Section 7-2. Properties of Ionic Compounds And Metallic Bonding and it s Properties
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1 Properties of Ionic Compounds And Metallic Bonding and it s Properties
2 Properties of Ionic Compounds Positive and negative ions exist in a ratio determined by the number of electrons transferred from the metal atom to the nonmetal atom. The repeating pattern of particle packing in an ionic compound is called an ionic crystal. Also called crystal lattice. (crystalline solid)
3 Properties of Ionic Compounds (cont.) The strong attractions among the positive and negative ions result in the formation of the crystal lattice. A crystal lattice is the three-dimensional geometric arrangement of particles, and is responsible for the structure of many minerals. Ionic Compounds are also categorized as salts.
4 Properties of Ionic Compounds (cont.) Melting point, boiling point, and hardness depend on the strength of the attraction. Melting & Boiling points are high compared to molecular compounds
5 Properties of Ionic Compounds (cont.) In a solid, ions are locked into position and electrons cannot flow freely solid ions are poor conductors of electricity. Ionic compounds are soluble in water. Solid ionic compounds, when dissolved in water, can conduct electricity. Liquid (Molten) ions or ions in aqueous solution have electrons that are free to move, so they conduct electricity easily. An ion in aqueous solution that conducts electricity is an electrolyte.
6 Properties of Ionic Compounds (cont.) This figure demonstrates how and why crystals break when an external force is applied. Ionic Compounds: shatter (nonmalleable) Are hard/brittle (hardness)
7 Energy and the Ionic Bond Reactions that absorb energy are endothermic. Reactions that release energy are exothermic.
8 Energy and the Ionic Bond (cont.) The energy required to separate 1 mol of ions in an ionic compound is referred to as the lattice energy. Lattice energy is directly related to the size of the ions that are bonded.
9 Energy and the Ionic Bond (cont.) Smaller ions form compounds with more closely spaced ionic charges, and require more energy to separate. Electrostatic force of attraction is inversely related to the distance between the opposite charges. The smaller the ion, the greater the attraction.
10 Energy and the Ionic Bond (cont.) The value of lattice energy is also affected by the charge of the ion.
11
12 Section 7.4 Metallic Bonds and the Properties of Metals Objectives: Describe a metallic bond. Relate the electron sea model to the physical properties of metals. Define alloys, and categorize them into two basic types.
13 Section 7-4 Metallic Bonds and the Properties of Metals Metals: Metals are not ionic but share several properties with ionic compounds. Metals also form lattices in the solid state, where 8 to 12 other atoms closely surround each metal atom.
14 Section 7-4 Metallic Bonds and the Properties of Metals (cont.) Within the crowded lattice, the outer energy levels of metal atoms overlap. The electron sea model proposes that all metal atoms in a metallic solid contribute their valence electrons to form a "sea" of electrons. The electrons are free to move around and are referred to as delocalized electrons, forming a metallic cation.
15 Section 7-4 Metallic Bonds and the Properties of Metals (cont.) A metallic bond is the attraction of an metallic cation for delocalized electrons.
16 Section 7-4 Metallic Bonds and the Properties of Metals (cont.) Boiling points are much more extreme than melting points because of the energy required to separate atoms from the groups of cations and electrons.
17 Section 7-4 Metallic Bonds and the Properties of Metals (cont.) Metals are malleable because they can be hammered into sheets. Metals are ductile because they can be drawn into wires.
18 Section 7-4 Metallic Bonds and the Properties of Metals (cont.) Mobile electrons around cations make metals good conductors of electricity and heat. As the number of delocalized electrons increases, so does hardness and strength. Metallic compounds are insoluble in water. Metallic bonding is found in pure metals.
19 Section 7-4 Metal Alloys An alloy is a mixture of elements that has metallic properties. The properties of alloys differ from the elements they contain.
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