What is the ionic compound formula of sodium sulfate? What is the ionic compound formula of ammonium sulfate? What is the ionic compound formula of magnesium nitrate? What is the ionic compound formula of sodium hydroxide? What is the ionic compound formula of sodium phosphate? How do ionic bonds differ from covalent? How do ionic bonds dissolve in water? See all questions in Ionic Bond Formation. Impact of this question views around the world. Na has one valence electron an electron in the outermost orbital shell that can take part in bonding while Cl has seven valence electrons.
As a result, the transfer of one electron from Na to Cl is favored because both atoms will achieve a more stable electron configuration full outer orbital shells of eight electrons. Due to the transfer of its electron, Na is considered a cation , with a net positive charge.
Meanwhile, Cl now has a net negative charge and is considered an anion. The electrostatic or Coulombic attraction between oppositely charged ions is what is called the ionic bond. Ionic bonds form between atoms that vastly differ in their electronegativity values. A difference of 1. Ionic bonds most frequently form between metals and non-metals. Covalent Bond. The covalent bond is formed when adjacent atoms share valence electrons. Generally, sharing electrons in such a fashion allows each atom involved to achieve a more stable electron configuration.
Consider two chlorine atoms each with 7 electrons in each respective outer shell. The atoms will share one of their outer electrons with the other, such that each individual atom effectively has a complete outer orbital.
Covalent bonds form between atoms that have similar electronegativity values. This type of bond is common to organic compounds, where the atoms composing the compounds are non-metals. Polar Covalent Bond. A polar covalent bond is bond that has a mix of ionic character and covalent character. It is important to understand that all ionic compounds compounds formed by ionic bonds have some measure of electron sharing covalent bonding even though an ionic bond is not considered to be a type of covalent bond.
A large difference in the electronegativity of two atoms indicates a greater ionic character and is considered a purely ionic bond; whereas a very small, negligible difference is considered a purely covalent bond. A polar covalent bond exists when the electronegativity difference is somewhere in between, generally more towards the covalent side small electronegativity difference.
When a polar covalent bond is formed, the result is an unequal sharing of electrons between atoms. An example of a molecule with a polar covalent bond is hydrogen fluoride. In this molecule, hydrogen has a partial positive charge while fluorine has a partial negative charge. Metallic Bond. Similar to the covalent bond, the metallic bond involves electron sharing.
However, in a metallic bond, valence electrons are delocalized meaning that the electrons are mobile and can therefore be associated with any of the plentiful adjacent atoms. In this sense, the electrons form an electron cloud around the atoms, which is the basis for classic metallic properties such as: high electrical conductivity, ductility and luster.
Secondary Bonds. Secondary bonds, as opposed to primary bonds, are bonds with much smaller bonding energies that do not involve the transfer or sharing of electrons. These bonds are caused by permanent or temporary dipoles within the atom or molecule. Ionic bonds require an electron donor, often a metal, and an electron acceptor, a nonmetal. Ionic bonding is observed because metals have few electrons in their outer-most orbitals.
By losing those electrons, these metals can achieve noble gas configuration and satisfy the octet rule. Similarly, nonmetals that have close to 8 electrons in their valence shells tend to readily accept electrons to achieve noble gas configuration. In ionic bonding, more than 1 electron can be donated or received to satisfy the octet rule.
The charges on the anion and cation correspond to the number of electrons donated or received. In ionic bonds, the net charge of the compound must be zero. This sodium molecule donates the lone electron in its valence orbital in order to achieve octet configuration. This creates a positively charged cation due to the loss of electron. This chlorine atom receives one electron to achieve its octet configuration, which creates a negatively charged anion.
The predicted overall energy of the ionic bonding process, which includes the ionization energy of the metal and electron affinity of the nonmetal, is usually positive, indicating that the reaction is endothermic and unfavorable.
However, this reaction is highly favorable because of the electrostatic attraction between the particles. At the ideal interatomic distance, attraction between these particles releases enough energy to facilitate the reaction.
Most ionic compounds tend to dissociate in polar solvents because they are often polar. This phenomenon is due to the opposite charges on each ion. In this example, the sodium atom is donating its 1 valence electron to the chlorine atom.
This creates a sodium cation and a chlorine anion. Notice that the net charge of the resulting compound is 0. In this example, the magnesium atom is donating both of its valence electrons to chlorine atoms. Each chlorine atom can only accept 1 electron before it can achieve its noble gas configuration; therefore, 2 atoms of chlorine are required to accept the 2 electrons donated by the magnesium.
Notice that the net charge of the compound is 0. Covalent bonding is the sharing of electrons between atoms. This type of bonding occurs between two atoms of the same element or of elements close to each other in the periodic table.
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