Examples of atomic bonds

Atomic bonds

The atomic bonds are treated in the way in which one atom of a certain element is attached to another atom of the same element or another, either to form molecules of chemical compounds or to maintain grouped a certain amount of said element in a state of specific aggregation, as well as usually define the physical, chemical and electrical properties that matter can have.

Examples of atomic bonds

  1. H2O or water
  2. NaCi or table salt
  3. FeNaTi
  4. HCi Hydrochloric Acid
  5. CO2 Carbon Dioxide
  6. Hydrogen peroxide
  7. O3 Ozone
  8. C2H5OH Ethanol
  9. TiCI4 Titanium tetrachloride
  10. TiO2 Titanium dioxide
  11. OH Hydroxide
  12. Iron bars (Fe)
  13. Copper deposits (Cu)
  14. Pure Silver Bars (Ag)
  15. Magnesium oxide (MgO)
  16. Copper sulfate (CuSO 4 )
  17. Pure gold bars (Au)
  18. Glucose (C 6 H 12 O 6 )
  19. Potassium Iodide (KI)
  20. Manganese Chloride (MnCl 2 )
  21. Ammonia (NH 3 )
  22. Calcium carbonate (CaCO 3 )
  23. Freon (CFC)
  24. Iron sulfide (Fe 2 S 3 )
  25. Benzene (C 6 H 6 )
  26. Methane (CH 4 )

There are a variety of atomic bonds, each with its own characteristics, these are:

  • ionic bond where atoms share ions. They generally occur between metallic and non-metallic atoms, consisting of a constant transfer of electrons between the metallic atom and the non-metallic atom.
  • covalent bonds , the atoms share an external electron. In this sense, their relationship is between non-metallic atoms and atoms of electromagnetic charges that resemble, unite and share some pairs of electrons.
  • metallic bond where a metallic atom shares almost all its protons and electrons in almost totality with another atom of the same element or another metal. In this sense, we can say that it occurs only between metallic atoms that are part of the same element, generally constituting compact solid structures.
  • hydrogen bonds where a hydrogen atom shares its only electron with any other element for example the water molecule H2O. Y
  • the links van der Waals forces , which are the weakest links because they give basic physical reactions and phenomena in which matter can change easily aggregate state or return to their original state without much effort.

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