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Ionic Bonds

Ionic Bonds. Ch 6.1. Electron Configuration. Stable- Highest occupied energy level is filled with _______ Atom not likely to react Electron Dot Diagram- Lewis Dot Shows Valance Electrons. Ionic Bonds. Transfer of Electrons. Formation of Ions. Transfer of electrons to become more stable

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Ionic Bonds

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  1. Ionic Bonds Ch 6.1

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

  3. Ionic Bonds Transfer of Electrons Formation of Ions • 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

  4. Ionic Bonds Continued Formation of Ionic Bonds Ionization Energy • 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

  5. 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

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

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

  8. Covalent Bonds Ch. 6.2

  9. Covalent Bonds Sharing Electrons Molecules of Elements • 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

  10. Covalent Bonds • Multiple Bonds • Single Bonds H-H • Double Bonds C=C • Triple Bonds N N • Usually a nonmetal bonded with a nonmetal

  11. 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

  12. Attraction Between Molecules • Polar bonds are stronger than nonpolar bonds

  13. Naming compounds & Writing formulas Ch. 6.3

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

  15. Formulas for Ionic Compounds Calcium chloride • 1st- Write Symbols • Ca Cl • 2nd- Locate • Ca Cl Cation anion • 3rd- Find oxidation # • Ca+2 Cl-1 • Lose 2 electrons • Gain 1 electron • 4th- Criss cross, then write as subscript • CaCl2

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

  17. Naming Examples • CoBr2 • Cobalt(II) bromide • CrCl3 • Chromium(III) chloride • MnO2 • Manganese(IV) oxide • AgO • Silver(II) oxide

  18. Formula Examples • Iron(II) oxide • FeO • Iron(III) oxide • Fe2O3 • Gold(II) oxide • AuO • Platinum(III) oxide • Pt2O3

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

  20. Math Practice pg 174 • 1. • 2. • 3. • 4.

  21. Naming Molecular Compounds • 2 Nonmetals • 1st- Count how many of each element • Use prefixes • Di-, pent- • 2nd- Add element name and ending • Dinitrogenpentoxide

  22. Naming Examples • CO • Carbon monoxide • CO2 • Carbon dioxide • N2O4 • Dinitrogentetraoxide • N2O • Dinitrogen monoxide

  23. Formula Examples • Dicarbontetraoxide • C2O4 • Tetraboron dichloride • B4Cl2 • Arsenic hexoxide • AsO6 • Silicon pentsulfide • SiS5

  24. Structure of Metal s Ch. 6.4

  25. 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

  26. Properties of Metal • Mobility of electrons • Conduct electric current • Shared electons • Malleable & Ductile • Flexible lattice

  27. Alloys • Mixture • 2 or more elements • 1 is a metal • heterogenous • Characteristics of metals

  28. Alloys Copper Steel • Bronze • Tin • Brass • Harder, stronger than each metal alone • Iron • Carbon • Chromium • Different mixtures for different needs

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