key question: why do atoms combine in certain ratios?
TRANSCRIPT
Key Question:
Why Do Atoms Combine In Certain Ratios?
Review of Oxidation Numbers
Review of Oxidation Numbers
All compounds have an electrical charge of zero (they are neutral).
An oxidation number indicates the charge on the atom (or ion) when electrons are lost, gained, or shared in chemical bonds.
Oxidation Numbers
A sodium atom always ionizes to become Na+ (a charge of +1) when it combines with other atoms to make a compound.
Therefore, we say that sodium has an oxidation number of 1+.
What is chlorine’s oxidation number?
Ionic Bonds
On the periodic table, strong electron donors are on the left side (alkali metals).
Strong electron acceptors are on the right side (halogens).
The further apart two elements are on the periodic table, the more likely they are to form an ionic compound.
Covalent Bonds
Covalent compounds form when elements have roughly equal tendencies to accept electrons.
Elements that are both nonmetals and therefore close together on the periodic table tend to form covalent compounds.
Oxidation Numbers, Lewis Structures And Chemical Formulas
Remember, the oxidation numbers for all the atoms in a compound must add up to zero.
Multiple Oxidation Numbers
Some periodic tables list multiple oxidation numbers for most elements.
This is because more complex bonding is possible.
Naming Compounds and Writing Formulas
5 Types Of Chemical Compounds
•Binary ionic - metal ion – nonmetal ion
•Ternary ionic - at least one ion is a polyatomic ion
•Binary molecular - two nonmetals
•Binary acid - H – nonmetal
•Ternary acid - H – Polyatomic ion
Tips To Keep In Mind When Naming And Writing Formulas:
•Always keep your Periodic Table handy – You should have it in front of you ALWAYS when you are naming and writing formulas.
•Remember that metalsmetals (except Hydrogen) are found to the left of the stairstep on the Periodic Table.
•NonmetalsNonmetals are found on the right side of the stairstep of the Periodic Table.
•Metalloids Metalloids are the 7 elements on or below the stairstep are the 7 elements on or below the stairstep except Al and At. For naming purposes they will tend to except Al and At. For naming purposes they will tend to behave like nonmetals.behave like nonmetals.
Naming Binary Compounds
A binary ionic compound is held together by ionic bonds.
Binary molecular compounds consist of covalently bonded atoms.
Each type of compound has its own naming rules.
How Do You Name Binary Ionic Compounds?
(Composed Of Two Elements – A Metal And A Nonmetal)
•Name the first ion
•From groups 1, 2, 3, 13, zinc, cadmium, or silver. (You must use a Roman Numeral with the name for the other metals – we’ll discuss this later.)
•Name the second ion changing the suffix to –ide.
Naming Binary Ionic Compounds
MgBr2 is magnesium (name of first element) + brom (root name of second element) + ide suffix = magnesium bromide
Examples
BaNa2You should recognize a problem with this one
This is two metals – not a binary ionic compoundThe name of this is BananaBanana (haha!!)
What is the name of this compound:
HIJKLMNO?
WATER – “H” to “O”
You have to admit – that was funny!
Exit QuizNaCl
Name the metal ionSodium
Name the nonmetal ion, changing the suffix to –ide.
Chloride
CaO
Calcium Oxide
Al2S3
Aluminum Sulfide
MgI2Magnesium Iodide
What About The Transition Metals And Using Roman Numerals? How Does That Work?
Let’s See.FeO
Notice – metal and nonmetal.Name the first ion. Since the first ion is a transition element, you must use a Roman Numeral to represent the charge.
How do you know the charge?
Deductive reasoning.
•All compounds are neutral.
•Oxygen has a -2 charge (group 16)
•Therefore, iron must have a +2 charge since there is one iron and one oxygen. Iron gets a Roman Numeral (II).
Iron (II) Oxide
Isn’t this easy and FUN!!!
Cu2SName the first ion. Since it is a transition metal, you must use a Roman Numeral.
Which Roman Numeral? The Roman Numeral is the same as the charge of the ion.
How do you find the charge?
Deductive reasoning!
•All compounds are neutral
•Sulfur has a -2 charge (group 16)
•There are two coppers.
•Therefore each copper must have a +1 charge for all ions to be neutral
Copper (I)Sulfide
MnO2Name the first ion. Since it is a transition metal, you must use a Roman Numeral.
How do you determine the Roman Numeral?
It is the same as the charge.
What is the charge of Mn?
•All compounds are neutral.
•Oxygen (group 16) has a -2 charge.
•There are two oxygens and one Mn.
•Therefore Mn must have a +4 charge for this compound to be neutral.
Manganese (IV)oxide
So Why Must We Use Roman Numerals With Transition Elements?
•The metals in groups 1, 2, 3, and 13 have single, definite charges.single, definite charges.
•Group 1 metals have a +1+1 charge.
•Group 2 metals have a +2+2 charge.
•Groups 3 and 13 metals have a +3+3 charge.
•Transition metals may have multiple charges – usually two different positive charges.
For example, there are two copper oxide compounds:
Cu2O and CuO We can’t just say Copper oxide. Which one of these is Copper oxide? We must distinguish these
by using a Roman Numeral
Cu2O
Copper I oxide
Copper is +1
CuO
Copper II oxide
Copper is +2
There Are Three Transition Elements Which Do Not Require A Roman Numeral Because They Have Single
Definite Charges. These Are
Zinc – Zn2+ Cadmium – Cd2+ Silver – Ag+
You need to remember the charges for these.
Ag2O Name the first ion.
Silver Name the second ion changing the suffix to –ide.
oxide
ZnCl2Name the first ion.
Name the second ion changing the suffix to –ide.
Zinc chloride
No Roman Numerals needed for these.
How Do You Write Formulas For Binary Ionic Compounds Given The Name?
Two Simple Steps:
1. Write the symbol and charge of each ion
2. Balance the charges by providing subscripts
Magnesium chloride Write the symbol and charge of each ion.
Mg2+ Cl-Balance the charges by supplying subscripts. Subscripts tell how many of each atom is present.
You need a second Cl-1 to balance the charges
Cl-
MgCl2
Iron (III) bromide
Write the symbol and charge of each ion. The charge of the iron is provided by the Roman Numeral.
Fe3+ Br -
Balance the charges by supplying subscripts. The subscripts tell how many of each ion is needed to balance the compound.
You’ll need three bromine ions to balance the one iron.
Br -
Br -
FeBr3
Aluminum Sulfide Write the symbol and charge of each ion.
Al3+ S2- Balance the charges by supplying subscripts.
In this case the charges do not evenly divide into each other. You must find the least common multiple. SIX
How many aluminums are needed to arrive at a +6 charge?
How many sulfurs are needed to arrive at a -6 charge?
2
3
Al3+ S2-
S2-
Al2S3
Writing Formulas a Little Quicker
Iron and oxygen combine to form a compound. Iron (Fe) has an oxidation number of 3+. Oxygen (O) has an oxidation number of 2–.
Predict the chemical formula of this compound.
1. Given … Fe3+ and O2–
Write the subscripts so that the sum of the oxidation numbers equals zero.
2. Solution Two iron atoms = 2 × (3+) = 6+ Three oxygen atoms = 3 × (2–) = 6–
Writing Formulas a Little Quicker
Fe
3+ O
2-
3 2x = 6
Writing Formulas a Little Quicker
Fe 3+
+
= +6
Fe 3+
O2-
+O
2-
+O
2-
= -6+6
-6
0
Writing Formulas a Little Quicker
Fe
3+ O
2-
32
Writing Formulas a Little Quicker
Exit Quiz – Formula for magnesium chloride?Exit Quiz – Formula for magnesium chloride?
MgCl2
2+ 1-
Exit Quiz – Formula for sodium oxide?Exit Quiz – Formula for sodium oxide?
Na2O
1+ 2-
Exit Quiz – Name for:
Fe2O3
3+ 2-Iron (III) oxide
Exit Quiz – Formula for:
CrO2
4+ 2-Chromium (IV) oxide
Exit Quiz – Charge on Chromium?
Cr2O72-
6+ 2-
Second Category Of Compounds – Ternary Ionic Compounds.
These Compounds Contain At Least One Polyatomic Ion.
What is a polyatomic ion?
Let’s look at the name to try to understand.
•It is an ionion – that means it has a charge.
•It is polyatomicpolyatomic – that means it is made of more than one atom.
Let’s look at some examples of polyatomic ions.
CO32- carbonate
This ion is composed of one carbon and three oxygens and the entire group
has a charge of -2.
Polyatomic ion – Group of atoms that act as a unit and carry a charge.
You have been given a list of other polyatomic ions
You need to learn these!!!
How Do You Recognize Ternary Ionic Compounds?
Composed of two ions in which at least one is a polyatomic ion.
There is only one positive polyatomic ion (NH4+)
Three possible types of Ternary Ionic Compounds:
•Ammonium + negative ion (nonmetal)
•Metal (positive ion) + negative polyatomic ion
•Ammonium + negative polyatomic ion
Polyatomic Ion
Naming Compounds with Polyatomic ions
NH4Cl is ammonium (the name of the ion from chart) + chlor (root name of the second element) + ide suffix = ammonium chloride.
How Do You Name Ternary Ionic Compounds?
1. Name the first ion.
2. Name the second ion. Isn’t that simple??!!
Examples:Na2CO3
When you look at this compound you should recognize that this is NOT binary. There are THREE elements present. When you see this, immediately look for a polyatomic ion. CarbonateCarbonate is present here.
Name the first ion.
Sodium
Name the second ion.
carbonate
Notice that you do NOT change the suffix – just name the polyatomic
ion
Fe(OH)3 Name the first ion.
Iron Remember that iron requires a Roman Numeral since it is a transition element. What Roman Numeral should be used?
The Roman Numeral comes from the charge of the ion. How do you find the charge of the iron?
You know two things:
•All compounds are neutral.
•You know the charge of OH (-1)
Since there are 3 OH groups, each with a -1 charge, the charge of the iron must be +3 for the compound to be neutral
(III)
Name the polyatomic ion.
hydroxide
NH4Cl Name the first ion.
Ammonium Name the second ion.chloride
Notice that since the second ion is a nonmetal that, like binary ionic compounds, the suffix of the nonmetal changes to –ide.
(NH4)3PO4
Name the first ion.
Name the second ion.Ammonium phosphate
Looks like a monster, but it’s really a pussycat.
Cu2SO4Name the first ion.
CopperYou should realize that you need a Roman Numeral since copper is a transition metal.
The Roman Numeral is the same as the charge.
What is the charge?
The charge of sulfate is -2.
Since there are two coppers, the charge of the copper must be +1.
(I) sulfate
Name the second ion.
How Do You Write Formulas For Ternary Ionic Compounds?
Very Much Like Writing Formulas For Binary Ionic Compounds.
Three Steps:
1. Write the formulas/symbols of each ion.
2. Balance the charges by supplying subscripts.
3. If a subscript is needed for a polyatomic ion, it must be put in parentheses with the subscript on the outside.
Let’s do some!!
Aluminum nitrate First, you can tell from the name that there is a polyatomic ion present (nitrate). All binary ionic compounds have suffixes of –ide.
Write the formula/symbol and charge of each ion.
Al3+ NO3-
Balance the charges by supplying subscripts.
Since Al is +3 and NO3 is -1, you need a total of 3NO3- to
balance one Al3+
Since you will need a subscript of 3 for NO3-, you need to put
this in parentheses with the 3 outside.
Al(NO3)3
Lead (IV) acetate Write the formula/symbol and charge of each ion.
Pb4+ C2H3O2-
Balance the charges by supplying subscripts. Since Pb is +4 and C2H3O2 is -1, you will need 4 C2H3O2
-1 to balance 1Pb+4
Pb(C2H3O2)4
Calcium phosphateWrite the formula/symbol and charge of each ion.
Balance the charges by supplying subscripts. Since Ca is +2 and PO4 is -3, you will need 3 Ca+2 to balance 2 PO4
-3
Ca2+ PO43-
Ca3(PO4)2
Exit Quiz
Al3+ combines with sulfate (SO4)2– to make aluminum sulfate.
Write the chemical formula for aluminum sulfate.
Al3+(SO4)
2-
32
Exit Quiz Answer
The Third Category of Compounds –
Binary Molecular
What are Binary Molecular Compounds?
These compounds contain two elements (binary).
•The term “molecular” indicates that these elements are joined by a covalent bond.
•They must therefore be nonmetals.
•Bottom line – 2 elements – both nonmetals
•To name and write formulas for these, you must know some numerical prefixes.
Naming – You Must Use Prefixes.
1 = mono 3 = tri 5 = penta 7 = hepta 9 = nona
2 = di 4 = tetra 6 = hexa 8 = octa 10 = deca
Steps
1. The first nonmetal only gets a numeric prefix when there is more than one. No prefix if there is only one.
2. The second element always gets a numeric prefix and always has a suffix of -ide
Naming Binary Molecular Compounds
As with binary ionic compounds, the ending of the name of the second element in the compound is modified by adding the suffix –ide.
CO2
Carbon dioxide
CO
Carbon monoxide
N2O4
Dinitrogen tetraoxide
H2O
Dihydrogen monoxide
CCl4
Carbon tetrachloride
Name the first element. Since there is only one, no prefix is needed.
The second element always gets a prefix and a suffix of –ide.
Name the first element. Since there are two present, the prefix
“di” is needed. The second element always gets a prefix and
a suffix of –ide.
AlCl3What do you think about this one???
Be careful. This is a metal and nonmetal.
Always keep your Periodic Table in front of you for reference.
You may have been tempted to say “aluminum trichloride”. This is INCORRECT!
This is a binary IONIC compound. No prefixes are used. Simply name it aluminum chloride.
Given The Names Of Binary Molecular Compounds, How Do You Write The Formulas?
Very easily done!!! The prefixes tell you how to write the formulas. DO NOT CONSIDER CHARGES. NONMETALS ARE ALL NEGATIVE SO TO USE CHARGES DOES NOT
WORK!
Silicon dioxide
Diphosphorous pentachloride
Silicon and oxygen are both nonmetals.
The lack of a prefix on silicon means that there is only ONE silicon.
The prefix “di” in front of oxide means that there are TWO oxygens.
SiO2
Phosphorous and chloride are both nonmetals.
The prefix “di” means that there are TWO phosphorouses (Is that a word?)
The prefix “penta” before chlorine means that there are five chlorines.
P2Cl5
NO
Nitrogen monoxide
Nitrogen and oxygen are both nonmetals.
The lack of a prefix on nitrogen means only ONE nitrogen.
The prefix “mono” on oxygen indicates ONE oxygen.
Is this not sooooooo easy!??
CO2
Carbon dioxide
SO
Sulfur monoxide
N2O5
Dinitrogen pentaoxide
CF4
Carbon tetrafluoride
SO3
Sulfur trioxide
CO
Carbon monoxide
B2O3
Diboron trioxide
NF5
Nitrogen pentafluoride
Exit Quiz
More Practice with Covalent CompoundsMore Practice with Covalent Compounds
Covalent compounds are made of two nonmetals, which from the
periodic table are always expected to be negative
More Practice with Covalent CompoundsMore Practice with Covalent Compounds
But since covalent compounds are neutral species, it is not possible
for every element to retain its negative oxidation number
More Practice with Covalent CompoundsMore Practice with Covalent Compounds
ONLY THE MORE ELECTRONEGATIVE ELEMENT keeps
its negative oxidation number. Other nonmetals must adapt to keep the
compound neutral
Electronegativity TrendElectronegativity Trend
More Practice with Covalent CompoundsMore Practice with Covalent Compounds
SO2
Since oxygen is the more electronegative element, it will
have its normal oxidation number.
-2
More Practice with Covalent CompoundsMore Practice with Covalent Compounds
SO2
The compound is neutral, so the oxidation number of sulfur will be sufficient to balance out the two
oxygen atoms. What is it?
-2+4
More Practice with Covalent CompoundsMore Practice with Covalent Compounds
OF2
Since fluorine is the more electronegative element, it will
have its normal oxidation number.
-1
More Practice with Covalent CompoundsMore Practice with Covalent Compounds
OF2
The compound is neutral, so the oxidation number of oxygen will be sufficient to balance out the two fluorine atoms. What is it?
+2 -1
More Practice with Covalent CompoundsMore Practice with Covalent Compounds
PO43-
Since oxygen is the more electronegative element, it will
have its normal oxidation number.
-2
More Practice with Covalent CompoundsMore Practice with Covalent Compounds
PO43-
-2
The ion has a charge of negative three, so the oxidation numbers must add up to the total charge
of the ion. What is it?
+5
More Practice: Ionic Compounds with More Practice: Ionic Compounds with PolyatomicsPolyatomics
CaSO4
This is an ionic compound, so the charge of the metal cation is its oxidation number. What is it?
+2
More Practice: Ionic Compounds with More Practice: Ionic Compounds with PolyatomicsPolyatomics
CaSO4
The anion is a polyatomic ion, sulfate, and the charge of sulfate
is what? So the oxidation numbers of
sulfur and oxygen must add to -2.
+2
More Practice: Ionic Compounds with More Practice: Ionic Compounds with PolyatomicsPolyatomics
CaSO4
Oxygen is the more electronegative of the two, so it
keeps its normal oxidation number. What is it?
+2 -2
More Practice: Ionic Compounds with More Practice: Ionic Compounds with PolyatomicsPolyatomics
CaSO4
Sulfur and the four oxygen atoms must add to negative two (the charge of the sulfate anion).
What is the charge on sulfur?What is the name?
Calcium sulfate.
+2 -2+6
More Practice: Ionic Compounds with More Practice: Ionic Compounds with PolyatomicsPolyatomics
Pb(OH)4This is an ionic compound, so the charge of the metal cation is its oxidation number. But this is a transition metal, so we cannot know it from its position on the
periodic table.
More Practice: Ionic Compounds with More Practice: Ionic Compounds with PolyatomicsPolyatomics
Pb(OH)4But the anion, the hydroxide ion,
carries a charge of negative one. All four hydroxides are negative one, but
since the compound is neutral, the oxidation number of lead must
balance it out. What is it?
+4
More Practice: Ionic Compounds with More Practice: Ionic Compounds with PolyatomicsPolyatomics
Pb(OH)4Within the anion, oxygen is the more electronegative of the two elements, and keeps its normal oxidation number. What is it?
+4 -2
More Practice: Ionic Compounds with More Practice: Ionic Compounds with PolyatomicsPolyatomics
Pb(OH)4Within the hydroxide ion, the oxygen and
hydrogen must add to the charge of the ion, -1. What is the charge on H?
What is the name?Lead (IV) hydroxide
+4 -2 +1