Download Chapter 20 Resource: Chemical Bonds

Glencoe Science
Chapter Resources
Chemical Bonds
Includes:
Reproducible Student Pages
ASSESSMENT
TRANSPARENCY ACTIVITIES
✔ Chapter Tests
✔ Section Focus Transparency Activities
✔ Chapter Review
✔ Teaching Transparency Activity
✔ Assessment Transparency Activity
HANDS-ON ACTIVITIES
✔ Lab Worksheets for each Student Edition Activity
Teacher Support and Planning
✔ Laboratory Activities
✔ Content Outline for Teaching
✔ Foldables–Reading and Study Skills activity sheet
✔ Spanish Resources
✔ Teacher Guide and Answers
MEETING INDIVIDUAL NEEDS
✔ Directed Reading for Content Mastery
✔ Directed Reading for Content Mastery in Spanish
✔ Reinforcement
✔ Enrichment
✔ Note-taking Worksheets
Name
Date
Directed Reading for
Content Mastery
Class
Overview
Chemical Bonds
Directions: All of the statements below are false as written. In the space provided, write a term or phrase that
makes the statement true when it is substituted for the underlined words.
1. The properties of a compound are the same as the properties
of the elements that it contains.
Meeting Individual Needs
2. Superscript numbers in chemical formulas tell how many
atoms of each element are found in a unit of compound.
3. All the noble gases except helium have 18 electrons in
their outer energy level.
4. A(n) chemical formula is the force that holds atoms
together in a compound.
5. An ion is a(n) neutral particle that has either more or
fewer electrons than protons.
6. Oxidation numbers are written as subscripts.
Copyright © Glencoe/McGraw-Hill, a division of the McGraw-Hill Companies, Inc.
7. A(n) covalent bond is the force of attraction between the
opposite charges of the ions in an ionic compound.
8. The charge on a compound is always positive.
9. Equal sharing of electrons in covalent bonds results in
polar molecules.
10. Only two identical atoms can share electrons unequally.
11. A binary compound contains five different elements.
12. An oxidation number tells how many protons an atom
must gain, lose, or share to become stable.
13. The oxidation number of the copper(II) ion is 3+.
14. When writing chemical formulas, add superscripts so that
the sum of the oxidation numbers equals ten.
15. A polyatomic ion never has a positive or negative charge.
16. The polyatomic ion SO42 is called the sulfide ion.
Chemical Bonds
19
Name
Date
Directed Reading for
Content Mastery
Class
Section 1 Stability in Bonding
Section 2 Types of Bonds
■
■
Directions: In the blanks, write the terms from the word list that complete the definition. Words can be used
more than once.
positive
energy level(s)
force(s)
atom(s)
element(s)
charged
ion(s)
compound(s)
number(s)
electron(s)
negative
____________________ and the exact ____________________ of atoms of
each element in a unit of compound.
2. An atom is chemically stable when its outer ____________________ is
completely filled with ____________________.
3. A chemical bond is a ____________________ that holds ____________________
together in a compound.
4. An ____________________ that has lost or gained ____________________ is
called an ion.
5. An ionic bond is the ____________________ of attraction between the opposite
charges of the ____________________ in an ionic ____________________.
6. The attraction that forms between ____________________ when they share
____________________ is known as a covalent bond.
7. A polar molecule has a slightly ____________________ end and a slightly
____________________ end.
8. A nonpolar molecule does not have oppositely ____________________ ends.
Only atoms that are exactly alike can share their ____________________ equally.
20 Chemical Bonds
Copyright © Glencoe/McGraw-Hill, a division of the McGraw-Hill Companies, Inc.
Meeting Individual Needs
1. A chemical formula tells what ____________________ make up a
Name
Date
Directed Reading for
Content Mastery
Section 3
Class
■
Writing Formulas
and Naming
Compounds
Meeting Individual Needs
Directions: The words in each group below are related. Using all the words in the group, write a sentence that
shows how the words are related.
Example: compound, properties, elements
The properties of a compound differ from the properties of the elements that make up the compound.
1. hydrate, compound, water
2. oxidation number, element, electrons
3. zero, oxidation numbers, noble gases
Copyright © Glencoe/McGraw-Hill, a division of the McGraw-Hill Companies, Inc.
4. oxidation number, Roman numeral, element
5. chemical formulas, neutral, compounds
6. polyatomic, covalent, charged
7. Greek prefixes, binary covalent compounds
8. charge, oxidation number, ionic compounds
Chemical Bonds
21
Name
Date
Directed Reading for
Content Mastery
Class
Key Terms
Chemical Bonds
Directions: Match each term in Column I with its description in Column II. Write the letter of the correct term in
the space provided.
1. binary compound
2. chemically stable
Meeting Individual Needs
3. nonpolar molecule
4. ion
5. ionic bond
6. polar molecule
Column II
a. number that indicates how many electrons
an atom must gain, lose, or share to
become stable
b. shorthand that tells what elements a
compound contains and the exact number
of atoms of each element in a unit of the
compound
7. oxidation number
c. positively or negatively charged, covalently
bonded group of atoms
8. chemical formula
d. compound composed of two elements
9. covalent bond
e. describes an atom that has a full outermost
energy level
10. hydrate
11. chemical bond
12. polyatomic ion
f. molecule that has a slightly positive end
and a slightly negative end
g. the attraction that forms between atoms
when they share electrons
h. the force that holds atoms together in a
compound
i. a compound that has water chemically
attached to it
j. the force of attraction between the opposite
charges of the ions in an ionic compound
k. molecule made of two identical atoms that
share the electrons equally
l. a charged particle that has either more or
fewer electrons than protons
22 Chemical Bonds
Copyright © Glencoe/McGraw-Hill, a division of the McGraw-Hill Companies, Inc.
Column I
Name
Date
1
Reinforcement
Class
Stability in Bonding
Directions: Each statement below contains a pair of terms or phrases in parentheses. Circle the term or phrase
that makes each statement true.
1. The properties of a compound are (the same as, different from) the properties of the elements
that make up the compound.
2. Na and Cl are chemical (symbols, formulas).
4. In the formula H2O, the number 2 is a (subscript, superscript).
5. The number 2 in the formula H2O tells you that each unit of this compound contains two
(hydrogen, oxygen) atoms.
6. If a symbol in a chemical formula does not have a subscript after it, a unit of that compound
contains (no atoms, one atom) of that element.
7. The total number of atoms in Fe2O3 is (two, five, six).
8. There are (three, seven, ten) different elements in H2SO4.
9. An atom is chemically stable if its outer energy level (is filled with, contains no) electrons.
Copyright © Glencoe/McGraw-Hill, a division of the McGraw-Hill Companies, Inc.
10. For atoms of most noble gases and most other elements, the outer energy level is full when it
has (3, 8) electrons.
11. The noble gases do not readily form compounds because they (are, are not) chemically stable.
12. A chemical bond is a (force, chemical) that holds atoms together in a compound.
13. Chemical bonds form when atoms lose, gain, or (share, multiply) electrons.
Directions: Complete the table below by using the formula of each compound to identify the elements that
each compound contains and the number of atoms of each of these elements in a unit of the compound. The first
formula has been done for you.
Formula
Element 1
Element 2
HO
2 hydrogen
1 oxygen
2
14.
NaOH
15.
NaCl
16.
NH
17.
H SO
18.
SiO
Element 3
3
2
4
2
Chemical Bonds
27
Meeting Individual Needs
3. NaCl and NaOH are chemical (symbols, formulas).
Name
2
Date
Reinforcement
Class
Types of Bonds
Directions: Study the diagram below. Write your answers to the questions in the spaces provided.
A.
B.
12P
12N
8P
8N
b. how many electrons will atom B gain?
c. what will be the oxidation number of atom A?
d. what will be the oxidation number of atom B?
e. what will be the total charge of the compound formed?
f. what type of bond will form?
2. Explain why an element’s oxidation number is related to the group on the periodic table to
which it belongs.
Directions: Complete the table comparing ionic compounds and covalent compounds.
Characteristic
3. How the compound is formed
4. Smallest particle
5. Usual state at room temperature
28 Chemical Bonds
Ionic compounds
Covalent compounds
Copyright © Glencoe/McGraw-Hill, a division of the McGraw-Hill Companies, Inc.
Meeting Individual Needs
1. If atom A loses electrons to atom B,
a. how many electrons will atom A lose?
Name
3
Date
Class
Writing Formulas and Naming
Compounds
Reinforcement
Directions: Answer the following questions in the spaces provided. Refer to the periodic table for help.
1. Define an oxidation number.
2. What is the usual oxidation number of oxygen? Of hydrogen?
4. Explain the difference between CoCl2 • 6H2O and anhydrous cobalt chloride.
Directions: Use the periodic table in your textbook to identify the oxidation numbers of the elements in each group.
Group
Oxidation number
1
2
5.
6.
16
7.
17
8.
18
9.
Directions: Write the formulas for the following compounds. Use the periodic table in your textbook for help.
10. copper(II) sulfate
Copyright © Glencoe/McGraw-Hill, a division of the McGraw-Hill Companies, Inc.
11. calcium chloride
12. iron(II) oxide
13. copper(I) oxide
14. sodium sulfide
15. magnesium sulfate heptahydrate
Directions: Complete the following table by providing the name of the compound and the total number of
atoms in each formula given.
Formula
Name
Number of Atoms
16. NH4OH
17. NH4C1
18. Ag2O
19. K2SO4
20. Ca (NO3)2
21. Na2S
Chemical Bonds
29
Meeting Individual Needs
3. What is the sum of all the oxidation numbers in any compound?
Name
1
Date
Enrichment
Class
Electron Dot Diagrams
The electrons in an atom’s outer energy level are the electrons that are important to consider in
chemical bonds and chemical reactions. These electrons can be represented in a diagram called an
electron dot diagram. The outermost electrons are drawn as dots around the chemical symbol.
In this activity, you will draw electron dot diagrams for several elements.
Procedure
Example: The symbol for chlorine is Cl. In an electron
dot diagram, this symbol represents the nucleus and
the ten electrons in the first two energy levels.
2. Use the periodic table to determine how
many outer electrons the element has.
Do this by finding to which group the
element belongs.
3. Draw a dot to represent each electron
in the outer level of the element. Two
electrons can be placed on each side of the
symbol. The first two electrons should be
paired on the right side of the symbol.
The rest of the outer electrons should be
distributed counterclockwise one by one
around the other sides of the symbol.
Example: The electron dot diagram for chlorine is
Cl
Example: Chlorine belongs to Group 17, the
halogens, which have seven outer electrons.
Conclude and Apply
1. Write electron dot diagrams for the elements listed.
a. hydrogen
e. aluminum
b. neon
f. fluorine
c. sodium
g. argon
d. calcium
h. potassium
2. Why do sodium and potassium have the same number of dots in their electron dot diagrams?
What does this tell you about the chemistry of these two elements?
30 Chemical Bonds
Copyright © Glencoe/McGraw-Hill, a division of the McGraw-Hill Companies, Inc.
Meeting Individual Needs
1. Write the symbol for the element. For electron
dot diagrams, this symbol represents the
nucleus and all of the electrons of the atom
except the outermost electrons.
Name
Enrichment
Class
Paper Chromatography
Paper chromatography uses polarity to separate substances from a solution. The polarity of a substance affects how fast a particular substance dissolved in a particular solvent can move along paper.
Because the rates of movement are very specific, chromatography can also be used to identify substances.
In paper chromatography, a small sample of a solution is placed on absorbent paper. A solvent
passes through the sample and carries the dissolved substances. The various substances in the
solution move outward at different rates.
The procedure described below demonstrates how components of a mixture can be separated.
If a procedure is set up in a way that can identify how far the solvent travels and how far the dissolved substance travels, these distances can be measured and compared. The number obtained by
dividing the distance the dissolved substance traveled by the distance the solvent traveled is known
as R f. If specifics of the procedure such as temperature, solvent, and type of paper are controlled,
the R f values can be used to identify the substances in a solution.
Paper chromatography and other types of chromatography have many uses. An environmental
chemist might use chromatography to identify pollutants in water, or a medical chemist to identify poison or medicines in the blood of a patient.
Copyright © Glencoe/McGraw-Hill, a division of the McGraw-Hill Companies, Inc.
Materials
Pipe cleaner
petri dish
yellow food coloring
ink
round filter paper
metric ruler
pipe cleaner
toothpick
solvent (water, rubbing alcohol, or ethanol)
WARNING: Alcohol and ethanol are flammable.
Food coloring
Procedure
Solvent
1. Add a small amount of solvent to a petri dish.
2. Use a toothpick to place a small drop of food
coloring at the center of the filter paper.
3. Punch a small hole in the center of the filter
paper with the toothpick. Place the pipe
cleaner through this hole.
4. Carefully place the filter paper on top of
the petri dish so that the end of the pipe
cleaner touches the solvent. Observe what
Filter paper
Petri dish
happens as the solvent moves up the pipe
cleaner and across the filter paper
5. When the solvent has finished moving,
remove the filter paper from the dish.
Allow the filter paper to dry.
6. Repeat steps 2 through 5, using ink instead
of food coloring. Use a new pipe cleaner
and filter paper.
Conclude and Apply
1. Why do different bands of color appear on different areas of the filter paper?
2. A student used felt-tip markers to make labels for one of his collections. When water splashed
on the labels, the colors began to run and smear. Use your observations from this activity to
explain what happened to the writing.
3. When paper chromatography is used as an analytical tool, the solute and solvent must move
only in one direction. Explain why this controlled direction is necessary to calculate the R f.
Chemical Bonds
31
Meeting Individual Needs
2
Date
Name
Date
Enrichment
The Crisscross Method
Meeting Individual Needs
The process of writing chemical formulas can
be made easier by using oxidation numbers.
Remember that the total charge on a
compound must be zero. Remember also that
oxidation numbers describe the number of
electrons an atom or ion gains or loses when
forming compounds. Atoms in the same
group on the periodic table usually will have
the same oxidation number. Use the periodic
table to determine the oxidation numbers of
atoms. Refer to your textbook for oxidation
numbers of polyatomic ions.
Example: Write the formula for barium chloride.
Step 1: Determine the oxidation numbers for
the two elements or ions. Because barium is in
Group 2, its oxidation number is 2+. Elements
in Group 2 tend to lose the two electrons in
the outer energy level, leaving the ions with
positive charges. Chloride is in Group 17, so
its oxidation number is 1–. Elements in Group
17 have seven electrons in the outer energy
level and tend to gain one electron. The ions
are negative.
Step 2: Write the chemical symbols in the
correct order, with the metal ion first.
Ba
Cl
Now, write the oxidation numbers as
superscripts. For an ion with an oxidation
number of 1+ or 1–, write only the sign and
not the number.
Ba2 Cl
Next, crisscross the numbers only—not the
signs this time, writing the oxidation number
of one element as the subscript for the other.
Don’t write the number 1 here either.
Ba2 Cl
Ba
Cl2
Step 3: Determine whether the formula is
in its simplest form. Reduce the subscripts to
their simplest form by dividing by a common
denominator. The formula for barium chloride
is BaCl 2 , which cannot be further reduced.
Step 4: Check the formula by calculating the
total positive and total negative charges and
confirming that the total charge on the
compound is zero.
Barium
Chlorine
Oxidation
Number
(+2)
(–1)
Subscript
✕
(1) =
✕
(2) =
+2
–2
Directions: Use the crisscross method to write the chemical formulas for the compounds described below. Check
that the total charge on each compound equals zero.
1. Write the correct chemical formula for a compound containing barium and oxygen. What is
the name of this compound?
2. Write the formula for zinc iodide, a compound that is used as an antiseptic.
3. One of the uses of ammonium sulfate is in flameproofing fabrics and paper. Write the formula
for ammonium sulfate.
32 Chemical Bonds
Copyright © Glencoe/McGraw-Hill, a division of the McGraw-Hill Companies, Inc.
3
Class
Name
Date
Note-taking
Worksheet
Section 1
Class
Chemical Bonds
Stability in Bonding
A. Some elements combine chemically and no longer have the same ___________________ they
did before forming a compound.
B. A(n) _________________________ is composed of symbols and subscripts indicating the
C. Atoms form compounds when the compound is more _______________ than the separate atoms.
1. Noble gases are more __________________________ than other elements because they
have a complete outer energy level.
2. Elements that do not have full outer energy levels are more stable in __________________.
3. Atoms can lose, gain, or ______________ electrons to get a stable outer energy level.
4. A(n) ______________________ is the force that holds atoms together in a compound.
Section 2
Types of Bonds
A. A(n) ____________ is a charged particle because it has more or fewer electrons than protons.
Copyright © Glencoe/McGraw-Hill, a division of the McGraw-Hill Companies, Inc.
1. When an atom ______________ an electron, it becomes a positively charged ion; a superscript indicates the charge.
2. When an atom ______________ an electron, it becomes a negatively charged ion.
B. An ionic compound is held together by the ___________________—the force of attraction
between opposite charges of the ions.
1. The result of this bond is a(n) ________________ compound.
2. The sum of the charges on the ions in a unit of the compound is _____________.
C. __________________ are neutral particles formed as a result of sharing electrons.
1. A ______________________ is the force of attraction between atoms sharing electrons.
2. Atoms can form double or triple ______________ depending on whether they share two or
three pairs of electrons.
3. Electrons shared in a molecule are held _____________________ to the atoms with the
larger nucleus.
Chemical Bonds
33
Meeting Individual Needs
number of atoms of an element in a compound.
Name
Date
Class
Note-taking Worksheet (continued)
4. A(n) ______________ molecule has one end that is slightly negative and one end that is
slightly positive although the overall molecule is neutral.
5. In a(n) _________________ molecule, electrons are shared equally.
Section 3
Writing Formulas and Naming Compounds
A. Chemists use ________________ from the periodic table to write formulas for compounds.
B. ________________________—composed of two elements
become stable
2. Use oxidation numbers and their least common multiples to write _________________.
a. When writing formulas, remember that the compound is ________________.
b. A formula must have the correct number of positive and negative ions so
the charges ________________.
3. Use the name of the first element, the root name of the second element, and the suffix –ide
to write the _____________ of a binary ionic compound.
C. _______________________—positively or negatively charged, covalently bonded group
of atoms
1. The compound contains ______________ or more elements.
2. To write names, write the name of the _________________ ion first; then write the name
of the _________________ ion.
3. To write _________________, use the oxidation numbers, their least common multiple,
and put parentheses around the polyatomic ion before adding a subscript.
D. ________________—compound with water chemically attached to its ions
E. Name binary covalent compounds by using _________________ to indicate how many atoms
of each element are in the compound.
34 Chemical Bonds
Copyright © Glencoe/McGraw-Hill, a division of the McGraw-Hill Companies, Inc.
Meeting Individual Needs
1. _________________________—how many electrons an atom has gained, lost, or shared to
Name
Date
Chapter
Review
Class
Chemical Bonds
Part A. Vocabulary Review
Directions: Complete the sentence by writing the correct terms in the blanks.
1. An atom that has gained or lost electrons is called a(n) ____________________.
2. An atom is ____________________ when its outer energy level is filled with electrons.
3. A(n) ____________________ tells what elements make up a compound and the ratios of the
atoms of those elements.
4. A molecule that has a positive end and a negative end is a(n) ____________________ molecule.
5. A bond that forms between atoms when they share electrons is a(n) ____________________
bond.
6. A positive or negative number that is assigned to an element to show its combining ability in
a compound is a(n) ____________________.
7. A compound that is composed of only two elements is a(n) ____________________.
8. A group of atoms with a positive or negative charge is a(n) ____________________.
9. A(n) ____________________ is a compound that has water chemically attached to its ions.
a(n) ____________________.
11. Molecules that do not have oppositely charged ends are ____________________ molecules.
12. A(n) ____________________ is formed when atoms gain, lose, or share electrons.
Part B. Concept Review
Directions: Place a plus sign (+) beside each statement that agrees with what was said in your textbook. Place
a minus sign (–) beside each statement that does not agree, and rewrite the statement so that it is correct.
1. Compounds have properties unlike those of their elements.
2. In a chemical formula, a subscript tells how many atoms of an element are in a unit
of a compound.
Chemical Bonds
37
Assessment
Copyright © Glencoe/McGraw-Hill, a division of the McGraw-Hill Companies, Inc.
10. The force of attraction between the opposite charges of the ions in an ionic compound is
Name
Date
Class
Chapter Review (continued)
3. A chemical bond occurs when atoms lose, gain, or share electrons.
4. Because each noble gas has an outer energy level that is completely filled with electrons,
these elements form chemical bonds easily.
5. Compounds containing polyatomic ions can have both ionic and covalent bonds.
6. A covalent bond is the force of attraction between the opposite charges of the ions in
an ionic compound.
7. Neutral particles formed as a result of covalent bonding are called molecules.
Assessment
9. When writing the formula of a compound, the symbol of the element with the positive
oxidation number comes first.
10. When cobalt chloride unites with water to form cobalt hexahydrate, its formula is
written CoCl2 • 6H2O.
38 Chemical Bonds
Copyright © Glencoe/McGraw-Hill, a division of the McGraw-Hill Companies, Inc.
8. An element that loses electrons when bonding with other atoms has a negative
oxidation number.
Name
1
Date
Section Focus
Transparency Activity
Class
Picking Up the Pieces
Transparency Activities
1. Where do the remaining pieces belong? How do you know?
2. How might a compound and its individual elements compare to
a puzzle and its pieces?
44 Chemical Bonds
Copyright © Glencoe/McGraw-Hill, a division of the McGraw-Hill Companies, Inc.
Jigsaw puzzles can have hundreds—even thousands—of pieces. To
complete the puzzle, you need to infer how each piece fits together.
Size, shape, and markings all give clues as to how the pieces should be
placed to make a picture.
Name
2
Date
Section Focus
Transparency Activity
Class
A Crystal Nature
1. Describe the appearance of the salt in the picture.
2. What happens to salt in water? How might you recover salt from
ocean water?
Transparency Activities
Copyright © Glencoe/McGraw-Hill, a division of the McGraw-Hill Companies, Inc.
This picture shows salt crystals on the Dead Sea shore. When a salt
crystal is pure, it is in the shape of a colorless cube. Impurities can
make salt appear to be different colors, like white or gray. Table salt is
a compound of sodium and chlorine.
3. How do people use salt?
Chemical Bonds
45
Name
3
Date
Section Focus
Transparency Activity
Class
For Best Results,
Add Water
1. How might construction be different in the desert compared to a
rainy, temperate region?
Transparency Activities
2. What would happen if a bag of dry concrete got a little damp?
What if it got very wet?
3. When a new sidewalk is finally dry, where does the water go?
46 Chemical Bonds
Copyright © Glencoe/McGraw-Hill, a division of the McGraw-Hill Companies, Inc.
Why are these workers trying to keep the concrete wet rather than
letting it dry? Concrete doesn’t harden because it dries. It hardens by
incorporating water into its molecular structure. If there’s not enough
water, the concrete won’t harden properly, and it won’t be very
durable.
Beryllium
4
Be
Lithium
3
Li
Calcium
20
Ca
Potassium
19
K
88
Ra
87
Fr
Chemical Bonds
47
Transparency Activities
Radium
Francium
Sodium
56
Ba
55
Cs
Na
Barium
Cesium
Chlorine
Cl
Rn
Xe
→
49
In
Indium
31
Ga
81
Tl
Thallium
→
14
Si
Silicon
6
C
Carbon
4
5
Cl
84
Po
Polonium
52
Te
Tellurium
34
Se
Selenium
16
S
Sulfur
8
O
Oxygen
2
Sodium chloride
83
Bi
Bismuth
51
Sb
Antimony
33
As
Arsenic
15
P
Phosphorus
7
N
Nitrogen
Na
82
Pb
Lead
50
Sn
Tin
32
Ge
Gallium Germanium
13
Al
Aluminum
5
B
Boron
3
85
At
Astatine
53
I
Iodine
35
Br
Bromine
17
Cl
Chlorine
9
F
Fluorine
1
86
Rn
Radon
54
Xe
Xenon
36
Kr
Krypton
18
Ar
Argon
10
Ne
Neon
2
He
Helium
Date
38
Sr
37
Rb
Ar
Ne
0
Teaching Transparency
Activity
Rubidium Strontium
12
Mg
11
Na
Sodium Magnesium
2
1
H
Hydrogen
Kr
3
1
He
Copyright © Glencoe/McGraw-Hill, a division of the McGraw-Hill Companies, Inc.
Name
Class
Common Oxidation
Numbers of Selected Groups
Name
Teaching Transparency Activity
Date
Class
(continued)
1. When does an ionic bond form between elements?
2. What is a covalent bond?
3. The formula for baking soda is NaHCO3. Name the elements in baking soda.
4. How many pairs of electrons are shared when hydrogen and oxygen unite to form a molecule
of water?
6. Write the formula for barium (Ba2+) chlorate (ClO3–).
7. Name two pieces of information you can get from a dot diagram.
Transparency Activities
48 Chemical Bonds
Copyright © Glencoe/McGraw-Hill, a division of the McGraw-Hill Companies, Inc.
5. Using the oxidation numbers given on the transparency, write the formula for calcium
chloride, a compound of calcium and chlorine.
Name
Date
Assessment
Transparency Activity
Class
Chemical Bonds
Directions: Carefully review the tables and answer the following questions.
Group B
Water
H 2O
Epsom salts
Mg(OH)2
Carbon dioxide
CO2
Sugar
C12H22O11
Ammonia
NH3
Lye
Salt
NaCl
Baking soda
Methane
CH4
Vinegar
NaOH
NaHCO3
C 2H 4O 2
1. The compounds in Group A are different from the compounds in
Group B because only the compounds in Group A ___.
A are gases at room temperature
B are used in preparing food
C contain a metal and a nonmetal
D contain only two different elements
2. According to the chemical formula for lye, all of the following elements are found in a lye molecule EXCEPT ___.
F hydrogen
H oxygen
G nitrogen
J sodium
3. According to the information contained in the tables, which
compound has a total number of atoms greater than 10?
A Baking soda
C Sugar
B Methane
D Vinegar
Transparency Activities
Copyright © Glencoe/McGraw-Hill, a division of the McGraw-Hill Companies, Inc.
Group A
4. According to the tables, which compound has the LEAST number
of total atoms?
F Ammonia
H Salt
G Carbon dioxide
J Water
Chemical Bonds
49