What Is the Term for Bonding That Elements in the Oxygen Family Will Do as They Share Electrons?

Introduction to Bonding

Chemical bonding describes a diverseness of interactions that concord atoms together in chemical compounds.

Learning Objectives

List the types of chemical bonds and their full general backdrop

Key Takeaways

Key Points

• Chemical bonds are forces that agree atoms together to make compounds or molecules.
• Chemic bonds include covalent, polar covalent, and ionic bonds.
• Atoms with relatively similar electronegativities share electrons between them and are continued by covalent bonds.
• Atoms with large differences in electronegativity transfer electrons to form ions. The ions and so are attracted to each other. This attraction is known as an ionic bond.

Key Terms

• bail: A link or force between neighboring atoms in a molecule or compound.
• ionic bond: An allure between two ions used to create an ionic chemical compound. This attraction usually forms between a metal and a non-metal.
• covalent bond: An interaction between 2 atoms, which involves the sharing of 1 or more electrons to aid each atom satisfy the octet rule. This interaction typically forms between two non-metals.
• intramolecular: Refers to interactions within a molecule.
• intermolecular forces: Refers to interactions betwixt two or more molecules.

Chemical bonds

Chemical bonds are the connections between atoms in a molecule. These bonds include both stiff intramolecular interactions, such as covalent and ionic bonds. They are related to weaker intermolecular forces, such as dipole-dipole interactions, the London dispersion forces, and hydrogen bonding. The weaker forces will be discussed in a subsequently concept.

Chemic bonds: This pictures shows examples of chemical bonding using Lewis dot notation. Hydrogen and carbon are not bonded, while in water at that place is a single bond betwixt each hydrogen and oxygen. Bonds, especially covalent bonds, are often represented as lines between bonded atoms. Acetylene has a triple bail, a special type of covalent bond that will be discussed after.

Covalent Bonds

Chemical bonds are the forces of allure that tie atoms together. Bonds are formed when valence electrons, the electrons in the outermost electronic "trounce" of an atom, interact. The nature of the interaction betwixt the atoms depends on their relative electronegativity. Atoms with equal or similar electronegativity form covalent bonds, in which the valence electron density is shared between the two atoms. The electron density resides between the atoms and is attracted to both nuclei. This type of bond forms nigh ofttimes between 2 non- metals.

When at that place is a greater electronegativity difference than between covalently bonded atoms, the pair of atoms usually forms a polar covalent bond. The electrons are still shared betwixt the atoms, simply the electrons are not equally attracted to both elements. Every bit a result, the electrons tend to be found well-nigh i detail atom most of the fourth dimension. Again, polar covalent bonds tend to occur between non-metals.

Ionic Bonds

Finally, for atoms with the largest electronegativity differences (such every bit metals bonding with nonmetals), the bonding interaction is called ionic, and the valence electrons are typically represented as beingness transferred from the metal atom to the nonmetal. Once the electrons have been transferred to the non-metallic, both the metal and the not-metal are considered to be ions. The ii oppositely charged ions attract each other to form an ionic chemical compound.

Bonds, Stability, and Compounds

Covalent interactions are directional and depend on orbital overlap, while ionic interactions have no particular directionality. Each of these interactions allows the atoms involved to proceeds viii electrons in their valence shell, satisfying the octet rule and making the atoms more stable.

These atomic backdrop help describe the macroscopic properties of compounds. For instance, smaller covalent compounds that are held together past weaker bonds are frequently soft and malleable. On the other hand, longer-range covalent interactions tin can be quite strong, making their compounds very durable. Ionic compounds, though equanimous of potent bonding interactions, tend to class brittle crystalline lattices.

Ionic Bonds

Ionic bonds are a subset of chemical bonds that result from the transfer of valence electrons, typically betwixt a metal and a nonmetal.

Learning Objectives

Summarize the characteristic features of ionic bonds

Key Takeaways

Key Points

• Ionic bonds are formed through the substitution of valence electrons between atoms, typically a metallic and a nonmetal.
• The loss or proceeds of valence electrons allows ions to obey the octet rule and get more stable.
• Ionic compounds are typically neutral. Therefore, ions combine in ways that neutralize their charges.

Fundamental Terms

• valence electrons: The electrons of an atom that can participate in the formation of chemical bonds with other atoms. They are the furthest electrons from the nucleus.
• octet rule: An atom is most stable when there are eight electrons in its valence beat out.

Forming an Ion

Ionic bonds are a course of chemical bonds that upshot from the exchange of i or more valence electrons from one cantlet, typically a metal, to some other, typically a nonmetal. This electron exchange results in an electrostatic attraction between the 2 atoms called an ionic bond. An cantlet that loses ane or more valence electrons to get a positively charged ion is known every bit a cation, while an atom that gains electrons and becomes negatively charged is known as an anion.

This exchange of valence electrons allows ions to attain electron configurations that mimic those of the noble gases, satisfying the octet rule. The octet rule states that an atom is nearly stable when there are eight electrons in its valence beat. Atoms with less than eight electrons tend to satisfy the duet rule, having ii electrons in their valence shell. By satisfying the duet dominion or the octet rule, ions are more stable.

A cation is indicated by a positive superscript charge (+ something) to the right of the cantlet. An anion is indicated by a negative superscript charge (- something) to the correct of the atom. For instance, if a sodium atom loses ane electron, it will accept one more proton than electron, giving it an overall +1 charge. The chemic symbol for the sodium ion is Na⁺¹ or just Na⁺. Similarly, if a chlorine atom gains an actress electron, it becomes the chloride ion, Cl^–. Both ions form because the ion is more stable than the cantlet due to the octet rule.

Forming an Ionic Bond

Once the oppositely charged ions form, they are attracted by their positive and negative charges and form an ionic chemical compound. Ionic bonds are likewise formed when at that place is a large electronegativity difference between ii atoms. This deviation causes an unequal sharing of electrons such that 1 cantlet completely loses one or more than electrons and the other atom gains one or more electrons, such as in the creation of an ionic bond between a metallic cantlet (sodium) and a nonmetal (fluorine).

Germination of sodium fluoride: The transfer of electrons and subsequent attraction of oppositely charged ions.

Determining the Formula of an Ionic Chemical compound

To determine the chemical formulas of ionic compounds, the following two conditions must be satisfied:

1. Each ion must obey the octet dominion for maximum stability.
2. Ions volition combine in a mode that the overall ionic compound will be neutral. In other words, the charges of the ions must balance out.

Magnesium and fluorine combine to form an ionic chemical compound. What is the formula for the compound?

Mg most commonly forms a ii+ ion. This is because Mg has two valence electrons and it would like to get rid of those two ions to obey the octet dominion. Fluorine has seven valence electrons and usually forms the F ^– ion because it gains ane electron to satisfy the octet dominion. When Mg²⁺ and F ^– combine to form an ionic chemical compound, their charges must cancel out. Therefore, one Mg²⁺ needs two F ^– ions to neutralize the charge. The two+ of the Mg is balanced by having two -i charged ions. Therefore, the formula of the compound is MgF₂. The subscript two indicates that at that place are two fluorines that are ionically bonded to magnesium.

On the macroscopic scale, ionic compounds form crystalline lattice structures that are characterized by loftier melting and humid points and adept electrical conductivity when melted or solubilized.

Instance

Magnesium and fluorine combine to grade an ionic chemical compound. What is the formula for the compound?

Mg most commonly forms a two+ ion. This is because Mg has two valence electrons and it would like to get rid of those ii ions to obey the octet dominion. Fluorine has seven valence electrons and equally such, usually forms the F^– ion considering it gains i electron to satisfy the octet rule. When Mg²⁺ and F^– combine to form an ionic compound, their charges must cancel out. Therefore, one Mg²⁺ needs two F^– ions to residual. The 2+ of the Mg is balanced past having two -1 charged ions. Therefore, the formula of the compound is MgF_ii. The subscript two indicates that in that location are ii fluorines that are ionically bonded to magnesium.

Covalent Bonds

Covalent bonding involves ii atoms, typically nonmetals, sharing valence electrons.

Learning Objectives

Differentiate between covalent and ionic bonds

Key Takeaways

Key Points

• Covalent bonds involve two atoms, typically nonmetals, that share electron density to course strong bonding interactions.
• Covalent bonds include unmarried, double, and triple bonds and are equanimous of sigma and pi bonding interactions where two, 4, or six electrons are shared respectively.
• Covalent compounds typically have lower melting and boiling points than ionic compounds.

Central Terms

• electronegativity: The trend of an cantlet or molecule to concenter electrons and thus form bonds.
• unmarried bond: A type of covalent bail where only two electrons are shared between atoms.

Forming Covalent Bonds

Covalent bonds are a form of chemic bonds where valence electrons are shared betwixt two atoms, typically 2 nonmetals. The formation of a covalent bail allows the nonmetals to obey the octet rule and thus become more stable. For example:

• A fluorine cantlet has seven valence electrons. If it shares 1 electron with a carbon atom (which has four valence electrons), the fluorine will have a total octet (its 7 electrons plus the one it is sharing with carbon).
• Carbon will then have 5 valence electrons (its four and the ane its sharing with fluorine). Covalently sharing two electrons is as well known every bit a "single bond." Carbon volition accept to form four single bonds with four unlike fluorine atoms to make full its octet. The result is CF₄ or carbon tetrafluoride.

Covalent bonding requires a specific orientation betwixt atoms in lodge to achieve the overlap between bonding orbitals. Covalent bonding interactions include sigma-bonding (σ) and pi-bonding (π). Sigma bonds are the strongest type of covalent interaction and are formed via the overlap of diminutive orbitals along the orbital axis. The overlapped orbitals allow the shared electrons to movement freely between atoms. Pi bonds are a weaker blazon of covalent interactions and result from the overlap of ii lobes of the interacting atomic orbitals in a higher place and below the orbital centrality.

Covalent bonds can exist single, double, and triple bonds.

• Single bonds occur when two electrons are shared and are composed of ane sigma bond between the two atoms.
• Double bonds occur when four electrons are shared betwixt the two atoms and consist of one sigma bond and one pi bond.
• Triple bonds occur when six electrons are shared between the two atoms and consist of 1 sigma bail and two pi bonds (come across later concept for more info about pi and sigma bonds).

Ionic Compounds v. Molecular Compounds

Unlike an ionic bail, a covalent bond is stronger betwixt 2 atoms with similar electronegativity. For atoms with equal electronegativity, the bond between them will be a non- polar covalent interaction. In non-polar covalent bonds, the electrons are equally shared between the ii atoms. For atoms with differing electronegativity, the bond will be a polar covalent interaction, where the electrons will not be shared equally.

Ionic solids are by and large characterized by high melting and boiling points forth with brittle, crystalline structures. Covalent compounds, on the other hand, accept lower melting and boiling points. Unlike ionic compounds, they are often not soluble in h2o and do not conduct electricity when solubilized.

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Source: https://courses.lumenlearning.com/boundless-chemistry/chapter/types-of-chemical-bonds/

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