Name: ___________________
Date: ____________
Introduction to Ionic Bonding: A Flipped Lesson
Instructions: Use the QR codes or the three videos on Ms. Zagelbaum’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
2. Covalent (Molecular) Bonding
3. Metallic Bonding
Connects
______________ + ______________
Connects
nonmetal + nonmetal
Connects
metal + metal
Examples:
a) Silver chloride (__________)
b) Magnesium iodide ( _______)
Examples:
a) Water (__________)
b) Carbon dioxide ( ______)
b) Barium (____)
c) Aluminum oxide (_________)
c) Methane (________)
c) Aluminum (____)
1.
____________________
Highlight/underline the metal in
purple and the nonmetal in green.
Highlight/underline the 2 nonmetals
in green.
Examples:
a) Silver (____)
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”?
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 Why are sodium ion and chloride ion fused together after the transfer of an electron?
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Ms. Roman & Mrs. Zagelbaum
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)
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 How can sodium and fluorine “get happy” (stable)?
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ATOMS OF SODIUM & CHLORINE
Na0
Bohr Model of Sodium Atom
Cl0
p+_________
p+________
e-_________
e-________
Electron configuration:
Electron configuration:
__________________
__________________
Net charge: ____
Bohr Model of Chlorine Atom
Net charge: ____
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
Bohr Model of Sodium
Cation
Cl-1
p+_________
p+________
e-_________
e-________
Electron configuration:
Electron configuration:
__________________
__________________
Net charge: ____
Net charge: ____
Bohr Model of Chloride Anion
Ms. Roman & Mrs. Zagelbaum
Ionic Bonding, Part III
1. Why do electrons move from sodium to chlorine, and not vice versa?
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2. Define electronegativity:
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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-”?
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Ms. Roman & Mrs. Zagelbaum
Properties of Ionic Compounds
Compound
NaCl(s)
Sodium Chloride
NaF(s)
Sodium Fluoride
NH4NO3(s)
Ammonium Nitrate
Real-Life Application
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
Ms. Roman & Mrs. Zagelbaum
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. 2-8-8
6. 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
Ms. Roman & Mrs. Zagelbaum