The International School of Panama
IB Chemistry SLa – Notes on Review – Concepts and Nomenclature
Name: ______Block:____ Date: ______
Chemistry studies matter, its composition and its ______…
Matter is anything that has and occupies space…
There are two types of matter: ______substances and ______
Pure substances contain____________/ Mixtures contain______
______
Made of ______
______/ Made of ______
______
Cannot ______
______/ Can ______
______
Examples: / Examples:
Which are pure substances and which are mixtures?
Pure Substances
Matter
Mixtures
What is an element?
Where do you find most elements together?
Examples:
What is a compound?
Examples?
What is an atom?
The smallest particle of an element ______
______… They ______be split up into simpler substances by ordinary chemical means
Draw models of atoms:
Chemically bonded atoms form:______
______joined together by a ______
bond…If the atoms are of the same kind, then it is a molecule of ______, like the Mr. Brinclofh elements:
If the molecule is made of different kinds of atoms, it is a molecule of a ______(molecular) ______.
Draw models of molecules of water and ammonia:
What is a homogeneous mixture?
Give examples:
What is a heterogeneous mixture?
Give examples:
Classify each diagram as atoms, molecules of elements, molecules of compounds or mixture of elements and compounds:
Proportions / Properties / SeparationElement
Example: copper (Cu) / Only one type of
______/ Depend on the ______/ ______be converted to simpler substances by chemical means
Compound
Example: water
(H2O) / Always the ______proportion, for example water always contains ______hydrogen atoms for every oxygen atom / Totally ______from its elements.
For example water is liquid, while oxygen and hydrogen are ______/ Requires a chemical change to split up the components. For example, through ______, water molecules separate into______and ______
Mixture
Example: Air
A mixture of oxygen (O2), nitrogen (N2), argon (Ar), carbon dioxide (CO2), etc. / The proportion of the components ______
For example the proportion of the gases, especially Carbon dioxide and water vapor can vary / ______to its constituents
For example air supports ______like oxygen, etc. / The components can be separated through ______l means.
For example fractional ______
Nomenclature
Where are the metals in the PT? ______
The non metals?m______
What are binary compounds?
Binary compounds are chemical compounds formed ______
Examples:
NaCl = sodium chloride. CO2 = Carbon dioxide.
There are two types of binary compounds...
Binary Ionic Compounds (a metal and a non metal)
The metal looses electrons becoming positive (+)
http://www.shef.ac.uk/chemistry/webelements/webelements/elements/text/key/Na.html
The non metal gains electrons becoming negative (-)
Positive and negative ions attract each other...
http://www.shef.ac.uk/chemistry/web-elements/webelements/elements/text/key/F.html
What is the charge?
Group 1: ____ Group 2: ____ Group 13 (IIIA): _____
The nonmetals in:
Group 14: ____, Group 15: ____, Group 16: ____, Group 17: ____
Remember that metals only form positive ions (cations) while nonmetals, when forming ionic compounds with metals form negative ions (anions). (Nonmetals may have positive or negative oxidation states but metal have only positive oxidation states)
For example, how do we write the formula of a compound between calcium and fluorine ?
Write the positive element (metal) first with its charge (top right)
Then write the negative element (non-metal) with its charge
Do a cross multiplication (only the numbers not the signs)
Simplify if necessary…
• For example, suppose you want to write the formula of the compound formed between Gallium and Nitrogen…
Do you want to try by yourself?
• 1)Lithium and Oxygen
• 2) Potassium and Chlorine
• 3) Aluminum and Sulfur
• 4) Barium and Carbon
How do we name these compounds?
Name the metal first
Then the “root” of the non-metal
Finally add the ending “ IDE ”
Example Li2O
Metal= Lithium
Non-metal= Oxygen Root=Ox
Let’s practice again… write the names of:
1) CaF2
2) GaN
3) KCl
4) Al2S3
5) Ba2C
But there are some metals that have more than one possible charge
How do you combine for example Iron, Copper, and Lead with Oxygen?
You have two possibilities for each:
1) Fe 2+ +O2- ->
2) Fe 3+ + O2- ->
3) Cu1+ + O2- ->
4) Cu2+ + O2- ->
5) Pb 2+ + O2- ->
6) Pb 4+ + O2- ->
What do we do in this case?
Between the metal and the non metal, write the charge of the metal, in roman numerals and between parenthesis.
1) Fe 2+ +O2- -> FeO
2) Fe 3+ + O2- ->Fe2O3
Write the name of the others:
3) Cu1+ + O2- -> Cu2O ______
4) Cu2+ + O2- -> CuO ______
5) Pb2+ + O2- -> PbO ______
6) Pb4+ + O2- -> PbO2 ______
______
Write the name of the following compounds:
1. CuS ______
2. CoCl3 ______
3. Sn3N4______
Now the other way around
Write the formula of:
1) Iron (II) Chloride ______
2)Iron (III) Nitride ______
3) Mercury (I) Fluoride ______
What are polyatomic ions?
Remember that an ion is a particle with a ______.
Polyatomic ions are ______
______
Examples:
CO3 2- =
CO2 2- =
PO43- =
PO33- =
How do we combine these polyatomic ions ?
Let’s see some examples
How do we name these compounds?
Write the positive ion first with its charge
Then write the negative ion with its charge
Do a cross multiplication
Use parenthesis if you have to multiply a polyatomic ion
Let’s see some examples:
Write the formulas of the compounds formed between:
• 1)Ammonium and carbonate ______
• 2) Potassium and Chlorite ______
• 3) Aluminum and Sulfite ______
• 4) Barium and phosphate ______
Let’s practice … write the names of:
CaCO2 ______
Ga(NO3)3 ______
Fe(ClO)2 ______
(NH4)3PO4 ______
NH4Cl ______
More practice
Write the formula of:
Iron (II) Perchlorate ______
Potassium Nitrate ______
Mercury (I) Sulfite ______
Easy?
Remember!!! In compounds involving polyatomic ions
1. Consider the polyatomic ion as a ______
2. The charge is for ______
3. Use ______to multiply polyatomic ions
You can practice more!!!
Do you remember what are binary compounds?
______
• Examples: NaCl = sodium chloride and CO2 = Carbon dioxide.
There are two types of binary compounds...
-Binary molecular or covalent compounds... (two non-metals)
How to name binary molecular compounds…?
Use these prefixes to indicate the amount of atoms of each type:
Prefixes
______1 ______2 ______3 ______4 ______5
______6 ______7 ______8 ______9 ______10
• Name the ______element + the ______of the second + ______…
• But, before each element, use ______to indicate the amount of atoms of each type.
• Note: don't use ______for the ______element
Let’s see some examples:
CO2 ______N2O5 ______
P2O7______
Let's try the other way around...
Carbon Monoxide ______Dinitrogen pentoxide ______
Carbon tetrachloride ______Nitrogen dioxide ______
Remember!!!
Binary compounds (two ______)
Can be______(metal+non-metal) or molecular (two ______)
Recognizing an Acid
You will recognize an inorganic acid by the fact that its formula starts with
_____, as in these
Examples:
There are many acid formulas that do not start with H, but we will study them when we deal with organic acids..
There is one exception to this: the formula : ______(Organic Chem. style)
should be recognized as ______
An alternate way to write acetic acid is : ______(Inorganic Chem. style)
One last comment….
The formula H2O ______. It is the formula for water. It is not an acid. (When you study acid-base behavior, you will learn more about water's role in acid-base )
In order to explain acid naming, we will use the sequence ofChlorine acids
HCl
HClO
HClO2
HClO3
HClO4
What is the difference between the first and the others?
Binary Acids: Hydrogen + non metal
HCl is a ______. All binary acids are named the same way:
1. the prefix "______" is used.
2. the ______of the ______(negative element) is used.
3. the suffix "______" is used.
4. the word "______" is used as the second word in the name.
HCl = ______
Binary Acids: examples
HF: ______
HBr: ______
HI: ______
H2S: ______
HCN is not a binary acid (because it is made of three Elements).However it is named like a Binary acid because it doesn’t have ______.
HCN ______
Oxyacids: ______
To name an oxyacid, for example, HClO, you MUST:
1. Recognize when a polyatomic is present: Is there a polyatomic ion in HCLO? _____
2. Identify the polyatomic ion and its name: ______
3. THEN you change the _____to ____ and ____ to ____
4. Add the word acid: ______
Formula / Does it hava a polyatomic ion? / Formula of polyatomic ion / Name of polyatomic ion / Name of the acidHClO
HClO2
HClO3
HClO4
Formula / Binary, oxyacid or other? / Polyatomic ion (if applicable) or monoatomic ion / Acid Name
H3PO4
H2CO3
H2SO4
HIO3
HNO2
HF
Name / Binary oxyacid
Other? / Polyatomic ion (if applicable)
or monoatomic ion / Formula
hydrobromic acid
hydrocyanic acid
nitric acid
sulfurous acid
phosphorous acid
acetic acid