1. Chapter 8 Review “Covalent Bonding”

2. Chapter 8 Review
What is the correct electron configuration arrangement of the four valence electrons of the carbon atom in a methane molecule (CH4): a) 2s22p2, or b) 2s12p3?
Which noble gas has the same electron configuration as the oxygen in a water molecule?

3. Chapter 8 Review
When placed between oppositely charged metal plates, the region of a water molecule attracted to the negative plate is the ____.
When one atom contributes both bonding electrons in a single covalent bond, the bond is called a(n) ____.

4. Chapter 8 Review
The shape of the methane molecule (CH4) is called ____. What are the bond angles?
How is a pair of molecular orbitals formed?
Which elements can form diatomic molecules joined by a single covalent bond?
What is a typical characteristic of an ionic compound? Covalent?

5. Chapter 8 Review
Experimental evidence suggests that the H-C-H bond angles in ethene, C2H4, are ____ degrees.
A bond that is not symmetrical along the axis between two atomic nuclei is a(n) ____ bond.
Once formed, how are coordinate covalent bonds different from other covalent bonds?
120

6. Substances that show relatively strong attractions to an external magnetic field are said to be ____________?
Oxygen is an example of a substance that is ____________?

7. Chapter 8 Review What causes hydrogen bonding?
How many electrons can occupy a single molecular orbital?
According to the VSEPR theory, molecules adjust their shapes to keep ____ as far apart as possible.
Which of the following atoms acquires the most negative charge in a covalent bond with hydrogen: a) carbon, or b) oxygen?

8. Chapter 8 Review
How do atoms achieve noble-gas electron configurations in single covalent bonds?
What is required in order to melt a network solid?
Molecular orbital theory is based upon what model of the atom?
Where are the electrons most probably located in a molecular bonding orbital?

9. Chapter 8 Review
A molecule with a single covalent bond is: a) CO2, or b) Cl2?
A bond formed between a silicon atom and an oxygen atom is likely to be a(n) ____ bond.
Which of the following diatomic molecules is joined (seemingly) by a double covalent bond: a) O2, or b) N2?

10. Chapter 8 Review
What causes water molecules to have a bent shape, according to the VSEPR theory?
Which of these elements does not exist as a diatomic molecule: a) Ne, or b) F?
Which of the following elements can form diatomic molecules held together by triple covalent bonds: a) fluorine, or b) nitrogen?

11. Chapter 8 Review
Which of the following covalent bonds is the most polar: a) H-F, or b) H-N?
What is shown by the structural formula of a molecule or a polyatomic ion?
What is thought to cause the disperson forces?

12. Chapter 8 Review
What are the weakest attractions between molecules called?
Which type of solid has the highest melting point: a) ionic solids, or b) network solids?
Why do atoms share electrons in covalent bonds?

13. Chapter 8 Review
How many valid electron dot formulas – having the same number of electron pairs for a molecule or ion – can be written when a resonance structure occurs?

14. Chapter 8 Review
Which of the forces of molecular attraction is the weakest: a) hydrogen bonding, or b) dispersion forces?
In which of the following compounds is the octet expanded to include 12 electrons: a) PCl5, or b) SF6?
Why is hydrogen bonding only possible with hydrogen?

15. Chapter 8 Review What causes dipole interactions?
How many electrons does carbon need to gain in order to obtain a noble-gas electron configuration?
How many covalent bonds are in a covalently bonded molecule containing 1 phosphorus atom and 3 chlorine atoms?

16. Chapter 8 Review
How many electrons does a nitrogen atom need to gain in order to attain a noble-gas electron configuration?
What is the bond angle in a water molecule?
How many unshared pairs of electrons are in a molecule of hydrogen iodide?

17. Chapter 8 Review
How many electrons are shared in a single covalent bond?
What is the total number of covalent bonds normally associated with a single carbon atom in a compound?
How many valence electrons does an iodine atom have?
How many unshared pairs of electrons does the nitrogen atom in ammonia possess?

18. Chapter 8 Review
How many electrons are shared in a double covalent bond?
Know the shape/bond angles of the following: CO2, H2O, CCl4, NH3, SO3, PF5, SF6
End of Chapter 8 Review