9. Distance of atoms from each other (only an example): MgO= 2 nm and the bond length/distance are 1nm; NaCI = 3 nm and the bond %3D length/distance is 1nm Considering the information above, choose the CORRECT descriptions of ionic bonding in MgO. 1-The closer atomsof MgO creates stronger attraction than of the NaCl Il-The closer atoms of MgO creates repulsion of the atomic nuclei III- The higher charge difference of MgO creates stronger bond than of NaCI IV - The higher charge difference of MgO creates stronger repulsion V- The more lent and borrowed electrons between atoms of MgO attributed to stronger attraction VI - The more lent and borrowed electrons between atoms of MgO attributed to stronger repulsion VII - the atom size of MgO is relatively smaller than of NaCl, resulting to stronger bond O II, III, VI, and VII O II, IV, and V O. II, V, and VII OI, II, and V only
Types of Chemical Bonds
The attractive force which has the ability of holding various constituent elements like atoms, ions, molecules, etc. together in different chemical species is termed as a chemical bond. Chemical compounds are dependent on the strength of chemical bonds between its constituents. Stronger the chemical bond, more will be the stability in the chemical compounds. Hence, it can be said that bonding defines the stability of chemical compounds.
Polarizability In Organic Chemistry
Polarizability refers to the ability of an atom/molecule to distort the electron cloud of neighboring species towards itself and the process of distortion of electron cloud is known as polarization.
Coordinate Covalent Bonds
A coordinate covalent bond is also known as a dative bond, which is a type of covalent bond. It is formed between two atoms, where the two electrons required to form the bond come from the same atom resulting in a semi-polar bond. The study of coordinate covalent bond or dative bond is important to know about the special type of bonding that leads to different properties. Since covalent compounds are non-polar whereas coordinate bonds results always in polar compounds due to charge separation.
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