BIOL 1001 / 1001H Exam 1

Based off of chapters 1-3 in textbook and lectures. This is VERY thorough. If you only want to study some, star the ones you want and use features based on starred cards only.

Qualitative data

Descriptions, not a numerical value

Quantitative

Measurements, always a numerical value

Hypothesis

A specific proposition, makes predictions, is testable (and if wrong, falsifiable), and never truly proven

Theory

Backed by large amounts of evidence, broad explanation that gives ability to make predictions, never truly proven

Scientific Method

Observation, question, hypothesis, experiment, analysis, conclusion

Control groups

Controlled, not subjected to specific variable(s)

Experimental groups

Same as a control group, except for one variable, to see its effect. Should be able to replicate effect

Independent varibale

What’s being changed, seeing how it changes dependent variable

Dependent variable

What (should) be affected by independent variable

Population vs Sample

Population whole set of item of interest, sample is a portion of population

Null hypothesis

Proposes no statistical significance among observations

Alternative hypothesis

Proposes there is a statistical significance among observations

Standard deviations

Distribution of values from the average

Student T-Test

How true calculated mean and standard deviation from the experiment is to the population, based on mean, standard deviation, and the number in sample. Gives p-value, when less than .05, considered significant

Science

Observation, identification, experimental investigation, and theoretical explanation of natural phenomena

Model organisms

Organisms studied by many researchers who compare results and determine scientific principles that apply more broadly to other species

Ecology

Study of organisms in their natural environments

Anatomy

Study of structures of animals and plants

Physiology

Study of functions of animals and plants

Cell biology

Study of cells and their interactions

Molecular biology

Study of individual molecules in living cells due to genetic tools

Reductionism

Based on reducing complex systems to simple components and observing from there

Systems biology

Research approach in 1990s, based on trying to understand how emergent properties arise, apart of investigations of groups that work with a common purpose

Discovery-Based Science

Collection and analysis of data without the need for a preconceived hypothesis, usually done with hope of gathering clue for a hypothesis

Matter

Anything that has mass and occupies space, all life forms composed as such

Atoms

Smallest functional units, forms all matter, chemical substances, and all organisms. Has protons, electrons, and neutrons, with no net charge

Molecules

Two or more atoms bonded together

Compounds

Two or more different elements

Element

Made up of one type of atom, can’t be broken down farther. Has unique number of protons (equal to its atomic number)

Orbital

Region of space surrounding atomic nucleus where electrons travel in. Either spherical (s) or propeller/dumbbell (p). S fills first, then p by equal distribution

Electron shells

Where orbitals are found, first shell has 1s for 2 electrons, second shell has 1s and 3p

Energy

Capacity to do work or cause change, electrons have kinetic energy allowing them to spin

Valance electrons

Outer shell electrons that can interact with others, more stable / energetic when shell is fuller

Electronegativity

Ability for an atom to attract electrons, <.4 difference is nonpolar, .4-1.8 is polar, 1.8< is ionic

Atomic mass

Atom’s mass based on relativity to masses of other atoms such as carbon with a mass of 12. Uses dalton (Da) as unit, 1 Da = 1/12 Carbon atom. Mole is any substance with same number of particles as in 12g of carbon

Elements of Life

Carbon, hydrogen, oxygen, and nitrogen (makes up ~95% of living organisms, with oxygen being ~65%)

Mineral elements

Makes up ~1% of living organisms, but still need significant amount to sustain life, ex calcium and phosphorus

Trace elements

Elements present in very small quantities in living organisms, but still needed for function / growth, ex iron and copper

Isotopes

Has different number of neutrons than other elements than its standard, atomic mass (protons + neutrons) is where variance is noticable

Molecular formula

Chemical symbols of present atom

Emergent properties

Properties of a compound, can differ from properties of element is made of, ex sodium is metal till interacts with chlorine, making salt

Covalent bond

Between atoms, sharing electrons to fill valence shells, polar or nonpolar. Single bonds weaker than double

Structural formula

Line between elements representing bond

Nonpolar covalent bonds

Atoms with similar electronegativities who bond (less than .4)

Polar covalent bonds

Bonded atoms with electronegative difference of .04-1.8, unequal pull of shared electrons (closer to higher electronegative atom)

Ionic bond

Between atoms, electric attraction. Cation (+) binds to anion (-), / cation loses electrons, anion gains. When electronegativity difference is >1.8

Hydrogen bond

Occurs when atoms already in covalent bond. Hydrogen atom in polar molecule is electrically attached to an electronegative atom in another polar molecule, or within a large molecule. Very weak on own, but strong with large numbers

Ion

Atom that’s no longer neutral due to losing an electron (anion, -) or gaining an electron (cation, +)

Free radicals

Molecule containing atom with single, unpaired electron in outer shell; can steal electrons from molecules

Antioxidants

Protective compounds that protect molecules from free radicals, donating electrons without becoming unstable / reactive

Chemical reaction

Occurs when open or more substances are changes into other substances by making/breaking bonds and/or the removal/addition of electrons. Needs source of energy, and sometimes a catalyst. Always will reach equilibrium

Brownian motion

Atoms/molecules needing energy (usually by heat) to vibrate and move and therefore encounter others to cause chemical reactions

Solutes

Substances dissolved in liquid (solvent)

Solvent

Liquid the solutes dissolves in

Solution

Formed by solutes dissolving in solvent, “aqueous solutions" are ones made with water

Bond between O and H

Covalent and polar, oxygen is more electronegative, so hydrogens have partial + charge and oxygen has partial - charge

Hydrophobic

Molecules with few/no charges and/or nonpolar, doesn’t dissolve in water

Hydrophilic

Molecules with certain ionic and/or polar covalent bonds, dissolves in water

Amphipathic

Molecules with both types of dissolvability, polar sides face outward due to attraction and nonpolar face inwards

Solute concentration

Amount of solute dissolved in unit volume of solution

Molecular mass

Sum or all atomic masses of an atom in molecule

Molarity

Uses molecular mass, defines number of molecules of solute dissolved in 1 L of solution

Properties of water

High specific heat allowing stability; hydrogen bonds break fast as gas, constant as water, low as solid. Solid least dense of 3,

Specific heat

Amount of heat needed to be absorbed/lost f 1 gram of a substance to change its temp by 1 C

Heat of Vaporization

Heat required to vaporize 1 mol of any substance at its boiling point

Heat of Fusion

Amount of heat needed to be withdrawn / released to make substance go from liquid to solid state

Heat capacity

Amount of heat required to raise the temperature of entire object / particular amount of substance, ex larger beaker of water takes longer than small, but works at same tempature

Colligative properties

Depends strictly on total number of dissolved solute particles, ex pure water freezes at 0C and vaporizes at 100C, added solute can add/raise the two respectively

Hydrolysis reactions

Water used as a reactant to break covalent bonds between other reactants. When ionized, water becomes H+ and OH-. Used to break down polymers

Evaporation

Water becomes vaporized at normal temperature due to high energy molecules that break and become gaseous

Cohesion

Molecules of same type attracting one another, in water it’s due to hydrogen bonding

Adhesion

Ability of different molecules to be attracting to one another, such as water being attracted to charged surfaces

Surface tension

Measure of attraction between molecules at surface of liquid, ex hydrogen bond force causes water in air to form droplets, when on surface already, this allows them to pool into “sphere”

pH

Scale used to describe concentration of H+ and OH-, higher pH, lower H+, calculated by negative log(base10) of H+ concentration. pH < 7 = acidic, pH = 7 neutral, pH > 7 = alkaline.

Acids

Substances that release hydrogen ions, increasing H+

Base

Substances that decrease H+ concentration

Buffer

Pair of substances like acid and its base to minimize pH fluctuations in fluids of living organisms, will release/absorb H+ when needed

Organic molecules

Molecules that contain carbon, found in all forms of life. Has 4 valance electrons; very stable, strong and bondable

Macromolecules

Large, complex organic molecules. Main types are proteins, lipids, carbohydrates, and nucleic acids

Organic chemistry

Science of carbon-containing molecules

Hydrocarbons

Molecules with only carbon and hydrogen molecules (usually nonpolar and hydrophobic)

Functional groups

Groups of atoms with characteristic chemical structures and properties, can replace one or more of hydrogens bonded to carbon skeleton of hydrocarbon

Isomers

Two or more molecules with same chemical formula but with different structures and characteristics, types are structural, stereo, cis-trans, and enantiomer

Structural isomer

Same atoms, different bonding relationships / placement

Stereoisomers

Same bonding, different spatial positions of atoms

Cis-isomer

Double bond on same side

Trans-isomer

Double bond on opposite sides

Enantiomers

Mirror image molecules (L/R flipped)

Monomer

One big molecules made by many small molecules

Polymer

One bigger molecule formed by many small molecules and monomers

Dehydration reaction

Water is lost in reaction

Carbohydrates

Long chains of sugars composed of carbon, hydrogen and oxygen (Cn(H2O)n

Monosaccharides

Carbohydrate / simple sugars monomers, linear or ring shaped, has either 5 or 6 carbons

Pentose

Monosaccharide with 5 carbons, ex ribose and deoxyribose

Hexoses

Monosaccharide with 6 carbons, ex glucose

Disaccharides

Carbohydrate of two monosaccharides, joined by glycosidic bond

Glycosidic bond

Linking inside disaccharides involving removal of hydroxyl group from one monosaccharide and hydrogen from the other, releasing a water molecule and bonding through an oxygen atom

Polysaccharides

Many monosaccharides linked to form long polymers, structure/function determined by sugar monomers and positions of glycosidic bonds. Includes starches, glycogen, and cellulose

Cellulose

Polymer of B-D glucose with linear arrangement and no branching, can form hydrogen bonds with each other to create parallel pattern to strengthen plant cell walls