CHEMISTRY SHENANIGANS

-For monoatomic elements, a molecule= an element
-Diatomic element: Molecule (Cl2) Element (Cl)
-Molecules of Compounds H-O-H
--> molecule 2'H' atoms in 1 molecule, 1 'O' atom in 1 molecule
Example
Write ammonium carbonate (NH4)2CO3
N:2
H:8
O:3
C:1
Example
-moles<---->molecules
6.02x10^23 molec/1mol or 1mol/6.02x10^23molec

How many molecules are in 0.25 mol of CO2?
-0.25mol x 6.02x10^23molec/1mol = 1.505x10^23

5.1772x10^24 molecules of H2O = ? moles
-5.1772x10^24 molecules (1mol/6.02x10^23)=8.6mol

Find the number of 'H' atoms in 4.0mol of ammonia?(NH3)
- moles-->molecules--> H atoms
-4.0mol x 6.02x10^23/1mol= 2.41x10^24
-molecules x 3 = 7.22 x 10^24 'H" atoms

2Fe + 3CuCl₂ ---> 3Cu + 2FeCl₃

In our lab groups we dissolved copper chloride into water, added two iron nails into the solution, removed the two iron nails from the solution and dried them, and weighed the mass of the copper chloride, solution, and two iron nails each time a condition or characteristic of the material changed. Later, we discussed our recorded results with one another and handed in a lab report as a group.

Atomic Mass:
-The mass of 1 mole of atoms in an element
-The mass of 1.0 mol of 'C' atoms is 12.0g
-The mass of 1.0mol of 'Ca' atoms is 40.1g

Molecular Mass:
-The mass of 1.0 mole of atoms of an element or compound
N2, O2, H2, Br2, Cl2, F2, I2, P4, S8
-Assume all the rest are monoatomic
Element Symbol Formula Atomic mass Molar mass
Iodine I I2 126.9 g/mol 253.8g/mol
Silicon Si Si 28.1g/mol 28.1g/mol
Hydrogen H H2 1.0g/mol 2.0g/mol
Iron Fe Fe 55.8g/mol 55.8g/mol
Neon Ne Ne 20.2g/mol 20.2g/mol

Finding the molar mass of compounds:
-H2o
----> 2 H = 2(1.0) =2.0
----> 1 O = 1(16.0) =16.o
---->=18.0g/mol
-Find the molar mass of ammonium phosphate (NH4)3PO4
---->3N=2(14.0)
---->12H=12(1.0)
---->1P=1(31.0)
---->4O=4(16.0)
---->=149g/mol

Converting mass <----> moles:
-conversion factor g/mol or mol/g
-Find the mass of 2.5 mol of water
H20----> 18.og/mol 1mol/18.0g X 2.5mol =1/45g=45g
-Find the number of moles in 391g sample of nitrogen dioxide
NO2----> 1N=1(14.0), 2O= 2(16.0), =46g/mol
391 X 1mol/46g=8.5mol



In case you still don't understand, here's a short video:


And this is video is just for laughs:

1 Mole = {6.02 x10²³} known as Avogadro's number
= 602 000 000 000 000 000 000 000
.. therefore, 1 mole is just a really big number!

Hydrogen Bomb Equation
2H₂ + O₂ -> 2H₂0
is actually..
(2 H₂ molecules) and (1 O₂ molecule) = (2 molecules of H₂0)
is also..
12.04 x 10³ + 6.02 x 10³ --> 12.04 x 10²³
is also..
2 mol of H₂ + 1 mol of O₂ --> 2 mol of water

How big is Avogadro's number?
if 1 mole = 6.02 x 10³ was represented in dollars and divided among every person in the world..
about $1.0 x 10¹⁴ -> each person would have $100 trillion!!!!

How Gases Combine
- John Dalton looked at the masses of gases such as H₂, N₂, and C in comparison to O₂ but unfortunately, discovered there was no pattern.
- Joseph Gay-Lussac combined gases based on volume.
ex. 1L of H₂ reacts with 1L of Cl₂ -> 2L of HCl
1L of N₂ reacts with 3L of H₂ -> 2L of NH₃
2L of CO reacts with 1L of O₂ -> 2L of CO₂
He discovered that gases combine in simple, whole number ratios.

Avogadro's Hypothesis
- he came to believe that equal volumes of any gas at a constant temperature and pressure contain equal numbers of molecules (but have different mass)
ex. [(*) to represent one molecule]
H₂ (*)(*)(*)(*)
O₂ (*)(*)(*)(*)

And in case you still don't understand the mole, here is a video to help:

Acids
-solid, liquid or gas at SATP (25°, 100kPa)
-form conducting aqueous solutions
-turns blue litmus red
-dissolve in water to produce H+
-taste sour

-turn red litmus paper blue
-slippery
-nonconductive
-dissolve in water to produce OH-

- acids are aqueous (dissolved in water)
- hydrogen compounds are acids
-HCL_(aq) ---> Hydrochloric Acid
-H₂SO_4(aq) ---> Sulfuric Acid
-Hydogen appears first in the formula unless it is part of a polyatiomic group
-CH₃COOH_(aq) ---> Acetic Acid
-classical rules use the suffix ic and/or the prefix hydro-
ex. Hydrochloric acid
-IUPAC systme uses the aqueous hydrogen compound
ex. HCL_(aq) ---> Aqueous Hydrogen Chloride

-for now, all bases will be aqueous solutions of ionic hydroxide
-NaOH
-Ba(OH)₂
-use the cation name followed by hydroxide
-sodium hydroxide
-barium hydroxide

EXAMPLES:
-HI_(aq) hdroiodic acid
-H₃PO_4(aq) phospheric acid
-H₃PO_3(aq) phosphorous acid
-HNO_3(aq) nitric acid
-HNO_2(aq) nitrous acid
-Mg(OH)_2(aq) magnesium hyfroxide
-HBr_(aq) hydrobromic acid
-HOOCCOOH_(aq) oxalic acid

In additon to the notes we took today, Mr. Doktor also showed us a demo for acids and bases. We had baking soda ready to neurtalize the extremely, strong smell it produced.

Heres a video on how to make a ph indicator with red cabbage:

In today's class, we talked about hydrates and molecular compounds, as well as how to name them and the IUPAC formulas.

Hydrates: are compounds that form lattices which bond to water molecules, and the crystals that contain water inside can be released by heating

If a compound does not have water, it is often preceded by "anhydrous" (i.e. copper sulfate anhydrous)

How 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
    

ex. Cu(SO₄) · 5H₂O _(s) = copper II sulfate pentahydrate
ex. Nickel II sulfate hexahydrate = Ni(SO₄) · 6H₂O _(s)

The Prefixes in order to name the number of molecules:
Mono =1
Di = 2
Tri = 3
Tetra = 4
Penta =5
Hexa = 6
Hepta = 7
Octa = 8
Nona = 9
Deca = 10



Molecular compounds: are composed of two or more non-metals; they have a low melting point and boiling point; they share electrons; usually end in -gen, or -ine

• Diatomic molecules: (when 2 of the elements are the same) H₂, N₂, O₂, F₂, Br₂, I₂
• Polyatomic molecules: (S₈, P₄)

How to name molecular compounds:

1. Write the formula for the least electronegative ion first, then the formula for the most electronegative ion.
2. Criss-cross the charges, moving the numbers below.
3. Reduce the ion numbers to the lowest common multiples. Note: You do not need to write the subscript '1' or the ionic charges.

When writing a molecular compound back into words, remember to write the prefix in front in front of each element (mono, di, or tri, etc.). You MUST do this for both the first and second part of the compound. However, if there is only one of the first element, you do not write the prefix 'mono'. Also, do not forget to add the ending of 'ide' to the second ion.




Here's an example of a molecular compound. Look closely, and you'll see that the compound is bonded together due to the SHARING of electrons rather than the exchanging of electrons.



In addition, we learned some IUPAC formulas:

IUPAC NAME        FORMULA
Water*                         H₂0
Hydrogen Peroxide*     H₂0₂
Ammonia*                    NH₃
Glucose*                      C₆H₁₂0₆
Sucrose*                      C₁₂H₂₂0₁₁
Methane                       CH₄
Propane                       C₃H₈
Octane                         C₈H₁₈
Methanol                      CH₃0H
Ethanol                         C₂H₅0H

*important formulas to know for tests and future use


Here's a video about gas hydrates, talking about how ice can be used for fuel!

In today's class, we discussed atoms, ions, elements and compounds as well as how to name ionic binary compounds.

Things to know:

• An element is a substance that cannot be separated into simpler substances by a chemical change.
• A compound is a substance that contains two or more elements combined in a fixed proportion.
• A hydrate is any class of compound containing water. The procedure of how to name hydrates is in the following post.
• A multivalent element has more than one ionic charge. In the periodic table, the most common ionic charge will be placed first for the element.
• An atom is the smallest particle of an element that retains the chemical identity of the element; made up of negatively charged electrons, positively charged protons, and uncharged neutrons. Its structure:
• An ion is an atom or group of atoms that has a positive or negative charge because it has lost or gained electrons.
• The difference between an atom and an ion: an ion is an atom or group of atoms, normally electrically neutral, that has lost or gained one or more electrons.
• An ion consisting of a single atom is called a monatomic ion, and an ion consisting of multiple atoms is called a polyatomic ion. Larger ions containing many atoms are called molecular ions.

Remember, in chemical formulas, the ion charge is indicated by a superscript (a small number to the top right), and the number of ions is indicated by a subscript (a small number to the bottom right).
How to name ions:

• for metals, use the name of the element and write the ion charge
• for non-metals, remove the original ending and add 'ide' and write the ion charge
• for polyatomic ions, there are special names

How to name binary ionic compounds:

1. Write the formula for the cation first, and the formula for the anion.
2. Criss-cross the charges, moving the numbers below.
3. Reduce the ion numbers to the lowest common multiples. Note: You do not need to write the subscript '1' or the ionic charges.

Naming polyatomic compounds is quite similar to that of naming binary ionic compounds. The steps are exactly the same. The only difference is that there will be more than one element written in one ion. Don't get confused!

How to name multivalent ions:

• the more common charge will be placed on top in the periodic table
• remember to use roman numerals in parentheses to show the charge

The Periodic Table of Elements to help you name the compounds, which includes SOME of the elements' ionic charges:


Additional help on how to name ionic compounds: