Comparison in between Covalent and also Ionic Compounds

Covalent and also ionic compounds have distinct physical properties.

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Key Takeaways

Key PointsIonic compounds are developed from solid electrostatic interactions in between ions, which result in greater melting points and electrical conductivity compared to covalent compounds.Covalent compounds have bonds where electrons are shared in between atoms. Due to the share of electrons, they exhibit characteristic physics properties that include lower melting points and electrical conductivity compared to ionic compounds.Key Termsvalence electrons: electron in the outermost principal energy (valence) level of one atom that deserve to participate in the formation of chemical bonds with various other atoms.octet rule: atoms lose, gain, or share electron in stimulate to have actually a complete valence level of eight electrons. Hydrogen and also helium are exceptions since they can hold a best of two valence electrons.electronegativity: The tendency of one atom or molecule to lure electrons and form bonds.

Two great of Compounds

Compounds are identified as building materials containing 2 or an ext different chemical elements. Lock have unique chemical structures characterized by a fixed proportion of atoms held together by chemical bonds. Here, we comment on two great of compounds based on the bond kind that holds the atoms together: ionic and also covalent.

Covalent Compounds

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

Examples that compounds that contain just covalent bonds room methane (CH4), carbon monoxide (CO), and iodine monobromide (IBr).


Covalent bonding between hydrogen atoms: because each hydrogen atom has one electron, they room able to fill their outermost shells by sharing a pair of electrons with a covalent bond.

Ionic Compounds

Ionic bonding occurs as soon as there is a large difference in electronegativity in between two atoms. This large difference leads to the lose of one electron indigenous the much less electronegative atom and also the obtain of that electron by the much more electronegative atom, causing two ions. This oppositely charged ions feel an attraction to every other, and this electrostatic attraction constitutes an ionic bond.

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

Some examples of compounds through ionic bonding encompass NaCl, KI, MgCl2.

Formation of sodium fluoride (NaF): The transport of an electron from a neutral sodium atom to a neutral fluorine atom creates 2 oppositely fee ions: Na+ and F–. Attraction the the oppositely charged ions is the ionic bond between Na and also F.

Effect on physical Properties

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

At room temperature and also normal atmospheric pressure, covalent compounds might exist together a solid, a liquid, or a gas, conversely, ionic link exist only as solids.Although heavy ionic compounds do not command electricity since there are no free mobile ion or electrons, ionic compounds liquified in water do an electrically conductive solution. In contrast, covalent compounds do not exhibit any type of electrical conductivity, either in pure type or when liquified in water.Ionic compound exist in secure crystalline structures. Therefore, they have higher melting and boiling points compared to covalent compounds.

Single Covalent Bonds

Single covalent bonds space sigma bonds, which take place when one pair of electron is shared in between atoms.

Learning Objectives

Identify the 4 orbital types used in covalent link formation

Key Takeaways

Key points Covalent bonds occur when electrons are shared in between two atoms. A single covalent link is when only one pair of electrons is shared between atoms.A sigma bond is the strongest kind of covalent bond, in i beg your pardon the atom orbitals directly overlap in between the nuclei of two atoms.Sigma bond can happen between any kind of atom orbitals; the only necessity is the the atomic orbital overlap wake up directly in between the nuclei that atoms.Key Termssigma bond: A covalent bond who electron density is concentrated in the region directly between the nuclei.covalent bond: A form of chemistry bond where 2 atoms are associated to each various other by the sharing of 2 or more electrons.atomic orbital: A an ar in room around the atom’s nucleus wherein there is a probability of recognize an electron.

Hierarchical framework of the Atom

There are 4 hierarchical level that describe the position and also energy the the electrons an atom has. Below they are listed along with several of the feasible values (or letters) they have the right to have:

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

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

Atomic Orbitals

An atomic orbital is characterized as the probability of finding an electron in an area approximately an atom’s nucleus. Generally, orbital forms are attracted to explain the region in an are in which electron are most likely to be found. This is referred to as “electron density.”

Atomic orbitals: The shapes of the very first five atom orbitals are presented in order: 1s, 2s, and the 3 2p orbitals. Both blue and also orange-shaded regions represent areas in room where electrons can be uncovered ‘belonging’ to this orbitals.

Sigma Bonds

Covalent bonding occurs when two atom orbitals come with each other in close proximity and also their electron densities overlap. The strongest form of covalent bonds room sigma bonds, i m sorry are developed by the straight overlap the orbitals from every of the two bonded atoms. Nevertheless of the atomic orbital type, sigma bonds can happen as lengthy as the orbitals straight overlap between the nuclei that the atoms.

Orbital overlaps and also sigma bonds: These room all feasible overlaps in between different types of atom orbitals that result in the development of a sigma bond between two atoms. An alert that the area the overlap always occurs between the nuclei of the 2 bonded atoms.

Single covalent bonds take place when one pair of electrons is shared in between atoms as component of a molecule or compound. A single covalent bond have the right to be stood for by a solitary line in between the two atoms. For instance, the diatomic hydrogen molecule, H2, deserve to be created as H—H to suggest the solitary covalent bond in between the 2 hydrogen atoms.


Sigma bond in the hydrogen molecule: higher intensity the the red color indicates a better probability of the bonding electrons gift localized between the nuclei.

Double and also Triple Covalent Bonds

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

Learning Objectives

Describe the varieties of orbital overlap that happen in single, double, and also triple bonds

Key Takeaways

Key PointsDouble and triple covalent bonds room stronger than solitary covalent bonds and they are characterized by the sharing of 4 or 6 electrons between atoms, respectively.Double and also triple bonds are comprised of sigma bonds between hybridized orbitals, and also pi bonds in between unhybridized ns orbitals. Twin and triple bond offer added stability to compounds, and restrict any type of rotation around the shortcut axis. Bond lengths in between atoms with multiple bonds are shorter than in those with single bonds.Key Termsbond strength: directly related come the amount of energy required to rest the bond between two atoms. The much more energy required, the stronger the link is claimed to length: The distance between the nuclei of two bonded atoms. It deserve to be experimentally determined.orbital hybridization: The concept of mixing atomic orbitals to kind new hybrid orbitals suitable for the qualitative description of atom bonding properties and also geometries.atomic orbitals: The physical an ar in space around the nucleus whereby an electron has a probability of being.

Double and also Triple Covalent Bonds

Covalent bonding occurs when electrons room shared between atoms. Double and triple covalent bonds happen when 4 or six electrons room shared in between two atoms, and also they are suggested in Lewis structures by drawing two or 3 lines connecting one atom to another. It is important to note that only atoms with the require to get or lose at the very least two valence electrons through sharing have the right to participate in multiple bonds.

Bonding Concepts


Double and also triple bonds deserve to be described by orbital hybridization, or the ‘mixing’ of atomic orbitals to form new hybrid orbitals. Hybridization defines the bonding situation from a specific atom’s suggest of view. A mix of s and p orbitals outcomes in the development of hybrid orbitals. The newly developed hybrid orbitals all have the very same energy and also have a particular geometrical arrangement in room that agrees with the observed bonding geometry in molecules. Hybrid orbitals room denoted as spx, wherein s and p represent the orbitals provided for the mix process, and the value of the superscript x ranges from 1-3, depending upon how numerous p orbitals are compelled to describe the observed bonding.


Hybridized orbitals: A schematic the the result orientation in an are of sp3 hybrid orbitals. An alert that the sum of the superscripts (1 because that s, and also 3 for p) offers the total variety of formed hybrid orbitals. In this case, 4 orbitals are developed which suggest along the direction that the vertices that a tetrahedron.

Pi Bonds

Pi, or pi, bonds occur when over there is overlap between unhybridized ns orbitals of two nearby atoms. The overlap does no occur between the nuclei of the atoms, and this is the an essential difference between sigma and also pi bonds. Because that the link to kind efficiently, there has to be a suitable geometrical relationship in between the unhybridized p orbitals: they have to be top top the same plane.

Pi link formation: Overlap between surrounding unhybridized p orbitals to produce a pi bond. The electron density corresponding to the shared electrons is not focused along the internuclear axis (i.e., between the two atoms), uneven in sigma bonds.

Multiple bonds in between atoms constantly consist of a sigma bond, v any extr bonds being of the π type.

Examples of Pi Bonds

The simplest example of an essential compound v a double bond is ethylene, or ethene, C2H4. The double bond in between the 2 carbon atoms is composed of a sigma bond and also a π bond.

Ethylene bonding: an instance of a simple molecule v a double bond in between carbon atoms. The bond lengths and also angles (indicative the the molecule geometry) are indicated.

From the view of the carbon atoms, each has three sp2 hybrid orbitals and one unhybridized p orbital. The 3 sp2 orbitals lied in a single plane at 120-degree angles. Together the carbon atoms approach each other, your orbitals overlap and kind a bond. Simultaneously, the p orbitals approach each various other and kind a bond. To preserve this bond, the p orbitals should stay parallel to every other; therefore, rotation is no possible.

A triple bond involves the sharing of six electrons, v a sigma bond and two pi bonds. The most basic triple-bonded organic link is acetylene, C2H2. Triple bonds space stronger than twin bonds due to the the presence of two pi bonds quite than one. Each carbon has actually two sp hybrid orbitals, and one of them overlaps v its equivalent one native the other carbon atom to kind an sp-sp sigma bond. The remaining 4 unhybridized p orbitals overlap with each various other and type two pi bonds. Similar to double bonds, no rotation approximately the triple shortcut axis is possible.

Observable consequences of many Bonds

Bond Strength

Covalent bonds deserve to be share in terms of the amount of power that is compelled to break them. Based on the experimental observation that much more energy is required to break a bond in between two oxygen atoms in O2 than two hydrogen atom in H2, us infer the the oxygen atoms are much more tightly tied together. We say the the bond in between the two oxygen atom is stronger 보다 the bond in between two hydrogen atoms.

Experiments have presented that dual bonds are stronger than single bonds, and triple bonds are stronger than twin bonds. Therefore, it would certainly take an ext energy to break the triple shortcut in N2 contrasted to the twin bond in O2. Indeed, that takes 497 kcal/mol to break the O2 molecule, while the takes 945 kJ/mol to perform the exact same to the N2 molecule.

Bond Length

Another an effect of the presence of multiple bonds between atoms is the difference in the distance between the nuclei the the bonded atoms. Dual bonds have shorter distances than single bonds, and triple bonds room shorter than dual bonds.

Physical properties of Covalent Molecules

The covalent bonding design helps predict many of the physical properties that compounds.

Learning Objectives

Discuss the qualitative predictions of covalent bond theory on the boiling and also melting points, link length and strength, and conductivity the molecules

Key Takeaways

Key PointsThe Lewis theory of covalent bonding claims that the bond strength of dual bonds is twice that of solitary bonds, which is not true.General physics properties that have the right to be described by the covalent bonding model encompass boiling and also melting points, electric conductivity, bond strength, and bond length.Key Termsbond length: The distance in between the nuclei of two bonded atoms. It can be experimentally determined.intermolecular forces: Attractive forces or interactions in between different molecules in a sample that a substance. The strength of these interactions is vital factor the determines the substance’s physical strength: straight related to the lot of energy required to rest the bond in between two atoms. The much more energy required, the stronger the bond is claimed to be.octet rule: atoms lose, gain, or share electrons in stimulate to have actually a complete valence shell of eight electrons. Hydrogen is an exception because it can hold a preferably of two electrons in that is valence level.

First described by Gilbert Lewis, a covalent bond occurs as soon as electrons of different atoms are shared between the two atoms. These instances of electron sharing deserve to be guess by the octet rule. The octet preeminence is a chemical rule that generalizes the atoms of short atomic number (2, and also the halogens (F2, Cl2, Br2, I2). A H atom requirements one added electron to fill its valence level, and also the halogens require one much more electron to to fill the octet in their valence levels. Lewis bonding theory claims that this atoms will certainly share their valence electrons, effectively permitting each atom to create its own octet.

Several physics properties that molecules/compounds are concerned the presence of covalent bonds:

Covalent bonds in between atoms are quite strong, but attractions in between molecules/compounds, or intermolecular forces, deserve to be fairly weak. Covalent compounds normally have low boiling and melting points, and are discovered in all 3 physical states at room temperature.Covalent compounds do not command electricity; this is due to the fact that covalent compounds perform not have charged particles capable of delivering electrons.Lewis theory also accounts for bond length; the more powerful the bond and 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 theory predicts that with more shared electrons, the bond between the two atoms must be stronger. Follow to the theory, triple bonds are stronger than twin bonds, and twin bonds are stronger than single bonds. This is true. However, the theory indicates that the bond toughness of double bonds is double that of solitary bonds, i beg your pardon is no true. Therefore, while the covalent bonding version accounts for numerous physical observations, it does have actually its limitations.