Introduction to Ionic Bonding: A Flipped Lesson
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1 Name: _ Date: Period: Unit 4: Bonding Introduction to Ionic Bonding: A Flipped Lesson Instructions: Use the QR codes or the three videos on Ms. Roman s website to complete the flipped lesson on ionic bonding. Ionic Bonding, Part I As you watch the video, fill in the flow chart below about the three different types of bonds. Types of Chemical Bonds Covalent (Molecular) Bonding 3. Metallic Bonding + a) Silver chloride ( ) b) Magnesium iodide ( ) c) Aluminum oxide ( ) nonmetal + nonmetal a) Water ( ) b) Carbon dioxide ( ) c) Methane ( ) metal + metal a) Silver ( ) b) Barium ( ) c) Aluminum ( ) Highlight/underline the metal in purple and the nonmetal in green. Highlight/underline the 2 nonmetals in green. Highlight/underline the metal in purple. Example of Ionic Bonding: NaCl (sodium chloride) Steps (3:22) 1. Start with separate atoms. Diagrams 2. Sodium transfers an electron to chlorine. 3. Atoms get a charge and become ions. What is the difference between chlorine and chloride? Why are sodium ion and chloride ion fused together after the transfer of an electron?
2 Ionic Bonding, Part II Draw Bohr models of sodium and fluorine atoms below, and calculate the numbers of subatomic particles. Make sodium s electron s purple and fluorine s electrons green. (You don t have to draw the empty electron spots, as they are in the video. I would leave them out.) Why are the atoms of sodium and fluorine unhappy (unstable)? (2:57) How can sodium and fluorine get happy (stable)? ATOMS OF SODIUM & CHLORINE Na 0 p + e - Bohr Model of Sodium Atom Cl 0 p + e - Bohr Model of Chlorine Atom Draw Bohr models of sodium and chloride ions below, after the transfer of sodium s valence electron to chlorine. IONS OF SODIUM & CHLORIDE Na +1 p + Bohr Model of Sodium Cation Cl -1 p + Bohr Model of Chloride Anion e - e -
3 Ionic Bonding, Part III 1. Why do electrons move from sodium to chlorine, and not vice versa? 2. Define electronegativity: 3. In general which type of elements have higher electronegativity? 4. Check off the appropriate box for each description below: Metals High electronegativity Low electronegativity Lose electrons in ionic bonding Gain electrons in ionic bonding Form cations Form anions Ionic radius is LARGER than atomic radius Ionic radius is SMALLER than atomic radius Nonmetals 5. Why don t ionic compounds, like sodium chloride, hang out separate from one another, as shown at right? 6. Draw a lattice structure below to represent how sodium chloride would be arranged. (Try google if you re not sure how to represent this 3-D structure on your paper.) 7. Synthesis of Sodium Chloride Chemical Equation 2Na(s) 0 + Cl2(g) 0 2NaCl(s) Word Equation plus yields 8. Why is it incorrect to write sodium chloride as Na + Cl -?
4 Properties of Ionic Compounds Compound Real-Life Application NaCl(s) Sodium Chloride NaF(s) Sodium Fluoride NH4NO3(s) Ammonium Nitrate Key Properties of Ionic Compounds Identify five key properties of ionic compounds AND give a brief explanation of why each property exists. 1. (0:35) 2. (0:35) 3. (1:27) 4. (2:12) 5. (2:57) Applying What You ve Learned 1. Which element reacts with oxygen to form ionic bonds? a. calcium b. hydrogen c. chlorine d. nitrogen 2. An ionic compound is formed when there is a reaction between the elements a. strontium and chlorine b. hydrogen and chlorine c. nitrogen and oxygen d. sulfur and oxygen 3. The bonds in BaO are best described as a. covalent, because valence electrons are shared b. covalent, because valence electrons are transferred c. ionic, because valence electrons are shared d. ionic, because valence electrons are transferred
5 4. Compared to a calcium atom, the calcium ion Ca2+ has a. more protons b. fewer protons c. more electrons d. fewer electrons 5. A neutral atom with the electron configuration 2-6 would most likely form a bond with an atom having the configuration a. 2 b. 2-2 c. 2-8 d An ionic compound consists of positive and negative ions each with 10 electrons. Half of these ions have a charge of 1+ and the other half have a charge of 1. What is the formula of this compound? a. KF b. KCl c. NaF d. NaCl 7. Element X is in Group 2 and element Y is in Group 17. What happens when a compound is formed between these two atoms? a. X loses electrons to Y to form an ionic bond. b. X loses electrons to Y to form a covalent bond. c. X gains electrons from Y to form an ionic bond. d. X gains electrons from Y to form a covalent bond. 8. When combining with nonmetallic atoms, metallic atoms generally will a. lose electrons and form negative ions b. lose electrons and form positive ions c. gain electrons and form negative ions d. gain electrons and form positive ions 9. Hydrogen forms a negative ion when it combines with sodium to form NaH. This is primarily because hydrogen a. loses an electron to sodium b. has a greater attraction for electrons than sodium has c. is a larger atom than sodium d. has a smaller ionization energy than sodium 10. Which compound is ionic? a. HCl b. CaCl2 c. SO2 d. N2O
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