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Ionic Bonding

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Published in: Chemistry
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This PowerPoint presentation offers a thorough exploration of ionic bonding, one of the fundamental types of chemical bonds. It begins with a basic introduction to the nature of chemical bonds and the importance of understanding how atoms combine to form compounds. The presentation then focuses on ionic bonding, explaining that it occurs when atoms transfer electrons to achieve a stable electron configuration. This process typically happens between metals and nonmetals, where metals lose electrons to become positively charged cations, and nonmetals gain those electrons to become negatively charged anions. The presentation concludes by emphasizing the significance of ionic bonding in chemistry, as it explains the formation of many essential compounds and helps predict the properties of materials based on their bonding.

Mudasir A / Jammu

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  1. Ionic Bonding A sodium Na chloride A sodium cation chloride anion
  2. CA Standards Students know atoms combine to form molecules by sharing electrons to form covalent or metallic bonds or by exchanging electrons to form ionic bonds. Students know salt crystals, such as NaCl, are repeating patterns of positive and negative ions held together by electrostatic attraction.
  3. Bonds C] Forces that hold groups of atoms together and make them function as a unit. Ionic bonds - transfer of electrons Covalent bonds - sharing of electrons
  4. The Octet Rule - Ionic Compounds Ionic compounds form so that each atom, by ggining-gc-!esing electrons, has an octet of electrons in its highest occupied energy level. Metals lose electrons to form positively-charged cations Nonmetals gains electrons to form negatively- charged anions
  5. Ionic Bonding: The Formation of Sodium Chloride C] Sodium has 1 valence electron Cl Chlorine has 7 valence electrons Cl An electron transferred gives each an octet Na: 1s22s22p63sl Cl: 1s22s22p63s23p5
  6. Ionic Bonding: The Formation of Sodium Chloride This transfer forms ions, each with an octet: Na+ 1s2 s22 6
  7. Ionic Bonding: The Formation of Sodium Chloride The resulting ions come together due to electrostatic attraction (opposites attract): Na+ Cl- The net charge on the compound must equal zero
  8. Examples of Ionic compounds Mg2+Cl-2 Na+202- A 13+ 52- Magnesium chloride: Magnesium loses two electrons and each chlorine gains one electron Sodium oxide: Each sodium loses one electron and the oxygen gains two electrons Aluminum sulfide: Each aluminum loses two electrons (six total) and each sulfur gains two electrons (six total)
  9. Metal Lithium Sodium Potassium Magnesium Calcium Barium Aluminum Monatomic Cations Li+ Na+ Mg2+ Ca2+ Ba2+ A 13+ Ion name Lithium Sodium Potassium Magnesium Calcium Barium Aluminum
  10. Nonmetal Fluorine Chlorine Bromine Iodine Oxygen Sulfur Nitrogen Phosphorus Monatomic Anions Cl- 1- 02- 52- Ion Name Fluoride Chloride Bromide Iodide Oxide Sulfide Nitride Phosphide
  11. Sodium Chloride Crystal Lattice Ionic compounds form solid crystals at ordinary temperatures. Ionic compounds organize in a characteristic crystal lattice of alternating positive and negative ions. All salts are ionic compounds and form crystals.
  12. Properties of Ionic Compounds Structure : Melting point: Boiling Point: Electrical Conductivity: Solubility in water: Crystalline solids Generally high Generally high Excellent conductors, molten and aqueous Generally soluble