CHM 1032C Tentative Grading Outline Fall 2015
Chapter 3 Ionic Compounds Homework Packet
A. _____ (03) e-1 Configuration of Ions-lecture (3.1-3.3) Answers
B.
_____ (02) Periodic
Ionic Character-Section 3.2 Answers
C._____ (02)
Bond
Recognition/Compound Classification-Sections 3.3, 4.1Answers
D _____(02) Binary Ionic Compounds-Section 3.9 Answers
E. _____(05) Polyatomic Ions-Section – section 3.8 Answers
F. _____(04) Ternary Ionic Compounds-Section 3.9 Answers
G. _____(02) Binary Acids/ Ternary Oxyacids-Section 3.11 Answers
_______(20)
Chapter 3 Total
Chapter Three: Part A: Electron
Configuration of Ions 3 points
Given
the following ions, use arrows to fill-in the electron configuration of the
ion, then rewrite the configuration into the chemist’s shorthand:
1. Cl1- ion Chemist Shorthand:
___________________________
2. K1+ ion Chemist
Shorthand: _____________________________
3. H1+ ion Chemist
Shorthand: _____________________________
4. H1-ion Chemist Shorthand: _____________________________
Chapter
Three: Part B Periodic Ionic Properties 2
points
Using a periodic chart, write the ionic character (monoatomic ionic
charge) of the following elements: (The number
before the element is its atomic number)
1. 19 K ________ 6. 9F _____
2. 20Ca _______ 7. 1H _____
_____
3. 7N _______ 8. 16S _____
4. 17Cl _______ 9. 10Ne _____
5. 53I ______ 10. 15P _____
Chapter Three: Part C Bond Recognition
2 Points
Read the short
discussion in Sections 3.1 and 4.1 on the difference between Ionic and covalent
bonding.
There are three types of chemical bonds:
Ionic,
Covalent, and Metallic.
There is a
simpler way to predict if two atoms will transfer their electrons or share
their electron in pairs making a compound. Read about the Pauling’s Scale of Electronegativity
in Section 4.9. Corwin Figure
12.9 shows the electronegativity
of each element on the periodic chart. This table will be needed in Chapter 4
Part II Bond Polarity.
If
the difference in electronegativity
between two atoms is
greater than 1.8 (Corwin), the electrons will transfer from one
atom to the other to make ions and Ionic
Compounds. Ionic (sometimes called Electrovalent) Compounds are also called
salts
and in nature they are called minerals
and in Sports medicine Body Electrolytes. We will over simplify
this concept to say if a metal meets a nonmetal ionic bonds are formed (Just a
Rule of Thumb)(if a table of electronegativity is not included). Hein (14th)
states on page 227 if the difference in electronegativity is greater than 2.0
the bonding is strongly ionic, while less than 1.5 strongly covalent. Then he
states between 1.7-1.9 the bonding will be more ionic than covalent.
For this course, if the difference between the electronegativity of two atoms is less than 1.7 then the two atoms will share electrons in pairs. Two types of sharing bonds are formed. Metallic and Covalent.
Metallic Bonds are
formed when two metals share electrons such as alloys of metals. 24 karat gold
is pure gold and is very soft. But Jewelry is usually 10-18
Karat Gold, meaning that another metal is mixed with gold to make the solid
harder. We will not study Metallic Bonds in this course, but you should
know that two metals share electrons in pairs to make Metallic Bonds.
“Metallic
bonding occurs as a result of electromagnetism
and describes the electrostatic attractive force that occurs between conduction electrons (in the form of an
electron cloud of delocalized electrons) and positively charged
metal ions. It may be described as the sharing of free electrons among a lattice
of positively charged ions (cations). In a more quantum-mechanical view, the conduction electrons
divide their density equally over all atoms that function as neutral
(non-charged) entities.[citation needed] Metallic
bonding accounts for many physical properties of metals, such as strength, ductility, thermal and electrical resistivity and
conductivity, opacity, and luster.[1][2][3][4]
Metallic
bonding is not the only type of chemical
bonding a metal can exhibit, even as a pure substance. For example,
elemental gallium
consists of covalently-bound pairs of atoms in both liquid and solid
state—these pairs form a crystal lattice with metallic bonding between them.
Another example of a metal–metal covalent bond is mercurous
ion (Hg2+2).“
Covalent Bonds are formed when two nonmetals bond together. The elements carbon, oxygen, hydrogen, sulfur, nitrogen, phosphorus, chlorine, and bromine will be the main nonmetals studied in drawing dot structures of molecules. Bonds between these nonmetals are always Covalent.
Part
C of Chapter 3 should now be easy. Predict what type of bond will be made if
two atoms combine:
In General:
Metal-Metal = Metallic Bond (example: Ag(5)-Au(14)-Cu(5) = 14 Karat Gold)
Metal-Nonmetal = Ionic Bond (example: Na-Cl)
Nonmetal-nonmetal
= Covalent Bond
(example: H2O)
Chapter Three: Part C Sample Bond Recognition 2 points
Using
a periodic chart (Rule of Thumb), predict the bond that would form between the
two elements:
1. Fe-Al ________________
2. P-S
________________
3. C-O ________________
4. B-Cl ________________
5. K-I ________________
For the following element pairs use the electronegativity table below to determine if the bond is ionic or covalent.
6. Na-P ________________ 9. P-H ________________
7. Ca-Br ________________ 10.
Be-Cl
________________
8. Ge-O ________________
Chapter 3: PART D:
BINARY (IONIC) COMPOUNDS
Most Common Ionic
Charges for Monatomic Ions
PART D:
BINARY (IONIC) COMPOUNDS (Salts)(Minerals)
The element written first
in either the name or the formula is a metal.
The element written second
is a nonmetal.
Salts are metallic and
nonmetallic ionic compounds.
There are no molecules of salts-just
macro ionic lattices.
Name the metallic element.
If the metallic element has more than one ionic state, write a ROMAN NUMERAL after
the element’s name (In Parenthesis) to indicate which charge state the metallic
element is using to form the compound.
Drop the suffix
off the nonmetal’s name and add -ide which indicates the
salt is binary (exceptions: cyanide & hydroxide which are polyatomic ions).
No prefixes are used to indicate how many atoms are present in the formula.
Examples:
NaCl
Sodium Chloride (table salt)
Al2O3
Aluminum oxide
FeS Iron(II) sulfide (Note: No
space between the metal and the parenthesis)
Fe2O3
Iron(III) oxide (rust)
To write the formula from the name of the salt
use the following procedure:
(a) Write the symbols (or
formulas for radicals) of the ions represented
For Example:
Calcium nitride
(a)
Ca N
(b) Use the periodic chart to write the ion charge of each element (or polyatomic ion) as superscripts:
Ca+2
N-3
(c ) Find the L.C.M. (Least common multiple) of the positive and negative charge.
The LCM is the smallest number that both charges will decide into evenly. The LCM is the total electrons transferred. Therefore, it represents the total positive charge created by the metallic ions and the total negative charge created by the nonmetallic ions. This may be proved by drawing the dot structure of the compound showing all electrons transferred.
The LCM of +2
and -3 is 6, therefore 6 e-1
are transferred creating a total positive charge of +6, and the total negative charge
of -6
--> 6e-1-->
Ca+2 N-3
(d) Divide the LCM by the positive
charge, this dividend will represent the subscript behind the
metallic ion in the formula.
+6 divided by +2 = 3;
therefore half of the formula is: Ca3Nx
(e) Divide the LCM by the negative charge, this dividend will represent the number of nonmetallic ions in the formula.
-6 divided by -3 = 2; therefore the other half of the formula is: Ca3N2
Example:
Potassium
phosphide
Write Symbols
and the Charges:
K+1 P -3
LCM:
3
Balance the chemical formula:
K3P
In addition to working the sample tests, you must practice on writing the names and formulas for Ionic Compounds. He following are online homework for 2 points each:
D. Binary Ionic
Names:
http://www.fscj.me/Nomenclature/BinarySalts/32BinaryIonicJT.html
D1. Binary
Ionic Formulas:
http://www.northcampus.net/Nomenclature/BinaryIonicFormula/32BinaryIonicFormula.html
Submit
grades on separate grading Sheet when taking after taking Chapter 4 exam
Chapter
Three: Part D Binary Ionic Compounds 2 points
Using
a periodic chart, write the names or the balanced formulas for the following
compounds depending on whether the formula or the name is given:
1. Copper II phosphide _________ (Cupric phosphide)
2. Iron III Oxide (rust) _________ (Ferric Oxide)
3. Lead IV sulfide _________ (Plumbic sulfide)
4. Sodium chloride _________
5. Tin II fluoride (in toothpaste) _________ (Stannous Fluoride)
6. MgCl2 ________________________
7. NiF2 ________________________
8. K3N ________________________
9. Al2O3 ________________________
10.
CuBr ________________________
Online Study Guide: http://www.fccj.us/chm1025/AssignmentOutline/M4PartD.htm
Chapter 3: PART E:
Polyatomic Ions
Ion Flowchart
You can predict the Monoatomic Anions or Cations by the position the element resides on the periodic chart. If the ion come from a Representative Element (IA-VIIIA) there is one and only one ionic charge. If cation is a transitional metal with several different charges you have to rely on the Name
Periodic
Table of Selected Ions
Note the charges for groups IA,
IIA,
By now you should have
practiced: C-3
Part A, then try C-3 Part D and write the formulas for Binary Ionic Compounds.
Almost all chemistry
textbooks have sections dedicated to polyatomic ions and include a list of
common ions.
What
is a polyatomic ion?
A group of atoms bound together (covalent bonds)
that bears an overall negative or positive charge.
Corwin (7th) suggests that you use flash cards listing the name on one side and the formula with its charge on the other to aide your memorization of these formulas. Most chemistry teachers require you to know some of the common polyatomic ions by the end of the course whether it is from repetition of use with a help table or from memory from the first day of introduction. Below are tables from various chemistry books used:
Polyatomic Ion
Charts from Textbooks
2045 McMurray: Table
3.2 1025 Corwin: Table 7.03 1032 McMurry GOB: Table 3.
2045 Silverberg: Table
2.5 1020 Tillery:
Table
9.3 1025 Hein Table 6.5
2045 Kotz: Table 3.1 1020 Hill: Table
5.04
Here is a sample polyatomic ion table:
Hill’s
Table 5.4 (and Hill suggest for you to memorize the
entire table):
After you start memorizing, during the course
the formulas may be swimming in your head and the charges too. To write balance
Ternary Ionic Compounds, you must be able to write the formula and the charge
of each polyatomic ion required.
Corwin suggests there is only
one (Hill has two) common polyatomic Cation(s) and both end in –ium suffix. He notes
most of the Anions have an –ate
suffix, while a few have –ite, and two have –ide in their name. How do we accomplish this list?
Our McMurry GOB text suggests
are students should learn the common polyatomic ions in Chapter 3 Section 3.8 Table
3.3:
Knowing dot structures of
polyatomic ions McMurry GOB Section 4.7) (Corwin Chapter 12 section 12.5), and
some keen observations you can boil it down to six questions:
1. What is the formula
for the –ate polyatomic ion?
2. What is the charge
on –ate polyatomic ion?
3. What happens when you attach hydrogen atom(s) to the polyatomic
2- and 3-
anions?
4. What does –ite mean?
5. How do the hypo-
and per- prefixes
apply to polyatomic ions?
6. What are the two –ide polyatomic ions and
two -ium positive
Anions?
Your First task is to
memorize the formulas and the charges for the polyatomic ions in your text book
(Table 3.3) for a short test:
Progressive
Polyatomic Ions McMuury GOB (1 point)
Name |
Formula
with charge |
Acetate ion |
|
Ammonium ion |
|
Carbonate ion |
|
Hydrogen Carbonate ion |
|
Chromate ion |
|
Dichromate ion |
|
Cyanide ion |
|
Hydroxide ion |
|
Hypochlorite ion |
|
Nitrate ion |
|
Nitrite ion |
|
Oxalate ion |
|
Permanganate ion |
|
Phosphate ion |
|
Hydrogen |
|
Dihydrogen Phosphate ion |
|
Sulfate ion
|
|
Hydrogen sulfate
ion |
|
Sulfite ion |
|
Progressive Polyatomic
Ions Corwin (1 point))
Write the
formula and the charge for the following polyatomic ions: Corwin(Table
6.3) 1 point if your text is Corwin.
Name |
Formula with charge |
Acetate |
|
Ammonium |
|
Carbonate |
|
Chlorate |
|
Chlorite |
|
Chromate |
|
Cyanide |
|
Dichromate |
|
Hydrogen Carbonate |
|
Hydrogen sulfate |
|
Hydroxide |
|
Hypochlorite
|
|
Nitrate |
|
Nitrite |
|
Perchlorate |
|
Permanganate |
|
Phosphate |
|
Sulfate |
|
Sulfite |
|
Progressive
Polyatomic Ions Hein (1 point)
Write the formula and the charge for the following
polyatomic ions: Hein(Table 6.5 page 109) 1 point if
Hein Text
Name |
Formula
with charge |
Acetate |
|
Ammonium |
|
Arsenate |
|
Carbonate |
|
Chlorate |
|
Chromate |
|
Cyanide |
|
Dichromate |
|
Hydrogen Carbonate |
|
Hydrogen sulfate |
|
Hydroxide |
|
Nitrate |
|
Nitrite |
|
Permanganate |
|
Phosphate |
|
Sulfate |
|
Sulfite |
|
So: it is time for you to discover, what I saw over 50 years ago. It is not in any textbook. The books just say know or memorize these tables. Go to:
http://www.fccj.us/PolyatomicIons/polyionformula.html
When you go to the site above (which looks like the
image below), click on the X for each polyatomic ion and note if the # of
oxygen atoms are three or four in the formula.
To
expose the threes and the fours in the lower left hand corner (Taylor’s ¾ rule)
click the numbers 0,1…8,9 Border three rule, then
1,2..5,6 in the box of six rule. Also do the 0,1…7,8
Transitional O4 Rule.
Taylor’s
¾ rule is summarized at:
http://www.fccj.us/PolyatomicIons/Taylor34OxygenRuleHandout.htm
Then
do the same for the box just to the right of Taylor’s ¾ Rule, and discover
Taylor’s Charge Rule.
Taylor’s
Charge Rule is summarized at:
http://www.fccj.us/PolyatomicIons/TaylorChargeRuleHandout.htm
The
story behind how your instructor related the periodic table to a long list of
polyions, read the abstract for his talk at 2YC3:
http://www.fccj.us/PolyatomicIons/2YC3HowTeachPolyatomiIonsInChemistry.htm
Now
comes the big task!
You
may either memorize 55 polyatomic ions or learn to read the periodic table with
six rules and be able to write formulas and the charges for the required 1025/1032/2045
list:
http://www.fscj.me/PolyatomicIons/25MemorizeList.htm
Either
make a hard copy set of polyatomic ion flash cards or practice the 65
polyatomic ions Flash Card web site for 2 points at:
http://www.fscj.me/Nomenclature/PolyatomicIonFormula/ProgressivePolyatomicIonFormula.html
Chapter
Three: Part E Polyatomic Ions 2 points
Using
a periodic chart write the names or formulas of the following polyatomic ions
depending on whether the formula or name is given:
1. CO32- _____________________
2. SO32- _____________________
3.
PO33- _____________________
4. ClO31- _____________________
5. NO31- _____________________
6. Hydroxide ________
7. Ammonium ________
8. Hypochlorite ________
9. Nitrite ________
10. Phosphate ________
Textbook
(Corwin 7th) Reference: Chapter 6 Section 6.3 Table 6.3 Optional End of Chapter p184 #13-18
Hein
(14th): Section 6.5 Memorize the formulas and charges of Hein Table
6.5 (18 ions)
Online
Required Homework
(2 Points Each):
E:
Polyatomic Ion Names Homework: http://www.northcampus.net/Nomenclature/PolyatomicIon/32PolyatomicIon.html
E1.
Polyatomic Ion Formulas: http://www.northcampus.net/Nomenclature/PolyatomicIonFormula/32PolyatomicIonFormula.html
Submit
grades on separate grading Sheet (Goldenrod) when taking Chapter 4 exam or
download the form from:
http://www.fscj.me/chm1032/NomenclatureGradingLabForm.htm
CHM
1032C Chapter 3 Homework Packet
In chemistry,
a ternary compound is a compound containing three different elements. An
example of this is sodium phosphate, Na3PO4.
The sodium ion has a charge of 1+ and the phosphate ion has a charge of 3-.
Therefore, three sodium ions are needed to balance the charge of one phosphate
ion. Another example of a ternary compound is calcium carbonate. In naming and
writing the formulas for ternary compounds, we follow rules that are similar to
binary compounds.(CaCO3).
Ste that uses least common multiple balance method:
http://web.tenafly.k12.nj.us/chemquest2/ternary_compounds.htm
Sites (You-tubes) that use the crossing method(UGH):
You-Tube: http://www.youtube.com/watch?v=8eJtYffLWKc
Another You-Tube: http://www.youtube.com/watch?v=cXyxrzUw99A
Chapter 3: Part F Ternary Ionic Compounds 2 points
Using
a periodic chart write the names or formulas of the following compounds
depending on whether the formula or name is given:
1. Na2CO3 _____________________
2. K2SO4 _____________________
3. (NH4)3PO4 _____________________
4. Ca(ClO3)2 _____________________
5. CuNO3 _____________________
6. Aluminum Hydroxide ____________
7. Ammonium carbonate ____________
8. Sodium Hypochlorite ____________
9. Magnesium Nitrate ____________
10. Iron III sulfite _____________
McMurry GOB:
Sections 3.9 & 3.10/Corwin Text Sections 6.4 & 6.6
Online
Homework (2 Points Each Required):
F:
Ternary Ionic Compound Names Homework: http://www.northcampus.net/Nomenclature/TernarySalts/32ternaryIonic.html
F1.
Ternary Ionic Compound Formulas: http://www.northcampus.net/Nomenclature/TernarySaltFormula/32ternaryionicformula.html
Submit
grades on separate grading Sheet when taking Chapter-4 Exam
Chapter 3 Part G: Binary/Ternary Acids
What is an acid?
A substance that releases hydrogen ions (H+) when dissolved in water. Inorganic formulas of acids have ionizable hydrogen(s) written first in the formula.
Strong Acids Weak Acids
Strong acids ionize 100% in a water solution, while Weak Acids
ionize
less than 5% in a water solution.
There are Binary/Ternary Acid online homeworks for your practice for M-4 Part G:
G: Binary/Ternary Acid Names:
http://www.northcampus.net/Nomenclature/Acids/32Acids.html
G1: Binary/Ternary Acid Formulas:
http://www.northcampus.net/Nomenclature/AcidFormulas/32AcidFormulas.html
( Chapter 6 Bishop
Sections 6.3-6.4 )give you instructions for naming and writing formulas of
acids. );
(Chapter 6 Corwin 7th covers
binary acids in section 6.8; while section 6.9 covers ternary acids.) (Hein 14th
covers acids in section 6.6.
A brief tutorial for names and formulas of acids follows:
If hydrogen is written first in a chemical formula, there is two
ways to name the compound. As a pure
molecular compound or as an aqueous acid:
If the compound is a pure molecular compound
then you name it just as if it were an ionic compound:
HCl
hydrogen chloride H2CO3
hydrogen carbonate
HClO
hydrogen hypochlorite H2SO4
hydrogen sulfate
HClO2
hydrogen chlorite H2SO3 hydrogen sulfite
HClO3
hydrogen chlorate HC2H3O2
hydrogen acetate
HClO4
hydrogen Perchlorate H2C2O4 hydrogen oxalate
H3PO4
hydrogen phosphate HBr hydrogen bromide
HF hydrogen fluoride
Writing hydrogen first in a chemical formula indicates
that when you dissolve the compound in water, a water molecule has the
ability to pull the hydrogen off (from
strong electronegative elements like oxygen) the molecule HXO3
and creating hydronium ions, H3O1+ and a negative
ion XO31- (cation).
The way you indicate this ionic solution is to write the formula followed by (aq) meaning a water solution: HXO3 (aq) .
The
first step is to drop the first word hydrogen and
add a second word acid:
HCl
hydrogen chloride acid (aq)
HClO
hydrogen hypochlorite acid (aq)
HClO2
hydrogen chlorite acid (aq)
HClO3
hydrogen chlorate acid (aq)
HClO4
hydrogen perchlorate acid (aq)
H3PO4
hydrogen phosphate acid (aq)
H2CO3
hydrogen carbonate acid (aq)
H2SO4
hydrogen sulfate acid (aq)
H2SO3 hydrogen sulfite acid (aq)
HC2H3O2
hydrogen acetate acid (aq)
H2C2O4 hydrogen oxalate acid (aq)
HBr hydrogen bromide acid (aq)
HF hydrogen fluoride acid (aq)
The next step is to drop the suffix from the cation and make the following substitution with another suffix:
Change the -ate to -ic
Change the -ite to -ous
but the instead of coming up with a
third suffix for -ide , they
reused the -ic for -ide and
added a prefix hydro- (Do not
get this confused with the prefix hypo- which
means 'under'.)
HCl
hydrochloric acid (aq)
HClO
hypochlorous acid (aq)
HClO2 chlorous acid (aq)
HClO3
chloric acid (aq)
HClO4
perchloric acid (aq)
H3PO4
phosphoric acid (aq) (Put the -or- syllable back in the name)
H2CO3
carbonic acid (aq)
H2SO4
sulfuric acid (aq) (Put the -ur- syllable back in the name)
H2SO3 sulfurous acid (aq) (Put the -
HC2H3O2
acetic acid (aq) (Notice the three
hydrogens written after carbon are NOT ionizable and not written first in the
formula)
H2C2O4 oxalic acid (aq)
HBr hydrobromic acid (aq)
HF hydrofluoric acid (aq)
On Corwin 7th
page 185 Questions 49-56 will give you more practice on writing names and
formulas of acids.
At the end
of chapter 6 Hein 14th exercises 17, 18, 19, and 20 pages 116-117
are additional acid nomenclature problems.
McMurry GOB introduces
acids in Section 3.11, then goes into acids but does teach how to name in Chapter 10.
Chapter 3: Part G Binary/Ternary Acids 2 points
Using
a periodic chart write the names or formulas of the following compounds
depending on whether the formula or name is given:
1. HCl
_____________________
2. H2SO4 ____________________
3. HNO3 _____________________
4. HNO2 ___________________
5. H2CO3 ___________________
6. Hypochlorous acid _________
7. Phosphoric acid _________
8. Sulfurous acid _________
9. Perchloric acid _________
10. Hydrofluoric acid ________
Corwin 7th
Text Sections 6.8 and 6.9
Optional Additional Homework: p 185 Q
#49-56
Online
Homework (2 Points Each Required):
G:
Binary/Ternary Acid Names Homework: http://www.northcampus.net/Nomenclature/Acids/32Acids.html
G1.
Binary/Ternary Acid Formulas:
http://www.northcampus.net/Nomenclature/AcidFormulas/32AcidFormulas.html
Submit
grades on separate grading Sheet when taking Chapter-4 Exam
Online Study Guide:
http://www.fccj.us/chm1025/AssignmentOutline/M4PartG.htm