hmm
remember chemistry lesson in class X and XI ..
maybe it helps if these days I divide up the
material on the chemical bond ..
CHEMICAL BONDING
Chemical bonds in principle derived from the interaction between the electrons that exist in outer orbit, or partially filled orbit or orbit freely in the other atom.
1. The interaction of metal atoms (bond metallic / metal bonding).
In the interaction between the metal atoms, chemical bonds formed by the attractive force-pulls electrons by the core (nucleus) are different. Originally owned by the atomic electrons are drawn by the neighbor-charged atomic nuclei +, and these electrons dg be shared equally by the gravity of other nuclei around it. Due to the low number of valence electrons and there is a large amount of space kososng, then e-has plenty of places to move. Such circumstances can lead to e-migrate freely between these cations. These electrons are called "delocalized electrons" and the bond is also called "delocalized bonding".
Free electrons in orbit is acting as an adhesive or glue. Cation who live near each other to attract electrons as cement.
2. Covalent bond
2.1. Bonds with non-metals
In principle, all chemical bonds attractive forces derived from the core (nucleus) of the e +-charged negatively charged, the attractive force is determined by Coulomb's law.
F =
F: Tensile attract or repel
Q1 and Q2: Loads of particles 1 and 2
r: distance between particles 1 and 2
k: dielectric Konstante
If Q1 and Q2 equal charges, they are repulsive, otherwise if Q1 and Q2 opposite charge will be attractive.
Covalent bonds are formed, because almost all the elements have empty space and outer low-energy orbit. The lower the orbital energy, high stability Nakin electrons in it. All non-metallic elements have at least 4 of 8elektron that might be in outer orbit, except: H, He, and B.
The difference in the non-metal to metal is not have excess space for the deployment of low-energy electrons will be shared. Electrons can be shared in a non-metallic elements do not experience the "delocalised" as in metallic bonding (metallic bonding). So electrons stay localized in the proximity between two nuclei (covalent bonds).
Example: H2 formation of two atomic H. In the H2 molecule there are three forces acting are:
a). Repulsion between the two nuclei
b). Repulsion between two electrons
c). Force of attraction between the nucleus of an atom with electrons from other atoms. Magnitude of c is greater than the amount of force a and b.
Covalent bond in H2, 2 electrons be shared by two atoms and the orbit of the 2 electrons also be shared by two atoms.
Covalent bond: attractive force (net), which occurs when each atom supplies one unpaired electrons to be paired with another, and there is an empty space to accept electrons from other atoms, so that the two electrons are attracted by both nuclei are .
2.2. Valence or force merger
Valence of an atom is the number of covalent bonds that can be formed. Example: valence H = 1, He = 0, F = 1, O = 2, Li = 1.
3. Non-bonding metal to metal
Pairs of electrons that form a bond between the metal atom and the non-metal is in an orbit overlap between the two atoms. Because non-metal atom has no empty space with low energy, the electrons will be scattered in areas that overlap orbit.
Atoms of different elements have a different ability to attract a pair of electrons in a covalent bond.
F, O, Cl: strong pulling capability
Na, K: weak pull capabilities.
Electro-negativity: the relative ability of a substance to satisfy a negative electrical charge.
2.4. Ionic bonding (electro-valent, hetero-polar)
This bond is derived from the electrostatic attractive forces between charged ions berlawnan [Cations (+) and anions (-)]. (Coulomb's law)
For most elements, the release of electrons or tethering is an endothermic process (requires energy). This means that the ionic form is less stable than the uncharged atoms.
Na Na + + (-) - Energy
½ O2 + 2 (-) O-2 - Energy
Compounds that have the highest degree of the ionic bond is formed by the reaction between alkali elements with halogen.
Example: NaCl Na + Cl.
Both have a large electronegativity difference, so that the electron pairs form bonds more attracted by the Cl atom.
The greater the difference in electro-negativity greater the ioniknya character. However there are exceptions to F and Cs, F has the strongest electro-negativity, being Cs has an electro-negativity weakest, so the bond is not completely ionic. However there is a pure covalent bond in a molecule composed of the same molecule (H2, Cl2, CC) or a molecule that is composed of atoms that have electro-negativity is almost the same, for example: CH.
From an assortment of ties can be concluded as follows:
a). Compounds with covalent bonds are dominant, electrons of the atoms that bond is made bond. Among the different molecules was weak bonds called "van der Waals". The same thing happens to the compound to "coordinate covalent bonds". Different molecules to form separate units. In this molecule the distance between atoms in a molecule is smaller than the distance between atoms and molecules nearby.
b). Compounds with metallic and ionic bonding is dominant, it is made by bonding electrons be shared. In tensile metal comes from "delocalised electron", are in ionic compounds derived from attractive forces between positive and negative ions. In these compounds, the charged particles are positioned at the same distance from each other, so there is no possibility to distinguish or separate the intact molecule (discrete). In metals, each atom is usually positioned at the same distance of 6, 8 or 12 atoms are other shows that bond with all the different atoms have the same power.
In solid form, the structure of ionic like NaCl, each Na + is surrounded by 6 Cl at the same distance, each Cl-is surrounded by 6 Na + was also at the same distance, which suggests that each Na + drawn by six Cl-dg equal strength, each Cl - was also drawn by 6 Na + dg same power. Shape is only soluble in polar solvents (water) that can break ionic bonds with nature and form ion polarity hydrate (diseliputi ions with a coat of water).
Chemical bonds in principle derived from the interaction between the electrons that exist in outer orbit, or partially filled orbit or orbit freely in the other atom.
1. The interaction of metal atoms (bond metallic / metal bonding).
In the interaction between the metal atoms, chemical bonds formed by the attractive force-pulls electrons by the core (nucleus) are different. Originally owned by the atomic electrons are drawn by the neighbor-charged atomic nuclei +, and these electrons dg be shared equally by the gravity of other nuclei around it. Due to the low number of valence electrons and there is a large amount of space kososng, then e-has plenty of places to move. Such circumstances can lead to e-migrate freely between these cations. These electrons are called "delocalized electrons" and the bond is also called "delocalized bonding".
Free electrons in orbit is acting as an adhesive or glue. Cation who live near each other to attract electrons as cement.
2. Covalent bond
2.1. Bonds with non-metals
In principle, all chemical bonds attractive forces derived from the core (nucleus) of the e +-charged negatively charged, the attractive force is determined by Coulomb's law.
F =
F: Tensile attract or repel
Q1 and Q2: Loads of particles 1 and 2
r: distance between particles 1 and 2
k: dielectric Konstante
If Q1 and Q2 equal charges, they are repulsive, otherwise if Q1 and Q2 opposite charge will be attractive.
Covalent bonds are formed, because almost all the elements have empty space and outer low-energy orbit. The lower the orbital energy, high stability Nakin electrons in it. All non-metallic elements have at least 4 of 8elektron that might be in outer orbit, except: H, He, and B.
The difference in the non-metal to metal is not have excess space for the deployment of low-energy electrons will be shared. Electrons can be shared in a non-metallic elements do not experience the "delocalised" as in metallic bonding (metallic bonding). So electrons stay localized in the proximity between two nuclei (covalent bonds).
Example: H2 formation of two atomic H. In the H2 molecule there are three forces acting are:
a). Repulsion between the two nuclei
b). Repulsion between two electrons
c). Force of attraction between the nucleus of an atom with electrons from other atoms. Magnitude of c is greater than the amount of force a and b.
Covalent bond in H2, 2 electrons be shared by two atoms and the orbit of the 2 electrons also be shared by two atoms.
Covalent bond: attractive force (net), which occurs when each atom supplies one unpaired electrons to be paired with another, and there is an empty space to accept electrons from other atoms, so that the two electrons are attracted by both nuclei are .
2.2. Valence or force merger
Valence of an atom is the number of covalent bonds that can be formed. Example: valence H = 1, He = 0, F = 1, O = 2, Li = 1.
3. Non-bonding metal to metal
Pairs of electrons that form a bond between the metal atom and the non-metal is in an orbit overlap between the two atoms. Because non-metal atom has no empty space with low energy, the electrons will be scattered in areas that overlap orbit.
Atoms of different elements have a different ability to attract a pair of electrons in a covalent bond.
F, O, Cl: strong pulling capability
Na, K: weak pull capabilities.
Electro-negativity: the relative ability of a substance to satisfy a negative electrical charge.
2.4. Ionic bonding (electro-valent, hetero-polar)
This bond is derived from the electrostatic attractive forces between charged ions berlawnan [Cations (+) and anions (-)]. (Coulomb's law)
For most elements, the release of electrons or tethering is an endothermic process (requires energy). This means that the ionic form is less stable than the uncharged atoms.
Na Na + + (-) - Energy
½ O2 + 2 (-) O-2 - Energy
Compounds that have the highest degree of the ionic bond is formed by the reaction between alkali elements with halogen.
Example: NaCl Na + Cl.
Both have a large electronegativity difference, so that the electron pairs form bonds more attracted by the Cl atom.
The greater the difference in electro-negativity greater the ioniknya character. However there are exceptions to F and Cs, F has the strongest electro-negativity, being Cs has an electro-negativity weakest, so the bond is not completely ionic. However there is a pure covalent bond in a molecule composed of the same molecule (H2, Cl2, CC) or a molecule that is composed of atoms that have electro-negativity is almost the same, for example: CH.
From an assortment of ties can be concluded as follows:
a). Compounds with covalent bonds are dominant, electrons of the atoms that bond is made bond. Among the different molecules was weak bonds called "van der Waals". The same thing happens to the compound to "coordinate covalent bonds". Different molecules to form separate units. In this molecule the distance between atoms in a molecule is smaller than the distance between atoms and molecules nearby.
b). Compounds with metallic and ionic bonding is dominant, it is made by bonding electrons be shared. In tensile metal comes from "delocalised electron", are in ionic compounds derived from attractive forces between positive and negative ions. In these compounds, the charged particles are positioned at the same distance from each other, so there is no possibility to distinguish or separate the intact molecule (discrete). In metals, each atom is usually positioned at the same distance of 6, 8 or 12 atoms are other shows that bond with all the different atoms have the same power.
In solid form, the structure of ionic like NaCl, each Na + is surrounded by 6 Cl at the same distance, each Cl-is surrounded by 6 Na + was also at the same distance, which suggests that each Na + drawn by six Cl-dg equal strength, each Cl - was also drawn by 6 Na + dg same power. Shape is only soluble in polar solvents (water) that can break ionic bonds with nature and form ion polarity hydrate (diseliputi ions with a coat of water).
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