CHEMISTRY 161 Chapter 3
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Transcript of CHEMISTRY 161 Chapter 3
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CHEMISTRY 161
Chapter 3
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1. Structure of an Atomsubatomic particleselectrons(cloud)protons(nucleus)neutrons(nucleus)m(n) / m(e) 2000 m(n) > m(p)
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2. Atomic & Mass Numberatomic number(number of protons)(number of electrons)mass number(number of protons plus neutrons)
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Compounds & Chemical Reactions Compounds
2. The Chemical Formula
3. The Chemical Equation
4. The Name of Chemicals
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1. Compoundsmolecular compoundsionic compoundsEXPI
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Molecular Compounds1. consist of electrically neutral particles called molecules 2. each molecule consists of atoms3. atoms are connected via electrons 4. connections are called bonds(springs)EXPII
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Molecular Compounds Group Period IVA VA VIA VIIA Noble Gas 2 CH4 NH3 H2O HF Ne 3 SiH4 PH3 H2S HCl Ar 4 GeH4 AsH3 H2Se HBr Kr 5 SbH3 H2Te HI Xelots of molecules contain hydrogenEXPIII
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H2, HeJupiterPH3CH4EXPIV
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H2, HeSaturnNH3/PH3CH4H2O (s)
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atom(neutral)add electron(s)(reduction)anion(Cl-)(negative charge)(non-metal)take electron(s)(oxidation)cation(Na+)(positive charge)(metal)Ionic Compounds I1. consist of charged particles2. charged particles are called ions3. ions are formed by electron transfers from atoms
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Ionic Compounds II4. ionic compounds are held together by electrostatic forcesmetalnon-metalNaClMgOEXPV
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Compounds & Chemical Reactions 1. Compounds
2. The Chemical Formula
3. The Chemical Equation
4. The Name of Chemicals
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2. The Chemical Formulacollection of chemical symbols used to describe the composition of elements and compoundsNaClH2OFe2O3CaSO4 2 H2O
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2. The Chemical Formulacollection of chemical symbols used to describe the composition of elements and compoundsEXPVI
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F2EXPVII
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O2
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S8
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N2
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P4
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H2
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Compounds & Chemical Reactions 1. Compounds
2. The Chemical Formula
3. The Chemical Equation
4. The Name of Chemicals
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3. The Chemical Equationchemical equation describes what happens in a chemical reactionchemical reaction is combination of elements and/or compoundsH2 + O2 H2Obalancing & mass conservation22
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3. The Chemical Equation2 H2 + O2 2 H2Os = solid l = liquid g = gas aq = aqueous solution2 H2(g) + O2 (g) 2 H2O (l)
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phosphor with oxygen2. sulfur with oxygenExamples3. methane with oxygen
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Compounds & Chemical Reactions 1. Compounds
2. The Chemical Formula
3. The Chemical Equation
4. The Name of Chemicals
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Organic Compoundscompounds containing mostly hydrogen and carbonminor amount other elements (N, O, S, P)hydrocarbonsHCalkanes CnH2n+2
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CO2COH2OH2COC4H10Organic Compounds?C4H10 combustionEXPVIII
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Titan Saturns Largest Moon
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Cassini-Huygens Mission
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Cassini-Huygens Mission
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Inorganic Compoundsbinary compoundscompounds consisting of ONLY TWO different elementsNaClCO2CaSO4nomenclaturenaming compoundsnomen (Latin) = name
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symbol stem first element second element O ox- oxygen oxide S sulf- sulfur sulfide N nitr- nitrogen nitride P phosph- phosphorus phosphide F fluor- fluorine fluoride Cl chlor- chlorine chloride Br brom- bromine bromide I iod- iodine iodidepart one (metal)part twoEnglish name ofelementstem + ideNaClMgOBeSMetal (Main Group) + Non-Metal
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ionic compounds(metal + non-metal)stem + ideNomenclature Inorganic Compoundsmain groupmetal element +
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ionic compounds(metal + non-metal)stem + ideNomenclature Inorganic Compoundsmain groupmetal element +molecular compoundsprefix + element +prefix + stem + ide
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Greek Prefixes mono- = 1 (often omitted) hexa- = 6 di- = 2 hepta- = 7 tri- = 3 octa- = 8 tetra- = 4 nona- = 9 penta- = 5 deca- = 10PF3PF5COCO2HClNONO2N2O5Molecular Compounds
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ionic compounds(metal + non-metal)stem + ideNomenclature Inorganic Compoundsmain groupmetal trans. groupmetal element +molecular compoundsprefix + element + prefix + stem + idestem + ideelement +oxstate +FeOFe2O3
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ionic compoundscations & anionsMn+Em-metalstransition metalsnonmetalscompounds must be electrically neutralcharge state of ions
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-/+3/5-2-10+1+2+3-/+2/4K2SCaCl2main group metals always start with cation
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NiCl2CuOCuCltransition metals always start with anionsoxidation statesMn2O3B2O3
Chromium
Cr2+, Cr3+Zinc
Zn2+
Manganese
Mn2+, Mn3+Silver
Ag+
Iron
Fe2+, Fe3+CadmiumCd2+
Cobalt
Co2+, Co3+Gold
Au+, Au3+
Nickel
Ni2+
Mercury
Hg22+, Hg2+
Copper
Cu+, Cu2+
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molecular compoundsionic compoundspolyatomic ionic compoundsammonium chloridesodium dichromatemagnesium carbonaterubidium sulfatecalcium phosphate
ion
name
ion
name
NH4+ammonium ionCO32-carbonate ion
OH-hydroxide ionH3O+hydronium ion
NO2-nitrite ion
SO32-sulfite ion
NO3-nitrate ion
SO42-sulfate ion
ClO2-chlorite ion
CrO42-chromate ion
ClO3-chlorate ion
Cr2O72-dichromate ion
PO43-phosphate ion
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ionic compounds(metal + non-metal)stem + ideNomenclature Inorganic Compoundsmain groupmetal trans. groupmetal element +molecular compoundsprefix + element + prefix + stem + idestem + ideelement +oxstate +
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Mass Percentage Composition P4O10=X 100 %=X 100 %
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Example
A sample was analyzed and contains 0.1417 g of nitrogen and 0.4045 g of oxygen. Calculate the percentage composition.1. mass of whole sample2. percentages of elements=X 100 %
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EMPIRICAL FORMULAH2OH2O2MOLECULAR FORMULAHOH2OH2OP4O10P2O5P2*2O2*5
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Example A sample contains 0.522 g of nitrogen and 1.490 g of oxygen. Calculate its empirical formula.
N2O5
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COMBUSTIONCxHyCO2H2OEXPIX
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COMBUSTIONC3H8CO2+ H2O0.013068 g+ O2How many grams of oxygen are consumed?balance equationconvert to moles
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The combustion of a 5.217 g sample of a compound of C, H, and O gave 7.406 g CO2 and 4.512 g of H2O.
Calculate the empirical formula of the compound.
How many grams of Al2O3 are produced when 41.5 g Al react?2Al(s) + Fe2O3(s) Al2O3(s) + 2 Fe(s)
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Compounds & Chemical Reactions Compounds
2. The Chemical Formula
3. The Chemical Equation
4. The Name of Chemicals
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ionic compounds(metal + non-metal)stem + ideNomenclature Inorganic Compoundsmain groupmetal trans. groupmetal element +molecular compoundsprefix + element + prefix + stem + idestem + ideelement +oxstate +