Introduction to Inorganic Chemistry
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andrewsimerson on December 15, 2011
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141 terms
Terms | Definitions |
|---|---|
 matter | that which has mass and occupies space |
| atom | the smallest part of an element having the chemical properties of the element |
| element | a substance that cannot be broken down into simpler substances by ordinary chemical means |
| mole concept | a method that allows the relative number of reactant particles involved in a chemical reaction to be known one mole of any substance will contain approximately 6.02x10 to the 23 power particles (avogadro's number) |
| chemical symbols | capitalized first letter of the english or latin name of the element or a single letter or a 2 letter representation for the element |
| molecule | a unit in which the atoms of two or more elements are held together by chemical bonds |
| compound | a substance that is characterized by constant composition and that can be chemically broken down into elements |
| charge | electricity due to the build-up of one of two kinds of electrical charges, either positive or negative |
| chemical formula | a combination of symbols of various elements that make up a compound |
| chemical reaction | a process in which one substance is changed into another |
| properties | characteristics of matter which are classified as chemical or physical |
| chemical properties | a property that causes a substance to change into a new substance |
| physical properties | properties such as color, height, or weight that do not involve a change in the chemical identity of the matter |
| solids | have a definite shape and a definite volume, which is independent of changes in temperature and pressure |
| liquids | have no definite shape but have definite volume, which is independent of changes in temperature and pressure. designated by (l) or (aq) |
| gases | have neither a definite shape nor volume and are made of widely separated particles properties are dependent on changes in temperature and pressure designated by (g) |
| melting point | the temperature at which a solid begins to change into a liquid |
| boiling point | the temperature at which the pressure of the vapor escaping from the liquid equals the atmospheric pressure (760mm Hg or mercury) |
| density | the amount of mass per unit volume of a substance it is the ratio of mass (M) to volume (V) |
| specific gravity | the ratio of the density of that substance to the density of a substance used as a reference standard at the same temperature |
| solubility | the amount of a substance that will dissolve in a specific volume of solvent at a given temperature |
| concentration | the amount of a specified substance in a unit amount of another substance |
| physical quantity | a property of matter to which we can assign both a numeric value and a unit of measurement |
| mass | the quantity of matter that an object contains expressed in grams (g) |
| volume | the size, measure, or amount of an object in three dimentions expressed in liters (L) |
| length | the distance between two points expressed in meters (m) |
| energy | the ability to do work mechanical, chemical, electrical, heat, nuclear, light |
| temperature | a physical property of a system related to thermodynamics celsius (C) fahrenheit (F) Kelvin (K) |
| kelvin | (K) measures extreme hot or cold |
| classifications of matter | pure substance mixtures |
| pure substance | a substance that has only one component |
| mixtures | combination of two or more pure substances in which each substance retains its own identity may be either homogeneous or heterogeneous |
| homogeneous | consists of only one phase uniform mixture (the same throughout) example: air, soft drink, ocean water |
| heterogeneous | consist of more than one phase having visible differing parts example: chocolate chip cookies, salt and pepper, and oil in water |
| conclusions of Bohr | proposed a planetary model of the atom |
| modern theory | electrons do not move in simple orbits, like the planetary model suggested |
| nuclear structure of an atom (nucleus) | protons-positive charge +1 neutrons-neutral charge |
| atomic number | the positive charge on its atomic nuclei, or total number of protons in an atom defines each element |
| mass number | the total number of protons and neutrons contained in the nucleus of an atom |
| atomic weight | the average mass of the atoms of various forms (isotopes) of an element, as they occur naturally |
| outer structure of an atom | electrons energy levels orbitals |
| electrons | determine the chemical behavior of atoms charge is negative one (-1) mass is 1/1832 atomic mass unit (amu) symbol is e or e- electrical neutrality (protons equal to electrons) electron configuration (arrangement of electrons) |
| energy levels | regions around a nucleus where electrons may be found |
| orbital's | specific regions within energy levels where electrons are found |
| atomic structure and light-electron states | ground state excited state relaxation electronic transitions electromagnetic radiation |
| ground state | the lowest possible energy condition of an electron |
| excited state | when an electron absorbs energy, it travels from a lower energy level to a higher level |
| relaxation | the release of energy by an atom resulting from electrons falling back into lower energy levels |
| electronic transitions | the promotion and relaxation of electrons |
| electromagnetic radiation | energy released by atoms traveling as waves that can be broken into characteristic bands called wavelengths |
| isotopes | atoms of the same element having different masses because they contain different numbers of neutrons |
| isotope notation | the representation of a specific isotope the atomic number is listed below the symbol, the mass number above |
| stable isotopes | atoms which do not breakdown spontaneously |
| unstable isotopes | radioactive isotopes, either natural or artificially created having an unstable nucleus that decays, emitting alpha, beta or gamma rays |
| purpose of the periodic table | provides specific information about each element organizes the elements according to physical and chemical properties |
| general format of the periodic table | periods-7 horizontal rows groups (families)-vertical columns metals-substance whose atoms tend to lose electrons during chemical reactions. left side of the heavy staircase nonmetals-found on the right-hand side of the heavy staircase transition elements (heavy metals)-have incomplete inner shells |
| important groups of elements | alkali metals-group IA, do not occur as free elements alkaline earth metals-group IIA, less reactive transitional metals-group IB-VIIIB, conduct heat and electricity halogens-group VIIA, extremely reactive noble gases-inert gases-group VIIIA, completely unreactive |
| symbols | a shorthand way to write the name of an element |
| atomic number | usually located at the top portion of an element box on the periodic table |
| atomic weight | usually located in the bottom of an element box of the periodic table |
| chemical bonds | the electrical force of attraction between combining elements |
| valence | the combining capacity of an element |
| valence electrons | electrons in the outermost shell which are involved or have the potential to be involved in the bonding process |
| octet rule | atoms try to attain the valence of their nearest noble gas neighbor elements will gain, lose or share the minimum number of electrons necessary to have 8 electrons in their outermost shell |
| ions | positively or negatively charged atoms or groups of atoms |
| cations | positively charged ions |
| anions | negatively charged ions |
| complex ions | ions composed of two or more covalently bonded atoms (radicals, polyatomic ions) |
| covalence | valence resulting from the sharing of electrons |
| electronegativity | the relative tendency of an atom to gain an electron |
| ionic bonds | involves a transfer of one or more electrons from one atom to another, leading to the formation of an ionic bond |
| covalent bonds | involves a sharing of electrons resulting in the covalent bond |
| polar covalent bonds | when a covalent bond is formed between atoms of different electronegativities, the share pair of electrons stays closer to the more electronegative atom, and the resulting bond is polar |
| nomenclature | the assignment of a correct and unambiguous name to each and every chemical compound |
| chemical formulas | a chemical formula represents a molecule of a substance and is made up of the symbols of the elements of which it is composed |
| ionic compounds | metals and nonmetals react to produce these compounds resulting from the transfer of one or more eleectrons |
| subscripts | a number placed below and to the right of the symbol |
| parentheses | used, along with the subscript, to indicate the number of complex ions present in a molecule |
| coefficients | used to indicate the number of molecules |
| steps in formula writing (metal to non-metal) | determine the proper symbol and valence of each element place the positive element (cation) first and the negative last (anion) balance the valences using subscripts by crossing over |
| formula writing examples | aluminum fluoride-starting with the cation we can predict that aluminum has three valence electrons by looking it up on the chart of common elements the anion fluorine is in group VII, it has 7 valence electrons, a -1 charge, it is necessary to multiply -1 x 3 to result in a zero charge answer = AIF3 |
| ionic compound | contain two different elements (usually a metal and a nonmetal) |
| stock system (official system) | roman numerals placed in parentheses after the name of the metal are used to indicate its variable charge or oxidation state |
| compounds containing two nonmetals | the chemical bond that exists between two nonmetal elements is predominantly covalent the most electropositive element is named first |
| oxygen containing radicals (complex ions and polyatomic ions) | oxygen containing ions with varying amounts of oxygen less oxygen-"ite" more oxygen-"ate" |
| chemical equation | a qualitative and quantitative expression of the reacting substances and their products in a chemical reaction |
| reactants | substances resulting from a chemical reaction |
| products | substances resulting from a chemical reaction |
| equilibrium | when the rate of the forward reaction and the rate of the reverse reaction of a reversible reaction are equal, the reaction is said to have reached equilibrium |
| law of conservation of mass | matter cannot be either gained or lost in a chemical reaction the total mass of the products must equal the total mass of the reactants |
| reactants | written to the left of the reaction arrow |
| products | written to the right of the reaction arrow |
| basic symbols | plus sign (+) combines reactants or products arrow (yield) shows direction of the reaction single (---------->) reaction goes to completion generating products double (======>) reversible reaction (equilibrium) heat may be required to start a chemical reaction and may also be the product of a chemical reaction the symbol used to represent heat is a small triangle |
| example of chemical equation | sodium hydroxide reacts with hydrochloric acid to yield sodium chloride and water NaOh + HCl ----------> NaCl + H2O |
| potential energy (chemical bonds) | energy a system possesses by virtue of its position, condition, or composition |
| kinetic energy (motion) | energy a system possess by virtue of its motion |
| molecular collisions | are usually necessary for chemical reactions to occur |
| activation energy | energy which two molecules must have to take part in a chemical reaction |
| catalysts | a substance that changes the rate of a reaction by lowering the activation energy without being permanently changed itself |
| exothermic reactions | reactions that liberate (release) energy |
| endothermic reactions | reactions that absorb energy |
| complete chemical reaction | irreversible |
| incomplete chemical reaction | reversible |
| concentration | rate or speed of a chemical reaction is proportional to the molecular concentration of each of the reacting substances |
| equilibrium constant | ratio at equilibrium that is reached in a system when the conversion of reactants into products and the conversion of products back to reactants is the same |
| balancing chemical equations | the relative number of moles of each product and reactant is indicated by placing a whole number coefficient before the formula of each substance in the chemical equation the coefficient 1 is assumed when a numbered coefficient is absent the equation, as written, is not balanced we cannot alter any chemical substance in the process of balancing the equation we can only introduce coefficients into the equation we must never change subscripts |
| steps to a method for balancing chemical equations | step 1 count the number of atoms of each element on both the product and reactant side step 2 determine which elements are not balanced step 3 balance one element at ta time using coefficients try to balance hydrogen last step 4 check to be certain that the total mass of the products is equal to the total mass of the reactants |
| five major factors that influence the rate of a reaction | 1 structure of the reacting species 2 concentration of the reactants 3 temperature of the reactants 4 physical state of the reactants 5 presence of a catalyst |
| types of chemical reactions | oxidation-reduction electrochemical reactions combination reactions decomposition reactions replacement reactions neutralization |
| oxidation-reduction | transfer of negative charge (one or more electrons) from one reactant to another |
| oxidation | loss of electrons addition of oxygen removal of hydrogen |
| reduction | gain of electrons removal of oxygen addition of hydrogen |
| combustion | (rapid oxidation) oxidation accompanied by noticeable light and heat |
| slow oxidation | oxidation not accompanied by noticeable light and heat |
| oxidizing agents | a substance that gains electrons from another, causing the latter to be oxidized |
| reducing agents | a substance that gives up electrons to some other substance, causing the latter to be reduced |
| electrochemical reactions | deals with those chemical changes either produced by electric current or with the production of electric current |
| combination reactions | involve the direct union or combination of two substances producing one new substance |
| decomposition reactions | reactions of a single substance being decomposed or broken down into two or more different substances |
| replacement reactions | single replacement-a reaction in which one atom or complex ions replaces another in a compound, producing a new compound double replacement-a reaction in which two compounds react with each other and exchange atoms |
| neutralization | acid/base reaction |
| classical acid (arrhenius) | a hydrogen containing substance that dissociates to produce hydrogen ions only in aqueous solution |
| bronsted-lowery (proton donor) | a compound that donates a hydrogen ion, or proton, to another compound in a specific reaction is an acid |
| since water accepted the proton (H+ ion) | it behaves as a base |
| hydronium ion | the product (H3O+)of a reaction between a hydrogen ion and a water molecule |
| strong acids | ionize virtually 100% in water to yield hydronium ions (H30). strong acids are also strong electrolytes. hydrochloric (HCl) is a strong acid. |
| weak acids | do not ionize completely in water, yield much less than 100% hydronium ions. weak acids are also weak electrolytes. carbonic (H2CO3) is a weak acid |
| monoprotic acid | an acid that contains only one ionizable hydrogen ion or proton, per formula weight in solution |
| polyprotic acid | acids that can donate more than one hydrogen ion or peoton, per formula weight in solution |
| physiological importance of acids | digestion absorption of food nerve function enzyme action other biochemical reactions necessary for life |
| properties of acids | taste-sour litmus paper-turns blue litmus red neutralization reaction (acid + base) |
| classical base | a chemical compound that yields a hydroxide ion in a water solution |
| bronsted-lowery (proton acceptor) | a compound that accepts a hydrogen ion is a base (anything that accepts a proton) |
| strong bases | ionize virtually 100% in water to yield ions a strong base will acquire a proton |
| weak bases | do not ionize completely in water a base with a low tendency to gain a proton |
| clinical importance of bases | digestion, absorption of food, nerve function, enzyme action and other biochemical reaction necessary for life lime water (calcium hydroxide) is used to overcome excess acidity of the stomach milk of magnesia (dilute solution of magnesium hydroxide) is used as an antacid, the suspension is used as a laxative spirit of ammonia or smelling salts (ammonium hydroxide) heart and respiratory stimulant |
| properties of bases | taste-bitter or astringent taste touch-slippery feeling (like soap) litmus paper-turns red litmus blue |
| dissociation of water (self-ionization of water) | water has both acidic and basic properties, dissociation produces both the hydronium ion and hydroxide ion |
| amphoteric | compound that can act as both a proton donor or proton acceptor |
| pH | the molar concentration of hydrogen ions in a solution as expressed in the equation pH = -log[H+] "p" is the negative power to which the number 10 must be raised and "H" is the molar concentration of hydrogen ions |
| pH scale | has values that range from 0 (very acidic) to 14 (very basic) a pH of 7, the middle of the scale, is neutral and neither acidic nor basic normal blood pH is maintained from 7.35-7.45 |
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