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Chapter 8

Chapter 8. Ionic Compounds. THINGS YOU MUST KNOW!!!!!!!. Pg 222 Common Ions Must be written correctly Fe 2+ Fe 3+ (correct) 2+, FE 3+ , Fe3+, Fe 3+ (Incorrect) Pg 224 Polyatomic Ions Groups of covalently bonded atoms that have an overall charge and act like an ion. SO 4 2- Sulfate

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Chapter 8

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  1. Chapter 8 Ionic Compounds

  2. THINGS YOU MUST KNOW!!!!!!! • Pg 222 • Common Ions • Must be written correctly • Fe2+ Fe3+ (correct) • 2+, FE3+,Fe3+, Fe3+ (Incorrect) • Pg 224 Polyatomic Ions • Groups of covalently bonded atoms that have an overall charge and act like an ion. • SO42- Sulfate • What is C2H3O2-? • Acetate • What is NaC2H3O2? • Sodium acetate • On your quizzes you will be given the name. You must give the ion or formula.

  3. Ionic Bonds • Ion • Charged atom • Cations • Metals • Metals lose electrons and become positive • Anions • Nonmetals • Nonmetals gain electrons and become negative

  4. Why does bonding occur? • Every atom wants to be stable • Pseudonoble gas configuration • Pseudo means false • An atom that is not a noble gas but has the electron configuration of a noble gas. • This is achieved through bonding and makes the atoms involved stable.

  5. Rule: The sum of the charges for ionic compounds must equal 0. • Always written metal nonmetal • Examples: • Mg and Cl • You do: Rb and O • Do not swap charges to make subscripts.

  6. Ionic compounds form crystal lattices • 3-D repeating pattern of ions • Ions are bonded by lattice energy • Energy required to separate ions • Expressed as a negative value • The more negative the number the more energy required to separate the ions

  7. Characteristics of ionic compounds • High melting and boiling points • Hard • Strong bond • Nonconductors in solid state • Conductors in liquid state • Electrolytes • Ions in aqueous solution that conduct electricity • When ionic compounds come apart in a solution it is called dissociation

  8. Why do atoms gain and lose electrons? • Do ionic compounds form molecules? • No, because they form a crystal lattice. • Repeating pattern of ions based upon 3-D orientation of the way ions pack around one another. • The simplest ration of ions is called the formula unit. • Also why ionic compounds in a solid state are brittle, nonconductors, and hard. • Lattice energy is affected by 2 things • Size – The smaller the ion the greater the energy • Charge – The greater the charge the greater the energy

  9. Metallic bonds are similar to ionic bonds but they are not ionic bonds. • Metallic bonding is the reason metals have their properties. • Ductile, malleable, conduct electricity. • The outer shell of electrons are delocalized. • Not associated with one nucleus • Electron sea model • Used to illustrate metallic bonding

  10. Metals can form alloys • Mixture of metals • 2 types • Interstitial alloys • Smaller atom fills the interstasis • Substitutional alloys • Occurs when atoms are the same size

  11. Writing Ionic Compounds • Sum of charges must equal 0 • Metal Nonmetal • Ex. Strontium and Bromine • Sr2+ and Br- SrBr2 • Potassium and Oxygen • K+ and O2- K2O • You do: Aluminum and sulfur • You do: Calcium and arsenate

  12. Things You Must Know • 2NaCl • What does the 2 mean? • SrBr2 • What does the 2 mean?

  13. Naming Ionic Compounds • Metal and monatomic anion • Name of the metal and root of the anion with –ide ending. • Ex. Rb2S • Rubidium Sulfide • Metal w/ multiple charges and monatomic anion • Name of the metal with a roman numeral representing charge and root of the anion with –ide ending. • Ex. Copper and Bromine • Could be Cu+Br- or Cu2+Br- • Cu+Br- would be named copper (I) bromide • Cu2+Br- would be named copper (II) bromide

  14. Metal and polyatomic anion • Metal polyatomic anion • Ex. NaC2H3O2 • Sodium acetate • Metal w/ multiple charges and a polyatomic • Metal w/ charge and polyatomic • Ex. AuNO3 • Gold (I) nitrate • Fe(ClO)3 • Iron (III) hypochlorite

  15. Multiple Polyatomic Groups: Oxyanions • All contain oxygen • Two possibilities • -ate or –ite • -ate is used to show the polyatomic that contains the greater number of oxygen atoms • -ite is used to show the polyatomic that contains the leaser number of oxygen atoms. • Ex. NO3- is nitrate; NO2- is nitrite • Ex. SO42- is sulfate; SO32- is sulfite

  16. There are four possibilities with halogens that form a polyatomic anion. • Per- -ate -ate -ite Hypo- -ite • Ex. ClO4- is perchlorate ClO3- is chlorate ClO2- is chlorite ClO- is hypochlorite • You name: NaBrO

  17. Writing Formulas from Names • Aluminum selenide • Al3+ and Se2- Al2Se3 • Tin (IV) oxide • Sn4+ and O2-  SnO2 • Lead (II) hydrogen carbonate • Pb2+ and HCO3-  Pb(HCO3)2

  18. Homework • Pg. 237 74-84

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