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Ionic Bonding

Ionic Bonding. Chapter 5. Bonding. Ch.5 ionic bonding Ch.6 covalent bonding What is a bond? What is bonding?. Learning Objective. Students will learn how to predict the type of ion that a given element forms from its position on the periodic table.

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Ionic Bonding

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  1. Ionic Bonding Chapter 5

  2. Bonding Ch.5 ionic bonding Ch.6 covalent bonding What is a bond? What is bonding?

  3. Learning Objective Students will learn how to predict the type of ion that a given element forms from its position on the periodic table. Youtube: What are Ions | The Chemistry Journey | The Fuse School

  4. 5.1 Simple ions • How much an element reacts depends on it’s valence electron configuration • The noble gases show almost no chemical reactivity. • Why? • Because they have a full valence shell of electrons

  5. 5.1 Simple ions Octet rule ‘Atomsreactsothattheycanachievethesameelectronconfigurationsasthenoblegases.’ ‘Atoms react so that they can achieve the same electron configurations as the noble gases.’ Exception = ?

  6. Scratch paper Write the electron configuration of POTASSIUM Write the electron configuration of CHLORINE How many valence electrons do each of these elements have?

  7. 5.1 Simple ions: metals Example: Potassium (K) 1s22s22p63s23p64s1 Potassium wants to lose it’s one valence electron to achieve the same valence electron configuration as Ar 1s22s22p63s23p6 K  K+ + e

  8. 5.1 Simple ions: metals After giving up one electron…. potassium still has 19 protons….. but only 18 electrons. +19-18 = +1 Because the numbers are not the same, there is an overall electrical charge = ION K  K+ + e

  9. CATions have a positive charge. “Mr Turner feels positive about cats.” “Cats have paws.” Metals lose electrons to form cations. “Metals go Meow” 5.1 KWS: Cation

  10. 5.1 Simple ions: nonmetals Chlorine is reactive because it has seven valence electrons. 1s22s22p63s23p5 If chlorine gains one electron it has the same electron configuration has a noble gas Cl atom + e- Cl- ion 1s22s22p63s23p5 1s22s22p63s23p6

  11. 5.1 Simple ions: nonmetals • How many total electrons does a chlorine ion have? • ANS = 18 • How many protons does Chlorine ion have? • ANS = 17 • +17-18 = -1 • Therefore the chlorine ion has a -1 charge.

  12. 5.1 KWS: Anion Memory clue • “An aNion has a Negative charge.” • “Onions make us cry. We feel negatively about onions” (anions)

  13. 5.1 Think about it….. • What is the name of the type of ion with a negative charge: cation or anion? • Give an example of an element that loses electrons to form an ion with a positive charge.

  14. 5.1 Worksheet ‘Lewis Dot Structures of Atoms and Ions’

  15. Practice Write the electron configuration for: Magnesium Oxygen

  16. 5.1 Simple ions • What is the charge on the ion formed by Mg? [Mg] = 1s22s22p63s2 Mg atom  Mg 2+ ion + 2e • Cation or anion? • = cation • How many electrons does Mg 2+the ion have? • How many protons does the Mg 2+ion have?

  17. 5.1 Simple Ions What kind of ion is formed by oxygen? [O] = 1s22s22p4 O + 2e- O2- Anion!! By gaining two electrons, oxygen is said to have “completed it’s octet”

  18. 5.1 Simple Ions Misconception: ‘An atom and its ion have the same chemical properties.’ WRONG!!!! e.g. potassium atom vs potassium ion An atom and its ion have different chemical properties.

  19. 5.1 Simple Ions Misconception: When an atom loses/gains electrons to form an ion, it achieves an electron configuration identical to a noble gas. That does not mean it becomes a noble gas! Ar vs Cl-

  20. 5.2 Ionic Compounds Learning Target: What happens when cations and anions combine together? ‘What are Ionic Bonds? | The Chemistry Journey | The Fuse School”

  21. 5.2 Ionic Bonds When sodium and chlorine react….. sodium gives it’s valence electron to chlorine. Both elements ‘complete their octet’. Sodium + Chlorine  Sodium Chloride (NaCl) Element + Element  Compound Teacher Notes: VId: Reaction of Sodium and Chlorine Lewis structure

  22. 5.2 Ionic Bonds Metal + Nonmetal  Salt In chemistry, a salt is not just sodium chloride, Salt =the scientific name given to many different ionic compounds Sodium + Fluorine  NaF (a salt)

  23. Ionic compounds

  24. 5.2 Ionic Bonds • What is the force that holds a salt together? Electrostatic attraction: Opposites attract! • The force of attraction between a positive charge and a negative charge.

  25. 5.2 Crystal lattice

  26. 5.2 Ionic Compounds Learning Target: What are the properties of ionic compounds?

  27. Standard c. Analyze and interpret provided data about bulk properties of various substances to support claims about the relative strength of the interactions among particles in the substance. Youtube: Ionic Bonding (Mexus) https://www.youtube.com/watch?v=UeNJ7vKxcAo

  28. 5.2 Ionic Bonding crystal lattice: Salt crystals are made of repeating units of anions and cations

  29. 5.2 Ionic Bonding Ionic bonds are very strong

  30. 5.2 Ionic Bonding • Attractive forces involve more than a single cation and anion. • Six Na+ ions surround each Cl ion and • Six Cl- ions surround each Na+ ion. Youtube: Sodium Chloride Crystal lattice

  31. 5.2 X-ray crystallography

  32. Born-Haber Cycle p.169

  33. Notes: Bond making/breaking Breaking chemical bonds requires (releases/requires) energy Forming chemical bonds releases (releases/requires) energy

  34. Standard d. Develop a representation to show that energy is required to separate the atoms in a molecule and that energy is released when atoms at a distance come together to form molecules that are more stable.

  35. An ionic compound conducts electricity when dissolved in water ‘Electrolyte’ Demo: conductivity meter Youtube: Gatorade Hydration Institute : 5.2 Conductivity p.172

  36. 5.2 Ionic Bonding Notes: “To conduct an electric current, a substance must satisfy two conditions: • it must contain charged particles • those particles must be free to move” Teacher Notes: http://phet.colorado.edu/en/simulation/soluble-salts/ conductivity meter

  37. 5.3 Names & Formulas of ionic compounds Objectives • When given the formula of a compound we can write the name • E.g. NaCl = Sodium Chloride • When given the name of a compound we can write the formula • E.g. Sodium Chloride = NaCl

  38. 5.3 Names & Formulas of ionic compounds Formula  Name The name of an ionic compound is made up of just two words: • First, name of the cation • Cations have the same names as the elements. • For example, K+ = potassium ion. • Second, the name of the anion • For anions, the name ends in -ide. • For example, chlorine becomes chloride For example, KCl is potassium chloride

  39. 5.3 Names & Formulas of ionic compounds Formula  Name • For anions, the name ending changes to in -ide. • F- = fluoride • Cl = chloride • Br- = bromide • I- = iodide • O2- = oxide

  40. 5.3 Names & Formulas of ionic compounds Formula  Name • The name of a binary ionic compound is made up of just two words: the name of the cation followed by the name of the anion. NaClsodium chloride K2O potassium oxide Al2S3aluminum sulfide Practice: • Concept Review p. 7 #16-31 • (skip # 24,28, 30,31)

  41. 5.3 Names & Formulas of ionic compounds Exception • Many transition elements form more than one possible ion • For example, the names of the two copper ions are: Cu+ Cu2+ Teacher notes: Common Ions handout

  42. Example: Cu+ = copper (I) Cu2+ = copper (II) 5.3 Transition metal ions p.163

  43. 5.3 Transition metal ions p.163 If there is more than one possible ion….. roman numerals are used to indicate the charge.

  44. 5.3 Names & Formulas of ionic compounds Objectives • When given the formula of a compound we can write the name • E.g. NaCl = Sodium Chloride • When given the name of a compound we can write the formula • E.g. Sodium Chloride = NaCl Worksheet: Chemical Formulas and Names of Ionic Compounds

  45. Crystal lattice The formula of an ionic compound just tells us the ratio of ions in that compound e.g. NaCl = Na1Cl1 Na+:Cl- 1:1

  46. 5.2 Ionic Bonding Ionic Compounds Do Not Consist of Molecules There are no individual, separate molecules in an ionic compound.

  47. 5.3 Names & Formulas of ionic compounds Name  Formula • ionic compounds have no overall charge The rule: • total positive charge (cations) + total negative charge (anions) = 0

  48. 5.3 Names & Formulas of ionic compounds p.177 Try: magnesium chloride Procedure: • Write the symbol and charges for the cation and the anion (remember sec 5.1) • Determine the ratio that the ions must combine in so that their charges cancel (Tip: look for the lowest common multiple) • Use subscripts to denote the ratio of cations to anions e.g. AxBy

  49. Chapter 5 5.3 Names & Formulas of ionic compounds Name  Formula Guided Practice: • Sodium oxide • Calcium oxide • Aluminum oxide • Independent Practice: • Concept Review p. 6 # 9-15 • Concept Review p. 7 # 24,28, 30,31 • Finished? • Try: p.180 #6 b,c,d #7 a,b,c ‘crossing technique’

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