We're the Grade 11s in Mr. Doktor's chemistry 11 class.
We're in Block A, Day 1.
We are
Theresa Nguyen
Dominika Skibicki
Charles Perea
Tim Pang
This is our blog.

ATOMIC MASS:
Atomic Mass= the mass of 1 mole of atoms in an element.

MOLECULAR MASS:
Molecular Mass= the mass of 1.0 mol of molecules of an element or compund.
(Eg.) If you have the element Magnesium, the symbol and formula is Mg. When you look at the atomic mass of the element it is 24.3 g/mol, making the molar mass the same. However if you have a diatomic compound like Iodine the symbol would be I and the formula would be I2. the atomic mass would be 126.9 g/mol but because the element is never by itself you have 2 of them. This means that you take the atomic mass and multiply it by 2, giving you a molar mass of 253.8 g/mol.

FINDING THE MOLAR MASS OF COMPOUNDS:
(Eg.) Iron(III)Sulphide: Fe2S3
The formula shows that there are: 2 Fe
3 S
and their atomic masses are: 55.8
32.1
you multiply the masses by the number of atoms: 55.8* 2=111.6
32.1* 3=96.3
now you add the 2 molar masses and get: 207.9 g/mol

CONVERTING MASSES <-> MOLES:
The conversion factors are g/mol or mol/g
(Eg.) find the mass of 2.5 mol of water...
H2o-> 18g/mol-> 2.5 mol* 18 g/1 mol= 45g October 19, 2009
1 mole= 602 000 000 000 000 000 000 000 (6.02* 10^23)
The mole is called Avogadro's number since he discovered it. His hypothesis was that if the volumes of any gas at a constant temperature is equal and preasure was contained then the number of molecules would be equal. To the wonderful world of acids and bases we go!!!

Acids

Can be a solid liquid or gas at SATP*
*SATP
=> A really fancy way of saying 25 Degrees Celcius or 100kPa
Form conducting aqueous solutions
Turn blue litmus paper to red
Dissolve in water to produce H+
Taste Sour

Naming Acids

Acids are aqueous(dissolved in water)
Hydrogen compounds are acids
=>HCl(aq) -> Hydrochloric Acid
=>H2SO4(aq) -> Sulfuric Acid(IMPORTANT)
Hydrogen appears first in the formula unless it is part of a polyatomic group
=>CH3COOH(aq) -> Acetic Acid
Classical rules use suffix -ic and/or the prefic hydro-
=>Hydrochloric Acid
IUPAC system uses the aqueous hydrogen compound
=>HCl(aq) -> Aqueous Hydrogen Chloride

Bases

Turn red litmus blue
Slippery
Nonconductive
Dissolve water to produce OH-

Naming Bases

For now, all bases will be aqueous solutions of ionic hydroxides
=>NaOH
=>Ba(OH)2
Use the cation name followed by hydroxide
=>Sodium Hydroxide
=>Barium Hydroxide

Examples

HI(aq) -> Aqueous Hydrogen Iodide/Hydroiodic Acid
H3PO4(aq) -> Phosphoric Acid
=>H3PO3 -> Phophorous Acid
HNO3(aq) -> Nitric Acid
=>HNO2 -> Nitrous Acid
Mg(OH)2 -> Magnesium Hydroxide
HBr(aq) -> Hydrobromic Acid/Aqueous Hydrogen Bromide
HOOCCOOH(aq)(TRICKEY) -> Oxalic Acid(Pretty small name for a big formula, eh?)

Spontaneous Video(Part 1)

Spontaneous Video(Part 2)
Oct 6, 2009

Alot of super duper things happend today (especially since i got to light a bunsen burner) but sadly it has to be summarized, so here it goes:

To Name Hydrates

1.Write the name of the Chemical Formula
2. Add a prefix* indicating the number of water molecules
3. Add Hydrate after the prefix

*We learnd 10 different prefixes today
1 - Mono........6 - Hexa
2 - Di..........7 - Hepta
3 - Tri.........8 - Octa
4 - Tetra.......9 - Nona
5 - Penta......10 - Deca

-Example:
Cu(SO4) . 5H20 => Copper(II) Sulfate pentahydrate
Li(SO4) . 3H2O => Lithium Perchlorate trihydrate



Molecular Compounds

- Composed of 2 or more non-metals
- Low melting and boiling point
- Share(not exchange) electrons
- Usually end in -gen or -ine
=> Hydrogen, Oxygen, Nitrogen
- Seven molecules are Diatomic
=> H2, N2, O2, F2, Cl2, Br2, I2
- Two molecuales are polyatomic
=> S8, P4

Examples:
N204 - Dinitrogen tetraoxide
CS2 - Carbon disulfide
P4O10 - Tetraphosphorous Decaoxide
CO - Carbon Monoxide

Backwards
Nitrogen trichloride - NCl3
Sulpher dibromide - SBr2
Dihydrogen oxide - H2O

Today, we learned even more interesting information and here is what we studied:

Chemical Nomenclature

-Naming chemical compounds has been a very difficult task and different systems have been used through the centuries

-Today, the most common system is IUPAC for most chemicals:
->Ions (have a charge)
->Binary Ionic
->Polyatomic Ions
->Molecular compounds
->Acids



Chemical Formulas

-Be aware of the differences between ion and compound formulas
e.g. Zn(2+)<-ion charge
BaCl2<- number of ions



Naming Ions

-For metals use the name of the element and add ion
->Al(3+)=Aluminium Ion

-For non-metals, remove the orginal ending and add -ide
->F(-)=Fluorine=>Fluoride

-Polyatomic Ions have special names(see table on your periodic table)



Binary Ionic Steps

1.Write the formula for the cation first and then the formula for the anion.

2.Criss-cross charges moving the numbers below.

3.Reduce ion numbers to lowest common multiples, omit 1 and omit charges .



Multivalent Ions

-Some elements can form more than one ion.
e.g.Iron->Fe(3+) or Fe(2+)
Copper->Cu(2+) or Cu(1+)

-the more common ion is the top one of the Periodic Table

-IUPAC uses roman numerals in parethesis to show the charge

-Classical(i.e.old) systems uses latin names of elements and the suffix -ic(larger charge) and -ous(smaller charge)
E.g.FeO->Ferrous Oxide
Fe203->Ferric Oxide

Other Classical Names

-Ferr->Iron
-Cupp->Copper
-Mercur->Mercury
-Stann->Tin
-Aunn->Gold
-Plumb->Lead

Example: What is the chemical formula for Barium Phosphate?
Answer: Ba3(PO4)2 Today, our class learned alot from Mr. Doktor and here are some materials we learned:) :

Classification of Matter

-Understanding matter begins with how we name it. We can divide matter into two types: Homogeneous substances
Heterogeneous substances

-Homogeneous: consists of only one visible component
e.g. Distilled Water, Oxygen, Graphite

-Heterogeneous: contain more than one visible component
e.g. Chocolate Chip Cookie, Granite



Pure Substances

-There are two types of Pure Substances: Elements and Compounds

-Elements: substances that cannot be broken down into simpler substances by chemical reactions
e.g. Oxygen, Iron, Magnesium

-Compounds: substances that are made up of 2 or more elements and can be changed into elements(or other compounds) by chemical reactions
e.g. Water, Sugar



Telling the Difference

- It is often very difficult to know if something is an element or a compound
->the differences are only "visible" on the atomic level

- One method is to connect the substance to an electric current. This technique called electrolysis can split the compound apart into its constituent elements



Solution

- A solution is a homogeneous mixture of two or more substances
-> sloutions usually involve liquids but don't have to (Fog, Steel)

- The component present in greater amount is the solvent
-> water is the most common solvent
-> the symbol(aq) is used when something is dissolved in water

- The component present in smaller amount is the solute
-> in salt water, salt is the solute

Mixtures

- Many mixtures are easy to identify, but others are easily confused as pure substances

- In Heterogeneous mixtures the different parts are clearly visible (Granite, Sand, Fog)

- In Homogeneous mixtures the different parts are not visible
(Salt Water, Air, Brass)

Separating Mixtures

- There are many methods to separate mixtures, depending on the type of mixture
-> By hand
-> Filtration
-> Distillation
-> Crystallization
-> Chromatography

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