Name ___________________________________ Date ______________________ Class ______________________
Chapter 7 – Ionic and Metallic Bonding
Guided Reading
Section 1 - Ions - This section explains how to use the periodic table to infer the number of valence electrons in an atom
and draw its electron dot structure. It also describes the formation of cations from metals and anions from nonmetals.
As you read Chapter 7 Section 1 define the following words:
Valence electrons –
Electron dot structures –
Octet rule –
Halide ions –
As you read Chapter 7 Section 1 complete the following questions:
How can you find the number of valence electrons an atom has?
Describe, in your own words, what the octet rule is.
what is an electron dot structure?
Draw the electron dot structures for the following elements: He, Ne, Li, Mg, Si, S, and Cl.
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Octet comes from the Greek work okto, meaning "eight." There are eight electrons in the highest occupied energy level
of the noble gases, except for helium. How do you think the term octet might also be applied to music or poetry?
Describe how cations form.
In Figure 7.2 How many electrons are in the highest energy level of Na+?
Describe how anions form.
In Figure 7.5 In which group of the periodic tale to the elements bromine and iodine belong?
Fill in the blanks of the following statement: Metallic atoms tend to lose their valence electrons to produce a(n)
_______________, or a positively charged ion. Most nonmetallic atoms achieve a complete octet by gaining or
_______________ electrons.
Which noble gas has the same electron configuration as a chloride ion?
How many electrons do halogen atoms need to gain in order to achieve the electron configuration of a noble gas?
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Section 2 - Ionic Bonds and Ionic Compounds - This section lists the characteristics of an ionic bond. It also describes
the use of these characteristics to explain the electrical conductivity of ionic compounds when melted and when in
aqueous solution.
As you read Chapter 7 Section 2 define the following words:
Ionic compounds –
Ionic bonds –
Chemical formula –
Formula unit –
Coordination number –
As you read Chapter 7 Section 2 complete the following questions:
Describe how ionic bonds form.
If ionic compounds are neutral how can they be composed of charged particles?
Compare and contrast chemical formula and formula unit.
What is the formula unit for magnesium chloride?
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In Figure 7.8 How does the arrangement of ions in a sodium arrangements of ions in a sodium chloride crystal help
explain why the compound is so stable?
In Conceptual Problem 7.2 it shows how to use electron dot structures to determine formula units. Use electron dot
structures to determine the formula units of the ionic compound formed when potassium reacts with iodine.
List at least three properties of ionic compounds.
In Figure 7.9 What is something that all of the picture of crystals have in common?
How is the coordination number of an ionic compound is determined?
What is the coordination number of Ti4+ in TiO2?
In Figure 7.11 What would happen if the voltage was applied across a solution of NaCl dissolved in water?
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Section 3 - Bonding in Metals - This section uses the theory of metallic bonds to explain the physical properties of
metals. It also describes the arrangement of atoms in some common metallic crystal structures.
As you read Chapter 7 Section 3 (Pages 201 - 203) define the following words:
Metallic bond –
Alloys –
As you read Chapter 7 Section 3 complete the following questions:
In your own words describe metallic bonds.
In Figure 7.12 What causes the ionic crystal to break apart?
Define ductile.
Define malleable.
State the three crystalline shapes that metals form and how many neighbors they have.
In Figure 7.14 Which of these arrangement is the most closely packed?
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What metals crystallize in a face-centered cubic pattern?
Why are alloys important?
Fill in the blanks of the following statement: ____________________ alloys have smaller atoms that fit into the spaces
between larger atoms. ____________________ alloys have component atoms that are roughly equal in size.
Bronze is an alloy that is composed of which elements and how many parts of each?
Use Table 7.3 to tell what elements are in the following alloys:
Sterling silver:
Cast iron:
Stainless steel:
Spring steel:
Surgical steel:
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