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Science 1206 - Naming and Writing Formulas for Chemical Compounds NAME:____________________________ IUPAC ! ! ! International Union of Pure and Applied Chemists This is a global organization that sets the standards in chemistry. One job of the IUPAC is to give compounds SYSTEMIC NAMES. SECTION OUTLINE ! BOHR DIAGRAMS FOR ATOMS ! TYPES OF CHEMICAL BONDS ! MOLECULAR COMPOUNDS " TYPES # SIMPLE COVALENT # COMMON NAME ! BOHR DIAGRAMS FOR IONS ! IONIC COMPOUNDS " SIMPLE IONIC " MULTIVALENT " POLYATOMIC/COMPLEX " HYDRATED IONIC ! ACIDS BOHR DIAGRAMS FOR ATOMS ! Bohr diagrams, also called ____________________________, are a means of drawing atoms in a 2-D manner. ! Keep in mind that atoms are actually 3-D, and there are more complex representations of atoms. ! Bohr models always include the _______________ and the _________________________ of an atom. ! There are 3 types of SUBATOMIC PARTICLES found in the nucleus: " PROTONS (_____) _____________________________________________________ _____________________________________________________ " ELECTRONS (_____) _____________________________________________________ _____________________________________________________ " NEUTRONS (_____) _____________________________________________________ _____________________________________________________ ! NUCLEUS " __________________________________________________________ __________________________________________________________ ! ELECTRON ENERGY LEVELS " __________________________________________________________ __________________________________________________________ " 3 Levels First Level (Closest to Nucleus) __________________ Second Level __________________ Third Level (Outermost) __________________ ! VALENCE LEVEL " Definition:_________________________________________________ " Electrons in this level are called:____________________ " Atoms with FULL valence shells are STABLE, meaning they will not bond with other atoms in normal conditions. " The atoms of Group ____, the _______________, have full valence levels. " Atoms that do not have full electron energy levels are unstable and must __________, __________, or __________ electrons to be stable. ATOMIC NUMBER ! Located in the top of each element box on the periodic table ! ATOMIC NUMBER = ___________________________ ATOMIC MASS (Molar Mass) ! Located in the bottom of each element box on the periodic table ! Round it off for calculating. ! ATOMIC MASS = __________________________________________ EXAMPLE: ! DRAW BOHR DIAGRAMS FOR: ! - Li - lithium atom - Ne - neon atom - S - sulfur atom HOMEWORK: Do WORKSHEET on following page. TYPES OF CHEMICAL BONDS ! CHEM ICAL BONDS " DEFINITION:___________________________________________________________ " There are 2 TYPES OF Chem ical Bonds: # COVALENT # IONIC ! COVALENT BONDS " AKA:_____________________________ " “co” - ______________________________, “valent” - ___________________________ " DEFINITION: _______________________________________________________________ " ! IONIC BONDS " DEFINITION: _______________________________________________________________ " ! BETW EEN:________________________________________________ Solutions of covalently bonded substances are __________________________. BETW EEN:________________________________________________ Solutions of ionic bonded substances are ______________________________. Com pounds consist of atom s or ions of two or m ore elem ents bonded together. MOLECULAR COMPOUNDS ! Form when ________________ share electrons in ___________________. ! 2 TYPES: " " BINARY Molecular Compounds TRIVIAL NAME Molecular Compounds BINARY Molecular Compounds ! Also called SIMPLE molecular compounds. ! Binary Molecular Compounds use IUPAC prefixes: " We will write these prefixes in the following table. 1 2 3 4 5 6 7 8 9 10 ! GIVEN MOLECULAR FORMULA, WRITE NAME " RULES: _____________________________________________________ _____________________________________________________ _____________________________________________________ _____________________________________________________ _____________________________________________________ - EXAMPLE: # N2O4 # P2O5 # CCl4 _________________________ _____________________________________ _________________________ ! GIVEN MOLECULAR NAME, WRITE FORMULA " RULES: _____________________________________________________ _____________________________________________________ _____________________________________________________ EXAMPLE # carbon monoxide _______________ # triphosphorus pentabromide _______________ # sulfur hexafluoride _______________ ! TRIVIAL NAME Molecular Compounds " Also called COMMON NAME molecular compounds " There are SOME molecular compounds that still go by their common names. " These common names must be memorized: FORM ULA TRIVIAL/COM M ON NAM E O3 H 2O H 2O 2 NH 3 CH 4 CH 3OH C 2H 5OH C 6H 12O 6 C 12H 22O 11 ! HOMEWORK: Complete the 3 sheets on the following pages. IONS ! RECALL: " As mentioned earlier, atoms other than the NOBLE GASES are unstable, and need to GAIN, LOSE, or SHARE ELECTRONS to become more stable. " If they SHARE electrons, this forms a COVALENT BOND to another atom. " If they LOSE or GAIN electrons, atoms become IONS and form IONIC BONDS with other atoms. ! OCTET RULE " __________________________________________________________ ! WHAT IS AN ION? " Ions are ____________________ that have lost or gained electrons to achieve the valence configuration of a noble gas. " TWO TYPES: CATIONS # _____________ ions that are formed from a __________ of electrons. # It has more ___________ than ______________ and therefore has a net _________________ charge. # _____________ form cations. # MEMORY TOOL:__________________________________ # EXAMPLE - lithium ion - ANIONS # _____________ ions that are formed from a __________ of electrons. # It has more ___________ than ______________ and therefore has a net _________________ charge. # change the ending of the name of anions to ________ # _____________ form anions. # MEMORY TOOL:__________________________________ # EXAMPLE - fluoride ion BOHR DIAGRAMS FOR IONS ! ! METALS " ATOMS of METALS will LOSE electrons to become CATIONS. " ATOMS with 1, 2, or 3 VALENCE electrons will LOSE these electrons to form 1+, 2+, or 3+ ions respectively. " GROUP 1 ATOMS - ____________________ # ________ valence electrons(s) # ________ ion " GROUP 2 ATOMS - ____________________ # ________ valence electrons(s) # ________ ion " GROUP 3 ATOMS # ________ valence electrons(s) # ________ ion NONMETALS " ATOMS of NONMETALS will GAIN electrons to become ANIONS. " ATOMS With 5, 6, or 7 VALENCE electrons will GAIN more electrons to form 3-, 2-, or 1- ions respectively. " GROUP 15 ATOMS # ________ valence electrons(s) # ________ ion " GROUP 16 ATOMS # ________ valence electrons(s) # ________ ion " GROUP 17 ATOMS - ___________________ # ________ valence electrons(s) # ________ ion " GROUP 18 ATOMS - __________________ FULL outer valence levels ! TO DRAW: " ! Draw a Bohr diagram for: # A sodium atom AND a sodium ion # A chlorine atom AND a chloride ion HOMEWORK: Do the following 2 worksheets for homework. IONIC COMPOUNDS ! Form when at least _______________________ transfer electrons in an _____________________. ! Metals will become CATIONS and ___________ electrons and nonmetals will become ANIONS and ___________ electrons. ! These ions, with opposite charges, attract, and form ionic bonds. ! ! ! Unlike covalent bonds, these bonds are not “ACTUAL BONDS,” but forces of attraction between oppositely charged ions. They stay together in a _________________________. EXAMPLE - NaCl ! 3 TYPES: " " " BINARY Ionic Compounds SIMPLE Ionic Compounds MULTIVALENT Ionic Compounds POLYATOMIC Ionic Compounds HYDRATED Ionic Compounds BINARY IONIC COMPOUNDS " “Binary” - ___________________________________________________ SIMPLE Ionic Compounds ! Simple ionic compounds are composed of a metal ion (+) and a nonmetal ion (-). ! GIVEN FORMULA, WRITE NAME " RULES: _____________________________________________________ _____________________________________________________ _____________________________________________________ _____________________________________________________ _____________________________________________________ _____________________________________________________ _____________________________________________________ _____________________________________________________ _____________________________________________________ - " ! EXAMPLE: # MgBr2 _____________________________________ # KCl _____________________________________ # Na2S _____________________________________ # Mg3P2 _____________________________________ # Ba3N2 _____________________________________ What’s Wrong with the Following Names for BaS? - barium sulfur _____________________________________ - Barium Sulfide _____________________________________ - barium sulfuride _____________________________________ HOMEWORK: Do the sheet on the following page. ! GIVEN NAME, WRITE FORMULA " RULES: _____________________________________________________ _____________________________________________________ _____________________________________________________ _____________________________________________________ _____________________________________________________ _____________________________________________________ _____________________________________________________ _____________________________________________________ - ! EXAMPLE: # sodium bromide ______________________ # barium iodide ______________________ # magnesium oxide ______________________ # aluminum oxide ______________________ HOMEWORK: Do the next 2 sheets on the following pages. MULTIVALENT Ionic Compounds ! Ions of some _____________________ can have more than one possible charge. ! Such elements are called MULTIVALENT species. ! For example what are the 2 possible charges for copper - Cu? " _____________ " _____________ ! WE use ROMAN NUMERALS to indicate the type of charge on these multivalent ions. " 1 + –> ______ " 2 + –> ______ " 3 + –> ______ " 4 + –> ______ " 5 + –> ______ " 6 + –> ______ # ONLY USE THESE ROMAN NUMERALS WITH MULTIVALENT IONS!!!! ! GIVEN NAME, WRITE FORMULA " RULES: _____________________________________________________ _____________________________________________________ _____________________________________________________ _____________________________________________________ - ! EXAMPLE: # copper (II) oxide ________________________________ # lead (IV) sulfide ________________________________ # tin sulfide ________________________________ HOMEWORK: Do the sheet on the following page. ! GIVEN FORMULA, WRITE NAME " RULES: _____________________________________________________ _____________________________________________________ _____________________________________________________ _____________________________________________________ _____________________________________________________ _____________________________________________________ - ! EXAMPLE: # PbI2 _____________________________________ # Fe2O3 _____________________________________ # CuCl _____________________________________ # MnO2 _____________________________________ HOMEWORK: Do the next 2 sheets on the following pages. POLYATOMIC Ionic Compounds ! DEFINITION: " __________________________________________________________ __________________________________________________________ ! On the back of your periodic table, there is a POLYATOMIC ION TABLE. " You do not have to memorize them, but from use, you will become very familiar with them. " Example: nitrate _______________ nitrite _______________ cyanide _______________ hydroxide _______________ bicarbonate _______________ chlorate _______________ carbonate _______________ sulfate _______________ phosphate _______________ ammonium _______________ acetate _______________ ! Endings of polyatomic ions are easily recognizable as they are often _________ or ____________. # These endings are good clues that an ionic compound contains polyatomic ions. ! GIVEN NAME, WRITE FORMULA - EXAMPLE: # lithium sulfate __________________________ # ammonium carbonate __________________________ # hydrogen dichromate __________________________ # sodium acetate __________________________ ! GIVEN FORMULA, WRITE NAME " RULES: - ! EXAMPLE: # HNO3 __________________________ # NaOH __________________________ # KMnO4 __________________________ # Cu2SO4 __________________________ HOMEWORK: Do next 2 sheets on following page for homework. HYDRATED Ionic Compounds ! Hydrated ionic compounds that have _________________ attached to their crystal lattice structure. ! Solutions become hydrated when they are crystallized from a water solution. ! They are often recognizable by eye because they are often ________________ and ___________________. ! Examples:_____________________________________________________ ! Bluestone –> CuSO4 ! 5 H2O " __________________________________________________________ __________________________________________________________ __________________________________________________________ ! We indicate the presence of water with the word _______________ and we indicate the number of water molecules with our GREEK PREFIXES " __________________________________________________________ __________________________________________________________ ! ANHYDROUS:____________________________________________________ ! GIVEN NAME, WRITE FORMULA " EXAMPLE: barium chloride dihydrate ! ! _____________________ - potassium hydroxide hexahydrate _____________________ - sodium carbonate octahydrate _____________________ - cobalt (II) chloride decahydrate _____________________ GIVEN NAME, WRITE FORMULA " EXAMPLE: CaSO4 C 2 H2O ________________________________ - Na3PO4 C 4 H2O ________________________________ - HCN C 3 H2O ________________________________ HOMEWORK: Do the sheet on the following page.