Chapter 8 Ionic Compounds
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1 Chapter 8 Ionic Compounds I. Forming Chemical Bonds How do Compounds Form? Stability Compounds want to have a noble gas configuration (8 valence electrons)
2 I. Why do atoms form bonds? Chemical Bond - strong attractive force between atoms or ions in a compound. stability - goal is to reach the most energetically favorable condition bond energy - energy involved in process of bond forming or bond breaking Valence Electrons outermost electrons
3 Highest Energy Level Valence Electrons? 3s 2 3p 6
4 How do you represent Valence Electrons? Electron Dot Structures 1. What is the atomic number of this element? 2. Write the electron configuration. 3. Identify just the valence electrons (hint use the A roman numerals on the periodic table).
5 How do you represent Valence Electrons? Electron Dot Structures 4. Write the symbol for the element. 5. Use a dot for each valence electron. An element with a complete valence shell (8 e-) will look like this: Try these examples: Li B N F Be C O Ne X
6 Valence electron 1. shows valence electrons, for example lets try these Li B N F Be C O Ne
7 Stable Octet (new words, octet rule): 8 electrons in valence shell, stable configuration
8 II. Ionic Bonding: process by which one or more electrons are transferred from the valence shell of one atom to the valence shell of another atom. (usually forms salts)
9 Unstable 3s 1 3p 5 3s 2 Electons Transferred = ionic bond Stable 11P + 10e - 1+charge Electrostatic attraction full octets 17P + 18e - 1- charge
10 Ionic Bonding
11 8.3. Names and Formulas for Ionic Compounds (8.3 pgs ) A. Formulas tell: 1. which elements make up the compound (qualitative) 2. ratios of atoms contained (quantitative) Hydrogen & Oxygen in element H 2 O # of H s and O s in molecule
12 B. Made from a metal + a nonmetal 1. metals form (+) ions - cations 2. nonmetals form (-) ions - anions
13 C. Using ion charge to write formulas 1. write the chemical symbol 2. using the periodic table assign a charge (to be written as a subscript) Group IA, IIA, IIIA, VA, VI, VIIA
14 3. add charges together to equal zero, use charge of one ion as subscript for the other ion, or use criss-cross method 4. when subscripts are equal they reduce to 1 5. for polyatomics (more than one atom combined that has an overall charge), use parenthesis when subscript is 2 or more
15 examples: Calcium chloride Ca 2+ + Cl 1- + Cl 1- = 0 CaCl 2
16 examples: Calcium chloride Magnesium phosphate CaCl 2 Aluminum oxide Barium sulfate Al 2 O 3 Magnesium sulfide Ammonium chloride MgS
17 examples: Magnesium phosphate Mg 2+ PO Mg 3 (PO 4 ) 2
18 examples: Barium sulfate Ammonium chloride BaSO 4 NH 4 Cl
19 D. Naming ionic compounds 1. binary compounds - two different kinds of atoms a. name the first element b. name the second element,drop the last syllable, add -ide.
20 examples: Na 2 S = Sodium Sulfide MgO = Magnesium Oxide
21 Naming ternary compounds 2. ternary compounds - name the first element, then name the polyatomic ion
22 examples: Ca(NO 3 ) 2 = Calcium Nitrate Na 2 SO 4 = Sodium Sulfate
23 E. atoms that form more than one type of ion (examples: Cu, Fe, Hg, Pb, Sn) 1. old system - call the ion with the greater charge -ic, and the ion with the lesser change -ous. (use Latin names as roots)
24 Cu +1 cuprous CuF cuprous fluoride Cu +2 cupric CuF 2 cupric fluoride Fe +2 ferrous FeF 2 ferrous fluoride Fe +3 ferric FeF 3 ferric fluoride
25 2. new system (or stock system), name ion by atom. The name is followed by roman numeral telling its charge.
26 Cu +1 copper(i) Cu +2 copper(ii) ` CuF copper (I) fluoride CuF 2 copper (II) fluoride Fe +2 Iron(II) FeF 2 iron (II) fluoride Fe +3 Iron(III) FeF 3 iron (III) fluoride
27 III. Properties of Ionic Compounds: Crystal Lattice- three dimensional arrangement of cations & anions List Properties here Crystal shape Hard & brittle High melting pt High boiling pt When dissolved, or molten, conducts electricity
28 Properties of Ionic Solids
29 Electrons transferred = ionic bond Electrostatic Attraction
30 Crystal shape Unit cell simplest, repeating unit
31 IV. Energy and the Ionic Bond: During any chemical or physical reaction energy is neither created or destroyed Energy that is absorbed is called endothermic Energy that is release is called exothermic The formation of ionic compounds from positive and negative ions is always exothermic. The compound formed is more stable and of lower energy.
32 IV. Energy and the Ionic Bond: The energy required to separate one mole of the ions of an ionic compound is referred to as the lattice energy. The more negative the lattice energy, the stronger the force of attraction. Which would have more negative lattice energy, lithium chloride or lithium bromide? Lithium chloride MgO is almost four times greater then the lattice energy of NaF, why? MgO, charge of the ions is greater
33 V. Names and Formulas for Ionic Compounds(8.3 pgs )(see previous notes)! Describe a Pot of Gold (physical and chemical properties of the pot and the gold coins) High luster High Melting/Boiling Pt. Malleable Ductile Solid Conductive
34 VI. Metallic Bonds and Properties of Metals (8.4 pgs ) 1. Metals form a lattice with eight to 12 other metal atoms surrounding each metal atom. 2. metals have at least one valence electron, they do not form ions or share their electrons 3. metals are crowded with electrons and the outer energy levels of the metal atoms overlap
35 VI. Metallic Bonds and Properties of Metals (8.4 pgs ) 4. The electron sea model proposed that all the metal atoms in a metallic solid contribute their valence electrons dot form a sea of electrons.
36 5. Electrons are not held tightly by any specific atom, electron are free to move around and are referred to delocalized electrons.
37 6. The attraction of a metallic cation for delocalized electrons is called a metallic bond.
38 Properties of Metallic Bonding
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