Chapter Two; Bio 210 (Cells) Flashcards
Matter
anything that takes up space
Energy
ability to move matter (w=f/d)
Potential Energy
stored energy
Kinetic Energy
moving matter
Chemistry
study of matter and changes it undergoes
Inorganic v.s Organic Chemistry
Organic- always contain carbon (Carbons has to either bond with another carbon or hydrogen bond C-H or C-C)
Inorganic- do not have a carbon to carbon or a h-h bond
4 different types of energy
Thermal, Mechanical, Light, Electrical, Sound, Chemical, and Gravitational
Two laws of thermodynamics
1- Energy can not be created nor destroyed
2- In an energy transaction energy is always lost as heat
Element
are the building blocks of matter (pure substance)
Explain: Understanding the fundamental nature of life is accomplished within the context of chemistry
Life is always undergoing change, if one can understand chemistry, which is the study of matter and change it undergoes, one can understand the nature of life
Name six elements that make up about 98% of the human body? And 96%?
96%- CHON (carbon, hyrdogen, oxygen, nitrogen)
98%- Calcium and Phosphorus
Atoms
smallest particle of an element that can display the characteristics of that element, and enter into a chemical reaction
(H= one atom of Hydrogen, C= one atom of Carbon)
Nucleus
the center of an atom in which electrons move around
Proton
one positive charge
Neutron
no electric charge
Electron
one negative charge (2,8,18,32,50,72)
Isotopes of elements
(C-12; 6p 6n) (C-13; 6p 7n)
different number of neutrons in different atoms of the same element
Atomic number
number of protons in nucleus
Mass number (atomic mass)
of protons and # of neutrons
Atomic Weight
average mass number of all isotopes of an element
Outer energy level
valence shell
Octet rule (H and He only exceptions)
no matter how many shells exist in an atom from energy level to energy level seven, the max number of electrons in the valence shell is 8
(when atoms fill their valence shell the atoms are stable)
Ion
more electrons OR less electrons than protons
Cation +
more protons than electrons
Anion -
more electrons than protons
Ionic Bond
Cation + Anion
Ex: NaCl (see leather book for picture)
Ionic bonds are WEAK
Covalent Bond
atoms SHARE electrons to make new substances
Non Polar and Polar
Non Polar covalent bond
atoms of the same element form together because the same element has the same number of electrons
Ex: H + H => H2
Polar covalent bond
atoms shared unequally
Ex: H2+O => H2O (molecular compound)
covalent bonds are STRONGER than ionic bonds
(See leather book for picture)
Hydrogen Bonds
when a POSITIVE end of one polar molecule is weakly attracted to the NEGATIVE end of another polar molecule
(occur mostly between H,O,N)
weaker than ionic and covalent bonds
(their function is to hold molecules together and dictate shape of molecule)
Ionic bonding FACT
When atoms come together to form ionic bonds, the atoms DO NOT share valence electrons. Atoms give away or accept valence e-. This creates ions. The reason they stay together is because of the opposite charges between the cation and anion. Negative forces pull them together. Their bonds are WEAK and tend to cluster together forming crystaline structures… salt.
Molecules of elements vs compunds
Compounds: Only covalent compunds are molecules, not ionic because they do not share electrons.
Elements: non polar covalent bonds
Dissociate
when ions seperate.
Ex: NaCl is put into water. The cation goes towards the negative ends of h20 and the anion attracted to positive ends of h20.
Metabolism
sum of all chemical reactions in the body
Metabolism:
Anabolic
Catabolic
Anabolic- chemical reaction when smaller substances form larger substances
Catabolic- chemical reaction when larger substances BREAK into smaller substances
Energy Flow in Chemical Reaction:
Energonic
Exergonic
Endergonic- stores energy
Exergonic- releases energy
Reactants and Products in Chemical Reactions
Anabolic (endergonic)
Metabolism—–>
Catabolic (exergonic)
Endergonic (anabolic) Energy Flow----->
Exergonic (catabolic)
4 Factors that influence the Rate of Chemical Reactions
* R C T C *
Reactants and ability to react: all elements react differently to other elements
Concentration of the reactants: greater the concentration, more likely the reacting molecules are to come into contact with one another
Temperature: greater the temp. greater the reaction
Catalysts: increase rate of chemical reaction without being changed in the reaction (enzymes)
Synthesis Reaction
(Dehydration synthesis reaction)
ABC=A+B+C
Reactant=product
occurs when two or more reactants combine to form larger, more complex product
Ex: C6H12O6—> C12H22O11 + H2O
(Anabolic, endergonic reaction) STORES ENERGY
Decomposition Reaction
Hydrolysis
occurs when reactants are broken down into smaller less complex products. (Digestion of food molecules)
Ex: C12H22O11 + H2O —–> C6H12O6 + C6H12O6
(catabolic, exergonic reaction) RELEASES energy
Water universal solvent for living organisms
Water dissaciates different compounds and elements because of the positive and negative attractions of H20 because of the polarity of water
Water’s interactions with hydrophilic and hydrophobic molecules
Hydrophilic- mixes with water (NaCl)
Hydrophobic- does not mix with water (fats, lipids, waxes)
Importance of water because it is a polar molecule
Water can seperate compunds
Water creates hydrogen bonds
hydrogen bonds allow other chemicals to attach to them to be transported throughout the blood such as nutirents. It attaches to the hydrogen bonds that water produces (H2O)
ADP to ATP
ADP + P + E ====> ATP ( []-P~P~P )
ATP - P - E =====> ADP 9molecule has less energy than ATP)
Electrolyte
soluble inorganic substance whose ions will conduct an electrical current when dissociated in a solution (ALL ionic compounds are electrolytes) SALT
Acid
a substance that dissociates in water, releasing “free” hydrogen ions. ( H+ )
Buffers remove hydrogen ions when in a solution together
Base
a substance that either accepts H+, or releases hydroxide ions in a solution ( OH- )
Buffers
Resists rapid changes in pH. Weak acid and weak base. Bicarbonate buffer system in the blood (Buffer System)
pH rising in blood
alkalosis
pH falling in blood
acidosis
Calcium
Ca can deposit elsewhere and can cause problems. Cowboy bones, calcium deposits in the heart
Isomers
molecules with the same chemical formula but a different chemical structure. Ex: Glucose and Fructose (C6H12O6)
Amino Acid (monomer)
building blocks of proteins. AA-AA-AA-AA-AA (multiple AA’s put together are polymers)
Proteins
contain C,H,O,N and most have sulfur.
Carbohydrates
energy storage or energy usage (most sugars end in ‘ose’)
Monosaccharides
simple sugars (single sugars) only have 3 to 7 carbons
Ex: C6H12O6
Used for energy because it’s small
Disaccharides
combining two monosaccharides together
Ex: Sucrose
Polysaccharides
putting many and many of monosaccharides together. Ex: Starch and Cellulose (glycogen is animal starch)
COOH
acid group
Saturated Fats
no double C bonds
Ex: C-C-C-C-C-
Unsatruated Fats
double Carbon bonds
Ex: C-C-C=C=C-C
Fatty Acid
determines chemical property of Triglycerides
Determined saturation by the length of bond between carbon atoms (most are 14-18 carbons)
Mono, Di and Triglycerides
Functions of Trigylcerides
Energy Storage
Insulation ** ( P I E ) **
Protection
Phospholipids
most abundant molecules of plasma membrane in living cells. Important for structure and permeability
Head of phospholipids
Polar, hydrophillic
Tail of phospholipid
Lipid, non polar, hydrophobic
Steroids
Cholesterol ! all steroids derived from cholesterol (Sex hormones: testosterone, estrogen and Bile Salts)
Proteins
are polymers made of monomers called amino acids
-most abundant organic molecule in the body (20% of body weight) ALL contain CHON
Polypeptide
2-99 amino acids
Proteins
> 100 amino acids
Peptide v.s Proteins
the only difference is the number of amino acids
Functions of proteins in the body
Catalysts Structure and protection Plasma membranes of cells Transport Receptors (sense that something is wrong) Markers (self v.s non self, kill anything that doesn't belong) Muscle contraction
Enzyme
increase the rate of a reaction without being permanently changed
Substrates
attach to enzymes to carry out the enzymes function. (Lactase to lactose, fructase to fructose)
Substration attachment
once a substrate attaches to the enzyme the enzyme breaks and quickly changes shape.
Energy of Activation
minimum energy needed to start a chemical reaction
ENZYME EXAMPLE
molecule A…..
ENZYME……
molecule B…..
molecule A+moleculeB+ENZYME=> enzyme breaks=> moleculeAB
Specificity
the enzymes can’t just react with ANYTHING
Factors that affect enzyme catalyzed reactions
Cofactors and Cozenzymes
Temperature
pH
Concentration of enzyme or substrate
Competetive Inhibition
when a substrate and another molecule compete for the active site of an enzyme
Noncompetetive Inhibition
when a molecule beats the substrate to the allosteric site, In return, altering the shape of the active site
Active Site
structural site where the substrate can perfectly fit in the enzyme
Allosteric Site
the second site on an enzyme that can sometimes be a different site from the active site. (Square shape v.s round shape)
