Unit One

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

Two Classes of Elements What are the Two Main Classes of Elements? Metals and Nonmetals Noble Elements

What Makes Elements Stable? (Lose e -1 ) (Gain e -1 ) Losing or Gaining e -1. Do metals Lose or Gain e -1 ? Do nonmetals Lose or Gain e -1 ? Oxidation Reduction

Stabilizing Sodium How many e -1 for Na? 11e -1 What is the noble element closest to Na? Ne How many e -1 for Ne? 10e -1 Sodium loses/gains how many electrons? 1e -1 Na  Na +1 + e -1 (protons) + (electrons)=charge (+11)(-10)+1 Oxidation or reduction?

Stabilizing Oxygen How many e -1 for O? 8e -1 What is the noble element closest to O? Ne How many e -1 for Ne? 10e -1 Oxygen loses/gains how many electrons? 2e -1 O + 2e -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 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? 2e -1 means Na 2 O two Na one O High Electronegativity Low Electronegativity

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, 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 Finding Oxidation Numbers 2(+3)+3(S)=Zero sum of the oxidation #’s = Find Ox #’s for Al 2 S 3 ? zero 2(Al)+3(S)=Zero S =

Example Two Finding Oxidation Numbers sum of the oxidation #’s = zero Find Ox #’s for Ca 3 (PO 4 ) 2 ? 3(Ca)+8(O)=Zero +5 2(P)+ 3(+2)+8(-2)=Zero2(P)+ =+5P

Finding Oxidation #’s for Compounds H 3 PO 4 H2OH2O HNO H 2 SO Hg 2 SO Na 2 Cr 2 O H 2 CO (NH 4 ) 2 CO Ca 3 (AsO 4 ) Fe 2 (SO 4 ) Ba(ClO 4 ) Al 2 (CO 3 )

Formula of Water Lab A Water will be converted in to elements by passing and electric current through the water. Acid( contains + and -ions) is needed in order to pass an electric current through water.

Lab A Setup

Formula of water Lab A results 7. What gasses are being produced in the tubes? 8. When the electrode-tube with the most gas is 2/3 full, switch the alligator clips and finish filling the tubes. Observations 9. What is the identity of the gas with greater volume?

Formula of water Lab A results QUESTIONS: 1. What is the ratio of volumes for the gases collected 2. What is the formula for water? 3. Does the result of your work confirm the ratio of elements in water's formula? 4. Explain how it does so. 5. What mixture of hydrogen to oxygen should give off the best reaction using the spark device? 6. Why was the sulfuric acid solution used in this demonstration?

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

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 NO 3 -1 SO 4 -2 N -3 Positive Negative

Example One Name the formula Fe 2 (CrO 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 CrO 4 -2

Fe 2 (CrO 4 ) 3 Fe +2 Fe +3 CrO 4 -2 Iron(II) Chromate Iron(III) Fe +2 CrO 4 -2 Iron(II) Chromate (+2) (-2) Y+=0 X=1Y=1 Fe CrO 4 X (+2) (-2) 1+=01 Fe +3 CrO 4 -2 Iron(III) Chromate (+3) (-2) Y+=0 X=2Y=3 X (+3) (-2) 3+=02 Fe 2 (CrO 4 ) 3 Example One

Al 2 (CO 3 ) 3 Al +3 CO 3 -2 Carbonate Aluminum Al +3 CO 3 -2 Aluminum Carbonate (+3) (-2) Y+=0 X=2Y=3 X (+3) (-2) 3+=02 Al 2 (CO 3 ) 3 Example Two

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

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

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

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

Eight Rows Seven 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 G 1.24G 1.50G 2.25G 3.50G 2.07G 48 beads 15 beads 18 beads 27 beads 42 beads 25 beads

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

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

Rounding Atomic Mass C Fe O Bi K Au Os Mg Na

Formula Mass Example One Calculate the formula mass for 1 mole of C 6 H 12 O 6. C H O 6 x 12 x 6 x 12.0 = 1.0 = 16.0 = g/mol E # Mass How many molecules of C 6 H 12 O 6 is 180.0g/mol? 6.022x molecules

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

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

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Empirical Formula Example Two 3) Write the formula What is the empirical (simplest) formula containing 69.58% Ba, 6.090% C, 24.32% O? X by 1 to get whole numbers 1) Calculate moles of each element. Ba C g ÷ g ÷ = = mol Ba mol C E Q Mass 2) Calculate the lowest ratio. Ba C mol ÷ mol ÷ mol = E MolesLowest Ratio BaCO 3 O24.32 g ÷16.00 = mol O O mol ÷ mol = 3.00 Mass

Percent Composition Example Two Calculate the percentage composition of Fe(ClO 4 ) 3. Cl O 3 x 12 x 35.5 = 16.0 = g/mol E # Mass 2) Divide the each contribution by the total mass. 3) Add the percentages to check work. 1)Calculate the formula mass for 1 mole of Fe(ClO 4 ) 3. Cl O ÷ ÷ = % 54.2 % 100.1% Fe 1 x55.8 = 55.8 Fe 55.8 ÷354.3 = % ( x 100) = 15.8% ( x 100) = 30.06% ( x 100) = 54.19% Answer

Formula Mass Example Three Calculate the formula mass for 1 mole of Al 2 O 3 Al O 2 x 3 x 27.0 = 16.0 = g/mol E # Mass How many molecules of Al 2 O 3 is102.0g/mol? 6.022x molecules

Formula Mass Example Two Calculate the formula mass for 1 mole of CaCO 3. Ca C O 1 x 3 x 40.1 = 12.0 = 16.0 = g/mol E # Mass How many molecules of CaCO 3 is100.1g/mol? 6.022x molecules