Unit 3 Study Guide – Bonding & Nomenclature
At the conclusion of this unit you will be able to…

Name and write formulas for ionic & covalent compounds, acids, and hydrates

Explain the octet rule

Explain what valence electrons are

Explain how ionic, covalent, and metallic bonds form

Explain the properties of ionic, covalent, and metallic bonds

Predict if a bond will be ionic, covalent, or metallic

Use electronegativities to predict if a bond will be ionic, polar covalent, or non-polar covalent

Draw Lewis Structures for elements

Draw Lewis Structures for ionic and covalent compounds

Identify the correct Lewis Structures of elements and compounds

Predict how many covalent bonds an atom can form, based on its Lewis Structure

Predict the number of bonding pairs of electrons and lone pairs of electrons there are in a molecule, and
specifically around the central atom

Determine the number electrons being shared in single, double, and triple bonds

Use VSEPR theory to predict the shape of a molecule
 Use VSEPR theory to predict the bond angles in a molecule. Define and give examples of the following
terms.
Perform the following calculations. Work must be shown in the format done in class (dimensional analysis).
1. Convert 30.2 g of copper to liters. (hint: use density)
2.
Convert 0.789 hL acetone (density = 0.791 g/mL) to pounds.
Answer the following questions:
3.
What is the charge (and the name for the copper ion) on the copper ion is in: Cu 2CO3
4.
What does the Roman numeral in the name Iron (III) phosphate stands for?
5. How can you tell if atoms have the same number of valence electrons?
6.
How many valence electrons does Oxygen have?
7.
How many electrons does an atom generally need in its outer level to be the most stable?
8.
What are the electrons in an atom’s outermost orbitals are called?
9.
Which atoms are most likely to form a 1- ion?
10. Sarah just bought herself a long silver chain. Interested to know how much silver she just bought she
massed the chain and found it to be 5.0g. If the density of silver is 10.5g/cm3, what is the volume of
Sarah’s new chain?
11. What is the charge of phosphate in K3PO4?
12. What does density converts to/from:
13. What are the correct formulas for the following compounds?
a. Barium sulfate
f.
Lead (II) ions bonded to chromate ions
b.
Aluminum bromide
g.
Barium hydroxide tetrahydrate
c.
Ammonium nitrate
h.
Sulfuric acid
d.
Copper (II) acetate
i.
Hydrochloric acid
e.
Magnesium nitrate
j.
Dicarbon pentahydride
14. What are the correct names for the following formulas?
o CO2
o
K2SO4
o
Fe3(PO4)2
o
HNO3
o
Cu2SO4
o
SF6
15. Describe the behavior of electrons using words/and or pictures for each of the following types of bonds:
a. Ionic Bond
c. Metallic Bond
b. Polar Covalent Bond
d. Non-Polar Covalent Bond
16. Draw the Lewis Structure for the following compounds, indicate whether these compounds are ionic or
covalent
N 2H 4
C2Cl4
N2
C2H2
17. A double bond, such as the one in O2 , O=O, consists of how many total electrons?
18. The chemical NH3 has what shape and bond angle?
19. Given boron’s electron configuration of [He]2s22p1, draw its electron-dot structure.
20. A chemical bond that occurs when atoms share electrons is a(n) ____ bond.
21. A group of covalently bonded atoms that acts together as one charged particle is a __________________.
22. Which atom is most likely to form a 1- ion?
a. I
b. S
c. Ag
d.
e.
P
Na
23. Which combination of elements would be expected to produce the most polar covalent bond?
a. O-O
c. O-Cl
b. O-N
d. O-H
24. There are __________bonding pairs and ___________lone pairs around “P” in PH3.
25.
If sodium reacts with a certain element “X” to form the compound NaX, than what would the formula
be for a compound formed between beryllium and this element, X?