Ionic bonds are characterized by the complete transfer of electrons
from one atom to another, resulting in the formation of two charged
particles known as ions, which are held together with the help of
electrostatic force. Learn more about this intriguing occurrence in
chemistry where atoms of different elements combine to form a new
substance.
Read more at : http://www.sumichem.blogspot.com
Read more at : http://www.sumichem.blogspot.com
Chemistry is fascinating and it is present everywhere around us -
be it the beautiful raindrops on your 
windowpane, sweet sugars in the
fruits or the salt that makes your food tastier. Talking about salt,
have you ever wondered how sodium and chlorine combine to form the salt
(sodium chloride)? Well, it is due a process of bond formation known as
ionic bonding.
Basic Concepts in Chemical Bonding
All the chemical compounds are formed due to various combinations of constituent elements. Atoms of the same element or different elements are combined by various chemical bonds in order to keep the molecules together and thus, confer stability to the resulting compounds. Chemical bonds are of various types and possess varied strengths.
1. Valence Electrons and Electronegativity
All the elements possess a certain charge, which is expressed in the number of electrons they carry in the outermost shell or valence shell of their orbit. These electrons are termed as valence electrons and they play a key role in bond formation. The electronegativity of every element depends on the number of valence electrons it carries. Owing to the fact that different elements have different number of valence electrons, they can exhibit different number of valence states.
2. Why are Chemical Bonds Formed?
The purpose behind the formation of chemical bonds of any kind is given by the octet rule, which states that it is the natural tendency of the atoms of elements with lower atomic numbers (less than 20) to attain octet configuration, which is nothing but 8 electrons in the outermost shell. Thus, these atoms are very eager to combine with other elements to attain the configuration of the nearest noble gas. Why? Well, it's simply because noble gas configuration is the most stable.
3. Types of Chemical Bonds
These elements form a bond by donating, accepting or sharing electrons. This is the basic of chemical bonding. The most common types of chemical bonds include:
Covalent bond
Ionic bond
Metallic Bond
While the sharing of electrons by atoms forms covalent bonds, the transfer or electrons from one atom to another form ionic bonds. Here we will discuss in detail the various aspects of ionic bonding.
Understanding the Concept of Ionic Bonding
Ionic bonding is nothing but a type of chemical bond formation that involves complete transfer of electrons from one atom to another. When the atoms lose or gain electrons, they become differentially charged ions or oppositely charged ions. The charged ions are then attracted towards each other due to the electrostatic force, which brings the oppositely charged ions together, resulting in the formation of an ionic bond.
Example
The most common example of ionic bonding is the formation of sodium chloride in which an atom of sodium combines with a chlorine atom.
Let us have a look at the electronic configurations of each.
Sodium (Na) : 2,8,1 and Chlorine (Cl) : 2, 8, 7.
Thus, we see that an atom of chlorine requires only one electron to attain the configuration of the nearest noble gas i.e. Argon (2,8,8). An atom of sodium, on the other hand, requires to get rid of the single electron in its outermost shell to acquire the configuration of the nearest noble gas i.e. Neon (2,8).
In such a scenario, the sodium atom donates its outermost electron to the chlorine atom, which requires only one electron to attain octet configuration. The sodium ion becomes positively charged due to the loss of an electron, whereas the chloride ion becomes negatively charged due to the gain of an additional electron. The oppositely charged ions thus formed, are attracted to each other and result in the formation of an ionic bond.
Characteristics of Ionic Bonds
The presence of ionic bonds affect the chemical and physical properties of the resulting compounds. There exist several prominent characteristics of ionic bonds and here is a list of some of these characteristics:
Owing to the fact that metals tend to lose electrons and non-metals tend to gain electrons, ionic bonding is common between metals and non-metals. Hence, unlike covalent bonds that can only be formed between non-metals, ionic bonds can be formed between metals and non-metals.
While naming the ionic compounds, the name of the metal always comes first and the name of the non-metal comes second. For instance, in case of sodium chloride (NaCl), sodium is the metal whereas chlorine is the non-metal.
Compounds that contain ionic bonds readily dissolve in water as well as several other polar solvents. Ionic bonds, thus, have an effect on the solubility of the resultant compounds.
When ionic compounds are dissolved in a solvent to form a homogeneous solution, the solutions tends to conduct electricity.
Ionic bonding has an effect on the melting point of the compounds as well, as ionic compounds tend to have higher melting points, which means that ionic bonds remain stable for a greater temperature range
windowpane, sweet sugars in the
fruits or the salt that makes your food tastier. Talking about salt,
have you ever wondered how sodium and chlorine combine to form the salt
(sodium chloride)? Well, it is due a process of bond formation known as
ionic bonding.Basic Concepts in Chemical Bonding
All the chemical compounds are formed due to various combinations of constituent elements. Atoms of the same element or different elements are combined by various chemical bonds in order to keep the molecules together and thus, confer stability to the resulting compounds. Chemical bonds are of various types and possess varied strengths.
1. Valence Electrons and Electronegativity
All the elements possess a certain charge, which is expressed in the number of electrons they carry in the outermost shell or valence shell of their orbit. These electrons are termed as valence electrons and they play a key role in bond formation. The electronegativity of every element depends on the number of valence electrons it carries. Owing to the fact that different elements have different number of valence electrons, they can exhibit different number of valence states.
2. Why are Chemical Bonds Formed?
The purpose behind the formation of chemical bonds of any kind is given by the octet rule, which states that it is the natural tendency of the atoms of elements with lower atomic numbers (less than 20) to attain octet configuration, which is nothing but 8 electrons in the outermost shell. Thus, these atoms are very eager to combine with other elements to attain the configuration of the nearest noble gas. Why? Well, it's simply because noble gas configuration is the most stable.
3. Types of Chemical Bonds
These elements form a bond by donating, accepting or sharing electrons. This is the basic of chemical bonding. The most common types of chemical bonds include:
Covalent bond
Ionic bond
Metallic Bond
While the sharing of electrons by atoms forms covalent bonds, the transfer or electrons from one atom to another form ionic bonds. Here we will discuss in detail the various aspects of ionic bonding.
Understanding the Concept of Ionic Bonding
Ionic bonding is nothing but a type of chemical bond formation that involves complete transfer of electrons from one atom to another. When the atoms lose or gain electrons, they become differentially charged ions or oppositely charged ions. The charged ions are then attracted towards each other due to the electrostatic force, which brings the oppositely charged ions together, resulting in the formation of an ionic bond.
Example
The most common example of ionic bonding is the formation of sodium chloride in which an atom of sodium combines with a chlorine atom.
Let us have a look at the electronic configurations of each.
Sodium (Na) : 2,8,1 and Chlorine (Cl) : 2, 8, 7.
Thus, we see that an atom of chlorine requires only one electron to attain the configuration of the nearest noble gas i.e. Argon (2,8,8). An atom of sodium, on the other hand, requires to get rid of the single electron in its outermost shell to acquire the configuration of the nearest noble gas i.e. Neon (2,8).
In such a scenario, the sodium atom donates its outermost electron to the chlorine atom, which requires only one electron to attain octet configuration. The sodium ion becomes positively charged due to the loss of an electron, whereas the chloride ion becomes negatively charged due to the gain of an additional electron. The oppositely charged ions thus formed, are attracted to each other and result in the formation of an ionic bond.
Characteristics of Ionic Bonds
The presence of ionic bonds affect the chemical and physical properties of the resulting compounds. There exist several prominent characteristics of ionic bonds and here is a list of some of these characteristics:
Owing to the fact that metals tend to lose electrons and non-metals tend to gain electrons, ionic bonding is common between metals and non-metals. Hence, unlike covalent bonds that can only be formed between non-metals, ionic bonds can be formed between metals and non-metals.
While naming the ionic compounds, the name of the metal always comes first and the name of the non-metal comes second. For instance, in case of sodium chloride (NaCl), sodium is the metal whereas chlorine is the non-metal.
Compounds that contain ionic bonds readily dissolve in water as well as several other polar solvents. Ionic bonds, thus, have an effect on the solubility of the resultant compounds.
When ionic compounds are dissolved in a solvent to form a homogeneous solution, the solutions tends to conduct electricity.
Ionic bonding has an effect on the melting point of the compounds as well, as ionic compounds tend to have higher melting points, which means that ionic bonds remain stable for a greater temperature range
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