Types of Chemical Bonds

When two or more atoms form a molecule, they join together by means of a junction between electrons of its last layers, the most superficial. This union is called Chemical bond. For a chemical bond to form, the atoms must have their incomplete octet, that is, less than eight electrons in their last shell, which is the number that will give them chemical stability.

There are three types of chemical bonds:

1. Ionic bonds
2. Covalent bonds
3. Metal links

Ionic bonds

Ionic bonds are those in which the valence electrons are attracted by electrostatic forces. The atom (s) that have 1 to 4 valence electrons can deliver them to form the bond; This gives it a positive charge, because it would be getting rid of the negative charges. On the other hand, the atom (s) with 5 to 7 valence electrons will be able to receive those necessary to reach 8.

This gives them a negative charge, because they pick up electrons, which are negative. The fact that electrons can be captured or delivered gives the atoms the electrical charge

. According to Coulomb's law, the charges formed on both atoms they are going to attract each other with a force, which is the electrostatics mentioned above. Negative charges attract positive charges and vice versa. Opposite charges attract. Once this force binds them together, the molecule is formed.

Ionic bonds occur mostly between metal and nonmetal atoms. Metals give up their electrons and always carry a positive charge, participating as a cation (+). Nonmetals are electron receptors and generally carry a negative charge, participate as anions (-) but it also happens that they carry a positive charge, this when they form groups of charged atoms called radicals, as ammonium NH₄⁺, carbonate CO₃^-2, phosphate PO₄^-3.

Among the chemical compounds that are formed by ionic bonds are:

• Binary salts
• Oxisales

When these substances are dissolved in water they dissociate, namely, separate into their electrical charges and these are dispersed in the water together with the hydrogen ions H⁺ and hydroxyl (OH^-) that form water. The mixture that forms is a solution called electrolyte.

• Continue reading: Ionic bond

Covalent bonds

Covalent bonds are those in which electrons are shared without detaching them from the atom, that is, without the formation of electrical charges. The atoms are held together by proximity and use the force with which the nucleus attracts electrons. Once the bond is formed, the two or more nuclei of the atoms end up attracting the shared electrons, thereby fulfilling the octet rule and making the molecule stable.

There are several forms of covalent bonding, and they are:

• Covalent bond
• Coordinate covalent bond
• Polar covalent bond
• Nonpolar covalent bond

The covalent bond It is just like the one described at the beginning. The participating atoms share electrons so that they all have their complete octet. There are no electrical charges here, because no electrons are shed, they are just shared.

In the coordinate covalent bond it is only one atom that contributes all the electrons necessary for the bond. The other atom simply binds together and takes these electrons as its own. The molecule is formed like this. This is the case, for example, of sulfuric acid H₂SW₄ in which sulfur shares two pairs of electrons with oxygen atoms.

In the polar covalent bond, the forces between the atoms are tilted to one side of the molecule. This when there are different types of atoms in the molecule. This force is measured in Debye units, and the higher its value on one side of the molecule, the more polar it will be. This means that poles are formed in the structure, and that is why they are given this name. Its forces are asymmetric.

In the nonpolar covalent bond, the forces between the atoms are uniform throughout the entire molecule, and therefore no poles are formed in its structure. It works as a single unit and that is why it is very difficult, almost impossible, to divide its loads. This makes it insoluble in water. This is the case of compounds such as alkanes, which have their equal forces throughout the molecule. Its forces are symmetrical.

• Continue reading: Covalent bond

Metallic bond

The atoms of a metal are held together by means of metallic bonds. In this type of bond, the electrons of all the atoms are attracted to form a crystalline lattice that remains firm. The bonds of the crystal lattice have all electrons interspersed and arranged to carry electrical current and heat when it is transmitted to them. In transition metals this structure of metallic bonds is more remarkable, because their atoms are larger.

Examples of ionic bonding

Some substances that present ionic bonds are:

1. NaCl sodium chloride. Its ions are Na⁺ and Cl^-.
2. Potassium chloride KCl. Its ions are K⁺ and Cl^-.
3. Calcium chloride CaCl₂. Its ions are Ca⁺² and Cl^-.
4. Magnesium chloride MgCl₂. Its ions are Mg⁺² and Cl^-.
5. Strontium Chloride SrCl₂. Its ions are Sr⁺² and Cl^-.
6. Barium Chloride BaCl₂. Its ions are Ba⁺² and Cl^-.
7. Aluminum Chloride AlCl₃. Its ions are Al⁺³ and Cl^-.
8. Na sodium sulfate₂SW₄. Its ions are Na⁺ And so₄^-2.
9. Potassium K sulfate₂SW₄. Its ions are K⁺ And so₄^-2.
10. Calcium sulfate CaSO₄. Its ions are Ca⁺² And so₄^-2.
11. Calcium sulfate MgSO₄. Its ions are Mg⁺² And so₄^-2.
12. Strontium Sulfate SrSO₄. Its ions are Sr⁺² And so₄^-2.
13. Barium Sulfate BaSO₄. Its ions are Ba⁺² And so₄^-2.
14. Na sodium phosphate₃PO₄. Its ions are Na⁺ and PO₄^-3.
15. Potassium K phosphate₃PO₄. Its ions are K⁺ and PO₄^-3.
16. Magnesium Phosphate Mg₃(PO₄)₂. Its ions are Mg⁺² and PO₄^-3.
17. Calcium phosphate Ca₃(PO₄)₂. Its ions are Ca⁺² and PO₄^-3.
18. Aluminum Phosphate AlPO₄. Its ions are Al⁺³ and PO₄^-3.
19. Ferrous Phosphate Fe₃(PO₄)₂. Its ions are Fe⁺² and PO₄^-3.
20. Ferric Phosphate FePO₄. Its ions are Fe⁺³ and PO₄^-3.

Examples of covalent bonding

Some substances that present covalent bonds are:

1. Methane CH₄.
2. Ethane C₂H₆.
3. Propane C₃H₈.
4. Butane C₄H₁₀.
5. Pentane C₅H₁₂.
6. Hexane C₆H₁₄.
7. Heptane C₇H₁₆.
8. Octane C₈H₁₈.
9. Propylene CH₂= CH₂–CH₃.
10. Acetylene C₂H₂.
11. Methyl alcohol CH₃
12. Ethyl alcohol C₂H₅
13. Propyl alcohol C₃H₇
14. Isopropyl alcohol CH₃CH (OH) CH₃.
15. 2-propanone or acetone CH₃Car₃.
16. Formaldehyde HCHO.
17. Acetaldehyde CH₃
18. Propionaldehyde CH₃CH₂
19. Butyraldehyde CH₃CH₂CH₂
20. Formic acid HCOOH.

Examples of metallic bond

Some substances that present metallic bond are:

1. Zinc Zn
2. Cadmium Cd
3. Copper Cu
4. Silver Ag
5. Gold Au
6. Nickel Ni
7. Palladium Pd
8. Platinum Pt
9. Cobalt Co
10. Rhodium Rh
11. Iridium Go
12. Iron Fe
13. Ruthenium Ru
14. Osmium Os
15. Manganese Mn
16. Chromium Cr
17. Molybdenum Mo
18. Wolfram W
19. Vanadium V
20. Zrconium Zr

Follow with:

• Atoms
• Ion
• Metals
• No metals
• Alkanes
• Solutions