How To Add Pokemon Fire Red Cheats On Gpsphone

Learning to name the chemicals

UNIT 3:
LEARNING TO APPOINT THE CHEMICALS

3.1: Sales, 3.2: Oxides; 3.3: Acids, 3.4 hydride, 3.5; Hydroxides

3.1: THE SALES

ionic compounds are formed two ions: a.
Cation called a positive ion in the formula is always written first, but is named at the end. B.
A negative ion called an anion, the formula is always written at the end and was named to the top.

cation: monatomic cations consist mostly of metallic elements. These ions are named the same element. Examples
;
March 2
Na ion Zn ion sodium ion zinc aluminum Al

If the element can form more than one positive ion, the positively charged ion indicated by the Roman numeral after the name of metal.
Examples:
2    2  3
iron ion Fe II Fe III iron ion copper ion Cu I Cu II ion copper
An ancient method still widely used to distinguish between two different loads of a metal ion, use the endings "BEAR" or " ICO ", these terms represent the lowest load and the highest ion respectively. It uses the Latin root of the element. Examples
;
2  3 
Fe ferric ferrous iron Fe

 2 
cuprous ion Cu cupric ion Cu
The only polyatomic cations are listed below:
 2 
ammonium ion NH4 Hg I or mercurous mercury ion

3.2: BASIC OR METAL OXIDES

are binary compounds . When you combine a metal with oxygen (oxidation number 2 ) form the core or metal oxides. 
METAL OXIDE OXYGEN BASIC RULE NOMENCLATIRA

.
1. To write the formula is written first metal (cation) and then the oxygen (anion).
2. To name is written first oxides word "rust" followed by the preposition "de" and the name of "metal." Examples
;
 2  3  2 
O Na Na2O sodium oxide Al O  aluminum oxide Al2 O3

When the metal has several oxidation states as in the case of transition metals (Group B periodic table), the metal oxidation state is indicated by a roman numeral after their name. Examples
;
2  2  
Fe O II FeO iron oxide or iron oxide


Fe 3 O   Fe2 O3 III iron oxide or ferric oxide oxides



acid or anhydride compounds are binary. When NO combines metal with oxygen (oxidation number  2) oxides form acids or anhydrides.
NO METAL OXIDES   OXYGEN ACIDS CLASSIFICATION RULE


oxides to name acids, the prefixes mono, of, tri-, tetra, etc, to indicate the number of atoms of "oxygen" and the number of atoms "non-metal." Examples

;
CO 
carbon monoxide sulfur trioxide SO3 
O5 N2 nitrogen pentoxide 
O10 P4 phosphorus tetra  Decaóxido

Note: OXIDES acid or anhydride to react with WATER Oxoacids (acids with oxygen).
OXIDE ACID  WATER  Oxoacids

SO3  H2 O  H2SO4

CO2  H2O  H2CO3

3.3: ACID

An acid can be described as a substance that releases hydrogen ions (H +) when dissolved in water: The formulas of the acids contain one or more hydrogen atoms and an anionic group. According to the definition of Bronsted-Lowry acid is any substance that can donate protons (H +). In the formulas of all the acids the hydrogen element is written first. There are two kinds of acidic
(a) HYDRAZIDE
which contains no oxygen. Binary acids are formed by the combination of hydrogen with a non metal. Are named using the word acid generic Latin name followed by the non-metallic element with the ending water. At hydracids are considered as hydrides of the elements of groups VI and VII.
EXAMPLES: hydrogen sulfide H2S


HI hydroiodic acid HBr ácidobromhídrico
HF hydrofluoric acid
HCl hydrochloric acid
REMEMBER, HX (X = F, Cl, Br, I) in gaseous state is not an acid, in water dissociates to produce H + ions, its aqueous solution is called acid

EXAMPLE:
HCl (g) + H2O (l) → HCl (aq)
hydrogen chloride hydrochloric acid

3.4: HYDRIDES

IONIC OR METAL HYDRIDES. Are binary compounds. Ionic hydrides the hydrogen form with more electropositive metals such as alkali and alkaline earth, becoming negatively charged hydrogen. METAL
  HYDRIDE HYDROGEN
CLASSIFICATION RULE

The nomenclature of hydrides or metal ion is done with the word "hydride" the preposition "de" and the name of "metal." Examples
;

Na H    NaH sodium hydride


Ca 2 H    calcium hydride CaH

HYDRIDES covalent. Are binary compounds. The number of hydrogen compounds are those which form covalent bonds, the number of compounds of hydrogen with carbon is enormous and most non-metals form several compounds with hydrogen.
NO METAL HYDRIDE   hydrogen covalently

CLASSIFICATION RULE
In covalent hydrides known common name is more prevalent than for the systematic nomenclature (IUPAC). Examples
;
CH4 Methane Carbon Hydride Hydride

NH3 Ammonia nitrogen

PH3 Phosphine Phosphorus Hydride

3.5: HYDROXIDES

When you combine a basic oxide or metal with water to form a hydroxide.

OXIDE HYDROXIDE BASIC   WATER

hydroxides are characterized by the hydroxyl radical (OH ), also called hydroxyl or hydroxyl. CLASSIFICATION RULE


To name these compounds enter the word "hydroxide", followed by the preposition "de" and the name of "metal" indicating its oxidation number Roman number (if it has several oxidation numbers). Examples
;

   K OH KOH potassium hydroxide

2    OH
Sr Sr (OH) 2 strontium hydroxide

2   
Cu OH Cu (OH) 2 Copper II hydroxide

4    OH
Sn Sn (OH) 4 hydroxide tin IV