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Atom (definition, composition, where things inside of it are located)
Basic unit of matter; composed of protons (+), neutrons (0), and electrons (-); protons and neutrons located in nucleus; electrons move around the nucleus (# of electrons=# of protons)
Neutron
Subatomic particle found in the nucleus of an atom, carrying no electric charge but contributing to the atom's mass.
Atomic Number
The number of protons in an atom's nucleus. It determines the element's identity on the periodic table.
Molecule
Two or more atoms bonded together
Compound
Two or more different atoms bonded together
Nucleus
Organelle in a cell that contains genetic material and controls cell activities.
Electron
Subatomic particle with a negative charge found in atoms, involved in chemical bonding and electricity conduction.
Element
A substance made up of only one type of atom, characterized by its atomic number and chemical properties.
What are the four common elements that make up 96% of living things?
Oxygen, carbon, nitrogen, and hydrogen
Matter
Anything that take up space and has mass
Atomic Structure
Inner to outer=2,8,8
Isotopes
Atoms of the same element that have a different number of neutrons
When the energy levels are not filled, atoms tend to react with other atoms to fill them. This is called the _____ ____.
Octet rule
Chemical Bonds
The forces that hold together atoms that make up compounds
Ionic Bond
Bond in which electrons are transferred from one atom to another
Ions
Charged atoms that have lost or gained electrons
Covalent Bonds
Bond in which electrons are shared between atoms
Polar Covalent Bond
Unequal sharing of electrons
Non-Polar Covalent Bond
Equal sharing of electrons
Hydrophilic
Water loving, ionic compounds, polar covalent
Hydrophobic
Water fearing non-polar covalent
How to find the number of neutrons
Atomic mass - atomic number
Nonstable Atom
An atom with an unstable nucleus that undergoes radioactive decay to achieve a more stable configuration.
Hydrogen Bond
Weak attraction between a hydrogen atom and an electronegative atom like oxygen or nitrogen in a molecule.
Double Bond
Type of covalent bond where two pairs of electrons are shared between two atoms, creating a stronger bond than a single bond.
Stable Atom
Has a balanced number of protons and electrons, ensuring it does not decay or undergo radioactive decay.
Does making a bond store energy or release energy?
Releases
Cohesion
Attraction between molecules of the SAME substance
Surface Tension
The property of a liquid that allows it to resist an external force due to the cohesive nature of its molecules at the surface.
Electronegativity
Electronegativity is the measure of an atom's ability to attract and hold onto electrons in a chemical bond.
Adhesion
Attraction between molecules of DIFFERENT substances
Water is a _____ ________ ________ compound.
Polar covalent molecule
Charge of Hydrogen and Oxygen
Hydrogen=+, oxygen=-
Why is water like a magnet?
Because the hydrogen has a positive pole and the oxygen has a negative pole
Hydrogen Bonding
The partial + and - charges allow H2O molecules to attract each other or stick together through hydrogen bonds
Hydrogen bonds are ____ bonds that can be ______ ______.
Weak; easily broken
Water’s Heat Capactity
Water can absorb large amounts of thermal energy before its own temperature begins to rise; water acts like a heat buffer for the globe
Ice is ____ _____ than liquid water.
Less dense
Why is water the universal solvent?
Because it can dissolve most substances
Soultion
Liquid consisting of uniform mixture of two or more substances
What are the two parts of a soultion?
Solvent (liquid (dissolving agent)) and solute (substance dissolved)
Dissasociation
Breaking apart of water molecules
If the number of ________ ____ is _______ than hydroxide ions, the solution is an ____.
hydrogen ions; greater; acid
If the number of ________ ____ is _______ than hydrogen ions, the solution is a ____.
hydroxide ions; greater; base
Buffer
Chemical substance that neutralizes small amounts of either an acid or a base
pH
pH is a measure of the acidity or basicity of a solution on a scale from 0 to 14
A beaker of acid would have more…
H + (hydrogen)
A beaker of base would have more…
OH - (hydroxide)
pH scale
Below 7=acidic, 7=neutral, above 7=basic
Activation Energy
The energy needed to get a reaction started
Catalyst
Lowers the amount of activation energy needed for a chemical reaction to begin (also known as an enzyme)
Enzyme
Proteins that speed up chemical reactions that take place in cells by lowering activation energy
Enzymes are _______.
Specific
What do enzymes typically end in?
ase
Substrate
Reactants of an enzyme catalyzed reaction
Complex
Joining together of the enzyme and substrate
How is an enzyme made?
The substrate binds to the active site which have complementary shapes (like the lock and key model)
Can enzymes be used multiple times?
Yes, as long as their active site does not change
Denatured
Protein’s shape is changed
What two factors can denature an enzyme?
pH (too high or low) and temperature (to high)
Exergonic Reaction
A chemical reaction that releases energy to the surroundings, usually in the form of heat or light.
Endergonic Reaction
A chemical reaction that requires an input of energy to proceed, typically absorbing energy from the surroundings.
Organic Chemistry
Carbon based compounds associated with living organisms
Inorganic Chemistry
Non-carbon based compounds associated with non-living things
Why is carbon a unique element?
Because of its ability to form a wide variety of molecules
Functional Groups
The non-hydrocarbon parts of the molecule
Functional groups are a cluster of _____ that influence the ________________ of the molecule they compose.
Atoms; characteristics
Hydroxyl Group
-OH
Carbonyl Group
-C=O
Carboxyl Group
-COOH (hydroxyl + carbonyl)
Phosphate Group
-PO4
Amino Group
-NH2
Monomer
Small building blocks that make up cells
Polymer
Many monomers bonded together (monomer--→polymer—→macromolecule)
Polymers are built and broken down into monomers using what two reactions?
Dehydration synthesis and hydrolysis
Dehydration Synthesis (aka condensation reactions)
A chemical reaction where two molecules combine to form a larger molecule, producing a water molecule as a byproduct.
Hydrolysis
Process of breaking down a compound by reacting it with water. Commonly used in digestion to break down large molecules into smaller ones for absorption.
Polymerization
Forming complex molecules by joining monomers together
Carbohydrates contain…
C,H,O (1:2:1 ratio)
Function of Carbohydrates
Store short term energy
Carbohydrates typically end in…
ose
Carbohydrates Functional Groups
Hydroxyl and carbonyl
Monomers of Carbohydrates
Monosaccharides
Examples of carbohydrates
Glucose (product of photosynthesis), fructose (found in fruit), galactose (found in milk)
Isomer
Compounds with the same chemical formula but different structural formulas
Polymers of carbs
Disaccharide and polysaccharide
Disaccheride
A carbohydrate molecule made up of two monosaccharides joined together through a glycosidic bond.
Examples of Disaccharides in carbs
Maltose (found in malted milkshake), sucrose (plant sap/table sugar), lactose (sugar found in milk)
Polysaccharide
A complex carbohydrate made up of multiple sugar units bonded together.
Examples of Polysaccharides in carbs
Starch (plant energy storage), glycogen (animal energy storage, muscles), cellulose (gives plants structure, cell wall, AKA fiber)
Lipid
Organic compounds that are insoluble in water but soluble in organic solvents.
Lipids contain…
C,H,O
Function of Lipids
Waterproof coverings, long term energy storage in animals, aids in insulation and protection (adipose tissue), makes up cellmembrane which is made up of phospholipids, hormones and vitamins
Monomers of Lipids are…
Glycerol and fatty acids
The glycerol portion of the lipid is _____ (__________), while the fatty acid tail is ___________ (__________).
polar (hydrophilic); non-polar (hydrophobic)
Saturated Fats
Have only single bonds between the carbons (solid at room temp.)
Examples of Saturated Fats
Butter and animal fats
Unsaturated Fats
Have at least one or more double or triple bonds between the carbons (liquid at room temp.)
Examples of Unsaturated Fats
Oils
Types of lipids
Triglyceride, phospholipid, steroids