Chapter 3 outline

Chapter 3 - OutlineMolecules, Ions & Their CompoundsCompounds & Molecules• Atoms are the ___smallest____ unit of an __element_____ that retains the ____chemical characteristics___________ of that element (ref. H, He, Li, Be, N, etc.).• Molecules are made up of ____elements____ and are the smallest unit of a ___compound______ that retains the ________chemical characteristics____________ of that compound(ref. H2O, CH4, H2SO4, etc.).• Compounds are… ____Pure elements_________. A combination of 2 or more ___elements_____. Held together by ______chemical bonds_______ Atomic ratios by __mass___.Compounds & Molecules• A molecule is formed when two or more ___atoms__ join together ____chemically_____.• A compound is a molecule that contains at least two different ___elements_____. All compounds are ___molecules_______ but not all molecules are ______compounds____.• Molecular hydrogen (H2), molecular oxygen (O2) and molecular nitrogen (N2) are ___ __not compounds________ because each is composed of a _____single element _______.• Water (H2O), carbon dioxide (CO2) and methane (CH4) are ____compounds_____ because each is made from more than one __elements__.• The smallest bit of each of these substances would be referred to as a ___molecule_____.– For example, a single molecule of molecular hydrogen is made from two atoms of hydrogen while a single molecule of water is made from two atoms of hydrogen and one atom of oxygen.Compounds & MoleculesWhen forming a compoundThe ___properties_____ of each element is lost.Elements That Exist As Molecules_____Alletropes_____ of CDifferent forms of the ____ same element________Chemical FormulasMolecular Formulas• Formula for glycine is C2H5NO2• In one molecule there are– 2_ C atoms– 5_ H atoms– 1_ N atom– 2_ O atomsWriting Formulas• ____condensed_____ FormulaCan also write glycine formula asH2NCH2COOH to show atom ordering• ___structural _____ Formula Gives more structural detailEmpirical FormulasAn __Empirical______ formula is the simplest _____whole number_______ atom __ratio___ of a moleculeMolecular Formula - _C2H6____Empirical Formula - _CH3__Molecular ModelingMolecular Mass & Molar MassMolecular Weight & Molar MassMolecular weight = sum of the ______ atomic weights atoms of all the atoms in the molecule____. Molar mass = molecular weight in __grams___.What is the molar mass of ethanol, C2H6O?1 mol contains2_ mol C (12.01 g C/1 mol) = __24.02___ g C6_ mol H (1.01 g H/1 mol) = __6.06__ g H1_ mol O (16.00 g O/1 mol) = _16.00____ g OTOTAL = molar mass = __46.08___ g/molHow many moles of Ethanol are there in 21.3 g of C2H6O?(a) Molar mass of C2H6O = 46.08 g/mol(b) Calc. moles of alcoholHow many molecules of Ethanol are there in 21.3 g of C2H6O?= 2.78 x 1023 moleculesHow many atoms of C are there in 21.3 g of C2H6O?= 5.57 x 1023 C atomsIonic CompoundsIons & Ionic Compoundssee Screen 3.5IONS - atoms or groups of atoms with a ___positive_____ or ____negative____ charge. • CATION (___positive____ charge) ___loses___ an electron.• ANION (____negative____ charge) ___gaining____ an electron. Ion FormationReaction of aluminum and bromineCOMPOUNDS FORMED FROM IONSNa+ + Cl- --> NaClIonic CompoundsSome Ionic CompoundsCa2+ + 2 F- ---> CaF2Mg2+ + NO3- ----> Mg(NO3)2magnesium nitrateFe2+ + PO43- ----> Fe3(PO4)2iron(II) phosphateForming Cations & AnionsA ___cation____ forms when an atom loses one or more electrons.An ___anion___ forms when an atom gains one or more electronsFigure 3.5Predicting Ion ChargesIn general• ___metals___ (Mg) lose electrons ---> cations• _____nonmetals____ (F) gain electrons ---> anionsCharges on Common IonsMonoatomic & Diatomic IonsElements That Exist As Monoatomic IonsSingle ___atoms__ that have lost or gained ____electrons____Metals From Group 1A-3ACharge = ___group number________Predicting Charges on Monatomic IonsFigure 3.7Elements That Exist As Monoatomic IonsSingle __atoms___ that have lost or gained ___electrons_____Transition ElementsCharge - No __Easily__Predictible______ PatternPredicting Charges on Monatomic IonsFigure 3.7Elements That Exist As Monoatomic Molecules Single _atoms__ that have lost or gained ___electrons_____Nonmetals Charge = 8 - _____Group number_____Predicting Charges on Monatomic IonsFigure 3.7Elements That Exist As Diatomic MoleculesH2, N2, O2, F2, Cl2, Br2, I2Polyatomic IonsPolyatomic IonsGroups of atoms with a charge.____Memorize_____ the names and formulas in Table 3.1, page 107.Polyatomic IonsSO42- __sulfate____ ionSO32- __sulfite___ ionPolyatomic IonsNO3- __nitrate____ ionNO2- __nitrite___ ionPolyatomic IonsPO43- ____phosphate_____ ionCO32- _____carbonate____ ionPolyatomic IonsNH4+ _____ammonium_____ ionOne of the few common polyatomic _______Polyatomic IonsCO32- ___Carbonate______ ionHCO3- ______Bicarbonate_____ ionhydrogen carbonateNaming Ionic CompoundsMetalsM ---> n e- + Mn+where n = periodic groupNa+ ___sodium____ ionMg2+ _____magnesium_____ ionAl3+ ____aluminum_____ ionTransition metals --> M2+ or M3+ are commonFe2+ __iorn(II)___ ionFe3+ __Iorn(III)___ ionNonmetalsNONMETAL + n e- ------> Xn- where n = 8 - Group no.Naming Ionic CompoundsThe name of an Ionic Compound is built from the names of the ___positive_____ and ____negative____ ions in a compound.For Compounds with __Oxygen____, __Sulfur___, and the ___halogens_____, the H atom is written __first__. The other nonmetal is named like a ___negative ion______.Naming Ionic CompoundsCompound Ions Involved NameCaBr2 _Ca2+__ and 2 Br-________ _____Calcium Bromide__ ________NaHSO4 __Na+ and HSO4-_ ____ __Sodium Hydrogen Sulfate_ ___ _____Mg(OH)2 __Mg2+ and 2 OH-__ ______Magnesium Hydroxide__ _________TiCl2 __TI2+ and Cl-_ _ ___Titanium(II) Chloride________ ________Naming Molecular CompoundsNaming Molecular CompoundsAll Molecular Compounds are formed from two or more ___nonmetals______. As Opposed To…Ionic compounds generally involve a __metal___ and ___nonmetal____ (NaCl)Molecular CompoundsCompounds without IonsNaming Molecular CompoundsHydrogen Forms ____Binary Compounds_______ with all nonmetals.For Compounds with __oxygen__, __sulfer__, and the ___halogens_____, the H atom is written __first__. The other nonmetals are named like a __negative ion___.Naming Molecular CompoundsCompound Common nameHF ____Hydrogen___Flouride______HCl ____Hydrogen Chloride________HS2 ____Hydrogen Sulfide_________Naming Molecular CompoundsVirtually all binary molecular compounds of nonmetals are a combination of ___elements_____ from Groups _4A-7A___ with ___one another_______ or with ____hydrogen_____.The formula is generally written by putting the elements in orderof ___increasing group number__________.When naming the compound, the ___number____ of atoms of a given type are designated with a __prefix____:“ _Di-__ ” “ __Tri-_ ” “ ___Tetra-___ ” “___Penta-___” Etc.Naming Molecular CompoundsCompound Common nameNF3 ___Nitrogen_____Triflouride_________NO ___Nitrogen_____Monoxide_____NO2 ___Nitrogen____ _Dioxide_____N2O ___Dinitrogen_____ _monoxide _______PCl3 ____Phosphorous___ trichloride__________PCl5 ____Phosphorous___ _pentachloride___________SF6 ___Sulfur_____Hexaflouride_______S2F10 _____Disulfur__ ____Pentaflouride________Naming Molecular CompoundsMany Binary Compounds of nonmetals have common nameCompound Common nameCH4 ____Methane____C2 H6 ___Ethane___C3 H4 ____Propane___