Bonding Unit Test Review
Use your notes to answer the following questions.
Name _________________________________________Period ______
1. What are valence electrons? These are the electrons that are the farthest from
the nucleus.
2. The elements in a group have _______The same_____________ number of
valence electrons.
3. Tell the number of valence electrons in each group:
a. Group 1
1 valence electron
b. Group 2
2 valence electrons
c. Group 13
3 valence electrons
d. Group 14
4 valence electrons
e. Group 15
5 valence electrons
f. Group 16
6 valence electrons
g. Group 17
7 valence electrons
h. Group 18
8 valence electrons
i. Groups 3-12 # of valence electrons varies
4. Cations lose valence electrons and have a ____positive____ ionic charge.
5. Anions gain valence electrons and have a _____negative___ ionic charge.
6. How do the electrons behave in a covalent bond?
The valence electrons are shared between atoms.
7. How do the electrons behave in an ionic bond?
The valence electrons are transferred. Atoms will either gain or lose electrons.
8. How do the electrons behave in a metallic bond?
Electrons flow freely between atoms.
9. Which type of bond dissolves easily in water?
Ionic Bonds
10. Which type of bond has a high melting point? Low melting point?
Ionic bonds and Metallic bonds have high melting points. Covalent bonds have a
low melting point.
11. Which type of bond has the most energy stored in it?
Covalent Bond
12. Which type of bond conduct electricity as a solution? As a solid?
Ionic bonds conduct electricity as a solution. Metallic bonds conduct electricity
as a solid.
13.
Ca(NO3)2
a. Identify the number and kinds of atoms in calcium nitrate.
Ca =1 atom
N=2 atoms
O =6 atoms
b. What type of bond is found in calcium nitrate?
Ionic bond
2+
Ca ion combined with NO314. Write the name of the following compounds:
a. Fe(NO3)3 _____________Iron (III) Nitrate________________________________
b. N2O5 __________________Dinitrogen Pentoxide_________________________
c. Ca(OH)2_________Calcium Hydroxide__________________
d. CoCl2 _________________Cobalt (II) Chloride_____________________________
e. SnBr4 __________________Tin (IV) Bromide_______________________________
f. CO _____________Carbon Dioxide_____________________
g. Al2(SO4)3 ______________Aluminum Sulfate____________________________
15. Write the formulas of the following compounds:
a) lithium chloride _________LiCl_____________________________
b) calcium nitrate _________Ca(NO3)2_________________________
c) iron (II) sulfate __________FeSO4___________________________
d) phosphorus pentabromide ____PBr5________________________
e) sodium fluoride _________NaF____________________________
f) copper (II) carbonate____CuCO3____________________________
g) calcium nitrate _________CaNO3__________________________
16. How do the properties of a compound compare to the properties of the elements
that make up that compound?
The properties of a compound are DIFFERERENT than the properties of the
elements that make it up.
17. How do the Properties of compounds made from the same elements, but in
different ratios, compare?
The properties are DIFFERERENT in compounds that are made of the same
element but in different ratios. Ex. water (H2O) and hydrogen peroxide (H2O2)
18. Can you predict the properties of a compound based on the properties of the
elements that it is composed of?
No, the properties of a compound are DIFFERERENT than the properties of the
elements that make it up.
19. What are the characteristics of a metallic bond?

•
•
•
•
•
•
•
•
Metal + Metal
In metals, valence electrons are shared, free to move about.
Good conductors of heat and electricity in all states.
Malleable solid
Strong bond, but weakest of the three bond types.
High melting point and boiling point.
Insoluble in H2O.
Insoluble in nonpolar solvents.
Lustrous
20. What are the characteristics of an ionic bond?










Metal + Nonmetal
One atom gains, one loses electrons.
Strong Bond but not as strong as a covalent bond.
Crystalline solid.
brittle
Very high melting point.
Soluble in H2O.
Insoluble in nonpolar solvents.
Nonconductor of heat and electricity in solid form.
Conducts electricity in aqueous solutions or when melted.
21. What are the characteristics of a covalent bond?









Nonmetal + Nonmetal
Formed by sharing electron pairs
Strongest bond type
Gas, liquid, or a soft solid at room temperature.
Low melting point and low boiling point.
Most are Insoluble in H2O
Soluble in nonpolar solvents.
Nonconductor of heat and electricity.
Nonlustrous
22. Name the type of bond that results from each:
a. Metal + Metal = _______Metallic Bond_____________
b. Nonmetal + Nonmetal = _Covalent Bond______________
c. Metal + Nonmetal = _____Ionic Bond_________________
23. What is electronegativity?
Electronegativity is the ability of an atom to attract electrons.
24. How does electronegativity affect a chemical bond?
•
If the difference in electronegativities is between:
–
1.7 to 4.0: Ionic
–
0.3 to 1.7: Polar Covalent
–
0.0 to 0.3: Non-Polar Covalent
25. Differentiate between an element, compound, molecule, and mixture (both
homogeneous and heterogeneous)
 An element is made from one type of atom.
 A compound is two or more different atoms bonded together. Must be at
least two different elements.
 A molecule is two or more atoms bonded together whether it is the same
element or different elements.
 A mixture contains two or more pure substances (elements and
compounds) and has variable composition. The substances are not
bonded and they retain their chemical properties.
o A homogeneous mixture is a substance in which two or more
substances are uniformly spread out.
o A heterogeneous mixture is a mixture that contains substances
that are not evenly mixed.
26. What causes a compound to be polar?
A polar molecule is an unequal sharing of electrons that result in a slight negative
charge on one side of the molecule and a slight positive charge on the opposite
side of the molecule.
27. What is an intermolecular force?
An intermolecular force is a force of attraction between different molecules rather
than bonding forces within the same molecule.
28. Describe the following:
a. Hydrogen Bond Bonding between hydrogen and more electronegative
neighboring atoms such as oxygen and nitrogen. IT IS NOT A BOND.
b. Dipole –Dipole force Attractive forces between polar molecules
c. Ion-Dipole force Attractive forces between an ion and a polar molecule
d. Ion induce dipole force Attractive forces that arise as a result of temporary
dipoles induced by an ion.
e. Dipole induced force Attractive forces that arise as a result of temporary
dipoles induced by a polar molecule.
29. Describe the propertied of water.
 Formula = H2O
 High specific heat
 State at Room Temperature = Liquid
 Melting Point = 0 oC
 Boiling Point = 100 oC
 Less Dense as a solid
 High surface tension
 Capillary action
 Essential to all living organisms
30. What is capillary action?
Capillary action results from the adhesive force between the molecules of liquid
and the side of the tube. This is how water moves through plants.
31. What is surface tension?
Surface tension is the tendency of liquids to keep a low surface area. It creates a
“skin” on the surface of the liquid. Water has a high surface tension.
32. What property of water makes it a universal solvent?
Water molecules are polar which allows for it to dissolve many compounds and
makes it the universal solvent.
33. Why is water essential to all living organisms?
 It is a major component in cells
 Water has many useful biological roles such as:
o being a solvent
o a coolant
o an insulator
o as support
o a lubricant
o a reagent.
 Water is used
o in chemical reactions
o for transporting
o providing a suitable environment
34. Diagram the following molecules. Tell the shape of the molecules, the type of
bond in each molecule, and if the molecule is polar or nonpolar. Show the
polarity of the bonds using this symbol
a. Water H2O
Molecular Geometry = Bent
Bond Type= Covalent
Polar Molecule
b. Methane CH4
Molecular Geometry = Tetrahedral
Bond Type= Covalent
Nonpolar Molecule
c. Ammonia NH3
Molecular Geometry = Trigonal Pyramid
Bond Type= Covalent
Polar Molecule