Unit One Notes One Unit One Two Classes

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Unit One

Unit One

Notes One Unit One • • Two Classes of Elements Periodic Table Info? What

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? •

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 = #

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

What Makes Elements Stable? • • Eight Electrons…… Which orbitals? Highest S and P……

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

Stabilizing Sodium • How many electrons does sodium have? • 11 Na • What

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

Stabilizing Oxygen • How many electrons does oxygen have? • 8 O • What

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

Sodium Loses electrons to Oxygen • Na Na+1 + e-1 (Stable Like Neon) Ox

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

Oxidation Numbers • All elements Lose or Gain e-1. • Some have multiple loss

Oxidation Numbers • 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,

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 (NO 3 -1) ion is always +5 (SO 4 -2) ion is always +6

Example One • Find the oxidation numbers. • Al 2 S 3 • Algebra

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

Example Two • Find the oxidation numbers. • Ca(NO 3)2 • Algebra is useful

Example Two • Find the oxidation numbers. • Ca(NO 3)2 • Algebra is useful ! (Ca)+ 2(N)+ 6(O)= 0 • 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

Finding Oxidation #’s for Compounds +1 -2 H 2 O +1+5 -2 H 3

Finding Oxidation #’s for Compounds +1 -2 H 2 O +1+5 -2 H 3 PO 4 +1+5 -2 HNO 3 +1+6 -2 H 2 SO 4 +1 +6 -2 Hg 2 SO 4 +1+4 -2 H 2 CO 3 -3 +1+4 -2 (NH 4)2 CO 3 +2 +5 -2 Ca 3(As. O 4)2 +3 +6 -2 Fe 2(SO 4)3 +2 +7 -2 Ba(Cl. O 4)2 +1 +6 -2 +3 +4 -2 Na 2 Cr 2 O 7 Al 2(CO 3)3

Now it is time for class work !!! • A 101: paper practice (Work

Now it is time for class work !!! • A 101: paper practice (Work Together) • CA 101 : computer assignment • Both will be due at beginning of class next time • Ready Set Break !!!

Notes Two Unit One • • • Naming Inorganic Salts Example One Thinking Example

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

Naming Inorganic Salts • • • • TWO parts to the name 1) Cation

Naming Inorganic Salts • • • • TWO parts to the name 1) Cation Positive 2) Anion Negative Cation Examples Ca+2 Al+3 Fe+2 Na+1 Anion Examples Cl-1 NO 3 -1 SO 4 -2 N-3

Example One • Name the formula Fe 2(Cr. O 4)3 • Step #1 Find

Example One • Name the formula Fe 2(Cr. O 4)3 • Step #1 Find The + Ion(s). Iron(II) Fe+2 Iron(III) Fe+3

Example One • Step #2 Find The - Ion(s) Chromate Cr. O 4 -2

Example One • Step #2 Find The - Ion(s) Chromate Cr. O 4 -2

Example One Fe 2(Cr. O 4)3 Fe+2 Iron(II) Fe+3 Iron(III) Cr. O 4 -2

Example One Fe 2(Cr. O 4)3 Fe+2 Iron(II) Fe+3 Iron(III) Cr. O 4 -2 Chromate Iron(II) Chromate Iron(III) Chromate Fe+2 Fe+3 Cr. O 4 -2 X (+2) + Y (-2) = 0 X=1 Y=1 1 (+2) + 1 (-2) = 0 Fe. Cr. O 4 -2 X (+3) + Y (-2) = 0 X=2 Y=3 2 (+3) + 3 (-2) = 0 Fe 2(Cr. O 4)3

Example Two Al 2(CO 3)3 Al+3 Aluminum CO 3 -2 Carbonate Aluminum Carbonate Al+3

Example Two Al 2(CO 3)3 Al+3 Aluminum CO 3 -2 Carbonate Aluminum Carbonate Al+3 CO 3 -2 X (+3) + Y (-2) = 0 X=2 Y=3 2 (+3) + 3 (-2) = 0 Al 2(CO 3)3

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

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

Writing a Formula From a Name X (+? ) + Y (-? ) =

Writing a Formula From a Name X (+? ) + Y (-? ) = 0 (Cation+? )X(Anion-? )Y If X or Y is 2 or greater. . . and the ion is polyatomic. Ba+2 Cr 2 O 7 -2 Hg 2+2 Lowest Whole Number Ratio Pb+4 Lithium Nitrate (Li+1 )_( 1 NO -1 )_ 1 3 Hydrogen Phosphate (H+1 )_( 3 PO -3 )_ 1 4 Ammonium carbonate ( NH 4+1 )_( 1 2 CO 3 -2)_ Calcium Arsenate (Ca+2)_( 2 3 As. O -3 )_ 4 Iron(III) periodate (Fe+3)_( 1 IO -1 )_ 3 4 Mercury(I) Sulfate (Hg 2+2 )_( 2 SO -2 )_ 2 4 Barium Perchlorate (Ba+2 )_( 2 1 Cl. O 4 -1 )_ Sodium Dichromate (Na+1)_( 1 2 Cr O -2 )_ 2 7 Lead(IV) Sulfate (Pb+4)_( 4 2 SO -2)_ 4 Li. NO 3 H 3 PO 4 (NH 4)2 CO 3 Ca 3(As. O 4)2 Fe(IO 4)3 Hg 2 SO 4 Ba(Cl. O 4)2 Na 2 Cr 2 O 7 Pb(SO 4)2

Notes Three Unit One • • • Standard Amounts One Gopher One Mole Formula

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

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 equals 12 items What is the mass of one gopher of… A)

One Gopher equals 12 items What is the mass of one gopher of… A) white beads? 2. 81 g/G B) blue beads? 0. 50 g/G C) orange Beads? 1. 67 g/G

Seven Rows Eight Rows

Seven Rows Eight Rows

One Gopher(12 items) • In Six groups • (1) How many gophers of beads

One Gopher(12 items) • In Six groups • (1) How many gophers of beads are in… (2) How many beads are in… 48 beads A) 2. 00 ___g 4. 00 G 15 beads B) 3. 49 ___g 1. 24 G 18 beads C) 2. 51 ___g 1. 50 G 27 beads D) 3. 75 ___g 2. 25 G 42 beads E) 1. 75 ___g 3. 50 G 5. 82 2. 07 G 25 beads F) ___g

One Mole One mole is 6. 022 x 10+23 items. Each element on the

One Mole One mole is 6. 022 x 10+23 items. Each element on the period table has a mass per mole. N 14. 0 g 6. 022 x 10+23 atoms O 16. 0 g 6. 022 x 10+23 atoms C 12. 0 g 6. 022 x 10+23 atoms How many moles are in each? How many atoms are in each? N 7. 0 g ÷ 14. 0 g/m =0. 50 m x 6. 022 x 10+23 atoms/m =3. 01 x 10+23 atoms O 4. 0 g ÷ 16. 0 g/m =0. 25 m x 6. 022 x 10+23 atoms/m =1. 51 x 10+23 atoms C 18. 0 g÷ 12. 0 g/m=1. 50 m x 6. 022 x 10+23 atoms/m =9. 03 x 10+23 atoms

Calculations Bases on Chemical Formulas • Formula mass (Molecular Mass or Gram-Formula Mass) •

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

Rounding Atomic Mass C 12. 011 Fe 55. 847 O 15. 9994 Bi 208.

Rounding Atomic Mass C 12. 011 Fe 55. 847 O 15. 9994 Bi 208. 980837 K 39. 0983 Au 196. 96654 Os 190. 23 Mg 24. 3050 Na 22. 98968 12. 0 55. 8 16. 0 209. 0 39. 1 197. 0 190. 2 24. 3 23. 0

Formula Mass Example One Calculate the formula mass for 1 mole of C 6

Formula Mass Example One Calculate the formula mass for 1 mole of C 6 H 12 O 6. E C H O # Mass 6 x 12. 0 = 72. 0 12 x 1. 0 = 12. 0 6 x 16. 0 = 96. 0 180. 0 g/mol 12. 011 1. 0079 15. 9994 How many molecules of C 6 H 12 O 6 is 180. 0 g/mol? 6. 022 x 10+23 molecules

Empirical Formula Example One What is the empirical (simplest) formula containing 36. 8% N,

Empirical Formula Example One What is the empirical (simplest) formula containing 36. 8% N, 63. 2% O? 1) Calculate moles of each element. Q Mass E Mass N 36. 8 g ÷ 14. 0 = 2. 63 mol N 14. 0067 15. 9994 O 63. 2 g ÷ 16. 0 = 3. 95 mol O 2) Calculate the lowest ratio. Moles Lowest Ratio E N 2. 63 mol N ÷ 2. 63 mol = 1. 00 O 3. 95 mol O ÷ 2. 63 mol = 1. 50 3) Write the formula N 2 O 3 X by 2 to get whole numbers

Percent Composition Example One Calculate the percentage composition of H 2 O. 1)Calculate the

Percent Composition Example One Calculate the percentage composition of H 2 O. 1)Calculate the formula mass for 1 mole of H 2 O E # Mass H 2 x 1. 0 = 2. 0 1. 0079 O 1 x 16. 0 = 16. 0 15. 9994 18. 0 g/mol 2) Divide each contribution by the total mass. H 2. 0 ÷ 18. 0 =(0. 11 x 100) = 11% O 16. 0 ÷ 18. 0 =(0. 889 x 100) = 88. 9% 3) Add the percentages to check work. 11% 88. 9% 100. % Answer

Empirical Formula Example Two What is the empirical (simplest) formula containing 69. 58% Ba,

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. Q Mass E 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 Ba. CO 3 X by 1 to get whole numbers

Percent Composition Example Two Calculate the percentage composition of Fe(Cl. O 4)3. 1)Calculate the

Percent Composition Example Two Calculate the percentage composition of Fe(Cl. O 4)3. 1)Calculate the formula mass for 1 mole of Fe(Cl. O 4)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. 3 g/mol 2) Divide the each contribution by the total mass. Fe 55. 8 ÷ 354. 3 = ( 0. 1575 x 100) = 15. 8% Cl 106. 5 ÷ 354. 3 = ( 0. 3006 x 100) = 30. 06% Answer O 192. 0 ÷ 354. 3 = (0. 5419 x 100) = 54. 19% 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 Al 2

Formula Mass Example Three Calculate the formula mass for 1 mole of Al 2 O 3 E Al O # Mass 2 x 27. 0 = 54. 0 3 x 16. 0 = 48. 0 102. 0 g/mol 26. 98154 15. 9994 How many molecules of Al 2 O 3 is 102. 0 g/mol? 6. 022 x 10+23 molecules

Formula Mass Example Two Calculate the formula mass for 1 mole of Ca. CO

Formula Mass Example Two Calculate the formula mass for 1 mole of Ca. CO 3. E Ca C O # Mass 1 x 40. 1 = 40. 1 1 x 12. 0 = 12. 0 3 x 16. 0 = 48. 0 100. 1 g/mol 40. 078 12. 011 15. 9994 How many molecules of Ca. CO 3 is 100. 1 g/mol? 6. 022 x 10+23 molecules