Unit 6 – Lab 1
Separation of water into its gaseous elemental components using the Hoffman apparatus
involved using an electric current. What about our current model of matter could explain this?
Title:
Question:
Hypothesis:
Procedures:
1. Take a 15 cm piece of transparent tape and make a handle on the end by folding
under the first cm of tape, sticky side to sticky side. Place this tape on the lab table.
This is the base tape.
2. Take a second 15 cm piece of transparent tape, make a handle as before, and place
this tape on top of the base tape. Label this tape “B” for bottom.
3. Attach a third similarly prepared strip of tape onto the bottom tape. Label this tape
“T” for top.
top
base
bottom
table
4. Repeat steps 1 through 3 above. You now have two sets of 3-layer tapes.
5. Obtain 2 pieces of paper, the same dimensions as the tapes, and hang one from the
edge of the table. Label the hanging paper “P." Approach the hanging paper with
the other piece of paper. Describe what you see.
6. Obtain 2 pieces of aluminum foil, the same dimensions as the tapes, and hang one
from the edge of the table. Label the hanging foil “F." Approach the hanging foil
with the other piece of foil. Describe what you see. 7. Peel one set of T and B tapes from its base tape, keeping the T and B tapes together.
Run your finger down the non-sticky side, then quickly peel them apart.
8. Hang each strip next to the hanging
paper and foil.
F
P
T
B
table
9. Repeat step 7 with the other set of
tapes.
10. With a T tape hanging from one hand
and a B tape hanging from the other, experiment by approaching each of the
hanging tapes, the foil strip and the strip of paper. Be sure to describe the kind of
interaction you see as you bring each of the tapes near the hanging tapes and strips.
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185 Data Top
Bottom
Foil
Paper
Top
Bottom
Foil
Paper
Plastic
(Other)
Analysis After you have summarized your findings (attraction, repulsion or no interaction) for
the two tapes, foil and paper, rub a hard rubber or plastic rod with fur or wool.
Approach the T tape, the B tape, the foil and the paper with the rod. Describe what
you see. Does the rod behave more like the T tape or the B tape?
Based on a number of observations scientists have assigned the label of negative (–)
to the charge of a rubber or plastic rod rubbed with fur or wool. The fur or wool
becomes positively charged (+). Based on your observations from using the rod, label
the T and B tapes as either a (+) or (–). Explain.
Now, reflect on the relative strengths of the interactions between the tapes, foil
and paper. How did attraction between the T or B tape and the foil or paper
compare to the interaction between tapes? (Did the tapes exhibit a stronger
attraction than the tape and paper/foil?) You may need to repeat step 10 to
answer this question.
Post-Lab Questions
1. Prior to the Sticky Tape Lab, we imagined the particles that make up various
substances to look sort of like tiny marbles or bb’s. The evidence gathered in
this lab forces us to change our model for the atom. What changes are
necessary? Draw a sketch of our “newly revised model” of the atom.
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186 2. Was the top tape positively (+) or negatively (-) charged? How do you
know (based on the evidence collected in the laboratory)?
3. Was the bottom tape positively (+) or negatively (-) charged? How do you
know (based on the evidence collected in the laboratory)?
4. What happened when the T (top) tape interacted with the B (bottom) tape?
Draw a diagram to show what is happening at the particle level.
Top Tape Bottom Tape 5. Did the top tape react differently with the foil than it did with the paper?
Are the particles that make up the aluminum different from the particles
that make up the paper? Draw diagrams that illustrate differences between
the foil and the paper at the particle level. Explain.
Foil Top Tape Paper 6. What happened when one piece of paper was interacted with another piece of
paper? Draw diagrams that illustrate what is happening at the particle level.
Explain.
Paper Modeling Chemistry
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Paper 187 Additional Particle Diagram Practice
Draw and explain the following particle diagrams.
1.
Bottom tape vs. top tape
Top Tape 2.
Bottom tape vs. bottom tape
Bottom Tape 3.
Bottom Tape Bottom tape vs. foil
Foil 4.
Bottom Tape Bottom Tape Bottom tape vs. paper
Top Tape Modeling Chemistry
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Bottom Tape 188 Name:______________________________________
Veritas:______________________________________
Unit 6, Worksheet 1—
Thomson Model of the Atom
J. J. Thomson performed experiments with cathode rays in an attempt to understand electricity – which was still a mystery in the late 1800s. Review the website A Look Inside the Atom to find the conclusions that Thomson and other physicists drew regarding the mysterious cathode rays. (http://www.aip.org/history/electron/jjhome.htm) Thomson’s 1897 Experiments -­‐ state the conclusions Thomson drew from each of his famous cathode ray experiments: 1.
First Experiment: Thomson directed the beam at an electrometer and tried
to separate the evidence of charge from the path of the beam. What connection did
Thomson find between charge and the cathode rays? Was the charge positive or
negative?
2.
Second Experiment: Thomson tried passing the cathode ray through an
electric field. How did cathode ray beam behave when it passed through an electric
field? What did he conclude after his second experiment?
3.
Third Experiment: Thomson did some careful measurements on how much
the path of the cathode ray was bent in a magnetic field and how much energy they
carried. From this work Thomson could describe the mass/charge ratio of the
cathode ray particles. What amazing result did Thomson find?
3 Hypotheses:
123Thomson’s Atomic Model: Thomson presented three hypotheses from his
experiments. Only two were accepted by physicists – in fact the third was shown to be
wrong! From the first two came a model of the atom known as the Plum Pudding
model. Complete the atom drawing below to illustrate Thomson’s plum pudding model.
Explain how this fits with his observations.
Which component of the model was based on evidence? Which component of the model was based on reasoning, not evidence? Modeling Chemistry
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189 Unit 6 — Free Notes Page
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190 Unit 6 – Lab
We have seen differences in the mobility of negative charge in the atoms of various
substances. Perhaps we could use this to sort compounds.
Title:
Question/Purpose:
Hypothesis:
Procedures:
Do not contaminate substances. Clean electrodes between each use (wipe, dip in
water, wipe again). Only the electrodes should be put into water/solutions. (Do not
submerge any other part of the tester.)
Part 1: Metals
Make sure that your switch is in the ON position. Test each of the metals listed
below for conductivity. To obtain accurate results, the metal must make a good
connection with both electrodes at the bottom of the tester. Use the scale given on
the back of the conductivity tester and record results.
1.
Copper wire
2.
Aluminum wire
Part 2: Solid compounds
Place a sample of each solid into the micro-well plate. Test each of the solids listed
below for conductivity. Make sure that you clean the electrodes thoroughly with a
paper towel when changing substances. Record your results.
1.
sodium bicarbonate (baking soda)
2.
sodium chloride (table salt)
3.
sucrose (granulated white sugar)
Part 3: Dissolved solids
Test each of the solutions for conductivity. Make sure that you clean and dry the
electrodes thoroughly with a paper towel when changing substances. Record your
results.
1.
sodium bicarbonate solution (baking soda dissolved in distilled water)
2.
sodium chloride solution (table salt dissolved in distilled water)
3.
sucrose solution (granulated white sugar dissolved in distilled water)
Part 4: Liquids
Test each liquid for conductivity. Make sure that you clean and dry the electrodes
thoroughly with a paper towel when changing substances. Record results.
1.
distilled water
2.
tap water
3
ammonia
4.
vinegar
5.
rubbing alcohol
6.
hydrochloric acid (0.1M)
7.
liquid hand soap or liquid starch
8.
vegetable oil
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191 Cleanup:
Turn off the tester. Organize all materials on the table and throw away trash. Wipe
up any spills and leave your lab station clean.
Data:
Divide your substances into one of three categories: strong electrolytes, weak
electrolytes, non-electrolytes.
Strong electrolytes
Weak electrolytes
Non-electrolytes
Discuss the behavior observed in metals.
Discuss the behavior observed in the various liquids.
Discuss the two types of behavior observed in compounds:
1.
2.
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192 Unit 6 – Lab 3
We have sorted substances based on conductivity data. Now, let’s examine the crystal
structure of these substances.
Title:
Question/Purpose:
Hypothesis:
Procedures:
Part 1: Look at the X-Ray Crystallography image of water, what
distinguishing features can you cite?
1.
____________________________ 2. _____________________________
Part 2: Complete the table below for the solids listed.
A. The types of particles (ions, atoms, or molecules)
B. The connections between those particles (T-connected throughout, Sconnected only in some directions,
N-no connections between particles).
C. Identify the type of solid that best describes each row and write a brief
statement summarizing what the solids in each row have in common.
Type of
Particles
in the Solid
Row 1
1. Argon
Connections
Within and
Between
Particles in
the Solid 2. Copper
3. Graphite Type of Solid (atom, molecule, ion//
metal, non-metal) Generalization
Concerning Particle
Types and
Connections
Row 2 1. Dry Ice (CO2)
2. Sulfur ( S8)
3. Sugar (C12H22O11) Row 3 1. Table Salt (NaCl)
2. Marble (CaCO3)
3. Baking Soda
(NaHCO3) Modeling Chemistry
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193 Part 3: On a white board, develop a set of “Rules for Identification” of these 3
categories of solids.
Your Rules for Identification must:
• Allow for correct classification of any substance.
• Identify the type of particles involved in the class of solids.
• Specify the types of connections or lack of connections between
particles belonging to this category.
Notes -
Part 4: Write the “Rules for Identification” of the 3 classes of compounds agreed
upon by the class.
Atomic Solids _______________________________________________________________________
_______________________________________________________________________
_______________________________________________________________________
Molecular Solids ______________________________________________________________________
______________________________________________________________________
______________________________________________________________________
Ionic Solids (Formula Unit Solids) –
_______________________________________________________________________
_______________________________________________________________________
_______________________________________________________________________
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194 Argon: Graphite: Water: Sulfur (S8): Sucrose: Calcium carbonate (CaCO3): Copper: Salt (NaCl): Dry Ice (CO2): NaHCO3: Modeling Chemistry
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195 Modeling Chemistry
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196 Unit 6 – Lab 2 and 3
Tying it all together
Atomic Solids
Molecular Solids
Ionic Solids
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197 Unit 6 – Free Notes Page
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198 Name:______________________________________
Veritas:______________________________________
Unit 6, Worksheet 2—
Why Structure is Important
In the table below, identify the type of solid (atomic, molecular, ionic) each substance
forms. Then predict in which phase (solid, liquid or gas) each substance would exist
on the Earth, on Mercury and on Pluto.
Substance
Crystal structure
NaCl
Type
melting pt (°C)
boiling pt (°C)
801
1413
Phase at
room temp
on
Earth
(25°C)
Mercury
(450°C)
Pluto
(-230°C)
CaCO3
520
decomposes at
825
E
M
P
S8
Cu
115
444
1084
2567
E
M
P
E
M
P
H2O2
-0.41
150
E
M
P
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199 PbI2
402
954
E
M
P
CO2
-78
-57
E
M
P
Ar
-189
-186
E
M
P
Account for differences in the melting and boiling points of the three types of
structures.
Predict which of these substances would conduct electricity when molten.
Would any of these conduct electricity as a solid?
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200 Chemistry Unit 6 – Naming Ionic Compounds
A. Use this method when the compound joins a metal and a non-metal. The metal
forms only one type of cation (positive ion).
B. Name the metallic element first and give its full name.
C. Name the non-metal last. Give only its root and substitute the suffix
–ide.
Directions: Name the following binary ionic compounds by using the rules
outlined above.
1. MgCl2
2. LiBr
3. Na2O
4. KI
5. CaS
D. When the metal is a transition metal capable of forming more than one cation,
use the rules outlined above except use a Roman numeral in parenthesis after
the name of the metal which gives the charge on the cation (positive ion).
Directions: Name the following binary ionic compounds, which contain
transition metals.
5. Cu2S
6. CuS
7. MnO
9. Mn2O3
10. FeO
11. Fe2O3
12. Ag2S
13. ZnCl2
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201 E. When the compound contains a polyatomic cation, use the rules above
except name the ion instead of the element. If the compound contains a
polyatomic anion, do not change the suffix to –ide. Instead, simply name
the ion. See Common Ions List for naming information.
Example: NaNO3 Sodium nitrate
14. Be(HCO3)2
15. Al(CN)3
16. Pb(SO4)2
17. NaNO3
18. KOH
F. It is also important to be able to write formulas given the compound name. For
ionic compounds, you can determine the subscripts in the formula by balancing out
the charges of the ions.
Example: Sodium nitride
+1 -­‐3 +1 +1 14. lithium oxide
15. aluminum iodide
16. ammonium sulfide
17. beryllium hydroxide
18. Iron (II) oxide
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202 Name
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Chemistry Unit 6 – Worksheet 3
Ionic Compounds
Properties:
Basic Structural Unit:
1. Write the name of the following simple binary ionic compounds.
a. Na2O __________________
h. CsI ____________________
b. K2S____________________
i. AgF____________________
c. MgCl2__________________
j. Na3N___________________
d. CaBr2__________________
k. K2O____________________
e. BaI2___________________
l. AgBr___________________
f. Al2S3___________________
m. MgI2___________________
g. CsBr___________________
n. SrO____________________
2. Write the formula for the following ionic comnpounds.
a. Lithium bromide __________
h. Lithium oxide ___________
b. Sodium iodide_____________
i. Potassium oxide__________
c. Silver sulfide______________
j. Silver oxide_______________
d. Cesium oxide______________
k. Aluminum sulfide_________
e. Beryllium iodide___________
l. Sodium nitride____________
f. Barium hydride____________
m. Barium chloride___________
g. Aluminum fluoride_________
n. Strontium hydride_________
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203 3. Write the name of the following ionic compounds using a Roman
numeral to specify the charge of the cation.
a. SnBr2 _____________________
k. Fe(HCO3)2 _____________
b. SnBr4_____________________
l. CoBr2 __________________
c. CrO_______________________
m. Mn2(SO3)3 _____________
d. Cr2O3_____________________
n. Pb(SO4)2 _______________
e. Hg2I2_____________________
o. PbCl2___________________
f. HgI2______________________
p. Fe2O3__________________
g. Cu2O _____________________
q. SnI2____________________
h. YClO3 __________________
r. Hg2O___________________
i. SnS2 ___________________
s. HgS____________________
j. Cu(NO2)2 _______________
t. CuI_____________________
4. Write the formula of the following ionic compounds.
a. Chromium (III) chloride _______
k. Cobalt (III) oxide ____________
b. Tin (IV) oxide_________________
l. Iron (II) phosphate __________
c. Lead (II) oxide________________
m. Titanium (II) selenide _______
d. Copper (II) iodide_____________
n. Copper (II) chlorate _________
e. Cobalt (II) oxide______________
o. Gold (III) chloride____________
f. Cobalt (III) oxide______________
p. Titanium (IV) chloride________
g. Chromium (III) sulfide________
q. Iron (II) bromide_____________
h. Manganese (IV) oxide_________
r. Iron (II) oxide________________
i. Chromium (III) hydroxide _____
s. Vanadium (VI) phosphate _____
j. Tin (II) nitrite _______________
t. Lead (II) nitride ______________
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204 Name
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Chemistry Unit 6 – Worksheet 4
Representing Ions and Formula Units
IONS 1. Ca2+ and FORMULA Br– 2. Fe2+ and Cl– 3. K+ 2–
SO4 and
NAME 4. 5. 6. 7. Al3+ and NO3– Pb2+ and S2– _____ and _____ NH4OH _____ and _____ KHCO3 Modeling Chemistry
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205 8. _____ and _____ Mg(NO2)2 _____ and _____ ZnCO3 _____ and _____ Na3PO4 9. 10. 11. 12. 13. 14. 15. _____ _____ _____ _____ _____ and and and and and _____ _____ _____ _____ _____ Modeling Chemistry
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For 11 – 15 state the total number of atoms and the number of ions in the compound silver chromate atoms ions lithium chlorate atoms ions copper (II) nitrate atoms ions iron (III) sulfide atoms ions calcium sulfate atoms ions 206 Name:______________________________________
Veritas:______________________________________
Unit 6, Worksheet 5—
More Practice with Ionic Compound Nomenclature
IONS FORMULA 1. 2. Na+ and Br– Cu+ and SO42– 3. Pb2+ and Cl– 4. K+ and 5. 6. 7. 8. 9. 10. 11. 12. 13. 14. 15. 16. Sn2 + and F– _____ and _____ _____ and _____ _____ and _____ _____ and _____ _____ and _____ _____ and _____ _____ and _____ _____ and _____ _____ and _____ _____ and _____ Mg2+ and NO3– 17. 18. 19. 20. Cu2+ and OH– _____ and _____ _____ and _____ _____ and _____ Modeling Chemistry
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S2– BaI2 AlCl3 Mg(NO3)2 KOH (NH4)2SO4 NaHCO3 NAME silver oxide lithium bromide copper (II) nitrate magnesium chloride calcium carbonate iron (III) sulfide potassium chromate 207 Write the names of the following ionic compounds. 1) Na2CO3 _______________________ 11) 2) NaOH ________________________ 12) 3) MgBr2 ________________________ 13) 4) KCl ____________________________ 14) 5) FeCl2 ___________________________ 15) 6) FeCl3 ___________________________ 16) 7) Zn(OH)2 _______________________ 17) 8) Be2SO4 _________________________ 18) 9) CrF2 ____________________________ 19) 10) Al2S3 ____________________________ 20) Write the formulas of the following ionic compounds. PbO _____________________________ Li3PO4 __________________________ TiI4 _____________________________ Co3N2 ___________________________ Mg3P2 ___________________________ Ga(NO2)3 ________________________ Ag2SO3 ___________________________ NH4OH __________________________ Al(CN)3 ___________________________ Be(CH3COO)2 ___________________
22) 23) 24) 25) 26) 27) 28) 29) 30) 31) sodium phosphide ______________ magnesium nitrate ______________ lead (II) sulfite __________________ calcium phosphate ______________ ammonium sulfate ______________ silver cyanide ___________________ aluminum sulfide _______________ beryllium chloride ______________ copper (I) arsenide _____________ 32) 33) 34) 35) 36) 37) 38) 39) 40) gallium nitride __________________ iron (II) bromide _______________ vanadium (V) phosphate ______ calcium oxide ___________________ magnesium acetate ____________ aluminum sulfate _______________ copper (I) carbonate ____________ barium oxide ____________________ ammonium sulfite ______________ iron (III) oxide __________________ Modeling Chemistry
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208 Chemistry Unit 6 – Naming Molecular Compounds
A. Use this method only when the compound contains two non-metals.
B. Name the elements in the order that they appear in the chemical formula.
C. Drop the last syllable in the name of the final element and add
–ide.
D. Use the prefixes to indicate the number of atoms of each element present.
Mono-
1
penta-
5
nona-
9
di-
2
hexa-
6
deca-
10
tri-
3
hepta-
7
tetra-
4
octa-
8
Note: The prefix mono- is often omitted in common practice for the first element in the
name of a compound.
Directions: Name the following molecular compounds using the rules
outlined above.
1. SiO2
4. CO
2. CSe2
5. N2O5
3. S4N2
6. PCl5
Directions: Write the correct chemical formula for each of the following
molecular compounds using the rules outlined above.
7. Chlorine dioxide
8. Dichlorine monoxide
9. Diphosphorous tetroxide
10. Carbon tetrachloride
11. Arsenic pentachloride
12. Sulfur hexafluoride
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209 Write the formulas for the following covalent compounds: 1) antimony tribromide ______________________________ 2) hexaboron silicide _________________________________ 3) chlorine dioxide ____________________________________ 4) hydrogen iodide ____________________________________ 5) iodine pentafluoride ________________________________ 6) dinitrogen trioxide __________________________________ 7) ammonia _____________________________________________ 8) phosphorus triiodide ________________________________ Write the names for the following covalent compounds: 9) P4S5 __________________________________ 10) O2 ____________________________________ 11) SeF6 __________________________________ 12) Si2Br6 ________________________________ 13) SCl4 __________________________________ 14) CH4 __________________________________ 15) B2Si __________________________________ 16) NF3 __________________________________ Modeling Chemistry
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210 Name:______________________________________
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Unit 6, Worksheet 6— Molecular Nomenclature
Properties of Molecular Compounds:
Basic Structural Unit of Molecular Compounds:
1. Name each of the following binary compounds of non-metallic elements.
a. CBr4 _______________________
g. GeH4_______________________
b. N2P3_______________________
h. N2Br4______________________
c. PCl3_______________________
i.
P2S5_______________________
d. ICl_________________________
j.
SeO2_______________________
e. N2O_______________________
k. NH3_______________________
f.
l.
SiF4_______________________
SiO2_______________________
2. Write the formula for the following binary compounds of nonmetallic elements.
a. Phosphorous triiodide ________
g. Nitrogen monoxide ___________
b. Silicon tetrachloride__________
h. Sulfur hexafluoride___________
c. Dinitrogen pentoxide_________
i.
Dinitrogen tetrachloride_______
d. Carbon monoxide____________
j.
Carbon tetraiodide____________
e. Dinitrogen tetroxide_________
k. Phosphorous pentaflouride_____
f.
l.
Carbon dioxide______________
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Diphosphorous pentoxide______
211 3. Name each of the following binary compounds of non-metallic elements.
a. SiF4 __________________________________________________
b. N2S3 _________________________________________________
c. HBr __________________________________________________
d. Br2 __________________________________________________
e. P2O5 __________________________
f.
SiO2 __________________________
g. N10O4 ___________________________
4. Write the formula for the following binary compounds of nonmetallic elements.
a. diboron hexahydride ____________________________________
b. nitrogen tribromide ______________________________________
c. sulfur hexachloride ______________________________________
d. diphosphorus pentoxide __________________________________
e. carbon disulfide ________________________________________
f.
boron trifluoride ________________________________________
g. carbon tetrafluoride _____________________________________
h. diboron tetrabromide ____________________________________
i.
carbon nonoxide _________________________________________
j.
octaphosphorus heptoxide ________________________________
k. trinitrogen monosulfide ___________________________________
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212 Name:______________________________________
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Unit 6, Worksheet 7—
Ionic and Molecular Nomenclature Practice
Indicate whether the compound is ionic (I) or molecular (M) on the left and then provide
the name of the compound on the right.
________1.
HCl
________19.
H3PO4
________2.
KOH
________20.
CsOH
________3.
Hg(OH)2
________21.
Li2O
________4.
KCl
________22.
Ca(OH)2
________5.
FeCl3
________23.
CaBr2
________6.
HNO3
________24.
Fe2O3
________7.
NH4OH
________25.
H2SO4
________8.
Cu2O
________26.
FeCO3
________9.
Al2(SO4)3
________27.
SO3
________10.
N 2O 5
________28.
Ba(BrO3)2
________11.
NaOH
________29.
Al(OH)3
________12.
CO2
________30.
HClO4
________13.
HF
________31.
NaC2H3O2
________14.
Pb(OH)2
________32.
Na2SO3
________15.
NH4NO3
________33.
H2CO3
________16.
NaHCO3
________34.
HFO2
________17.
HgO
________35.
ZnF
________18.
Zn(NO2)2
________36.
LiB
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213 First indicate whether the compound is ionic (I) or molecular (M). Then, write the
names of the following compounds
1. 2. 3. 4. 5. 6. 7. 8. 9. 10. 11. 12. 13. 14. 15. Cu(NO3)2 ____________________________________________________________ BaCl2 ____________________________________________________________ HgO ____________________________________________________________ Ni(OH)2 ____________________________________________________________ Na3PO4 ____________________________________________________________ CaCO3 ____________________________________________________________ CS2 ____________________________________________________________ SnBr4 ____________________________________________________________ (NH4)2CrO4__________________________________________________________ Mg(NO3)2 ___________________________________________________________ Li2O ____________________________________________________________ FeS ____________________________________________________________ NI3 ____________________________________________________________ H2SO4 ____________________________________________________________ K2C2O4 ____________________________________________________________ First indicate whether the compound is ionic (I) or molecular (M). Then, write the
formulas for the following compounds.
1. copper (II) sulfate 3. iron (III) chloride 5. aluminum oxide 7. potassium phosphate 9. ammonium carbonate 11. carbon tetrachloride 13. sulfur hexafluoride 15. chromium (III) oxide Modeling Chemistry
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2. sodium chromate 4. silver sulfide 6. zinc nitrate 8. strontium fluoride 10. magnesium hydroxide 12. phosphorus tribromide 14. sulfur dioxide 17. Lead (II) iodide 214 Name:______________________________________
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Unit 6, Worksheet 7— Extra Practice Problems
I. Sticky Tape: from Dalton’s model of the atom to Thomson’s model.
1. Recall your representations of the atoms in the Sticky Tape activity. Below is a
pair of tapes before they have been pulled apart. Explain why they would not exert
a force (either attractive or repulsive) on one another.
TT
BT
2. Below are groups of the inner cores of the atoms of the tapes after they have been
pulled apart. Sketch in the mobile negative charges to show what happens to the
charge of the tapes. To the right, explain your diagrams.
TT
BT
3. What evidence allowed us to conclude that the top tape was (+)?
4. Below is a group of the inner cores of a piece of paper. Sketch in where you would
expect to find the negative charges if a top (+) tape (shown below) were brought to
the left of the paper. Explain your diagram.
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215 5. Below is a group of the inner cores of a piece of metal foil. Sketch in where you
would expect to find the mobile negative charges if a top (+) tape (shown below) were
brought to the left of the foil. Explain why this diagram is different than the
diagram in #4.
6. Describe how JJ Thomson concluded that the mobile charged particle in the atom
had a (–) charge.
II. Atomic v. Molecular v. Ionic Solids
7. A solution of salt conducts electricity; a solution of sugar does not. Explain.
8. Below left is a 2-D array that represents an ionic solid. At right is a 2-D array
that represents a molecular solid. In what ways are they similar? In what ways are
they different?
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216 9. Why do ionic solids have higher melting and boiling points than do most
molecular solids?
10. Why do we use the term “formula unit” rather than “molecule” when we refer to
the simplest repeating unit of an ionic solid?
III. Naming Ionic and Molecular Compounds
11. Apart from making life difficult for beginning chemistry students, why do
chemists refer to CO2 as carbon dioxide, yet use the name tin (IV) oxide to describe
SnO2?
12. Which combinations of elements give rise to ionic compounds and which form
molecular compounds? (In other words, how do you recognize, based on a formula
alone, whether a compound is ionic or molecular?)
13. Write M for molecular compounds and I for ionic compounds to the left. Then,
write the correct name or the correct formula for the compound to the right.
_____HNO3
_______________
_____Ammonium phosphate __________
_____CO2
_______________
_____Potassium sulfate ______________
_____Hg(OH)2 _______________
_____P2O5___________________________
_____P2O5___________________
_____Sulfur dioxide ________________
_____FeCl3____________________
_____Carbon monoxide ______________
_____Cu2O___________________
_____ Lead (IV) xide ________________
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217 15.
Fill in the blanks and then sketch the ions and the solid ionic compound that is
formed. Use different colors or different textures in your diagram to
distinguish between ions. Ions should be labeled with charge.
IONS
FORMULA
A.
Mg2+ and
Cl–
B.
Na+
CO32–
C.
_____ and
_____
Fe(OH)2
D.
_____ and
_____
K2SO4
E.
_____ and
_____
and
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NAME OF COMPOUND
chromium(III) oxide
218 Write chemical formulas for the compounds in each box. The names are found by finding the intersection between the cations and anions. Example: The first box is the intersection between the “zinc” cation and the “chloride” anion, so you should write “ZnCl2”, as shown. zinc iron (II) iron (III) gallium silver lead (IV) chloride ZnCl2 acetate nitrate oxide nitride sulfate Write the formulas for the following compounds
1) 9) copper (II) chloride ____________ 2) 3) vanadium (III) selenide ________ 5) beryllium oxide _________________ sodium sulfate __________________ aluminum arsenide _____________ 8) 14) sodium hydroxide _______________ 7) ammonium nitrate ______________ 13) copper (II) acetate ______________ 6) vanadium (V) fluoride __________ 12) manganese (IV) nitride _________ tin (II) sulfite ____________________ 11) 4) 10) lithium acetate __________________ chromium (VI) cyanide _________ potassium permanganate ______ Modeling Chemistry
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15) 16) 17) lithium oxide ____________________ cobalt (III) carbonate ___________ aluminum sulfide _______________ 219 18) 19) 20) 21) 22) 23) 24) ammonium cyanide _____________ iron (III) phosphide ____________ vanadium (V) phosphate _______ sodium permanganate _________ manganese (III) fluoride _______ beryllium nitrate ________________ nickel (III) sulfite _______________ 25) 26) 27) 28) 29) 30) 31) 32) potassium oxide ________________ silver bromide __________________ zinc phosphate _________________ copper (II) bicarbonate ________ nickel (II) selenide ______________ manganese (IV) carbonate _____ lead (IV) nitride _________________ tin (II) hydroxide _______________
Naming Ionic Compounds Practice Worksheet Name the following ionic compounds
1) NH4Cl ___________________________________ 2) 11) Fe(NO3)3 ________________________________ 3) TiBr3 _____________________________________ 5) 6) 7) 8) 9) 10) Al(CN)3 _________________________________ Modeling Chemistry
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lithium iodide__________________________ 19) chromium (III) hydroxide _____________ 18) Mn2(SO3)3 _______________________________ vanadium (V) sulfide __________________ 17) Be(HCO3)2 _______________________________ titanium (II) acetate ___________________ 16) Pb(SO4)2 _________________________________ cobalt (III) oxide _______________________ 15) GaAs ____________________________________ tin (II) nitrite __________________________ 14) SnSe2 ___________________________________ vanadium (IV) carbonate _____________ 13) Cu3P _____________________________________ chromium (VI) phosphate _____________ 12) 4) Write the formulas for the following compounds: lead (II) nitride ________________________ 20) silver bromide _________________________
220 Name the following compounds: 1) NaBr __________________________________ 2) Sc(OH)3 _______________________________ 3) V2(SO4)3 _______________________________ 4) NH4F __________________________________ 5) CaCO3 __________________________________ 6) NiPO4 __________________________________ 7) Li2SO3 __________________________________ 8) Zn3P2 __________________________________ 9) Sr(C2H3O2)2 ____________________________ 10) Cu2O __________________________________ 11) Ag3PO4 _________________________________ 12) YClO3 __________________________________ 13) SnS2 ____________________________________ 14) Ti(CN)4 _________________________________ 15) KMnO4 __________________________________ 16) Pb3N2 __________________________________ 17) CoCO3 __________________________________ 18) CdSO3 __________________________________ 19) Cu(NO2)2 _______________________________ 20) Fe(HCO3)2 ______________________________ Modeling Chemistry
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Write the formulac of the ompounds: 21) lithium acetate ________________________ 22) iron (II) phosphate _____________________ 23) titanium (II) selenide _________________ 24) calcium bromide ______________________ 25) gallium chloride _______________________ 26) sodium hydride ________________________ 27) beryllium hydroxide ___________________ 28) zinc carbonate __________________________ 29) manganese (VII) arsenide _____________ 30) copper (II) chlorate ____________________ 31) cobalt (III) chromate __________________ 32) ammonium oxide _____________________ 33) potassium hydroxide __________________ 34) lead (IV) sulfate _______________________ 35) silver cyanide __________________________ 36) vanadium (V) nitride __________________ 37) strontium acetate _____________________ 38) molybdenum sulfate __________________ 39) platinum (II) sulfide ___________________ 40) ammonium sulfate _____________________ 221 For each of the following questions, determine whether the compound is ionic or covalent and name it appropriately. 1) Na2CO3 _____________________________________ 2) P2O5 ________________________________________ 3) NH3 _________________________________________ 4) FeSO4 _______________________________________ 5) SiO2 _________________________________________ 6) GaCl3 ________________________________________ 7) CoBr2 ________________________________________ 8) B2H4 _________________________________________ 9) CO ___________________________________________ 10) P4 ___________________________________________ For each of the following questions, determine whether the compound is ionic or molecular and write the appropriate formula for it. 11) 12) 13) 14) 15) 16) 17) dinitrogen trioxide _____________________________ nitrogen _________________________________________ methane _________________________________________ lithium acetate __________________________________ phosphorus trifluoride _________________________ vanadium (V) oxide _____________________________ aluminum hydroxide ____________________________ 18) 19) 20) zinc sulfide _______________________________________ silicon tetrafluoride _____________________________ silver phosphate _________________________________ Modeling Chemistry
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222 Write the names of the following chemical compounds: 1) BBr3 _____________________________________ 16) 2) CaSO4 ____________________________________ 17) 3) C2Br6 ____________________________________ 18) 4) Cr(CO3)3 _________________________________ 19) 5) Ag3P _____________________________________ 20) 6) IO2 ______________________________________ 21) 7) VO2 ______________________________________ 22) 8) PbS ______________________________________ 23) 9) CH4 ______________________________________ 24) 10) N2O3 _____________________________________ 25) 11) NaBr ____________________________________ 26) 12) Ca(C2H3O2)2 _____________________________ 27) 13) P2O5 ____________________________________ 28) 14) Ti(SO4)2__________________________________ 29) 15) FePO4 ___________________________________ 30) Write the formulas of the following chemical compounds: 11) tetraphosphorus triselenide ___________________________ 12) potassium acetate ______________________________________ 13) iron (II) phosphide _____________________________________ 14) disilicon hexabromide _________________________________ 15) titanium (IV) nitrate ___________________________________ 16) diselenium diiodide ____________________________________ 17) copper (I) phosphate ___________________________________ 18) gallium oxide ___________________________________________ 19) tetrasulfur dinitride _____________________________________ 20) phosphorus _____________________________________________ Modeling Chemistry
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K3N _____________________________________ SO2 ______________________________________ CuOH ____________________________________ Zn(NO2)2 ________________________________ V2S3 ______________________________________ NaBr _____________________________________ Ca(C2H3O2)2 _____________________________ P2O5 _____________________________________ Ti(SO4)2 _________________________________ FePO4 ____________________________________ K3N ______________________________________ SO2 _______________________________________ CuOH ____________________________________ Zn(NO2)2 _______________________________ V2S3 _____________________________________
223 Write the formulas for the following chemical compounds: 11) 12) 13) 14) 15) 16) 17) 18) 19) 20) silicon dioxide ______________________________________________ nickel (III) sulfide __________________________________________ manganese (II) phosphate ________________________________ silver acetate ______________________________________________ diboron tetrabromide _____________________________________ magnesium sulfate heptahydrate ________________________ potassium carbonate ______________________________________ ammonium oxide _________________________________________ tin (IV) selenide ___________________________________________ carbon tetrachloride _______________________________________ Name the following chemical compounds: 11) silicon dioxide _______________________________________________ 12) nickel (III) sulfide ___________________________________________ 13) manganese (II) phosphate __________________________________ 14) silver acetate ________________________________________________ 15) diboron tetrabromide _______________________________________ 16) magnesium sulfate heptahydrate __________________________ 17) potassium carbonate ________________________________________ 18) ammonium oxide ____________________________________________ 19) tin (IV) selenide ______________________________________________ 20) carbon tetrachloride __________________________________________
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224