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Matter anything that has weight and takes up space including solids, liquids and gases Matter is composed of fundamental particles called elements Elements compounds, bulk elements, trace elements and ultra trace elements Elements common ones are iron, copper, gold, aluminum, carbon, hydrogen and oxygen Bulk Elements large amounts in body l carbon, hydrogen, oxygen, nitrogen, sulfur & nitrogen Trace Elements small amounts that are apart of enzymes and proteins Ultra Trace Elements vital in small amounts but toxic in large amounts Atoms smaller particles that compose elements Atoms made up of protons, electrons and neutrons Atoms central portion called the nucleus made up of protons, electrons & neutrons Protons positively charged particles Electrons negatively charged particles Neutrons neutrally charged particles Atomic # the number of protons in the atom Atomic # organizes the Periodic Table Atomic Weight the number of protons + neutrons Isotopes atoms that have the same # of protons but different # of neutrons Isotopes same atomic # but different atomic weight Isotopes atomic weight is usually listed as the average of all isotopes of that element Radioisotopes unstable isotopes of an element Radioisotopes unstable nuclei that decompose releasing energy or piece of themselves until they reach a stable state Radioisotopes they are radioactive and their energy released is atomic radiation Atomic Radiation 3 common forms Alpha 2 protons & 2 neutrons that move slowly and cant penetrate matter Beta electrons - travel faster and penetrate matter Gamma X-radiation - most penetrating Molecules 2 or more atoms combine to form a distinctive kind of particle Compounds formed when 2 or more atoms of different elements combine Molecular Formula short hand to write number and types of atoms in molecule Molecular Formula example H2 O Bonds atoms combine with other atoms forming links Electron Shells electrons found in region of space around the nucleus Electron Shells also called energy shells Electron Shells can only hold specific number of electrons in each shell First Shell 2 electrons ( closest to nucleus) Second Shell 8 electrons Third Shell 8 electrons usually but can hold up to 18 Outer Shell what determines the atom's ability to react Lower Shells shells closest to the nucleus have to be filled first Octet Rule eight electrons in the outer shell of an atom makes it more stable Inert atoms with their outermost shells filled Ions atoms with incompletely filled shells that tend to lose, gain or share electrons Anions atoms that carry a negative charge due to having more electrons than protons Anions tend to donate or share electrons Cations atoms that carry a positive charge due to having more protons than electrons Cations tend to gain or share electrons Ionic Bond opposite charged ions attract ( anions & cations) Ionic Bond donating electrons make that atom positive and the one receiving negative Ionic Bond after donating they attract and become bonded together Covalent Bond atoms bond by sharing electrons Covalent Bond shared electrons orbit around the nuclei of all the atoms Covalent Bond if more than one electron is shared this called a double or triple bond Bonds Ionic- giving away Covalent- sharing Polar unevenly shared electrons Polar electrons spend more time at one end of the molecule Polar have uneven number or electrons and protons due to uneven distribution making one end negative and other positive Polar attraction between polar molecules form hydrogen bonds Hydrogen Bond involves the hydrogen atom of the molecule attracting another polar molecule Hydrogen Bond usually a weak bond Chemical Reactions break or form bonds Reactants molecules, atoms or ions that are being changed by the reaction Products what results from the reaction Synthesis when reactants bond together to form a more complex product Synthesis Example A+B becomes AB Decomposition when the reactants break down to form a simpler product Decomposition Example AB becomes A+B Exchange Reaction parts of two molecules change or trade positions Exchange Reaction Example AB +CD becomes AD+CB Reversible Reactions can go either direction and symbolized by arrows going both directions Reversible Reactions amount of energy, product and reactants determine direction Catalyst molecules that influence the rate of the reactions Electrolytes electrically charged particles that conducts electric currents, substances that release ions in water, water being polar ionically bonds with salt to dissociate into individual ions Solvent liquid, usually water, in which particles are mixed Solutes particles mixed in the solvent Solution mixture of solvent and solutes that does NOT settle out when left set Suspension mixture of solvent and solutes, DOES settle out if left set Colloid mixture of solvent and solutes, does NOT settle out when left set, semi-solid and gelatinous Acid substance the release hydrogen in water Base substance that releases ions that combine with hydrogen ions, usually (OH-) Salt substance formed by the reaction between an acid and a base pH measures the concentration of acids and bases pH as the concentration of hydrogen increases the pH decreases and the solution becomes more acidic pH as the concentration of hydrogen decreases the pH increases and the solution becomes more alkaline or basic pH distilled or pure water is neutral a 7 on the scale pH scale 0-6.99 acid 7 neutral 7.7-14 basic Human Body and pH ideal is 7.35 to 7.45 below is acidosis and above is alkalosis Inorganic Substances water, oxygen, carbon dioxide and inorganic salts Water the most organic that makes up 2/3 of the human body, most reactions occur in water, responsible for transporting substances through the body, while also absorbs and transports heat Oxygen used in most energy producing reactions in the cells Carbon Dioxide produced as a waste product from most metabolic reactions Inorganic Salts source of ions and electrolytes, essential for electrolyte balance and utilized in many metabolic processes in the body Organic Substances generally contain carbon and hydrogen consist of carboydrates, lipids, proteins and necleic acids Carboydrates provides energy, contains C, H, and O Simples Carboydrates monosaccharides (glucose, fructose and galactose) and disaccharides (surcrose and lactose) Complex Carboydrates polysaccharides that include cellulose, glycogen and starch Lipids perform vital functions in cells and form the cell membrane Lipids include fats, phospholipids, and steroids that contains C, H, and O Fats supplies energy, composed of fatty acids and glycerol Saturated Fat single carbon-carbon bonds linking the carbon atoms the fatty acid Mono-saturated Fat one double bond linking carbon atoms Poly-saturated Fat two or more double carbon bonds Triglyceride glycerol molecule is united with 3 fatty acid molecules Phospholipid Molecules have 2 fatty acid molecules a glycerol molecule and a phosphate group Phosphate Group makes it partially soluble in water (hydrophilic) Fatty Acid portion is insoluble in water (hydrophobic) Phospholipid Molecules essential for the formation of the cell membrane and other cellular structures Steroids complex structures of connected rings of carbon atoms Steroids cholesterol is the most important steroid in the human body, forms the basis for other steroids such as hormones Proteins many functions such as: structural materials, energy sources, hormones, receptors, antibodies and enzymes Amino Acids building blocks of proteins, containing C, H, O, N and sometimes S Amino Acids 20 different amino acids in living organisms Amino Acids comprised of amino group (NH2) at one end and a carboxyl group (COOH) at the other end, there is a single bond between these, bonded to this central carbon is a hydrogen atom on one side and a side chain or R group on the other R Group is what makes each amino acid different Proteins covalent bonds link amino acids together Dipeptide 2 amino acids linked Tripeptide 3 amino acids linked Polypeptide more than 3 amino acids linked 100 amino acids linked together constitues a protein 4 Levels of Protein Structures primary, secondary, tertiary and quaternary Primary chain Secondary pleated or twisted Tertiary folded Quaternary polypeptides linked to form a bigger structure Proteins shape 3 dimensional shape or conformations is what gives proteins their distinct functions Denature when proteins lose their shape (denature) they can no longer perform their functions Nucleic Acids building blocks of gene, direct the cell's activity and contains C, H, O P, and N Nucleotides form the nucleic acids Nucleotides consist of a 5-carbon sugar, a phopate group and one of several organic bases Nucleotides linked in a chain form a polynucleotide Nucleic Acids two types- RNA (ribonucleic acid) and DNA (deoxyribonucleic acid) DNA double polynucleotide chain, has the ability to replicate or make copies of itself