Key Concepts
Chapter 1
1. Alchemy - a pseudo-science that has sought to transform base metals such as lead, gold, medieval science, which aimed to find a universal cure for the disease, and the magic potion of immortality
Second Biochemistry - the study of chemicals extracted from plants and animals
3. Chemical science, which studies the composition and properties of matter
4th Experiences - a scientific approach to data collection and record observations in a controlled
5th Hypothesis - A tentative proposal for a scientific principle that attempts to explain the importance of a data set collected in an experiment
6th Inorganic Chemistry - the study of chemicals that do not contain carbon
7. Natural law - a proposal widely tested in a scientific principle that states a measurable relationship under different experimental conditions
8th Organic Chemistry - the study of chemicals that contain carbon
9. The scientific method - the method approach to explore the natural and logical explanations for the results
10th Theory - a proposal widely tested in a scientific principle that explains the behavior in the wild
Chapter 2
First centimeters or meters - a common metric unit of length
2. gram or a kilogram - a common metric units of mass
3. milliliters or liters - A unit of measurement of volume
4. mass - the amount of the target, was measured in the balance
5. Weight - The force of gravitational attraction between an object and the planet is measured.
Sixth significant digits - the digits of a measurement known with certainty, plus a number that is estimated.
7. scientific notation - a method to express very large or small by placing the comma after the first significant digit, and adjusting the size with a power of 10.
8th percentage - The ratio (times 100) of a single volume with respect to all volumes in a group and parts per hundred.
9. instrument - a recording of a measure such as length, mass or volume
10. measure - a numeric value and unit expressing a physical quantity such as length, mass or volume
11. nonsignificant digits - the numbers to an extent that exceeds the accuracy of the instrument
12. uncertainty - the degree of inaccuracy in measurement instruments
13. Method unit of analysis - a systematic procedure to solve the problems that some procereds response units conversion value reated
14. factor unit - a ration of two quantities that are equivalent and can be applied to convert from one unit to another, for example, an inch foot/12
Chapter 3
1. calories - the amount of heat required to Reais 1 gram of water 1 ° C
2. Celsius (° C) - the basic unit of temperature in the metric system
3. Density - the amount of mass in a unit volume
4. Degrees Fahrenheit (OF) - The basic unit of the temperature of the English system
5. Heat - A measure of the total energy in a system
6th International System (SI) - a comprehensive system of measurement for the seven basic units
7. Joule - a unit of energy is the SI system
8th unit Kelvin (K) - - the basic unit of temperature in the SI
9. metric - a decimal system of measurement with the basic units
10. seconds - - the basic unit of time in the metric system
11. specific gravity (sp gr) - the relationship between the density of a liquid compared to the density of water at 4 ° C
12. specific heat - the heat required to raise 1 g of substance 1 º C
13. Temperature - A measure of the average energy in a system, the average kinetic energy of molecules in motion
14. volume on the go - a technique for determining the volume of water displaced
15. absolute zero - the theoretical temperature at which the kinetic energy of a gas is equal to zero.
Chapter 4
1. League - a homogeneous mixture of two or more metals
2. Atomic number - a number that identifies a certain part of
3. chemical changes - changes in materials, which change the chemical composition of
4. chemical symbol - an abbreviation of the name of an element
5. compound - a substance that can be decomposed into simpler substances
6. deposit - a change of state of a gas derict a solid
7th ductile - belongs to a metal, which can be drawn into a wire
8th element - a substance that can not be decomposed by chemical reaction
Ninth law of conservation of energy - the law states that energy can not be created or destroyed
10th Law of conservation of mass and energy - the law is called the total mass and energy are constantly
11. malleable - the property of a metal that can be machined in one piece
12. Periodic Table - a table that organizes the elements according to their properties
13. physical changes - a feature that can not be obse4rved change the formula of the substance
14. The potential energy (PE) - energy stored in the field due to hold its position or composition of the
15. pure substance - issues with a clear composition and properties of Constance, for example, and the element or compound
16th fitness - Designates the status of a substance existing in solid, liquid or gas.
17th sublimation - direct change of state from a solid to a gas without forming a liquid
18. molecule - The smallest particle that represents a compound
19. The kinetic energy - the energy associated with the movement of molecules.
20. homogeneous material - the material to the standard configuration, a feature consistent and clear
21st element - a pure substance that can not be divided again by ordinary chemical reaction
22. compound - a pure substance that can be decomposed into two or more simpler substances by chemical reaction
23. heterogeneous mixture - Material that has a variable composition and properties of materials indeterminate consists of two or more substances which may be separated physically.
24. homogeneous mixture - issues associated with a variable composition, but a characteristic clear and consistent, are examples of natural gas, gasoline, and bronze.
25th atom - The smallest particle that represents an element
26th chemical formula - a symbolic representation of a complex indicates the number of atoms of each element
27. metal - an element that is usually shiny in appearance, has a high density and high melting point, and is a good conductor of heat and electricity
28. Non-metallic - an element that is usually boring in appearance, has a low density and low melting point, and is not a good conductor of heat and electricity
29. semimetal or metalloid - An element that is usually metal, as in the appearance and properties that are between a metal and nonmetallic.
30th law of constant composition or final - the principle that a compound that still contains the same elements in the same proportion by mass
31. Physical feature - a feature that can be detected without changing the chemical formula of the substance.
Chapter 5
1. atomic mass unit - a unit of mass equal to exactly 1.12 the mass of an atom of C-12
2. atomic notation - a symbolic method to express the composition of an atomic nucleus
3. electronic assembly - fast arrangement of electrons in the description of the authors' of the sublevels of the growing energy needs
4. spectrum of emission lines - a collection of narrow bands of light produced by the atoms of a particular element, releasing energy
5. sublevel energy - energy of electrons division level because of my energy level
Sixth orbital - a region around the nucleus, where it is very likely to find and electrons with a given energy
7. photon - a partical of radiant energy
8th quantum atom - a sophisticated model of the atom that describes the energy of an electron according to its probability of being found in a particular location around the nucleus
9. uncertainty principle - a statement that it is impossible to accurately measure the location and energy of a particle at the same time
10th Electron - A subatomic particle that has a negligible mass and charge of a relative minus
11. protons - subatomic particle with a mass of about 1 AMU and the equivalent for more than one
12. Neutron - a neutral particle in an atom, whose mass is about 1 amu
13. atomic nucleus - a region of high density in the center of the atom
14. Atomic number - number of the feature that indicates the number of protons in the heart of one of its atoms
15th lot of numbers - A number representing the total number of protons and neutrons in the nucleus of an atom
16. isotopes - atoms that have the same atomic number but different mass numbers. Atoms of the same element that have different numbers of neutrons in the nucleus.
17. Atomic mass - mass weighted average of the natural isotopes of the element.
18. Bohr atom - the atomic model of the images of the electron around the nucleus of specific orbital energy.
Chapter 6
1.
2. alkali metals - Group IA elements / 1, hydrogen is not
3. alkaline earth metals - Group II / 2 elements
4. Halogen - The Group of elements VIIA/17
5. noble gases - Group elements VIIIA/18
6. Group - A vertical column of the periodic table, a family of elements with similar properties.
7. period - a horizontal line on the periodic table, a series of elements with properties ranging from non-metallic metal.
8. Representative Elements - Group A elements (1,2,13-18) in the periodic table, also called main group elements.
9. transition elements - Group B (3-12) of the periodic table of elements.
10. Valence electrons - electrons that take the outermost atomic and sub sp, which are involved in chemical reactions
11. electrons points formula - a representation of an atom and its valence electrons, which shows the chemical symbol surrounded by a dot for each valence electron.
12th Ion - An atom that carries a charge due to gain or lose valence electrons
13. ionization energy - the amount of energy needed to remove the electron-neutral atom in a gaseous state
14. isoelectronic - refers to two or more of the ions with the same electronic configuration, for example, O2 and Mg 2 + each have 10 electrons, and their electron configurations are the same as the noble gas neon.
15th inner transition elements - the elements of the lanthanide series and actinide
16. lanthanide series - elements with atomic number 58-71
17. series actinides - elements with atomic number 90-103
Chapter 7
1. organic compound - any compound containing the element carbon.
2. inorganic compound - a compound does not contain the element carbon.
3. tion - a positively charged ion.
4. anion - a negatively charged ion.
5. formula units - the smallest particle of representative ionic compound.
6th aqueous solution - a substance dissolved in water
7. Binary acid - a slurry containing hydrogen and a nonmetal
8. ionic binary compound - a compound containing two nonmetals
9th IUPAC - the international system of rules for naming chemical compounds
10th Latin system - a system that means the tax on a cation with the suffix-ic or-UO
11. molecule - the only particle that represents a composite of non-metal atoms
12. monatomic ion - an atom that has a positive or negative charge
13. oxyanion - polyatomic anion that contains one or more elements combined with oxygen
14. polyatomic ion - a group of atoms bonded together with a positive or negative global charge
15th System images - a system that means the tax on a cation with Roman numerals
16. ionic ternary compound - a compound that contains three elements, including at least one metal
17. ternary oxyacid - combined with water, which contains hydrogen, nonmetal, and oxygen
Chapter 8
1. acid - hydrogen-containing compound that releases ions (H +) when dissolved in water.
Second base - A substance that releases hydroxide containing hydroxide ions (OH-) when dissolved in water.
3. an aqueous solution - a substance dissolved in water
4th chemical reaction - the process of undergoing a chemical change.
5. chemical equation - shorthand representation of formulas and symbols to describe the chemical changes.
6th reactive - A substance that undergoes chemical transformation.
7th product - a substance caused by a chemical change.
8. Catalyst - A substance that speeds up a reaction, but can be recovered without being changed forever.
9. exothermic reaction - a reaction that develops thermal energy.
10th endothermic reaction - a reaction that absorbs heat energy.
11. series of activities - a relative order of elements arranged by their ability to undergo reactions, also called electromotive series.
12. precipitate - an insoluble substance in the solution produced by a reaction.
13. combination of reaction - a reaction, in which the two substances produce a single compound.
14. decomposition reaction - a reaction in which two or more substances are produced from a single compound.
15th single replacement reaction - a reaction where a more active element displaces a less active for a solution or compound.
16. double displacement reaction - a reaction in which two different cations in ion exchange.
17. neutralization reaction - reaction of an acid and a base produces water and salt.
18th Salt - An ionic substance produced by an acid-base reaction, an ionic compound that does not contain hydroxide ions.
19. redox reaction - A chemical reaction in which electron transfer takes place.
20. coefficient - a figure in front of a chemical reaction that helps to balance a chemical equation
21. Index - a number in a chemical formula that represents the number of atoms or ions that appear on the substance
22. diatomic molecule - a particle composed of two nonmetal atoms
Chapter 9
1. Avogadro's Number (N) - the number of atoms, molecules or formula units, which form one mole of a substance, 6.02 x 1023 individual units.
2nd Mole - The amount of substance containing the same number of units as there are atoms in exactly 12 g of carbon-12.
Third molar mass - mass of a mole pure substance in grams, the mass of Avogadro's number of atoms, molecules or formula units.
4. empirical formula - The chemical formula of a compound that expresses the relationship simplest of atoms in a molecule or ion in a formula unit.
5th Molecular Formula - The chemical formula of a compound that expresses the actual number of atoms in a molecule.
6. molar volume - the volume of one mole of gas at standard temperature and pressure.
7. standard temperature and pressure or STP - A temperature of 0 ° C and atmospheric pressure arbitrarily chosen standard conditions
8. Avogadro's law - equal volumes of gas under the same conditions of temperature and pressure contain the same number of molecules.
9. gas density - the ratio of the mass per unit volume ofr a gas, in grams per liter
10th percentage composition - a list of the percentage mass of each element in a compound
Chapter 11
1. atmospheric pressure - The pressure exerted by gas molecules in the air at sea level this pressure is compatible with a column of 760 mm of mercury.
2. Barometric pressure - the pressure can be measured in the atmosphere.
3rd Torr - A unit of pressure equal to 1 mm Hg
4th vapor pressure - The pressure exerted by the molecules in gaseous form in dynamic equilibrium with the same type of molecules in a liquid state, for example, the water molecules of liquid water.
5. Boiling point - temperature at which the vapor pressure of the fluid is the same pressure.
6. Dalton is the partial pressure - pressure in the gas mixture is equal to the sum of the pressures exerted by each gas mixture.
7. partial pressure - The pressure exerted by a gas in a mixture of two or more gases.
8. vacuum - the volume, which contains none of the gas molecules.
9. Boyle's law - air temperature, pressure and volume of the gas are inversely proportional.
10. Avogadro's law - equal volumes of gas under the same conditions of temperature and pressure contain the same number of molecules.
11. standard temperature and pressure or STP - A temperature of 0 ° C and atmospheric pressure arbitrarily chosen standard conditions
12. Charles Law '- a constant temperature pressure, volume and Kelvin gas directly proportional.
13. ideal gas - a hypothetical gas that obeys the kinetic theory of perfect.
14. absolute zero - a temperature where the kinetic theory of gases is equal to zero.
15th ideal gas law - relationship PV = nRT for an ideal gas.
16. Combined Law - an indication that the pressure and the Kelvin temperature are directly proportional to the gas at constant pressure
17th Dalton law of partial pressure - a declaration that the pressure from a gas mixture is equal to the sum of the pressure of each gas
18. gas pressure - the pressure exerted by the molecules in the air
19. real gas - a real gas deviates from ideal behavior, which, under certain conditions
20. ideal gas constant - A constant principle of proportionality, the equation PV = nRT
Chapter 12
1. monatomic ion - a single atom, which is a positive or negative charge
2nd diatomic molecule - a particle that consists of two non-metal atoms
3. Valence electrons - electrons in atoms outer shell of energy that are available for bonding.
4th ionic bond - A chemical bond characterized by the attraction of a cation and an anion.
5. Covalent bond - a chemical bond characterized by sharing one or more pairs of valence electrons.
6. formula unit - the smallest body representative of a compound are held together by ionic bonds.
7th molecule - The smallest unit representing a compound held together by covalent bonds.
8th bonding electrons - the valence electrons in a molecule that is shared.
Nonbonding electrons 9th - the valence electrons in a molecule that is not shared.
10th Electron points formula - (.) A diagram of a molecule or polyatomic ion, where each atom is represented by its chemical symbol for each surrounded by a bonding or nonbonding electron, also called a Lewis structure.
11th structural formula - A diagram of a molecule of polyatomic ions, where each atom is represented by its chemical symbol associated with one row for each pair of bonding electrons.
12th Single Bond - A link consists of an electron appears as a unique link between them.
13. double bond - A bond consisting of two pairs of electrons showed that the two dashes between two atoms.
14th Triple Bond - A bond that consists of three pairs of electrons are represented by three lines between two atoms.
15. Electronegativity - the ability to split an atom to attract electrons in a pair of chemical bonding.
16th nonpolar covalent bond - A bond in which one or more pairs of electrons are shared equally.
17th Polar covalent bond - A bond in which one or more pairs of electrons are shared unequally.
18. Binding energy - the amount of energy needed to break the covalent bond two atoms
19. Bond length - distance from the nuclei of two atoms joined the covalent bond
20th chemical bond - the generic title of the attraction between two ions, or two atoms
21. molecular form - the geometric shape formed by atoms to the central atom in a molecule
22. Electron pair geometry - the geometric shape formed by the union and non-bonding electron pairs on the central atom of a molecule
23. VSEPR Theory - a model that explains the shapes of molecules as a result of the pairs of electrons on the central atom repel each other
24th octet rule - the claim that an atom tends to bind to acquire eight valence electrons
25. Delta notation - a method to indicate a partial negative charge and positive part in a chemical bond
26. polyatomic ions - a group of atoms bound together, and in general positive or negative charge
Chapter 13
1. vapor pressure - the pressure of gas molecules in a dynamic equilibrium of the same type of molecules in the liquid state, for example, water molecules in liquid water.
2. Viscosity - resistance of the fluid flow as a result of molecular attraction.
3. surface pressure - molecular attraction, which causes the liquid has a minimum area.
4. dispersion of forces - attraction of molecules based on the temporary dipoles of the molecules, also called London forces.
Fifth hydrogen bond - a bond that intermolecular between hydrogen and oxygen in both molecules have a polar group-OH.
6. heat of fusion - The heat required to convert a solid to a liquid at its melting point.
7. heat of vaporization - The heat required to convert a liquid into a gas at its boiling point.
8th hydrate - A substance that contains a number of water molecules per unit formula of a crystalline substance.
9. Anhydrous - means a compound that contains no water.
10. hard water - water that contains a variety of anions and cations such as Ca2 +, Mg2 +, Fe3 +, CO32-, SO42-, PO43.
11. Boiling point - temperature at which the vapor pressure of the fluid is the same pressure
12. demineralized water - water purified by the removal of ions by an ion exchange method, also called demineralized water
13th dipole force - an intermolecular attraction based on the permanent dipoles
14th electrolysis - the chemical reaction produced by an electric current through an aqueous solution
15. heavy water - water molecule, with hydrogen atoms has been replaced by a hydrogen atom with a neutron
16. metal oxide - a compound that reacts with water to form a solution, also called oxide-based
17. net dipole - the general direction of a partial negative charge is a molecule with two or more dipoles
18. non-metallic oxide - a compound that reacts with water to form an acid solution, also known as acid oxide
19. freshwater - water contains sodium ions and anions other than
Chapter 14
1. net dipole - the general direction of a partial negative charge is a molecule with two or more dipoles
Second solution - a component that is dissolved in a solvent to form a solution.
3. solvent - in the solution, part of the largest concentrations occur, usually in a liquid in which the solute dissolves.
Fourth solution - a homogeneous mixture at the atomic scale, molecular and / or ion consisting of a solute (or solutes) dissolved in a solvent.
5. Henry's Law - the principle that the solubility of a gas in a liquid is proportional to the partial pressure of gas above the liquid.
6. miscible - refers to two liquids that are soluble in one another.
7. immiscible - refers to two liquids that are insoluble in the other, and if mixed, separated into two layers.
8. a saturated solution - A solution in which the dissolved and undissolved solute are in dynamic equilibrium. A solution containing solute as much as possible to a specific temperature.
9. supersaturated solution - a solution unstable, which contains more than the solvent-impregnated at the same temperature.
10th dipole - a region of a polar molecule with a partial negative charge and partially positive
11th that dissolves as a rule - the principle that the solubility is greater when the polarity of the solute is similar to that of the solvent
12th non-polar solvents - a solvent which is composed of nonpolar molecules
13. polar solvent - a liquid compound polar solvent molecules
14. Solubility - the maximum amount of solute that can dissolve in a solvent at a given temperature
15. solvent cage - a group of solvent molecules around a solute particle in a solution
16. Unsaturated solution - a solution that contains less than the maximum amount of solute that can dissolve at a given temperature
Chapter 15
1. acid-base indicator - a chemical that changes color depending on the pH of the solution.
2. Arrhenius acid - a substance that provides hydrogen ions dissolved in water.
Arrhenius third base - A substance that allows hydroxide ions when dissolved in water.
4. hydronium ion H3O + or - ion that best represents the hydrogen ion in aqueous solution.
5. dissociation - an ionic compound dissolves in water and separated into positive and negative ions, for example, NaOH is dissolved in water, so that sodium ions and hydroxide ions.
6. amphiprotic - a substance that can accept or donate a proton in an acid-base
7. The Brønsted-Lowry acid - a substance that gives a proton in an acid-base
8th Bronsted-Lowry Base - a substance that accepts a proton in an acid-base reaction
9. buffer - a solution that resists changes in pH when acid or base is added
10th test - the scene in a titration when the indicator changes color
11th ionization constant of water (KW) - a constant that is equal to the molar hydrogen ion concentration and the molar concentration of hydroxide ions
12. Net ionic equation - the equation representing the chemical reaction in the viewer after the ion-ion have been deleted
13. pH - hydrogen ion concentration expressed on a scale molecular exponential
14th proton acceptor - a term used interchangeably with the acceptor of hydrogen ions
15th proton donor - a term used interchangeably with the donor hydrogen-ion
16. salt - a product derived from the neutralization reaction, in addition to water
17th spectator ions - ions that are dissolved in water, but does not appear in the net ionic equations
18th standard solution - a solution whose concentration was determined accurately
19th strong electrolyte - an aqueous solution, it is a good conductor of electricity
20. weak electrolytes - aqueous solution, which is a poor conductor of electricity
21st assay - a procedure to deliver a measured amount of solution through a burette
22nd Total ionic equation - an equation that represents the chemical substances highly ionized ionic form and slightly ionized substances in ionic form,
Chapter 16
1. reversible reaction - a reaction that moves forward and to the products as well as in the opposite direction towards the reaction.
Second balance - a dynamic state of a reversible reaction, where the rate of reaction front and rear are equal.
Third solid electrolytes - An aqueous solution containing a substance that implements strong electric current, for example, strong acids, strong alkalis, soluble salts.
4th weak electrolyte - An aqueous solution containing a substance that causes an electric current easily, for example, weak acids, weak alkalis, easily soluble salts.
5. exothermic reaction - a reaction that evolves heat energy.
6. endothermic reaction - a reaction that absorbs heat energy.
7th Catalyst - a substance that gives a reaction go faster by lowering the activation energy.
8. Heat of reaction - the energy difference between reactants and products
9. reaction rate - the rate at which the concentrations decrease in response per unit of time
Chapter 17
First Oxidation - A chemical change in which a substance loses electrons or an increase in oxidation number occurs.
Second oxidation number - a value assigned to an atom in a molecule or ion to keep track of electrons gained or lost value can be positive or negative and is zero in the free form.
3. Reduction - A chemical change in which electrons substances increase or a decrease in oxidation number.
4th oxidant - essentially reduced to a redox reaction.
5. reducing agent - the substance is oxidized in a redox reaction.
6. electrochemical cell - a generic term for devices that contain two different solutions in different sectors of the electrodes connected to run the wire.
7. Anode - The electrode in an electrochemical cell where oxidation occurs.
8. cathode - electrode electrochemical cell, where the reduction takes place.
9. photovoltaic cells or batteries - A general term for any electrochemical cell which produces electricity spontaneously.
10th redox reaction - a chemical reaction in which electron transfer takes place
11. electrochemistry - the study of the interconversion of chemical and electrical energy
12th electrolysis - it supplies electricity to a redox process nonspontaneous to provoke a reaction
Chapter 18
1. activity - the number of radioactive nuclei during the break in tha sample pieces to give time, for example, 500 dpm
2. alpha particles - nuclear radiation identical to helium-4 nuclear
Third atomic number (Z)-value indicating the number of protons in a nucleus
4. Beta particles - radioactive radiation, identical to that of the electron
5. chain reaction - nuclear fission reaction in which neutrons released to initiate a second reaction, which in turn, starts the third reaction, and so on
6. a critical mass - the minimum mass of fissile nuclide necessary to maintain a reaction chiain
7. Deuterium - hydrogen nuclide is a neutron
8. electron capture (EC) - a nuclear reaction in which a large nuclide is based on its inner core electrons in the nucleus
9th gamma rays - a nuclear radiation, similar to the light of high energy
10. The half-life - the amount of time required for 50% of the radioactive nuclei in a sample of corruption
11. mass number - the value indicating the number of protons and neutrons in a nucleus
12. the nuclear equation - with shorthand representation of the atomic notation to describe the nuclear reaction
13th Nuclear fission - a nuclear reaction in which a nucleus divides into two or more lighter nuclei
14. nuclear fusion - the nuclear reaction in which two light nuclei combine into a single core
15. nuclear reaction - a change that involves high-energy core
16. nuclide - the atom, which has a number of protons and neutrons
17. positrons - Identical to nuclear radiation byt the same opposite to the electron
18. Radiation - emission of particles or nuclear energy in an unstable
19th Transmutation - the conversion of one element to another by a nuclear reaction
20. tritium - the nuclide of hydrogen with two neutrons
Chapter 19
First hydrocarbon - an organic compound containing hydrogen and carbon.
Second alkane or saturated hydrocarbons - a hydrocarbon that contains only a single bond.
3rd unsaturated hydrocarbon - a hydrocarbon containing a double or triple bond.
4th aromatic hydrocarbons - a hydrocarbon containing a benzene ring.
Fifth structural formula - a chemical formula that shows the actual arrangement of atoms in a molecule.
6. Structural isomers - compounds with the same molecular formula but different structural formula.
7. combustion reaction - a chemical reaction with the hydrocarbon burns and is oxidized into carbon dioxide and water.
8th Polymer - A high molecular compound is composed of small repeating chemical units.
9. monomer - The chemical repeating unit in a compound of high molecular weight.
10th Polyester - A type of polymer formed by the reaction of a dicarboxylic acid and a dihydric alcohol.
11th polyamide - A type of polymer formed by the reaction of a dicarboxylic acid and diamine.
12th alkenes - a family of compounds consisting of unsaturated hydrocarbons containing a double bond
13th alkynes - a family of compounds consisting of unsaturated hydrocarbons having a triple bond
14th functional group - a family of drugs, where all members have the same structural characteristics
Chapter 20
1. Biochemistry - The study of biological compounds and their reactions.
2. polypeptide - a polymer of amino acids combined with organic amide.
3. amino acids - a biological compound contains both amino and carboxylic acid.
4. Peptide bond - amide link, which connects two amino acids.
Fifth enzyme - a biological compound that catalyzes a specific biochemical reaction.
6. carbohydrates - a biological compound, which is a polyhydroxy aldehyde or ketone.
7. monosaccharide - simple sugars such as glucose or fructose.
8th Lipid - A biological agent which is insoluble in water, such as a grease or oil.
9th fatty acids - a carboxylic acid with a long hydrocarbon chain.
10. fat - a lipid that consists mainly of saturated fats and fatty acids esterified to glycerol.
11th Oil - A lipid consisting mainly of unsaturated fatty acids esterified to glycerol.
12. nucleic acid - a polymer containing biological genetic information.
13. protein - a biological compound which is a polymer of amino acids
