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Ionic Compounds

Ionic Compounds. Ion formation. Octet rule- atoms want a full valence shell _____ valence electrons for most atoms ____ and atoms that become isoelectronic with __ are satisfied with ____ valence electrons H can be satisfied with ___ or ___ _____________

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Ionic Compounds

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  1. Ionic Compounds

  2. Ion formation • Octet rule- atoms want a full valence shell • _____ valence electrons for most atoms • ____ and atoms that become isoelectronic with __ are satisfied with ____ valence electrons • H can be satisfied with ___ or ___ • _____________ • Low electronegativities and ionization energies • Electrons are __________ until octet rule is satisfied (more complicated in the transition metals) • ______________ • High electronegativities and ionization energies • Electrons are ________ until octet rule is satisfied

  3. 1 2 3 4 5 6 7 8 Valence electrons

  4. Ions • An atom with a _____________ • Imbalance of _________ and _________ • _____ or ______ electrons • Two Types • Cation- __ charge because electrons are __ • Cation with a common charge • Multivalent cation • Polyatomic cation • Anion- _ charge because electrons are ____ • Anion with a common charge • Polyatomic anion

  5. Cations with a Common Charge Atoms that predictably form a cation with a certain charge Group 1 elements- form cations with __ charge Group 2 elements- form cations with ___ charge Al- forms cations with a ___ charge Some of the other metals will also only form one common ion

  6. Multivalent Cations Atoms that form multiple types of cations All other metals not on the common cation list

  7. Polyatomic Cations Cation made up of multiple atoms bonded together You only memorized one + NH4+

  8. Naming Cations • Cations with a common charge • “Element name” ion • For example • Na+ is _____________ • Ca+2 is _____________ • Multivalent cations • “Element name” (Roman numeral for charge) ion • For example • Fe+2 is _____________ • Fe+3 is _____________ • Polyatomic cations • “Polyatomic name” ion • NH4+ is _______________

  9. Anions with a Common Charge Atoms that predictably form a anion with a certain charge Group 17 non-metals- form anions with __ charge Group 16 non-metals- form anions with __ charge Group 15 non-metals- forms anions with a ___ charge Sometime Group 14 non-metals form anions with a ____ charge

  10. Polyatomic Anions 2- • Anion made up of multiple atoms bonded together • You memorized 10, but by learning a set of rules you know more than 10. • For polyatomics with oxygen ending with –ate • Add one more oxygen, name is _________ • Take away one oxygen, name is ________ • Take away two oxygens, name is ________ CO32-

  11. Polyatomic Anions (cont) • For example: • You memorized ClO3- is chlorate • This ion has one chlorine and three oxygen atoms with a negative one charge • ClO4- is _____________ • This ion has one chlorine and four oxygen atoms (one more than the –ate ion) with a negative one charge • ClO2- is ____________ • This ion has one chlorine and two oxygen atoms (one less than the –ate ion) with a negative one charge • ClO- is _____________ • This ion has one chlorine and one oxygen atom (two less than the –ate ion) with a negative one charge

  12. Naming Anions • Anions with a common charge • “Element name with ending changed to -ide” ion • For example • Cl- is ____________ • O-2 is ____________ • Polyatomic anions • “Polyatomic name” ion • For example • CO3-2 is ___________ • NO3- is ___________ • NO2- is ___________

  13. Ionic bonding • Ions of opposite charges are attracted to each other • This attraction is a chemical bond

  14. F Room for extra valence electron Fluorine atom (9 electrons)

  15. Na Lonely valence electron Sodium atom (11 electrons)

  16. Electron is transferred Na F

  17. Charges +1 -1 Na F Lost an electron Gained an electron

  18. Atoms are attracted to each other +1 -1 Na F And each have 8 valence electrons

  19. Bonds Chemical bonds are _______________ They act between atoms within a molecule

  20. Why does bonding occur? • Bonding occurs to maximize stability of the atoms involved. • More stable = LOWER potential energy

  21. Ionic Compounds • Will often form a crystal structure • Can be identified by name or formula • If given one, you can find the other • Formulas give the smallest whole number ratio between the ions

  22. Naming Ionic Compounds • Determine the name of the cation and anion involved in the ionic bond • Name both (cation before anion) leaving off the “ion” • For example • An ionic compound between a magnesium ion and a fluoride ion would be ________________ • An ionic compound between a copper (I) ion and a phosphate ion would be _________________

  23. Formulas • Elements in the compound are listed with the number of atoms of each type listed as subscripts • For example, NaCl • Has a 1:1 ratio of sodium ions to chloride ions • CaI2 • Has a 1:2 ratio of calcium ions to iodide ions

  24. Formulas (cont.) • Formulas with polyatomic ions can have parenthesis with a subscript on the outside • The subscript on the outside denotes how many polyatomic ions are there • For example, Al(NO3)3 • Has a 1:3 ratio of aluminum ions to nitrate ions

  25. Switching Between Names and Formulas • Name to Formula • Identify the symbol and charge of the anion and the cation • Determine how many of cations and anions are needed to balance the charges to neutral • Write the formula (cation first) with subscripts denoting how many are needed of each ion • Remember to put polyatomic ions in parenthesis if adding a subscript to them

  26. Switching Between Names and Formulas Name to Formula example • What is the formula for calcium bromide?

  27. Switching Between Names and Formulas Name to Formula example • What is the formula for iron (II) chloride?

  28. Switching Between Names and Formulas Name to Formula example • What is the formula for potassium hydroxide?

  29. Switching Between Names and Formulas • Name to Formula example • What is the formula for gold (II) phosphate?

  30. Switching Between Names and Formulas • Name to Formula example • What is the formula for ammonium bromide?

  31. Switching Between Names and Formulas • Formula to name • Identify the name of the cation and anion in the formula • Remember multivalent cations need a Roman numeral as part of their name. You will have to determine the charge from the formula clues. • Name the compound

  32. Switching Between Names and Formulas • Formula to name examples • LiBr • NiO

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