Microbiology Chapter 2 P.1 Chemical Principles Flashcards by Alexis Thomas

Chemistry

study of interactions between atoms and molecules

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Atom

smallest unit of matter can’t be subdivided into small substances

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Protons and Neutron makes up what

Nucleus

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Electrons move around what

around the nucleus

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Which atom has a negative charge

electron

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Which atom has a positive charge

proton

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Which atom has a neutral charge “0”

neutron

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Atoms with the same number of protons are classified as the same….

chemical element

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atomic number

number of protons in nucleus

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atomic mass

total number of protons and neutrons in an atom

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Isotopes of Oxygen

16 Oxygen 17 Oxygen 18 Oxygen

8 8 8

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What are electrons arranged in

electron shells

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How are electrons arranged in electron shells

corresponding to different energy levels

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2n^2 what is (n)

principal energy level

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what does 2n^2 show

maximum occupancy per shell

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valence

number of missing or extra electrons in outermost shell

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how do atoms form molecules

by combining to fill their outermost shells

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Why do molecules hold together

valence electrons of the combining atoms form attractive forces called chemical bonds between the atomic nuclei

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chemical bonds

attractive forces

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compound

molecule that contains two or more kinds of atoms

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what is an example of a compound

water : 2 atoms of hydrogen one atom of oxygen

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what are equal in an atom

number of protons and electrons

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ions

charged atoms that have gained or lost electrons

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cations

atoms that lose electrons and become positively charged ions

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anions

atoms that gain electrons and become negatively charged ions

ionic bonds

attraction between ions of opposite charge | one atom loses electrons and another gains

covalent bonds

form when 2 atoms share one or more pairs of electrons | are stronger and more common in organisms than ionic bonds

hydrogen bonds

form when hydrogen atom that is covalently bonded to an O or N atoms in attracted to another N or O atom in another molecule

molecular mass

sum of atomic mass in a molecule

one mole of a substance is its...

molecular mass in grams

what is the unit of molecular mass

dalton (da)

chemical reactions

involve the making or breaking of bonds between atoms

a change in chemical energy occurs during what

chemical reaction

exergonic reactions

reactions that release energy

endergonic reactions

absorbs energy

synthesis reactions

occur when atoms, ions, or molecules combine to form a new larger molecule Atom, ion or + reactants B atom, ion or molecule = combine to form Product AB molecule New molecule

anabolism

synthesis of molecules in a cell

decomposition reactions

occur when a molecule is split into smaller molecules, ions, or, atoms Reactant AB = A atom, ion, or molecule + productions B atom, ion, or molecule B

catabolism

decomposition reactions in a cell

exchange reactions

are part synthesis and part decompostion

Example of exchange reaction

NAOH + HCL = NaCl + H2O

reversibility of chemical reactions

can readily go either direction may need special condition Reactants < ------> Product A+B HEAT AB

example of reversibility chemical reaction

NH4Cl (s) <---- NH3(g) + HCL (g) | ---->

What are the important biological molecules

organic and inorganic compounds

organic compound

always contain carbon and hydrogen typically structurally complex

inorganic compound

typically lack carbon, usually small and structurally simple

inorganic compound | water

inorganic; polar molecule; solvent; hydrogen bonds

polar molecule

unequal distribution of charges

polar substances undergo what

dissociation in water forming solutes

dissociation

one water molecule donates its proton to another water molecule

solutes

component dissolved in the solvent

hydrogen bonds absorb what

heat (temperature buffer)

Process of how water acts as a solvent for sodium chloride (NaCl)

sodium chloride crystal ---> A) sodium ion dissolved in water B) chloride ion dissolved in water

Acids

substances that dissociate into one more hydrogen ions (H+) and one or more negative ions HCL---> H+ + Cl-

Bases

Substances that dissociate into one or more hydroxide ions (OH-) and one or more positive ions NaOH ---> Na+ + OH-

Salts

substances that dissociate into cations, neither of which is H+ or OH- NaCl---> Na+ + Cl-

Acid Base Balance

concept of pH PH= -log10 [H+] increasing [H+] increases acidity increasing [OH-] increases alkalinity

concentration of H+ in a solution

most organisms grow best between which pH

pH 6.5 & 8.5

PH scale

0 to 6 acidic solution 7 neutral pure water [H+]=[OH-] 8 to 14 is basic solution

organic compounds commonly contain which elements

oxygen, and or nitrogen in addition to carbon

the chain of carbon atoms in an organic molecule is what

carbon skeleton

functional groups

bond to carbon skeletons and are responsible for most of the chemical properties of a particular organic compound

example of a functional group

hydroxyl group of alcohols ---> methanol, ethanol, isopropanol

funct. group ---> alcohol | biological importance?

lipids, carbohydrates

functioning group- aldehyde biological importance?

biological importance: reducing sugars such as polysaccharides

FG-Ketone BI?

BI: metabolic intermediates

FG: Methyl BI?

BI:DNA, energy metabolism

FG: Ester BI?

bacterial and eukaryotic plasma membranes

FG: Ether BI?

archaeal plasma membranes

FG: sulfhydryl bi?

energy metabolism protein structure

FG: carboxyl bi?

organic acids

FG: phosphate bi?

ATP; DNA

what are the 10 functional groups

alcohol, aldehyde, ketone, methyl, amino, ester, ether, sulfhydryl, carboxyl, and phosphate

in aldehyde molecule a C-- double bond O is at the end of a molecule in contrast to ...

the internal C-- double bond O in a ketone

small organic molecules can combine into large ....

macromolecules

polymers consisting of many small repeating molecules

monomers

small repeating molecules

dehydration synthesis

R-OH+OH-R--->R-R+H2O | losing water