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Unit: Chemical Bonding

Test Review ANSWERS

What to study?

• 
  Homework: worksheets #1-#6
  
• 
  Notes: Bonding BasicsPolarity
  
• 
  Bell Ringers: Review of Ionic Bonding, Review of Covalent Bonding, Review of electron dot diagrams, Reviewing Ionic vs. Covalent compounds
  

What will the questions be like? What can I expect?

This test will be just like the previous quizzes you have taken.

• 
  Matching
  
• 
  Multiple choice
  
• 
  Application (of writing formulas)
  

Sample questions/Important Topics

1. 
   Fill in the best answer for each of the following:
   

1. 
   The electrons in an atom’s outermost shell are called its valence electrons.
   
2. 
   Sodium wants to lose one electron to become isoelectronic with Neon.
   
3. 
   When magnesium gets the same electron configuration as Ne it has a +2 charge.
   
4. 
   A single covalent bond consists of 2 shared electrons.
   
5. 
   The octet rule says that most atoms want 8 electrons in their outermost shell.
   

6. 
   In ionic bonding, the two ways atoms can get the same configuration as a noble gas is by gaining or losing electrons.
   
7. 
   In covalent bonding, atoms share electrons.
   
8. 
   Atoms in group 15 will gain three electrons to get a –3 charge.
   
9. 
   Molecules with 5 atoms, like CH₄, will have a tetrahedral shape.
   
10. 
    The VSEPR theory stands for the valence shell electron pair repulsion theory.
    
11. 
    Ar and Cl^-1 have the same electron configuration, so they are isoelectronic with each other.
    
12. 
    I^-1 has the same electron configuration as the noble gas Xenon.
    
13. 
    Helium is the only noble gas with 2 valence electrons.
    
14. 
    Ionic compounds are made up of crystals, which are very large structures consisting of alternating + and – ions.
    
15. 
    When atoms lose electrons they get a positive charge.
    
16. 
    When nitrogen bonds covalently it will make a total of three bonds.
    
17. 
    Ionic compounds will not conduct an electric current in the solid state.
    

18. 
    Metals are malleable, which means they can be hammered into different shapes.
    
19. 
    Hydrogen is the only element in group 1 to bond covalently.
    
20. 
    Molecules with a trigonal bipyramidal shape have a total of six atoms in the molecule.
    

21. 
    The difference between the trigonal planar and pyramid shapes is that the pyramid shape has an unshared pair of electrons on the central atom.
    
22. 
    A double covalent bond consists of four shared electrons.
    
23. 
    The 2 types of bonding are covalent and ionic.
    

z) In a polar covalent bond, electrons are shared unequally.
2
.
. a) Write the electron configuration for K 1s² 2s² 2p⁶ 3s² 3p⁶ 4s¹

2. 
   Write the electron dot structure for K: K
   

2. 
   How many electrons will K lose or gain to attain a noble gas configuration? Lose 1
   

2. 
   What charge will K have when it loses or gains those electrons? +1
   

2. 
   Write the new electron configuration for K 1s² 2s² 2p⁶ 3s² 3p⁶
   

(after it loses or gains those electrons)

2. 
   What noble gas is K now isoelectronic with? Argon
   

3. 
   a
   .
   
   .
   
   .
   ) Write the electron configuration for N 1s² 2s² 2p³
   

.

.

2. 
   Write the electron dot structure for N: N
   

2. 
   How many electrons will N lose or gain to attain a noble gas configuration? Gain 3
   

2. 
   What charge will N have when it loses or gains those electrons? -3
   

2. 
   Write the new electron configuration for N 1s² 2s² 2p⁶
   

(after it loses or gains those electrons)

2. 
   What noble gas is N now isoelectronic with? Neon
   

3. 
   If K and N bonded together, what would the formula be for the compound they would form? Use electron dot structures to show how this would happen.
   

Formula = K₃N (Show work below)