bio chemistry of life quiz 1

1. Compare the structures and functions of DNA and RNA, noting similarities and differences.

double-stranded helix that stores genetic information

single-stranded and carries out protein synthesis

1. Explain how a protein’s shape determines its functions.

protein has to have the right shape for it to function but if it denatures then it looses the function entirely

creating unique binding sites

1. compare the processes of dehydration synthesis and hydrolysis.

Monomers are joined to form larger polymers, with a water molecule being released or removed in the process. 

Polymers are broken down into their constituent monomers by the addition of a water molecule, which breaks the covalent bond holding them together

1. Explain the relationship between monomers and polymers.

monomers form polymers

1. List the four main classes of macromolecules important to life.

carbs, proteins, lipids, nucleic acid,

1. Define organic compounds and an isomer.

molecules primarily built around a core of carbon atoms, often bonded to hydrogen

one of two or more compounds that have the exact same molecular formula (the same number and type of atoms) but different arrangements

1. Explain why carbon is unparalleled in its ability to form large, diverse  molecules.

a carbon is unparallel in its ability to form large diverse molecules because it can go off in 4 directions and bond to 4 other atoms.

1. explain how buffers function.

buffers minimize changes in pH by accepting H+ when it is in excess and donating H+ when it is depleted (example: sodium bicarbonate)

1. Explain the basis of the pH scale

Higher numbers=more basic, lower numbers=more acidic. Each number represents a tenfold change in concentration (eg: lemon juice at pH 2 has 10 times more H+ than an equal amount of grapefruit juice (pH 3), 100 times more H+ than an equal amount of tomato juice (pH 4) and 100,000 times more H+ than an equal amount of pure water)

1. Explain how acids and bases directly or indirectly affect the hydrogen ion concentration of a solution.

Acids either give H+ ions to a solution or take up OH- ions which has the affect of increasing H+ concentration and therefore making the solution more acidic. Bases do the opposite - they either take up H+ ions or donate OH- ions which has the affect of decreased the H+ concentration and making the solution more basic.

1. Define a solute, a solvent, and a solution.

A solute is a substance dissolved by a solvent. A solution is a liquid consisting of a uniform mixture of two or more substances. An aqueous solution is a solution in which water is the solvent.

1. Define and distinguish between cohesion and  adhesion.

Cohesion is the sticking together of molecules of the same kind (in water because of hydrogen bonds) but surface tension is how difficult it is to stretch or break the surface of a liquid.

1. Describe the special properties of water that make it vital to living systems.

1. Explain how these properties are related to hydrogen bonding.

Because of hydrogen bonds, water has a high boiling point and when it freezes, ice has a lighter density than the liquid because the hydrogen bonds are stable and farther apart. Because ice floats on top of water, water organisms can live through the winter. Water is also called the universal solvent because it dissolve so many solutes.

1. Distinguish between covalent bonds, nonpolar polar covalent bonds, polar  covalent bonds, hydrogen bonds, and ionic bonds, noting their relative strengths and how and where they form.

Covalent bonds are bonds in which two atoms share one or more pairs of outershell electrons. Non-polar covalent bonds are bonds where the electrons are shared equally between the atoms. Polar covalent bonds are bonds in which there is an unequal sharing of electrons. And ionic bond is when two ions with opposite charges attract each other, and when the attraction holds them together this is called an ionic bond. Hydrogen bonds are bonds in which the hydrogen connected with an element such as oxygen and is left with a positive charge.

1. Explain how the electron configuration of an atom influences its chemical  behavior.

Only electrons are directly involved in chemical activity of an atom. The valence shell or the outermost she'll of electrons determines the chemical properties of an atom. Atoms who's outer shells are not full or have unpaired electrons tend to interact with other atoms that is to participate in chemical reactions. Chemicals with full valence shells are inert or unreactive.

1. Define an isotope and explain what makes some isotopes radioactive.

An isotope of an element has the same number of protons and behave identically in chemical reactions, but they have different numbers of neutrons. A radioactive isotope is one in which the nucleus decays spontaneously giving off particles and energy. This can cause cellular molecules to become damaged and can pose a risk to living organisms. They can be helpful in the use of dating fossils or be used in biological research and medicine

1. Distinguish between the size, location, and properties of protons, electrons, and neutrons.

A proton is a subatomic particle with a single positive electric charge within the nucleus of an atom. And electron is a subatomic particle with a single negative charge. It is the subatomic particle that circles the atom and does not have much mass. It moves around the nucleus at almost the speed of light. The neutron is a subatomic particle that is electrically neutral and is located in the nucleus of an atom. The proton and the neutron have the same mass.

1. Define matter, an element, a compound, and a trace element.

Matter is anything that occupies space and has mass. An element is a substance that cannot be broken down to other substances by ordinary chemical means. A compound is a substance consisting of two or more different elements combined in a fixed ratio. Lastly, a trace element is an element that is essential to life but only in minute quantities.

polynucleotide

a nucleic acid polymer

rna nitrogenous bases

a, c, g, u

dna nitrogenous bases

a, t, c, g

nucleotide monomer

5 carbon sugar, phosphate group, nitrogenous base

quaternary structure

2 or more polypeptides combine to make final protein

tertiary structure

r groups interact overall 3d shape of a single polypeptide

secondary structure

coiling into an alpha helix or folding into a beta pleated sheet, held in place by h bonds, 3d ish

primary structure

unique amino acids sequence encoded by dna

denature

change in shape in proteins, permanent, caused by heat ph extremes,

protein functions

structural, contractile, receptor, transport

enzymes

metabolic catalysts regulate chemical reactions in cells

polypeptides

joining amino acids together

peptide bonds

how amino acids are linked together

amino acid monomer

monomer of proteins

saturated fatty acids

all single bonds between carbon, tightly packed fatty acids, solid at room temp

unsaturated fatty acids

have at least one double bond causes kinks in fatty acid chains

;liquid at room temp

triglycerides

helps form lipids

steroids

lipids with four ring structure

phospholipids

2 fatty acid chains and phosphate group

attached to glycerol

has hydrophobic and hydrophilic

fats

large lipids made from glycerol and 3 fatty acids

lipid functions

long term energy storage, cell membrane, hormones

carbs function

energy storage and structural

polysaccharides

polymers composed of 1000s of monosaccharides

disaccharides

2 monosaccharides joined by dehydration

monosaccharides

carbs monomer

hydrolysis

breaks apart polymers into monomers with water

dehydration reactions synthesis

releases water, mediated by enzymes and broken down by hydrolysis

macromolecules monomers

formed by dehydration synthesis, links monomers together

carbs proteins lipids nucleic acid macromolecules

polymers and made of subunits bonded together

functional groups for organic compounds

group of atoms attached to carbon skeleton

helps determine the properties of organic compounds

isomers

isomers are molecules with same molecular formula but different results

carbon organic compound

carbon can make four covalent bonds

single double and triple bonds

bonds itself and other elements

forms chains rings and branched molecules

hydroxide ions OH- and hydrogen ions (h+)

adeqous solution

adeqous solution water is the solvent

in liquid water, some molecules break apart into ions such as those

solvent of life

solution

solvent

solute

solution-liquid consisting of a uniform mixture or two or more substances

solute-substance that is dissolved

solvent-dissolving agent

temperature moderation with water

water resists change, energy absorbed to break hydrogen, lot of energy before increase in temp, energy released when h forms as h20 cools

water adhesion v cohesion

cohesion: 2 of same kind bound with hydrogen

much stronger, surface tension

adhesion: 2 or more different bond with hydrogen

hydrogen bonds and ionic bonds

hydrogen has partial positive charge, attracted to negatives, weak but numerous, large

polar v nonpolant covalent bond

polar are unequal sharing of electron, molecule has partial postiive and neg charge

non polar are equal sharing of electrons

electrons

directly involved in chemical activity, electron shells, outermost shell involved, forms chemical bonds

radioactive isotopes v isotopes

radio: nucleus decays spontaneously, gives off energy, not all

isotopes: same number of protons, diff electrons

behave identically

subatomic particles

protons, neutrons, electrons

electrons are outside nucleus

compounds

2 different elements combined in a fixed ratio

table salt, sodium chloride

trace elements

required in small amounts like iron

matter

made of chemical elements like carbon hydrogen oxygen and nitrogen

substances that cannot be broken down

matter elements and compounds

organisms are composed of matter, anything that occupies space has mass