Introduction to Bonding

Chemical bonding defines a variety of interaction that host atoms with each other in chemistry compounds.

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Key Takeaways

Key Points chemistry bonds are pressures that organize atoms together to do compounds or molecules.Chemical bonds encompass covalent, polar covalent, and also ionic bonds.Atoms with reasonably similar electronegativities share electrons in between them and are linked by covalent bonds.Atoms with large differences in electronegativity deliver electrons to kind ions. The ions then space attracted to every other. This attraction is recognized as an ionic bond.Key Termsbond: A link or force between neighboring atom in a molecule or compound.ionic bond: an attraction between two ions supplied to develop an ionic compound. This attraction normally forms between a metal and a non-metal.covalent bond: an interaction in between two atoms, which requires the sharing of one or much more electrons to help each atom satisfy the octet rule. This interaction commonly forms between two non-metals.intramolecular: describes interactions within a molecule.intermolecular forces: describes interactions between two or an ext molecules.

Chemical bonds

Chemical bonds space the connections between atoms in a molecule. This bonds incorporate both strong intramolecular interactions, such as covalent and ionic bonds. They are pertained to weaker intermolecular forces, such as dipole-dipole interactions, the London dispersion forces, and also hydrogen bonding. The weaker forces will be debated in a later concept.


Chemical bonds: This photos shows instances of chemistry bonding utilizing Lewis dot notation. Hydrogen and also carbon space not bonded, when in water there is a single bond in between each hydrogen and oxygen. Bonds, specifically covalent bonds, are often represented as lines in between bonded atoms. Acetylene has actually a triple bond, a special type of covalent bond that will certainly be debated later.

Covalent Bonds

Chemical bonds room the forces of attraction that tie atom together. Bonds are developed when valence electrons, the electrons in the outermost digital “shell” of an atom, interact. The nature the the interaction between the atoms depends on their loved one electronegativity. Atoms through equal or comparable electronegativity form covalent bonds, in which the valence electron density is shared in between the 2 atoms. The electron thickness resides between the atoms and also is attractive to both nuclei. This form of bond forms most frequently between two no metals.

When over there is a higher electronegativity difference than in between covalently bonded atoms, the pair of atoms usually creates a polar covalent bond. The electrons space still shared between the atoms, yet the electrons are not equally attracted come both elements. As a result, the electrons tend to be found near one particular atom many of the time. Again, polar covalent bonds tend to occur in between non-metals.

Ionic Bonds

Finally, because that atoms with the largest electronegativity distinctions (such as steels bonding v nonmetals), the bonding interaction is called ionic, and also the valence electron are typically represented as being transferred from the metal atom to the nonmetal. Once the electrons have been moved to the non-metal, both the metal and also the non-metal are thought about to be ions. The 2 oppositely fee ions lure each various other to form an ionic compound.

Bonds, Stability, and Compounds

Covalent interactions are directional and also depend on orbit overlap, when ionic interactions have actually no specific directionality. Each of this interactions allows the atoms affiliated to acquire eight electrons in your valence shell, satisfying the octet rule and also making the atoms much more stable.

These atomic properties help describe the macroscopic nature of compounds. Because that example, smaller sized covalent compounds the are hosted together by weaker bond are commonly soft and malleable. ~ above the various other hand, longer-range covalent interactions deserve to be quite strong, making your compounds an extremely durable. Ionic compounds, though created of solid bonding interactions, tend to kind brittle crystalline lattices.

Ionic Bonds

Ionic bonds room a subset of chemistry bonds that an outcome from the transport of valence electrons, typically in between a metal and a nonmetal.

Key Takeaways

Key clues Ionic bond are created through the exchange the valence electrons between atoms, commonly a metal and a nonmetal.The loss or gain of valence electrons enables ions to obey the octet rule and become much more stable.Ionic compounds are frequently neutral. Therefore, ions incorporate in methods that neutralize your charges.Key Termsvalence electrons: The electron of one atom that have the right to participate in the formation of chemical bonds with other atoms. They space the furthest electron from the nucleus.octet rule: one atom is many stable when there are eight electron in that valence shell.

Forming an Ion

Ionic bonds space a course of chemical bonds that result from the exchange that one or much more valence electrons from one atom, commonly a metal, to another, typically a nonmetal. This electron exchange outcomes in an electrostatic attraction between the 2 atoms dubbed an ionic bond. An atom that loses one or an ext valence electrons to end up being a positively charged ion is well-known as a cation, when an atom the gains electrons and becomes negatively charged is known as an anion.

This exchange the valence electrons permits ions to accomplish electron configurations that mimic those that the noble gases, to solve the octet rule. The octet dominance states the an atom is many stable as soon as there space eight electrons in that valence shell. Atom with less than eight electrons have tendency to fulfill the duet rule, having two electron in your valence shell. By to solve the duet rule or the octet rule, ions are more stable.

A cation is shown by a optimistic superscript fee (+ something) to the ideal of the atom. One anion is shown by a an adverse superscript charge (- something) to the right of the atom. For example, if a sodium atom loses one electron, the will have actually one more proton than electron, offering it an overall +1 charge. The chemistry symbol because that the salt ion is Na+1 or just Na+. Similarly, if a chlorine atom profit an extra electron, it becomes the chloride ion, Cl–. Both ions type because the ion is an ext stable than the atom as result of the octet rule.

Forming an Ionic Bond

Once the oppositely charged ion form, they room attracted by their positive and an adverse charges and type an ionic compound. Ionic binding are likewise formed as soon as there is a large electronegativity difference in between two atoms. This difference causes an unequal sharing of electron such that one atom totally loses one or much more electrons and the various other atom profit one or an ext electrons, such together in the development of an ionic bond in between a metal atom (sodium) and also a nonmetal (fluorine).

Formation of salt fluoride: The move of electrons and subsequent attraction of oppositely fee ions.

Determining the Formula of an Ionic Compound

To identify the chemistry formulas of ionic compounds, the following two conditions must it is in satisfied:

Each ion should obey the octet rule for maximum stability.Ions will combine in a means that the as whole ionic compound will certainly be neutral. In various other words, the dues of the ions need to balance out.

Magnesium and fluorine combine to type an ionic compound. What is the formula because that the compound?

Mg most typically forms a 2+ ion. This is since Mg has two valence electrons and it would favor to eliminate those 2 ions to follow the octet rule. Fluorine has seven valence electrons and usually creates the F – ion because it benefit one electron to meet the octet rule. Once Mg2+ and F – incorporate to kind an ionic compound, your charges need to cancel out. Therefore, one Mg2+ needs two F – ions to neutralize the charge. The 2+ that the Mg is balanced by having two -1 charged ions. Therefore, the formula that the compound is MgF2. The subscript two indicates that there space two fluorines that are ionically bonded to magnesium.

On the macroscopic scale, ionic compounds form crystalline lattice structures that are characterized by high melting and also boiling clues and great electrical conductivity as soon as melted or solubilized.


Magnesium and fluorine integrate to kind an ionic compound. What is the formula because that the compound?

Mg most commonly forms a 2+ ion. This is since Mg has actually two valence electrons and it would favor to remove those 2 ions to obey the octet rule. Fluorine has seven valence electrons and also as such, usually creates the F– ion because it profit one electron to meet the octet rule. When Mg2+ and F– integrate to type an ionic compound, your charges must cancel out. Therefore, one Mg2+ needs two F– ions to balance. The 2+ that the Mg is balanced by having actually two -1 charged ions. Therefore, the formula of the compound is MgF2. The subscript two shows that there are two fluorines that room ionically bonded to magnesium.

Key Takeaways

Key points Covalent bonds involve 2 atoms, generally nonmetals, that share electron thickness to type strong bonding interactions.Covalent bonds encompass single, double, and triple bonds and also are created of sigma and also pi bonding interactions whereby 2, 4, or 6 electrons are mutual respectively.Covalent compounds commonly have lower melting and boiling points 보다 ionic compounds.Key Termselectronegativity: The tendency of an atom or molecule to attract electrons and also thus type bonds.single bond: A kind of covalent link where just two electrons space shared between atoms.

Forming Covalent Bonds

Covalent bonds space a class of chemical bonds wherein valence electrons space shared in between two atoms, commonly two nonmetals. The formation of a covalent bond allows the nonmetals to follow the octet rule and also thus become much more stable. Because that example:

A fluorine atom has seven valence electrons. If it share one electron with a carbon atom (which has four valence electrons), the fluorine will have actually a full octet (its seven electrons add to the one that is sharing v carbon).Carbon will then have five valence electrons (its four and the one its sharing through fluorine). Covalently sharing 2 electrons is also known together a “single bond.” Carbon will have actually to kind four single bonds v four different fluorine atom to fill its octet. The result is CF4 or carbon tetrafluoride.

Covalent bonding needs a specific orientation in between atoms in bespeak to achieve the overlap in between bonding orbitals. Covalent bonding interactions encompass sigma-bonding (σ) and pi-bonding (π). Sigma bonds space the strongest form of covalent interaction and also are developed via the overlap of atom orbitals along the orbit axis. The overlapped orbitals permit the common electrons to relocate freely between atoms. Pi bonds space a weaker kind of covalent interactions and result from the overlap of two lobes of the connecting atomic orbitals above and listed below the orbital axis.

Covalent bonds have the right to be single, double, and also triple bonds.

Single bonds occur when two electrons are shared and are created of one sigma bond between the two atoms. Twin bonds occur when four electrons are shared in between the two atoms and consist the one sigma bond and one pi bond.Triple bonds take place when six electrons room shared in between the two atoms and consist of one sigma bond and also two pi bond (see later principle for much more info around pi and sigma bonds).

Ionic compounds v. Molecule Compounds

Unlike an ionic bond, a covalent bond is stronger in between two atoms with comparable electronegativity. For atoms with equal electronegativity, the bond between them will certainly be a non- polar covalent interaction. In non-polar covalent bonds, the electrons are equally shared in between the two atoms. For atoms with differing electronegativity, the bond will certainly be a polar covalent interaction, wherein the electrons will not be mutual equally.

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Ionic solids are generally defined by high melting and boiling points together with brittle, crystalline structures. Covalent compounds, top top the various other hand, have lower melting and boiling points. Unlike ionic compounds, lock are often not soluble in water and do not conduct electrical power when solubilized.