Comparison between Covalent and Ionic Compounds

Covalent and also ionic compounds have distinctive physical properties.

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Key Takeaways

Key PointsIonic compound are created from solid electrostatic interactions between ions, which result in higher melting points and also electrical conductivity contrasted to covalent compounds.Covalent compounds have bonds wherein electrons room shared between atoms. Because of the share of electrons, they exhibit characteristic physics properties that incorporate lower melt points and electrical conductivity compared to ionic compounds.Key Termsvalence electrons: electron in the outermost principal energy (valence) level of one atom that can participate in the formation of chemical bonds with various other atoms.octet rule: atom lose, gain, or share electrons in order to have a complete valence level that eight electrons. Hydrogen and also helium are exceptions since they have the right to hold a best of two valence electrons.electronegativity: The tendency of one atom or molecule to attract electrons and type bonds.

Two classes of Compounds

Compounds are identified as building materials containing two or much more different chemical elements. Castle have distinct chemical structures characterized by a fixed ratio of atoms organized together by chemical bonds. Here, we comment on two classes of compounds based upon the bond type that hold the atoms together: ionic and covalent.

Covalent Compounds

Covalent binding are defined by the share of electrons in between two or much more atoms. This bonds greatly occur between nonmetals or between two the the same (or similar) elements.Two atom with similar electronegativity will certainly not exchange an electron from your outermost shell; the atoms instead share electrons so the their valence electron shell is filled.

Examples the compounds the contain just covalent bonds space methane (CH4), carbon monoxide (CO), and also iodine monobromide (IBr).


Covalent bonding between hydrogen atoms: since each hydrogen atom has one electron, they are able to fill their outermost shells by sharing a pair that electrons v a covalent bond.

Ionic Compounds

Ionic bonding occurs once there is a big difference in electronegativity between two atoms. This huge difference leader to the loss of one electron native the much less electronegative atom and also the gain of that electron by the much more electronegative atom, bring about two ions. These oppositely charged ion feel an attraction to every other, and this electrostatic attraction constitutes an ionic bond.

Ionic bonding occurs in between a nonmetal, i beg your pardon acts as an electron acceptor, and a metal, i m sorry acts as an electron donor. Steels have few valence electrons, vice versa, nonmetals have closer to eight valence electrons; to easily satisfy the octet rule, the nonmetal will accept one electron donated by the metal. More than one electron deserve to be donated and also received in an ionic bond.

Some instances of compounds v ionic bonding include NaCl, KI, MgCl2.

Formation of sodium fluoride (NaF): The move of an electron native a neutral salt atom come a neutral fluorine atom creates two oppositely charge ions: Na+ and F–. Attraction that the oppositely charged ion is the ionic bond between Na and also F.

Effect on physical Properties

Covalent and ionic compounds deserve to be identified easily because of their different physical properties based on the nature of your bonding. Here are some differences:

At room temperature and also normal atmospheric pressure, covalent compounds might exist together a solid, a liquid, or a gas, whereas ionic link exist only as solids.Although heavy ionic compounds perform not conduct electricity because there space no cost-free mobile ion or electrons, ionic compounds dissolved in water do an electrically conductive solution. In contrast, covalent compounds execute not exhibit any type of electrical conductivity, either in pure form or when liquified in water.Ionic link exist in secure crystalline structures. Therefore, lock have higher melting and also boiling points contrasted to covalent compounds.

Single Covalent Bonds

Single covalent bonds room sigma bonds, which occur when one pair of electron is shared between atoms.

Learning Objectives

Identify the four orbital species used in covalent bond formation

Key Takeaways

Key points Covalent bonds happen when electrons room shared between two atoms. A solitary covalent link is once only one pair of electron is shared in between atoms.A sigma shortcut is the strongest type of covalent bond, in i beg your pardon the atom orbitals straight overlap between the nuclei of 2 atoms.Sigma bonds can happen between any kind of atomic orbitals; the only necessity is that the atom orbital overlap wake up directly in between the nuclei the atoms.Key Termssigma bond: A covalent bond whose electron density is focused in the region directly in between the nuclei.covalent bond: A kind of chemical bond where 2 atoms are associated to each various other by the sharing of two or much more electrons.atomic orbital: A region in an are around the atom’s nucleus whereby there is a probability of detect an electron.

Hierarchical framework of the Atom

There are 4 hierarchical level that define the position and also energy the the electrons an atom has. Right here they are detailed along with few of the possible values (or letters) they deserve to have:

Principal energy levels (1, 2, 3, etc.)Sublevels (s, p, d, f)OrbitalsElectrons

Principal power levels space made the end of sublevels, i m sorry are subsequently made out of orbitals, in which electrons space found.

Atomic Orbitals

An atom orbital is characterized as the probability of detect an electron in an area roughly an atom’s nucleus. Generally, orbital shapes are attracted to describe the an ar in an are in which electron are likely to it is in found. This is referred to as “electron density.”

Atomic orbitals: The forms of the very first five atomic orbitals are displayed in order: 1s, 2s, and the 3 2p orbitals. Both blue and also orange-shaded areas represent regions in space where electrons deserve to be uncovered ‘belonging’ to these orbitals.

Sigma Bonds

Covalent bonding occurs when two atomic orbitals come with each other in near proximity and their electron densities overlap. The strongest form of covalent bonds space sigma bonds, i beg your pardon are developed by the direct overlap of orbitals from every of the 2 bonded atoms. Regardless of the atomic orbital type, sigma bond can occur as long as the orbitals directly overlap between the nuclei of the atoms.

Orbital overlaps and also sigma bonds: These room all possible overlaps between different varieties of atom orbitals that result in the formation of a sigma bond between two atoms. An alert that the area of overlap constantly occurs in between the nuclei that the two bonded atoms.

Single covalent bonds occur when one pair of electrons is shared between atoms as part of a molecule or compound. A solitary covalent bond deserve to be represented by a single line in between the two atoms. Because that instance, the diatomic hydrogen molecule, H2, can be written as H—H to show the single covalent bond between the two hydrogen atoms.


Sigma shortcut in the hydrogen molecule: greater intensity that the red color indicates a better probability that the bonding electrons gift localized in between the nuclei.

Double and also Triple Covalent Bonds

Double and triple bonds, consisted of of sigma and pi bonds, boost the stability and restrict the geometry that a compound.

Learning Objectives

Describe the varieties of orbit overlap that take place in single, double, and also triple bonds

Key Takeaways

Key PointsDouble and also triple covalent bonds room stronger than single covalent bonds and also they are identified by the sharing of 4 or 6 electrons in between atoms, respectively.Double and triple bond are made up of sigma bonds between hybridized orbitals, and pi bonds between unhybridized p orbitals. Twin and triple binding offer included stability come compounds, and also restrict any type of rotation about the link axis. Bond lengths between atoms v multiple bonds are shorter than in those with solitary bonds.Key Termsbond strength: straight related come the lot of energy required to break the bond between two atoms. The an ext energy required, the more powerful the shortcut is stated to length: The distance in between the nuclei of 2 bonded atoms. It can be experimentally determined.orbital hybridization: The concept of mixing atomic orbitals to kind new hybrid orbitals perfect for the qualitative summary of atom bonding properties and also geometries.atomic orbitals: The physical region in room around the nucleus whereby an electron has a probability the being.

Double and also Triple Covalent Bonds

Covalent bonding occurs once electrons are shared in between atoms. Double and triple covalent bonds take place when 4 or 6 electrons are shared in between two atoms, and also they are shown in Lewis structures by drawing two or three lines connecting one atom come another. That is essential to keep in mind that only atoms v the require to gain or lose at the very least two valence electrons with sharing have the right to participate in lot of bonds.

Bonding Concepts


Double and also triple bonds can be explained by orbit hybridization, or the ‘mixing’ of atom orbitals to kind new hybrid orbitals. Hybridization explains the bonding case from a specific atom’s point of view. A combination of s and p orbitals outcomes in the formation of hybrid orbitals. The newly developed hybrid orbitals all have actually the exact same energy and have a specific geometrical arrangement in room that agrees v the it was observed bonding geometry in molecules. Hybrid orbitals room denoted as spx, where s and p represent the orbitals offered for the mix process, and the value of the superscript x varieties from 1-3, relying on how many p orbitals are required to describe the it was observed bonding.


Hybridized orbitals: A schematic that the result orientation in an are of sp3 hybrid orbitals. Notification that the amount of the superscripts (1 because that s, and also 3 because that p) offers the total variety of formed hybrid orbitals. In this case, four orbitals are created which suggest along the direction that the vertices of a tetrahedron.

Pi Bonds

Pi, or pi, bonds occur when there is overlap between unhybridized p orbitals the two surrounding atoms. The overlap does not occur in between the nuclei that the atoms, and also this is the crucial difference between sigma and pi bonds. Because that the bond to kind efficiently, there has to be a appropriate geometrical relationship in between the unhybridized p orbitals: they must be on the very same plane.

Pi shortcut formation: Overlap between nearby unhybridized p orbitals produces a pi bond. The electron density equivalent to the common electrons is not focused along the internuclear axis (i.e., in between the 2 atoms), uneven in sigma bonds.

Multiple bonds between atoms constantly consist the a sigma bond, with any extr bonds gift of the π type.

Examples that Pi Bonds

The simplest example of an necessary compound through a double bond is ethylene, or ethene, C2H4. The double bond in between the two carbon atoms is composed of a sigma bond and also a π bond.

Ethylene bonding: an example of a simple molecule v a twin bond between carbon atoms. The shortcut lengths and angles (indicative of the molecular geometry) are indicated.

From the perspective of the carbon atoms, each has actually three sp2 hybrid orbitals and one unhybridized p orbital. The 3 sp2 orbitals lie in a single plane in ~ 120-degree angles. As the carbon atoms technique each other, your orbitals overlap and form a bond. Simultaneously, the p orbitals approach each various other and form a bond. To preserve this bond, the p orbitals have to stay parallel to every other; therefore, rotation is no possible.

A triple bond requires the share of 6 electrons, through a sigma bond and also two pi bonds. The most basic triple-bonded organic compound is acetylene, C2H2. Triple bonds are stronger than dual bonds as result of the the visibility of 2 pi bonds quite than one. Each carbon has actually two sp hybrid orbitals, and one of lock overlaps with its corresponding one from the other carbon atom to kind an sp-sp sigma bond. The remaining four unhybridized p orbitals overlap v each various other and type two pi bonds. Comparable to dual bonds, no rotation approximately the triple link axis is possible.

Observable after-effects of lot of Bonds

Bond Strength

Covalent bonds deserve to be divide in terms of the quantity of power that is compelled to rest them. Based upon the experimental observation that more energy is necessary to break a bond in between two oxygen atoms in O2 than 2 hydrogen atom in H2, we infer the the oxygen atom are more tightly bound together. We say that the bond in between the 2 oxygen atom is stronger 보다 the bond in between two hydrogen atoms.

Experiments have displayed that dual bonds space stronger than single bonds, and also triple bonds space stronger than double bonds. Therefore, it would take more energy to rest the triple bond in N2 contrasted to the dual bond in O2. Indeed, it takes 497 kcal/mol to break the O2 molecule, while the takes 945 kJ/mol to do the very same to the N2 molecule.

Bond Length

Another an effect of the visibility of multiple bonds between atoms is the difference in the distance between the nuclei of the external inspection atoms. Dual bonds have actually shorter distances than solitary bonds, and also triple bonds room shorter than dual bonds.

Physical nature of Covalent Molecules

The covalent bonding model helps predict countless of the physics properties the compounds.

Learning Objectives

Discuss the qualitative guess of covalent bond concept on the boiling and also melting points, bond length and strength, and also conductivity that molecules

Key Takeaways

Key PointsThe Lewis concept of covalent bonding states that the bond strength of double bonds is twice that of solitary bonds, i m sorry is no true.General physics properties that deserve to be defined by the covalent bonding model encompass boiling and also melting points, electric conductivity, link strength, and also bond length.Key Termsbond length: The distance in between the nuclei of 2 bonded atoms. It can be experimentally determined.intermolecular forces: Attractive forces or interactions in between different molecule in a sample of a substance. The toughness of this interactions is critical factor that determines the substance’s physics strength: straight related to the lot of energy required to break the bond between two atoms. The much more energy required, the stronger the shortcut is stated to be.octet rule: atoms lose, gain, or share electron in order to have a complete valence covering of eight electrons. Hydrogen is an exception due to the fact that it deserve to hold a maximum of 2 electrons in its valence level.

First explained by Gilbert Lewis, a covalent link occurs once electrons of different atoms are shared in between the 2 atoms. These situations of electron sharing deserve to be predicted by the octet rule. The octet preeminence is a chemical preeminence that generalizes the atoms of low atomic number (2, and also the halogens (F2, Cl2, Br2, I2). A H atom needs one added electron to to fill its valence level, and also the halogens need one more electron to to fill the octet in their valence levels. Lewis bonding theory says that these atoms will certainly share your valence electrons, effectively enabling each atom to develop its very own octet.

Several physical properties of molecules/compounds are pertained to the visibility of covalent bonds:

Covalent bonds in between atoms are rather strong, but attractions between molecules/compounds, or intermolecular forces, can be fairly weak. Covalent compounds typically have low boiling and melting points, and are found in all three physical claims at room temperature.Covalent compounds do not command electricity; this is because covalent compounds perform not have actually charged particles capable of delivering electrons.Lewis theory likewise accounts because that bond length; the stronger the bond and also the much more electrons shared, the shorter the bond size is.

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However, the Lewis theory of covalent bonding does no account for some observations of compound in nature. The concept predicts the with an ext shared electrons, the bond in between the 2 atoms must be stronger. Follow to the theory, triple bonds room stronger than twin bonds, and dual bonds room stronger than solitary bonds. This is true. However, the theory indicates that the bond stamin of dual bonds is twice that of solitary bonds, which is not true. Therefore, when the covalent bonding version accounts for many physical observations, that does have actually its limitations.