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Chemical Compounds - Vocabulary

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Chemical Compounds - Vocabulary CHEMICAL COMPOUNDS - VOCABULARY COVALENT COMPOUND A compound that has only covalent bonds between atoms of which it is made. The covalent bond results from sharing valence electrons between two atoms. The representative unit of a covalent compound is usually a molecule. IONIC COMPOUND A compound that is built of monatomic or polyatomic ions of opposite charges. The bonds between ions of opposite charges are called ionic bonds. Many, but not all ionic compounds contain a metallic element. The representative unit of an ionic compound is always a formula unit. There no molecules in ionic compounds. Ions per se are not compounds. FORMULA UNIT The smallest combination of atoms or ions that correctly represents the ratio in which they are combined in a chemical compound. Formula unit is a more general term than a molecule. ORGANIC COMPOUND A compound that is built of atoms of carbon and other elements (most commonly, hydrogen, nitrogen, oxygen, sulfur, and halogens) except for carbon monoxide, carbon dioxide, carbonic acid, carbonates, and hydrogen carbonates. If there is no carbon present, a compound is certainly inorganic. The simplest organic compound is CH4, methane. BINARY COMPOUND Ionic or covalent compound that is made of atoms of two different elements. Examples: MgCl2; Al2O3; HCl; H2O; CH4. DIATOMIC MOLECULE A molecule that is built of exactly two atoms either of the same element or of two different elements. Examples: O2; N2; CO; HF. MONATOMIC ION A single atom that lost or gained one or more electrons as compared to the neutral atom of the same element. The electric charge must be indicted when a formula of it is written unless the ion is combined with another ion in the formula of an ionic compound. Examples: Na+; Fe3+; Br–; S2–. POLYATOMIC ION A group of atoms either of the same element or different elements held together by covalent bonds like atoms in a molecule, but unlike a molecule carrying nonzero electric charge. Polyatomic ion per se is not a compound, but it can be part of an ionic compound when combined with an ion of opposite charge. The electric charge must be indicted when a formula of it is written unless the ion is combined with another ion in the formula of an ionic compound. + 2+ – 2– 2– Examples: NH4 ; Hg2 ; NO3 ; SO3 . (SO3 is not the same as SO3 .) ACID A covalent compound whose molecules have a special hydrogen atom that can be detached from the rest of the molecule as hydrogen ion (H+) in an aqueous solution. The rest of the molecule becomes a negatively charged ion. A pure acid may not conduct electricity, but its aqueous solution (acid mixed with water) does conduct electricity. The sour taste of acids is due to hydrogen ion. Matter (solid, liquid, gas) Substances Physical Mixtures (constant composition) Change (variable composition) Organic Elementary Chemical Compounds Homogeneous Compounds Heterogeneous Substances Change Mixtures Mixtures Inorganic (or Solutions) Compounds Metals Nonmetals Metalloids Ionic Covalent Compounds Compounds Representative Molecule Formula Unit Atom Atom Molecule Atom Formula Unit Particle O2, O3, Cl2, SiO2(quartz), P4, S8 SiC SUMMARY OF NOMENCLATURE SYSTEM SUBSTANCE NAME FORMULA OR ION Elementary Name of element Symbol of element; common exceptions: Substance H2, N2, O2, F2, Cl2, Br2, I2 Monatomic Cation Name of element followed by ion; if element Symbol of element followed by superscript forms more than one monatomic cation, to indicate charge elemental name is followed by ion charge in Roman numerals and in parentheses Monatomic Anion Name of element changed to end in –ide Symbol of element followed by superscript followed by ion to indicate charge Compounds made First element in formula followed by second, Symbol of first element in name followed up of atoms of two change to end in -ide; each element by symbol of second element, with nonmetals preceded by prefix to show the number of subscript to show number of atoms in the atoms in the molecule molecule Acid Most common: middle element changed to H followed by symbol of nonmetal followed end in -ic by O (if necessary), each with appropriate One more oxygen than -ic acid: add prefix subscript per- to name of -ic acid MEMORIZE THE FOLLOWING: One fewer oxygen than -ic acid: change Nitric acid: HNO3 ending of -ic acid to -ous Sulfuric acid: H2SO4 Two fewer oxygens than -ic acid: add prefix Carbonic acid: H2CO3 hypo- to name of -ous acid Phosphoric acid: H3PO4 No oxygen: Prefix hydro- followed by name of Chloric acid: HClO3 second element changed to end in –ic Acetic acid: HC2H3O2 Polyatomic anion Replace -ic in acid name with -ate, or replace Acid formula without hydrogen plus from total -ous in acid name with -ite, followed by ion superscript showing negative charge equal ionization of to number of hydrogens removed from oxyacid acid formula Polyatomic anion Hydrogen followed by name of ion from total Acid formula minus one (or two for H3PO4) from step-by-step ionization of acid (dihydrogen in the case of hydrogen(s), plus superscript showing – ionization of H2PO4 ) negative charge equal to number of oxyacid hydrogen atoms removed from acid formula + Other polyatomic Ammonium ion NH4 ions Hydroxide ion OH– 2+ Mercury (I) ion Hg2 Ionic Compound Name of cation followed by name of anion Formula of cation followed by formula of (omitting ion in each of the names) anion (usually no charges indicated), each taken as many times as necessary to yield a net charge of zero (polyatomic ion formulas enclosed in parentheses if taken more than once) Hydrated Salt Name of anhydrous compound followed by Formula of anhydrous compound followed (number prefix)hydrate, where (number by “∙X H2O” where X is the number of prefix) indicates the number of water water molecules associated with one molecules associated with one formula unit of formula unit of anhydrous compound anhydrous compound Naming Inorganic Compounds yes Metal no (= ionic compound) or NH4? (= covalent compound) yes Group I or II; no yes no H in front? Al, Ag, Zn, NH4? yes O is present, no but not H2O or H2O2? yes no (aq) is written? Type I Ionic Type II Ionic Oxyacid Nonoxyacid Binary Covalent Compound Compound Compound Al2O3 (s) CuCl(s) HClO(aq) HCl(aq) HCl(g) P2O5(s) aluminum oxide copper(I) chloride hypochlorous acid hydrochloric acid hydrogen chloride diphosphorus pentoxide LiOH (s) CuCl2(s) HClO2(aq) H2S(aq) H2S(g) NO2(g) lithium hydroxide copper(II) chloride chlorous acid hydrosulfuric acid hydrogen sulfide nitrogen dioxide AgNO3(s) Fe2O3(s) HClO3(aq) HCN(aq) HCN(g) S2Cl2(l) silver nitrate iron(III) oxide chloric acid hydrocyanic acid hydrogen cyanide disulfur dichloride Na2O2(s) FeO(s) HClO4(aq) or (l) CO(g) sodium peroxide iron(II) oxide perchloric acid H2O2(l) carbon monoxide CaCO3(s) Cr2(SO4) 3(s) H2SO3(aq) hydrogen peroxide PF5(g) calcium carbonate chromium(III) sulfate sulfurous acid H2O(l) phosphorus pentafluoride NH4NO3(s) MnS(s) H2SO4(aq) or (l) water XeF4(s) ammonium nitrate manganese(II) sulfide sulfuric acid xenon tetrafluoride Sn(NO3) 2(s) NH3(g) tin(II) nitrate ammonia CH4(g) methane CHEMICAL SYMBOLS AND FORMULAS Al 1) Element aluminum Example: Al is the third most abundant element in the Earth crust. 2) Elementary substance (aluminum metal) Example: 5.0 grams of Al. 3) One atom of aluminum 2Al Two (individual) atoms of aluminum 2H Two (individual) atoms of hydrogen H2 1) Molecular hydrogen; substance (hydrogen gas) Example: A balloon is filled with H2 gas. 2) One molecule of hydrogen H2O 1) Water as a substance (a covalent compound) Example: 50 mL of H2O. 2) One molecule of water 2H2O Two molecules of water 2Al + 3O2 Two atoms of aluminum mixed with three molecules of oxygen Al2(SO4)3 1) Aluminum sulfate as a substance (an ionic compound) Example: 3.30 grams of Al2(SO4)3. 2) One formula unit of aluminum sulfate: each 2 atoms of aluminum chemically combined with 3 SO4 groups (atoms of aluminum, sulfur and oxygen chemically combined in the ratio of 2:3:12) GREEK PREFIXES FOR NAMING COMPOUNDS Number Prefix 1/2 hemi- 1 mono- 2 di- bicycle 3 tri- tricycle 4 tetra- 5 penta- the Pentagon 6 hexa- 7 hepta- September 8 octa- October 9 nona- (Latin) November 10 deca- December 11 undeca- (Latin) 12 dodeca- 13 trideca- 20 icosa- Prefixes that are in bold should be memorized!!! NAMES AND FORMULAS OF COMMON IONS POSITIVELY CHARGED IONS (CATIONS) NEGATIVELY CHARGED IONS (ANIONS) The charges of these ions can be figured out The charges of these ions can be figured out using the periodic table: using the periodic table: hydrogen ion H+ hydride ion H– lithium ion Li+ fluoride ion F– sodium ion Na+ chloride ion Cl– potassium ion K+ bromide ion Br– rubidium ion Rb+ iodide ion I– cesium ion Cs+ oxide ion O2– beryllium ion Be2+ sulfide ion S2– magnesium ion Mg2+ nitride ion N3– calcium ion Ca2+ phosphide ion P3– strontium ion Sr2+ barium ion Ba2+ aluminum ion Al3+ These ions must be memorized: These ions must be memorized: + – hydronium ion H3O acetate ion C2H3O2 + – ammonium ion NH4 hydroxide ion OH silver ion Ag+ cyanide ion CN– cadmium ion Cd2+ cyanate ion OCN– zinc ion Zn2+ thiocyanate ion SCN– + – copper (I) or cuprous ion Cu perchlorate ion ClO4 2+ – copper (II) or cupric ion Cu chlorate ion ClO3 2+ – mercury (I) or mercurous ion Hg2 chlorite ion ClO2 mercury (II) or mercuric ion Hg2+ hypochlorite ion ClO– 2+ – lead (II) or plumbous ion Pb nitrate ion NO3 4+ – lead (IV) or plumbic ion Pb nitrite ion NO2 iron (II) or ferrous ion Fe2+ permanganate ion MnO– iron (III) or ferric ion Fe3+ carbonate ion 2– CO3 4 2+ – manganese (II) ion Mn hydrogen carbonate or
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