“Passes” – 4 oxygens “-ate” ending Polyatomic Ions “Passes” – The Big Four P As S Se -3 -3 -2 phosph ate P O4 -3 arsen ate O4 As Phosph orus Sulf ur -2 -3 -2 selen ate O4 Se -2 sulf ate O4 S Arsen ic Selen ium “Passes” – 4 oxygens “-ate” ending

“Passes” – 3 oxygens “-ite” ending Polyatomic Ions “Passes” – The Big Four P As S Se -3 -3 -2 phosph ate P O4 -3 phosph ite P O3 Phosph orus Sulf ur O4 S -2 -3 -2 ate sulf ite sulf O3 S -2 Arsen ic Selen ium “Passes” – 3 oxygens “-ite” ending

P As S Se Polyatomic Ions “Passes” Recap -3 -2 -3 -2 ate O4 ite O3 Charge on polyatomic ion determined by how many positions it is away from noble gas

Little Three - 3 oxygens “-ate” ending Polyatomic Ions The Little Three Cl -1 -1 chlor ate Cl O3 -1 -1 Br brom ate O3 Br -1 ate O3 iod I -1 I Little Three - 3 oxygens “-ate” ending

Little Three - 2 oxygens “-ite” ending Polyatomic Ions Cl -1 -1 chlor ate Cl O3 -1 chlor ite O2 Cl -1 Br I O3 -1 ate iod -1 I ite O2 I -1 iod Little Three - 2 oxygens “-ite” ending

Cl Br I Polyatomic Ions -1 Recap -1 -1 ate O3 ite O2 Charge on polyatomic ion determined by how many positions it is away from noble gas. I

Polyatomic Ions nitrate NO3 -1 nitrite NO2 -1 carbonate CO3 -2 One less oxygen! carbonate CO3 -2 Hydrogen carbonate HCO3 -1 Adding a hydrogen changes charge to -1 ! chlorate ClO3 -1 perchlorate ClO4 “per” means one more oxygen than -ate

di (2) chromate (7 oxygens) Polyatomic Ions -2 -2 chromate CrO4 dichromate Cr2O7 di (2) chromate (7 oxygens) -1 hydroxide OH +1 ammonium NH4 -1 acetate CH3COO -1 permanganate MnO4

Daily Challenge 1/4/2012 How can the periodic table be used to make predictions about elements?

Ba(OH)2 + 2NaClO3 -> Ba(ClO3)2 + 2NaOH Where are we going? Naming and writing compounds and reactions Describing how and why atoms bond to form compounds Ba(OH)2 + 2NaClO3 -> Ba(ClO3)2 + 2NaOH Barium hydroxide and sodium chlorate react to produce barium chlorate and sodium hydroxide

The Great Divide Metals, Non-Metals, Metalloids, and Noble Gases

Metals Non - Metals Most of the Periodic Table Most abundant elements Lose electron(s) to form positively charged ions (“cations”) Form ionic bonds with non-metals Form metallic bonds with metals Most abundant elements Gain electron(s) to form negatively charged ions (“anions”) Form ionic bonds with metals Form covalent bonds with non-metals

Metalloids Noble Gases Can either gain or lose electrons Can either form covalent, ionic or metallic bonds Do not gain or lose electrons 8 valence electrons; full “octet” Very stable; few chemical compounds

Recall…. Atoms are electrically neutral. # of protons = # of electrons. Electrons are located outside of the nucleus.

What if… # of protons  # electrons? How many electrons can a single atom gain or lose? What would its resulting charge be? How do I know if an atom gains or loses electrons? What do we know about electrons, do they really just surround the atom in an “electron cloud”?

Niels Bohr - 1913 Proposed that electrons in an atom can reside only in certain energy levels or orbitals; the energy of an electron in an atom is quantized. Niels Bohr Nobel Laureate 1922

Bohr model Bohr viewed electron orbits as energy levels. Electrons resided in these levels and never in between. Since an electron is assigned to a given energy level/orbit its energy is quantized.

Each orbital holds a known amount of electrons Bohr model 1st orbital holds 2 e- 4th orbital holds 8 e- 4th orbital holds 8 e- 3rd orbital holds 8 e- 3rd orbital holds 8 e- 2nd orbital holds 8 e- Each orbital holds a known amount of electrons

Example Bohr model Ca - 20 p+ & 20 e- 20 p+ 2 e- 8 e- 8 e- 2 e-

Valence Electrons Electrons present in the outermost orbital (energy level) of an atom that are used for bonding. 20 p+ Calcium has two valence electrons 2 e- 8 e- 8 e- 2 e-

Bohr Diagram Practice Calcium Nitrogen Sodium Fluorine

Lewis Dot Structure Illustrates the valence electrons associated with a given atom. The notation consists of a chemical symbol surrounded by dots (max. two per side) representing valence electrons. PZ X PY S Px

Lewis Dot Structure Rules First two valence electrons are placed at the “s” position. Each additional valence electron is placed individually in Px, PY, Pz. Valence electrons are paired in Px, PY, Pz only after each has one electron. PZ X PY S Px

X X Lewis Dot Structure PZ PY S Px 2 valence electrons “s” gets filled first 2 valence electrons PY S Px

X X Lewis Dot Structure PZ PY S Px 5 valence electrons 1 electron into PZ X 5 valence electrons PY S “s” gets filled first 1 electron into PY Px 1 electron into PX

Lewis Dot Structure Practice Calcium Nitrogen Sodium Fluorine

Gain or lose electrons? Atoms will gain or lose valence electron(s) to achieve a full outer orbital (generally 8). Calcium atom 20 p+ 2 e- 8 e- 8 e- 2 e- Gain 6e- Lose 2e- 20 p+ 2 e- 8 e- 20 p+ 2 e- 8 e-

Gain or lose electrons? Atoms will gain or lose valence electron(s) to achieve a full outer orbital (generally 8). Fluorine atom 9 p+ 2 e- 7 e- Gain 1e- Lose 7e- 9 p+ 2 e- 8 e- 9 p+ 2 e-

Gain or lose electrons?

Draw a Bohr diagram and a Lewis dot structure for the following elements Phosphorus Magnesium Oxygen Argon

Vocabulary Monatomic Ion-Consists of a single atom with a + or – charge Polyatomic Ion-A tightly bound group of atoms that behave as a unit and carry a net charge. Binary Compound-Compound composed of two different elements

Cations – Positive Ions Formed when # p0  # e- 20 p+ 2 e- 8 e- 20 p+ 2 e- 8 e- Lose 2e- Calcium atom Calcium ion 20 p+ + 18 e- = +2 20 p+ + 20 e- = 0 Ca Calcium atom Ca+2 Lose 2e- Calcium ion METALS LOSE ELECTRONS TO FORM POSITIVE IONS “CATIONS”

NONMETALS GAIN ELECTRONS TO FORM NEGATIVE IONS “ANIONS” Anions – Negative Ions Formed when # p0  # e- 9 p+ 2 e- 7 e- Fluorine atom 9 p+ + 9 e- = 0 9 p+ 2 e- 8 e- Fluoride ion Gain 1e- 9 p+ + 10 e- = -1 Fluoride ion F -1 Gain 1e- F Fluorine atom NONMETALS GAIN ELECTRONS TO FORM NEGATIVE IONS “ANIONS”

Monatomic Ions If the ion is negatively charged its name will have an –ide ending. Gain 1e- F Fluorine atom Fluoride ion -1 Gain 3e- N Nitrogen atom Nitride ion -3

Monatomic Ions Na Na Be Be +1 +2 If the ion is positively charged and found in column 1, 2 or is Al, its name will have a (metal) ion ending. +1 Na Na Lose 1e- Sodium atom Sodium ion +2 Be Be Lose 2e- Beryllium atom Beryllium ion

Monatomic Ions – Transition Metals Transition metals form cations The charge on the transition metal is given in roman numerals. Ti (IV) = Ti+4 “Titanium four” “Titanium four ion” Fe (III) = Fe+3 “Iron three” “Iron three ion”

For each of the following give the lewis dot structure, the ion symbol, and the name: Potassium Sulfur Iodine Beryllium

BINARY IONIC COMPOUNDS 2 elements (anion(-) + cation(+)) Metal ALWAYS written 1st Overall compound charge = ZERO Always ends in – ide.

Writing Ionic Compound Formulas 1 Formulas are written so that the overall charge on the compound is zero. By rule, cations are always written first. Na + Cl 1 : 1 Na+1 Cl-1 1 1 +1 -1 1 (+1) + 1 (-1) = 0 NaCl Sodium chloride

Writing Ionic Compound Formulas 1 Formulas are written so that the overall charge on the compound is zero. By rule, cations are always written first. 1 : 2 Mg+2 F- Mg + F 1 2 +2 -1 1 (+2) + 2 (-1) = 0 MgF2 Magnesium fluoride

Writing Ionic Compound Formulas 1 Formulas are written so that the overall charge on the compound is zero. By rule, cations are always written first. Mg+2 N-3 Mg + N 3 2 +2 -3 3 (+2) + 2 (-3) = 0 Mg3N2 Magnesium nitride 3 : 2

Mg N Mg Mg N + N Mg N A Little Tip… - + 2 3 + 2 - 3 1 Formulas are written so that the overall charge on the compound is zero. By rule, cations are always written first. Mg N Mg Mg N - + 2 3 + 2 + N - 3 Mg N

Writing Ionic Compound Formulas 2 Formulas are expressed in the smallest whole numbers possible. Incorrect Formulas Correct Formulas Ca2O2 CaO Al3N3 AlN Li3N Sn2O4 SnO2

Practice Write the formula or name for the following: Barium sulfide Magnesium nitride Chromium (II) chloride Titanium (IV) oxide Aluminum bromide

Practice Write the name for the following: K3N MgF2 PbO2 CuS

Daily Challenge 12/9 Given the following information indicate the formula or name Iron (II) sulfide PbO2 Na2S Magnesium phosphide

Polyatomic Ion Group of atoms that have a positive or negative charge. The name and charge of a polyatomic ion depends on the atoms in the group. Sulfate ion SO4-2 Phosphate ion PO4-3

PbSO4 Lead sulfate NaCl Ionic Compounds Formed between a metal and non-metal. Binary compounds contain two different atoms. Ternary compounds contain three different atoms. NaCl sodium chloride PbSO4 Lead sulfate

Writing Ionic Compound Formulas 3 Parentheses are used…. a. only around polyatomics and b. only if more than 1 of that polyatomic is needed to make a neutral compound

Mg+2 + (PO4)-3 Mg3(PO4)2 Writing Ionic Compound Formulas 3 Parentheses…. Mg+2 + (PO4)-3 Mg3(PO4)2 As a group has -3 charge!! Parentheses because... a) polyatomic b) more than one (2) Magnesium phosphate

Li+1 + (PO4)-3 Li3(PO4)1 Li3PO4 Writing Ionic Compound Formulas 3 Parentheses…. Li+1 + (PO4)-3 Li3(PO4)1 As a group has -3 charge!! Li3PO4 CORRECT!!! NO parentheses because... b) not more than one Lithium phosphate

Writing Ionic Compound Formulas 3 Parentheses…. Al+3 + (PO4)-3 Al3(PO4)3 INCORRECT!!! Can be reduced… Al1(PO4)1 INCORRECT!!! No parentheses… 1 Al atom assumed 1 polyatomic group AlPO4 CORRECT!!! Aluminum phosphate

Practice… Lithium sulfate Calcium chlorate Lead (IV) phosphate Nickel (II) phosphide Aluminum acetate Copper (II) carbonate

Practice… MgCr2O7 Pb(ClO4)4 CrS K3PO4 (NH4)2SO4 Sn(CrO4)2

Daily Challenge 1/10/12 Complete the following table Compound name Cation Anion Formula Barium sulfate Mg2+ Cl1- Fe(SO4)2

Daily Challenge 1/9/12 Iron (IV) phosphide SnSO4 Potassium nitrite For the following, give the formula or name Iron (IV) phosphide SnSO4 Potassium nitrite

The surface of Venus consists of sulfuric acid, H2SO4 Acids A neutral ionic compound that contains one or more hydrogen ions (H+1) as the cation. Produces hydrogen ions (H+1) when dissolved in water. This is what Acid is... The surface of Venus consists of sulfuric acid, H2SO4

Monatomic or polyatomic anion Acids Have a general formula of… HnX Monatomic or polyatomic anion Indicates the number of hydrogen atoms that combine with anion (X) to form neutral compound

Naming Acids Anion (X) ending Acid name ide hydro – (stem) – ic acid ite (stem) – ous acid - ate (stem) – ic acid (chlor)ide, Cl-1 Hydro(chlor)ic acid (sulf)ite, SO3-2 (sulfur)ous acid (nitr)ate, NO3-1 (nitr)ic acid

HnX Writing Acid Formulas Work backwards from acid name to determine anion. Add enough hydrogen ions (H+1) to anion to make neutral compound. HnX

Example Hydrofluoric acid 1 Determine anion name fluoride Determine anion symbol F-1 Make anion neutral by adding H+1 HF

Example Chlorous acid 2 Determine anion name chlorite Determine anion symbol ClO2-1 Make anion neutral by adding H+1 HClO2

Example Sulfuric acid 3 Determine anion name sulfate Determine anion symbol SO4-2 Make anion neutral by adding H+1 H2SO4

Bases A neutral ionic compound that contains one or more hydroxide ions (OH-1) as the anion. Produces hydroxide ions (OH-1) when dissolved in water. Naming and writing bases is same as ionic compounds with polyatomic ions…

Practice… H3N LiOH H3PO4 H2SO3 Cr(OH)3 HF

Practice… Magnesium hydroxide Hydrophosphoric acid Nitrous acid Iron (IV) hydroxide Sulfuric acid

Daily Challenge 12/16 Complete the following table with the correct information. Compound Name Cation Anion Formula Hydronitric acid H2CrO4 CrSO4

Binary Molecular Compounds Composed of two nonmetals include B, Si & H as nonmetals Consist of uncharged molecules, not charged ions like ionic compounds. Have varying ratios of elements C O C O Carbon dioxide CO2 Carbon monoxide CO

Naming Binary Molecular Compounds The name must identify the elements in the molecule and indicate the amounts of each atom in the molecule. The second element in all binary molecular compounds always ends in – ide. Prefixes are used to indicate the number of each atom in the molecule. EXCEPTION: If the first element only has 1 atom no prefix is used NEVER reduce a molecular compound

Prefix Number Mono 1 Di 2 Tri 3 Tetra 4 Penta 5 Hexa 6 Hepta 7 Octa 8 Nona 9 Deca 10

Examples – Molecular Compounds MAKE SURE THE COMPOUND CONSISTS OF TWO NONMETALS!!! 1 N2O nitrogen oxygen Apply prefixes!! dinitrogen monoxygen Last element – ide dinitrogen monoxide

Examples – Molecular Compounds MAKE SURE THE COMPOUND CONSISTS OF TWO NONMETALS!!! 2 CBr4 carbon bromine Apply prefixes!! carbon tetrabromine No prefix on first atom because only 1 atom Last element – ide carbon tetrabromide

Examples – Molecular Compounds MAKE SURE THE COMPOUND CONSISTS OF TWO NONMETALS!!! 3 B2H4 boron hydrogen Apply prefixes!! diboron tetrahydrogen Last element – ide diboron tetrahydride

Examples – Molecular Compounds MAKE SURE THE COMPOUND CONSISTS OF TWO NONMETALS!!! 4 Tetracarbon dihydride 4 carbon 2 hydrogen C4H2 Do Not reduce!!

Naming Review - ide ending = binary compound (ionic = charges) - ate or - ite ending = ionic compound with polyatomic. Bases = OH-1 or hydroxide Molecular = prefixes & no charges Acids (H+1)  hydro = binary (2 elements) ic = ate polyatomic (> 2 elements) ous = ite polyatomic (1 less O than ate)

Practice… N2O4 CrO P2N3 HClO3 CCl5 Mg(ClO4)2 Pb(OH)4 H2S Trinitrogen disulfide Carbon octafluoride Ammonium phosphate Sodium sulfide Nitrous acid Manganese (III) nitrate Hydrosulfuric acid

Dinitrogen trihydride Mg3(PO4)2 Sulfurous acid Cl3F5 Daily Challenge 12/18 For the following, give the formula or name Dinitrogen trihydride Mg3(PO4)2 Sulfurous acid Cl3F5

Law of Definite Proportions Joseph Louis Proust (1754 – 1826) Each compound has a specific ratio of elements It is a ratio by mass Water is always 8 grams of oxygen for every one gram of hydrogen Photo pg 100 Ihde text (Edgar Fahs SmithCollection) Joseph Louis Proust (1754- 1826), French chemist given credit for law of definite composition. Whether synthesized in the laboratory or obtained from various natural sources, copper carbonate always has the same composition. Analysis of this compound led Proust to formulate the law of definite proportions.

Law of Definite Proportions A compound contains the same elements in exactly the same proportions by mass regardless of the size of the sample or source of the compound. Is the composition of Cookeville water same as that of Boston or Tsunami water? A compound has the same elements in a certain definite proportion and no other combinations

Law of Definite Proportions Whether synthesized in the laboratory or obtained from various natural sources, copper carbonate always has the same composition. Analysis of this compound led Proust to formulate the law of definite proportions. + + 103 g of copper carbonate 53 g of copper 40 g of oxygen 10 g of carbon

The mass ratio is fixed as 10:1.55 for the reaction • Is it possible to tell when reaction is complete or when too much starting material is present? • Conclusion: The mass ratio is fixed as 10:1.55 for the reaction

Law of Multiple Proportions John Dalton (1766 – 1844) If two elements form more than one compound, the ratio of the second element that combines with 1 gram of the first element in each is a simple whole number. e.g. H2O & H2O2 water hydrogen peroxide Ratio of oxygen is 1:2 (an exact ratio)

What? Water is 8 grams of oxygen per gram of hydrogen. Hydrogen peroxide is 16 grams of oxygen per gram of hydrogen. 16 g to 8 g is a 2:1 ratio True, because you have to add a whole atom, you can’t add a piece of an atom.

Law of Multiple Proportions Elements can combine in different ways to form different compounds, but the mass ratios of the different substances are small, whole-number multiples of each other.

Practice… Hydronitric acid Tin (II) phosphate Dinitrogen pentachloride Barium hydroxide Carbon trioxide Lead (IV) sulfide Chlorous acid

Daily Challenge 12/21 Explain how the ending of a name determines the type of compound you have.

Chapter 9 Review Vocab Bohr Diagrams Lewis Dot Structures Monatomic/polyatomic Cation/anion Acid/base Binary compounds (ionic/molecular) Bohr Diagrams Lewis Dot Structures Identifying charge by Group # Identifying metal/nonmetal

Chapter 9 Review Naming Ionic vs. Molecular When to use roman numerals When to use prefixes Ionic vs. Molecular Difference between name endings ide ate ite

Chapter 9 Review How to identify Laws of multiple proportions Acid/base/neither Molecular/ionic Laws of multiple proportions Laws of definite proportions (composition) Table (like homework) ~10 compounds Formula from name & Name from formula ~40 Draw Bohr diagrams and Lewis Dots Mass ratio problem

Vocab Ions Formulas Names Misc 100 200 300 400 500

CONSISTS OF A GROUP OF ATOMS WITH A POSITIVE OR NEGATIVE CHARGE VOCABULARY – 100 CONSISTS OF A GROUP OF ATOMS WITH A POSITIVE OR NEGATIVE CHARGE POLYATOMIC ION

ATOM OR GROUP OF ATOMS HAVING A NEGATIVE CHARGE VOCABULARY – 200 ATOM OR GROUP OF ATOMS HAVING A NEGATIVE CHARGE ANION

PRODUCES A HYDROXIDE ION WHEN DISSOLVED IN WATER VOCABULARY – 300 PRODUCES A HYDROXIDE ION WHEN DISSOLVED IN WATER BASE

TYPE OF COMPOUND FORMED BETWEEN A METAL AND NON-METAL VOCABULARY – 400 TYPE OF COMPOUND FORMED BETWEEN A METAL AND NON-METAL IONIC

TO SUBDIVIDE (AS ENERGY) INTO SMALL BUT MEASURABLE INCREMENTS VOCABULARY – 500 TO SUBDIVIDE (AS ENERGY) INTO SMALL BUT MEASURABLE INCREMENTS QUANTIZE

IONS – 100 ALUMINUM ION Al+3

IONS – 200 SULFITE SO3-2

IONS – 300 AMMONIUM NH4+1

IONS – 400 MnO4-1 PERMANGANATE

IONS – 500 PHOSPHITE PO3-3

FORMULAS – 100 ALUMINUM HYDROXIDE Al(OH)3

Diboron tetrachloride FORMULAS – 200 Diboron tetrachloride B2Cl4

FORMULAS – 300 Lithium phosphate Li3PO4

Manganese (IV) carbonate FORMULAS – 400 Manganese (IV) carbonate Mn(CO3)2

FORMULAS – 500 SULFUROUS ACID H2SO3

Dicarbon tetrahydride COMPOUND NAMES – 100 C2H4 Dicarbon tetrahydride

COMPOUND NAMES – 200 Cu3PO4 Copper (I) phosphate

COMPOUND NAMES – 300 MgN Magnesium Nitride

COMPOUND NAMES – 400 H3S Hydrosulfuric Acid

COMPOUND NAMES – 500 H3PO3 Phosphorous acid

THE LEWIS DOT STRUCTURE FOR ALUMINUM MISCELLANEOUS – 100 THE LEWIS DOT STRUCTURE FOR ALUMINUM Al

THE BOHR DIAGRAM FOR THE FLUORINE ATOM MISCELLANEOUS – 200 THE BOHR DIAGRAM FOR THE FLUORINE ATOM 9 p+ 2 e- 7 e-

MISCELLANEOUS – 300 THIS ARTIST HOLDS THE RECORD FOR THE BIGGEST ALL-TIME SALES FOR A SOLO ARTIST MICHAEL JACKSON

MISCELLANEOUS – 400 GROUP OF ATOMS THAT ARE THE MOST ABUNDANT AND FORM BOTH IONIC AND COVALENT BONDS NON-METALS

“GUILTY UNTIL PROVEN INNOCENT” IS THE STANDARD FOR THIS FEDERAL AGENCY MISCELLANEOUS – 500 “GUILTY UNTIL PROVEN INNOCENT” IS THE STANDARD FOR THIS FEDERAL AGENCY IRS