Dear all G9A and G9B

I sent you the lead, Introduction, and MLA Format through your emails, please read them well. When you submit your FINAL WRITTEN REPORT, PLEASE make sure that you have the following:

1- FINAL WRITTEN REPORT (HARDCOPY - PRINTED).
2- INDIVIDUAL RUBRICS FOR WRITING FOR EACH MEMBER IN THE GROUP, STAPLE THEM TOGETHER.
3- A PAPER MENTIONED IN IT THE NAMES OF STUDENTS THAT PARTICIPATED IN THE FOLLOWING: LEAD, INTRODUCTION, CONCLUSION, CHECKING GRAMMAR AND SENTENCE STRUCTURE, VISUAL ELEMENTS, CHOOSING QUOTES, CITATIONS. (ALL OF YOU SHOULD PARTICIPATE IN THIS)

PLEASE I NEED THE ITEMS MENTIONED ABOVE IN A PLASTIC FOLDER PER GROUP. AND SEND ME THE SOFTCOPIES OF YOUR FINAL WRITTEN REPORTS TO MY GMAIL. This is my email for students who don't know it:

eng.nagla.sh@gmail.com

COULD ANYONE SEND ME AN EMAIL TO CONFIRM THAT YOU RECIEVED MINE.

thanks a lot, Dear all I appreciate your effort.

WARNING!!!!

The following groups have missing work for their research:

1- The group of Lina Helmy, Raghad El Shaer and Donia Abbas 9B- (Compound: Calcium Chloride) did not submit the second and third step of the research which are the : Bullet points (keywords) and turning those keywords to paragraph.

2- Mohamed Marzouk 9B in the group who choose Sulfuric Acid did not submit the 2nd and 3rd step of the research which are: Bullet points (keywords) and turning those keywords to paragraph.

3- The group of Summer Nasr, Habiba Sharaf and Zeinab El Tawil 9A (Compound: Silicon Dioxide) is missing the 3rd step of the research: turning the keywords to paragraph.

4- The group of Daeum, Ahmed Adeeb, Mazen Yassin and Sary Montasser 9A (Compound: Propane)  is missing the 3rd step of the research: turning the keywords to paragraph.

BE AWARE I HAVE TO SUBMIT YOUR GRADES BY TOMORROW MORNING

SUNDAY 5-12-2010 BEFORE NOON 1:00 p.m, PLEASE SEND YOUR WORK TO THE FOLLOWING E-MAIL: eng.nagla.sh@gmail.com

IF I RECEIVE YOUR WORK BY TODAY SATURDAY 4-12-2010  OR SUNDAY 5-12-2010 BEFORE 1:00 p.m (NOON); IT WILL BE LATE 10%, IF I RECEIVE IT BY MONDAY 6-12-2010 IT WILL NOT JOIN YOUR GRADES AND IT IS LATE 20%. 

HOWEVER IF I RECEIVE YOUR WORK AS A SOFTCOPY I EXPECT TO HAVE IT ALSO BY MONDAY 6-12-2010 AS A HARDCOPY (PRINTED ON PAPER)

THANKS AND GOODLUCK

                           Polyatomic ion

A polyatomic ion, is a charged ion composed of two or more atoms covalently bonded or of a metal complex that can be considered as acting as a single unit in the context of acid and base chemistry or in the formation of salts. The prefix "poly-" means "many," in Greek, but even ions of two atoms are commonly referred to as polyatomic.

For example, a hydroxide ion is made of one oxygen atom and one hydrogen atom: its chemical formula is (OH)⁻. It has a charge of −1. An ammonium ion is made up of one nitrogen atom and four hydrogen atoms: its chemical formula is (NH₄)⁺. It has charge of +1.

Nomenclature

There are two "rules" that can be used for the learning the nomenclature of polyatomic ions. First, when the prefix bi- is added to a name, hydrogen is added to the ion's formula and its charge is increased by 1, the latter being a consequence of the hydrogen ion carrying a +1 charge. An alternate to the bi- prefix is to use the word hydrogen in its place: the anion derived from H⁺ + CO₃²⁻, HCO₃⁻ can be called either bicarbonate or hydrogen carbonate.

The second rule looks at the number of oxygens in an ion. Consider the chlorine oxoanion family:

oxidation state	−1	+1	+3	+5	+7
anion name	chloride	hypochlorite	chlorite	chlorate	perchlorate
formula	Cl−	ClO−	ClO2−	ClO3−	ClO4−

First, think of the -ate ion as being the "base" name, in which case the addition of a per- prefix adds an oxygen. Changing the -ate suffix to -ite will reduce the oxygens by one, and keeping the suffix -ite and adding the prefix hypo- reduces the number of oxygens by two. In all situations, the charge is not affected. The naming pattern follows within many different oxyanion series based on a standard root for that particular series. The -ite has one less oxygen than the -ate, but different -ate anions might have different numbers of oxygen atoms.

These rules will not work with all polyatomic ions, but they do work with the most common ones (sulfate, phosphate, nitrate, chlorate).

Examples of common polyatomic ions

The following tables give examples of commonly-encountered polyatomic ions. Only a few representatives are given, as the number of polyatomic ions encountered in practice is very large.

Anions
Acetate (ethanoate)	CH3COO− or C2H3O−2
Benzoate	C6H5COO− or C7H5O−2
Bicarbonate (hydrogen carbonate)	HCO−3
Carbonate	CO2−3
Cyanide	CN−
Hydroxide	OH−
Nitrate	NO−3
Phosphate	PO3−4
Sulfate	SO2−4

Cations
Ammonium	NH+4
Hydronium	H3O+
Mercury(I)	Hg2+2

Research Topics

Here is a list of compounds; choose one compound and research its chemical formula, molecular structure, bonding type, everyday uses and impact on our lives. Also, what makes it important, and is it safe or dangerous; harmful, such as a pollutant; or beneficial, such as a requirement for maintaining our health. Consider the following when choosing a compound (Remember choose your groups with three members in a group):

• Chemical formula
• Molecular Structure
• Type of bonding
• Physical properties of the compound
• Chemical properties of the compound
• Uses of the compound
• Harms of the compound

The list of the compounds:

1.     Potassium Chlorate

2.     Ascorbic Acid

3.     Borax (Sodium Tetraborate Decahydrate)

4.     Boric Acid

5.     Butane

6.     Calcium Carbonate

7.     Calcium Chloride

8.     Calcium Hydroxide

9.     Calcium Oxide

10.  Calcium Sulfate

11.  Carbon Dioxide

12.  Copper(II) Sulfate and Copper Sulfate Pentahydrate

13.  Magnesium Sulfate

14.  Naphthalene

15.  Propane

16.  Silicon Dioxide

17.  Potassium Chloride

18.  Sodium Acetate

19.  Sodium Bicarbonate

20.  Sodium Hydroxide

21.  Sucrose (Saccharose)

22.  Sulfuric Acid

                                       Chemical Bonding: Covalent Bonding

·      Covalent bonding occurs when two (or more) elements share electrons.

·      Covalent bonding occurs because the atoms in the compound have a similar tendency for electrons (generally to gain electrons).

·      This most commonly occurs when two nonmetals bond together. Because both of the nonmetals will want to gain electrons.

·      Covalent Compounds:

1. Gases, liquids, or solids (made of molecules)
2. Low melting and boiling points
3. Poor electrical conductors in all phases
4. Many soluble in nonpolar liquids but not in water.

·      A good example of a covalent bond is that which occurs between two hydrogen atoms. Atoms of hydrogen (H) have one valence electron in their first electron shell. Since the capacity of this shell is two electrons, each hydrogen atom will "want" to pick up a second electron. Hydrogen atoms will react with nearby hydrogen (H) atoms to form the compound H₂. Because the hydrogen compound is a combination of equally matched atoms, the atoms will share each other's single electron, forming one covalent bond.

·      Unlike ionic compounds, covalent molecules exist as true molecules. Because electrons are shared in covalent molecules, no full ionic charges are formed.  Thus covalent molecules are not strongly attracted to one another.  As a result, covalent molecules move about freely and tend to exist as liquids or gases at room temperature.  

·      For every pair of electrons shared between two atoms, a single covalent bond is formed. When two oxygen atoms form the compound O₂, they share two pairs of electrons, (4 electrons) forming two covalent bonds.   

·      Lewis structures can also be used to show bonding between atoms. Each dash represents one pair ( 2 electrons) of electrons, or one bond

·         Elements which are close together in electron negativity tend to form covalent bonds and can exist as stable free molecules. Carbon dioxide is a common example.

·          Polar and non-polar covalent bonding: two subtypes of covalent bonds.

·      Non-polar Covalent bonding:

1.      The H₂ molecule is a good example of the first type of covalent bond, the non-polar bond; because both atoms in the H₂ molecule have an equal attraction (or affinity) for electrons.

2.       The bonding electrons are equally shared by the two atoms, and a non-polar covalent bond is formed.

3.      Whenever two atoms of the same element bond together, a non-polar bond is formed.

·     Polar Covalent bonding:

1.      A polar bond is formed when electrons are unequally shared between two atoms.

2.      Polar covalent bonding occurs because one atom has a stronger affinity for electrons than the other (yet not enough to pull the electrons away completely and form an ion). In a polar covalent bond, the bonding electrons will spend a greater amount of time around the atom that has the stronger affinity for electrons.

3.       A good example of a polar covalent bond is the hydrogen-oxygen bond in the water molecule.

                                                    Chemical Bonding: Ionic Bonding

• Compounds are formed when two or more atoms chemically bond together, the resulting compound is unique both chemically and physically from its parent atoms.

·         Ionic bonding: In ionic bonding, (It is called an ionic bond because the atoms become ions, a charged atom that has either lost an electron or has extra electrons) electrons are completely transferred from one atom to another. In the process of either losing or gaining negatively charged electrons, the reacting atoms form ions. The oppositely charged ions are attracted to each other by electrostatic forces, which are the basis of the ionic bond.

For example, during the reaction of sodium with chlorine: Notice that when sodium loses its one valence electron it gets smaller in size, while chlorine grows larger when it gains an additional valence electron. This is typical of the relative sizes of ions to atoms. Positive ions tend to be smaller than their parent atoms while negative ions tend to be larger than their parent.

sodium (on the left) loses its one valence electron to chlorine (on the right),

resulting in

A positively charged sodium ion (left) and a negatively charged chlorine ion (right).

Ionic compounds share many features in common:

• Ionic bonds form between metals and nonmetals.
• In naming simple ionic compounds, the metal is always first, the nonmetal second (e.g., sodium chloride).
• Ionic compounds dissolve easily in water and other polar solvents.
• In solution, ionic compounds easily conduct electricity.
• Ionic compounds tend to form crystalline solids with high melting temperatures. The fact that ionic compounds are solids, results from the intermolecular forces (forces between molecules) in ionic solids.  

Each sodium ion is attracted equally to all of its neighboring chlorine ions, and likewise for the chlorine to sodium attraction. The concept of a single molecule does not apply to ionic crystals because the solid exists as one continuous system. Ionic solids form crystals with high melting points because of the strong forces between neighboring ions.

	Cl-1 Na+1 Cl-1 Na+1 Cl-1 Na+1 Cl-1 Na+1 Cl-1 Na+1 Cl-1 Na+1 Cl-1 Na+1 Cl-1 Na+1 Cl-1 Na+1 Cl-1 Na+1
Sodium Chloride Crystal	NaCl Crystal Schematic

·         Elements from opposite ends of the periodic table will generally form ionic bonds. They will have large differences in electron negativity and will usually form positive and negative ions. The elements with the largest electron negativities are in the upper right of the periodic table, and the elements with the smallest electron negativities are on the bottom left. If these extremes are combined, such as in RbF, the dissociation energy is large. As can be seen from the illustration below, hydrogen is the exception to that rule, forming covalent bonds.