Term
| What are the levels of life, smallest to largest? |
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Definition
| Atom, molecule, cell, tissue, organ, organ system, multi-cellular organism, species, population, community, ecosystem, biosphere |
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Term
| What is the smallest particle of life? |
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Definition
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Term
| What does a molecule consist of? |
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Definition
An assembly of atoms
Like two hydrogen atoms plus one is a water molecule |
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Term
| What is the smallest unit of life? |
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Definition
| Cell. Living organisms can be unicellular or multi-cellular |
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Term
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Definition
Only found in multi-cellular organisms
Composed of similar cells that perform a similar function
Ex: muscle tissue=combination of muscle cells |
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Term
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Definition
ructure made up of several tissues that function as a unit
Ex: Heart, lungs, brain |
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Term
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Definition
2 or more organs, working together to execute a specific bodily function
Ex: Heat makes up part of circulatory system
Lungs make up part of respiratory system |
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Term
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Definition
Similar, potentially interbreeding organisms
Ex: Human, Bengal tiger, Antelope |
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Term
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Definition
Members of one species inhabiting the same area
Ex: Antelope herd |
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Term
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Definition
2 or more populations of different species of living organisms interacting within same area
Ex: Antelope, hawks, snakes & grass on a prairie |
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Term
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Definition
A community and its non-living environment
Antelope, hawks, snakes, grass, rocks, stream |
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Term
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Definition
Multiple ecosystems combined
Ex: Entire Earth surface |
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Term
| Which level of life does a scientist study? |
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Definition
| Depends on the question they ask |
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Term
| Principle of natural causality |
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Definition
All events can be traced to natural causes
Ex: Lightning is an electrical discharge |
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Term
| Principle of common perception |
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Definition
Assumption: all humans perceive natural events in similar ways
Common perceptions allow us to accept other humans’ observations .
Ex: An apple falls from a tree. We all see it fall to the ground & no one perceives it as floating up into the air |
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Term
| Principle of uniformity in space & time |
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Definition
| Natural laws apply to every time & place |
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Term
| What are the 5-6 steps of the scientific process, in order? |
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Definition
| Observation, Questions, Hypothesis, Experiment, Results, Conclusion |
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Term
| What is the difference between a theory and a hypothesis? |
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Definition
| A hypothesis is more of an educated guess, but a theory is an accepted explanation with a lot of data to back it up |
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Term
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Definition
| Process of creating a generalization theory based on many observations & results that support it |
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Term
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Definition
| Process of generating hypothesis about the outcome of an experiment based on a well-supported generalization (or theory) |
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Term
| What are the characteristics of life? |
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Definition
| Composed of cells, Acquire & utilize materials & energy from environment, Grow Reproduce, Undergo homeostasis, Respond to stimuli, Evolve |
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Term
| Where does energy ultimately come from? |
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Definition
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Term
| What are the 3 criterion of domains? |
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Definition
Cell type (prokaryotic or eukaryotic) cell number (unicellular or multicellular)
energy acquisition (autotroph or heterotroph) |
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Term
| Prokaryotic vs. Eukaryotic cells |
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Definition
Pro:
Do not have a nucleus
Genetic material is free in cytoplasm
Small in size
Lack membrane bound organelles
Bacteria & Arachnea domains
Eukaryotic:
Possess a membrane
Larger in size
Contain a variety of organelles
Eukarya domain |
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Term
| What are the four most common elements in the human body? |
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Definition
| Oxygen,Carbon, Hydrogen, Nitrogen |
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Term
| What are the three sub-atomic particles, and what are their charges? |
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Definition
| Protons (positive), Neutrons (neutral), Electrons (negative) |
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Term
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Definition
| # of protons (+) = # of electrons (-) |
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Term
| True or False: Hydrogen has neutrons |
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Definition
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Term
| How is the periodic table organized? |
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Definition
| By atomic number and chemical property |
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Term
| Where is the atomic number, atomic mass, and chemical symbol on an element on the periodic table? |
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Definition
| Top Left, Top Right, Big letter(s) in the middle |
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Term
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Definition
Atoms of same element that vary in # of neutrons
Most are stable
Some are radioactive
Spontaneously break apart
Release energy |
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Term
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Definition
| Electrons want their valence shell filled with 8 electrons. If not filled, they are reactive and unstable. If filled, they are inert and stable. |
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Term
| What two elements are exceptions to the Octet Rule? |
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Definition
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Term
| What part of the atom provides stability? |
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Definition
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Term
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Definition
| Form of attraction between atoms, holds them together to make molecules |
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Term
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Definition
Molecules in which atoms have one or more unpaired electrons in valence shell
Highly unstable
Achieve stability by capturing or releasing electrons from nearby molecules |
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Term
| Why do free radicals form? |
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Definition
Radiation, chemicals, heavy metals
Normal cellular processes |
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Term
| What is a chemical reaction? |
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Definition
process by which new chemical bonds form or existing bonds break
Forms a new substance |
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Term
| What are the 3 types of chemical bonds? |
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Definition
| Ionic, Covalent, and Hydrogen |
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Term
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Definition
atoms that have lost or gained electrons & now carry a positive or negative charge
Negative Ions = atoms that Gain electrons
Positive Ions = atoms that lose electrons |
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Term
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Definition
| Electrical attraction between oppositely charged ions |
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Term
| What are covalent bonds? Name the two types of them. |
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Definition
Bonds between uncharged atoms that share electrons
Polar, and non-polar |
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Term
| Difference between polar and non polar covalent bonds? |
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Definition
Nonpolar covalent bonds = atoms share electrons equally
Molecule is uncharged and so are its poles (opposite ends)
Ex: 2 hydrogen atoms share electrons equally & form H2
Polar covalent bonds = shared electrons spend more time with one atom than the other
Molecule is uncharged , but its poles are charged
Atom that has electrons more slight negative charge
Atom that has electrons less slight positive charge
Ex: Water (H2O)
Electrons shared between each H atom & central O atom
Electrons spend more time near the O atom
Oxygen pole slightly negative & Hydrogen poles slightly positive |
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Term
| What kind of bond do most biological molecules use? |
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Definition
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Term
| What kind of bond does not involve electron sharing? |
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Definition
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Term
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Definition
Attractive forces between slightly positive hydrogen in one polar molecule & slightly negative pole of a neighboring molecule
Polar molecules form when hydrogen atoms bond with nitrogen, oxygen & fluorine atoms
Hydrogen bonds form between individual polar molecules or within polar regions of same large molecule |
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Term
| What makes up 60-90% of most organisms' body weight? |
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Definition
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Term
| Cohesion of water molecules creates ______; Adhesion is _________ |
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Definition
| Surface tension; tendency of water to stick to surfaces |
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Term
| Why does water serve as an excellent solvent? |
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Definition
| Water’s polar nature attracts it to other polar molecules & ions. |
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Term
| What is the difference between a solvent and a solution? |
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Definition
Solvent = substance that dissolves other substances
Solution = solvent containing one or more dissolved substances |
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Term
| Difference between hydrophilic and hydrophobic molecules |
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Definition
Hydrophilic molecules are "water loving" and dissolve readily in water. Ex: Salt
Hydrophonic molecules are "water fearing" and do not dissolve. Ex: Oil |
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Term
| Small non-polar molecules |
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Definition
Still “dissolve” in water, but in a different way
Small size allows them to fit into spaces between water molecules
Don’t disrupt hydrogen bonds between water molecules |
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Term
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Definition
When H+ ions outnumber OH- ions
Acid = substance that releases hydrogen ions when dissolved in water |
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Term
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Definition
When OH- ions outnumber H+ ions
Base = substance that combines with free H+ ions in water thereby reducing number of H+ ions |
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Term
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Definition
When H+ ions equals the OH- ions
Ex: Water |
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Term
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Definition
| Each unit = tenfold change in H+ concentration |
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Term
| True or false: Neutral pH levels are essential to maintaining life |
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Definition
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Term
| What is a buffer/ buffer solution? |
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Definition
Buffer maintains a relatively constant pH in a solution
Responds to changes in H+ ion concentration
If H+ concentration rises, buffer accepts H+ ions
If H+ concentrations falls, buffer releases H+ ions
Common buffers in biological organisms
Bicarbonate (HCO3-)
Phosphates (H2PO4- and HPO42-) |
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Term
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Definition
| Energy required to heat 1 gram of substance by 1º C |
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Term
| True or False: It takes a lot of energy to heat up water? |
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Definition
| True, most of the energy is used to break up hydrogen bonds instead of actually raising the temperature |
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Term
| What is the specific heat of water? |
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Definition
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Term
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Definition
| Amount of heat needed to cause substance to evaporate |
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Term
| True or false: Ice is less dense than liquid water? |
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Definition
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Term
| Difference between Organic and Inorganic Molecules? |
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Definition
Organic Molecules = biological molecules
Building blocks for cells
Can be synthesized & used by living organisms
Most are large and complex
Contain carbon (C) backbone bonded to hydrogens (H)
Inorganic Molecules
Simpler molecules
All molecules without carbon
Ex: water (H2O), salt (NaCl)
Carbon dioxide (CO2) No hydrogen! |
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Term
| What is the most important element in organic materials? |
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Definition
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Term
| What are functional groups? |
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Definition
Groups of atoms attached to carbon backbone
Determine:
Physical characteristics of molecule
Chemical reactivity of molecule
Less stable than carbon backbone
More likely to participate in chemical reactions |
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Term
| What is the difference between monomers and polymers? |
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Definition
Monomers = small molecules which are subunits of larger molecules
Polymers = molecules made up of chains of monomers
Larger & more complex |
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Term
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Definition
Polymer is split into monomers using water
Water donates:
Hydrogen ion (H+) to one monomer
Hydroxide ion (OH-) to other monomer |
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Term
| What are the two steps of synthesis of organic molecules? |
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Definition
Atoms are joined to form monomers
Occurs if preassembled monomers not present
2) Monomers are joined in chains to form polymers
Dehydration synthesis = chemical reaction that joins monomers by removing water |
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Term
| What are the 4 categories of biological molecules? |
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Definition
| Carbohydrates, Proteins, Lipids, and Nucleotides/Nucleic Acids |
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Term
| What are the four functions of carbohydrates |
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Definition
Energy source & energy storage
Structural support in cell walls & cell membranes
Form protective body “armor” of insects, crustaceans, etc.
Component of RNA & DNA |
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Term
| What are the 3 groups of carbohydrates? |
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Definition
Monosaccharides
Backbone of 3-7 carbon atoms
Ex: Glucose
Disaccharides
2 monosaccharides linked together
Ex: Sucrose
Polysaccharides
Polymer of many monosaccharides
Ex: Starch |
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Term
| What are monosaccharides, and what are the 5 most common? |
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Definition
Glucose (C6H12O6 )
Energy storage
Fructose (C6H12O6)
Energy storage
Galactose (C6H12O6)
Energy storage
5 – Carbon sugars
Ribose (C5H10O5)
Found in RNA
Deoxyribose (C5H10O4)
Found in DNA |
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Term
| What are disaccharides? List some common ones |
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Definition
2 monosaccharides linked together
Sucrose, Lactose, Maltose |
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Term
| What are polysaccharides? List 4 common types |
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Definition
Polymer of single type of monosaccharides
Chitin, Starch, Glycogen, Cellulose |
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Term
| Where is starch found? Glycogen? |
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Definition
| Seeds & roots of plants; Liver and muscle tissues |
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Term
| What are the 3 groups of lipids? |
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Definition
Fats, oils, & waxes
Energy storage & waterproofing
Phospholipids
Component of cell membranes
Steroids
Component of cell membranes
Hormones (regulate various processes in body) |
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Term
| What are the 6 main functions of proteins? |
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Definition
Enzymes (e.g. lipase, amylase)
Promote chemical reactions
Structural protein (e.g. keratin)
Found in: skin, tendons, muscles, nerves, hair, spider webs, etc.
Hormones(e.g. insulin)
Influence cell activity
Movement (e.g. actin & myosin, hemoglobin)
Involved in contractions of muscles & movement of other molecules
Immune defense (e.g. Antibodies!)
Aid in fighting off diseases
Toxins (e.g. snake venom) |
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Term
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Definition
| Polymers with 1 or more chains of amino acids joined by peptide bonds |
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Term
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Definition
Bonds that join amino acids
Formed by dehydration synthesis |
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