* Your assessment is very important for improving the workof artificial intelligence, which forms the content of this project
Download 10/18/11 - Note: Once it is downloaded, click SET
Bond valence method wikipedia , lookup
Atomic nucleus wikipedia , lookup
Computational chemistry wikipedia , lookup
Electrolysis of water wikipedia , lookup
Coordination complex wikipedia , lookup
Bremsstrahlung wikipedia , lookup
History of chemistry wikipedia , lookup
Molecular Hamiltonian wikipedia , lookup
Photoelectric effect wikipedia , lookup
Electronegativity wikipedia , lookup
Inductively coupled plasma mass spectrometry wikipedia , lookup
Low-energy electron diffraction wikipedia , lookup
Hypervalent molecule wikipedia , lookup
Electrochemistry wikipedia , lookup
Electrical resistivity and conductivity wikipedia , lookup
Metastable inner-shell molecular state wikipedia , lookup
Molecular orbital diagram wikipedia , lookup
Atomic orbital wikipedia , lookup
Auger electron spectroscopy wikipedia , lookup
Homoaromaticity wikipedia , lookup
IUPAC nomenclature of inorganic chemistry 2005 wikipedia , lookup
Stoichiometry wikipedia , lookup
Extended periodic table wikipedia , lookup
Gaseous detection device wikipedia , lookup
Resonance (chemistry) wikipedia , lookup
X-ray photoelectron spectroscopy wikipedia , lookup
Gas chromatography–mass spectrometry wikipedia , lookup
Photosynthetic reaction centre wikipedia , lookup
Rutherford backscattering spectrometry wikipedia , lookup
Chemical bond wikipedia , lookup
Metallic bonding wikipedia , lookup
History of molecular theory wikipedia , lookup
Metalloprotein wikipedia , lookup
Electron configuration wikipedia , lookup
10/18/11 Electrons Charge- negative Mass- 0 Location- outside the nucleus Electron Configuration- a way to describe the arrangement of the electrons around the nucleus of an atom. -arrangement -location -laid out Hund’s Rule- Each orbital is occupied before pairing begins. (orbital- probable location of each electron - at least 2 electrons per orbital - no electrons=no orbital) Quantum Numbers- a number that describes the properties of electrons and consists of 4 numbers (Quantum- a certain number) Pauli’s Exclusion Principle- only 2 electrons can occupy a single orbital 10/19/11 We can describe an electron in 2 ways. -Particle with a very small mass -Wave Electrons- determine chemical properties -“Chemistry” Nucleus- nuclear chemistry -tremendous energy (ex: the sun) Chemists describe electrons with: - Wave-particle duality - Quantum numbers - Periodic table Position of electron is energy which means orbitals are energy. 10/20/11 Orbitals- space where electrons could be found from Quantum numbers Sublevels- S- 1- up to 2 electrons P- 3- up to 6 electrons D- 5- up to 10 electrons F- 7- up to 14 electrons Aufbau Principle Lowest Energy Level Highest Energy Level 10/21/11 Electron Configuration PracticeBoron- 5 electrons 1s22s22p1 (2+2+1=5) Hydrogen- 1 electron 1s1 Be- 4 electrons 1s22s2 (2+2=4) Nitrogen- 7 electrons 1s22s22p3 (2+2+3=7) Silicon- 14 electrons 1s22s22p63s23p2 (2+2+6+2+2=14) Calcium- 20 electrons 1s22s22p63s23p64s2 (2+2+6+2+6+2=20) 10/24/11 valence electrons- electrons found in the outermost shell (energy level) of an atom - also determines the atom’s properties - outer shell electrons participate in chemicals reactions There are 7 shells (energy levels) Examples: Mg- 12 electrons valence electrons 2 6 2 1s22s 2p 3s outermost shell (2 valence electrons) Ar- 18 electrons 2 valence electrons 2 6 2 6 1s 2s 2p 3s 3p outermost shell (8 valence electrons) S- 16 electrons valence electrons 2 2 6 2 4 1s 2s 2p 3s 3p outermost shell (6 valence electrons) Electron Dots Mg: (2 valence electrons) .. ·S: (6 valence electrons) ˙ .. :Ar: (8 valence electrons) (octet rule- there can be, at most, 8 valence electrons) ˙˙ Ca: (2 valence electrons) 10/25/11 Quiz review Chapter 3.3- Electron Configuration What’s involved? Periodic table, electron, atomic number Electrons are arranged in orbitals around the nucleus Things to know: -Hund’s Rule, Aufbau Principle, Pauli’s Exclusion Principle -Electron Dot- shows how many valence electrons it has. -SPDF (orbitals) S- 1- up to 2 electrons P- 3- up to 6 electrons D- 5- up to 10 electrons F- 7- up to 14 electrons - Valence electrons are found in the outer shell - Atoms are mostly space Examples: Ca- 20 electrons 1s22s22p63s23p64s2 Ar- 18 electrons 1s22s22p63s23p6 Cl- 17 electrons 1s22s22p63s23p5 (2 valence electrons) Ca: .. (8 valence electrons) :Ar: ˙˙ .. (7 valence electrons) :Cl: ˙ Chapter 4 Periodic Law- the properties of the elements are a periodic function of their atomic number. (repeats itself) -Elements in each column of the periodic table have the same number of valence electrons in their outer shell. Group or Column- vertical- all have the same properties Period or Row- horizontal (energy levels)- same energy levels 10/26/11 Main Group Elements (Representative Elements) S-Block (groups 1-2) P-Block (groups 13-18) Group1-Alkali metals -1 valence electron - Li, Na, K, Rb, Cs, Fr Group2- Alkaline Earth Metals - 2 valence electrons - Be, Mg, Ca, Sr, Ba, Ra Group17- Halogens - Highly reactive (really close to having a full outer shell) - F, Cl, Br, I, At Group18- Noble gases - full outer shell, unreactive (8 valence electrons) - Ne, Ar, Kr, Xe, Rn 10/27/11 Metals - conduct electricity (conductors) - malleable (can be shaped) - ductile (drawn out into wire) - left side of “staircase” on periodic table Transition Metals - D-block elements (groups 3-12) - Lanthanides - Actinides (radioactive) F- block Nonmetals - right of “staircase” - not conductors Metaloids - touching “staircase” - semi conductors Big Bang Theory- Elements were created from Hydrogen being condensed in stars. 11/2/11 Periodic Trends 1) Atomic Radius- distance from the nucleus to the edge of the electron cloud increases decreases Electron cloud 2) 3) 4) 5) 6) -Bond Radius – half the distance between bonding atoms (nucleii) Electron Affinity- energy change when a neutral atom gains an electron Electronegativity- the measure of the ability of an atom in a compound to attract electrons decreases increases Ionic Size- the increase or decrease in the size of an atom when it gains or loses electrons (ion- an atom with a charge) Ionization Energy- the energy required to remove an electron from an atom or ion BP/MP(boiling point/melting point)- changes in state due to energy changes 11/9/11 Chemists measure moles Atomic Mass - Atomic Mass Unit P+= 1AMU N0= 1AMUmass of nucleus e- = 0AMU The Mole 1 mole = 6.02x1023 Mole - defined in terms of carbon - the number of atoms in exactly 12 grams of the carbon isotope-12 - 1 mole = atomic mass on periodic table Molar Mass- the mass, in grams, of 1 mole of an element - g/mol - the mass of 1 mole of an element = the element’s atomic mass (from P.T.) Avogadro’s Number- the number of particles in 1 mole of a substance grams moles #particles moles Examples: Given: x grams oxygen ? moles oxygen x grams oxygen 1 mol oxygen 16 grams oxygen Given: x moles calcium ? grams calcium x moles calcium 40 g calcium 1 mol calcium = x/16 = = x40 = a mol oxygen a g calcium HW Review: 1) Given: 1 mol U ? mass U 1 mol U 238 g U = 1238 = 238gU 1 mol U 2) Given: .0050 mol U ? mass U .0050 mol U 238 g U = .0050238 = 1.19gU 1 mol U 3) Given: .850gH ? moles H .850 gH 1molH = .8501 = .850molH 1gH Given: .850molH ? mass in gH .850 molH 1gH = .8501 = .850gH 1molH 4) Given: 2.3456molPb ? mass in gPb 2,3456molPb 207.2gPb = 2.3456207.2 = .486gPb 1molPb Given: 2.3456gPb ? molPb 2,3456gPb 1molPb = 2.3456/207.2 = .01132molPb 207.2gPb 11/15/11 23 1mol=6.02x10 Example: Given: 0.30molF ? # atoms F 0.30molF 6.02x1023atomsF = .306.02x1023 = 1.8x1023atomsF 1molF Given: 3.01x1023SO2 ? mol SO2 3.01x1023 atomsSO2 1molSO2 = 3.01x1023/6.02x1023 = .5molSO2 23 6.02x10 atomsSO2 11/18/11 Practice: Given: 3.01x1023SO2 ? mol SO2 3.01x1023 atomsSO2 1molSO2 = 3.01x1023/6.02x1023 = .5molSO2 23 6.02x10 atomsSO2 Given: 25gF ? molF 25gF 1molF 19gF = 25/19= 1.32molF 11/28/11 Find the mass, in grams, of 2.44x1024atomsC (particlesmass) 2.44x1024atomsC 1 molC 12gC = 2.44x102412 = 48gC 23 6.02x10 atomsC 1molC 6.02x1023 11/28/11 Molar Mass (7.2) mass of each element from P.T. CaCO3 1Ca: 1x40= 40 1C: 1x12= 12 3O: 3x16= +48 100g/mol molar mass of CaCO3 CaSO3 1Ca: 1x40= 40 1S: 1x32= 32 3O: 3x16= +48 120g/mol molar mass of CaSO3 Al(NO3)3 1Al: 1x27= 27 3N: 3x14= 42 9O: 9x16= +144 213g/mol molar mass of Al(NO3)3 11/29/11 HW Review 7a) ? ions 3molNa2CO3 2molNa2+ 6.02x1023ions = 6.02x102332= 3.61x1024ions 1molNa2CO3 1molNa2+ 8a) ? moles 3.01x1023moleculesH2O 9a) ? mass 4.30x1016atomsHe 1molH2O = 3.01x1023/6.02x1023= .5molH2O 23 6.02x10 moleculesH2O 1molHe 4gHe = 4.30x1016 4 = 2.86x10-7gHe 6.02x1023atomsHe 1molHe 6.02x1023 10a) ? ions 1gI- 1molI- 6.02x1023ionsI- = 6.02x1023/126.9= 4.74x1021ionsI126.9gI- 1molI11a) ? mass 6.02x1023moleculeIb 1molIb 206.31gIb = 6.02x1023206.31= 206.31gIb 6.02x1023moleculeIb 1molIb 6.02x1023 12a) ? mass 4.01x1023atomsCa 1molCa 40.08gCa = 64.01x102340.08 = 26.7gCa 23 6.02x10 atomsCa 1molCa 6.02x1023 13a) ? molecules 2.00molH2 6.02x1023moleculesH2 = 6.02x10232 = 1.204x1024moleculesH2 1molH2 Notes KCl 2 atoms 1K: 1x40 = 40 1Cl: 1x35.5= +35.5 molar mass 75.5g/mol Fe2O3 5 atoms 2Fe: 2x55.85 = 111.7 3O: 3x16 = +48 molar mass 159.7g/mol C6H12O6 24 atoms 6C: 6x12 = 72 12H: 12x1 = 12 6O: 6x16 = +96 molar mass 180g/mol 11/30/11 Do Now: Find the Molar Mass KClO4 1K: 1x39 = 39 1Cl: 1x35.5= 35.5 4O: 4x16 = +64 139.5g/mol (NH4)2SO4 2N: 8H: 1S: 4O: 2x14 = 28 8x1 = 8 1x32 = 32 4x16 = +64 132g/mol MUST KNOW THIS: 1mol or 23 6.02x10 1mol molar mass or atomic mass or 6.02x1023 1mol molar mass or atomic mass 1 mol Practice 1) Calculate the grams in 1 molCaCl2 1Ca: 1x40 = 4 1molCaCl2 111gCaCl2 = 111gCaCl2 2Cl: 2x35.5 = +71 1molCaCl2 111g/mol 2) Calculate the grams in 3molCO2 1C: 1x12 = 12 3molCO2 44gCO2 = 132gCO2 2O: 2x16 = +32 1molCO2 44g/mol 3) 2) Calculate the number of moles in 32gCH4 1C: 1x12= 12 32gCH4 1molCH4 = 2molCH4 4H: 4x1 = + 4 16gCH4 16g/mol 4) 2) Determine the mass of 40 moles of Na2CO3 2Na: 2x23= 46 40molNaCO3 106gNaCO3 = 4240gNaCO3 1C: 1x12= 12 1molNaCO3 OR 3O: 3x16= +48 4.24x103gNaCO3 106g/mol pg 239 1a)CsI 1Cs:1x133= 133 1I: 1x127= +127 260g/mol b)CaHPO4 1Ca: 1x40 = 40 1H: 1x1 = 1 1P: 1x31 = 31 4O: 4x16 =+64 136g/mol c) C12H22O11=342g/mol d) I2=254g/mol e) HC2H3O2=60g/mol f) Mg3(PO4)2=262g/mol 3a) C6H5CH3=92g/mol b) ?moles 7.51gToluene 1molToluene = .08molToluene 92gToluene 4a) PtCl2(NH3)2= 299g/mol b) Find the mass of 4.115x1021 F.U. PtCl2(NH3)2 4.115x1021 FU 1mol PtCl2(NH3) 299g PtCl2(NH3)2 =2.04gPtCl2(NH3)2 6.02x1023FU 1mol PtCl2(NH3)2 12/2/11 Examples: CuNH4Cl3 1) How many elements? 4 (Copper, Nitrogen, Hydrogen, Chlorine) 2) How many atoms? 9 3) How many H atoms in 1 mole CuNH4Cl3? 6.02x10234=2.408x1024atomsH 4) How many Cl atoms in 6 moles CuNH4Cl3? 6.02x102336=1.08x1025atomsCl 5) What is the mass in grams of 1 molecule CuNH4Cl3? 1CuNH4Cl3 1molCuNH4Cl3 299g PtCl2(NH3)2 =2.04gPtCl2(NH3)2 23 6.02x10 CuNH4Cl3 1molCuNH4Cl3 6) How many moles would be in 6.84gCuNH4Cl3? 6.84gCuNH4Cl3 1molCuNH4Cl3 =.0367CuNH4Cl3 186.55gCuNH4Cl3 12/5/11 7.2 & 7.3 Chemical Formulas - Express Composition ex: H2O Hydrogen and Oxygen - Used to calculate molar mass - Give ratios of Polyatomic Ions (2 atoms) (has a charge) ex: C6H12O6 Ca(OH)2 Percent Composition -percent, by mass, of each element in a compound molar mass of the part molar mass of the whole ex: XeF4 1Xe: 1x131= 131 %Xe: Xe = 131 100 = 63.3% 4F: 4x19 =+76 XeF4 207 207 %F: F4 = 76 100 = 36.7% XeF4 207 ex: Fe2O3 2Fe: 2x56= 112 %Fe: Fe2 = 112 100 = 70% 3O: 3x16=+48 Fe2O3 160 160 %O: O3 = 48 100 = 30% Fe2O3 160 Empirical Formula- A chemical formula that shows the composition of a compound in terms of the relative numbers and kinds of atoms in the simplest ratio. ex: C6H12O6= CH2O ex: Ammonium Nitrate Actual Formula: NH4NO2 (or N2H4O2) Empirical Formula: NH2O (simplest ratio) Start with % composition- chemical analysis Ex: Sample problem G (from text) Given: C: 60.0% H: 13.4% O: 26.6% Empirical Formula? 1) Assume you are given 100g sample Convert %’s to grams C: 60.0%60gC H: 13.4%13.4gH O: 26.6%26.6gO 2) Convert gmoles C: 60gC 1molC = 5molC 12gC H: 13.4gH 1molH = 13.4molH 1gH O: 26.6gO 1molO = 1.67molO 16gO 3) Divide each number of moles by the smallest mole. 5/1.67=3 13.4/1.67=8 new subscripts in chemical formula 1.67/1.67=1 (if these are not whole numbers or close to it, you must multiply the equation by a number until they are whole numbers) 4) Empirical Formula = C3H8O 12/6/11 Do Now: Determine the molar mass of C4H3FN2O2, Fluorouracil Cream. What is its Empirical Formula? 4C: 4x12= 48 3H: 3x1 = 3 1F: 1x19= 19 2N: 2x14= 28 2O: 2x16= +32 130g/mol Empirical Formula: C4H3FN2O2 (subscripts are already in the simplest ratio) HW Review (pg 243 1-4) 1)Mn2O3 2)Cl= 38.77%38.77gCl 1molCl 1molCl 35.5gCl 2(ClO3.8) = Cl2O7 O= 61.23%61.23gO 3)Fe= 72.4%72.4gFe 1molO 3.8molO 16gO 1molFe 1.3molFe 55.8gFe O= 27.6%27.6gO 1molO 1.7molO 16gO 1.3/1.3= 1 (divide by the smallest mole) 1.7/1.3=1.3 3(FeO1.3)= Fe3O4 4) C= 18.0%18.0gC 1molC =1.5molC 12gC 1.5/1.5= 1 H= 2.26%2.26gH 1molH =2.26molH 1gH 2.26/1.51.5 Cl= 79.7%79.7gCl 2.28/1.51.5 1molCl =2.28molCl 35.5gCl 2(CH1.5Cl1.5)= C2H3Cl3 Empirical Formula- the simplest whole number ratio of atoms in a compound -Sometimes empirical formulas and molecular formulas are the same. ex: H2O Empirical and molecular formula HNO3(nitric acid) Empirical and molecular formula Molecular formulas are often whole number ratios of the empirical formula. Molar Mass of a compound is equal to the molar mass of the empirical formula times a whole number. 12/7/11 HW Review (pg 248 1-5, 7) 1)a. Given the % composition, we need the atomic mass from the periodic table to find the empirical formula. b. Experimental molar mass 2) Molecular Formula- C8H18 Empirical Formula- C4H9 (lowest ratio) 3) You need the molar mass. 5) Experimental molar mass: 64g/mol ? molecular formula (exp. Molar mass)64g/mol= 1(SO2)=SO2 (from 4b, we know the empirical formula is SO2) (emp. Molar mass)64g/mol 7) AgC2H3O2 1Ag:1x108= 108 Ag = 108 = 64.62%Ag 2C = 24 = 14.39%C 2C: 2x12 = 24 AgC2H3O2 167 AgC2H3O2 167 3H: 3x1 = 3 2O: 2x16 = +32 3H = 3 = 1.82%H 2O = 24 = 19.17%O 167g/mol AgC2H3O2 167 AgC2H3O2 167 Notes n(Molar Mass of Emp. Formula)= Molar Mass of Molecular Formula Sample H (from text pg 245) Given: Empirical Formula- P2O5 Experimental Molar Mass- 284g/mol ? Molecular Formula P2O5 2P: 2x31= 62 (exp molar mass)284g/mol = 2(P2O5)= P4O10 5O:5x16= +80 (emp molar mass)142g/mol 142g/mol 12/8/11 Do Now: Find the % composition of NaClO Na = 23 = 30.89%Na Na:1x23 = 23 NaClO 74.45 Cl: 1x35.45= 35.45 O: 1x16 = +16 Cl = 35.45 = 47.61%Cl 74.45g/mol NaClO 74.45 O = 16 = 21.49%O NaClO 74.45 HW Review(pg 245 1-3) 1) Given: Experimental Molar Mass- 78g/mol Empirical Formula- CH C: 1x12= 12 (exp molar mass)78g/mol = 6(CH) = C6H6 H: 1x1 =+1 (emp molar mass)13g/mol 13g/mol 2) Given: Experimental Molar Mass- 90g/mol Empirical Formula- CH2O C: 1x12= 12 (exp molar mass)90g/mol = 3(CH2O) = C3H6O3 H: 1x1 = 1 (emp molar mass)30g/mol O: 1x16=+16 30g/mol 3) Given: Experimental Molar Mass- 46g/mol Empirical Formula- NO2 N: 1x14= 14 (exp molar mass)46g/mol = 1(NO2) = NO2 O: 2x16=+32 (emp molar mass)46g/mol 46g/mol Chapter 8 (8.1) Chemical Equations -chemical reactions rearrange atoms, but the number and kind of atoms remain the same. 2Na+2H2O2NaOH+1H2 2Na2Na 4H4H 2O2O Due to the Law of Conservation of Mass, chemical equations must be balanced. 12/9/11 Do Now: Find the Empirical Formula for: 63.52%K63.52gK 1molK = .68molK 39gK .68 =1 35.35%Cr35.35gCr 1molCr = .68molCr 52gCr .68 =1 38.07%O38.07gO 1molO = 2.38molO 16gO .68=3.5 Chemical Equations Reactants yields Products 2(KCrO3.5)= K2Cr2O7 Solid-s Liquid-l Gas-g Solid dissolved in water- aq (aqueous) Writing Balanced Chemical Equations: - Determine the reactants and products - Assemble the equation - Balance the equation - # all reactant atoms = # all product atoms When you balance chemical equations, you can only add numbers in front of the elements or compounds. 12/12/11 Do Now- Determine the % composition of Fe(OH)2 Fe: 56 Fe = 56 = 62.2%Fe 2O = 32 = 35.5%O 2O: 32 Fe(OH)2 90 Fe(OH)2 90 2H: +2 90g/mol 2H = 2 = 2.2%H Fe(OH)2 90 HW Review 4c) Sodium Hydrogen CarbonateSodium Carbonate + Carbon Dioxide + Water 2NaHCO3 Na2CO3+CO2+H2O (we balance because of the Law of Conservation of Mass) 5c) 3 AgNO3 + AlCl3 3 AgCl + Al(NO3)3 7) Any compound with 2 molecules containing 2 atoms P each 4 atoms P ex: 4Al(NO3)3 4Al 12N 36O Notes Balancing Chemical Equations Coefficients- the number in front of the formula - multiplies the number of each element in the formula that follows ex: 2H2O2H2 + O2 ex: Ca(NO3)2 3Ca(NO3)2 1Ca 3Ca 2N 6N 6O 18O - Never Change subscripts - Polyatomic ions can be balanced as a unit C3H8 + 5 O2 3 CO2 + 4 H2O 3C 3C 8H 8H 10 O 10 O 12/13/11 Do Now- Balance the Chemical Equations 2 Al + Fe3N2 2 AlN + 3 Fe 2 Na + Cl2 2 NaCl 2 H2O2 2 H2O + O2 HW Review (pg 285 #8 balance only) 8)a. Cl2 + 2NaBr 2NaCl + Br2 b. CaO + H2O Ca(OH)2 c. Ca(ClO3)2 CaCl2 + 3O2 d. 2AgNO3 + K2SO4Ag2SO4 + 2KNO3 e. already balanced as written f. 2C8H18 + 25O216CO2 + 18H2O Types of Chemical Reactions Single Displacement Rxn- one element displaces (or replaces) another in a compound Ex: A + BC=B + AC Ex: 2Al(s) + 3CuCl2(aq)3Cu(s) + 1AlCl3(aq) Double Displacement Rxn- positive and negative portions of 2 compounds are interchanged. Ex: AB + CD AD + CB Ex: HCl + NaOH HOH + NaCl (or H2O) Decomposition Rxn- substances break up into simpler substances when energy is applied. Ex: ABA + B Ex: 2H2O electricity 2H2 + O2 Synthesis Rxn- Two or more substances combine to form a new substance. Ex: A + B AB Ex: C + O2 CO2 Combustion Rxn- Oxidation reaction of an organic compound in which energy is released. Every combustion has O2, CO2, and H2O. Ex: + O2 CO2 + H2O + energy Ex: C3H8 + 5O23CO2 + 4H2O + energy 12/14/11 Do Now- Balance and name the type of reaction 2Na + Cl2 2NaCl Synthesis Rxn C6H12O6 + 6O2 6H2O + 6CO2 Combustion Rxn 4(NH4)3PO4 + 3Pb(NO3)4 Pb3(PO4)4 + 12NH4NO3 Double Disp Rxn 2BF3 + 3Li2SO3 B2(SO3)3 + 6LiF Double Disp Rxn 8Ag2S16Ag + S8 Decomposition Rxn Notes Chemical Reactions are like recipes -show the physical state -reaction conditions Ex: N2(g)+ 3H2(g) catalyst 2NH3(g) Symbols: (s)(l)(g)- physical state (aq)- dissolved in water heat or add energy catalyst name or formula of catalyst reversible reaction 12/15/11 Do Now 1) Determine the molar mass of (NH4)2SO4 2N: 2x14= 28 8H: 8x1 = 8 4O: 4x16 = 64 1S: 1x32 = +32 132g/mol 2)Find the empirical formula for: Given: 50.1%S50.1gS 50.1gS 1molS = 1.565 =1 49.9gO 1molO = 3.12=2 SO2 49.9%O49.9gO 32gS 1.565 16gO 1.565 3)Given the experimental Molar Mass of 64g/mol, find the molecular formula. 2O: 2x16 = 32 1S: 1x32 = +32 64g/mol = (64g/mol) n n=1(SO2)=SO2 64g/mol 64g/mol 64g/mol Balance: 2Ag(CH3COOH)+CaCl2 Ca(CH3COOH)2+2AgCl (double displacement reaction) HW Review (pg 285 1-10) 1) 2 smaller compounds come together to form a larger one. 6) They are very reactive so they replace other elements. 7) For a double displacement reaction, 2 new compounds must be produced. 10) a) 2HgO2Hg+O2 (decomposition) b) 2C3H7OH+O26CO2+8H2O (combustion) c) Zn+CuSO4ZnSO4+Cu (single replacement) d) BaCl2+Na2SO4BaSO4+Na2Cl2 (double displacement) e) Zn+F2ZnF2 (synthesis) f) C5H10+O2C5O2+H10 (single displacement) Notes-Stoichiometry 2C3H2OH + 9O2 6CO2+8H2O -Balanced: massR=massP -combustion reaction 12/16/11 Do Now 1) What is the % composition of CuCl2? CuCl2=1Cu: 1x63.55= 63.55 Cu:63.55100=48% 2Cl: 2x35.45= +70.90 134.45 134.45g/mol 2) Balance: CaCo3(S)CaO(S)+CO2 3) What type of reaction is this? Decomposition 4) What do these mean? (s): solid (l): liquid (g): gas (aq): aqueous 5) Why do we use an activity series? To predict reaction activity. Cl2:70.90 100=52% 134.45 12/20/11 Do Now- Define the following: Mole- 6.02x1023 particles, atoms, molecules, ions Molar Mass- mass in grams of 1 mole of a substance Chapter 9- Stoichiometry 1mole 5moles 3moles 4moles C3H8 + 5 O2 3 CO2 + 4 H2O (combustion reaction) atoms = atoms mass = mass energy = energy MOLES = MOLES - need a balanced chemical equation - Coefficients give the amounts of reactants and products - Mass-Mass Problems 12/21/11 Do Now- pg 304 #1 Calculate the amount requested if 1.34 mol H2O2 completely reacts according to the following equation: 2H2O22H2O + O2 a)moles of oxygen formed? Given: 1.34 mol H2O2 1.34molH2O2 1molO2 = .67molO2 Unknown: ?molO2 2molH2O2 b)moles of water formed? Given: 1.34 mol H2O2 Unknown: ?molH2O 1.34molH2O2 2molH2O = 1.34molH2O 2molH2O2 HW Review (pg 311 #1-7) 5) 2C2H2(g) + 5O2(g)4CO2(g) + 2H2O(g) a) given:15.9L C2H2 15.9L C2H2 1molC2H2 4molCO2 = 1.4molCO2 ? molCO2 22.4L C2H2 2molC2H2 (hint: 1molC2H2=22.4L C2H2) 4) Br2 + Cl2 2BrCl a) 2.74molCl2 1molBr2 = 2.74molBr2 1molCl2 b) 239.7gCl2 1molCl2 35.4gCl2 c) 4.53x1025Cl2 2molBrCl 1molCl2 115.4gBrCl = 1562.8gBrCl 1molBrCl 1molCl2 1molBr2 159.8gBr2 = 12024.82gBr2 6.02x1023Cl2 1molCl2 1molBr2 12/22/11 Mole Ratio- uses coefficients -Molesknown (or given)mole ratiomolesunknown -Molesgiven Molesunknown Mole Molesgiven ratio C6H12O6 + 6O26CO2 + 6H2O + energy Coefficients are in green, tell us the number of moles Do Now Fe2O3 + 2Al2Fe + Al2O3 a) ?molesAl MOLE RATIO given: 3.3molFe2O3 3.3molFe2O3 2molAl = 6.6molAl 1molFe2O3 b) ?molFe MOLE RATIO given: 3.3molFe2O3 3.3molFe2O3 2molFe = 6.6molFe 1molFe2O3 MOLE RATIO c) ?molAl2O3 3.3molFe2O3 1molAl2O3 = 3.3molAl2O3 1molFe2O3 12/23/11 Do Now: Fe2O3 + 2Al2Fe + Al2O3 1) Given: 135gFe2O3 ?gAl 135gFe2O3 1molFe2O3 2molAl 27gAl = 45.6gAl 160gFe2O3 1molFe2O3 1molAl 2) Given: 23.6gAl ?gAl2O3 23.6gAl 1molAl 2molAl2O3 102gAl2O3 = 44.5gAl2O3 27gAl 1molAl 1molAl2O3 3) Given: 475gFe ?gFe2O3 475gFe 1molFe 1molFe2O3 160gFe2O3= 679gFe2O3 56gFe 2molFe 1molFe2O3 1/3/12 Do Now Write 23800 in scientific notation: 2.38x104 Balance : 4Fe(s) + 3O2(g) 2Fe2O3(s) L#Atoms #Moles State of Molar Mass 4 3 2 55.8g/mol 32g/mol 159.6g/mol Products Reactants Mole Ratio (or flipped) R Fe O2 Fe2O 4 6 4 6 2 S G S Fe O2 Fe2O3 4molFe/3molO2 3molO2/2molFe2O3 4molFe/2molFe2O3 3 Br2(l)+5F2(g)2BrF5(l) (synthesis reaction) ?moleculesBrF5 Given: 384gBr2 384gBr2 1molBr2 2molBrF5 6.02x1023moleculesBrF5 = 2.89x1024moleculesBrF5 160gBr2 1molBr2 1molBrF5 1/4/12 Do Now - Where are p+ and no found? In the nucleus of an atom. - Where are the e-‘s mostly to be found? In the electron cloud. - Which subatomic particle does not carry a charge? Neutron - Atomic number of an element = number of protons - Mass # of an element with 12p+ and 13no is? 25 - What is the electron configuration for oxygen? 1s22s22p4 Br2(l)+5F2(g)2BrF5(l) ? moleculesBr2 Given: 1.11x1020moleculesF2 1.11x1020molecF2 1molF2 1molBr2 6.02x1023molecBr2 = 2.22x1019molecBr2 23 6.02x10 molecF2 5molF2 1molBr2 Ratios: Molar Mass: 1mol/g OR g/1mol Avogadro’s Number: 1mol/Avogadro’s Number OR Avogadro’s Number/1mol Mole Ratio: GivenMol/UnknownMol OR UnknownMol/GivenMol (from balanced chemical equation) What mass of H2O is produced if 65.2gCaCO3 reacts with H3PO4 to form Ca3(PO4)2,H2O, and CO2? 3CaCO3 + 2H3PO4 Ca3(PO4)2 + 3H2O + 3CO2? ?massH2O 65.2gCaCO3 1molCaCO3 3molH2O 18gH2O = 100gCaCO3 3molCaCO3 1molH2O Do Now . Write Electron dot for Boron-B? B How many valence electrons are in Argon-Ar? 8 What is the total number of e-‘s in Li+? 2e-‘s What are the 4 orbitals? S(sphere), P(dumbbells), D, F How many shapes does each one have? 1, 3, 5, 7 (respectively) How many e-‘s can each one hold? 2, 6, 10, 14 (respectively) (reactants) 1/5/12 (products) Notes- Stoichiometry A+ B AB Limiting Reactant- the substance that controls the quantity of the product that can be formed in a chemical reaction. The limiting reactant forms the least amount of product. (runs out) Excess Reactant- the substance that is not used up completely in a reaction. HW (pg 319 #1,2,8) 1/6/12 Theoretical yield- the maximum quantity of product that a reaction could make if everything works perfectly. Actual yield-the mass of the product actually formed. Why? -The actual yield is less than the theoretical yield. - Many reactants do not completely use up limiting reactants. - Purification - Unwanted “side reactions” Do Now Who developed the PT? Mendeleev How are the elements arranged on the PT? Increasing atomic number Where are the: Alkali metals: group 1 Alkali Earth Metals: group 2 Metals: left side of staircase Nonmetals: right side of staircase Halogens: group 17 Noble Gases: group 18 Transition Metals: d block S: from block 1-2 P: from block 13-18 D: from block 3-12 F: from Lanthanide-Actinide series What are vertical columns called? Families/groups What are horizontal rows called? Periods 1/10/12 Do Now What is the most reactive nonmetal? Fluorine Define: Atomic Radius- distance from the nucleus to the edge of the electron cloud Electronegativity- the measure of the ability of an atom in a compound to attract Electrons Notes moles(unknown)/moles(given)(mole ratio) 1mole/6.02x1023(Avogadro’s Number) 1mole/molar mass(PT) 1mole/22.4liters (molar volume) PCl3+3H2OH3PO4+3Hcl g g mol mol g mol % yield- actual yield x100 theoretical yield 1/11/12 Do Now 1) 6.02x1023=1mole (Avogadro’s number) 2) How many moles of CO2 are present in 11.2L? 11.2LCO2 1molCO2 = .5molCO2 22.4LCO2 3) What is the %mass of Mg in MgO? Mg= 24 x100 = 60%Mg MgO= 40 4) Define theoretical yield- the maximum quantity of product that a reaction could make if everything works perfectly. % yield- actual yield x100 theoretical yield Notes Determine the limiting reactant, theoretical yield and %yield if 14.0gN2 are mixed with 9gH2 and 16.1gNH3 form. N2+3H22NH3 14g 9g 16.1g (actual yield) 14gN2 1molN2 2molNH3 17gNH3 = 17gNH3 theoretical yield 28gN2 1molN2 1molNH3 (17 is smaller then 51 so N2 is the limiting reactant) 9gH2 1molH2 2molNH3 17gNH3= 51gNH3 2gH2 3molH2 1molNH3 %yield- actual yield = 16.1g x100 = 94.7% theoretical yield 17g 1/12/12 Do Now- balance and classify 4Al+3O22Al2O3 (synthesis) AlCl3+3NaOHAl(OH)3+3NaCl (double displacement) 2NaCl2Na+Cl2 (Decomposition) Ba+2HClBaCl2+H2 (single replacement) HW Review (pg 319 #7) Determine the theoretical yield if 100gP4O10 are mixed with 200gH2O. P4O10+6H2O4H3PO4 100gP4O10 1molP4O10 4molH3PO4 98gH3PO4 = 138gH3PO4 theoretical yield 284gP4O10 1molP4O10 1molH3PO4 200gH2O 1molH2O 4molH3PO4 98gH3PO4 = 544gH3PO4 18gH2O 6molH2O 1molH3PO4 %yield- 126.2gH3PO4 x100 = 91.4% 138gH3PO4 1/13/12 Notes P4+10Cl24PCl5 What quantity, in moles Cl2, reacts with 4.0 moles of P4? 4molP4 10molCl2 = 40molCl2 1molP4 3NO2+H2ONO+2HNO3 How many moles of water are needed to react with 8.4 moles NO2? 8.4molNO2 1molH2O = 2.8 molH2O 3molNO2 P4+6F24PF3 How many grams of Fluorine are needed to react with 6.2g of phosphorous? 6.2gP 1molP 6molF2 38gF2 = 45.6gF2 31gP 1molP 1molF2 H2O+SO3H2SO4 If 36gH2O is used, how many moles of H2SO4 is made? 36gH2O 1molH2O 1molH2SO4 98gH2SO4 = 196gH2SO4 18gH2O 1molH2O 1molH2SO4 1/16/12 Do Now 4Al+3O22Al2O3 ?gO2 8) given: 27gAl 1molAl 3molO2 32gO2 = 24gO2 27gAl 4molAl 1molO2 this graduated cylinder measures to 70.3mL What is the last thing you do in a lab? Wash your hands. Notes Significant figures in measurements -Significant figures in a measurement include all of the digits that are known, plus one more digit that is estimated. -Measurements must be reported to the correct number of significant figures. Rules for counting significant figures -Non-zeroes always count as significant figures - 3456 had 4 significant figures Zeros - Leading zeroes do not count as significant figures. - 0.0486 has 3 significant figures - Captive zeroes always count as significant figures - 16.07 has 4 significant figures 1/17/12 Do Now A cube has a mass of 20 grams and a volume of 8.5mL. What is its density? D=m/v=20g/8.5mL=2.35g/mL What is the composition of Cl-35? p+=17, e-=17, no=18 What is the electron configuration for N? 1s22s22p3 How many moles are present in 27gH20? 27gH2O 1molH2O = 1.5molH2O 18gH2O Notes- Sig Figs Zeros - Trailing zeros are only significant if the number contains a written decimal point - 9.300 has 4 significant figures Two special situations have an unlimited number of significant figures - Counted items (ex- 23 people or 425 thumbtacks) - Exactly defined quantities (60 minutes = 1 hour) Sig Fig Practice#1 1.0070m = 5 sig figs 17.10kg = 4 sig figs 100,890L = 5 sig figs 3.29x103s = 3 sig figs 0.0054cm = 2 sig figs 3,200,000mL = 2 sig figs 5 dogs = unlimited sig figs (counted value) - In general, a calculated answer cannot be more precise than the least precise measurement from which it was calculated. - Ever heard that a chain is only as strong as the weakest link? - Sometimes, calculated values need to be rounded off Rounding Calculated Answers - Decide how many significant figures are needed (more on this very soon) - Round to that many digits, counting from the left. - Is the next digit less than 5? Drop it - Next digit 5 or greater? Increase by 1 1/18/12 Do Now Define: Hypothesis- a reasonable and testable explanation for observations Mass- the quantity of matter in an object (grams) Kinetic energy- The energy of an object that is due to the objects motion. Energy- the capacity to do work How many grams is 3.75kg? 3750g HW Review(pg 63 1-11) 6a) 0.8102mx3.44m = 2.79m2 b) 94.20g/3.16722mL = 29.74g/mL 7) 63J/8.0g(340k-314k) = .30J/gk 8a)129g/29.2mL = 4.42g/mL 11) 11.50g/9.03mL = 3 sig figs Notes- Sig Figs Addition and Subtraction- The answer should be rounded to the same number of decimal places as the least number of decimal places in the problem. Multiplication and Division - round your answer to the same number of significant figures as the least number of significant figures in the problem. - # sig figs in the result equals the number in the least precise measurement used in calculation. - 6.38x2.0 = 12.76 = 13 (2 sig figs) Sig Fig Practice#2 Calculation Calculator Says Answer 3.24m x 7.0m 22.68m2 23m2 100.0g/23.7cm3 4.219409g/cm3 4.22g/cm3 0.02cm x 2.371cm 0.04742cm2 0.05cm2 710m/3.0s 236.66666m/s 240m/s 1/19/12 Do Now Standard metric system units: KHD-G-bDCM Mass- grams (g) Temperature- Celcius ©, Kelvin (K) = C+273 Volume- Liter (L or mL) Distance- Meter (m) Temperature (C) Dependant Variable y 100 0 -8 -20 ENERGY ADDED Independent Variable x heat added energy (Joules) 1/20/12 Do Now 1) What is the most reactive nonmetal? F 2) Atomic Models: Chocolate Chip Cookie Model= Thompson’s Models 3) In order to occupy the same orbital, two electrons must have: opposite spin 4) How many moles of CO2 are present in 11.2L? (1mol=22.4L) 11.2LCO2 1molCO2 = .5molCO2 22.4LCO2 5) State of matter symbols: Solid-s, liquid-l, gas-g, aqueous-aq 1/23/12 Do Now Balance: CaCO3+2HClCaCl2+CO2+H2O How many moles of CaCl2 are produced when 50gCaCO3 react? 50gCaCO3 1molCaCO3 1molCaCl2 = .5molCaCl2 100gCaCO3 1molCaCO3 Balance: 2NO2N2+2O2 What type of reaction is this? Decomposition How many moles of NO2 are used? 2 1/30/12 Chapter 5- Chemical Names and Formulas Sec 5.1- Naming Ions Objectives: -Identify the charges on monatomic ions by using the periodic table, and name the ions. - Define a polyatomic ion and write the names and formulas of the most common polyatomic ions. -Identify the two common endings for the names of most polyatomic ions. Atoms and Ions -Atoms are electrically neutral - Because there is the same numner of protons (+) and electrons (-). -Ions are atoms, or groups of atoms, with a charge (positive or negative) - They have different numbers of protons and electons. - Only electrons can move, and gaining or losing electrons makes ions. An Anion is… -A negative ion -Has gained electrons -Nonmetals can gain electrons -Charge is written as a superscript on the right F1- has gained one electron (-ide is the new ending = fluoride) O2- has gained two electrons (oxide) A Cation is… -A positive ion -Formed by losing electrons -More protons than electrons -Metals can lose electrons K1+ Has lost one electron (no name change for positive ions) Ca2+ has lost two electrons Predicting Ionic Charges - Group 1A: Lose 1 electron to form 1+ ions (H1+, Li1+, Na1+, K1+, Rb1+, Cs1+, Fr1+) - Group 2A: Loses 2 electrons to form 2+ ions (Be2+, Mg2+, Ca2+, Sr2+, Ba2+, Ra2+) - Group 3A: Loses 3 electrons to forms 3+ ions (B3+, Al3+, Ga3+, In3+, Tl3+) - Group 4A: Do they lose 4 electrons or gain 4 electrons? Neither! Group 4A elements rarely form ions, the share) - Group 5A: Gains 3 electrons to form 3- ions (N3-, P3-, As3-, Sb3-, Bi3-) - Group 6A: Gains 2 electrons to form 2- ions (O2-, S2-, Se2-, Te2-, Po2-) - Group 7A: Gains 1 electron to form 1- ions (F1-, Cl1-, Br1-, I1-, At1-) - Group 8A: Stable noble gases no not form ions! Group B elements: Many transition elements have more than one possible oxidation state. Iron (II) = Fe2+, Iron (III) = Fe3+ Note the use of Roman Numerals to show charges Naming Cations - Two methods can clarify when more than one charge is possible: - Stock system- uses roman numerals in parenthesis to indicate the numerical value - Classical method- uses root word and suffixes (-ous, -ic) - We will is the Stock System - Cation- if the charge is always the same (like in the Group A metals) just write the name of the metal. - Transition metals can have more than one type of charge. - Indicate the charge by roman numerals Some of the post-transition metals elements also have more than one possible oxidation State. Tin (II) = Sn2+, Tin (IV) = Sn4+ Exceptions: - Some of the transition metals have only one ionic charge Do not need to use roman numerals for these Silver is always 1+ (Ag1+) Cadmium and Zinc are always 2+ (Cd2+ and Zn2+) 1/31/12 Do Now- What ions do the following form: Ca- Ca2+ cation Na- Na1+ cation Cl- Cl1- anion Al- Al3+ cation Kr- none O- O2- anion CATIONS Practice by naming these: Na1+: Sodium Ion Ca2+: Calcium Ion Al3+: Aluminum Ion Fe3+: Iron(III) Ion Fe2+: Iron(II) Ion Pb2+: Lead(II) Ion Li1+: Lithium Ion Write symbols for these: Potassium Ion: K1+ Magnesium Ion: Mg2+ Copper(II) Ion: Cu2+ Chromium(VI) Ion: Cr6+ Barium Ion: Ba2+ Mercury(II) Ion: Hg2+ ANIONS Naming Anions: - Anions are always the same charge - Change the monatomic element ending to – ide - F1- a Fluorine atoms will become Fluoride ion Practice by naming these: Cl1- : Chloride NaCl is Sodium Chloride N3- : Nitride Br1- : Bromide O2- : Oxide Ga3+ : Gallium Ion Write symbols for these: Sulfide Ion: S2Iodide Ion: I1Phosphide Ion: P3Strontium Ion: Sr2+ 2/1/12 Do Now- Name O2 : Oxide Mg2+ : Magnesium Ion Cl1- : Chloride Al3+ : Aluminum Ion Fe2+ : Iron(II) Ion Pb4+ : Lead(IV) Ion Write Formula Potassium Ion: K1+ Sulfide Ion: S2Strontium Ion: Sr2+ Nitride Ion: N3Copper(II) Ion: Cu2+ Chromium(VI) Ion: Cr6+ Roman Numeral Review: 1-I 2-II 3-III 4-IV 5-V 6-VI Polyatomic Ions are… -Groups of atoms that stay together and have an overall charge, and one name. -Usually end in –ide or –ite -Acetate: C2H3O21-Nitrate: NO31-Nitrite: NO21-Permanganate: MnO41-Hydroxide: OH1- and Cyanide: CH1-Sulfate: SO42-Sulfite: SO32-Carbonate: CO32-Chromate: CrO42-Dichromate: Cr2O72- -Phosphate: PO43-Phosphite: PO33-Ammonium: NH41+ (one of the few positive polyatomic ions) If the polyatomic ion begins with H, then combine the word hydrogen with the other polyatomic ion present: H1+ + CO32- HCO31Hydrogen + Carbonate Hydrogen Carbonate Ion Naming and Writing Formulas for Ionic Compounds -Objectives: -Apply the rules for naming and writing formulas for compounds containing polyatomic ions Example: Barium nitrate (note the 2 word name) Ba2+ + NO31- Ba(NO3)2 1) Write the formulas for the cations and anions, including CHARGES! 2) Check to see if charges are balanced. 3) Balance charges, if necessary, using subscripts. Use parentheses if you need more than one of a polyatomic ion. Use the criss-cross method to balance subscripts. 2/2/12 Do Now Name: NO31- : Nitrate Hg1+ : Mercury(I) Ion SO32- : Sulfite PO43- : Phosphate Pb4+ : Lead(IV) Ion Write Formula: Carbonate: CO32Nitride: N3Chlorate: ClO31Nitrite: NO21Copper(II): Cu2+ Sulfate: SO42Notes Example: Ammonium sulfate (note the two word name) NH1+ + SO4 2- (NH4)2SO4 1) Write the formulas for the cations and anions, including CHARGES! 2) Check to see if charges are balanced. 3) Balance charges, if necessary, using subscripts. Use parentheses if you need more than one of a polyatomic ion. Use the criss-cross method to balance subscripts. Example: Iron(III) Chloride Fe3+ + Cl1- FeCl3 Example: Aluminum sulfide Al3+ + S2- Al2S3 Example: Magnesium carbonate Mg2+ + CO32- MgCO3 Example: Zinc hydroxide Zn2+ + OH1- Zn(OH)2 Example: Aluminum phosphate Al3+ + PO43- AlPO4 Naming Ionic Compounds 1) Name the cation first, then anion 2) Monatomic cation=name of the element -Ca2+ = calcium ion 3) Monatomic anion = root + -ide - Cl1- = chloride - CaCl2 = calcium chloride 2/3/12 Write Formula: Ammonium chloride- NH4Cl Aluminum(III) oxide- Al3+O2-Al2O3 Potassium bromide- K1+Br1-KBr Potassium sulfide- K1+S2-K2S Tin(II) iodide- Sn2+I1-SnI2 Write name: Ba(OH)2 : Barium hydroxide Cr2(SO4)3 : Chromium(III) sulfate Au(ClO3)3 : Gold(III) chlorate NaClO : Sodium hypochlorite SiC : Silicone carbide HW Review- (Read 5.3, #1-8 pg 180) 5d) Copper(I) acetate 6b) Magnesium phosphide- Mg3P2 c) Silver(I) sulfide- Ag2S d) Niobium(V) chloride- NbCl5 7a) Rb2O- Rubidium oxide b) FeF2- Iron(II) flouride c) K3N- Potassium nitride 8b) Lithium thiosulfate- Li2S2O3 c) Ammonium phosphate- (NH4)3PO4 d) Potassium permanganate- KMnO4 2/6/12 Do Now Write Name: Fe(C2H3O2)3- Iron(III) acetate Cs2CO3- Cesium carbonate MnSO3- Manganese(II) sulfite Hg2Cl2- Mercury(I) chloride Rb2CrO4- Rubidium chromate Write Formula: Radium nitrate- Ra(NO3)2 Barium hydroxide- Ba(OH)2 Aluminum(III) acetate- Al(C2H3O2)3 Magnesium nitrite- Mg(NO2)2 Gold(III) chlorate- Au(ClO3)3 Naming Ionic Compounds - some metals can form more than one change (usually the transition metals) - use a Roman numeral in their name: PbCl2- use the anion to find the charge on the cation (chloride is always 1-) Pb2+ is the Lead(II) cation PbCl2 = Lead(II) chloride Things to look for: 1) If cations have (), the number in the parenthesis is their charge. 2) If anions end in –ide they are probably off the periodic table (monatomic) 3) If anion ends in –ate or –ite, then it is polyatomic. Practice: Iron(II) phosphate- Fe3(PO4)2 Potassium sulfide- K2S Ammonium chromate- (NH4)2CrO4 MgSO4- Magnesium sulfate FeCl3- Iron(III) chloride 2/7/12 Naming and Writing Formulas for Molecular Compounds -Objectives: -Interpret the prefixes in the names of molecular compounds in terms of their chemical formulas. -Apply rules for naming and writing formulas for binary molecular compounds. Molecular Compounds are… - made of just nonmetals - smallest piece is a molecule - can’t be held together by opposite charge attraction - can’t use charges to figure out how many charges of each atom (there are no charges present) Molecular compounds are easier! -Ionic compounds use charges to determine how many of each. -you have to figure out charges -may need to criss-cross numbers -Molecular compounds: the name tells you the number of atoms -uses prefixes to tell you the exact number of each element present 2/8/12 1- mono 2- di 3- tri 4- tetra 5- penta 6- hexa 7- hepta 8- octa 9- nona 10- deca - to write the name, write two words: prefix and name –ide - one exception is we don’t write mono if there is only one of the first element. - normally, we do not have double vowels when writing names (oa oo) Practice by naming these: -N2O = dinitrogen monoxide (also called nitrous oxide or laughing gas) -NO2 = nitrogen dioxide -Cl2O7 = dichlorine heptoxide -CBr4 = carbon tetrabromide -CO2 = carbon dioxide -BaCl2 = barium chloride Write formulas for these: -diphosphorus pentoxide = P2O5 -tetraiodine nonoxide = I4O9 -sulfur hexafluoride = SF6 -nitrogen trioxide = NO3 -carbon tetrahydride = CH4 -phosphorus trifluoride = PF3 -aluminum chloride = AlCl3 Write the correct name for: -As4O10 = tetrarsenic decoxide -BrO3 = bromine trioxide -BN = boron mononitride -N2O3 = dinitrogen trioxide -NI3 = nitrogen triodide -SF6 = sulfur hexafluoride -XeF4 = xenon tetrafluoride -PCl3 = phosphorus trichloride -CO = carbon monoxide -PCl5 = phosphorus pentachloride 2/9/12 Do Now Name: NO- Nitrogen monoxide CO- Carbon monoxide H2O- Dihydrogen monoxide P2S5- Diphosphorus pentasulfide SbCl5- Antimony pentachloride Write formula: Sulfur trioxide- SO3 Nitrogen dioxide-NO2 Dihydrogen monoxide- H2O HW Review (pg209 9&10) 9a) tin tetraiodide b) dinitrogen trioxide c) phosphorus trichloride d) carbon diselenide 10a) PBr5 b) P2O3 c) AsBr3 d) CCl4 Naming and Writing Formulas for acids and bases Objectives: -Apply three rules for naming acids 2/14/12 Acids are… -Compounds that give off hydrogen ions (H1+)when dissolved in water (the Arrhenius definition) -Will start the formula with H -There will always be some Hydrogen next to an anion -The anion determines the name Rules for naming acids: Name it as a normal compound first 1) If the anion attached to hydrogen ends in –ide, out the prefix hydro- and change –ide to –ic acid -HCl- hydrogen ion and chloride ion = hydrochloric acid -H2S- hydrogen ion and sulfide ion = hydrosulfuric acid -If the anion has oxygen in it, then it ends in –ate or –ite 2) change the suffix –ate to –ic acid (use no prefix) -Example: HNO3 Hydrogen and nitrate ions = Nitric acid 3) change the suffix –ite to –ous acid (uses no prefix) - Example: HNO2 Hydrogen and nitrite ions = Nitrous acid Naming Acids Normal Ending Acid name is…. -ide hydro-ic acid -ate -ic acid -ite -ous acid 2 additional rules (not mentioned in book) 4) If the acid has 1 more oxygen than the –ic acid, add the prefix per- HClO3- (Hydrogen Chlorate) is chloric acid - HClO4- would be perchloric acid 5)If there is 1 less oxygen than the –ous acid, add the prefix hypo- HClO2- (Hydrogen Chlorite) is chlorous acid then HClO would be hypochlorous acid 2/15/12 Perchloric acid- HClO4 Chloric acid- HClO3 Chlorous acid- HClO2 Hypochlorous acid- HClO Practice: HF- Hydroflouric acid H3P- Hyrdophosphoric acid H2SO4- Sulfuric acid H2SO3- Sulfurous acid H2CrO4- Chromic acid Writing Acid Formulas- in reverse! - Hydrogen will be listed first - the name will tell you the anion - be sure the charges cancel out - starts with prefix hydro?- there is no oxygen, -ide ending for anion - no prefix hydro? 1) –ate anion comes form –ic endings 2) –ite anion comes from –ous ending Examples: Hydroiodic acid- HI Acedic acid- HC2H3O2 Carbonic acid- H2CO3 Phosphorus acid- H3PO3 Hydrobromic acid- HBr 2/16/12 PRACTICE: HNO3- Nitric acid HClO- Hypochlorous acid 2/27/12 Properties of Substances with metallic, ionic, and covalent bonds - metallic- electrons move throughout atoms - ionic- transfer of electrons - covalent- share electrons Lewis Electron-Dot Structures – show valence electrons - As you go from element to element across the periodic table, you add a dot to each side of the element’s symbol. - You do not begin to pair dots until all four sides of the element’s symbol have a dot - An element with an octet of valence electrons has a stable configuration - The tendency of bonded atoms to have octets of valence electrons is called the octet rule. - When two chlorine atoms form a covalent bond, each atom contributes one electron to a shared pair. - An unshared pair, or a lone pair, is a nonbonding pair of electrons in the valence shell of an atom - A single bond is a covalent bond in which two atoms share one pair of electrons - The electrons can pair in any order. However, any unpaired electrons are usually filled in to show how they will form a covalent bond. H Draw a Lewis structure for CH3I. .. .. C H H H :I: H: C :I: ˙ ˙˙ ˙˙ H Multiple Bonds - For O2 to make an octet, each atom needs two more electrons. The two atoms share four electrons. :O::O: or :O=O: - For N2 to make an octet, each atom needs three more electrons. The two atoms share six electrons. :N N: or :NN: 2/28/12 Draw the Lewis structure for formaldehyde CH2O . .. C H H O: Objectives: - Predict the shape of a molecule using VSEPR theory - Associate the polarity of molecules with the shapes of molecules, and relate the polarity and shape of molecules to the properties of a substance. Determine Molecular Shapes - The three-dimensional shape of a molecule is important in determining the molecule’s physical and chemical properties A Lewis Structure can help predict molecular shape - You can predict the shape of a molecule by examining the Lewis structure of the molecule - The valence shell electron pair repulsion (VSEPR) theory is a theory that predicts some molecular shapes based on the idea that pairs of valence electrons surrounding an atom repel each other. - According to the VSEPR theory, the shape of a molecule is determined by the valence electrons surrounding the central atom - Electron pairs are negative, so they repel each other - Therefore, the shared pairs that form different bonds repel each other and remain as far apart as possible. - For CO2, the two double bonds around the central carbon atom repels each other and remain far apart CH4 but three dimensional 2/29/12 HW Review 2) They are linear because there are only 2 3) Lewis Dot helps us predict the shape of a molecule 6) Br2 is linear because there are only 2 shapes. HBr is linear because there are only 2 shapes. HBr is more polar. 3/1/12 The four shared pairs of electrons in CH4 are farthest when each pair is positioned at the corners of a tetrahedron. Draw the Lewis structure for H2O. Water has 2 shared and 2 unshared pairs of electrons Find the shape that allows the shared and unshared pairs of electrons to be as far apart as possible. The water molecule will have a bent shape. Shape affects polarity - One property that shape determines is the polarity of a molecule - The polarity of a molecule that has more than two atoms depends on the polarity of each bond and the way the bonds are arranged in space. - If two dipoles are arranged in opposite directions, they will cancel each other. - If two dipoles are arranged at an angle, they will not cancel each other out. - Compare the molecules of nonpolar carbon dioxide, CO2, which has a linear shape, and polar water, H2O, which has a bent shape. 3/2/12 linear tetrahedral trigonal planar trigonal bipyramidal 9) If water is not a good conductor of electric current, why is it dangerous to handle an electrical appliance when hands are wet or when you are standing on wet ground? Because of all the minerals and 3/6/12 Review for 6.3 quiz Lewis Dot structure- element and valence electrons Covalent bond- a bond that shares electrons Ionic bond- a bond that transfers electrons Double bonds have 4 electrons Electrons that exist outside the bond are unshared, unbonded, lone pairs of electrons. Planar trigonal- 4 atoms Tetrahedral- 5 atoms bent Angular or bent- 3 atoms Linear can be 2 or 3 atoms What does VSEPR stan d for? Valence shell electrons pair repulsion Single, double, triple bonds 3/8/12 Heat -q- is the energy transferred between objects which are at different temperatures. The unit for heat is joules. Energy is never created nor destroyed. Temperature -T- a measure of the average kinetic energy of a substance. (kinetic energythe energy of motion) 3/12/12 Temperature Heat u Density is intensive Intensive Property- Extensive PropertyDoes not depend on the amount of the substance Does depend on the amount of the sample Enthalpy- the total energy of a sample motion- KE light- solar electromagnetic energy heat- thermal chemical nuclear potential sound Thermodynamics- the branch of science concerned with the energy changes that accompany chemical and physical changes. Gases- Intro to gases Properties- great distance between molecules. - low densities - highly compressible - fill any container - fluid Kinetic Theory - Gas molecules are in constant, rapid, random motion - Gas molecules are very far apart relative to their size -The pressure exerted by a gas is a result of collisions of the gas molecules against the walls of the container Pressureunits- KPa- kilopascals - Atm- atmospheres - mmHg- millimeters Mercury - Torr- millimeters Mercury - psi- pounds per square inch 1atm = 101.3kPa = 760mmHg = 14.7psi = 760 torr 3/14/12 Gas Laws - Volume - Pressure - Temperature 3/15/12 Boyle’s Law- Pressure and volume of a gas are inversely related. Temperature remains constant. V1P1=V2P2 Charles Law- Volume and temperature of a gas are directly related. Pressure remains constant. V1/T1=V2/T2 They move in the same direction. Gay-Lussac’s Law- Pressure and Temperature of a gas are directly proportional. P1/T1=P2/T2 3/16/12 Do Now Write the untis for: Pressure: atm, psi, kPa, mmHg, Torr Temperature: C, K, F Volume: L, mL, cm3 3/19/12 Notes STP- standard temperature and pressure, 0C and 1 atm Combined Gas Laws- V1P1 = V2P2 T1 T2 3/23/12 Practice: -What is the volume of a gas stored at 45C and 1376mmHg if the same gas occupies 148cm3 at -43C and 3608mmHg V1=? V1P1 = V2P2 V1(1376mmHg) = (148cm3)(3608mmHg) T1 = 45C = 318K T1 T2 318K 230K P1 = 1376mmHg V2 = 148cm3 (148cm3)(3608mmHg)(318K) = V1(1376mmHg)(230K) T2 = -43C = 230K V1 = 536.5cm3 P2 = 3608mmHg -A 35,800L balloon is held at 15875mmHg and 120C. The balloon is then stored at 24,928mmHg and 40C. What is the new volume? V1= 35,800L V1P1 = V2P2 (35,800L)(15,875mmHg) = (V2)(24,928mmHg) T1 = 120C = 393K T1 T2 393K 313K P1 = 15,875mmHg V2 = ? (35,800L)(15,875mmHg)(313K) = V2(24,928mmHg)(393K) T2 = 40C = 313K V2 = 18,158L P2 = 24,928mmHg Ideal Gas LawIdeal Gas Equation- PV=nRT P= pressure V= volume n= moles = n/M = g/(g/mol) M= molar mass R= gas constant = 8.31(LkPa/molK) = 0.082(Latm/molK) T= temperature 3/26/12 Example: -A 240mL sample of gas at 100C ad 755mmHg is found to have a mass of 1.12g. What is the Molar Mass of the gas? R=8.31(LkPa/molK) = 0.0821(Latm/molK) 1atm = 760mmHg = 101.kPa Given: P= 755mmHg = 100.63kPa V=240mL = .24L R= 8.31(LkPa/molK) = 0.0821(Latm/molK) T= 100C = 373K m= 1.12g M= molar mass= ? VP=nRT VP=(m/M)RT M=mRT M=(1.12g) 8.31LkPa (373K) = 143g/mol VP (.24L) molK (100.63kPa) 3/27/12 Notes: Effusion- to move from a high concentration to low concentration through a hole Diffusion- the movement from an area of high concentration to low concentration Dalton’s Law of Partial Pressure PT = P1+P2+P3+…+Pn Patm = PN2+PO2+PH2O+PCO2+…Pn 1atm=101.3kPa=760mmHg=14.7psi 3/29/12 Do Now Name: CaCl2 = Calcium Chloride LiBr = Lithium Bromide Write Formula: Strontium Phosphate = Sr +2 PO4 -3 = Sr3(PO4)2 Aluminum Sulfide = Al+3S-2 = Al2S3 NotesMixtures: Iced Tea, Lemonade, Meat, cereal, crunch yogurt, rock, salt water, pool water, medicine Heterogeneous Mixture- the particles can be seen with (at least) a microscope, has at least 2 phases (same properties) 3/30/12 Do Now Write formula: Calcium phosphate Ca+2PO4-3 Ca3(PO4)2 Sodium sulfate Na+1SO4-2 Na2SO4 Write the name: AgCl2 Silver(II) chloride H2O Dihydrogen monoxide 4/3/12 Do Now Write the name: PF3- Phosphorous trifluoride SCl4- Sulfur tetrachloride BrCl4- Bromine tetrachloride Write formula: Carbon dioxide- CO2 Sulfur trioxide- SO3 Krypton difluoride- KrF2 Notes Heterogeneous Mixtures- 2 phases, depending on size Homogeneous Mixtures- 1 phase (same phase) - appear uniform, - solutions-solvent- the substance that does the dissolving -solute- the substance that is dissolved Suspension- heterogeneous mixture in which different parts separate over time. - largest size solutes Colloid- a mixture consisting of particles that are sized between a suspension and a solution. - Does not separate over time. - Stable 4/4/12 Write the name: H2SO4- Sulfuric Acid HCl- Hydrochloric Acid H3PO4- Phosphoric Acid H2S- Hyrdosulfuric Acid Write formula: Nitric Acid- HNO3 Hydrobromic Acid- HBr Carbonic Acid- H2CO3 Solutions- Smallest particle size, molecules, atoms Colloids- Middle size Suspension- Largest size Separating Mixtures- Distilling 4/5/12 Do Now MgF2-(Ionic) Magnesium fluoride H2O2- (Covalent) Dihydrogen dioxide H3PO4- (acid) Phosphoric Acid Sodium chloride- (salt) NaCl Carbon tetrahydride- (methane) CH4 Acetic Acid- (vinegar) HC2H3O2 ` Separating Mixtures- Distilling (based on BP), Filtering, Evaporation, centrifuge, chromatography Liquids- fluid - enough energy to allow molecules to move past one another - Viscosity- the degree to which a fluid will flow viscosity flow - high viscosity- molasses - low viscosity- water Cohesion- the attractive forces molecules have for each other Ex- beads of water on a waxed car Adhesion- the attractive forces molecules have for a solid Ex- meniscus