Unit One

Notes One Unit One Two Classes of Elements Periodic Table Info? What Are Stable Elements? Stabilizing Sodium Stabilizing Oxygen Sodium Loses electrons to Oxygen Oxidation Numbers Key Elements and Examples

Two Classes of Elements What are the Two Main Classes of Elements? Metals and Nonmetals (Stair-Step)

What information doe the Periodic Table give us? Atomic Number # Protons = # of Electrons Electron structure Mass Number = # P + # N

What Makes Elements Stable? Which orbitals? Eight Electrons…… Highest S and P…… Noble Gases (electronically stable) He, Ne, Ar, Kr, Xe, and Rn Lose or Gain to get 8e-1 (to become stable) Do metals Lose or Gain electrons? Do nonmetals Lose or Gain electrons? Which Family? (Lose) (Gain)

Stabilizing Sodium How many electrons does sodium have? 11Na What is Sodium’s Short-Hand Element? 10Ne How many Valence Electrons for Sodium? 1e-1 What is the shorthand electron configuration? Sodium loses/gain how many electrons? Na Na+1 + e-1 Oxidation or reduction? (protons) + (electrons)=charge 1 [10Ne] 3s (+11) (-10) +1

Stabilizing Oxygen How many electrons does oxygen have? 8O What is oxygen’s Short-Hand Element? 2He How many Valence Electrons for oxygen? 6e-1 What is the shorthand electron configuration? Oxygen loses/gains how many electrons? 2e-1 O + 2e-1 O-2 Oxidation or reduction? (protons) + (electrons)=charge [2He] 2s 2 2p 4 (+8) (-10) -2

Sodium Loses electrons to Oxygen Na Na+1 + e-1 (Stable Like Neon) Ox or Red? O + 2e-1 O-2 (Stable Like Neon) Ox or Red? How many sodium atoms are needed to satisfy oxygen’s electron hunger? 2e-1 means How many oxygen atoms are needed to satisfy sodium’s electron loss? Na2O High Electronegativity two Na Low Electronegativity One O

Oxidation Numbers Fe+2 Fe+3 S-2 S+4 S+6 All elements Lose or Gain e-1. Some have multiple loss or gain possibilities. Fe+2 Fe+3 S-2 S+4 S+6

Key Elements (99%) H+1 H-1 (99%)O-2 O-1 (Always) Li+1, Na+1, K+1, Rb+1, Cs+1, Fr+1 (Always) Be+2, Mg+2, Ca+2, Ba+2, Sr+2, Ra+2 (Always) Al+3 (with only a metal) F-1, Cl-1, Br-1, I-1 (NO3-1) ion is always +5 (SO4-2) ion is always +6

Example One Find the oxidation numbers. Al2S3 Algebra is useful! Al+3 key element 2(+3) + 3(S)=0 S= -2 2(Al) + 3(S)=

Example Two Find the oxidation numbers. Ca(NO3)2 Algebra is useful ! Ca+2 and O-2 key elements (+2)+2(N)+6(-2)=0 (+2)+2(N)+(-12)=0 2(N)+(-10)=0 2(N)=10 N= +5 (Ca)+ 2(N)+ 6(O)=

Finding Oxidation #’s for Compounds +1 -2 +1 +4 -2 H2O H2CO3 +1 +5 -2 -3 +1 +4 -2 H3PO4 (NH4)2CO3 +2 +5 -2 +1 +5 -2 Ca3(AsO4)2 HNO3 +1 +6 -2 +3 +6 -2 H2SO4 Fe2(SO4)3 +1 +6 -2 +2 +7 -2 Hg2SO4 Ba(ClO4)2 +3 +4 -2 +1 +6 -2 Na2Cr2O7 Al2(CO3)3

Now it is time for class work !!! A101: paper practice (Work Together) CA101 : computer assignment Both will be due at beginning of class next time Ready Set Break !!!

Notes Two Unit One Naming Inorganic Salts Example One Example One Thinking Example Two Computer Assignment One

Naming Inorganic Salts TWO parts to the name 1) Cation 2) Anion Cation Examples Ca+2 Al+3 Fe+2 Na+1 Anion Examples Cl-1 NO3-1 SO4-2 N-3 Positive Negative

Example One Iron(II) Fe+2 Iron(III) Fe+3 Name the formula Fe2(CrO4)3 Step #1 Find The + Ion(s). Iron(II) Fe+2 Iron(III) Fe+3

Example One Step #2 Find The - Ion(s) Chromate CrO4-2

Example One Fe2(CrO4)3 Fe+2 Iron(II) Fe+3 Iron(III) CrO4-2 Chromate (+2) + Y (-2) = X (+3) + Y (-2) = X=1 Y=1 X=2 Y=3 1 (+2) + 1 (-2) = 2 (+3) + 3 (-2) = Fe CrO4 Fe2(CrO4)3

Example Two Al2(CO3)3 Al+3 Aluminum CO3-2 Carbonate Aluminum Carbonate (+3) + Y (-2) = X=2 Y=3 2 (+3) + 3 (-2) = Al2(CO3)3

Computer Assignment One/Two NAMING IONIC COMPOUNDS LEVELs ONE AND TWO

Writing a Formula From a Name (Cation+?)X(Anion-?)Y X (+?) + Y (-?) = If X or Y is 2 or greater... Lowest Whole Number Ratio and the ion is polyatomic. Ba+2 Cr2O7-2 Hg2+2 Pb+4 ( )_( )_ Lithium Nitrate Li+1 1 NO3-1 1 LiNO3 ( )_( )_ Hydrogen Phosphate H+1 3 PO4-3 1 H3PO4 ( )_( )_ Ammonium carbonate NH4+1 2 CO3-2 1 (NH4)2CO3 ( )_( )_ Calcium Arsenate Ca+2 3 AsO4-3 2 Ca3(AsO4)2 ( )_( )_ Iron(III) periodate Fe+3 1 IO4-1 3 Fe(IO4)3 ( )_( )_ Mercury(I) Sulfate Hg2+2 2 SO4-2 2 Hg2SO4 ( )_( )_ Barium Perchlorate Ba+2 1 ClO4-1 2 Ba(ClO4)2 ( )_( )_ Sodium Dichromate Na+1 2 Cr2O7-2 1 Na2Cr2O7 ( )_( )_ Lead(IV) Sulfate Pb+4 2 SO4-2 4 Pb(SO4)2

Notes Three Unit One Standard Amounts One Gopher One Mole Formula mass Percent Composition Empirical Formula

Standard Amounts How many dollars is… A) 120 pennies? 1.2 dollars B) 2 quarters? 0.5 dollars C) 15 nickels? 0.75 dollars How many dozens is… D) 48 eggs? 4 dozen E)18 apple fritters 1.5 dozen

One Gopher One Gopher equals 12 items What is the mass of one gopher of… A) white beads? 2.81g/G B) blue beads? 0.50g/G C) orange Beads? 1.67g/G

Seven Rows Eight Rows

One Gopher(12 items) In Six groups (1) How many gophers of beads are in… (2) How many beads are in… A) ___g B) ___g C) ___g D) ___g E) ___g F) ___g 2.00 48 beads 4.00G 3.49 15 beads 1.24G 2.51 18 beads 1.50G 27 beads 3.75 2.25G 1.75 3.50G 42 beads 5.82 2.07G 25 beads

One Mole N O C One mole is 6.022x10+23 items. Each element on the period table has a mass per mole. N 14.0g 6.022x10+23atoms O 16.0g 6.022x10+23atoms C 12.0g 6.022x10+23atoms How many moles are in each? How many atoms are in each? N 7.0g ÷14.0g/m =0.50m x6.022x10+23atoms/m =3.01x10+23atoms O 4.0g ÷16.0g/m =0.25m x6.022x10+23atoms/m =1.51x10+23atoms C 18.0g ÷12.0g/m =1.50m x6.022x10+23atoms/m =9.03x10+23atoms

Calculations Bases on Chemical Formulas Formula mass (Molecular Mass or Gram-Formula Mass) Empirical Formula Percent Composition

Rounding Atomic Mass C 12.011 12.0 Fe 55.847 55.8 O 15.9994 16.0 Bi 208.980837 209.0 K 39.0983 39.1 Au 196.96654 197.0 Os 190.23 190.2 Mg 24.3050 24.3 Na 22.98968 23.0

Formula Mass Example One Calculate the formula mass for 1 mole of C6H12O6. E # Mass C 6 x 12.0 = 72.0 12.011 H 12 x 1.0 = 12.0 1.0079 O 6 x 16.0 = 96.0 15.9994 180.0g/mol How many molecules of C6H12O6 is 180.0g/mol? 6.022x10+23 molecules

Empirical Formula Example One What is the empirical (simplest) formula containing 36.8% N, 63.2% O? 1) Calculate moles of each element. E Q Mass Mass N 36.8 g ÷ 14.0 = 2.63 mol N 14.0067 O 63.2 g ÷ 16.0 = 3.95 mol O 15.9994 2) Calculate the lowest ratio. E Moles Lowest Ratio N 2.63 mol N ÷ 2.63 mol = 1.00 O 3.95 mol O ÷ 2.63 mol = 1.50 3) Write the formula X by 2 to get whole numbers N2O3

Percent Composition Example One Calculate the percentage composition of H2O. 1)Calculate the formula mass for 1 mole of H2O E # Mass H 2 x 1.0 = 2.0 1.0079 O 1 x 16.0 = 16.0 15.9994 18.0g/mol 2) Divide each contribution by the total mass. H 2.0 ÷ 18.0 = ( x 100) = 11% 0.11 Answer O 16.0 ÷ 18.0 = 0.889 ( x 100) = 88.9% 3) Add the percentages to check work. 11% 88.9% 100.%

Empirical Formula Example Two What is the empirical (simplest) formula containing 69.58% Ba, 6.090% C, 24.32% O? 1) Calculate moles of each element. E Q Mass Mass Ba 69.58 g ÷ 137.33 = 0.50666 mol Ba C 6.090 g ÷ 12.01 = 0.50708 mol C O 24.32 g ÷ 16.00 = 1.520 mol O 2) Calculate the lowest ratio. E Moles Lowest Ratio Ba 0.50666 mol ÷ 0.50666 mol = 1.000 C 0.50708 mol ÷ 0.50666 mol = 1.001 O 1.520 mol ÷ 0.50666 mol = 3.00 3) Write the formula X by 1 to get whole numbers BaCO3

Percent Composition Example Two Calculate the percentage composition of Fe(ClO4)3. 1)Calculate the formula mass for 1 mole of Fe(ClO4)3. E # Mass 55.847 Fe 1 x 55.8 = 55.8 35.453 Cl 3 x 35.5 = 106.5 15.9994 O 12 x 16.0 = 192.0 354.3g/mol 2) Divide the each contribution by the total mass. Fe 55.8 ÷ 354.3 = ( x 100) = 15.8% 0.1575 Cl 106.5 ÷ 354.3 = ( x 100) = 30.06% 0.3006 Answer O 192.0 ÷ 354.3 = ( x 100) = 54.19% 0.5419 3) Add the percentages to check work. 15.8 % 30.1 % 54.2 % 100.1%

Formula Mass Example Three Calculate the formula mass for 1 mole of Al2O3 E # Mass Al 2 x 27.0 = 54.0 26.98154 O 3 x 16.0 = 48.0 15.9994 102.0g/mol How many molecules of Al2O3 is102.0g/mol? 6.022x10+23 molecules

Formula Mass Example Two Calculate the formula mass for 1 mole of CaCO3. E # Mass 40.078 Ca 1 x 40.1 = 40.1 12.011 C 1 x 12.0 = 12.0 15.9994 O 3 x 16.0 = 48.0 100.1g/mol How many molecules of CaCO3 is100.1g/mol? 6.022x10+23 molecules