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Unit I -- Families of Chemical Compounds Section-1 Compounds can be classified into ______________ based on their physical and chemical properties One such classification is _________ versus _______________ Acids ____________ taste - but DON’T use taste for ID of chemicals Affect the __________ of indicators (an indicator is a compound that shows a definite color change when mixed with an acid or a base) Turns blue litmus paper to _______ (acid) Phenolphthalein is ______________ in acid React with ________ metals to form hydrogen gas and a metal compound Contain hydrogen produces H+ ions when dissolved in _________ Therefore defined as a proton (H+) donor The H+ ion reacts with water to form the hydronium ion H3O+ Not all hydrogen containing compounds produce H+ ions therefore not all are acids 3 most common acids are (know these formulas!) These three are all STRONG acids H2SO4 = __________ acid HNO3 = ___________ acid HCl = ___________________ acid The more ionization occurring, the stronger the acid Strong acids make good _______________ (substance whose water solution conducts electricity) These are all WEAK acids HC2H3O2 = ____________ acid H2CO3 = _______________ acid H3BO3 = ______________ acid Weak acids are ________________ electrolytes because they release only a few H+ ions Bases __________ taste - again do not ID chemicals by taste or touch _____________ to the touch Can be ______________ or corrosive Turns red litmus paper ____________ (base) Phenolphthalein turns from colorless to BRIGHT __________ in a base Emulsify (dissolve) fats and oils to form a ___________ Produces OH- ion (______________ ion) when dissolved in water The OH- ion combines with H+ ion to form ______________ Therefore bases are defined as a _______________ (H+) acceptor Know the common bases… These are ____________ bases KOH = ____________ hydroxide NaOH = ____________ hydroxide Strong bases are ____________ electrolytes These are _____________ bases NH4OH = ________________ hydroxide Al(OH)3 = _________________ hydroxide Weak bases are ___________ electrolytes When water is ionized, here is the reaction: 2H2O H3O+ + OH- Section-2 Solutions can be ___________, basic, or neutral The pH scale is used to measure ____________ of a solution The _______ of solution is a measure of the hydronium (H3O+) concentration pH indicates how _________ a solution is pH scale goes from 0 to 14 _____ is neutral (neither an acid or a base) pH 7 = acid The lower the number, the more _________ pH 7 = base The higher the number, the more _________ An indicator is used to determine pH (litmus paper/phenolphthalein…. Other indicators are pH paper, methyl orange, bromothymol blue, red cabbage juice, and tea The most accurate measurements are done with a pH ________ When acids react with bases, they form _________ compounds A salt is a compound formed from the positive ion of a base and the negative ion of an acid Example H+Cl- + Na+OH- H2O + NaCl (Double replacement reaction) Acid base H+ and OH- salt This is called a ____________________ reaction Many salts formed this way are only slightly soluble in water or insoluble in water They __________________ out of solution and remain in the solid phase (they precipitate out of solution…. Therefore they are called ___________________) __________________ = a solid substance that crystallizes out of solution and remains in the solid phase The process of forming of a precipitate is called _______________ Section-3 __________________ is in more than 15 million compounds Compounds containing carbon are called ________________ compounds All organic compounds contain carbon Organic means "____________ _________ ___________" because scientists once thought only "living" organisms could produce organic compounds (they were wrong -- _________________ made urea in 1828…. It is an organic compound) All organic compounds contain carbon but not all carbon containing compounds are organic -- some are __________________ (Examples: calcium carbonate, carbon dioxide, carbon monoxide (have carbon but are not organic…. These are inorganic) There are so many carbon compounds because of its ability to bond with __________ and ___________ elements Carbon forms ____________ bonds which occur in chains (straight or branched) and rings (single or joined together) The bonds can be ___________ (one pair of electrons), ___________ (two pair of electrons), or _______________ (three pair of electrons) covalent bonds The simplest organic compound contains just hydrogen and carbon (H and C) These are called ____________________ _______________ compounds usually exist as gases, liquids, or low melting point solids They have _______________ odors and low boiling points They do not conduct electricity (nonelectrolytes) and generally do not ___________ in water _______________ formula = shows the elements in the compound and the # of atoms of elements in the compound but does not show the arrangement Example: H2O 1 molecule (2 H atoms and 1 O atom) ______________ formula = shows the kind, #, and arrangement of atoms in a molecule (model of a molecule) In a structural formula a dash (-) is used to represent the pair of electrons shared forming the covalent bond = is a double bond = is a triple bond Carbon has ___ valence electrons and needs ___ to fill the shell When writing a structural formula you cannot have dangling bonds (dangling dashes)… all must be filled! H Example: methane (the carbon has single bonds) H-C-H H ______________ = compounds with the same molecular formula but different structural formulas Example: Butane and Isobutane H H H H H HH | | | H-C-C -C-C-H H-C-C-C - H | | | | / | \ H H H H C4H10 H C H C4H10 / | \ H HH As the number of carbon atoms in a molecule ___________, the number of isomers _____________ Section-4 __________________ = contain only H and C Hydrocarbons are classified as ______________ and ______________ Saturated = all carbon bonds are ___________ covalent bonds Unsaturated = one or more carbon bonds is a ___________ or _________ covalent bond _____________ = straight chained or branched chain hydrocarbons where all carbon bonds are single covalent bonds (saturated) The simplest alkane is _____________ (CH4) Each successive alkane has ___ more carbon and ___ more hydrogen Example: ethane C2H6, propane C3H8… etc) The general formula is CnH2n+2 where n=the # of carbons atoms in the alkane All alkanes end in ______________ The __________ tells the # of carbon atoms Meth = 1, Eth = 2, Prop = 3, But = 4, Pent = 5, Hex = 6, Hept = 7, Oct = 8, Non = 9, Dec = 10 _______________ = hydrocarbons with at least one pair of carbon atoms joined by a double covalent bond (unsaturated hydrocarbon) The simplest alkene is ethene (C2H4) H H All alkenes end in -ene \ / The general formula is CnH2n C=C / \ H H Alkenes are more _______________ than alkanes because a double bond is more _____________ broken than a single bond ______________ = hydrocarbons with at least one pair of carbon atoms joined by a triple covalent bond (unsaturated hydrocarbon) The simplest alkyne is ethyne (C2H2) ethyne is also called acetylene All alkynes end in -yne The general formula is CnH2n-2 Alkynes are more reactive than alkenes because there is not much __________ needed to break a triple bond Some hydrocarbons form _________ (instead of straight or branched chains) These are called aromatic hydrocarbons They have strong ___________ odors (aromas) The basic structure is a ring of 6 carbon atoms joined by alternating single and double bonds The simplest aromatic hydrocarbon is benzene (C6H6) H | C // \ H-C C-H /\ | || OR |O| H-C C-H \/ \\ / C | H Section-5 ______________ hydrocarbon = formed when one or more hydrogen atoms in a hydrocarbon chain or ring is ______________ by a different atom or group of atoms Example: alcohols, organic acids, esters, and halogen derivatives ________________ = (substituted hydrocarbons) have one or more hydrogen atoms replaced by an -OH group (hydroxyl group) The simplest alcohol is methanol (CH3OH) (one of the Hydrogen atoms from methane CH4 is replaced by OH) _________________ is used to make plastic, synthetic fibers, gas de-icer, and as a solvent It is very _____________ (even externally) All alcohols end in -ol This ______________ is added to the name of the corresponding hydrocarbon Example: ethanol C2H5OH is ethane C2H6 H to OH Ethanol is produced by the action of _________ or _____________ on sugar stored in grains ________________ is a good solvent for organic compounds that don't dissolve in water Ethanol is also used in ____________ and ___________ beverages H H | | H-C - C-OH Ethanol | | H H ______________ alcohol = ethanol made unfit for beverage purposes by adding ____________ compounds such as methanol to it Alcohols can be in rings or chains ___________ = alcohol formed by replacing one hydrogen atom in a benzene ring with an -OH group Phenol is used for preparation of _________ and as a _______________ ___________ acids = (substituted hydrocarbon) one hydrogen is replaced by a -COOH group (carboxyl group) In the carboxyl group, one of the carbon oxygen bonds is a double bond C-OH || O Examples of organic acids: formic acid (HCOOH) and acetic acid (CH3COOH) _________ acid is the _________ organic acid It is also called __________ acid and is found in _________ (in stinging nettle plants and in some ants) The ending -oic is added to the name of the corresponding hydrocarbon However common names are used more frequently __________ acid is also called ethanoic acid It is found in ____________ __________ acid which is derived from propane (propanoic acid) is found in ________________ fruits It is written C2H5COOH Esters = formed when an ___________ and an ___________ acid combine Esters have a pleasant ___________ and ______________ The sweet smell of __________ comes from esters (example: strawberries, bananas, pineapples) Many esters occur naturally but we can make synthetic esters too (for _________ and ________________) ______________ derivatives = formed when the hydrogen in a hydrocarbon is __________________ by a halogen (still a substituted hydrocarbon) Example: methyl chloride CH3Cl, tetrachloroethane C2H2Cl4, and dichlorodifluoromethane CCl2F2