CHEMISTRY
Chemical Compounds Unit
Day 1: Objectives 6.1.1, 6.1.2, 6.1.3, 6.1.4
Before class: Read section 6-1
Answer the following. Complete sentences are not needed.
1. Define: a. chemical bond, b. ionic bonding, c. covalent bonding,
d. nonpolar-covalent bond, e. polar-covalent bond
After class:
Write the letter of the best answer.
1. A large difference in electronegativity between two atoms in a bond results in
a. polar covalent bonding
b. nonpolar covalent bonding
c. ionic bonding
d. repulsion between two atoms
2. Which of the following happens when atoms bond with each other?
a. The atoms increase in potential energy.
b. The potential energy of the compound is maximized.
c. Their electronegativity dramatically incrases.
d. They create arrangements of matter that are more stable.
Element
Electronegativity Element
Electronegativity
Hydrogen
2.1
Oxygen
3.5
Sodium
0.9
Carbon
2.5
Calcium
1.0
Cobalt
1.8
Lithium
1.0
Nitrogen
3.0
3. Use the electronegativity values above to classify the bonds that would form between
atoms of the following elements as ionic, polar-covalent, or nonpolar-covalent
a. H and O, b. H and C, c. Na and Co, d. Li and N, e. Ca and H,
f. N and O, g. Li and Ca, h. N and Ca, i. Na and O, C and O
Day 2: Objectives 6.2.1, 6.2.2
Before class: Read pages 164 – 170
Answer the following. Complete sentences are not needed.
1. Define: a. molecule, b. molecular compound, c. chemical formula,
d. molecular formula, e. diatomic molecule, f. bond length, g.
bond energy, h. octet rule, i. electron-dot notation
After class:
Write the letter of the best answer.
1. The molecular formula H2O indicates a molecule
a. with two atoms of oxygen bonded with one atom of hydrogen.
b. with two atoms of hydrogen bonded with one atom of oxygen.
c. that includes only ionic bonds.
d. that is diatomic.
CHEMISTRY
Chemical Compounds Unit
2. Which statement is true?
a. A molecule can exist only if two of the same type of atom are
bonded.
b. The strength of attraction between charged particles depends
only on the type of atom involved in the bond.
c. An atom of any element is a unit that can stand on its own.
d. The strength of attraction between charged particles depends on
the distance between the atoms involved in the bond.
3. Noble-gas atoms are able to exist independently in nature because
a. they are exceptions to the octet rule.
b. their bond energies are low compared to their bond lengths.
c. their electron configurations are more stable that those of other
atoms.
d. they share electrons in overlapping orbitals with other noble-gas
atoms.
4. Which statement is true?
a. As atoms are drawn together, the potential energy decreases.
b. Potential energy is at a maximum when attractive forces are
balanced by repulsive forces.
c. The composition of an element is given by its molecular formula.
d. Hydrogen is the only element that bonds to achieve noble-gas
configurations
5. Use Table 6-1 to create a graph comparing bond length to bond energy. Plot bond
length on the x-axis in units of pm and bond energy on the y-axis in unts of
kJ/mol. Remember to give your graph a title and label your axes.
6. What does your graph (from 8.) show about the relationship between bond length
and bond energy?
Day 3: Objectives 6.2.3, 6.2.4
Before class: Read pages 170 – 175
Answer the following. Complete sentences are not needed.
1. Define: a. unshared pair, b. Lewis structure, c. structural
formula, d. single bond, e. double bond, f. triple bond, g. multiple
bonds, h. resonance
CHEMISTRY
Chemical Compounds Unit
After class:
Write the letter of the best answer.
1. Which of the following statements is true?
e. A pair of dots in electron-dot notation always represents an
electron pair of a lone atom in a compound.
f. Only valence electrons of a particular atom are shown in
electron-dot notation.
g. A single bond is formed when a single electron brings two atoms
together.
h. Covalent bond formation involves the electrons closest to the
nuclei of the atoms.
2. Draw Lewis structures of each of the following:
a. CH4O, b. CH4, c. CS2, d. HCN, e. NH3, f. SOCl2 (S is the
central atom)
Day 4: Objectives 6.3.1,6.3.2, 6.3.3, 6.3.4
Before class: Read section 6-3
Answer the following. Complete sentences are not needed.
1. Define: a. ionic compound, b. formula unit, c. lattice energy, d.
polyatomic ion
After class:
Write the letter of the best answer.
1. Which of the following statements is true of molecular compounds?
a. When dissolved in water, they conduct electricity.
b. They are hard, brittle substances.
c. Their lattice energies are positive rather than negative.
d. Some are completely gaseous at room temperature.
2. Which statement is true of ionic compounds?
a. The distances between the ions vary throughout the crystal.
b. All ionic crystals have the same structure.
c. The ions cannot move in the solid state.
d. All ionic compounds are able to dissolve in water.
3. Which statement is true?
a. Calculating lattice energies helps chemists compare bond
strengths in ionic compounds.
b. Table salt is a molecular compound.
c. Na2Cl2 is a formula unit.
d. Ionic crystals for, so that the potential energy of a compound is
minimized.
CHEMISTRY
Chemical Compounds Unit
4. Which statement is true?
a. Molecular formulas represent the simplest formulas for
compounds.
b. The forces holding ions together in ionic bonds are relatively
weak.
c. Intermolecular attractions that hold molecules together are
stronger than ionic attraction.
d. A polyatomic ion with a shortage of electrons has a positive
charge.
5. Each of the following compounds is either ionic or molecular. Based on
the information given, write ionic if the compound is more likely to be
ionic or write molecular if it is more likely to be molecular
a. Compound A is a gas at room temperature.
b. Compound B breaks easily.
c. Compound C conducts electricity when dissolved in water.
d. Compound D has a value for lattice energy.
e. Compound E has a low melting point.
f. Compound F is not soluble in water.
g. The components of compound G are held together by electrical
attraction.
Day 5: Objectives 6.4.1, 6.4.2, 6.4.3
Before class: Read section 6-3
Answer the following. Complete sentences are not needed.
1. Define: a. metallic bonding, b. malleability, c. ductility
After class:
Write the letter of the best answer.
1. Why are metals able to conduct electricity?
a. The valence electrons that make up a metal are highly mobile.
b. Electrons are bound to individual ions that are held in place in
metallic crystal structures.
c. Metals are shiny and malleable.
d. The shortage of electrons in metals gives them a positive
electrical charge.
2. A blacksmith can shape metal into a horseshoe. This shows that the
metals is
a. ductile
b. a good conductor of electricity
c. malleable
d. a liquid at room temperature
CHEMISTRY
Chemical Compounds Unit
3. Create the Venn diagram to compare and contrast metals and ionic compounds.
In the overlapping area, note how the two substances are similar. In the
individual areas, list qualities pertaining only to that particular substance.
Ionic Compounds
Metals
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Day 6: Conductivity Lab
Day 7: Objectives 6.5.1, 6.5.2
Before class:
Read pages 183 - 187
Answer the following. Complete sentences are not needed.
1. Define: a. molecular polarity, b. VSEPR theory
After class:
Write the letter of the best answer.
1. Which is true of an AB4 molecule?
a. The electron pairs separate to form a tetrahedron.
b. The molecule contains hydrogen.
c. The molecule has ionic bonds.
d. The molecule has both single and double bonds.
2. A molecule with 2 atoms bonded to the central atom generally has
which shape?
a. linear
b. bent
c. trigonal planar
d. either a or b
3. Create a flow chart or an outline to show the steps in using VSEPR theory to
predict molecular geometry of a compound. Consider the use of Lewis structure
in valence electrons as you create your chart or outline.
4. Illustrate the steps in your chart or outline as you use VSEPR theory to predict the
molecular geometry of Cl2O.
Day 8: Objectives 6.5.3, 6.5.4, 6.5.5
Before class:
Read pages 187 – 193
Answer the following. Complete sentences are not needed.
1. Define: a. hybridization, b. hybrid orbitals, c. intermolecular
forces, d. dipole, e.dipole-dipole forces, f. hydrogen bonding, g.
London dispersion forces
CHEMISTRY
Chemical Compounds Unit
After class:
Write the letter of the best answer.
1. The higher the boiling point of a substance
a. the weaker the force between particles
b. the stronger the force between particles
c. the more likely it is the substance is nonpolar-covalent
d. the more likely it is that the substances is polar-covalent
2. In general, intermolecular forces are
a. stronger than bonds that join atoms in molecules
b. weaker than bonds that join atoms in molecules, but stronger
than ionic bonds
c. stronger than bonds that join metal atoms in solid metals
d. weaker than bonds that join atoms in molecules and ions in ionic
compounds
3. Which statement is true?
a. London forces explain the high boiling point of water.
b. Individual bond dipoles are contained only in ionic solutions.
c. Hydrogen bonding explains the high boiling point of ammonia.
d. Intermolecular forces are the forces of attraction between atoms
4. Hydrogen bonding is a special type of
a. sp3 orbital
b. London dispersion force
c. dipole-dipole force
d. molecular geometry
Complete the following sentences.
5. Hydrogen bonding is responsible for __________________ of water.
6. London forces are the only intermolecular forces that act
upon_____________________.
7. As atomic or molar masses increase, London forces _________________.
Answer the following using complete sentences.
8. How can a polar molecule induce a dipole in a nonpolar molecule?
9. In what direction does current in a dipole flow?
Days 9 and 10: Molecular Geometry Lab
Day 11: Objectives 7.1.1, 7.1.2, 7.1.3
Before class:
Read pages 203 - 211
Answer the following. Complete sentences are not needed.
1. Define: a. monatomic ions, b. binary compounds,
c. nomenclature, d. oxyanions
CHEMISTRY
Chemical Compounds Unit
After class:
Write the letter of the best answer.
1. Which statement is true?
a. All main-group elements are able to form ions
b. The total numbers of positive charges and negative charges
must be equal in a binary compound.
c. The nonmetals of groups 15, 16, and 17 lose electrons to form
cations.
d. Elements in the d block form ions of only one charge.
2. Why do many main-group elements lose or gain electrons to form ions?
a. The elements are unstable and therefore lose electrons.
b. Their tendency is to maximize potential energy.
c. The elements form covalent bonds, sharing their electrons with
other atoms.
d. Their tendency is to form a complete outermost octet in a noblegas configuration.
3. Which is the correct formula for a compound made of Sn2+ and NO3– ?
a. Sn2NO3
b. Sn(NO3)2
c. Sn3NO2
d. 2Sn3NO
4. Which is the correct formula for silver chloride?
a. Ag+Cl–
b. 2Ag2Cl
c. AgClO
d. AgCl
Answer the following using complete sentences.
5. Explain what each chemical formula tells you about the composition of
the compound. The first one has been done for you.
a. NaNO3 The subscript 3 refers to the number of oxygen atoms.
There are one atom of sodium and one atom of nitrogen for every
three atoms of oxygen.
b. AgCl
c. Ba(OH)2
d. (NH4)2SO4
Matching
6. Br – ________
a. nitrate
–
___________
7. OH
b. chlorite
–
8. NO2 _______
c. hydroxide
9. NO3 – _______
d. bromide
–
10. O2 ________
e. nitrite
11. CN – _______
f. ammonium
–
12. ClO2 ______
g. oxide
+
13. NH4 _______
h. cyanide
CHEMISTRY
Chemical Compounds Unit
14. Copy and complete the chart by supplying the missing information
Name of Compound or Ion
Formula of compound or ion
Copper (II) ion
NH4+
Bismuth (III) bromide
Tin(II) fluoride
MgF2
Iron (III) cyanide
S2 –
Potassium permanganate
Day 12: Objectives 7.1.2, 7.1.3, 7.1.4, 7.1.5
Before class:
Read pages 211 - 215
Answer the following. Complete sentences are not needed.
1. Write the name, formula, and charge for each of the following:
a. acetate, b. ammonium, c. chlorate, d. chlorite, e. hydroxide,
f. hypochlorite, g. nitrate, h. nitrite, i. perchlorate,
j. permanganate, k. carbonate, l. peroxide, m. sulfate,
n. sulfite, m. phosphate
After class:
Write the letter of the best answer.
1. Which is the correct formula for phosphorus pentafluoride?
a. P5F
b. PFl5
c. PF5
d. PF
2. NaF6 is the formula for which compound?
a. sodium hexafluoride
b. sodium pentafluoride
c. hexafluoride sodium
d. hexasodium fluoride
3. Which of the following is the formula for silicon dioxide?
a. S2O
b. Si2O
c. SO2
d. SiO2
4. H2SO3 is the formula for what compound?
a. sulfuric acid
b. sulfurous acid
c. dihydrous sulfuric acid
d. hydrosulfuric acid
CHEMISTRY
Chemical Compounds Unit
15. Copy and complete the charts by supplying the missing information.
Try not to use your book.
Number
1
2
3
4
5
6
7
8
9
10
Prefix
Name of Compound
Formula of Compound
CO2
Nitrogen dioxide
S2Cl2
Carbon Tetrachloride
P4O7
SF6
Ice
Diphosphorus pentoxide
Day 13: Chemistry Bingo
Day 14: Objectives 7.2.1, 7.2.2, 7.2.3
Before class:
Read section 7 – 2
Answer the following. Complete sentences are not needed.
2. Define: a. oxidation numbers
After class:
Write the letter of the best answer.
1. What are the oxidation numbers for the atoms in AlCl3
a. +3, -1
b. +3, +1
c. -3, -1
d. -3, +1
CHEMISTRY
Chemical Compounds Unit
2. In a ClO4 – ion, what is the oxidation number of Cl?
a. +4
b. -4
c. +5
d. +7
3. What is the Stock system name of SO2?
a. sulfur dioxide
b. sulfur trioxide
c. sulfur(IV) oxide
d. sulfur(II) oxide
4. HNO2 is the formula for which compound?
a. huydrogen nitrogen dioxide
b. nitrogen(II) dioxide
c. nitrous acid
d. ammonium(II) oxide
16. Copy and complete the chart by supplying the missing information
Stock system name
ChemicalFormula Prefix system name
Carbon(IV) iodide
Sulfur(VI) oxide
Arsenic(III) sulfide
Nitrogen(III) chloride
Phosphorus (V) chloride
Water
Lead(IV) oxide
Nitrogen(I) chloride
Day 15: Objective 7.3.1
Before class:
Read pages 221 – 224
Answer the following. Complete sentences are not needed.
1. Define: a. formula mass, b. molar mass
After class:
Write the letter of the best answer.
1. In the compound Al2(SO4)3 there are
a. 2 mol Al, 3 mol S, 12 mol O
b. 2 mol Al, 4 mol S, 4 mol O
c. 6 mol Al, 3 mol S, 12 mol O
d. 2 mol Al, 3 mol S, 7 mol O
CHEMISTRY
Chemical Compounds Unit
Complete the charts by supplying the missing information
Compound
Number of moles of atoms of each element
in one mole of the compound
CO2
1 mol C, 2 mol O
AlCl3
Cu2O
Ba(SCN)2
LiH
H2SO4
Compound
CO2
SnI4
NaH2PO4
Hg2Cl2
Ca(C2H3O2)2
molar mass
Day 16: Objective 7.3.2, 7.3.3, 7.3.4
Before class:
Read pages 224 – 228
Answer the following. Complete sentences are not needed.
3. Define: a. percentage composition
1. Example: What is the mass in grams of 3.04 mol of ammonia vapor, NH3?
2. You try: what is the mass in grams of 0.257 mol of calcium nitrate, Ca(NO3)2?
3. Example: how many moles of SO2 are in 3.82 g?
4. You try: how many moles of Cl2 are there in 77.1 g?
5. Example: How many molecules are there in 77.1 g of Cl2?
6. You try: How many molecules are in 4.15 x 10-3 g of C6H12O6?
7. Example: Find the percentage composition of sodium nitrate, NaNO3.
8. You try: find the percentage composition of silver sulfate, Ag2SO4.
After class:
Write the letter of the best answer.
1. How many moles of H2O are in 24.0 g?
a. 144.48 x 1023
b. 432.38
c. 1.41
d. 1.33
2. What is the total mass of oxygen in 146.7 g of Hg2SO4?
a. 0.30 g
b. 19.19 g
c. 497.21 g
d. 1.807 x 1023 g
CHEMISTRY
Chemical Compounds Unit
3. What is the percentage composition of N2O5?
a. 20% N, 50% O
b. 28.02% N, 80.0 % O
c. 25.9% N, 74.1% O
d. none of the above
4. What is the percentage of potassium in 14.8 g of KOH?
a. 69.7%
b. 28.5%
c. 1.78%
d. 56.1%
5. Solve each problem below. Show your work.
a. What is the mass in grams of 9.03 moles of H2S?
b. Find the percentage composition of KCl
c. Calculate the percentage of nitrogen in 84.65 g of ammonium nitrate, NH4NO3.
Day 17: Objectives 7.4.1, 7.4.2
Before class:
Read pages 229 – 231
Answer the following. Complete sentences are not needed.
1. Define: a. empirical formula
Example: A compound is analyzed and found to contain 36.70% potassium, 33.27% chlorine, and
30.03% oxygen. What is the empirical formula of the compound?
You try: Determine the empirical formula of the compound that contains 17.15% carbon, 1.44%
hydrogen, and 81.41% fluorine.
Example: A 60.0 g sample of tetraethylead, a gasoline additive, is found to contain 38.43 g lead, 17.83
g carbon, and 3.74 g hydrogen. Find its empirical formula.
You try: A 170.00 g sample of an unidentified compound contains 29.84 g sodium, 67.49 g chromium,
and 7.67 g oxygen. What is its empirical formula?
Discuss: Find the empirical formula of a compound that contains 53.70% iron and 46.30% sulfur.
After class:
Write the letter of the best answer.
Which statement is true?
a. The empirical formula and molecular formula for a given compound are always
the same.
b. The molecular formula of a substance tells how the atoms in the molecule are
connected.
c. The molecular formula gives the actual number and types of atoms in the
molecule.
d. The percent composition of a compound and the molecular weight are not
sufficient information to determine the molecular formula.
Solve each problem below. Show your work.
What is the empirical formula of a compound that is 51.4% Cu, 38.8% O, and 9.7% C?
What is the mass in grams of 0.257 mol of sucrose, C12H22O11?
Calculate the percent composition of the compound C2H4O2.
Day 18: Objectives 7.4.3, 7.4.4
Before class:
CHEMISTRY
Chemical Compounds Unit
Read pages 232 – 233
Answer the following. Complete sentences are not needed.
1. Define: a. molecular formula
1. Example: The empirical formula for trichloroisocyanuric acid is OCNCl. The molar mass of this
compound is 232.41 g/mol. What is its molecular formula?
2. Example: Determine the molecular formula of a compound with an empirical formula of NH2 and
a formula mass of 32.06 amu.
3. You try: Determine the molecular formula of the compound with an empirical formula of CH and a
formula mass of 78.110 amu.
4. Example: If 4.04 g of N combine with 11.46 g of O to produce a compound with a formula mass of
108.0 amu, what is the molecular formula of this compound?
5. You try: The molar mass of a compound is 92 g/mol. Analysis of a sample of the compound
indicates that it contains 0.606 g N and 1.390 g O. Find its molecular formula.
After class:
1. Solve each problem below. Show your work.
a. The molar mass of NaSO2 is 174 g/mol. What is the molecular formula of the
compound?
b. What is the molecular formula of a substance with a molar mass of 28.0 g/mol
and an empirical formula of CH2?
c. What is the molecular formula of a substance with a molar mass of 216 g/mol
and an empirical formula of C3H2O?
d. What is the molecular formula of a substance with a molar mass of 116.07
g/mol that is 41.39% carbon, 3.47% hydrogen, and 55.14% oxygen?
e. What is the molecular formula of a substance with a molar mass of 168.19
g/mol that is 64.27% carbon, 7.19% hydrogen, and 28.54% oxygen?
Day 19: Objectives 7.4.2, 7.4.3
Before class:
Read the lab on pages 813 – 815. We will be skipping procedure #12.
Day 20: All Objectives
During class:
The following questions are suggested for study. They are not graded. They are not required. I
recommend reading through them, and working through the ones that don’t seem obvious to you.
Chapter 6 review 2, 6, 9, 15, 16, 22, 24, 27, 29 – 32, 48
Chapter 7 review 2, 4 – 7, 9 – 11, 17, 18, 20 – 23, 26, 33, 34, 36, 38, 39