All Bio 1001H vocab

Cellular organization

Cellular organization

all livings things are made from one or more cells

Ordered complexity

living systems are made more than the sum of their parts (all living things are complex and made up of many different things with different molecular structures)

Sensitivity and Responsivness

organisms respond to stimuli from their environment

Growth, development, and reproduction

all living things increase in size (or mass) and pass on characteristics (via DNA)

Homeostasis

all living things have mechanisms to maintain a steady, stable internal state

Evolutionary adaptation

Organisms change over time to become better suited to changing environments

Negative feedback

reduces the gap between the set point (homeostasis) and the environmental conditions

Development

the process an organisms undergoes to move from a simpler form to a more complex form (immature to mature state)

Growth

the process an organism undergoes to get bigger and to increase their number of cells over time (by dividing)

Deductive reasoning

hypothesis that starts with general observations to predict something specific

Inductive reasoning

hypothesis that starts with specific observations (or experimental findings) to make a general conclusion

Statistical Purpose

helps scientists understand their results and if there is a correlation between things/groups

Standard Deviation

the amount of variability in the data

Mode

the most frequently occurring data in a data set

p-value > 0.05

high probability that the samples are from the same population (accept null hypothesis and is likely not statistically significant)

P-value < 0.05

low probability that the samples are from the same population (rejects the null hypothesis and data is statistically significant) (likely that samples are from different populations)q

Nominal scales of neasurement

word or numbers that are used to classify, label, or categorize observations (Ex: color : blue, green, yellow…)

Ordinal scales of measurement

classifying the order of something (putting results in order/ ranking)

Interval/ratio scale of measurement

quantities (measurements) or differences (interval between measurements can be calculated) (Ex: ages of dogs: 1-3yrs, 4-5 yrs…)

Orbital

The region surrounding the nucleus of an atom where the probability is high of finding a particular electron (balloon of space where an electron is likely to be) can only contain 2 e- max

Energy

the capacity to do work or to cause a change

Isotopes

atoms that have the same amount of protons, but vary in the amount of neutrons

Radioisotopes

unstable isotopes (emit radiation as they decay)

Trace elements

elements in a living thing that are found in very small quantities (still important to the living things)

When are atoms most stable?

when their outer shells are fully or half filled with electrons

molecular formula

tells us the number of elements and what elements make up a molecule or compound

Covalent bonds

when atoms share a pair of electrons

Double bond

covalent bond where two pairs (4 total) of electrons are shared

Structural formula

when covalent bonds are shown with a line (usually lewis dot structures)

Electronegativity

an atom’s ability (measured) to attract electrons (to create a bond)

High electronegativity

attraction between elements is strong

low electronegativity

weak attraction to another atom’s electrons

Non-polar covalent bonds

when electronegativity differ by less than 0.4

Ionic bonds

when electronegativity differs by more than 1.8 (cation+anion)

polar covalent bonds

electrons shared unequally (when electronegativity differs by 0.4-1.8)

Cation

atom or molecule with a net positive charge

Anion

atom or molecule that has a net negative charge

van de waals dispersion forces

attractive forces between molecules in close proximity to each other (because of electron density)

Free radical

a molecule containing an atom with a singular, unpaired electron in the outer shell

Solutes

substances that are dissolved in a liquid

Solvents

the liquids that dissolve something

Hydrophilic

loves water (attracted to water) (tend to be polar molecules)

Hydrophobic

hates water (repelled by water) (tend to be non-polar molecules)

Amphipathic

molecules that both love an hate water (some regions polar, some regions non-polar)

Micelles

formed by amphipathic molecules (polar heads face towards water, non-polar tails face away from water) creates little bubble looking things

Solute concentration

the amount of a solute dissolved in a certain volume of a solution

Molarity (M)

how many moles of a substance are in 1L of a solution

Heat of vaporization

the heat required to vaporize 1 mol of any substance (boiling point)

heat of fusion

amount of heat/energy that is required to melt a solid substance into a liquid

Specific heat

the amount of heat/energy required to raise the temp of 1g of a substance by 1ºC

Heat capacity

the amount of heat required to raise the temp of an entire object/ a particular amount of a substance

Colligative properties

properties that depend strictly on the total number of dissolved solute particles

Hydrolysis reaction

reaction which breaks apart water (ex: H20 → H+ and OH-)

Cohesion

when molecules of the same type attract to each other (ex: h20 + h20 attraction)

Adhesion

ability of unlike particles to be attracted to each other (ex: h20 to glass attraction)

Surface tension

the attraction between molecule at the surface of a liquid

Acids

substances that release H+ ions (more H+ ions, lower pH)

Bases

substances that release OH- ions (increases OH- concentration → higher pH)

pH

a measure of H+ concentrations in a solution (pH=-log[H+])

Buffers

a pair of substances that minimize pH fluctuations (usually and acid and its related base)

Macromolecules

carbohydrates, proteins, lipids, and nucleic acids

organic molecules

molecules containing carbon

Inorganic molecules

molecules that are not found in living organisms

Hydrocarbons

molecules with a high proportion of hydrogen and carbon atoms bonded

Functional groups

groups of atoms with characteristic chemical structures and properties

Isomers

2 or more molecules with the same chemical formulas, but different structures

sterioisomers

identical building relationships, but spacial positioning of atoms differ

cis isomer

when the two hydrogen atoms are on the same side of the carbon double bonds

trans isomer

when the two hydrogen atoms are on different sides of the carbon double bonds

enantiomer

one pair of molecules that are mirror images of each other

Enzyme

molecules that catalyze rates of chemical reactions (lowers the activation energy of a reaction)

monomers

one part of a polymer

polymer

many monomers

Condensation/dehydration reaction

when 2 molecules combine to produce a larger molecule and RELEASES a water molecule

Hydrolysis reaction

when a polymer is broken down into monomers (requires water)

Carbohydrates

organic molecules made of C,H, and O atoms

monosaccharides

the monomer of carbohydrates (the simplest

Disaccharides

2 monosaccharides that are linked together by a dehydration reaction (glycosidic bond)

Glycosidic bond

bond formed between 2 sugars (dehydration reaction) (the bond that holds polysaccharides together)

polysaccharides

many monosaccharides linked together by glycosidic bonds (forms long polymers)

Cellulose

a polymer of monosaccharides with a linear arrangement of carbon-carbon bonds (NO branching)

Lipids

hydrophobic molecules composed of hydrogen and carbon atoms, with some oxygen atoms. (non-polar, insoluble, includes fats, phospholipids, steroids, and waxes)

Triglycerides

fats that are formed when glycerol bonds to 3 fatty acids

Ester bond

the bond that is formed between the fatty acids and the glycerol in a triglyceride

Saturated fatty acids

formed when all the carbons are linked by single covalent bonds (can’t wiggle and are packed tightly together)

unsaturated fatty acids

fatty acids that contain 1 or more carbon double bond (which create “kinks” in the chain)

cis fats

unsaturated fats that exist in nature

trans fats

unsaturated fats that do NOT exist in nature

phospholipids

similar in structure to triglycerides, but one hydroxyl group of glycerol is linked to phosphate group instead of a fatty acid

Steroids

four fused carbon atoms rings that typically have 1 or more polar hydroxyl groups attached to the ring structure

Waxes

Complex lipids which contain 1 or more hydrocarbons and long structures (that resemble a fatty acid) are attached to its carboxyl group to another long hydrocarbon chain (very non-polar)

Amino Acids

monomers of proteins (only 20 amino acids)

polypeptide

a linear sequence of animo acids joined together by peptide bonds

Peptide bonds

the covalent bonds formed between a carboxyl group and an amino acid

protein

A FUNCTIONAL unit composed of 1 or more polypeptides

N-terminus

the amino group on a protein (NH3) connected to the alpha carbon

C-terminus

the carboxyl group on a protein connected to the alpha carbon

peptide backbone

the amino group, the alpha carbon, and the carboxyl group

primary structure

the amino acid sequence of polypeptides (single chain)

secondary structure

the helix (alpha helix) or pleated (beta pleated) sheet structure that is stabilized by hydrogen bonds