Nomenclature. Sections 2.7, , RW Session ID = MSTCHEM1

Transcription

1 Nomenclature Sections 2.7, , 3.12 RW Session ID = MSTCHEM1

2 Group (Column) 1 Atomic # H Symbol Hydrogen Name Molar mass Phase Solid Liquid Gas Main Group Elements Metals Semimetals (metalloids) Nonmetals Alkali Metals Alkali Earth Metals Halogens Noble Gasses Period (Row) H Hydrogen 2 Transition Metals Li Be B C N O F Ne Lithium Beryllium Boron Carbon Nitrogen Oxygen Fluorine Neon Na Mg Al Si P S Cl Ar Sodium Magnesium Aluminum Silicon Phosphorous Sulfur Chlorine Argon K Ca Sc Ti V Cr Mn Fe Co Ni Cu Zn Ga Ge As Se Br Kr Potassium Calcium Scandium Titanium Vanadium Chromium Manganese Iron Cobalt Nickel Copper Zinc Gallium Germanium Arsenic Selenium Bromine Krypton Rb Sr Y Zr Nb Mo Tc Ru Rh Pd Ag Cd In Sn Sb Te I Xe Rubidium Strontium Yttrium Zirconium Niobium Molybdenum Technetium Ruthenium Rhodium Palladium Silver Cadmium Indium Tin Antimony Tellurium Iodine Xenon [98] Cs Ba 57 to Hf Ta W Re Os Ir Pt Au Hg Tl Pb Bi Po At Rn Cesium Barium Hafnium Tantalum Tungsten Rhenium Osmium Iridium Platinum Gold Mercury Thulium Lead Bismuth Polonium Astatine Radon [209] [210] [222] Fr Ra 89 to Rf Db Sg Bh Hs Mt Ds Rg Cn Uut Uuq Uup Uuh Uus Uuo Francium Radium 103 Rutherfordium Dubnium Seaborgium Bohrium Hassium Meitnerium Darmstadium Roentgenium Copernicium Ununtrium Ununquadium Ununpentium Ununhexium Ununseptium Ununoctium [223] [226] [267] [268] [271] [267] [269] [276] [281] [280] [285] [284] [289] [288] [293] [UK] [294] La Ce Pr Nd Pm Sm Eu Gd Tb Dy Ho Er Tm Yb Lu Lanthanum Cerium Praseodymium Neodymium Promethium Samarium Europium Gadolinium Terbium Dysprosium Holmium Erbium Tellurium Ytterbium Lutetium [145] Ac Th Pa U Np Pu Am Cm Bk Cf Es Fm Md No Lr Actinium Thorium Protactinium Uranium Neptunium Plutonium Americium Curium Berkelium Californium Einsteinium Fermium Mendelevium Nobelium Lawrencium [227] [237] [244] [243] [247] [247] [251] [252] [257] [258] [259] [262] He Helium

3 Elements Atomic Exist in nature with single atoms as their basic unit All metals and semimetals Na, K, Mg, Ca, Fe, Ni, B, Si, etc. Some nonmetals (including all noble gases) C, He, Ne, Ar, Kr, Xe, Rn Molecular Normally exist in nature as molecules Some nonmetals H 2, N 2, O 2, F 2, Cl 2, Br 2, I 2, P 4, S 8

4 Compounds Molecular (covalent) Consist of two or more covalently bonded nonmetals Referred to as molecules Ionic Composed of cations and anions bound together by ionic bonds (generally consist of at least one metal and one nonmetal) Referred to as formula units (the smallest electrically neutral collection of ions)

5 Chemical Bonds Ionic bonds Electrostatic forces between ions Generally occur between metals and nonmetals Metals tend to lose electrons forming cations Nonmetals tend to gain electrons forming anions Covalent bonds Sharing of electrons between atoms Occur between two or more nonmetals

6 Ions Charged particles Formed when a neutral species loses or gains electrons Cations Positively charged Formed when electrons are lost Anions Negatively charged Formed when electrons are gained

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8 Naming Monoatomic Ions Cations Cations with only one possible charge Element name + ion Na + sodium ion Ca 2+ calcium ion Zn 2+ zinc ion Cations with more than one possible charge Element name + (charge in Roman numerals) + ion Ni 2+ nickel(ii) ion Ni 3+ nickel(iii) ion Pb 4+ lead(iv) ion Anions Element root name + ide + ion N 3- nitride ion O 2- oxide ion Fˉ fluoride ion

9 Monoatomic Cations w/ one possible charge Element name + ion

10 Monoatomic Cations w/ more than one possible charge Element name + (charge in Roman numerals) + ion Latin System: -ous ending indicates lower charge -ic ending indicates higher charge

11 Monoatomic Anions Element root name + ide + ion

12 Polyatomic Ions Polyatomic ions containing oxygen (oxyanions) # of oxygen atoms Least Less More Naming system hypo- -ite ion -ite ion -ate ion SO 3 2- Sulfite ion SO 4 2- Sulfate ion Other polyatomic ions NH 4 + OH - CN - Most Per- -ate ion Ammonium ion Hydroxide ion Cyanide ion BrO - BrO - 2 BrO - 3 BrO - 4 Hypobromite ion Bromite ion Bromate ion Perbromate ion

13 Polyatomic Ions # of oxygen atoms Least Less More Naming system hypo- -ite ion -ite ion -ate ion Most Per- -ate ion

14 Ionic Compounds Contain a cation and an anion Ions combine in a ratio that forms a neutral unit Formula unit Generally at least one metal and one nonmetal Metals form cations Nonmetals form anions Naming ionic compounds Identify the cation and anion Name the cation and anion Combine the cation and anion names (remove ion from each) Writing ionic compound formulas Identify the cation and anion Combine the cation and anion in a ratio that will form a neutral unit

15 Naming Ionic Compounds Name each ion, combine, and remove ion LiBr Li + Br - Lithium ion Bromide ion Lithium bromide BaS Ba 2+ S 2- Barium ion Sulfide ion Barium sulfide K 2 O K + O 2- Potassium ion Oxide ion Potassium oxide Mg 3 P 2 Mg 2+ P 3- Magnesium ion Phosphide ion Magnesium phosphide

16 Naming Ionic Compounds For metals with more than one charge, indicate charge using roman numerals in parentheses CuCl Cu + Cl - Copper(I) ion Chloride ion Copper(I) chloride CuCl 2 Cu 2+ Cl - Copper(II) ion Chloride ion Copper(II) chloride

17 Hydrates Ionic compounds with associated water molecules Name the ionic compound Add the word hydrate with prefix to indicate the number of water molecules LiNO 2 H 2 O Mg(BrO 3 ) 2 6H 2 O CoSO 4 7H 2 O Lithium nitrite monohydrate Magnesium bromate hexahydrate Cobalt(II) sulfate heptahydrate

18 Molecular Compounds Prefixes indicate the number of each element Mono is omitted from first element Second element has ide ending S 3 Cl 2 S 2 O SF 6 Trisulfur dichloride Disulfur monoxide Sulfur hexafluoride *The ending a or o is dropped from a prefix if the element begins with a or o

19 Acids Release hydrogen ion when dissolved in water Acids are named based on the remaining anion -ide ion changes to hydro- -ic acid -ite ion changes to -ous acid -ate ion changes to -ic acid Cl - Chloride ion HCl(aq) Hydrochloric acid CN - Cyanideion HCN(aq) Hydrocyanic acid SO 3 2- Sulfiteion H 2 SO 3 (aq) Sulfurous acid SO 4 2- Sulfate ion H 2 SO 4 (aq) Sulfuric acid BrO - Hypobromiteion HBrO(aq) Hypobromousacid

20 Acids -ide ion to hydro- -ic acid -ite ion to -ous acid -ate ion to -ic acid

21 Organic Compounds Nomenclature prefix to indicate the number of carbons in a continuous chain suffix to indicate the functionality Hydrocarbons Alkanes single bonds Alkenes double bond Alkynes triple bond Hydrocarbon derivatives (functionalized hydrocarbons) Alcohols (-OH) Amines (-NH 2 ) Carboxylic acids (-CO 2 H) 1 Meth 2 Eth 3 Prop 4 But 5 Pent 6 Hex 7 Hept 8 Oct 9 Non 10 Dec

22 Alkane Alkene Alkyne H H H C C H H H H H C = C H H H C C H Ethane (C 2 H 6 ) Ethene (C 2 H 4 ) Ethyne (C 2 H 2 ) Alcohol -OH -ol Amine -NH 2 -ylamine Carboxylic acid -CO 2 H -oic acid H H C OH H H H C NH 2 H O H C OH Methanol (CH 3 OH) Methylamine (CH 3 NH 2 ) Methanoic acid (HCO 2 H)

23 Organic Compounds prefix indicates the number of carbons in a continuous chain suffix indicates the functionality

24 Chemical Nomenclature Summary Ionic Compounds (metal + nonmetal) Always identify the cation and anion first Naming name each ion and combine names, dropping ion from each Formulas combine in a ratio to form a neutral unit, placing subscripts to indicate the number of each ion needed and removing charges on each ion Hydrates are ionic compounds that absorb water Naming hydrate is added to the end of the ionic compound name with corresponding prefix to indicate number of waters Formulas dot H 2 O is added to the end of the ionic compound formula, with # indicating number of waters absorbed per unit

25 Chemical Nomenclature Summary Covalent Compounds (nonmetal + nonmetal) Also referred to as binary covalent or inorganic covalent Use element names with prefixes to indicate number of atoms of each element Add -ide ending to final element name Mono- prefix is never used on first element A s and o s never pair, drop a or o from end of prefix when this occurs

26 Chemical Nomenclature Summary Acids Acids are covalent compounds that release hydrogen ion (H + ) when placed in water (aqueous solution) Naming based on anion names -ide ion is replaced by hydro- -ic acid -ite ion is replaced by -ous acid -ate ion is replaced by -icacid Formulas identify anion by reversing above systematic and add enough H + to create a neutral substance

27 Chemical Nomenclature Summary Organic Compounds (mainly carbon and hydrogen) Nomenclature is based on prefixes to indicate number of carbons and suffixes to indicate functionality Functionalities suffixes Alkane (all single bonds between carbons) -ane Alkene (at least one double bond between carbons) -ene Alkyne (at least one triple bond between carbons) -yne Alcohol (contains -OH group) -ol Amine (contains -NH 2 group) -ylamine Carboxylic acid (contains -CO 2 H group) -oic acid Drawing structural formulas for organic compounds to determine formulas and names is much easier than memorizing them In organic compounds carbon always forms 4 bonds, nitrogen forms 3 bonds, oxygen forms 2 bonds, and hydrogen forms 1 bond