Term
|
Definition
| things all living things share |
|
|
Term
|
Definition
.1. cell is basic unit
.2. living organisms interact with their environments
.3. have energy requirements
.4. structure correlates to function
.5. able to externally and internally regulate themselves
.6. stimulus-response
.7. reproduction |
|
|
Term
| what is the basic structural and functional unit of life? |
|
Definition
|
|
Term
| ex: unicellular and multicellular organisms |
|
Definition
unicellular: bacteria
multicellular: humans |
|
|
Term
| what are the two cells that combine to form a zygote? |
|
Definition
|
|
Term
| how do humans begin as unicellular? |
|
Definition
| begin as union of sperm and egg into a zygote -- a unicellular organism |
|
|
Term
|
Definition
| spermatid and oocyte become a zygote |
|
|
Term
| obligate intracellular parasites |
|
Definition
|
|
Term
|
Definition
| the cell a virus takes over and uses its "machinery" to reproduce itself |
|
|
Term
| why do viruses need a host cell? |
|
Definition
| have no cellular structure of their own |
|
|
Term
| how do viruses function as if they have cellular structure? |
|
Definition
|
|
Term
| what are some ways a living organism interacts with its environment? |
|
Definition
| benefit from, contribute to, damage, are harmed by, etc. |
|
|
Term
| do living organisms interact with the living or the nonliving aspects of their environments? |
|
Definition
| both living and nonliving |
|
|
Term
| because no living organism can generate its own energy, how do they acquire it? |
|
Definition
| from interacting with their environments |
|
|
Term
| what are the two things a living organism must do to acquire energy from its environment? |
|
Definition
| TRANSFER energy (from the source) and TRANSFORM energy (into something it can use) |
|
|
Term
| what is an example of transfer and transformation of energy? |
|
Definition
| a plant transfers solar energy from the sun and transforms it into chemical energy |
|
|
Term
|
Definition
| processing one form of energy into another form for an organism's requirements |
|
|
Term
|
Definition
| the capacity to perform work |
|
|
Term
|
Definition
| when one must oppose some sort of force (and expend energy) |
|
|
Term
| structure of a living organism correlates to ___________ |
|
Definition
|
|
Term
| how can you extrapolate the basic function of an organism? |
|
Definition
|
|
Term
| how could you tell apart a skin cell from a lung cell based on their cell membranes, and what is this an example of? |
|
Definition
| the cell membrane designed to keep things out (skin) would be thicker, while the one designed to let air through (lung) would be thinner -- structure correlates to function |
|
|
Term
|
Definition
| pupil adjusts in size to take in the correct amount of light |
|
|
Term
|
Definition
| pancreas releases insulin to promote glucose entry into cells / glucose storage as glucose level rises |
|
|
Term
| what is the primary organ for glucose storage? |
|
Definition
|
|
Term
| what stimulates the liver to store glucose? |
|
Definition
|
|
Term
|
Definition
| the efforts of the body to maintain a constant internal environment |
|
|
Term
| what is the definition of the word "constant" relating to the body trying to maintain a constant internal environment? |
|
Definition
|
|
Term
| when the body receives information about a process that is over or under what is needed, and then responds by negating it, what is this called? |
|
Definition
|
|
Term
| what is a method of homeostasis? |
|
Definition
|
|
Term
| kinds of reproduction (3) and examples |
|
Definition
| whole organism reproduction (humans, bacteria); growth/development (cell division in reproduction - the zygote); tissue repair (skin) |
|
|
Term
|
Definition
| parent cell divides into two genetically identical daughter cells, not remaining as an individual |
|
|
Term
|
Definition
| male-female union results in offspring, whose genetic material is partially contributed to by mother and partly by father, who continue to live on independantly |
|
|
Term
| what prevents cells with a reproduce and replace brand of tissue repair going on from overgrowth? |
|
Definition
|
|
Term
| what are two examples of regeneration reproduction? |
|
Definition
- skin cells regularly shedding layers
- menstrual cycle (uterine lining sheds) |
|
|
Term
| what is the difference in regeneration between skin cells and liver cells? |
|
Definition
| liver, like other organs (but especially liver) has capacity to regenerate but won't unless it's actively damaged; skin regenerates as a matter of course |
|
|
Term
| what form of reproduction allows for partial organ donation? |
|
Definition
|
|
Term
| capacity for regeneration: nerve cells |
|
Definition
| very little capacity, especially after death |
|
|
Term
| explain why it is currently impossible to cure alzheimer's disease |
|
Definition
| because it kills nerve cells, which have very little capacity for regeneration |
|
|
Term
| what are the two classifications of living organisms? |
|
Definition
| PROTCARYOTES and EUCTARYOTES |
|
|
Term
| examples of prokaryotes (2) |
|
Definition
|
|
Term
|
Definition
animals
insects
plants
fungi |
|
|
Term
| what is the difference between protcaryotes and eutcaryotes? |
|
Definition
protcaryotes: organelles lack membranes - freely distributed throughout the cell
eutcaryotes: organelles HAVE membranes |
|
|
Term
| describe negative feedback as a case of stimulus-response |
|
Definition
| body detects something off-balance - this is the stimulus - and then RESPONDS by giving the negative feedback and negating it. |
|
|
Term
|
Definition
| body detects something positive happening in the body and sends signals to promote that activity |
|
|
Term
| what is the difference in cellular structure between eucaryotes and procaryotes? |
|
Definition
| in procaryotes the organelles lack membranes; they're freely distributed, unlike in eucaryotes |
|
|
Term
| four steps of the scientific method |
|
Definition
1. observation
2. hypothesis
3. experiment
4. conclusion |
|
|
Term
|
Definition
| don't tell the participants which group they're in (control/experimental) |
|
|
Term
| what are the two groups in a study? |
|
Definition
|
|
Term
| what is the aim of blinding a study? |
|
Definition
| trying to keep the only influence on the subjects the drug itself |
|
|
Term
|
Definition
| goes from specific observations to a general hypothesis |
|
|
Term
| if you observe the blood pressure of a lab rat going down with a certain medication, what would you reason INDUCTIVELY? |
|
Definition
| that this drug must make blood pressure go down (specific --> general) |
|
|
Term
|
Definition
| goes from a general hypothesis to specific applications |
|
|
Term
| if you had a general hypothesis that a given drug lowered blood pressure, what would be the DEDUCTIVE response? |
|
Definition
| that this drug could be usable in humans (general to specific applications) |
|
|
Term
| elements are ________ occuring substances that can sometimes be ______________ |
|
Definition
| elements are NATURALLY occuring substances that can sometimes be SYNTHESIZED in a lab |
|
|
Term
| a hypothesis must be TESTABLE and ________ |
|
Definition
| a hypothesis must be TESTABLE and FALSIFIABLE |
|
|
Term
|
Definition
| there is some way to reveal the hypothesis is NOT true |
|
|
Term
| scientific method (4 steps) |
|
Definition
1. observation
2. hypothesis
3. experiment
4. conclusion |
|
|
Term
| which four elements make up 96% of living matter? |
|
Definition
| Oxygen, Carbon, Nitrogen, Hydrogen |
|
|
Term
| what is the most concentrated use of Iodine in the body? |
|
Definition
|
|
Term
| what is the result of an iodine deficiency? |
|
Definition
| the thyroid gland swells (goiter) |
|
|
Term
|
Definition
| smallest unit of matter that retains the properties of an element |
|
|
Term
| what particles are smaller than atoms? |
|
Definition
|
|
Term
| without information to the contrary, we assume an atom is electrically _____________ |
|
Definition
| neural! (meaning all the charges are balanced) |
|
|
Term
|
Definition
| the capacity to cause change (like by doing work) |
|
|
Term
|
Definition
| energy posessed because of position (like water on a hilltop) |
|
|
Term
| which has greater potential energy - the electron in an inner shell or an outer shell of an atom? why? |
|
Definition
| the outermost atom has the MOST potential energy --> because it seeks to run "downhill" towards the nucleus, which it's attracted to |
|
|
Term
| how does an electron change into an outer shell? |
|
Definition
|
|
Term
| which electrons participate in chemical bonding? |
|
Definition
|
|
Term
| what determines the bonding qualities of an atom? |
|
Definition
|
|
Term
|
Definition
| every atom tries to have a filled outermost shell (8 valence electrons) |
|
|
Term
| what is a common source of iodine? |
|
Definition
|
|
Term
|
Definition
| specialized tissue structures that secrete hormone molecules into the blood |
|
|
Term
|
Definition
| molecules secreted by endocrine glands |
|
|
Term
| what element is necessary for the production of thyroid hormone? |
|
Definition
|
|
Term
| how would one visualize the structure and function of the thyroid? |
|
Definition
| inject iodine 131 (a radioactive isotope of iodine) into the blood. it decays and releases radioactive particles, which can be traced on camera and shows the shape of the thyroid (when the iodine 131 gets there) - or if it doesn't get to the thyroid, you can tell that something's wrong. |
|
|
Term
| what is an isotopal tracer? |
|
Definition
| a radioactive isotope injected into the body so you can trace the path of the radioactive energy |
|
|
Term
|
Definition
| an atom that has a net charge (has lost or gained electrons) |
|
|
Term
| how does the body take advantage of the fact that ionic bonds are relatively weak? |
|
Definition
| breaks / dissolves the bonds to get needed electrolytes |
|
|
Term
| bonding capacity of an atom |
|
Definition
| how many unpaired valence electrons it has - i.e. how many covalent bonds it can form |
|
|
Term
| why do two oxygen atoms form a covalent double bond? |
|
Definition
a) they both have nucleus of equal mass, so neither attracts the other more
b) both have 6 valence electrons - need two more - so share |
|
|
Term
| Why does H2O form a covalent polar bond? |
|
Definition
| O has greater electronegativity than H, so the shared electrons orbit more around O |
|
|
Term
|
Definition
| a measure of how strongly an atom attracts electrons while bonding - determined by the number of protons (mass) |
|
|
Term
| what sort of covalent bond is formed when the electronegativity of the atoms is equal? |
|
Definition
|
|
Term
| what sort of covalent bond is formed when the electronegativity of the participating atoms is UNequal? |
|
Definition
|
|
Term
| what does it mean when a covalent bond is "more polar" or "less polar"? |
|
Definition
| a more polar bond is when one participating atom has much greater electronegativity than the other. a less polar bond is when they both has similar electronegativities |
|
|
Term
| why are the H atoms in an H2O molecule partially positively charged (δ+), and the O atom partially negatively charged? (δ-) |
|
Definition
| because an H2O bond is so polar, the electrons spend much more time orbiting the O atom than the H atoms. However, they still spend SOME time orbiting the H atoms, so the H atoms only have a positive charge *most* of the time, and the O has a negative charge *most* of the time. |
|
|
Term
| what is another word for an ionic compound? |
|
Definition
|
|
Term
|
Definition
| an atom that has a net charge (has lost or gained an electron) |
|
|
Term
| what effect does electronegativity have on bonding? |
|
Definition
| a more strongly electronegative atom will be less likely to lose electrons and more likely to gain them |
|
|
Term
| in an ionic molecule, what is the charge of the molecule? what is the charge of the ions? |
|
Definition
| the molecule itself is neutral; but the ions are still individually charged. |
|
|
Term
|
Definition
| because a covalently bonded hydrogen is partially positively charged (δ+), it can be WEAKLY attracted to a DIFFERENT electronegative atom nearby. |
|
|
Term
| what is the most common form of hydrogen bonding? |
|
Definition
| hydrogen with nitrogen or oxygen |
|
|
Term
| which kind of bond is an INTERmolecular bond, and why? |
|
Definition
| hydrogen bonding -- the H ALREADY IN a polar covalent bond is attracted to a DIFFERENT electronegative atom |
|
|
Term
| in a hydrogen bond, what is ALWAYS the partially positively charged atom? |
|
Definition
| hydrogen (hence the name) |
|
|
Term
|
Definition
| WEAK bonding between two NONPOLAR molecules; even though they are nonpolar and don't have a permanant partial charge, the electrons move around, so for a short time they can be oppositely charged and attract one another. |
|
|
Term
| what is the nature of hydrogen bonding in liquid water? |
|
Definition
| weak hydrogen bonds constantly form and break; therefore, at any instance, a large percentage of molecules are bonded to their neighbors |
|
|
Term
| water is adhesive and cohesive; what do these two terms mean? |
|
Definition
adhesive: sticks to other things
cohesive: sticks to itself |
|
|
Term
|
Definition
| the force required to break the surface of a substance |
|
|
Term
| what property of water helps preserve homeostasis in the body? |
|
Definition
| the fact that it absorbs heat and withstands temperature change with such a great capacity -- we are made up of so much water, this is very important! |
|
|
Term
|
Definition
| because it has high polarity molecules so is constantly forming hydrogen bonds -- it sticks to itself |
|
|
Term
| why does water have such high surface tension? |
|
Definition
| because it's very cohesive (because it has lots of hydrogen bonds) |
|
|
Term
|
Definition
| because it forms hydrogen bonds with OTHER substances, making it stick to them (as well as with itself - cohesion) |
|
|
Term
| what determines kinetic energy? |
|
Definition
|
|
Term
| heat is a measure of what? |
|
Definition
|
|
Term
| with what do you measure kinetic energy? |
|
Definition
|
|
Term
|
Definition
| the amount of heat that must be absorbed or lost for 1g to change by 1 degree C |
|
|
Term
| why will you burn yourself on an iron pot while the water it contains is still lukewarm? |
|
Definition
| iron has a lower specific heat than water; i.e. it takes less energy to get it to change temperature |
|
|
Term
| what does it mean that water has a high specific heat? |
|
Definition
| it takes a lot of energy to get water to increase temperature a little |
|
|
Term
| when exposed to the same amount of heat as another substance with a lower specific heat, what happens to water? |
|
Definition
| water will change temperature less while absorbing the same amount of heat. |
|
|
Term
| what is the reason for water's high specific heat? |
|
Definition
| to break a hydrogen bond you need heat; water has so many hydrogen bonds, a relatively large amount of heat goes into breaking the bonds before the water molecules can move faster (increase in temperature) |
|
|
Term
| why does water release so much heat with a slight drop in temperature? |
|
Definition
| a lot of hydrogen bonds begin forming at once, the process of which releases heat |
|
|
Term
| why does a heated liquid become a gas? |
|
Definition
| heat increases temperature, which causes the molecules of a substance to move faster. When the molecules move fast enough, they overcome their attraction to one another and float off into the air as a gas. |
|
|
Term
|
Definition
| AVERAGE kinetic energy of molecules |
|
|
Term
|
Definition
| the amount of heat a liquid needs to absorb to convert 1g of it into a gas |
|
|
Term
| how does sweating regulate body temperature? |
|
Definition
| the water in our bodies must absorb a LOT of heat before the temperature rises. when the temperature DOES rise enough to evaporate from our bodies (sweat), it carries a lot of heat away with it! |
|
|
Term
| which is the least dense phase of a substance, and why? |
|
Definition
| gas -- because the molecules are further away from each other than in other forms. when you cool the gas, the molecules lose energy and move closer together |
|
|
Term
| most substances are more dense as a solid than as a liquid. what is the exception? |
|
Definition
|
|
Term
| why is ice less dense than liquid water? |
|
Definition
| normally, molecules of a substance get closer and closer together as they lose energy and freeze. but water will form more and more hydrogen bonds that actually keep the individual molecules AWAY from each other, making it less dense than liquid water, where the molecules don't always bond and can be closer together. |
|
|
Term
|
Definition
| a substance that donate an extra H+ ion to a solution -- increases the hydrogen ion concentration of that solution |
|
|
Term
| if you add a substance and suddenly there are more hydrogen ions, what did you add? |
|
Definition
|
|
Term
|
Definition
| the amount of a particular substance in a given volume |
|
|
Term
|
Definition
| a substance that ACCEPTS H+ ions within a solution |
|
|
Term
| what is a basic solution? |
|
Definition
| a solution with a higher concentration of OH- than H+ |
|
|
Term
| the higher the H+ solution, the _______________ the pH |
|
Definition
| the higher the H+ solution, the LOWER the pH |
|
|
Term
| pH + pOH of a solution is always equal to: |
|
Definition
|
|
Term
| what do brackets [ ] indicate in a pH equation? |
|
Definition
|
|
