Name: 
 

Bonding 2


Matching
 
 
Match each item with the correct statement below.
a.
coordinate covalent bond
d.
single covalent bond
b.
double covalent bond
e.
polar bond
c.
structural formula
f.
hydrogen bond
 

 1. 
a depiction of the arrangement of atoms in molecules and polyatomic ions
 

 2. 
a covalent bond in which only one pair of electrons is shared
 

 3. 
a covalent bond in which two pairs of electrons are shared
 

 4. 
a covalent bond in which the shared electron pair comes from only one of the atoms
 

Multiple Choice
Identify the letter of the choice that best completes the statement or answers the question.
 

 5. 
How many valence electrons are in an atom of phosphorus?
a.
2
c.
4
b.
3
d.
5
 

 6. 
How many valence electrons are in an atom of magnesium?
a.
2
c.
4
b.
3
d.
5
 

 7. 
How many valence electrons does a helium atom have?
a.
2
c.
4
b.
3
d.
5
 

 8. 
How many valence electrons are in a silicon atom?
a.
2
c.
6
b.
4
d.
8
 

 9. 
What is the electron configuration of the calcium ion?
a.
1s5test2_files/i0120000.jpg2s5test2_files/i0120001.jpg2p5test2_files/i0120002.jpg3s5test2_files/i0120003.jpg3p5test2_files/i0120004.jpg
c.
1s5test2_files/i0120005.jpg2s5test2_files/i0120006.jpg2p5test2_files/i0120007.jpg3s5test2_files/i0120008.jpg3p5test2_files/i0120009.jpg4s5test2_files/i0120010.jpg
b.
1s5test2_files/i0120011.jpg2s5test2_files/i0120012.jpg2p5test2_files/i0120013.jpg3s5test2_files/i0120014.jpg3p5test2_files/i0120015.jpg4s5test2_files/i0120016.jpg
d.
1s5test2_files/i0120017.jpg2s5test2_files/i0120018.jpg2p5test2_files/i0120019.jpg3s5test2_files/i0120020.jpg
 

 10. 
What is the charge on the strontium ion?
a.
2–
c.
15test2_files/i0130000.jpg
b.
1–
d.
25test2_files/i0130001.jpg
 

 11. 
The octet rule states that, in chemical compounds, atoms tend to have ____.
a.
the electron configuration of a noble gas
b.
more protons than electrons
c.
eight electrons in their principal energy level
d.
more electrons than protons
 

 12. 
What is the formula of the ion formed when potassium achieves noble-gas electron configuration?
a.
K5test2_files/i0150000.jpg
c.
K5test2_files/i0150001.jpg
b.
K5test2_files/i0150002.jpg
d.
K5test2_files/i0150003.jpg
 

 13. 
Which of the following ions has a pseudo-noble-gas electron configuration?
a.
Fe5test2_files/i0160000.jpg
c.
Cu5test2_files/i0160001.jpg
b.
Mn5test2_files/i0160002.jpg
d.
Ni5test2_files/i0160003.jpg
 

 14. 
Which of the following elements does NOT form an ion with a charge of 15test2_files/i0170000.jpg?
a.
fluorine
c.
potassium
b.
hydrogen
d.
sodium
 

 15. 
How many electrons does nitrogen gain in order to achieve a noble-gas electron configuration?
a.
1
c.
3
b.
2
d.
4
 

 16. 
What is the formula of the ion formed when phosphorus achieves a noble-gas electron configuration?
a.
P5test2_files/i0190000.jpg
c.
P5test2_files/i0190001.jpg
b.
P5test2_files/i0190002.jpg
d.
P5test2_files/i0190003.jpg
 

 17. 
How does oxygen obey the octet rule when reacting to form compounds?
a.
It gains electrons.
b.
It gives up electrons.
c.
It does not change its number of electrons.
d.
Oxygen does not obey the octet rule.
 

 18. 
What is the charge on the cation in the ionic compound sodium sulfide?
a.
0
c.
25test2_files/i0210000.jpg
b.
15test2_files/i0210001.jpg
d.
35test2_files/i0210002.jpg
 

 19. 
Which of the following occurs in an ionic bond?
a.
Oppositely charged ions attract.
b.
Two atoms share two electrons.
c.
Two atoms share more than two electrons.
d.
Like-charged ions attract.
 

 20. 
What is the net charge of the ionic compound calcium fluoride?
a.
2–
c.
0
b.
1–
d.
15test2_files/i0230000.jpg
 

 21. 
A compound held together by ionic bonds is called a ____.
a.
diatomic molecule
c.
covalent molecule
b.
polar compound
d.
salt
 

 22. 
Which of the following is true about an ionic compound?
a.
It is a salt.
c.
It is composed of anions and cations.
b.
It is held together by ionic bonds.
d.
all of the above
 

 23. 
Which of the following pairs of elements is most likely to form an ionic compound?
a.
magnesium and fluorine
c.
oxygen and chlorine
b.
nitrogen and sulfur
d.
sodium and aluminum
 

 24. 
Ionic compounds are normally in which physical state at room temperature?
a.
solid
c.
gas
b.
liquid
d.
plasma
 

 25. 
Which of the following is true about the melting temperature of potassium chloride?
a.
The melting temperature is relatively high.
b.
The melting temperature is variable and unpredictable.
c.
The melting temperature is relatively low.
d.
Potassium chloride does not melt.
 

 26. 
Under what conditions can potassium bromide conduct electricity?
a.
only when melted
b.
only when dissolved
c.
only when it is in crystal form
d.
only when melted or dissolved in water
 

 27. 
Which of the following is NOT a characteristic of most ionic compounds?
a.
They are solids.
b.
They have low melting points.
c.
When melted, they conduct an electric current.
d.
They are composed of metallic and nonmetallic elements.
 

 28. 
Which of the following particles are free to drift in metals?
a.
protons
c.
neutrons
b.
electrons
d.
cations
 

 29. 
What is the basis of a metallic bond?
a.
the attraction of metal ions to mobile electrons
b.
the attraction between neutral metal atoms
c.
the neutralization of protons by electrons
d.
the attraction of oppositely charged ions
 

 30. 
What characteristic of metals makes them good electrical conductors?
a.
They have mobile valence electrons.
b.
They have mobile protons.
c.
They have mobile cations.
d.
Their crystal structures can be rearranged easily.
 

 31. 
An ionic bond is a bond between ____.
a.
a cation and an anion
c.
the ions of two different metals
b.
valence electrons and cations
d.
the ions of two different nonmetals
 

 32. 
Which is a typical characteristic of an ionic compound?
a.
Electron pairs are shared among atoms.
b.
The ionic compound has a low solubility in water.
c.
The ionic compound is described as a molecule.
d.
The ionic compound has a high melting point.
 

 33. 
What is shown by the structural formula of a molecule or polyatomic ion?
a.
the arrangement of bonded atoms
c.
the number of metallic bonds
b.
the number of ionic bonds
d.
the shapes of molecular orbitals
 

 34. 
Which of these elements does not exist as a diatomic molecule?
a.
Ne
c.
H
b.
F
d.
I
 

 35. 
Why do atoms share electrons in covalent bonds?
a.
to become ions and attract each other
b.
to attain a noble-gas electron configuration
c.
to become more polar
d.
to increase their atomic numbers
 

 36. 
Which of the following is the name given to the pairs of valence electrons that do not participate in bonding in diatomic oxygen molecules?
a.
unvalenced pair
c.
inner pair
b.
outer pair
d.
unshared pair
 

 37. 
The shape of the methane molecule is called ____.
a.
tetrahedral
c.
four-cornered
b.
square
d.
planar
 

 38. 
What is the shape of a molecule with a triple bond?
a.
tetrahedral
c.
bent
b.
pyramidal
d.
linear
 

 39. 
A bond formed between a silicon atom and an oxygen atom is likely to be ____.
a.
ionic
c.
polar covalent
b.
coordinate covalent
d.
nonpolar covalent
 

 40. 
Which type of solid has the highest melting point?
a.
ionic solid
c.
metal
b.
network solid
d.
nonmetallic solid
 

 41. 
What is required in order to melt a network solid?
a.
breaking Van der Waals bonds
c.
breaking hydrogen bonds
b.
breaking ionic bonds
d.
breaking covalent bonds
 

Short Answer
 

 42. 
What is the formula for the oxide ion?
 

 43. 
Give the electron configuration for the chloride ion.
 

Numeric Response
 

 44. 
What is the charge of a particle having 9 protons and 10 electrons?

 

 45. 
How many unshared pairs of electrons are in a molecule of hydrogen iodide?

 

Essay
 

 46. 
Explain how scientists have used metallic bonding to account for many of the physical properties of metals, such as electrical conductivity and malleability.
 

 47. 
Describe a network solid and give two examples.
 



 
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