Ionic bonding 9 grade. All the characteristics of ionic compounds

Ionic bonding.All properties and uses

1. Lesson aims: understand how ionic bond forms. draw electron configurations of ions. name binary ionic compounds. explain the properties of ionic compounds based on their structure.

2. Ions are electrically charged particles formed when  atoms  lose or gain electrons .  Metal atoms  lose the electron, or electrons, in their highest energy level and  become positively charged ions-cations Non-metal atoms  gain an electron, or electrons, from another atom to become negatively charged ions-anions

3. Ionic bond The ionic bond is the type of chemical bond that involves the electrostatic attraction between oppositely charged metal and nonmetal ions

4. NaCl How does this compound formed?

5. Explanation : Sodium atom has 1 electron on outer shell and chlorine atom has 7 outer electrons, in order to reach octet sodium loses 1 electron and chlorine gain 1 electron TRANSFER OF ELECTRONS from metal to nonmetal forms positively charged metallic ion and negatively charged non-metallic ion

6. How to determine the charge of an ion using the Periodic Table? For metals: the group number shows the charge of an ion with the positive sign For monatomic ions (non-metals): 8-group number = charge of the ion with the negative sign

7. The Periodic Table with charges of ions

8. Memorise the table of ions and their charges with names

9. Group work Using the ion cards create the formulas of ionic compounds noticing on balancing their charges. Make your own combinations of ions in empty cells of the table. For example: What ratio will the +1 and -1 ions combine to balance the charge? What will be the formula for this compound?

10. Naming ionic compounds Rules for naming simple ionic compounds. 1. Name the metal by its elemental name. 2. Name the nonmetal by its elemental name and an -ide ending. 3. Name metals that can have different ions charges using roman numerals to indicate positive charge. Example Fe 2+ is Iron(II) 4. Name polyatomic ions by their names.

11. Complete the following tasks Video Help: https://www.youtube.com/watch?v=URc75hoKGLY Task 1. Write the formula of ionic compounds: sodium chloride magnesium oxide lithium sulfide calcium hydride

12. Complete the following tasks Task 2. Write the names of the following ionic compounds: Al 2 S 3 MgCl 2 K 2 O

13. The oppositely charged ions are arranged regularly in three dimensions to form giant ionic lattices . Ionic compounds  often form crystals as a result. Ionic lattice structures

14. State of matter: Solids Brittle and Hard Have a crystal lattice Have high melting and boiling points Conduct electricity in molten state and in aqueous solution Soluble in water Physical properties of ionic compounds

15. Demonstration: conductivity of different compounds Using the experimental set-up shown on the picture we will test conductivity of 5 different compounds: NaCl sodium chloride, sugar, distilled water, ethanol.Observe if the bulb lights and predict what is the best conductor of electricity.

16. Conductivity Solid ionic compounds do not conduct electricity (the ions are not free to move). Melted and dissolved ionic compounds conduct electricity (the ions are free to move).

17. Solubility Solubility is the measure of the maximum amount of solute that can be dissolved in a given quantity of solvent at a given temperature and pressure. Solubility is usually measured in molarity (M) or moles per liter (mol/L). A compound is termed soluble if it dissolves in water.

18. Ionic compounds are soluble in water When soluble salts dissolve in water, the ions in the solid separate and disperse uniformly throughout the solution; this process represents a physical change known as dissociation . Potassium chloride (KCl) is an example of a soluble salt. When solid KCl is added to water, the positive (hydrogen) end of the polar water molecules is attracted to the negative chloride ions, and the negative (oxygen) ends of water are attracted to the positive potassium ions. The water molecules surround individual K + and Cl − ions, reducing the strong forces that bind the ions together and letting them move off into solution as solvated ions. https://www.youtube.com/watch?v=xdedxfhcpWo

19. Uses of ionic compounds NaCl, sodium chloride: ordinary table salt Iodized salts are a mixture of table salt with some salt of iodine, most commonly potassium iodide (KI). Since it can be added to a common food item without altering the taste, it is an easy way to get iodine in the diet. The use of fluoride toothpaste is an important public health measure to both prevent and reduce the severity of dental caries in all age groups.

20. Uses of ionic compounds Baking soda is another most commonly found chemical in a household, specifically in the kitchen. It is one of the most vividly used leavening agents used in baking goods to improve their texture and appearance. In chemistry, it is known by the name sodium bicarbonate (IUPAC name: sodium hydrogen carbonate) Washing soda is an essential chemical compound found in laundry detergent powders and liquids. It is used to remove stubborn stains from laundry. The chemical name for washing soda is sodium carbonate decahydrate, Na2CO3 * 10 H2O

21. Uses of ionic compounds Bleach is a name given to all the compounds that are used for cleaning stains and/or removing color from fabric. It often refers, specifically, to a dilute solution of sodium hypochlorite, also called “liquid bleach.” Sodium hypochlorite (NaOCl) To keep up with the pace of the ever-developing world, people rely more and more on packaged foods and drinks. Nevertheless, there is always some concern about the contamination of packed food due to the growth of microorganisms such as yeast and bacteria. Thankfully, preservation techniques have come a long way in the past few years, allowing manufacturers and companies to increase the shelf life of their products and significantly lower the risk of food-borne illness. Sodium benzoate ( C6H5COONa ) is one such preservative that prevents the growth of microorganisms such as bacteria and fungi, and slow the oxidation of fats that cause rancidity. It is denoted by the E number E211 on the food products.

22. Which of the following will have ionic bonding? Copper chloride Iron Brass Sulphur dioxide Test

23. Which of the following is NOT true of ionic bonding? Metal ions have a + charge Non-metal ions have a - charge They form a 2 dimensional lattice They have giant structures

24. Which of the following is true about the oxide ion ? Formed by oxygen atoms losing 2 electrons. Oxygen ions have an empty second shell Exist in pairs Have a 2- charge 16 O 8

25. Which of the following is true about the sodium ion ? Has a 2,8,1 electron arrangement Formed by sodium atoms gaining 1 electron. Sodium ions have an empty second shell Have a 1+ charge 23 Na 11

26. Homework Using the following link https://teachchemistry.org/classroom-resources/matchmaker-ionic-bonding play the game and write the formulas of ionic compounds in your copybook