Chemical Bonding
Part 1
Ionic Bonding
Unit 4
(Ionic Compounds)
Objectives:
1.
2.
3.
4.
5.
6.
Using the octet rule, write the symbols for ions of the representative elements.
Using the charge, write the correct formula for an ionic compound.
Write the formula for a compound containing a polyatomic ion.
Given the formula for an ionic compound, write its correct name.
Describe the energy levels, sublevels, and orbitals in atoms.
Write the arrangement of electrons for atoms using the sublevel blocks on the
periodic table.
7. Given the name or symbol of an element, write the electron configuration.
8. Define solute and solvent; describe the formation of a solution.
9. Identify solutes as either electrolytes or non-electrolytes.
10. Define solubility; distinguish between an unsaturated and a saturated solution.
11. Identify an insoluble salt.
Vocabulary:
Ionic Bond, Ion, Polyatomic Ion, Metals, Nonmetals, Metalloids, Valence, Subscript,
Transition Metals, Conductivity, Solubility, Precipitate, Electron Configuration, Orbital,
Strong Electrolyte, Weak Electrolyte, Cation, Anion, Lone Pair, Formula
2
COMMON POLYATOMIC IONS
Quiz #1
Quiz #2
-
acetate
C2H3O2
______________________________________
perchlorate
C1O4-
chlorate
C1O3-
chlorite
C1O2-
CO32-
bicarbonate
HCO3(hydrogen carbonate)
_________________________
permanganate
MnO4-
hypochlorite C1O_________________________
chromate
CrO42dichromate
carbonate
Cr2O72-
oxalate
C2O42-
cyanide
CN-
hydroxide
OH-
ammonium
NH4+
Quiz #3
sulfate
SO42-
sulfite
SO32-
bisulfate
HSO4(hydrogen sulfate)
bisulfite
HSO3(hydrogen sulfite)
________________________
nitrate
NO3NO2____________________________________
nitrite
phosphate
PO43-
3
4
Crystal Lab PLW
1. Which chemicals do you need to be very careful of?
2. What will happen when you add the acid to the base?
3. How many times do you filter on day one?
4. What do you do with the contents of the filter paper?
5. Why should you be gentle with the alum crystals you form?
6. Ionic salts form crystal lattices at the atomic level. Draw an example of
these.
5
6
Crystal Lattice Lab
Purpose: The purpose of this lab is to create and examine various crystals. You will be
creating alum [potassium aluminum sulfate KA1(SO4)2] and comparing the
shape of those crystals to the shape of common table salt and sugar.
Safety: YOU MUST WEAR GOGGLES THROUGHOUT THIS LAB!! H2SO4 and
KOH are both very dangerous!!
Day One-synthesis of alum crystals
1. Get a piece of the aluminum foil provided by your teacher. It should be about 1 gram.
2. Tear the foil into small pieces and put into a 250 mL beaker.
3. Slowly add 25 mL of 3 M KOH. Stir with a stir rod. At first no reaction will seem to
take place but WATCH OUT!!!! After a few seconds, a vigorous reaction will
proceed. Continue to stir until all of the foil has dissolved.
4. Filter the hot solution using a funnel and flask. Discard the contents of the funnel.
5. Slowly add 35 mL of 3 M H2SO4 to the flask. BE CAREFUL!!! You are adding a
concentrated acid to a strong base. It will get HOT!!!!!
6. Filter the solution again and let sit overnight. Crystal will form after some time.
Day Two-collection of the crystals
7. Discard the contents of the filter paper.
8. Collect the crystals from the flask by scraping them gently into another filter.
9. Pour 50 mL of a 50/50 alcohol/water mix over them.
10.Gently scrape them into a paper towel to dry them off. Discard the filter paper in
the trash and pour all liquids down the drain with lots of water.
11. Examine them under a microscope.
Analysis of crystals
12. Obtain some of the small alum crystals. If you don’t have small ones, borrow some
from another group
13. Look at the alum crystals underneath the microscope.
14. Obtain some crystals of normal table sale, NaC1 and look at them under the scope.
15. Obtain some crystals of normal sugar, C12H22O11, and look at them under the scope.
7
Alum Lab Analysis
AlumFormula:
Draw the shape you see under the microscope
Table SaltFormula:
Draw the shape you see under the microscope
SugarFormula:
Draw the shape you see under the microscope
Questions
1. Which of the above three crystals had repeating, simple shapes of various sizes?
2. Which of the above three crystals had no repeating simple shape?
3. Look at the formulas of the different atoms in the three crystals examined in this lab.
Why does it make sense that one should be different?
8
332 CHEMISTRY
TEGIF
THE EXCITING GAME OF IONIC FORMULAS
THE GAME: Use your puzzle pieces to build chemical formulas for Ionic compounds.
Write correct formulas and names for the compounds.
THE RULES FOR PLAY:
1. For the first round—
Player 1 locates and plays the cation(s)
Player 2 locates and plays the anion(s)
Player 3 checks to be sure the proper number of each type of ion has been played
Player 4 records the formula and name of the compound
2. For the second compound, player 1 becomes the recorder, player 2 does cations,
player 3 does anions, and player 4 is the checker.
3. The roles continue to rotate for each new compound until all the assigned
combinations of ions have formulas and names.
THE RULES FOR FORMULAS AND NAMES:
1. The sum of all positive and negative charges in a formula must equal zero. (The total
length of the positive puzzle piece side(s) must equal the total length of the negative
puzzle piece side(s)). They must form a rectangle.
2. In formulas, positive ion (cations) is written first; negative ions are written second.
(Positive puzzle pieces are placed on the left, negative puzzle pieces are placed on the
right).
3. If more than one of an ion is needed in a formula, the number of that type of ion is
shown as a subscript following the symbol of thee ion.
4. If a polyatomic ion needs a subscript, the formula for the ion must be placed inside
parentheses. The subscript follows and is outside of the parentheses.
(For example, the 2 nitrate ions in calcium nitrate are shown as Ca(NO3)2.]
5. In names of compounds, the name of the cation comes first; the name of the anion
comes second.
6. Names of binary compounds usually end in ―--ide‖. Names of compounds containing
three or more elements often end in --ate‖ or --ite‖, although there are some
common exceptions like:
NH4Br ammonium bromide
A1(OH)3 aluminum hydroxide
9
CATION
ANION
Magnesium
Mg2+
Aluminum
Nitrate
NO3Chloride
Iron (II)
Hydroxide
Iron (II)
Nitrate
Sodium
Sulfate
Potassium
Phosphate
Ammonium
Oxide
Magnesium
Sulfide
Iron (II)
Sulfate
Iron (III)
Sulfate
Potassium
Nitrate
Aluminum
Sulfate
Ammonium
Chloride
Iron (II)
Sulfide
Magnesium
Chloride
Sodium
Phosphate
FORMULA OF
COMPOUND
Mg(NO3)2
NAME OF
COMPOUND
Magnesium Nitrate
10
Naming Ionic Compounds Rules
An ionic compound is a compound that contains a cation and an anion.
Cation:
Anion:
The cation is always written first. The cation will be a metal and the anion
will be a nonmetal Metals are located on the ____________side of the
periodic table. The nonmetals are located on the ____________side of the
periodic table.
An ionic compound is composed of a metal and a nonmetal.
To write an ionic compound, perform the following steps in the order that
they are presented.
1. Always write the cation the way it is presented on the periodic table.
2. Determine whether the anion is a polyatomic ion by referring to your
polyatomic ion sheet.
Polyatomic ion:
Examples:
3. If the anion is not a polyatomic ion then write the name of the element
from the periodic table and drop the ending, example: sulfur becomes
sulf. Add the suffix an ―ide‖ to the anion, example: sulfide.
4. If the anion is a polyatomic ion then write the polyatomic ion as it
appears on the reference sheet as your anion.
5. Look at the cation. If the cation is a transition metal then a roman
numeral needs to be inserted. The Roman numeral refers to the charge,
super script, that the cation has.
11
WRITING FORMULAS
(CRISS-CROSS METHOD)
Name ______________
Write the formulas of the compounds produced from the listed ions.
CICO3-2
OHSO4-2
PO4-3
NO3Na+
NH4+
K+
Ca+2
Mg+2
Zn+2
Fe+3
AI+3
Co+3
Fe+2
H+
12
Chemistry
S-332
Name _________________
Ionic Compounds – Worksheet #1
Chemical formulas and names
Elements
Charge of each
Formula
Name
1. Ca, Br
2. Li, O
3. Ag, I
4. O, Ca
5. Zn, Cl
6. Cs, S
7. O, Al
8. Ba, N
9. P, Sr
10.S, Mg
Name
Charge of each
Formula
1. Francium Fluoride
2. Rubidium Oxide
3. Magnesium Chloride
4. Silver Sulfide
5. Strontium Selenide
13
Chemistry
S-332
Name _______________
Ionic Formulas – Worksheet # 2
(transition metals)
Name
Charge of each
Formula
Charge of each
Name
1. Vanadium (III) Oxide
2. Nickel (II) Bromide
3. Copper (II) Oxide
4. Potassium Nitride
5. Sliver Chloride
6. Lead (IV) Sulfide
7. Gold (III) Bromide
8. Manganese (I) Nitride
9. Barium Fluoride
10.Magnesium Iodide
Formula
1. Cu3N2
2. CoCl
3. Fe2O
4. Cs3N
5. CaS
14
Chemistry
S-332
Name _______________
Ionic Formulas – Worksheet #3
(polyatomic ions)
Name
Charge of each
Formula
Charge of each
Name
1. Magnesium Sulfate
2. Barium Chlorate
3. Sodium Nitrate
4. Copper (II) Phosphide
5. Iron (II) Oxide
6. Aluminum Chromate
7. Sliver Bisulfate
8. Sodium Bicarbonate
9. Calcium Carbonate
10. Iron (II) Nitride
Formula
1. CuSO4
2. KMnO4
3. CsNO3
4. Mg(OH)2
5. HNO3
15
Chemistry
S-332
Name _______________
Ionic Formulas – Worksheet #4
Formulas
Charge
Name
NaBr
MgO
CuS
FeCl
VI4
NiF3
Ca3N2
Zn3P2
Al2S3
BaCl2
Name
Charge
Formula
Copper (I) Sulfide
Iron (III) Oxide
Vanadium (VI) Phosphide
Chromium (IV) Bromide
Sliver Nitride
Potassium Chloride
Nickel (II) Phosphide
Manganese (VI) Nitride
16
Name the following ionic compounds.
1. CuSO4
2. KC1
3. BaBr2
4. Na3PO4
5. Zn(OH)2
6. NaC1
7. LiBr
8. CaC12
9. A1PO4
10. KC2H3O2
11. NH4NO3
12. ZnC12
13. CaO
14. AgC1
15. CrBr3
16. FeSO4
17. FeC13
18. FeBr
17
18
Name ____________________
Solubility Lab PLW
1. How much of the solid are you to put into the test tube? Draw this.
2. How much water are you to put into the test tube? Draw this.
3. Why would it be important to shake the tube for at least 2 minutes?
4. How can you tell if a substance has dissolved in water?
5. What would be some evidence of a substance that has NOT dissolved in
water?
6. Draw a picture of how an ionic crystal is arranged on the atomic level.
19
20
Name ______________________
Solubility
Purpose: To investigate the solubility in water of several ionic substances in
an effort to generate a set of ionic solubility rules.
Safety: Goggles and Aprons must be worn.
Procedure:
1. At your lab table should be test tubes and two different chemicals.
2. Using the scoopula, add a very small amount of the chemical to the test tube.
You should use just enough to cover the bottom rounded portion of the tube.
Using too much will give poor results.
3. Add water until the tube is about ¾ full.
4. Place a stopper on the tube and shake vigorously for at least 2 minutes.
5. Examine each tube and decide if the solid chemical was soluble and dissolved
or was insoluble and did not dissolve.
6. Discard the contents of the tube down the drain with lots of water and clean
out the tube.
7. Rotate around the room until all 14 chemicals have been tested.
8. Return to your original table and clean it up.
9. Using your results, try to come up with a generalized set of rules which govern
ionic solubility.
Tube
Compound
1
Calcium Chloride
2
Sodium Phosphate
3
Aluminum Oxide
4
Aluminum Nitrate
5
Calcium Carbonate
6
Calcium Phosphate
7
Sodium Carbonate
8
Potassium Bromide
9
Cobalt Carbonate
10
Zinc Nitrate
11
Magnesium Oxide
12
Ammonium Sulfate
13
Copper (II)Carbonate
14
Potassium Chromate
Formula
Soluble?
21
Name _______________________
Date ______________ Per, _____
Solubility Lab Analysis
1. List all of the salts that were soluble.
2. What aspect do all of ions above have in common?
3. List all of the salts that were insoluble
4. What aspect do all of the ions above have in common?
5. Finish the following statement:
An ionic salt will most likely be soluble in water and dissolve if…
22
Name ________________________
Conductivity Lab
Purpose: To investigate the conductivity in water of several ionic substances.
Safety: Goggles and Aprons must be worn.
Procedure:
1. At your lab table should be 250 mL beakers and two different chemicals.
2. Add a medium scoop of one chemical to a 250 mL beaker.
3. Add about 200 mL of water to the beaker with the chemical
4. Using a clean stirring rod, stir the beaker vigorously for about a minute.
5. Dip the conductivity probes into the beaker and see if the light goes on.
6. Dump the contents of the beaker down the drain with lots of water and clean
out the beaker.
7. Clean the probes with a beaker of clean water and dry them off.
8. Rotate around the room so that all 14 chemicals are tested.
9. Return to your original table and clean it up.
Tube
Compound
1
Calcium Chloride
2
Sodium Phosphate
3
Aluminum Oxide
4
Aluminum Nitrate
5
Calcium Carbonate
6
Calcium Phosphate
7
Sodium Carbonate
8
Potassium Bromide
9
Cobalt Carbonate
10
Zinc Nitrate
11
Magnesium Oxide
12
Ammonium Sulfate
13
Copper (II)Carbonate
14
Potassium Chromate
Formula
Conducts?
23
Name ________________________
Conductivity Lab Analysis
1. When an ionic substance dissolves in water, what happens to the crystal
structure of the ions?
2. Compare the results of this lab to the results of the solubility lab. What
trend do you notice?
3. Explain the results of this lab in terms of ionic bonding and solubility in
water. Why do the results seen in the lab make sense? Why does it make
sense that the ones that conducted electricity did so?
24
PLW Precipitate Lab
1. What is an aqueous solution?
2.
3. What ions are in an aqueous solution of sodium chloride?
4. Draw a picture of the ions present in each aqueous solution
CaCl2(aq)
K2SO4(aq)
5. What is a precipitate and how does it form?
6. Write the formula for the following compounds:
a) sodium carbonate_________________
b) sodium chloride__________________
c) copper (II) nitrate_________________
d) sodium phosphate_________________
e) zinc nitrate______________________
f) magnesium nitrate_________________
7.
Step H of the lab asks you to observe if a precipitate will form in the spot plate.
What are some observations that will indicate that a precipitate has formed?
8.
A set of students conducted an experiment very similar to your Precipitate Lab.
Several aqueous solutions were combined to test for a precipitate. The data table
below shows the results of each test. .
Aqueous
Solutions
Li2SO4
Fe(ClO3)2
Cu2CrO4
Al(NO3)3
Na2CO3
BaI2
White ppt
NR
White ppt
NR
Red ppt
NR
Geen ppt
NR
Blue ppt
a. Which two ionic compounds form a red precipitate when combined together?
b. When Na2CO3 is combined with Cu2CrO4, what is the result?
c. What happens when the solution BaI2 is combined with the solution Li2SO4 ?
25
26
Precipitates Lab
Purpose: In this lab you will be using the solubility rules to predict whether
combinations of solutions will form precipitates.
Background: Write the formulas for each of the following chemicals.
a) sodium carbonate
______________________
b) sodium chloride
______________________
c) copper (II) nitrate
______________________
d) sodium phosphate
______________________
e) zinc nitrate
______________________
f) magnesium nitrate
______________________
Procedure:
a) Obtain and CLEAN six test tubes and one spot plate. Be sure to rinse each with a little
DI water.
b) Mark each test tube with one of the above chemicals names.
c) Pour enough of each solution into the proper test tube so that the tube is about ¼ full.
d) Examine the grid on the next page.
e) You will notice that the top and left side row and column are left blank. Fill the
chemical formulas above into the top row and the left column. (Put them into correct
order, a-f)
f) For each blank space on the chart, find the two chemicals which intersect there.
g) Combine 4-5 drops of each chemical in a well of a spot plate.
h) Observe if a precipitate forms or not. If a precipitate is formed, write PPT. If no
reaction occurs, write NR.
i) Dispose of the excess chemicals. Spot plates should be filtered and excess solutions in
test tubes should be rinsed down the sink one at a time with lots of water.
27
Precipitates Lab (Continued)
Data: Write the names of the chemicals at the top and along the left. If a precipitate
forms, write PPT. If no reaction occurs, write NR.
a
b
X
X
X
X
X
X
X
X
X
X
X
d
d
e
f
Ionic
Formulas
a
b
c
d
e
f
X
X X
X X X
X X X X
Analysis:
Based on the above data, can you determine the rules which govern the formations of
precipitates? Think back to the solubility rules for ionic compounds.
Conclusion:
Write out a situation which summarizes the rules on the formation of precipitates.
28
Name _______________________
Precipitates prediction worksheet
Use the following data to determine whether a ppt will form. Indicate the
formula of the ppt.
1. Calcium Nitrate
2. Sodium Phosphate
4. Lithium Chromate
5. Iron (lll) Nitrate
Ions to be
mixed
2
1
2
3
4
5
1
x
x
x
x
x
3
x
x
x
x
3. Sodium Carbonate
4
x
x
x
5
x
x
x
29
30
Name __________________________
Date _______________ Per. ________
Chemical Bonding Unit Review
1. Identify each as an element or a compound:
Ca
H2 O
CH4
H2SO4
CaCO3
N2
Fe
NaC1
2. What charge will each element have as an ion?
Nitrogen
________________
Lithium _____________
Barium
________________
Fluorine ____________
3. How many valence electrons does each of the following elements have?
Hydrogen
________________
Calcium ____________
Neon
________________
Sulfur
____________
4. Which elements are chemically stable and why are they inert (non-reactive)?
5. For each of the species listed below, list the number of protons, neutrons, and
electrons in each atom or ion.
23
Na+1
p : _____
no: _____
e-: _____
+
79
Br
p : _____
no: _____
e-: _____
+
35
C1-1
p : _____
no: _____
e-: _____
+
84
Kr
p : _____
no: _____
e-: _____
+
6. Complete the statement by circling the correct words:
Ionic bonds form due to charge attractions from the (sharing of electrons /transfer
of electrons) between a (metal and a non-metal /2 non-metals /2 metals).
7. Write the names of the following ionic compounds:
Fe2O3
____________________
Ca3(PO4)2
___________________________
NH4NO3
______________________________
Pb12
__________________
31
Name ________________________
Date _____________ Per. _______
8. It is noticed that neither solid calcium chloride nor calcium oxide will conduct
electricity. However when calcium chloride is added to water, the resulting solution
conducts electricity. Calcium oxide, though, continues to be non-conductive even when
added to water. Explain this phenomenon.
9. Circle which of the following ionic solids will dissolve in water.
Na3PO4
CaCO3
K2SO4
A1(NO2)3
10. Circle which of the following ionic solids will conduct electricity in water.
A12(Cr2O7)2
LiC1
BaSO4
Pb(NO3)2
11. Below are listed chemical formulae for groups of two solutions. Circle which
groupings would form a precipitate. For each grouping, write the formula of the
precipitate formed (if any) and list any ions that are still left in the solution.
A
NaC1
Cu(NO3)2
B
Ba(OH)2
Li2SO4
C
K2CO3
FeBr3
D
A1(NO3)3
K2CrO4
PPT ___________
____________
_____________
____________
IONS
LEFT__________
____________
_____________
____________
12. Rank the following ionic solids in order of expected increasing melting points:
A1PO4
NaC1
MgF2
CaO
Mg3(PO4)2
13. Below are listed some lattice energies for various ionic compounds:
BeO 1200
CaO 500
SrO 300
Predict the lattice energy for magnesium oxide:________________________
What difference in the formulae of the crystals above could account for the
changes in lattice energy?
14. Define ion:
32
Camp Electron
To: Potential summer camp employees of Camp Electron
From: Miss Daisy, Head Camp Director
Concerning: Assignment of campers to cabins and bunks.
What is Camp Electron?
Camp Electron is a place for electrons, much like yourselves, to come in for
the summer and experience arts and crafts, swimming, nature hikes,
horseback riding, and to learn wilderness survival skills.
When is Camp Electron?
Camp Electron takes place each week through out the summer for electrons
only. Yes, we understand there are protons and neutrons out there too, but it
seems that these electrons are so tiny that they feel neglected. They often
seem to go unnoticed in comparison to the giant protons and neutrons.
Where is Camp Electron?
Camp Electron is located in the woods north of Oshkosh, Wisconsin. It is
near Peshtigo, Wisconsin. It was built back in 1968.
Why are you receiving this information?
Normally, Camp Electron retires many of its previous workers, but it seems
to be in a crunch for this upcoming summer. We’re in need of camp
employees. This memo is to explain to you the paper work that is needed at
Camp Electron in the event that you may be interested in applying for a job.
It is necessary for you to have knowledge on how to assign electrons to
their-cabins and their bunks. Applications will be available at the end of
class.
33
Please observe the following camp rules and regulations. A short
explanation of the camp layout is provided.
1. Each cabin at Camp Electron is numbered and lettered: 1s, 2s, 2p,
3s and so on.
2. The circles following the cabin designations represent the bunks in
each cabin.
3. Two campers (electrons) may sleep in each bunk.
4. We had a mudslide a few years back and moved some of the cabins
from the original locations. Due to our limited budget (and
somewhat lazy maintenance staff) the cabin numbers have not been
changed. Please don’t let this upset you. Just assigned the campers
(electrons) to their bunks using the following rules.
a. Each new camper (electron) is assigned to the lowest cabin
on the hill in the lowest level that still has bunk space
available. The lowest cabin is the one that is closest to the
bottom of the map. Again, we know the cabin numbers are
messed up. Cabin 3d is really higher than cabin 4s. Cabin 4d
really is higher than cabin 5s and so. A cabin is full when all
of its bunks (circles) contain two campers (electrons).
b. Please remember-NO MORE THAN TWO CAMPERS IN
A BUNK. We don’t want to crowd them too much.
c. Don’t assign two campers (electrons) to the same bunk in a
cabin until all of the bunks in that cabin contain one camper.
Look at the 3d, for example. Each bunk (circle) must be
assigned one camper before you start pairing campers up.
Don’t crowd the campers before you have to.
We hope that you will consider a potential job as a camp counselor this
upcoming summer. Since the landslide we’ve been having trouble keeping
camp counselors for more than one summer. The cabin numbering system
34
seems to be the main problem, but we’re sure that you can handle the job
based on your teacher’s recommendations. Good luck and we hope to see
you this summer!
Electron summer Camp Cabins and Bunks
7p O O O
6d
OOOOO
5f
OOOOOOO
7s O ___________________
_____________________________________________________________Level 7____
6p O O O
OOOOO
5d
4f
OOOOOOO
6s O______________________
_____________________________________________________________Level 6___
5p O O O
4d
OOOOO
5s O _______
_____________________________________________________________Level 5____
4p O O O
3d
OOOOO
4s O_______
_____________________________________________________________Level 4____
3p O O O
3s O __
_____________________________________________________________Level 3____
2p O O O
2s O ___
_____________________________________________________________Level 2____
1s O_________________________________________________________ Level 1____
35
36
Camp Electron
Weekly Bunk Assignment
Summer 2010
To test your ability to assign campers (electrons) to their appropriate bunks within the
camp, below you will find the numbers for the first 14 weeks of this past summer. With a
partner, practice assigning campers (electrons) to the bunks within the cabins and then
share your results with the class.
Remember, each camper (electron) is assigned to the lowest cabin on the hill in the
lowest level bunk available. No one is assigned the top bunk until all the bottom bunks
are filled and no more campers (electrons) to a bunk.
Week #
1
# of Campers
N-7
Bunk Assignment
Head Office notation
1s2 2s2 2p3
1s 2s
2
P-15
3
F-9
4
Cu-29
5
Mg-12
6
C-6
7
K-19
8
Fe-26
9
O-8
2p
37
10
Cl-17
11
Ne-10
12
Ca-20
13
Al-13
14
Zn-30
38
Electron Configuration
What elements correspond to each of the following electron configurations?
1. 1s2 2s2 2p4
2. 1s2 2s2
3. 1s2 2s2 2p6 3s2 3p3
4. 1s2 2s2 2p6 3s2 3p6 4s2 3d5
5. 1s2 2s2 2p6 3s2 3p6 4s1
6. 1s2 2s2 2p6 3s2 3p6 4s2 3d10 4p6 5s2 4d3
7. 1s2 2s2 2p6 3s2 3p6 4s2 3d10 4p65s2 4d10 5p6 6s2
8. 1s2 2s2 2p6 3s2 3p6 4s2 3d10 4p4
Write the electron configuration found in each of the following atoms.
1. oxygen
11. aluminum
2. chlorine
12. chromium
3. titanium
13. scandium
4. beryllium
14. phosphorous
5. cobalt
15. zinc
6. calcium
16. bromine
7. strontium
17. potassium
8. nickel
18. vanadium
9. silicon
19. gallium
10. rubidium
20. selenium
39
Electron Configuration Practice
1. Sn
2. Ge+2
3. Te+2
4. Te-2
5, Which is more stable # 3 or # 4? Why?
6. Ne
7. Mg+2
8. Mg-2
9. Co+
10. Co11. Mo+3
12. Mo+
13. Mo
14. Cs
15. Er
16. Hg
17. At+
18. At19. Which is more stable #17 or # 18?
20. What element has a +2 charge and has configuration of 1s22s22p3?
21. What element has a -2 charge and has configuration of 1s2s22p3?
22. What element has a -3 charge and has configuration of [Kr] 5s24d7?
23. Os-3
24. U
40
Electron Configuration Battleship®
The idea for adapting the Battleship® game to Chemistry comes from Justin
Field of Oregon at ChemEd ’01; Battleship® are games by the MiltonBradley Company.
First some practice so you can hope to WIN!
Element
Configuration
Ti
1s22s22p63s23p64s23d2
Short Cut
Configuration
[Ar] 4s23d2
Valence
Electrons
4s23d2
Be
1s22s22p63s23p64s1
5s24d105p4
Ce
3s23p6
1s22s22p63s23p64s2
3d104p65s24d105p6
6s24f145d106p67s25f7
[Kr] 5d24d4
41
Game Rules:
1. You will work with a partner to play Battleship®. The goal is to
determine where your partner’s ships are on their periodic table.
2. First you need to privately ―hide‖ your six ships on the periodic
table by highlighting them with a marker. The ship sizes are:
a. TWO ships are three spaces
b. TWO ships are four spaces
c. TWO ships are five spaces
The ships may be placed on the periodic table horizontally (along a
period) of vertically (along a family).
3. Fold the periodic table and place in a standing textbook for
privacy.
4. You and your partner will take turns guessing the ―coordinates‖ of
the hidden ―ships‖. You will guess by………
a. First, Student A may guess 3s23p4. You may state either
full configuration, short cut configuration or valence
electrons. It is best to use different configurations each
time to practice all different types.
b. Student B will confirm the element saying, Sulfur. After
confirmation Student B will say ―HIT‖ (If they hit your
battleship) or ―MISS‖.
c. Both students must keep track of all guesses in the
following table.
5. The game ends when all of one players ships are sunk or after time
is called.
42
Electron Configuration Battleship®
Player
Guess
Example: [Ne] 3s23p4
Reply
Sulfur
Hit
Miss
X
A
1
2
3
4
5
6
7
8
9
10
11
12
13
14
15
16
17
18
18
20
B
1
2
3
4
5
6
7
8
9
10
11
12
13
14
15
16
17
18
19
20
43
Ionic Bonding Notes
44
Ionic Bonding Notes
45