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Definition What constitute a chemical bond? Types of bond 1. Strong bond Covalent bond Glycosidic bond Peptide bond Disulfide bond 2. Weak bond Hydrogen bond Van der waals bond Hydrophobic bond Ionic bond Conclusion References
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Definition What constitute a chemical bond? Types of bond 1. Strong bond Covalent bond Glycosidic bond Peptide bond Disulfide bond 2. Weak bond Hydrogen bond Van der waals bond Hydrophobic bond Ionic bond Conclusion References
Types of bond by KK Sahu sir
Types of bond by KK Sahu sir
KAUSHAL SAHU
Covalent bond
Covalent bond
gavin40
Thanks for the ppt template, the popp.com
Bond Formation (Ionic, Covalent, and Metallic Bonding)
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The electrons which are involved in bond formation between atoms are found in the outermost shell (sometimes in the next to the outer-most shell) of the neutral atom; these are called VALENCE ELECTRONS. The atoms of elements which have only one or two electrons in their outermost shells (active shells) may lose electrons when they combine with atoms of other elements. An atom which has lost one or more valence electrons possesses a positive charge, and is called a POSITIVE ION. The sodium atom loses its one valence electron and acquires a +1 charge when it enters into chemical combination with an atom of an element such as chlorine. The magnesium atom may lose its two valence electrons and assume a +2 charge. Na Na+ + e- The Na symbol to the left of the arrow represents a stable sodium atom while the Na+ symbol to the right of the arrow represents an unstable sodium ion which has had a single electron removed. Mg Mg++ + 2e- The Mg symbol to the left of the arrow represents a stable magnesium atom while the Mg++ symbol to the right of the arrow represents an unstable magnesium ion which has had two electrons removed. The smaller the number of valence electrons in the atom, the greater the tendency of the element to lose electrons and thus form positive ions during chemical combination with atoms of other elements. The energy required to remove an electron from a neutral atom to form a positive ion is called the IONIZATION POTENTIAL of the atom. Some metals have small ionization potentials and readily form positive ions. The nonmetals, which have more electrons in their outer shells than the metals, have large ionization potentials and show little tendency toward the formation of positive ions. Atoms which lack one or two electrons of having an outermost shell of eight electrons readily gain sufficient electrons from certain other atoms, such as sodium and magnesium, to make a full compliment of eight electrons in the outside shell. Neutral atoms become NEGATIVE IONS by gaining electrons. The nonmetals, such as Fluorine (F), Chlorine (Cl), Bromine (Br), Iodine (I), Oxygen (O), Nitrogen (N) and Sulfur (S), readily form negative ions. Cl + e- Cl- Chlorine, when in its stable form, possesses seven valence electrons and therefore has the ability to gain one electron (as represented to the left of the arrow) giving it a negative charge of one when in its unstable ionic form (as represented to the right of the arrow above). S + 2e- S-2 Sulfur, when in its stable form, possesses six valence electrons and therefore has the ability to gain two electrons giving it a negative charge of two when in its unstable ionic form. The attraction of a neutral atom for electrons is known as its ELECTRON AFFINITY. The nonmetals have high electron affinities and the metals have very low electron affinities. Thus, mainly the nonmetals tend to form negative ions during chemical combination. When a positive ion and a negative ion are brought close together, strong electr.
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Chemical Bonds
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Formation of Compounds
and Molecules
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