Chapter 2: Chemical Basic of Life

20 Amino acids required for animal life to exist....

(See chart)

Compound vs. mixtures

- Components in mixtures are physically mixed, not chemically bonded. Physically unchanged when combined. - Components in compounds are chemically bounded and can only be separated by breaking the chemical bond. Mixtures can be separated by filtration, straining, evaporation and centrifugation. - All compounds are homogeneous, mixtures can be both.

Glycerol (C3H8O3)

Molecule modified three carbon simple sugar

Primary structure (protein)

The sequence and number of amino acids that link together to form the peptide chain.

Composition of Matter

Elements and atoms

States of matter

Gas Liquid Solid The bodies of animals contain examples of each state.

Factors influencing the rate of reaction

- Concentration of reactants (Availability of the reactants) more that are available the more likely they will come in contact and be able to react with one mother. - Temperature of environment. Temp ^ speed of the molecular movement ^ chances of molecules meeting improves. ^ the velocity at which the reactants meet which provides the energy for the reaction.

Proteins (examples)

-Contractile structural proteins - that make up much (ex. Actin and myosin) -Other structural proteins - that make up cartilage and tendons (collagen,) and hair and skin (keratin) -Globular functionalists proteins - such as enzymes, antibodies, hemoglobin and many integral and peripheral proteins in the cell membrane

Water can fulfill important roles within a living organisms because...

-Universal solvent -Ideal transport medium -High heat capacity and a high heat of vaporization. -High heat of vaporization - Used for lubrication

How many elements are there (occur in nature)

118 92; rest are made artificially or are theoretical and not known to exisit.

Amino acids

20 different found in the boy. All share basic structure. Contains central carbon atom attached to a hydrogen atom, an amino group (NH2) a carbonyl group (COOH) and a unique group of side chain designated by the letter R (defines each one)

Electron capacity

2n^2 where n equals the principal a quantum number or energy level

Orbital model

3-D view of the most likely location of the electrons at any given times.

pH of animal body must be at around

7.4 , slightly basic

What elements make up a large percent of the body (%)

96% Oxygen Hydrogen Carbon Nitrogen

Dehydration synthesis (ex)

A chemical reaction in which water is created, it is extracted from the saccharides. Glucose and fructose making sucrose

Synthesis reaction

A new and more complex chemical is made by combining multiple smaller molecules or elements together. Bonds are formed. Underlie all anabolic ((constructive) processes and are particularly evident during growth and the repair of tissues.

Decomposition reaction

A single chemical is broken down into multiple smaller chemical units. Break down of chemical bonds. Foundation of catabolic (degradation) reaction.

RNA (structure)

A single strand of nucleotides; each nucleotide is composed of: a phosphate group; a ribose sugar, and one nitrogenous base (ex. Cytosine, guanine, alanine or uracil)

ATP (ex.)

ATP is used by the cell to carry out all active metabolic processes; when the terminal phosphate group is removed, energy is released and the molecule becomes adenosine diphosphate (ADP). ADP is transported back to the mitochondria where it is converted back to ATP

Used for lubrication (example)

Ability of water to surround molecules allow it to be a lubricant for moving parts in the body. Fluids in the pericardial sac allows the heart to move freely within the sac and synovial fluids in the joints allows bones to rub without pain when a limb is moved.

pH scale

Acidity and alkalinity are measured on a pH scale. From 1 (acidic) increase of H+ to 14 (alkaline or basic) 7 in the middle/neutral increase of OH-

5 nucleotides

Adenine Guanine Cytosine Uracil - only RNA Thymine - only DNA

AMP

Adenosine Monophosphate. As more glucose and other nutrients are metabolized, phosphate groups are joined to AMP, creating a renewed source of ATP. Without ATP, muscle cells could not contract, enzymatic reactions could not take place, and molecules could not be actively transported across cell membranes.

ATP

Adenosine triphosphate. The energy currency of cells. Cells need ATP to fuel any work that they do. ATP is an RNA nucleotide containing the nitrogen base adenine with two additional phosphate groups attached

Examples of gas in the body

Air that is inhaled Gas that is exhaled

Bases

Alkaline compounds that are ionically bonded also ionize in water but release a hydroxyl ion (OH-) not hydrogen ions, therefore bases are known as proton acceptors. Hydroxyl ions are attracted to H+ ions to form water.

Anabolism

Cells use synthesis reactions to build molecules needed for cellular functioning.

Glycogen, Starch,Cellulose

All polysaccharides, stores fuel in body tissues Similar functions in plant tissues. Most abundant organic molecule in the biosphere, provides structural strength to plants.

Colloid (ex. in body)

Also known as emulsions, Heterogenous. Larger sized solutes however do not precipitate to of colloids but they often reflect light. Translucent or milky. Cytosol

ATP (structure)

An ATP molecule is composed of: adenine, a ribose sugar and three phosphate groups (where energy is stored)

Archaebacteria (now exist?)

Ancient bacteria that survived the harsh O free environment of young earth. Still exist today in the extreme environment of hot springs, salt flats and the intestines of mammals

Matter (identify how)

Anything that occupies space and has mass; With our senses by touch, sight, taste and smell. Not based on weight. Composed of one or more atoms.

High heat capacity and high heat of vaporization

As chemicals in solutions react, they often give off energy as heat. Water is able to absorb heat so the temperature of a solutions doesn't rise too rapidly. Stabilization is necessary to keep living organisms in a stable temp range so that the reaction of life's processes can occur at a steady rate without interruption.

Exchange reaction

Certain atoms are exchanged between molecules. Combination of a synthesis and decomposition reaction. Bonds are broken and made. Most have no net energy requirements.

Silicone (Si)

Atomic # 14 Body mass 0.1 Component of some enzymes. TRACE

Potassium (K)

Atomic #!9 Body mass 0.4 Principal + ion within cells; important in nerve function MAJOR

Hydrogen (H)

Atomic #1 Body mass 9.5 Component of water and organic molecules; necessary for energy transfer and respiration; ion influences pH of fluids MAJOR

Sodium (Na)

Atomic #11 Body mass 0.2 Important + ion in extracellular fluids; important in nerve functions MAJOR

Magnesium (Mg)

Atomic #12 Body mass 0.1 Component of many energy-transferring enzymes MAJOR

Aluminum (Al)

Atomic #13 Body mass 0.1 Component of some enzymes. TRACE

Phosphorus (P)

Atomic #15 Body mass 1.0 Principal component in back on of nucleic acids; important in energy transfer (part of ATP); Component of bones MAJOR

Sulfur (S)

Atomic #16 Body mass 0.3 Component of most proteins MAJOR

Chlorine (Cl)

Atomic #17 Body mass 0.2 Ion is most abundant negative ion in extracellular fluids MAJOR

Calcium (Ca)

Atomic #20 Body mass 1.5 Components of bones and teeth; required for muscle contraction, nerve impulse transmission and blood clotting MAJOR

Vanadium (V)

Atomic #23 Body mass 0.1 Component of some enzymes. TRACE

Chromium (Cr)

Atomic #24 Body mass 0.1 Needed for proper glucose metabolism TRACE

Manganese (Mn)

Atomic #25 Body mass 0.1 Needed for fatty acid synthesis TRACE

Iron (Fe)

Atomic #26 Body mass 0.1 Critical component of hemoglobin TRACE

Cobalt (Co)

Atomic #27 Body mass 0.1 Needed for maturation of red blood cells TRACE

Copper (Cu)

Atomic #29 Body mass 0.1 Needed for myoglobin and myelin TRACE

Zinc (Zn)

Atomic #30 Body mass 0.1 Important component of many enzymes and proteins TRACE

Selenium (Se)

Atomic #34 Body mass 0.1 Antioxidants TRACE

Molybdenum (Mo)

Atomic #42 Body mass 0.1 Key component of some enzymes TRACE

Boron (B)

Atomic #5 Body mass 0.1 Component of some enzymes TRACE

Tin (Sn)

Atomic #50 Body mass 0.1 Component of some enzymes TRACE

Iodine (I)

Atomic #53 Body mass 0.1 Component of thyroid hormones TRACE

Carbon (C)

Atomic #6 Body mass 18.5 Primary component of organic molecules MAJOR

Nitrogen (N)

Atomic #7 Body mass 3.3 Component of proteins and nucleic acids MAJOR

Oxygen (O)

Atomic #8 Body mass 65.0 Necessary for cellular respiration; component of water. MAJOR

Fluorine (F)

Atomic #9 Body mass 0.1 Component of bones and teeth. TRACE

Isotopes

Atoms that contain a different number of neutrons.

Ideal transport medium

Blanketing property allows molecules in the water to move around freely and to be cushioned fro each other. Because many molecules can be easily dissolved, they can be carried easily to locations in the body

Examples of liquid in the body?

Blood is primarily composed of water, helps transport critical nutrients to hungry tissues

Amino acids (linking)

Can be linked in a # of ways to create a protein. DNA determines the nature and functions of the amino acids. They are linked by a dehydration synthesis reaction. Carbonyl group of one amino acid links with the amino group of another via a peptide bond, releasing a molecule of water.

Glycoprotein (role)

Carbohydrate that can be joined with other molecules (lipids or proteins) Macromolecule made of a carbohydrate attached to a protein; Adhesion of cell to other cells + recognition of molecules to be transported into the cell.

Messenger RNA

Carries the information (genetic code) out of the nucleus to cytosol

How enzymes work?

Catalyzing chemical reactions. Don't get destroyed or altered during process. Acts in a series of reaction one becoming the substrate of the next reaction.

Catalyst

Certain reactions require the presence of a catalyst. Usually special proteins that hold the reactant together so they may interact. It is not destroyed or used up by the reaction, the reaction speed is increased when there are more catalyst proteins present (enzymes)

Fatty acid

Chain of carbon atoms with one or two hydrogen atoms attached to each carbon by single or double bonds.

Functional proteins functions

Chemical reactions - Proteins enzymes: essential to almost every biochemical reaction in the body. Transport of molecules - Hemoglobin transports O in the blood Regulation of metabolism - Peptide hormones: regulate metabolic activity, growth and development Immune system - antibodies (immunoglobulins) are proteins created by immune cells that recognize foreign substances such as viruses

Endergonic

Chemical reactions that absorb energy because they contain more potential energy in their helical bonds than the reactants. Include most anabolic reactions.

Quaternary structure (protein)

Combination of more than one polypeptide chain; when unite to form the complete protein molecule. Hydrogen and covalent bonds between atoms of the proteins stabilize the shape of the macromolecule.

Polysaccharides

Combo of many monosaccharides, all joined by dehydration synthesis. Can have structural and fuel storage function.

Solutes

Component in a mixture that is present in a smaller amount.

Solvent (most important)

Component in a mixture that is present in the greatest amount; H2O

Organic compound (groups)

Composed of large molecules containing carbon. Carbohydrates, lipids, proteins and nucleic acids. Carbon is most stable when it has 4 covalent bonds with other atoms. Various structures can be built using a small selection of atoms.

Transfer RNA

Copies the information in the NDA molecule. Carries amino acids to docking station of mRNA

Early bacteria (function; their enzymes)

Created chemical energy needed to maintain themselves and reproduce; They created O gas ass water product, O increases in atmosphere making living organisms possible

Nucleic acids (types)

Deoxyribonucleic acid (DNA) Ribonucleic acid (RNA) Adenosine triphosphate (ATP)

DNA

Deoxyribonucleic acid exists mainly in the nucleus but also in mitochondria. The blueprint. Sugar in it is deoyxribose.

Eicosanoids (structure/ex.)

Derived from arachidonic acid, a 20-carbon fatty acid. Ex. Regulatory molecules that enhance the immune system and elicit inflammatory responses (e.g., prostaglandins, mediate inflammation; leukotrienes, mediate bronchoconstriction; thromboxanes, mediate platelet function

Acids and bases are

Electrolytes, when ionize in water, they can transmit electricity. When adding an acid and base into water they both neutralize each other. Able to join with other substances.

Activation energy

Energy required for the reaction to happen. When requiring the input of more energy the reaction occurs in a slower pace.

Atomic number

Equals to the number of protons found in the nucleus.

Other lipids substances

Fat-soluble vitamins Eicosanoids

Saturated fatty acid (found where)

Fatty acid inn which all bonds in the hydrocarbon chain are single bonds and as many hydrogen atoms as possible are attached to the carbon; Animal fats such as butter and lard

Compounds

Formed from the joining of elements, 2 types Inorganic - Don't contain hydrocarbons such as salts and water. Organic - Has hydrocarbons present which are usually bonded to another group of atoms know as "Functional group"

Ionic bonds

Formed when electrons are transferred from one atom to another. Most often with an atom with a nearly full shell and an atom with fewer than two electrons. Atom with fewer will be inclined to give up the electron so its "new" outer shell will be stable.

DNA (ex.)

Found in the nucleus where it condenses with his tone proteins to form chromosomes; also found in mitochondria, providing the molecular instructions for making the enzymes needed for cellular respiration

Polar molecules

Has oppositely charged ends. Slight + charge on the H, Slight - charge on the O, Position of the covalent bonds arrange the H atoms towards the same side of the O molecules.

Suspensions

Heterogenous mixtures containing large solutes that readily separate from the solution when there is no movement of the suspension.

6th electron shell (P)

Hod up to 72 electrons

1st electron shell (K)

Holds two electrons

3rd electron shell (M)

Holds up to 18 electrons

4th electron shell (N)

Holds up to 32 electrons

5th electron shell (O)

Holds up to 50 electrons

2nd electron shell (L)

Holds up to eight electrons

Solution

Homogeneous. Solutes in solutions are very tiny consisting of molecules. Because the solutes are minute, they are found evenly distributed throughout the solvent, do not settle out and do not refract light. Solutions are usually clear.

Elements making up 96% of living organisms

Hydrogen Oxygen Carbon Nitrogen

Sol-gel transformation

In Colloid the ability to transform from a fluid to a solid and back again.

All living entities are formed from...

Inorganic chemicals (water and salts) Organic chemicals (proteins, lipids, carbohydrates and nuclei acids)

Body; thousands of chemicals

Interacted with one another at rapid speed, Physiological process of life respiration, digestion, reproduction and movement

Chemical reactions (types)

Involves the formation and breaking of chemical bonds. Synthesis, decomposition and exchange.

Acids

Ionically bonded substances that, when added to water, freely release hydrogen ions (H+) Acids ionize in water and one of their ions is H+. H+ donors or proton donors since H+ is a proton with no electron

Net electrical charge

Is neutral, atoms contains equal # of protons and electrons. The + and - charges cancel each other out.

Nucleic Acids (classes)

Largest molecules in the body and are composed of carbon, oxygen, hydrogen, nitrogen, and phosphorus. DNA and RNA

What provided the energy needed to covert CH4,H20,NH4 into organic molecule..

Lightning Ultraviolet light Meteorite strikes Thermo reactions in the earth's crust and core

Eicosanoids

Lipids formed from a 20 C fatty acid and a ring structure. Important for mediation of complex chemical processes in the body and include: prostaglandins (PGs), which mediate inflammation; thromboxane, which mediates platelet function; and leukotrienes, which mediate bronchoconstriction and increased mucus production.

Steroids (structure/ex.)

Lipids that form four flat interlocking hydrocarbon rings (hydrophobic, nonpolar, little O) basic ring structure is synthesized from acetyl CoA Ex. Cholesterol, cortisol, testosterone, estrogen

Lipoprotein (purpose)

Macromolecule composed of proteins and lipids; Used to transport fats within the body. Hydrophilic proteins allow the fats to be shielded from the blood plasma and to be transported.

Many of the organic molecules used in the body are

Macromolecules - long complex molecules, often with repeating units.

Atomic nucleus

Made up of protons and neutrons grouped together each having an atomic mass of 1.

Neutral/simple fats (purpose)

Mainly used for energy; bonds are broken down and energy is stored in adipose tissues. Pad vital organs from trauma, help maintain body temperature. Do not mix with water.

Elements (types)

Matter made up of two or more elements. Single pure substances consisting of only one type of atom. - Metals - Metalloids - Nonmetals Each have their own properties, can join in different combinations with other elements to form all the matter exists in earth

Atmosphere of Earth contains

Methane gas (CH4) Water (H20) Ammonia (NH4)

Salts

Mineral compounds that have ionic ones, principal form of mineral that enter and are stored in the body. When salt is added to water they immediately ionize, or divide into separate ions.

Nucleotides (# and made of)

Molecular building blocks of nucleic acids. 5 different ones however all with the same basic structure. Nitrogenous base, plus a five-carbon (pentose) sugar, plus a phosphate group.

Simple carbohydrates (structure,ex.)

Monosaccharide; most stable as a single penthouse ring. Three to seven atoms in a chain or ring. Hexose - six carbon Pentose - five carbon Disaccharide; two pentose rings Ex. Glucose, fructose, ribose, deoxyribose

Hydrogen bond

More of an electrostatic attraction because electrons are neither shared nor transferred. Weakest bond. Can form between atoms within the same molecules and between atoms on separate molecules. Formed mostly between molecules and act to stabilize the solution. Forming bonds between parts of the age molecule stabilizes the molecule.

Proteins (used for)

Most abundant organic molecule in the body. Widest variety of functions; Used for cell structures and structural body tissues, for controlling chemical reactions, for regulating growth, and for defending the body from invaders. Proteins catalyze or speed up all reactions occurring in the body, and they transport ions and other molecules into and out of the cell and around the body.

Exergonic

Most catabolic and oxidative reactions are this because they yield products with less energy than the initial reactants. Much of the energy released is captured in ATP molecules.

H2CO3 -> H+ + HCO-3 HCO-3 -> H+ + CO3^2- (Complete reaction)

Most effective buffer. -Carbonic acid ionizes when placed in water, to free hydrogen ions and the weak base, bicarbonate. -Bicarbonate (HCO3-) can further ionize by losing a proton, resulting in carbonate (CO3^2-) (Bicarbonate acts as both a weak acid by losing a proton and a weak bae, by gaining one)

Examples of solids in the body?

Musculoskeletal system composed of bones, tendons, ligaments and muscles.

Secondary structure (protein)

Natural bend of parts of the peptide chain ass it forms in 3D. Bends are stabilized when the atoms of the protein molecule form weak hydrogen bonds with each other. Can be helical or pleated.

Lipids (types)

Neutral/simple fats Phospholipids Steroids Eicosanoids

What was the product of the first nuclear reaction?

New elements that were blown into the cosmos when stars exploded into supernova.

Compounds that make up a living organism (categories)

Organic and inorganic

Proteins (made of)

Organic molecules, C, O, H and N though some proteins also contain sulfur, iron and phosphorus.

Tertiary structure (protein)

Overall shape of a single protein molecule. Consists of either folded alpha helixes (spring shape) or beta pleats (accordion shape) shapes can occur in the same protein a different places.

What elements were forged in the beginning nuclear furnaces ?

Oxygen Nitrogen Iron Silicone Including other elements

Phospholipids (structure/ex./purpose)

Phosphate head (PO4,hydrophilic,polar) glycerol backbone and two fatty acid chains (hydrophobic) Ex. Key component of the bilateral of the cell membrane Main component of cellular membranes, also form myelin sheath of nerve cells.

Models to represent atoms?

Planetary and Orbital models

Complex carbohydrates (structures,ex.)

Polysaccharide Ex. Starches; glycogen: stores energy in liver; cellulose: derived from plants and provides insoluble fiber in diet.

Ions (in body)

Positively and negatively charged atoms. All ions are involved in essential functions in the animal body ex. contraction of muscle fibers, transmission of nerve impulses and maintenance of water balance.

Inorganic molecules (examples)

Rarely contain Caron and do not contain C-C or C-H bonds. Tend to be small molecules and often have ionic bonding. Water, salts, acids and bases

RNA

Ribonucleic acid. Transfer instructions out of the nucleus and into the cytoplasm of the cell and builds the proteins. Brings it where it needs to be. The sugar is ribose

Electrolytes

Salts in their ionic form. Substances that have the ability to transmit an electrical charge.

Most successful molecules are..

Self-replicating

Proteins (structure)

Shape determines its functions. Amino acids link to form peptide and polypeptide chains; proteins form primary, secondary, tertiary and quaternary structures. Made chiefly of carbon, oxygen, hydrogen, and nitrogen, though some proteins also contain sulfur, iron, or phosphorus. The amino acids make the protein unique and defines the functions of the protein.

Dipeptide; Tripeptide; Polypeptide; Protein

Short chain of two amino acids; Three amino acids linked together; Chain of 10 or more Exceeds 100 amino acids

Planetary model

Shows the protons and neutrons of the nucleus encircled by electrons, which orbit like planets around a sun. Clearer fashion, makes the atoms easy to understand the interactions.

Carbohydrates (types)

Simple and complex

Why is carbon an essential component of organic molecules?

Small in size, electrically neutral. Shares electrons with other atoms. Can form 4 covalent bonds. Can make up a hydrocarbon chain.

Functional group

Small relative to the entire molecule, is the reactive part of the molecule and determines the molecules chemical activity.

Molecule

Smallest unit of a compound that retains the properties of that compound.Forms when atoms joined together by chemical bonds. If two or more elements re joined together we call the result a molecule of the element.

Atom (parts)

Smallest unit of an element that retains the unique properties of the element; Proton, Neutron and Electron. In each storm there is the same # of protons and electrons

Mixtures (types)

Solution, Colloid and Suspension

Radioactive isotope

Spontaneously emits particles of energy at a constant rate and thereby changes into a stable non radioactive elements; Rate of decay. Measured in rock and is used to date fossils.

Structural protein (fibrous) (A)

Stable, rigid, water insoluble proteins that are used for adding strength to tissues or cells. Ex. Collagen, Fibrin and Keratin

How was the earth created?

Stardust; carbon blown off of slowly aging medium sized stars and condensed into minute dust particles.

Covalent bonds (types)

Strong chemical bond formed when atoms share electrons. Single, Double and Triple depends on the amount of electrons that are shared. Electrons spend more time near the electron acceptor rather then the electron donor.

Fibrous proteins

Such as collagen are long and firm, which allows them to be sued to add strength to tissues, ex. Connective tissue in ligaments and tendons.

Globular proteins

Such as immunoglobulins, also known as antibodies, have a specific shape, so they may join like a puzzle piece with a specific foreign protein that invades the body.

Organic Compounds (examples)

Tends to be large, complex molecules that contain carbon-carbon (C-C) covalent bonds or carbon-hydrogen (C-H) covalent bonds Proteins, carbohydrates, triglycerides and nucleic acids

Atomic weight

The # of neutrons and protons (+) together

Electron shell

The area around the nucleus where the electrons have their most likely position. The electron energy level determines which electron shell it will inhabit. The lowest the energy electron the closer to the nucleus.

ATP (process)

The bonds between the phosphate groups are called high-energy bonds. It is when these bonds are broken that energy is released from the ATP molecule. To use the energy stored in ATP, enzymes must move the terminal phosphate group to another molecule. The receiving molecule is then termed phosphorylated and temporarily has energy to do some work. During this process 44the ATP molecule loses a phosphate group and becomes adenosine diphosphate (ADP)

Precambrian Sea

The earliest evidence of life shown by calcified algal structures (stromatolites)

Coding (process)

The information needed to produce proteins is determined by the order of the nucleotides. Grouping of three nucleotides is the code for a specific amino acid. A gene is a sequence of nucleotides that carries the information to make one peptide chain. Long chains of genes are combined with protein to form chromosomes. Chromosomes replicate during cell division so that all daughter cells inherit an identical copy of the chromosomes from the parent cell.

Genes

The instructions that are coded in segments of the DNA

Chemical equation (parts)

The way in which the reaction is described in writing. Reactants (X and Y) Products (Z)

Chemical bonds (type)

The way that atoms join together to form a molecules is through a process. Atoms are sharing or transferring electrons between them. Covalent, ionic and Hydrogen.

Unsaturated fatty acid

There are some double bonds between the C and H atoms; Mainly plant origin, such as olive oil and corn oil.

RNA (ex.)

Three types of RNA: Transfer Messenger Ribosomal

Electrons (-)

Tiny "wavicles" that possess the properties of both waves and constant motion moving continuously around the nucleus. Most likely to be found in the region called electron clouds. Matter that cannot be divided by ordinary chemical processes into another substance

Early self replicating cells

Tiny, bacteria like units without a nucleus. Can use energy from the environment to make this own chemical energy.

Neutral/simple fats (structure/ex.)

Triglycerides: one glycerol molecule (backbone) and three fatty acid chains; fatty acid chains that ack double bonds are "saturated" while those with double bonds are "unsaturated" Ex. Saturated fatty acids are solid (fats) at room temperature and unsaturated fatty acids are liquid (oils) at room temperature; both are concentrated sources of energy

Water

Two H (+) and one O (-) Polar molecule, covalent bond. Can form hydrogen bonds with each other and other polar molecules.

DNA (structure)

Two parallel strands of nucleotides; each nucleotide is composed of: a phosphate group, a 2-deoxyribose sugar, and one nitrogenous base (ex. Cytosine, guanine, alanine, or uracil) strands are connected by H bonds. A - T G - C

Lipids (made of)

Used in the body for energy and re stored in fat for future energy needs. Chemical messengers in the form of some hormones; Made of C , H , and O (lower content) sometimes contains phosphorus.

Cholesterol (used for)

Used in the formation of bile salts, which aid in fat digestion. Used by adrenal glands, testes, and ovaries for creation of steroid hormones including cortisone, estrogen, progesterone and testosterone.

Fat-soluble vitamins (structure/ex.)

Variable molecular structure depending upon the specific vitamin; stored in liver and fat Vitamins A,D,E and K: stored in body fat; can be toxic if given in excess

Lock and key property of enzymes

Very specific to their reactions and substrates (substance being acted upon) Determined by the shape, charge and hydrophilic/hydrophobic properties.

Carbohydrates (ex./made of)

Water containing carbon Used in energy, storage of energy and cellular structures Cellulose, starch and table sugar. Composed of atoms of carbon, hydrogen and oxygen with hydrogen and oxygen in the same ratio as in water, two to one.

Hydrophobic

Water hating, molecules that do not mix well with water. Usually electrically neutral, no polar molecules such ass lipids. Gather together forming a droplet. No bond occurs.

Hydrolysis (ex)

Water is used in reactions to break down sucrose Sucrose is decomposed into its monosaccharide components, glucose and fructose. Decomposition reactions to release energy hold in bonds between atoms and to generate the simple molecular building blocks needed by the cell.

Hydrophilic

Water loving, chemicals that dissolve or mix well in water. Usually polar or ions.

High heat of vaporization

Water needs a fairly high temperature to change from liquid to a gas therefore it will remain in a liquid state through a wide range of temperatures.

Functional proteins (globular) (B)

Water soluble and have a flexible, 3D shape which can change under different circumstances. Changeable. Chemically active molecules. Ex. Hemoglobin, antibodies, protein based hormones and enzymes.

Universal solvent

Water. More chemicals can be dissolved in water than any other known solvent. - ends of water O surrounds + charged molecules. + ends of water H blanket - charged molecules.

The beginning..

Waves of hydrogen and energy, gravvity swirled the atoms crushing, igniting nuclear reactions (**)

Buffers (most common example)

Weak acids and bases act as buffer because they do not completely ionize in water. They buffer the solution where chemical reactions take place. pH is kept in a neutral range. Acids and bases are released in body as waste products and not allowed to accumulate; Carbonic acid (H2CO3) and bicarbonate. Carbonic acid ionizes, when placed in water, to free hydrogen ions and the weak base, bicarbonate (HCO3-)

The product of ionization

Weak base; a weak acid will initially ionize into free H+ ions, a weak base product and weak acid molecules. pH is not changed greatly because some of the chemical remains in acid form and some remains a weak base. strong base is added to the solution, the hydrogen ion will attach to the base and neutralize it, and the remains weak acid will ionize further.

Electrotatic attraction

When a two atoms are drawn to each other by their respective electrical charge; ionic bond.

Anion

When an atom gains an electron, It becomes negatively charged, has more electrons than protons.

Cation

When an atom loses an electron, It becomes positively charged, has more protons than electrons.

Ion

When an atom loses or gains an electron, it gives it a + or - charge. Each element has a naturally occurring specific number of neutrons

Full electron shell vs. not full

When it is complete it is chemically inactive or inert. When it is not complete the atoms are constantly trying to find electrons to complete their outer shell.

Lipid bilayer

When placed in water, hydrophilic heads form hydrogen bonds with the water and tails are repelled from the water and are most stable when abutting another tail.

Hydrolysis

When triglycerides are decomposed. Water molecules are consumed. Simple to reactions with carbohydrate synthesis and decomposition.

Disaccharide

When two monosaccharides are joined together the reaction is a synthesis reaction.

Ribosomal RNA

rRNA uses the information to create the proteins needed by the body.