Term
|
Definition
| the chemistry of living organisms |
|
|
Term
|
Definition
|
|
Term
|
Definition
|
|
Term
|
Definition
|
|
Term
|
Definition
|
|
Term
|
Definition
|
|
Term
|
Definition
|
|
Term
|
Definition
|
|
Term
|
Definition
| together: synthesis - process by which chemicals join to form new types of chemicals |
|
|
Term
|
Definition
| all matter is composed of one or more elements that take up space and have mass |
|
|
Term
|
Definition
| Energy of movement: thermal, mechanical, electrical, magnetic |
|
|
Term
|
Definition
| stored energy: chemical, elastic, nuclear, gravitational |
|
|
Term
|
Definition
| form of energy we can hear |
|
|
Term
|
Definition
| form of energy our eyes can detect |
|
|
Term
|
Definition
| substances that cannot be broken down into simpler substances by ordinary chemical methods. |
|
|
Term
|
Definition
| are unreactive because they already have the desired 8 total electrons in their outermost energy level |
|
|
Term
|
Definition
| smallest particle of an element that has the properties of that element |
|
|
Term
| major elements of the human body |
|
Definition
| oxygen, carbon, nitrogen, and hydrogen |
|
|
Term
|
Definition
| composed of 3 subatomic particles: proton, neutron, and electron |
|
|
Term
|
Definition
|
|
Term
|
Definition
|
|
Term
|
Definition
| carries a single negative charge (smaller than the proton and neutron, is not located in the nucleus) |
|
|
Term
|
Definition
| central part of the atom - composed of protons and neutrons. |
|
|
Term
|
Definition
| they spin around the nucleus at close to the speed of light. Electrons are equal to the number of protons |
|
|
Term
| what is the atomic number? |
|
Definition
| number of protons in the nucleus of one atom |
|
|
Term
|
Definition
| the total of protons and neutrons in an atom |
|
|
Term
|
Definition
| an atom with the same # of protons and electrons but a different # of nuetrons |
|
|
Term
| Heavy isotopes (medical imaging) |
|
Definition
| an isotope with more neutrons - often unstable and radioactive. some of these radioactive isotopes are used in medical imaging |
|
|
Term
|
Definition
| proton and electron don't change, always 1. The nuetron can change by having 0, 1, 2 etc neutrons |
|
|
Term
|
Definition
| easily identified with a device called a mass spectrometer, help researchers determine conditions in the blood and tissue when radioactivity is not desirable |
|
|
Term
|
Definition
| (positron emission tomography) can detect the activity of cells and reveal some cancerous masses bc cancer cells consume glucose at a high rate to fuel their rapid reproduction |
|
|
Term
|
Definition
|
|
Term
|
Definition
| the sum of protons and neutrons in an element |
|
|
Term
|
Definition
| two or more atoms combined |
|
|
Term
|
Definition
| 2 or more different kinds of atoms bound together (chemically combined) |
|
|
Term
|
Definition
| 2 or more compounds that are physically intermixed. There is no bonding |
|
|
Term
| are all molecules compounds?? Are all compound molecules?? |
|
Definition
| No, and yes. all molecules are not compounds but all compounds are molecules |
|
|
Term
|
Definition
| substance in the greatest amount |
|
|
Term
|
Definition
| substance in smaller amount |
|
|
Term
|
Definition
| completely mixed. same composition throughout |
|
|
Term
|
Definition
| composition is dissimilar in different areas of the mixture. not fully mixed together |
|
|
Term
|
Definition
| a solution is a homogenous mixture when 2 or more substances are dissolved together |
|
|
Term
|
Definition
| contains particles that are in-between in size. they do not separate into layers. fog is a colloid. a property of a colloid is the scattering of light. |
|
|
Term
|
Definition
| a suspension is a heterogenous mixture, it separates over time. a great example is oil and vinegar or sand and water. |
|
|
Term
|
Definition
| no chemical bonding, can be separated by physical means, can be homogenous OR heterogenous |
|
|
Term
|
Definition
| chemical bonding, can only be separated by breaking bonds, ALWAYS homogenous |
|
|
Term
|
Definition
| the outermost shell of an atom. the first shell can hold 2 electrons and each subsequent shell can hold 8 electrons |
|
|
Term
|
Definition
| stable and unreactive (noble gases) |
|
|
Term
| atoms with valence shells that are not full |
|
Definition
| are reactive and will want to form bonds with other atoms |
|
|
Term
|
Definition
| atoms link by forming a chemical bond. |
|
|
Term
|
Definition
| the valence shell is full |
|
|
Term
|
Definition
| do not have their outermost energy level fully occupied by electrons therefore are able to interact with other elements |
|
|
Term
|
Definition
| an atom that has an electrical charge - whether positive or negative - is an ion |
|
|
Term
|
Definition
| formed when 1 or more electrons are transferred from one atom to another. A reaction that links two elements with an ionic bond. completely transferred |
|
|
Term
|
Definition
| the atom that loses electrons becomes positive |
|
|
Term
|
Definition
| the atom that gains electrons becomes negative |
|
|
Term
|
Definition
| atoms share electrons (sharing is caring!) |
|
|
Term
|
Definition
| electrons are shared unequally. example water |
|
|
Term
|
Definition
| if electrons are shared equally. example carbon dioxide |
|
|
Term
|
Definition
| occurs when a hydrogen atom covalently bonded to something is attracted to another electron-needy atom. This is a very weak bond; their purpose is to break easily and come back together. this is important for protein and nucleic acid structure |
|
|
Term
|
Definition
| A+B=AB. bonds are created. forms larger and more complex molecules. important for body growth and tissue regeneration |
|
|
Term
|
Definition
| AB -> A+B bonds are broken, and large molecules are broken down into smaller molecules or atoms. important in digestion |
|
|
Term
|
Definition
| involve both synthesis and decomposition. bonds are made and broken. AB+C -> AC+B |
|
|
Term
| oxidation-reduction (REDOX) reactions |
|
Definition
| ALL three chemical reactions. decomposition, exchange (reactant losing electrons is the electron donor and is called oxidized) and synthesis (reactant taking on the electron is the electron acceptor and is called reduced.) |
|
|
Term
|
Definition
| reactions that release energy. Catabolic and oxidative reactions |
|
|
Term
|
Definition
| reactions that absorb energy. anabolic reactions |
|
|
Term
| factors that influence the rate of chemical reactions |
|
Definition
| temp - increased temp increases the rate of reaction, concentration - increased concentration increases the rate of the reaction, particle size - smaller particles make fast reactions, large make slower |
|
|
Term
|
Definition
| are substances that increase the rate of chemical reactions but themselves are not changed. example, enzymes |
|
|
Term
|
Definition
| the study of chemical composition and reactions of living matter |
|
|
Term
|
Definition
| always contain carbon. Carbon is ALWAYS covalently bonded. |
|
|
Term
|
Definition
| all other compounds that are not organic. ex. salts, water, acids, bases |
|
|
Term
|
Definition
| when bonds are broken, water is added |
|
|
Term
|
Definition
| when bonds are formed, a water is removed |
|
|
Term
|
Definition
| a substance that, when dissolved in water, dissociates into ions other than H+ or OH-. |
|
|
Term
|
Definition
| Universal Solvent - is polar and will attract and surround solute particles. causes ionic compounds, acids, and bases to dissociate. high heat capacity, high heat of vaporization, important reactant in chemical reactions. cushioning - cushions around organs, CSF surrounds the brain and spinal cord |
|
|
Term
|
Definition
| a substance that releases hydrogen ions (H+) when added to water |
|
|
Term
|
Definition
| substance that released hydroxyl ions (OH-) in solution, or one that accepts H+ already present in solution, when added to water |
|
|
Term
|
Definition
| parts hydrogen. measure of the relative acidity or alkalinity of a solution. going down the scale is more acid and going up is more basic |
|
|
Term
| what is the pH range of human blood |
|
Definition
| 7.35-7.45 - this is managed by buffer systems |
|
|
Term
|
Definition
| when acids and bases are combined - it results in water and salt. |
|
|
Term
|
Definition
chemicals that act to resist pH changes.
neutralize small amounts of acids or bases in body fluids |
|
|
Term
| 3 most important buffer system in body fluids are |
|
Definition
| bicarbonate, the phosphate, and the protein buffer system |
|
|
Term
| how many bonds can carbon make? |
|
Definition
| up to 4. Single, double, triple, and quadruple bonds with other carbon atoms. |
|
|
Term
| four organic compounds unique to living system |
|
Definition
| carbohydrates, lipids, proteins, nucleic acids. Organic molecules are large molecules that are made up of functional groups. Reactions occur withing those functional groups. |
|
|
Term
|
Definition
| subunits of organic compounds |
|
|
Term
|
Definition
| chain of monomers that make up organic compounds |
|
|
Term
|
Definition
| Carbon, Hydrogen, oxygen - with twice as many hydrogen as oxygen atoms. provide energy cell requires. include sugars and starches. provide body with ready, easily used of cellular fuel. Used to make ATP (energy molecule) |
|
|
Term
| carbohydrate simple molecular formula |
|
Definition
|
|
Term
|
Definition
| simple sugars, these are the monomers of carbohydrates. single unit molecules like: fructose, galactose, and glucose. |
|
|
Term
|
Definition
| polymers of simple sugars - joined by dehydration synthesis. important in: strange of energy as glycogen, fuel for cells, ATP DNA and RNA, glycolipids and glycoprotiens |
|
|
Term
| characteristics of Lipids |
|
Definition
| insoluble in water, soluble in other organic solvents like alcohol, include phospholipids, cholesterol, fats, steroids, waxes. contain C, H, and O but with proportionately less oxygen than in carbs. |
|
|
Term
|
Definition
| triglycerides, phospholipids, steroids |
|
|
Term
|
Definition
3 fatty acid chains bond to glycerol
fats when solid, oil when liquid
nonpolar, so they do not react with water
and provide the body's most efficient form of stored energy. fat offers insulation and protection for organs. |
|
|
Term
|
Definition
| no double bonds, found in tropical oils and animal fats, all carbons are "saturated" with hydrogens, solid at room temp |
|
|
Term
|
Definition
| vary number of double bonds, common in plants, all carbons are not fully bonded with hydrogens, chains are bent at double bonds, liquid at room temp |
|
|
Term
|
Definition
| diglycerides with a phosphorous-containing group and 2 fatty acid chains. this is the main component of the cell membrane. |
|
|
Term
|
Definition
another type of lipid
cholesterol is the base steroid
needed for cell membrane, synthesis of vitamin D, steroid hormones, and bile salts |
|
|
Term
|
Definition
| the basic structural material in the body. |
|
|
Term
|
Definition
| building blocks of protiens. |
|
|
Term
| characteristics of proteins |
|
Definition
| are structural materials, can function as enzymes. Contain C, H, O, and N and sometimes S. amino acids are building blocks of protein. two amino acids combine to form a peptid bond |
|
|
Term
|
Definition
|
|
Term
| primary protein structure |
|
Definition
|
|
Term
| secondary protein structure |
|
Definition
|
|
Term
| tertiary protein structure |
|
Definition
|
|
Term
| quarternary protein structure |
|
Definition
|
|
Term
|
Definition
|
|
Term
|
Definition
|
|
Term
|
Definition
| the substance on which an enzyme acts |
|
|
Term
|
Definition
| every reaction has an activation energy to make it go. Enzymes decrease the amount of activation energy needed. |
|
|
Term
|
Definition
| # of protons plus # of neutrons |
|
|
Term
|
Definition
|
|
Term
|
Definition
| fog, sprays, smoke, dust, emulsions |
|
|
Term
|
Definition
| sand and water, vinegar and oil, |
|
|
Term
| Most important catalyst in the human body |
|
Definition
| enzymes, they work by lowering the level of energy that needs to be invested in a chemical reaction |
|
|
Term
|
Definition
| when salt (NaCl) dissociates into water it turns into Na+ cations and Cl- anions and are surrounded by water molecules. these ions are called electrolytes, they are capable of conducting an electrical current. This property is critical to the function of ions in transmitting nerve impulses and prompting muscle contraction |
|
|
Term
| functional groups of carbon |
|
Definition
| Hydroxyl (-OH), carboxyl (-COOH), amino (-NH2), methyl (-CH3), and phospate (-P042) |
|
|
Term
|
Definition
| double sugar. 2 monosaccharides joined by dehydration synthesis. 2 unit molecules covalently bonded are: sucrose, and lactose |
|
|
