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bloom this spring, and you'll be the owner

my pollen.


spend the summer basking in the autumn came



shedding your touch


the winter cold in me.
till your vesos
Buelvas my

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script from the Wall p. 52.

daughter is the metaphor of free alveario

being being.
father
verse poetry and character
feeling

'm elated
mystical in romanticism
subsist in primitive rebel
dissatisfied

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shipping included.
To purchase this book of poems,
or comment on anything,
write to the author:
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Nogales Julián González Peñarroya-Pueblonuevo
, 1958
poet and playwright

c / Valderramas n º 12, 2 ª 14002 Cordoba
door

juliannogales@hotmail.es
http://juliannogales.blogspot.com

want to reach readers with my writing at a popular price is flat this writing mine does not require much knowledge to taste but a intuition Grodan

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Intermolecular Forces Liaison

METAL LINK
This link is presented in metals and alloys to form metallic glasses. Nature
link: Red crystal ions hardware (very electropositive elements) where the valence electrons are exchanged quickly.
Examples are substances that have: all metals, Au, Na, Fe, Ag, alloys such as steels, amalgams of mercury, copper and its alloys Cu - Zn, Cu-Ni, Cu - Sn, etc.
Properties derived from this type of link. Melting points, high boiling, metallic luster, hardness, malleability (rolling, stretching, bending), ductility (thread, wire), high electrical and thermal conductivity.
Another way to describe the metallic bonding is the existence of positive ions in a "sea electron gas" due to mobility of electrons, this mobility is due to the electrical conductivity and malleability.
In the "electron gas model" of metals, a regularly ordered lattice of positively charged metal ions is surrounded by electrons that can move freely. The easy mobility of the electron gas is responsible for the good electronic conductivity and thermal properties of metals.








If moving parts of a metallic glass, one over the other by a mechanical action (a). Each component in each new position above the same neighborhood, therefore, displacement, and thus the malleability of a metal, are easily possible without losing cohesion. By contrast, in an ionic crystal (b) components, by moving, are parties to the same charge: promotes mutual repulsion easily break the glass.


(a)

(b)
Note: The examples will be seen in class to visualize the diagrams, and drawings that does not accept the Blog.

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Metallic Covalent bond Ionic bond

The bond between two atoms that share electrons.
For example, the formation of the chlorine molecule, which exists as a diatomic molecule (Cl2). Their union as ionic bond is not possible, because a chlorine atom can not transfer an electron to another atom, chlorine also complete its octet, it would get the first six electrons in its valence shell.
To explain the link of this molecule and others in which atoms join the same or similar electronegativity. Lewis suggested that a chemical bond can be formed when two atoms share a pair of electrons, so that both atoms complete their octet in the valence shell.
2s22p6 3s2 3p2 17Cl 1s2 3p2 1s2 3p1 2s22p6
Cl2 3p2 3s2 3p2 1s2 3p2

17Cl 2s22p6 3s2 3p2 3p2 3p1
In this form of marriage, the two chlorine atoms have 8 electrons in its valence shell. This union is known as covalent bonding. This link is when the electronegativity of two atoms that bind the same or different (bends that electronegativity is the force with which an atom attracts the bonding electrons).
is necessary to consider that the more electronegative element is fluorine atom, with a value arbitrarily consider Lewis (4). When the electronegativity difference between atoms is too large the bonding electrons are transferred completely to the more electronegative atom, forming an ionic bond, and when this difference is small, it means that atoms have similar attractive force on the electrons, so that share, forming a covalent bond.
nonpolar covalent bond, polar and coordinated.
• nonpolar covalent. When the electronegativity difference is zero, the bond is covalent and the electron cloud of the link is evenly distributed around the two nuclei of atoms they join. When this happens, we say that it is a nonpolar covalent. Usually formed by two identical atoms, for example, hydrogen molecules (H2), chlorine (Cl2), fluorine (F2). Represent these samples using the Lewis structure and diagram area, the fluorine molecule. Lewis Diagram
:




covalent bond Cloud

electronic link


Nuclei

polar covalent
• The polar covalency occurs when the electronegativity difference is greater than zero but less than 1.7. analyze the formation of the molecule of hydrogen bromide, HBr. Electronegativades table (found in chemistry textbooks in the chapter on chemical bonding), we obtain the value of each atom and we can determine the difference in electronegativity. • Br ₌
2.8
-
H ₌ 2.1 0.7 Difference

electronegativity
The bromine atom more strongly attract the electron pair and the electron density is higher in this atom, as shown:


representation of the electron cloud of a polar molecule





From this analysis, We conclude that the polar covalence is that which occurs when two atoms are linked by covalent bond have a partial electrical charge separation (δ and δ ₊ ⁻) caused by the difference in electronegativities. Δ ₊ δ
⁻
H - Br
coordinate covalent bond Such
exists when one of the two atoms brings the pair of addresses. Given this name because there is coordination between the two atoms so that both can meet the octet rule.
This link occurs when an atom has a pair of free electrons (eg, nitrogen, oxygen and sulfur, among others) and shares with another atom that needs electrons to complete the pair with a layer of eight electrons valence.
An example of coordinate covalent bond is the formation of ammonium ion (NH4 ₊) from ammonia (NH3 ₊), which shares the nitrogen electron pair with a proton (H ₊), which requires the pair of electrons to stabilize. The diagram and explanation
present it the teacher in class.

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is defined as:
• The type of bond that is formed by the complete transfer of electrons.
• It is the electrostatic force that binds two ions of opposite charge.
Example: LiCl (lithium chloride) in this case the lithium transfers an electron to the chlorine atom and thus both acquire the configuration of a noble gas. 17Cl 3Li

₊ 1s2 2s1 1s2 3p2 3s2 3p2 2s2 3p1 2P6

an electron transfer

Atoms alkali metal (flu IA) can only provide an electron, which have in its valence shell. The alkaline earth metals (group IIA) can transfer two or more electrons. There are atoms such as halogens (group VIIA), which need only one electron to complete its octet, and others such as oxygen, sulfur they need more than one electron.

By losing electrons, atoms become positive ions, also called cations, and winning become negative ions or anions. There is an electrostatic attraction between the two, being the force that holds together the ions in an ionic compound. Li

₊ Li ₊ ₊ Cl Cl ⁻ ⁻
Cation Anion Salt
(Lithium) (chloride) (sodium chloride)

Run the following examples:

₊ I K potassium iodide KI O

2RB ₊

rubidium oxide Ca S ₊ calcium sulfide

₊ Mg Br Magnesium bromide
Cl
Al ₊

aluminum chloride ionic compounds are formed by reacting atoms less electronegative elements, for example: group IA, IIA, IIIA group elements, with more electronegative elements, such as the VIA and group VIIA.
Note: Due to the difficulty of representing here the formation of ionic compounds with Lewis structures, this will be presented by the teacher in the classroom. However, after studying them is from their atoms and by structure Lewis, following the formation of ionic compounds.

1. MgO

2. Na2S

3.

Al2O3 4. KL

5. CaCl2

6. BaS

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Stability of atoms

CHEMICAL BOND Stability of atoms
Development
the following atomic orbitals. 2HE
1s2 1s2 2s2
10Ne 18Ar
2P6 2P6 1s2 2s2 3p6 3s 2
3s 2P6 36Kr 23p6 1s2 2s2 4s2 4p6 3d10 1s2
54Xe 3s 23p6 2P6 2s2 4p6 3d10 4s2 5p6 5S2 4D10
86Rn 3s 23p6 2P6 1s2 2s2 4p6 3d10 4s2 5S2 4D10 5p6 6S2 6p6 5d10 4f14

1s 1s 2s 2p 3s 3p 4s 3d 4p 5s 4d 5p 6s 4f 5d 6p 7s 5f
2s 2p fill these orbitals with the number of electrons corresponding
3s 3p 3d.
4s 4p 4d 4f 5s 5p 5d 5f

6s 6p 6d 6f 7s 7p 7d 7f


How is the water molecule?
Both hydrogen and oxygen gain stability by sharing electrons.
8O +2 O 2p2 2s2 2p1
1s2 2p1 + 1s2 2s2 1S1 +1 s1 2p2 2p2 2p2 + H-H-
Oxygen won two electrons that takes the sub +2 and the hydrogen index lost 1 electron each therefore carries sub index -1.
Examples:
Writes electronic configuration of each of the following ions;

26Fe 17Cl
53I
47Ag 29Cu
Notes
who won and who lost electrons
Stresses ions have a noble gas electron configuration;
-2O
2P6 1s2 2s2 +2 Ca 2s2 1s2 3s2 3p6 2P6
+3 Fe (Ar) 4s2 3D3-3P
2P6 1s2 2s2 3p6 3s2 1s2 2s2-3N
2P6
We conclude that an atom takes on the stability of a noble gas to win, lose or share electrons in their valence shell when combined with other atoms forming chemical bonds. If the valence electrons are involved in the combination of atoms, then, to define valence as
COMBINATION BUILDING AN ATOM

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VALENCIA
is the combining capacity of an atom. To determine the valence of an atom, is referenced to the hydrogen atom, because when you are forming a binary compound (compound composed of two different elements) is never in combination with more than one atom of another element, which is why which gives a combined capacity of 1, ie its valence is 1.
Example:
hydrogen chloride or hydrochloric acid, HCl hydrogen atom combines with one of chlorine, so the valence of chlorine is also 1.
Cl-H1 CL17
2P6 3s2 3p2 1s2 3p2 2s2 3p1 + 1s2 1S1 3p2 3s2 3p2 2s2 3p2 2P6
H +
Therefore, the valence of hydrogen is +1 and that of chlorine is -1. D
The water molecule (H2O), oxygen combines with two hydrogen atoms, so their valence is -2. O8 O-2

3p2 2s2 3p1 1s2 3p1 1S1 + 1S1 + 3p2 1s2 3p2 2s2 3p2
H + H +
determines the valence following compounds: LiCl
,
CaCl2, AlCl3

metals (group IA) and alkaline earth (Group IIA) have a fixed valence +1, +2 respectively. There are other elements that have more than one valence or valence variable
Example:
carbon monoxide (CO) Carbon is the valence of +2 because it is combined with an oxygen atom, whose valence is -2, in the case of carbon dioxide (CO2) carbon has a valence of +4, then combined with two oxygen atoms in these cases the carbon valence of +2 and +4.
determines the valence of the following compounds:

N2O NO NO2


N2 O3 O5 N2
The nitrogen valences are 1, 2, 4, 3, 5 respectively.
the oxidation number is another concept used to describe the combining capacity of an atom. This is an integer that can be positive or negative and describes the combining capacity of an atom, as well as indicate the behavior of electrons in n compound.
In the compound lithium chloride (LiCl), lithium, losing an electron, remains ion (Li +) with an electrical charge of +1 or ion, which is equal to the number of oxidation, while chlorine, winning that electron, it becomes ion (CL-) with electric charge or oxidation number -1. As you can see by combining these two atoms, one loses an electron and the other wins, this indicates the behavior of the electron, ie, the oxidation number. LINKS BETWEEN ATOMS

Relationship between ionization energy and atomic number.
In the forming and breaking of chemical bonds, ionization energy and electrons play an important role. As we know, potential or ionization energy is the energy required to extract an electron from the atom, that energy must be able to break the force of attraction between electrons and protons in the nucleus. This force is inversely proportional to the distance between them, ie between an electron further away from the nucleus, the attraction will be less.
When an electron absorbs energy from outside the atom moves to a higher energy level (excited state) of which was (baseline), therefore, the distance from the nucleus increases and decreases the attractive force requiring less energy to remove it.
The ionization energy decreases in the periodic table upside down in a group and increases from left to right in a period analyzing the last paragraph and noting the position of the elements in the periodic table for those who are in a period closer to the noble gases, it takes more energy to remove an electron than those found at the beginning of the period, ie, the former tend to gain electrons and second to lose. Therefore
before starting the study of chemical bonds, we will explore ideas about the chemical bonds that provided the scientific Kossel and Lewis.

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Valencia Chemical Bond

CHEMICAL BOND
The unit I learned that chemistry is a science that is responsible for studying matter and its transformations also define the atom as the smallest particle of an element there, which is composed of electrons, protons and neutrons and can participate in a chemical reaction. Now analyze the chemical bond as the force that holds together two atoms or ions of opposite charge. But by joining the atoms, matter undergoes a transformation, and likewise, if we break this union, we are making a change in the structure of matter, so we can say that any transformation in the matter exists or break training chemical bonds, hence the importance of understanding how a bond is formed. DEFINITION OF CHEMICAL BOND
.
is the force that holds together two atoms or ions of opposite charge. CHEMICAL LINKS

1. Ion
2. Covalent. Non-polar, Polar, Coordinated
3. Metallic
4. Intermolecular forces. Hydrogen bond, Van der Waals forces
is important to remember that the links, the electrons play an important role, because in order to form there must be gain, loss or sharing of electrons between atoms that bind.
Example: look at the structure or electronic configuration of the element lithium (Li): Li3
1s2 2s1 valence shell
When compared with the noble gas helium (He) 1s2 He2

We realize that lithium, to acquire the configuration of helium, it makes up an electron. If lithium removes some form an electron, to stay with a proton more and, therefore, with an electric charge of + 1, then have the stable electronic configuration of noble gases:
Li3 1s2 2s1 Li + 1s2
I 1s2
now work with electronic configuration of chlorine (Cl): CL17
1s2 2s2 3s2 2P6 3P5 2P6
Ar18 1s2 2s2 3p6 3s2
purchase order for the chlorine argon configuration, it lacks an electron. If you somehow get the chlorine needed to achieve the electron configuration of argon, an electron will have more and, therefore, an electric charge of -1. Ie CL17
1s2 2s2 3s2 2P6 3P5 + e-Cl-2P6 2s2 1s2 3s2 1s2 2s2 3p6
Ar18 3s2 3p6 2P6
Now if combined lithium, you need to remove an electron, and chlorine that requires an electron, both acquire the settings stable noble gas, in this way is obtained the so-called lithium chloride:
Li · + Cl Li + Cl-
1s2 2s1 1s2 2s2 2P6 3S2 3P5 1s2 1s2 2s2 2P6 3s2 3p6