v Draw Lewis structures for each of the following. Give the total number of valence electrons, select from the lists the number of Regions of Electron Density (REDS) around the central atom, the molecular shape, and the bond angles. v Do not put covalent bonds between metals and nonmetals. v Put brackets around anions to show both charge and quantity. 1. HCI hydrogen chloride REDS 0, no central atom 2 3 4 valence e = REDS = Shapes tetrahedral shape = bond angles = pyramidal bent trigonal planar 2. CCI4 carbon tetrachloride linear diatomic monatomic ions valence e = Bond Angles 109.5° REDS = shape = bond angles = 120° 180° none, no central atom 3. Н.ССl dihydrogen carbon dichloride valence e = REDS = shape = bond angles =
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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