Alist – Unit 5 (Chap 7 from the book)
NAME _______________
Wednesday Sept 23 Begin Lecture/ Ionic bonds/ charge rules Practice problems –
Binary ionic with & w/o transitions
Thursday Sept 24 Continue working problems include transitions
Friday Sept 25 Practice naming with polyatomics / work on choices / make flash
cards
Monday Sept 28 Minilab Name acids - practice
Tuesday Sept 29 Quiz on naming - Day 1 Analytical lab
Wednesday Sept 30 Worktime/ Flow chart for nomenclature
Thursday Oct 1 Day 2 Analytical lab
Friday Oct 2 Homecoming activities (?) / Worktime
Monday Oct 5 Lab Report due Review
Tuesday Oct 6 TEST – NB due
Essential questions/Key questions:
EQ How are compounds named and formulas written?
KQ What are the ionic charges of any element on the table?
EQ Why are valence electrons related to the nature of the chemical bond?
KQ How does an ionic bond compare to a covalent bond?
GA performance standard SC1
c. Predict formulas for stable ionic compounds based on the balance of
charges.
d. Use IUPAC nomenclature for chemical names & formulas for ionic
compounds.
Checklist of stuff to know:
A) Explain how an ionic bond forms.
B) Know the charges (aka 0xidation number) as well as the exceptions for each element.
C) What are the rules for naming and writing formulas for ionic compounds?
D) Explain the different characteristics of metals/nonmetals/metalloids and the pattern
on the periodic table.
E) Know the names for each of the groups on the periodic table.
Vocabulary
Chemical formula, Compound, Cation, Anion, Ionic bond,
Polyatomic ion, Monatomic ion, valence electron, acid
Classwork/homework – all due on Tuesday, Oct 6
Graphic org for groups
Note guide / Handout for Binary ionic
PI flashcards
Handout for Ternary ionic/ acids
Flowchart for writing formulas of ionic compounds
+ choose 2 from the following:
1) Draw a one panel cartoon of a cation bonding with an anion in the correct ratio. Show the
transfer of electrons. Use a minimum of 4 colors and write a caption. It doesn’t have to be funny,
but if you can make me smile it is always a good thing.
2) Write 2 acrostic poems. One needs to include the word cation and the other needs to include
the word anion. Phrases in your poems should describe cations and anions.
3) Write a one page paper on the history of the IUPAC. What is their most recent contribution to
chemistry? Include 2 references minimum. Wikipedia is ok with me for one of your references, but
you may not access it from school.
4) Write a minimum 3 verse song + chorus that includes all nine vocabulary words. You may perform
if you like, but you don’t have to get credit. Turn in your lyrics.
5) Choose one of the groups on the periodic table to research. Create a flyer in Publisher that
includes several facts about the group you chose. Include similar traits of each element in the
group, uses for each element in the group and any exceptions. Include a minimum of three
graphics/pictures and 2 references. You may email it to me if you can’t print.
6) Teach the naming system to your parent/guardian. Have them explain the formula for any
Binary Ionic Compound in 4 or 5 sentences. Below his/her paragraph, he/she should write, “My child
understands how compounds are named and can explain it to me.” Have them sign it and include this
with your notebook.
Lab reports are due separately on Monday Oct 5 at the beginning of your class period. Late
grades are given for reports turned in later on in the period.
Chemical Nomenclature and Formula Writing
Chemical nomenclature is the system that chemists use to identify and name compounds. Compounds can
have two types of names: systematic names (names that identify the chemical composition of a chemical
compound) and common names (traditional names based on historical discovery or reactivity behavior).
For example, N2O has both a systematic name (dinitrogen monoxide) and a common name (laughing
gas).
If every substance were assigned a common name, chemists would be expected to memorize over nine
million names! This is why chemists generally prefer systematic names for identifying compounds. The
International Union of Pure and Applied Chemistry (IUPAC, see http://www.iupac.com) was founded in
1921 to provide a system of chemical nomenclature for scientists. IUPAC nomenclature rules can
provide valuable structural and reactivity information. On the other hand, most people would be hard
pressed to call dihydrogen monoxide by any other name but water, so both types of nomenclature have
their place.
Nomenclature leads naturally to formula writing. Compounds exist in distinct combinations of elements,
and knowing the proper combinations of elements is essential in chemistry. We expect sodium chloride to
be NaCl and not Na2Cl or NaCl2; knowing which combination or combinations exist in nature is crucial.
Binary ionic compounds – include one cation and one anion – named systematically
Ternary ionic compounds – include at least one polyatomic ion and another ion
Binary Covalent compounds – include 2 nonmetals – named with Greek prefixes
Organic compounds – include carbon – organic naming system
All ionic compounds have an overall charge of ________.
Examples: Binary ionics:
Examples: Binary ionics w/ transition metals:
Examples: Ternary ionics:
Binary Ionic compounds practice
NAME
cation
anion
1) Lithium bromide
chemical formula
_____ ______
2) Magnesium fluoride _____ ______
3) Potassium oxide _____ ______
___________________
___________________
___________________
4) Calcium sulfide _____ ______
___________________
5) Aluminum iodide _____ ______
___________________
6) Barium bromide _____ ______
___________________
7) Aluminum sulfide _____ ______
___________________
8) Calcium phosphide _____ ______
9)
Lithium selenide _____ ______
10) Magnesium arsenide _____ ______
___________________
___________________
___________________
11) Aluminum fluoride _____ ______
___________________
12) Beryllium iodide _____ ______
___________________
13) Barium carbide _____ ______
___________________
Binary ionics with Roman Numerals
1) Copper (I) oxide _____ ______
___________________
2) Copper (II) oxide_____ ______
__________________
3) Iron (II) oxide ______ _______
___________________
4) Iron(III) oxide _____ ______
__________________
5) Lead (IV) chloride_____ ______
__________________
6) Lead (II) fluoride_____ ______
__________________
7) _______________
_____ ______
NiS
8) _______________
_____ ______
Ni2S3
9) _______________
_____
Mn2O
10) _______________
_____
_____ ______
MnO2
Ternary Ionic practice
NAME ______________
Give the missing names, ions, and formulae.
Name
Ions
Formula
1) sodium sulfate
_____ ______
__________
2) lithium phosphate
_____ ______
__________
3) aluminum acetate _____ ______
__________
4) tin (II) nitrate
_____ ______
__________
5) ______________
_____ ______
K2CO3
6) iron (III) sulfite
_____ ______
__________
7) barium hydroxide
_____ ______
__________
8) ______________
_____ ______
Ca(HSO4)2
9) aluminum bicarbonate _____ ______
10) magnesium bicarbonate _____ ______
11) calcium nitrate
_____ ______
12) _____________
NH4+1 S-2
13) tin (IV) carbonate _____ ______
14) iron (III) sulfate _____ ______
15) ammonium phosphate _____ ______
__________
__________
__________
__________
__________
__________
__________
16) aluminum hydroxide _____ ______
__________
17) Cesium chromate
__________
18) Beryllium cyanide
______ ______
______ _______
__________
19) gold (I) sulfite ______ _______
__________
20) Strontium acetate ______ ______
__________
Polyatomic Ions
Group I
C₂H₃O₂⁻1= acetate
CO₃⁻2= carbonate
PO₃⁻3= phosphite
NO₂⁻1= nitrite
SO₃⁻2= sulfite
PO₄⁻3= phosphate
NO₃ ⁻1= nitrate
SO₄⁻2= sulfate
OH⁻1= hydroxide
NH₄⁺1= ammonium
Group II
CN⁻1= cyanide
C₂O₄⁻2= oxalate
MnO₄⁻1= permanganate
CrO₄⁻2= chromate
ClO⁻1= hypochlorite
Cr₂O₇⁻2= dichromate
ClO₂⁻1= chlorite
SiO₃⁻2= silicate
ClO₃⁻1= chlorate
ClO₄⁻1= perchlorate
Group III
H₂PO₄⁻1= Dihydrogen Phosphate
HSO₃⁻1= Hydrogen Sulfite
HPO₄⁻2= Hydrogen Phosphate
HSO₄⁻1= Hydrogen Sulfate
HCO₃⁻1= Hydrogen Carbonate (bicarbonate)
Group IV –AP only
S2O3-2 = thiosulfate
SCN-1 = thiocyanate
Hg2+2 = Mercury(I)
O2-2 = peroxide