1. Chapter 16 – Review “Covalent Bonding”
Milbank High School

2. Chapter 16 - Review
How many electrons are shared in a single covalent bond?
How many valence electrons does an atom of any halogen have?
How many electrons are shared in a double covalent bond?
How many electrons does a nitrogen atom need to gain to attain a noble-gas electron configuration?

3. Chapter 16 - Review
How many unshared pairs of electrons does the nitrogen atom in ammonia (NH3) possess?
How many electrons does carbon need to gain to obtain a noble-gas electron configuration?
What is the total number of covalent bonds normally associated with a single carbon atom in a compound?

4. Chapter 16 - Review
How many unshared pairs of electrons are there in a molecule of hydrogen iodide?
How many covalent bonds are there in a covalently bonded molecule containing 1 phosphorus atom and 3 chlorine atoms?
What is the name given to the energy required to break a single bond?

5. Chapter 16 - Review
How do atoms achieve noble-gas electron configurations in single covalent bonds?
Why do atoms share electrons in covalent bonds?
What is shown by the structural formula of a molecule or polyatomic ion?

6. Chapter 16 - Review
What is the name given to the pairs of valence electrons that do not participate in bonding in diatomic oxygen molecules?
Which elements can form diatomic molecules joined by a single covalent bond?
Which of these elements does not exist as a diatomic molecule: I, Ne, H, F

7. Chapter 16 - Review
What elements can form diatomic molecules held together by triple covalent bonds?
What elements can form diatomic molecules held together by double covalent bonds?
A covalent bond in which each atom contributes two electrons is a ___.

8. Chapter 16 - Review
A diatomic molecule with a triple covalent bond is _____.
A molecule with a single covalent bond is: CO2 or Cl2?
Which noble gas has the same electron configuration as the oxygen in a water molecule?

9. Chapter 16 - Review
What diatomic molecule is joined by a double covalent bond?
When one atom contributes both bonding electrons in a single covalent bond, the bond is called a(n) _______.
Once formed, how are coordinate covalent bonds different from normally formed covalent bonds?

10. Chapter 16 - Review
What is true concerning the resonant molecule dinitrogen tetraoxide (or any resonant structure for that matter!)?
When do exceptions to the octet rule occur?
Substances in which all of the electrons are paired are said to be ______.

11. Chapter 16 - Review
How many unpaired electrons are present in each molecule of a para-magnetic substance?
Which of the following types of magnetism is the strongest: paramagnetic; diamagnetic; or ferromagnetic?
Which of the following fails to follow the octet rule: fluorine or oxygen?

12. Chapter 16 - Review
In which of the following compounds is the octet expanded to include 12 electrons: SO3 or SCl6?
What is one way in which compounds that do not follow the octet rule can achieve stability?
Which of the following pairs of elements can be joined by a covalent bond: Mg and C; or N and C?

13. Chapter 16 - Review
What type of covalent bond is most stable between small atoms: polar or nonpolar?
According to VSEPR theory, molecules adjust their shapes to keep what items as far apart as possible?

14. Chapter 16 - Review
What causes water molecules to have a bent shape, according to VSEPR theory?
What is the measure of the tetrahedral bond angle?
What is the bond angle in a water molecule?
What is thought to cause the dispersion forces?

15. Chapter 16 - Review
Which of the forces of molecular attraction is the weakest?
What causes hydrogen-bonding?
Why is hydrogen-bonding only possible with hydrogen?