12/13 Do Now Draw a Bohr model for Chlorine Draw a Lewis Dot/Electron Dot diagram for Chlorine

HW: Pg 1, 2, 3 12/13 Agenda Do Now Begin Ch 13 Notes Begin HW (If time) HW: Pg 1, 2, 3

Chapter 13 Material on Midterm Chemical Bonding Chapter 13 Material on Midterm

Section 1: Electrons and Chemical Bonding Combining Atoms through Chemical Bonding Most atoms hate being alone…so they ________! Chemical bonding is the ________________ of atoms to form molecules or ionic compounds Properties of new substance are _______________ that the properties of the old substance The _________________________ is the interaction that holds the two atoms together. bond combining different chemical bond

6 + 6 + 12 = C6H12O6 aka glucose

Section 1: Electrons and Chemical Bonding Combining Atoms Through Chemical Bonding It’s all about the electrons When bonds form, electrons can… …be ______________ …be _____________ …be ________ shared gained lost

Section 1: Electrons and Chemical Bonding Electron Number and Organization We need to organize the electrons so we know what they will do if bonds are formed Review: How do I know how many electrons a neutral atom has? Same as its ________________________(proton #) atomic number

Section 1: Electrons and Chemical Bonding What are the rules for where the electrons go? 8 2

Section 1: Electrons and Chemical Bonding What are the rules for where electrons can go? NNESWESW EXCEPTION: Group 14: ____outer electrons Pattern: __________ 4 NESW

Section 1: Electrons and Chemical Bonding Outer-Level Electrons and Bonding Only the _____________ electrons are involved in forming chemical bonds The valence electrons are the electrons found in the _________________ shell of an atom valence outermost For group numbers over 10… subtract _____ to get valence electron number EXCEPT: _______ which has ____ 10 He 2

Section 1: Electrons and Chemical Bonding

Section 1: Electrons and Chemical Bonding Valence Electrons and the Periodic Table Elements in the same __________ have the same number of ___________________________(generally) If Lithium has 1…then Sodium, Potassium, rubidium, Cesium, and Francium all have…___! group valence electrons 1

Section 1: Electrons and Chemical Bonding To Bond or Not to Bond Not all atoms bond the _______ Group 18 have their outmost shell ____________. WANT TO GET TO 8! Group 8/18 already has ____ (except He), so they’re happy and DO NOT REACT same filled 8

Section 1: Electrons and Chemical Bonding To Bond or Not to Bond Filling the Outermost Level Less than 8? More likely to ___________. Will share, take, or lose electron(s) to get to the magic number What about 2? Some elements that are _________ (H, He, Li, Be), will try to get to ___ electrons for that first shell Will share, take, or lose electron(s) to get to this number react small 2

Section 2: Ionic Bonds Forming Ionic Bonds An ionic bond is a bond that form when electrons are ______________ from one atom to another atom This creates ions, which are ___________ particles that form when atoms gain or lose electrons As a result of an ionic bond, either _________ or ______________ ions can form transferred charged positive negative

Summary:

Section 2: Ionic Bonds Forming Positive ions Positive ions (cations) form when ________ atoms _______ electrons Na loses one electron---Na+ Sodium cation Ca loses two electrons –Ca2+ Calcium cation By losing electrons, metals can get to the ________ _________! Usually 8, could be 2 metal lose magic number

Summary:

Section 2: Ionic Bonds Forming Negative Ions Negative ions (anions) form when ____________ atoms ______ electrons Change ending to “ide” Cl gains one electron – Cl- Chloride anion O gains two electrons – O2- Oxide anion By gaining electrons, nonmetals can get to the ____________________! Usually 8, could be 2 nonmetal gain magic number

Predicting Ionic bonds An ionic bond would / wouldn’t form with aluminum and sodium because… An ionic bond would / wouldn’t form with Aluminum and oxygen because…

Predicting Ionic bonds An ionic bond would / wouldn’t form with sulfur and oxygen because… An ionic bond would / wouldn’t form with sulfur and neon because… An ionic bond would / wouldn’t form with sodium and neon because…

Section 2: Ionic Bonds Ionic Compounds When ionic bonds form, the number of electrons ________ by the metal EQUALS the number of electrons ____________ by the nonmetals Everyone is _________! The overall compound is neutral because the ions _________________ lost gained happy cancel out

Full sentences for full credit! Writing Prompt #2 (of 3) Write the answer What is the difference between how metals and nonmetals form ions? Even though positive and negative ions are formed, why is an atom overall neutral? Full sentences for full credit!

Writing Ionic Compounds Write the metal with its charge Write the nonmetal with its charge Criss- Cross the charges Only bring down the #, NOT the charge Examples: Sodium and Chlorine Barium and Fluorine Potassium and Oxygen Lithium and Sulfur

Naming Ionic Compounds -ide Name of Metal + nonmetal w/ ending ______ Examples: Sodium and Chlorine Barium and Fluorine Potassium and Oxygen Lithium and Sulfur

Write and name me! Lithium and oxygen Aluminum and phosphorus Magnesium and fluorine Calcium and sulfur

Section 2: Ionic Bonds crystal lattice When ions bond, they form a repeating 3D pattern called a ____________________ crystal lattice

Name and Draw! Sodium and sulfur Aluminum and Iodine

Section 3: Covalent and Metallic Bonds Atom v. molecule Atom Molecule ______ type of element _____ or more types of elements Smallest particle into which an ____________ can be divided and still be the same element Smallest particle into which a covalently bonded _____________ can be divided and still be the same compound One Two element compound

Section 3: Covalent and Metallic Bonds Covalent Bonds and Molecules A molecule is the smallest unit of a substance that keeps all the physical and chemical ______________ of that substance 2 or more atoms joined in a definite ratio properties

Section 3: Covalent and Metallic Bonds The Simplest Molecules Must have at least two covalently bonded atoms 2 of the same element? ________________ molecules Remember: HONClBrIF Hydrogen Oxygen Nitrogen Chlorine Bromine Iodine Fluorine Diatomic

Section 3: Covalent and Metallic Bonds More Complex Molecules Many different elements Many based on ___________ carbon

Section 3: Covalent and Metallic Bonds What are Covalent Bonds A covalent bond forms when atoms __________ one or more pairs of electrons Occurs between ________________ Helps them get to their MAGIC NUMBER (8 or 2) share nonmetals

Section 3: Covalent and Metallic Bonds Covalent Bonds and Molecules Easier way to draw them– _______________ Diagrams Remember, only the valence electrons are important for bonding! Electron-Dot

Covalent Compounds How to draw covalent molecules using electron dot diagrams Combine the elements where they can share electrons so each have a full outer shell. (The shared electrons are the covalent bond) Examples: Hydrogen + Chlorine Fluorine + Fluorine Water Oxygen + Oxygen

Naming Covalent Compounds Prefixes One = _______ Two = _______ Three = ______ Four = ________ Five = ________ Six = _______ Seven = ________ Eight= _______ Nine = ________ Ten = _______ Rules: Prefix + name Prefix + name –ide Rule: Do NOT use mono- on the first element Examples: CO CO2 C2H4 P2O5 N3P6 mono di tri tetra penta hexa hepta octa nona deca

Name and Draw! 3 Hydrogen and 1 Nitrogen Sulfur and 2 fluorine

88

Section 3: Covalent and Metallic Bonds Metals have properties like malleability and ductility because of their ___________________ ______________________ are bonds from between the attraction of positively charged metal ions and the electrons around them special bonds Metallic bonds

Section 3: Covalent and Metallic Bonds Movement of Electrons Throughout a Metal Bonding in metals is a result of the metal atoms being so close to another that their outermost energy levels _____________ Metals surrounded in a “sea” of _____________ overlap electrons

Section 3: Covalent and Metallic Bonds Properties of Metals Conducting Electric Current Valence electrons that are __________ Reshaping Metals Electrons free to move around…makes it easy to shape ____________ ________________ Bending without breaking Electrons can ________ in response to pressure so they can bend without breaking moving Ductility Malleability move

Full sentences for full credit! Writing Prompt #3 (of 3) Write the answer. How do metallic bonds explain ductility and malleability in metals? Full sentences for full credit!