Oxidation and reduction
When forming compounds, it is important to know something about the way atoms will react with each other. One of the most important behaviors in which atoms and / or molecules react to each other is the oxidation / reduction reaction. Oxidation / reduction reactions are the process of losing and getting each electron. Just remember, "Leo The Lion said Ger:" Losing electron oxidation, get electron reduction. The oxidation number is assigned to atoms and compounds as a way to tell scientists where electrons are in the reaction. This is often referred to as "costs" on atoms or compounds. The oxidation number is assigned according to a set of standard rules. They are as follows:
A pure element atom has a zero oxidation amount.
For single atoms in ions, their oxidation amount is the same as their costs.
Fluorine is always -1 in compounds.
Cl, Br, and I always -1 in the complex except when they are combined with O or F.
H usually +1 and o usually -2.
The amount of oxidation of compounds is equal to the amount of oxidation for each atom on the compound.
Form ionic compounds.
Knowing the amount of oxidation of compounds is very important when discussing ionic compounds. Ionic compounds are a positive and negative ion combination. They generally form when nonmetal and metal bonds. To determine which substances are formed, we must use the allegations of the ion involved. To make neutral molecules, positive charges from cations (positively charged ions) must be the same as the negative charge of anions (negatively charged ions). To create neutral molecules, you must combine atoms in certain proportions. Scientists use subscripts to identify how many of each atom form molecules. For example, when combining magnesium and nitrogen we know that magnesium ions have the cost of "+2" and nitrogen ions have a "-3" cost. To cancel this fee, we must have three magnesium atoms for every two nitrogen atoms:
13mg2++2n3-->mg3n2
Knowledge of allegations of ions is very important to know the formula of compounds formed.
Alkalis (column element 1) forms ions "+1" like Na + and Li +
Metal earth alkaline (column element 2) forms ion "2+" like mg2 + and ba2 +
Halogen (7th column element) forms ions "-1" such as Cl- and I-
Other general ions are listed in the table below:
Positive ion (cation) negative ion (anion)
1+ 1-
Ammonium (NH4 +) acetate (C2H3O2-)
Copper (i) (Cu +) Azide (N3-)
Hydrogen (H +) Chlorate (Clo3)
Silver (AG +) cyanide (CN-)
Dihydrogen phosphate (H2PO4-)
2+ Hydrides (H-)
Cadmium (CD2 +) Bicarbonate (HCO3-)
Cobalt (ii) (CO2 +) hydroxide (OH-)
Copper (II) (cu2 +) nitrate (no3-)
Iron (Fe2 +) nitrite (no2-)
Lead (PB2 +) perchlorate (CLO4-)
Manganese (ii) (mn2 +) permanganate (mno4-)
Mercury (I) (HG22 +) Thiocyanate (SCN-)
Mercury (II) (Hg2 +)
Nickel (ni2 +) 2-
Tin (SN2 +) Carbonate (CO32-)
Zinc (ZN2 +) Chromate (CRO42-)
Dikromat (CR2O72-)
3+ hydrogen phosphate (HPO42-)
Aluminum (AL3 +) oxide (O2-)
Chromium (III) (CR3 +) peroxide (O22-)
Iron (iii) (Fe3 +) sulfate (SO42-)
Sulfide (S2-)
Sulfite (SO32-)
3-
Nitride (N3-)
phosphate (PO43-)
Phosphide (P3-)
Naming ionic compounds.
The bottom line below gives a rule for naming ion compounds:
Positive ion
Monatomic cation (one atom with a positive charge) takes the name of the element plus the word "ion"
Example:
Na + = sodium ion
Zn + 2 = zinc ion
If an element can form more than one (1) positive ion, the charge is indicated by the Roman number in brackets followed by the word "ion"
Example:
Fe2 + = Iron (ii) ion
Ion fe3 + = iron (iii)
Negative ion
Anion Monatomic (one atom with a negative charge) changes their ending to "-ide"
Example:
O2- = ion oxide
Cl- = ion chloride
Oxoanian (negative-charged poliad ion containing o) ends on "-ate". However, if there is more than one oxyianion for a certain element, the tip is:
Two oxygen fewer than the most common start with "hypo-" and ends with "-ite" oxygen less than the most common end with "-ite"
Oxolanion is the most common end with "-ate"
One more oxygen from the most common start with "per-" and ends with "-ate"
Clo- = hypochlorite
Clo2- = KLORT
No2- = nitrite.
So32- = sulfite.
Oxyanion is the most common with four oxygen
So42- = sulfate.
PO43- = phosphate.
Cro42- = chromate.
The most common oxyanion with three oxygen
No3- = nitrate.
Clo3- = Chlorate.
Co32- = carbonate
Clo4- = perchlorate.
Anion polyatom (negatively charged ions containing more than one type of element) often add hydrogen atoms; In this case, the name Anion added "hydrogen-" or "bi-" to the beginning
Example:
CO32- Becoming HCO3-
"Carbonate" becomes "hydrogen carbonate" or "bicarbonate"
When combining cations and anions into ion compounds, you always enter the name of the cation first and then the name anion (the molecular formula is also written in this order.)
Example:
Na ++ Cl- -> NaCl
Sodium + chloride -> Sodium chloride
CU2 + + SO42- -> CUSO4
Copper (II) + sulfate -> copper (ii) sulfate
AL3 + + 3NO3- -> Al (No3) 3
Aluminum + Nitrate -> Aluminum Nitrate
Atomic settings.
In mention ions, it is important to consider "isomers." Isomers are compounds with the same molecular formulas, but different atom settings. Thus, it is important to enter several signals in the name of the ion that identifies the settings you are talking about. There are three main types of classification, geometric, optical and structural isomers.
Geometric isomers refer to the side of which ion atom lying. The prefix used to distinguish geometric isomers is the substituent of CIS meanings located on the same side as ions and trans which means they lie on the opposite side. Below is a diagram to help you remember.
Optical isomers differ in setting four groups around Kiral carbon. Both of these isomers are distinguished as L and D.
Structural isomers distinguish between placement of two chlorine atoms around hexagonal carbon rings. These three isomers are identified as O, M, and P. Once again we have given you some instructions to help your memory.
The pop-up nomenclator calculator is available for assistance when naming compounds and for practice problems.
Naming molecular binary compounds
Molecular compounds are formed from covalent bonds between non-metal elements. Nomenclature for this compound is explained in a series of the following rules.
More positive atoms are written first (atoms are the most far to the left and to the bottom of the periodic table)
The second more negative atom has an ending "-ide".
Every prefix shows the number of each atom in the complex.
The number awom prefix number of atomic prefix
1 mono 6 hexa
2 at 7 Hepta
3 tri 8 Octa
4 Tetra 9 Miss
5 Penta 10 Deca
Example:
CO2 = carbon dioxide
P4S10 = Tetraphosphorus Decasulfide
Naming inorganic acid
Binary Acid (H Plus Nonmetal Element) is an acid that separates into hydrogen and anion atoms in water. Acid which only releases one hydrogen atom known as monoprotic. Acid-acid that releases more than one hydrogen atom is called polyproticacids. When naming this binary acid, you just add "hydro-" (showing the existence of hydrogen atoms) to the beginning and "-ic acid" to the end of the name anion.
Example:
HCl = Chloride Acid
Hbr = hydrobromic acid
Acid Asnary (also called oxoacids, formed by hydrogen plus other elements plus oxygen) is based on the name anion. In this case, -ate, and -ite sufiks for anions are replaced with -ic and -ous. The name of the new anion is then followed by the word "acid." The chart below illustrates changes in nomenclature.
Acid name Anion name
Hypo___ite Hypo___ous Acid.
___ite ___ous acid.
___ate ___ic acid.
per___ate per___ic acid.
Example:
Clo4- to Hcllo4 => perchlorate to perchlorate acid
Clo- to Hclo => hypochlorite for hypochlor acid
Naming compounds
Detailed treatise about naming organic compounds outside the scope of these ingredients, but some basic is served. Chemical students Wise must consider memorizing the first ten organic compounds:
The amount of carbon prefix
1 Meth-
2 ET-
3 prop-
4 but---
5 pent-
6 hex-
7 hept-
October 8-
9 non-
10 Dec-
There are four basic types of organic hydrocarbons, chemicals only with carbon and hydrogen:
Single bonds (alake): Sufix is "ane", Formula CNH2N + 2
Double bonds (alkenes): Suffix is "ENE", CNH2N Formula
Triple Bonds (Alkyne): Suffix is "Yne", Formula CNH2N-2
Cyclic compounds: Use the "Cyclo" prefix
So, for example, organic compounds with the formula "C64" will be recognized as alkane with six carbon, so the name is "hexane".
Example:
N2O4 = Dinitrogen Tetraoxide
S2F10 = Dissafluoride
Practice problems
Find the following molecular-molecular formulas:
1. Aluminum Fluoride 8. Ammonium Dichromate
2. Carbon Tetrachloride 9. Magnesium acetate
3. Strontium nitrate 10. Zinc hydroxide
4. Sodium bisulfate 11. Nitric acid
5. Iron (iii) oxide 12. Hypoclor Acid
6. Mercury (II) nitrate 13. phosphoric acid
7. Sodium sulfite 14. Aluminum nitrate
Set solutions available for views.
Write the following molecular names:
1. CaCO3 8. MG3 (PO4) 2
2. SCL2 9. BA (NO 2) 2
3. LI2CRO4 10. HG2CL2
4. NASCN 11. NAHCO3
5. KCLO3 12. H2S
6. CA (C2H3O2) 2 13. H2SO3
7. K2CR2O7 14. SO3
0 Comments: