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Understanding Ionic Bonds: Formation, Properties, and Lattice Energy

This guide explores ionic bonds, which form through the transfer of electrons, resulting in positive and negative ions that attract to create ionic compounds like oxides and salts. We focus on the properties of ionic compounds, including their crystalline structure, high melting and boiling points, and electrical conductivity in liquid form. The concept of lattice energy is examined, emphasizing how ion size and charge affect bond strength. Quick checks encourage applying knowledge to predict compound behavior and energy characteristics.

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Understanding Ionic Bonds: Formation, Properties, and Lattice Energy

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  1. Forming Ionic Bonds • Electron transfer: one atom loses electrons - another atom gains those electrons • Positive and negative ions attract = ionic compound. • Metal + oxygen = OXIDE • Metal + nonmetals = SALT

  2. Ionic Bonds • Often binary (2 elements) • e- lost = e- gained (always) • Quick check: • How will sodium & chlorine combine? • How about calcium & sulfur? • How about lithium & phosphorus? • How about iron (III) & oxygen? Hint: use e- configurations or electron dot diagrams Then show box and table method to solve

  3. Quick Check • How will sodium & chlorine combine? calcium & sulfur? lithium & phosphorus? iron (III) & oxygen?

  4. Properties of Ionic Compounds • Crystals (not molecules) = many cations and anions packed into a repeating pattern (crystal lattice). • Chemical formula = ratio of atoms needed • Fairly strong bond = large amount of energy to break. • High melting & boiling points • Often rigid & hard

  5. More Properties • If a liquid or solution, good conductors of electricity (electrolytes) • If a solid, bad conductors because ions aren’t free to move • EXOTHERMIC (almost always) – means the ionic compound is more stable & requires less energy, so heat is given off when forming Ex: hand warmers = iron + oxygen combining

  6. Lattice Energy • Energy to break apart 1 mole of ions • Equals energy released when ions form • More negative number = stronger bonds • Smaller ions = greater lattice energy (nucleus is closer to the valence e-) • Greater ionic charge = greater lattice NRG

  7. Quick Check • Which would have the greater lattice energy? • LiCl or LiBr • KF or RbF • NaCl or MgF2 • SrCl2 or MgO • Which compound in each pair would have the higher melting point?

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