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Ions and Ionic Compounds

Ions and Ionic Compounds. Simple Ions . Chemical Reactivity – How much an element reacts depends on the electron configuration of its atoms. Ex: O and Ne Noble gases are least reactive. Alkali metals and halogens are most reactive. WHY?. Valence Electrons.

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Ions and Ionic Compounds

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  1. Ions and Ionic Compounds

  2. Simple Ions • Chemical Reactivity – How much an element reacts depends on the electron configuration of its atoms. • Ex: O and Ne • Noble gases are least reactive. • Alkali metals and halogens are most reactive. WHY?

  3. Valence Electrons • Group number tells you how many electrons are in an element’s valence shell. • Atoms gain and lose electrons to become stable.

  4. Characteristics of Stable Ions • An atom and its ion have different chemical properties. • Stable ion should not be confused with noble gas • Has a charge now and forms a compound.

  5. Atoms and Ions • Atoms of metals & nonmetal elements form Ions differently. • Almost all metals form cations • Ex: Mg – 1s2 2s2 2p6 3s2 • Takes less energy to lose 2 electrons, than gain 6. • Nonmetals form anions • Ex: O – 1s2 2s2 2p4 • Gaining 2 electrons requires less energy than losing 6.

  6. Ionic Bonding & Salts • Form between ions of opposite charges (+ & -). • Compound becomes electrically neutral. • Ex: NaCl

  7. Ionic Bonding & Salts • Ionization energy – energy needed to remove the outermost electron from an atom. • Endothermic – Needs energy to be put in the reaction in order for the reaction to occur. • Exothermic – Reaction releases energy (often heat).

  8. Ionic Bonds • Strong • Have high melting/boiling points • Rarely gas at room temp. • When dissolved conduct electric current. • Salts are hard and brittle.

  9. Names and Formulas: • Simple Ions: • Cation borrows name of element: K is potassium ion. • When element forms 2+ ions, roman numerals are used: • Ex: Cu+ : copper (I) ion • Cu 2+ : copper (II) ion • Anion also uses element name but, add ideto end. • Ex: chloride, oxide

  10. Naming a compound • Cation name followed by anion • Ex: NaCl sodium chloride • Ex: Mg3N2 magnesium nitride • Ex: K2 potassium oxide

  11. Writing ionic formulas • Must have no overall charge (neutral). • Ex: Mg 2+ and N3-

  12. Naming Polyatomic Ions • Presence of Oxygen – iteand -ate. The one with less O is ite, while the one with more O is ate. • Ex: SO32- is sulfite SO42- is sufate

  13. Naming of Polyatomic Ions • Presence of hydrogen indicated by using hydrogen. • Prefixes are used to indicate how many hydrogen • Ex: H2PO42- : dihydrogen phosphate. • MUST KNOW: CO32- , OH- , NO3- , NO2- , phosphate, sulfate, sulfite.

  14. Naming Compounds w/ Polyatomic Ions • K2CO3 • Name cation: name of the element. • Name anion: what is the charge? • Write it out • Potassium carbonate

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