02. Ionic Bonding T2

Success Criteria

• Define ionic bonding.

• Construct dot and cross diagrams to represent ionic bonding.

• Determine the empirical formula of ionic compounds.

Learning Objectives

• Analyze the formation of ionic bonds through electron transfer between atoms.

• Construct detailed dot and cross diagrams to accurately represent ionic compounds and their empirical formulas.

Date

• Friday, November 15, 2024

Key Vocabulary

• Ion: a charged atom or molecule.

• Empirical Formula: the simplest ratio of elements in a compound.

Page 1: Knowledge Check on the Periodic Table

• Write one thing you know about the periodic table.

• Write two things you know about the periodic table.

• Write three things you know about the periodic table.

Page 2: Questions and Drills

Do Now Questions

1. State the charge of electrons.

2. Explain what it means for an atom to be neutral.

3. Explain what it means for an atom to be stable.

4. Define an ion.

5. State where metals are found in the periodic table.

Drill

1. State the electronic configuration of lithium.

2. State the electronic configuration of sodium.

3. State the electronic configuration of potassium.

Page 3: Answers for Do Now

States:

1. Charge of electrons: -1

2. Neutral atom: has equal numbers of protons and electrons.

3. Stable atom: has a full outer shell of electrons.

4. Ion: an atom that has gained or lost electrons.

5. Metals are located on the left side of the periodic table.

Page 4: Drill Answers

1. Lithium: 2,1

2. Sodium: 2,8,1

3. Potassium: 2,8,8,1

Page 5: Atoms and Ions

• An ion is a charged atom or a group of atoms:

  • Negative Ion: gains electrons (typically formed by non-metals).

  • Positive Ion: loses electrons (typically formed by metals).

• Atoms form ions to achieve a stable electronic arrangement.

Example Charges

1. Potassium ion: K+

2. Fluoride ion: F-

3. Calcium ion: Ca2+

Page 6: Ionic Bonding

• Ionic bonding occurs in compounds formed from metals combined with non-metals.

  • Example: Sodium (Na) loses 1 electron, Fluorine (F) gains 1 electron.

  • Sodium ion: Na+, Fluoride ion: F-.

  • Resulting compound: Sodium Fluoride (NaF).

Page 7: Characteristics of Ionic Bonding

• Ionic bonding: strong electrostatic force of attraction between oppositely charged ions.

Page 8: Ionic Bonding Model

• Sodium loses an electron to form Na+; Fluorine gains an electron to form F-.

• Electrostatic forces hold oppositely charged ions together in compounds like Sodium Fluoride.

Page 9: Magnesium and Oxide Bonding

• Magnesium (Mg) loses 2 electrons, Oxygen (O) gains 2 electrons.

• Resulting ions: Magnesium ion Mg2+, Oxide ion O2-.

• Compound formed: Magnesium Oxide (MgO).

Page 10: Sodium and Oxygen Bonding

• Sodium loses 1 electron and forms Na+

• Oxygen gains 2 electrons and forms O2-.

• Result: Sodium Oxide (Na2O).

Page 11: Magnesium and Fluoride Bonding

• Magnesium transfers 1 electron to each Fluorine atom.

• Results in 1 Magnesium ion (Mg2+) and 2 Fluoride ions (F-).

• Empirical formula: Magnesium Fluoride (MgF2).

Page 12: Bonding in Lithium Fluoride

Steps to Success

1. Draw electronic configurations using dots and crosses.

2. Draw arrows to show electron transfer.

3. Draw ions with square brackets showing charge.

4. Example: Lithium Fluoride, LiF.

Page 13: Bonding in Lithium Oxide

• Example: Lithium Oxide, Li2O.

• Follow similar steps for dot and cross diagrams.

Page 14: Bonding in Sodium Chloride

• Example: Sodium Chloride, NaCl.

• Follow similar steps for dot and cross diagrams.

Page 15: Empirical Formula for Beryllium Oxide

• Beryllium Oxide: BeO not Be2O.

Page 16: Think-Pair-Share Activity

• Discussion Questions: a) Are ions neutral? b) Are ions stable?

Page 17: Drill Questions

1. Difference between sodium atom and ion?

2. Do metal atoms lose or gain electrons?

3. Valence electrons in chlorine?

4. Charge of group 7 atoms?

5. Charge relation in metals and their group number?

6. Charge relation in non-metals and their group number?

7. Sodium with fluorine interaction?

8. Sodium with oxygen interaction?

9. Why different symbols for electrons?

10. Explain sodium and fluorine interaction.

Page 18: Drill Answers

1. Neutral sodium atom: 2,8,1; Sodium ion: 2,8.

2. Metal atoms lose electrons.

3. Chlorine has 7 valence electrons.

4. Group 7 forms -1 charge.

5. Metals: group number equals ion charge.

6. Non-metals: group number equals ion charge × -1.

7. One sodium with one fluorine.

8. Two sodium with one oxygen.

9. Different symbols clarify electron transfer.

Page 19: Review and Practice

• Based on success in drilled questions, review specified resources or tasks.

Page 20: High Demand Exam Question Activity

• Plan answer, emphasizing electron transfer in sodium-oxygen reaction.

Page 21: Low Demand Exam Question Activity

• Describe sodium-fluorine reaction, focusing on electron transfer.

Page 22: Follow-up Questions

1. Correct representation of sodium ion?

   • Answer: B. Na+

2. True statement regarding metals:

   • Answer: C. Metal atoms lose electrons to become positive ions.

3. Empirical formula of lithium oxide:

   • Answer: C. Li2O.