Chapter 8. Ionic Compounds
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1 Chapter 8 Ionic Compounds
2 Chemical Bonds Chemical bonds form so elements can attain a stable electron structure 8 outer electrons is the most stable structure Atoms will gain/lose electrons to reach either 0 or 8
3 Chemical Bonds Pseudo Noble Gas When an ion forms that results in full s & p sub-levels (may be some d or f electrons still hanging on)
4 Cations (Positive Ions) Results from an atom losing electrons to increase their stability Charge is equal to the number of electrons lost Sodium loses 1 electron charge = 1+ All metals
5 Anions (Negative Ions) 1. Formed when elements gain electrons in bonding 2. To name add ide to element name 1. Sulfur = sulfide 3. Charge = number of electrons gained 1. Fluorine gains 1 charge = 1-
6 Assignment 1. Make a list of 10 elements 2. Exchange with a partner and give: 1. Electron configuration 2. Type of ion formed (cation/anion) 3. Electron dot diagram 4. Charge of the ion formed
7 Chapter 8.2 Ionic Compounds
8 Ionic Bond Electrostatic force holds oppositely charged particles together Formed between metals and non-metals
9 Binary Compounds Compounds that contain only two elements Metallic cation and nonmetallic anion Number of electrons lost by the cation must equal the number of electrons gained by the anion
10 Binary Compounds 1. Na 1+ + Cl 1- NaCl 2. Mg 2+ + Cl 1- MgCl 2 3. K 1+ + S 2- K 2 S
11 Properties of Ionic Compounds During the formation of ionic compounds the positive and negative ions are arranged in repeating patterns (crystal lattice) that determine the properties of the compound as a whole
12 Crystal Lattice 3-d geometric arrangement of particles Vary in shape due to the size and number of ions bonded
13 Crystal Lattice Melting and Boiling points and hardness are determined by the crystal lattice Lattice energy is a result of the electrostatic attractions between oppositely charged ions There is an inverse relationship between lattice energy and interionic distance
14 Electrolyte Ionic solution that conducts current Solid ionic compounds will not conduct since ions are not free to move
15 Energy Changes During Bond Formation 1. Exothermic Reaction Energy is released during a reaction 1. Formation of ionic compounds from positive and negative ions is always exothermic 2. Endothermic Reaction Energy is absorbed during a reaction
16 Assignment What is a chemical bond? Why do ions form? What family of elements is relatively unreactive and why? Describe the formation of both positive and negative ions What would be the ionic charge of each of the following: N S Ba Li What is an ionic bond? How does an ionic bond form List 3 physical properties of an ionic bond Describe the arrangement of ions in a crystal lattice What is lattice energy and how is it involved in an ionic bond? Explain the formation of the ionic compound for each of the following pairs: Na & N; Li & O; Sr & F; AL & S
17 Chapter 8.3 Writing Formulas and Naming Ionic Compounds
18 Rules for Writing Formulas for Ionic Compounds 1. Formula represents the simplest ratio of ions in a compound 2. Overall charge of the compound must equal 0 3. Cation is always listed first
19 Oxidation Numbers (determining charge) Monatomic Ions Ions composed of one element 1. Oxidation number is dependent on location on the periodic table 2. If a particular oxidation is not specified use the bold oxidation number
20 Oxidation Numbers (determining charge) Polyatomic Ions Ions composed of more than one element, but acting as a single cation or anion 1. Table 8-6 on page 224 must be copied on your periodic table 2. Charge on table is for the entire ion 3. NEVER change subscripts in a polyatomic ion
21 Write the correct formula for the following pairs of ions Potassium and iodide Magnesium and chloride Aluminum and bromide Cesium and nitride Barium and sulfide Sodium and nitrate Calcium and chlorate Aluminum and carbonate Potassium and chromate Magnesium and carbonate Assignment: How do you determine the correct subscripts in a chemical formula? What subscripts would most likely be used if the following substances formed an ionic compound? An alkali metal and a halogen An alkali metal and a nonmetal from group 16 An alkaline earth metal and a halogen An alkaline earth metal and a nonmetal from group 16 A metal from group 3 and a halogen
22 Naming Ionic Compounds Oxyanions Polyatomic ion with oxygen 1. Ion with most oxygen atoms = root of the nonmetal plus ate 2. Ion with fewer oxygen atoms = root of nonmetal plus -ite
23 Naming Ionic Compounds (Halogens) 1. Most O = per- root ate 1. ClO 4 = perchlorate 2. 1 fewer = root ate 1. ClO 3 = chlorate 3. 2 fewer = root ite 1. ClO 2 = chlorite 4. 3 fewer = hypo- root ite 1. ClO = hypochlorite
24 Binomial Nomenclature 1. Name cation first, anion last 1. Cation just use the name 2. Anion root of the name plus ide 2. If compound contains a polyatomic ion just name the ion 3. Transition Metals must include a roman numeral to indicate which oxidation state is used
25 What is the difference between a monatomic ion and a polyatomic ion How are the metals, nonmetals and polyatomic ions named in an ionic compound? Assignment: What is an oxyanion and how is it named? Complete the table by providing the correct formula for each combination: Potassium Barium Aluminum Ammonium Name the following compounds: NaBr CaCl2 KOH CU(NO3)2 Ag2CrO4 Oxide Chloride Sulfate Phosphate
26 Chapter 8.4 Metallic Bonds/Alloys
27 Metallic Bonding Formation of a lattice structure created when a group of atoms are crowded together and the outer-level orbitals overlap Electrons are not shared, nor are they gained or lost
28 Metallic Bonding Electron Sea Model Electrons overlap creating an artificial stability Overlap allows electrons to move freely from one atom to another
29 Delocalized Electrons Free to move between atoms Delocaliztion causes: High melting and boiling points Malleability and ductility Good conductivity Increase in hardness/strength with an increase in the number of electrons
30 Alloys Mixture of metallic elements Produced to attain properties not associated with any one metal Steel = Fe & C or Ni Brass = Cu & Zn Gold Jewelry = Au & Cu
31 Types of Alloys 1. Substitutional Atoms of one element replace the other due to similarities in size (most common) 1. Sterling silver (Ag&Cu) 2. Pewter (Sn, Sb & Pb) 2. Interstitial Formed when gaps between atoms are filled with smaller atoms
32 What is a metallic bond? Assignment: Explain how the conductivity of electricity and high melting points of metals are explained by metallic bonding. What is an alloy? How does a substitutional alloy differ from an interstitial alloy? In the lab, how could you determine if a solid has an ionic bond or a metallic bond?
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