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Group VAT Carbon is a nonmetal and is the element that started this group, which is also known as carbon family, the following two elements, silicon and germanium are metalloids; These first three elements form compounds with covalent character. Tin and lead, ending the group elements are metals.
The outer electron configuration of the elements of this group is (ns2np2). The present trend in the decrease of melting and boiling points of silicon to lead, indicating that the metallic nature of elements of this group is growing.
Carbon can be considered as the most important of this group, because from carbon are all organic compounds, ie the chemistry of life. Silicon is a very abundant element in Earth's crust and is used in the manufacture of chips for microcomputers. Germanium, as a semiconductor of electrical current, is used in the manufacture of transmitters, and the last, lead and tin are typical uses of metals. 6C
14Si 32Ge 50Sn 82Pb

VA
Group This group is known as a family of nitrogen. It is composed of nitrogen and phosphorus, which are non-metals; arsenic and antimony are metalloids, and bismuth, a metal. The outer electronic configuration has (ns2np3). Nitrogen, which exists as a diatomic gas, is a nonmetal, important as parent of the atmosphere (about 78%), and is vital for plants and animals. Phosphorus is a solid metal no biological significance to react with oxygen in the air violently burning off large amounts of heat. 33As 51Sb
83Bi 7N 15P


Form Group VIA's family consists of oxygen and oxygen, sulfur and selenium are nonmetals, as well as tellurium and polonium, which are metalloids. The outer electron configuration is presented (ns2np4). They tend to accept two electrons to complete its final layer to form ionic compounds with many metals.
The elements of this group of non-metals react with other groups to form molecular compounds, particularly oxygen, which is in the air as a diatomic molecule (O2) and ozone (O3). It is also very reactive, as it forms compounds with most elements. It is necessary for combustion and essential for life. 8O
34Se 16S 52Te 84Po


Known as Group VIIA halogen family show a very similar chemistry. The elements of this group are nonmetals and exist as diatomic molecules in their elemental state. Elements are very reactive at room temperature is liquid bromine and solid iodine. However, a radioactive element astatine and little is known about their properties. The outer electron configuration is presented (ns2np5) and tend to gain an electron to complete its last layer. Because of its high reactivity was not found in pure form in nature.; To anions that form to gain an electron are known as halides. Form ionic compounds with alkali or alkaline earth metals and molecular compounds between themselves or with other non-metals. 5I 35Br 17Cl 9F
85At

Group or Group VIIIA
zero in this group are the noble gases, helium, neon, argon, krypton, xenon and radon. Have their last full electronic layer (ns2np6), except helium, which is single layer (1s2), which is also full, hence, its tendency to combine with each other or with other components is low or almost nil. Do not have a tendency to gain electrons, because of this, for many years was called inert gases, it was thought that did not react. Currently, we have managed to synthesize some compounds, but is commonly used as pure gases.
Helium is the lightest. Compared with air, is the seventh of its weight, therefore, has considerable lifting power. Argon is an excellent conductor of heat, and is used in light bulbs and welding of magnesium to prevent rusting. Neon is widely used in retail, advertising lights. 10Ne 18Ar 36Kr 2HE
54Xe 86Rn



A Group B elements belonging to groups B in the periodic table are called transition elements, a transition element is one that has partially filled the orbital do f. They are located in the periods 4, 5, 6 and 7, those in the period 6 comprise the lanthanide series, and the period of 7, that of actinides, these two series are known as metal internal transition.
For the transition elements d-block, the atoms can have one and nine electrons in that orbital. When the d orbital is full, the item is no longer in transition. All transition elements are metals of great importance in the industrial level by high melting points and good mechanical properties.

Wordings For Appreciation

Periodic Table Periodic Table II

One of the major sources of information that the student account of Biotechnology, Chemistry and Biochemistry is the periodic table. Here the elements are classified based on the similarity of their properties, which repeated at regular intervals are called periodic properties.
The structure of the periodic table the proposals is due to Mendeleev, Meyer and Moseley, as well as A. Warner. In analyzing the periodic table the elements are ordered increasingly from its atomic number, divided into periods and groups, both horizontally and vertically, respectively. In addition, points out what metals, nonmetals, transition metals and other groups of elements known as rare earths.
The periodic table is a ranking of the 109 known chemical elements present, in order of increasing atomic number. There were several attempts that were made from 1817 to 1914 and more recently still, to classify elements.
The classification of elements based on atomic number resulting in the modern periodic table of Alfred Werner. This table contains all the elements found in nature as well as those obtained under laboratory conditions, and are arranged according to the electronic structure of atoms, showing a gradual accommodation of the valence electrons in energy levels {periods }. The elements have similar outer electron configurations, grouped in vertical columns are called families or groups.
also that the elements are located in the periodic table in ascending order, based on atomic number and, consequently, its electronic configuration, we can tell that it is also located kinds of elements, periods, groups or families and blocks.
classes of items.
When items are classified according to their physical and chemical characteristics, forming two main groups: metals and nonmetals. There is also a third set of elements that are characterized by the uncertainty of its properties located between metals and nonmetals, called metalloids or semimetals.

Metals Metals are recognized by their physical properties, such as metallic luster, electrical and thermal conductivity, hardness, ductility and malleability. In metals the same period is more reactive which has fewer electrons in its outer shell. Compared to sodium and aluminum, found in the second period, the more reactive sodium because it has a valence electron and aluminum has three, it is easier to give an electron to two or more. Na11
2P6 1s2 2s2 3s1 outer layer 1 valence electron
Al13 1s2 2s2 3s2 3p1 2P6 outer layer 3 valence electrons

Nonmetals Nonmetals are elements that tend to gain electrons to complete its outer shell with eight and thus achieve a stable configuration of noble gas. Are more reactive the lowest number atomic, because in this case the distance between the nucleus and the electrons of the last orbit is lower and, or both, the attraction of the nucleus to the electrons of other elements is greater. Thus, in the group of the most reactive halogen is fluorine, atomic number 9, and the less reactive is iodine, atomic number 53, because although both have seven electrons in its valence shell, the fluor are attracted more strongly, by being closer to the core, that iodine, which are at level five. Metalloids

The elements boron, silicon, germanium, arsenic, antimony, tellurium and polonium, which are above and below of the ladder line that divides metals from nonmetals are called metalloids because their properties are intermediate between metals and nonmetals, for example, conduct electricity, but not so much metal.
periods long
The periodic table is composed of seven periods, arranged horizontally from 1 to 7. These numbers correspond to the energy levels of the atom, where electrons are located. The number of the period where it is located an item indicates the maximum level of energy in the atom of that element will have electrons, for example, iron (iron) is located in period 4, which is the maximum power level which has electrons. Fe26
2P6 1s2 2s2 3s2 4s2 3p6 3d6
maximum electron energy level
In the first three periods are called short periods, and the remaining four long periods. The following table shows the number of elements that make up each period.


periods (energy levels) No. of items sublevels Ends Begins in
February 1 H He Li 1s Ne
August 2 August 3
2s 2p 3s 3p Na Ar K
April 18 Kr 4s 3d 4p Rb
May 1918 Xe 5s 4d 5p
June 1932 Rn Cs 6s 4f 5d 6p Fr Une
July 23 5f 7s 6d periods
Features
As you can see in the periodic table, the seventh period, which begins with France, has empty places for new items that are expected to have properties similar to those of the group elements corresponding to them.

Groups or families are a set of elements with similar properties. Are arranged in vertical columns and are identified by Roman numerals I through VIII. They are divided into groups A and B. For the elements of groups A, the IA to VIIA is called representative elements, and group B, the transition elements.
Description of groups or families

Group IA elements belonging to this group are known as alkali metals. All are soft and bright (except for hydrogen, which is a non metal), highly reactive with air and water, hence, are not free in nature and when able to isolate, to avoid reacting, must be kept submerged in certain liquids such as oils or petroleum ether. React with VIIA group elements form ionic compounds.
Its outer electron configuration is (ns1), tend to lose this electron and stay with oxidation number + 1. These metals are more electropositive. Francium is the last element of this group is radioactive.
In the periodic table hydrogen is placed in this group due to single electron who owns it is a gaseous element and its properties are not the same as the rest of the alkali metals. 1H
3Li 11Na 37Rb 19K 56Cs 87Fr


Group IA IIA
Group have certain properties similar to alkali metals, but are a little less reactive and they are known as alkaline earth metal. With oxygen in the air form oxides and react with the elements of group VIIA (halogen) to form salts.
have completed his orbital s in its outer shell (ns2) and tend to lose these electrons taking the noble gas configuration above them, hence, its oxidation number is +2.
The reactivity of these metals increases as you move from top to down on the group: for example, beryllium and magnesium react with oxygen to form oxides only at elevated temperatures, while calcium, strontium and barium do at room temperature. The radio, as well as France, the former group, is a radioactive element. Group IIA 4BE

12mg 20Ca 38Sr 56Ba 88Ra

IIIA
Group This group is composed of boron, aluminum, gallium, indium and thallium. Boron is a metalloid, and the four remaining metallic elements, perhaps the most important properties and abundance is aluminum, which when combined with oxygen, forms a cover which prevents any further reaction, which is why this metal is used in the preparation of articles and structural materials. The outer electron configuration is presented (ns2 np1). These elements also form molecular compounds, which are characteristic of non-metals, this is explained by the electronic configuration and its present location in the table, as they move from left to right in the periodic table, the metallic nature of representative elements gradually begins to lose. 5B

13Al Group IIIA 31Ga 49In 81Tl

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inorganic chemical nomenclature

CONTINUED

The substances are characterized by their name and their physical and chemical properties. However, there are several names misused, confused or rare.
Examples:
oil of vitriol (sulfuric acid)
blue vitriol (copper sulphate)
quicklime (calcium oxide)
off Cal (calcium hydroxide)
If we were to give a complete list of the properties of such substances as melting point, boiling point, color, shape, etc., would be an endless list that hardly anyone can hold in memory, it is easier to name the substance and thus associate its properties.
best in the eyes of a chemical is, the formula. A formula as a symbol, representing a large amount of information quantitative and qualitative chemical. CHEMICAL FORMULAS

A formula is the representation of the manner in which it formed a compound. For example the formula: H2O, we say that water contains two elements hydrogen and oxygen O. H Also tells us that each water molecule has two hydrogen atoms and one oxygen atom. The formula also tells us if the atoms are bound together by shared electrons (covalent bonds) or by electrostatic attraction of oppositely charged ions (link electrovalent).
What can we do to give names to many formulas?
The first is to use an appropriate nomenclature.
To facilitate communication between the formulas was a need to develop a unique language, systematic and uniform to identify chemicals. This language has been developed by the IUPAC (International Union of Pure and Applied Chemistry), which is under constant review in order to adapt to the compounds discovered every year. There
trivial nomenclature
compounds with names that have names that do not follow IUPAC rules, these names are considered trivial or common and learned in practice and not to rules and then some compounds are noted with their most common names : H2O Water


Ammonia NH3 N2H4 Hydrazine
Alumina Al2O3 CaO
Sosa Cal
NaOH KOH caustic potash


OXIDATION NUMBER
To remember the formulas of the compounds and write properly, it is useful to use a system called oxidation oxidation numbers. The oxidation number system was developed based on the composition of the compounds, the relative electronegativities of the elements forming compounds and a set of rules and arbitrary.
Some of these arbitrary rules are: a.
The oxidation number of an uncombined element is 0. B.
In a compound, the more electronegative elements have oxidation number negative, while the less electronegative elements have positive oxidation states. C.
In each formula of a compound, the sum of the negative oxidation numbers equals the sum of positive oxidation numbers, ie the algebraic sum of oxidation numbers of a compound should always be zero because molecules are neutral.
Examples:
₊ Na 1 Cl 1
Na2SO4 ₋ Na2 ₊ ₊ 1 S 6 O 4 2
CO2 ₋ calculate the oxidation
No. 2O7 Cl calculate the oxidation
No. OF2 calculate the oxidation
No. Table periodical is a guide to establish some criteria that will be useful for predicting the No. oxidation of the elements, according to the group to which they belong. Consider the following table:
GROUP IA IIA IIIA IVA VA VIA VIIA


No. oxidation
ng +1 +2 +3 +4 +5 +6 +7 +2 +3 +4 +5

2 +1

+1 +2 +3 4 3 2 1


As shown, the IA group elements always have oxidation number of +1, (hydrogen when combined with metals have oxidation number 1, but when combined with nonmetals its oxidation number is +1).
in group VIA is the oxygen that is always a Oxidation number of 2 (only in the peroxide oxidation number is 1).
also shows that the elements of groups IVA, VA, VIA and VIIA, has variable oxidation numbers. This is because certain elements give or share electrons in several ways.
For example, the Fe (has variable oxidation number like other transition elements) shows the oxidation numbers of +2 and +3. To avoid ambiguity in the names of the compounds, indicating the number of oxidation with Roman numerals.
iron II chloride FeCl2 FeCl3
iron III chloride
iron II sulphate FeSO4
This type of nomenclature is very recent so in most texts, the standard nomenclature is a bit different. A compound of an element with lower oxidation number is given and the termination bear higher oxidation numbers given termination ico. Ferrous chloride

FeCl2 FeCl3 Ferric Chloride Ferrous Sulfate FeSO4

Fe 2 (SO4) 3

ferric sulphate

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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

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There is a type of forces, although they are not true blogs, interact one to another molecule to produce an attractive force between them. These forces are known as intermolecular forces and are: hydrogen bonding and Van der Waals forces. Hydrogen bond



This type of forces present in compounds containing covalent bonds between hydrogen and a very electronegative atom, such as fluoride (HF), oxygen (HO) or nitrogen (HN, creating a dipole dipole attraction very strong. This type of binding occurs when a hydrogen atom from a molecule is attracted to a negative charge center of another molecule.
The attraction molecular hydrogen bridge can occur between the same or between different molecules. It is noted with a dotted line (.....) as shown in the example, (which the teacher presented in class.)
compounds whose molecules exhibit hydrogen bonding attraction have higher boiling points compared to analogous compounds of elements of the same group.
Examples: water boiling point 100 degrees Celsius.

Van der Waals forces
These are purely electrostatic forces. That is, they occur as a result of the attraction between opposite electrical load centers, very close together.
in the case of polar molecules, it is easy to understand the attraction between the positively charged (& positive) and the partial negative & negative). However, there are polar molecules, or which, when approaching each other, by the action of an external agent, such as temperature, induced dipoles are formed. With that also appear Van der Waals forces.