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Ionic Bonds

Ionic Bonds. What are those pesky compounds. What is a chemical bond?. A chemical bond is a mutual attraction between different atoms. Why do atoms chemically bond?. Atoms and ions are less stable existing by themselves. An atom’s potential energy is decreased by combining with another atom.

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Ionic Bonds

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  1. Ionic Bonds What are those pesky compounds

  2. What is a chemical bond? • A chemical bond is a mutual attraction between different atoms.

  3. Why do atoms chemically bond? • Atoms and ions are less stable existing by themselves. • An atom’s potential energy is decreased by combining with another atom. • When atoms bond their electrons rearrange promoting stability. • The Octet Rule. • “I want to be like a Noble Gas.”

  4. What is ionic bonding? • A bond resulting from electrostatic attraction of a cation and an anion. • Ions give up electrons to other atoms. • Unlike charges attract.

  5. Ionic Compounds – What do they look like? • Ionic compounds are composed of positively and negatively charged ions and are held together by electrostatic attractions. Ionic compounds do not contain molecules. Instead, because opposite charges attract one another, the ions stack themselves in crystals such that positive ions are surrounded by negative ions, and vice versa.

  6. What is an ionic compound? • A substance composed of positive and negative ions. • Most ionic compounds exist as crystalline solids.

  7. Naming Ionic Compounds • Binary Compounds • Charges must be equal. • Combine cation name with anion name. • The cation comes first followed by the anion.

  8. Naming Ionic Compounds • To name ionic compounds, name the cation then the anion. Monatomic cations have the same name as the element from which they form. For example, Ca+2 is calcium ion. The names of the simple monatomic anions are similar to the names of their element but end in an –ide suffix. S-2 is sulphide ion. The name of the ionic compound containing Ca2+ and S-2 is calcium (II) sulfide. See the periodic table section for common charges of monatomic ions.

  9. Naming Ionic Compounds Steps to write formulas of ionic compounds 1. write formulas of ions, positive one first. 2. use subscripts to increase the number of ions in the compound until the charges are equal but opposite (multiplication!!! and least common multiple) - to show more than one polyatomic ion, put parentheses around it and then use a subscript to balance charge 3. the final formula: rewrite so no charges are showing. 4. Check to see if empirical formula (lowest ratio of ions) Steps to naming an ionic compound from its formula 1. State the names of the ions involved, putting the cation (positive) name first 2. If the cation has more than one possible charge, name it properly (stock or traditional) by determining its charge using the anion Remember! -name tells what ions are involved but NOT how many -total negative = total positive, so compound is neutral -use least common multiple to help find charge and/or number of ions

  10. Practice naming • potassium chloride • Iron (II) sulfide • calcium cyanide • ammonium acetate • aluminum phosphate

  11. Practice naming • potassium chloride KCl • Iron (II) sulfide FeS • calcium cyanide Ca(CN)2 • ammonium acetate (NH₄)(CH₃COO) • aluminum phosphate AlPO₄

  12. Practice naming MgI2 K2O FeO Fe2O3 Cu3(PO4) 2 CuCN Co2(CO3)3 PbO2

  13. Practice naming MgI2 Magnesium Iodide K2O Potassium Oxide FeO Iron(II) Oxide or Ferrous Oxide Fe2O3 Iron(III) Oxide or Ferric Oxide Cu3(PO4)2 Copper(II) Phosphate or Cuprous Phosphate CuCN Copper(I) Cyanide or Cuprous Cyanide Co2(CO3)3 Cobalt(III) Carbonate PbO2 Lead(IV) Oxide or Plumbic Oxide

  14. Time for some real chemistry

  15. Ions to Memorize Names and formulas w/ charge of metals from s & p blocks: lithium Li+ sodium Na + potassium K + rubidium Rb + cesium Cs + francium Fr + beryllium Be2+ magnesium Mg2+ calcium Ca2+ strontium Sr2+ barium Ba2+ radium Ra2+ boron B3+ aluminum Al3+ gallium Ga3+ indium In3+ thallium Tl3+ germanium Ge4+ tin (II) / stannous Sn2+ tin (IV) / stannic Sn4+ lead (II) / plumbous Pb2+ lead (IV) / plumbic Pb4+ antimony Sb5+ bismuth Bi5+

  16. Elemental ions to memorize Names and formulas w/ charge of non-metals from s & p blocks: Some elements can be positive or negative: hydrogen H+ hydride H- carbon C4+ carbide C4- silicon Si4+ silicide Si4- arsenic As4+ arsenide As4- selenium Se6+ selenide Se2- nitride N3- phosphide P3- oxide O2- sulfide S2- fluoride F- chloride Cl- bromide Br- iodide I- astatide At- Pg 162

  17. Negativepolyatomic Ions to memorize - 2- MnO4 O2 - HCO3 2- CO3 peroxide cyanide CN- hydroxide OH- acetate permanganate perchlorate chlorate chlorite hypochlorite nitrate nitrite iodate hypoiodite carbonate hydrogen carbonate (bicarbonate) sulfate sulfite hydrogen sulfate (bisulfate) hydrogen sulfite (bisulfite) phosphate phosphite hydrogen phosphate chromate dichromate oxalate silicate - HSO4 - NO2 - - HSO3 NO3 - - IO3 IO - - - - ClO2 ClO4 ClO3 ClO 2- 2- 3- 2- 3- 2- 2- 2- 2- - PO3 HPO4 SO4 SO3 CrO4 Cr2O7 C2O4 SiO3 PO4 C2H3O2 Pg 163

  18. Other ions to include Multiple Charges: chromium (II) Cr2+ chromium (III) Cr3+ cobalt (II) Co2+ cobalt (III) Co3+ copper (I)/cuprous Cu+ copper (II)/cupric Cu2+ iron (II)/ferrous Fe2+ iron (III)/ferric Fe3+ mercury (I)/mercurous Hg2 mercury (II)/mercuric Hg2+ Only memorize one charge: silver Ag+ nickel (II) Ni2+ zinc Zn2+ manganese (II) Mn2+ Positive polyatomic ions: ammonium NH4 hydronium + 2+ + H3O Pg 163

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