1. IONIC BONDS Ch 6.1

2. TrueFalseStatementTrueFalse When an atom gains electrons it gets an (+) charge. When it loses electrons it gets a (-) charge Ionic bonds are between a metal and nonmetal Anions are (-) and cations are (+) Ionization energy is how much energy is needed to add an electron Crystal lattice is a shape ionic compounds make

3. Electron Configuration  Stable-  Highest occupied energy level is filled with _______  Atom not likely to react  Electron Dot Diagram-  Lewis Dot  Shows Valance Electrons

4. Ionic Bonds  Transfer of electrons to become more stable Na + Cl Na + Cl -  Ion- atom with a positive or negative electric charge  Losing electrons  + sign, Cation  Gaining electrons  - sign, Anion Transfer of ElectronsFormation of Ions

5. Ionic Bonds Continued  Chemical Bond- force that holds atoms or ions together  Ionic Bond- force that holds cations and anions together  - the amount of energy used to remove an electron  Lower I-energy = easier to remove Formation of Ionic BondsIonization Energy

6. Ionic Compounds  Compounds that contain ionic bonds  Usually a metal bonded to a nonmetal  Chemical Formulas- notation that shows what elements a compound contains and the ratio of atoms or ions of those elements

7. Crystal Lattice  Attraction between elements, that keeps the ions in fixed positions  Rigid, framework= lattice  Solids with lattice structures are called crystals

8. Ionic Properties  Strong attractions between ions within a crystal lattice  When melted, great conductors of electricity  Shatter when struck= _______

9. COVALENT BONDS Ch. 6.2

10. TrueFalseStatementTrueFalse Covalent bonds are between 2 nonmetals, that share valence electrons Bonds can be single, up to quadruple Polar covalent bonds, are not shared equally Nonpolar bonds are stronger than polar bonds Polar bonds include, (-) and (+) signs to show polarity

11. Covalent Bonds  Chemical bond where 2 atoms share a pair of valence electrons  Molecule- neutral group of atoms, joined by covalent bonds  Attraction between shared electrons and protons hold atoms together Sharing ElectronsMolecules of Elements

12. Covalent Bonds  Multiple Bonds  Single Bonds H-H  Double Bonds C=C  Triple Bonds N N  Usually a nonmetal bonded with a nonmetal

13. Unequal Sharing  Polar Covalent Bonds  Electrons are not shared equally  Atom with greater attraction for electrons has partial – charge  Atom with less attraction has partial + charge  Nonpolar Covalent Bonds  Equal sharing

14. Attraction Between Molecules  Polar bonds are stronger than nonpolar bonds

15. NAMING COMPOUNDS & WRITING FORMULAS Ch. 6.3

16. TrueFalseStatementTrueFalse When naming ionic compounds, anions are written 1 st, followed by cations When naming covalent compounds, you must use a prefix for every element Polyatomic ions are covalently bonded atoms with a (-) or (+) charge Oxidation #s tell the charge the ion would have if it gained or lost electrons -ide ending is added to the 1 st elements name in the compound

17. Naming Ionic Compounds  Metal to nonmetal  1 st - Cation  Metal without change  Sodium  2 nd - Anion  Nonmetal with suffix – ide  Chlorine = chloride  3 rd - Combine  Sodium chloride  Examples:  LiF  KO  CuS  BeCl

18. Formulas for Ionic Compounds Calcium chloride  1 st - Write Symbols  Ca Cl  2 nd - Locate  Ca Cl Cationanion  3 rd - Find oxidation #  Ca +2 Cl -1  Lose 2 electrons  Gain 1 electron  4 th - Criss cross, then write as subscript  CaCl 2

19. Transition Metals  Get oxidation # from anion  Must be neutral  Backward crisscross  Iron(II) oxide  Fe ? O -2  Fe +2 O -2  FeO

20. Naming Examples  CoBr 2  Cobalt(II) bromide  CrCl 3  Chromium(III) chloride  MnO 2  Manganese(IV) oxide  AgO  Silver(II) oxide

21. Formula Examples  Iron(II) oxide  FeO  Iron(III) oxide  Fe 2 O 3  Gold(II) oxide  AuO  Platinum(III) oxide  Pt 2 O 3

22. Polyatomic Ions  Covalently bonded group of atoms with either a positive or negative charge  Most common list pg 173

23. Math Practice pg 174  1.  2.  3.  4.

24. Naming Molecular Compounds  2 Nonmetals  1 st - Count how many of each element  Use prefixes  Di-, pent-  2 nd - Add element name and ending  Dinitrogen pentoxide

25. Naming Examples  CO  Carbon monoxide  CO 2  Carbon dioxide  N 2 O 4  Dinitrogen tetraoxide  N 2 O  Dinitrogen monoxide

26. Formula Examples  Dicarbon tetraoxide  C 2 O 4  Tetraboron dichloride  B 4 Cl 2  Arsenic hexoxide  AsO 6  Silicon pentsulfide  SiS 5

27. STRUCTURE OF METALS Ch. 6.4

28. TrueFalseStatementTrueFalse Metallic bonds are between a metal and a transition metal Metal bonds have a crystal lattice structure Alloys are mixtures, in which 1 is a metal Alloys are homogenous mixtures Alloys can be designed with specific properties for different tasks

29. Metallic Bonds  Attraction between a metal cation and the shared electrons surrounding it  2 metals, with no nonmetal to accept electrons  Cations form a lattice=strong bonds between cations and valence electrons  Neutral charge

30. Properties of Metal  Mobility of electrons  Conduct electric current  Shared electons  Malleable & Ductile  Flexible lattice

31. Alloys  Mixture  2 or more elements  1 is a metal  heterogenous  Characteristics of metals

32. Alloys  Bronze  Tin  Brass  Harder, stronger than each metal alone  Iron  Carbon  Chromium  Different mixtures for different needs CopperSteel