between Amino Acids
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Peptide Bonds
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Drawing of Amino Acid
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Phospholipid Drawing
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DNA Bond
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Phosphodiester bond
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High energy phosphate bond
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ATP
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When is ATP energy released
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when the terminal phosphate bond is broken
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Process within cell by which fule substrates are broken to CO2 and H20 to make ATP
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Cellular Respiration
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Why Do we breathe O2
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Cells take in O2 to make ATP
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Poison that prevents cells fro making ATP
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Cyanide
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ATP Dependent Processes
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Muscle Contractions
Urine Formation Thinking Sperm Protein Synthesis Steroid Hormone |
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Sum of total of all reactions occurring within a living system
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Metabolism
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2 Phases of Metabolism
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Anabolism
Catabolism |
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Reactions that build larger molecules from smaller ones
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Anabolism
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Decomposition of break down reactions where larger molecules are broken down into smaller ones
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Catabolism
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