Bellringer: 3/7/2018 **Get out the periodic table you colored and answer the following: Where can you find the halogens? What is the most reactive nonmetal What 2 elements are liquid at room temperature? STOTD **Have you turned in your Unit 3 Packet?

The Periodic Table By 1860 scientists had discovered 63 elements But there was no good way to organize them Scientists had to memorized everything This was changed by Mendeleev end

The Periodic Table Mendeleev’s Periodic Table: Elements with similar properties were placed in the same column The mass of the elements increased along each row end

The Periodic Table Mendeleev left several blank spaces in his periodic table For elements that had not been discovered yet He correctly predicted the properties of these elements based on the elements around them end

The Periodic Table The Modern Periodic Table: Based on Mendeleev’s table Similar Properties are in the Same Column Columns are called Groups Numbered 1 to 18 (from left to right) Atomic Numbers increase going across the table Rows are called Periods Numbered 1 to 7 (from top to bottom) end

The Periodic Table This is the full Periodic Table As you can see it is REALLY long Way too long to fit on a page end

The Periodic Table To make everything fit on 1 page, the Lanthanides and Actinides are moved to the bottom end

The Periodic Table Metals Left of the stair-step line Francium (Fr) is the most reactive Moving away from Fr, metals become less reactive Good conductors of electricity and heat Mostly solids at room temperature High melting and boiling points Malleable and ductile end

The Periodic Table Nonmetals Right of the stair-step line Fluorine (F) is the most reactive nonmetal Moving away from F, nonmetals become less reactive Poor conductors of heat and electricity Mostly gases at room temperature Low melting and boiling points Not malleable and not ductile end

The Periodic Table Metalloids Touching the stair-step line Have properties between metals and nonmetals Depends on the temperature end

The Periodic Table: Group Names Alkali Metals Lanthanide and Actinide Series Group 1 At the bottom of the table EXTREMELY REACTIVE! All are radioactive Alkaline Earth Metals Halogens Group 2 Group 17 Transition Metals Highly Reactive Groups 3 to 12 Noble Gases Have a wide variety of properties Group 18 Extremely Unreactive THEY DO NOTHING! end

The Periodic Table Atomic Size Valence Electrons Francium (Fr) is the largest atom Helium (He) is the smallest atom The closer to Fr, the larger the atom Valence Electrons Electrons in the highest energy level Give Elements their Chemical Properties Group: 1 2 13 14 15 16 17 18 # of 1 2 3 4 5 6 7 8 Valence: end

Chemical Bonds Chapter 6

Chemical Formulas Chemical Formula CO2 NaCl MgCl2 Na3P Shows what elements are in a compound If there is more than 1 atom of an element we add subscripts to show how many CO2 NaCl MgCl2 Na3P 1 C and 2 O 1 Na and 1 Cl O C O 1 Mg and 2 Cl CO2 3 Na and 1 P end

Chemical Formulas 7 5 3 8 4 How many total atoms are in each of these: H2SO4 KNO3 CaCl2 C2H6 H2O2 H2O Fe2O3 Hg2Cl2 7 5 3 8 4 O H O S O H H H2SO4 end

Chemical Formulas Some compounds have large groups of atoms Polyatomic Ions OH-, PO43-, NO3-, NH4+ Last page of your Reference Tables!!! If there is more than 1 Polyatomic Ion, Write the group inside ( ) And put a subscripts outside to tell how many end

Chemical Formulas Ba(OH)2 Cu (NO3)2 NH4NO3 (NH4)2O 1 Ba 1 Cu 2 OH end

Chemical Formulas How many total atoms are in each of these: Cu(NO3)2 KMnO4 Ba(OH)2 NH4Br Ca3(PO4)2 Al2(SO4)3 (NH4)3PO4 Mg(C2H3O2)2 9 6 5 13 17 20 15 end

Bellringer: How many atoms are in the following: STOTD H2SO4 KNO3 CaCl2 C2H6 STOTD

Electron Configuration Valence Electrons Valence Electrons are found in the highest energy level Electron Dot Diagrams are used to show the number of valence electrons Write the symbol for the element Place large dots around the symbol to represent each valence electron Put 1 dot on each side before pairing them up end

Valence Electrons “1,2, skip a few…” 1 8 2 3 4 5 6 7 Transition Metals beat to their own drum!

Electron Configuration Draw diagrams for the following: Sr Si Cl end

Bellringer: Draw an electron dot diagram for Sulfur. Count the total atoms: CaCO3 KBr Mg(NO3)2 3. STOTD

What is a valence electron? Bellringer: What is a valence electron? Draw a Bohr model for carbon-13. How many valence electrons does it have? STOTD

Electron Configuration All atoms want to have 8 valence electrons Atoms with 8 valence do not react with other things In order to get 8 valence atoms can either: Transfer Electrons: Lose Electrons Gain Electrons till they have 8 Share Electrons with other atoms, so everyone has 8 end

Chemical Bonding Chemical Bond 3 types The force that holds atoms or ions together 3 types Ionic Metal and Nonmetal (Including Polyatomic Ions) Covalent Nonmetal and Nonmetal Metallic Metal and Metal end

Chemical Bonding I C I C Identify the following as ionic or covalent CaCl2 LiBr CO2 SO3 H2O CH4 BaSO4 Na2CO3 K2O NaF MgO NH4Cl HCl KI I C I C end

Ionic Bonding Ionic Bonding Holds cations and anions together Between a metal and a nonmetal (or polyatomic ion) Electrons are transferred from the cation to the anion Cation Metal Anion Nonmetal end

Cation A positively charged atom, usually a metal Has Lost Electrons Anion A negatively charged atom, usually a nonmetal Has Gained Electrons

Ionic Bonding Groups 1, 2, 13 lose electrons/cations Group 14 can either gain or lose electrons Groups 15, 16, 17 gain electrons/anions As the number of electrons changes the atom becomes an ion (has a charge) This charge is called an Oxidation State end

Ionic Bonding Oxidation States follows the # of Valence Electrons There is a PT trend for Oxidation states! Oxidation States follows the # of Valence Electrons 1 2 13 14 15 16 17 18 Group Oxidation ve +1 0 +2 +3 +4 -3 -2 -1 1 8 2 3 4 5 6 7 end

Ionic Bonding We can show the transfer of electrons using an Electron Dot Diagram Start with sodium chloride (NaCl) Na + Cl  [ ]+ [ ]- Na Cl Draw Electron Dot Diagrams for: KF MgO MgCl2 end

Bellringer: What is an oxidation state? What is the oxidation state for group 1 elements? How are cations and anions different? STOTD

Ionic Bonding Ionic Compounds form a structure called a Crystal Lattice The cations and anions alternate to form a cube Cl- Na+ end

Naming Ionic Compound Naming Ionic Compounds is easy. There are 3 steps Name the Cation (the metal) Name the Anion (the nonmetal) Change the Ending on the anion to –ide Sodium Bromine Bromide Sodium NaBr Name the following: BaS MgF2 Ca3N2 end

Write the names of the following compounds: KCl BeO Na3P LiBr

Naming Ionic Compounds If there are more than 2 elements, YOU HAVE A POLYATOMIC ION!!! LOOK AT YOUR REFERENCE TABLE!!! Follow the same steps to name the compound Get the polyatomic’s name from the reference tables! But don’t change the endings for polyatomic ions NaNO3 Sodium Nitrate Name the following: (NH4)2O KOH Sr3(PO4)2 NaC2H3O2 end

Bellringer: Explain the difference between an ionic bond and a covalent bond. How would you name the following compounds: CaCl2 Ba(NO3)2 STOTD **ELEMENT QUIZ TODAY ** IONIC BONDING QUIZ FRIDAY

Writing Ionic Formulas To write formulas from the names: There are 3 easy steps: Write the positive ion, with charge Write the negative ion, with charge Cross the charge numbers to get your subscripts Do NOT put the “+” or “-” Write the formulas for the following: Beryllium Phosphide Calcium Fluoride Lithium Iodide Strontium Sulfide end

Writing Ionic Formulas Watch out for Polyatomic Ions Follow the same steps to write the formula Remember: The polyatomic ion IS A GROUP When you cross charges, the subscript applies to the WHOLE GROUP Write the formula for the following: Potassium Nitrate Barium Chlorate Aluminum Acetate Ammonium Sulfate end

Bellringer: What is the chemical formula for Francium Sulfide? What is the chemical formula for Aluminum Phosphate? What is the name of SrCl2? What is the name of Mg(OH)2? STOTD **Ionic bonding quiz on Friday

Transition Metals Transition Metals have 2 valence electrons But they have Many Oxidation States So we write their names differently end

Transition Metals Follow the same steps to write the formula The metal's charge is the Roman Numeral Vanadium (III) Sulfide V3+ S2- V2S3 Metal's Charge end

Transition Metals Write formulas for the following: Osmium (V) Fluoride Silver (I) Nitride Technetium (VII) Phosphate end

Transition Metals When naming you MUST put the charge as a Roman Numeral! To figure out the charge, uncross the subscripts! Fe2O3 Fe3+ O2- iron (III) oxide end

Transition Metals Name the following: HgF2 Hf2S5 YP end

Naming Ionic Compounds Complete the following on “Naming Binary Compounds (Ionic)” 3 12 4 13 5 16 6 19 7 20

HW Silver (I) oxide Copper (I) bromide Copper (II) bromide Iron (II) oxide Iron (III) oxide Chromium (II) chloride Chromium (III) chloride Mercury (I) Iodide Manganese (II) oxide Manganese (III) oxide

Bellringer: Compare and contrast metals and nonmetals. Be sure to mention the differences in their properties. How are transition metals different from all of the other elements on the periodic table. STOTD

Bellringer: Name the following: Write formulas for the following: Ca(OH)2 MgO Ti2S3 Write formulas for the following: Potassium chloride Barium phosphate Iron (II) bromide ***STOTD

Bellringer: Identify each bond as either covalent or ionic: N2O CaS CO2 Draw an electron dot diagram for iodine. How many atoms of sodium are there in sodium phosphide? STOTD

Covalent Bonding Covalent Bond Between a nonmetal and a nonmetal Atoms SHARE electrons There are 7 nonmetals that never exist by themselves. form pairs with each other These are called the Diatomics (H, N, O, F, Cl, Br, I) BrIN-Cl-HOF Look for the 7 on the P.T. end

Covalent Bonding The number of electrons that are shared create different types of bonds 2 shared electrons — single bond 4 shared electrons = double bond 6 shared electrons ≡ triple bond end

Covalent Bonding Show the electrons being shared with an Electron Dot Diagram Start with chlorine (Cl2) Cl + Cl  Cl Cl end

Covalent Bonding Draw the Electron Dot Diagrams for: H2 N2

Covalent Bonding Atoms never share electrons equally These are called Polar Molecules 1 side is negative Has the electrons And 1 side is positive It doesn’t have the electrons end

Naming Covalent Molecules Number Prefix 1 Mono- 2 Di- 3 Tri- 4 Tetra- 5 Penta- 6 Hexa- 7 Hepta- 8 Octa- 9 Nona- 10 Deca- When naming Covalent Molecules: Use a prefix for the first element If it is 1, do NOT use a prefix Name the first element Use a prefix for the second element Always!!! Name the second element and change the ending to –ide end

Naming Covalent Molecules Practice: As2O3 N2H4 CCl4 SO end

Naming Covalent Molecules Complete 1-10 on “Naming Molecular Compounds”

Writing Covalent Formulas Writing the formula for covalent molecules is easy: Write the symbol of the first element Use the prefix to write the subscript Write the symbol of the second element end

Formulas of Covalent Molecules Practice: Disulfur trioxide Dinitrogen monoxide Phosphorus pentachloride Diphosphorus pentoxide Carbon dioxide end

Bellringer: Name the following: Write formulas for the following: As2O3 N2H4 BaO K3PO4 Write formulas for the following: Dinitrogen monoxide Phosphorus pentachloride Francium Phosphide Magnesium Sulfate STOTD

Metallic Bonding Metallic Bond Between metals In metallic bonds valence electrons are shared between all of the atoms in the substance A “sea of electrons” end

Metallic Bonding The more valence electrons metals have to share the stronger the metallic bond will be Because there is a sea of electrons metals are malleable and conduct electricity Alloy Mixture of 2 or more elements 1 element must be a metal Alloys with specific properties can be created by mixing different types of elements in different amounts end

Properties of Ionic Bonds Conduct electricity when dissolved Not Malleable Not flammable High melting point and high boiling point Form a crystal

Properties of Covalent Bonds Will not conduct electricity Malleable Flammable Low melting point and boiling point Have many structures