When sodium and chlorine take part in bond formation they attain octet configuration by
electron transfer (Atomic number Na 11 and Cl 17)
a) Represent the electron dot diagram of the above bond formation ?
Answers
Answer:
A bond between two atoms can be formed by transfer of valence electrons between them. This type of bond is known as electrovalent bond or ionic bond.
Example : Formation of sodium chloride (NaCl) which is discussed below :
The atomic number of sodium (Na) is 11, so its electronic configuration is 2,8,1. Sodium has only one electron in its outermost shell. Sodium loses one electron to attain its nearest noble gas configuration (neon).
Na → Na+ + e−
The atomic number of chlorine (Cl) is 17, so its electronic configuration is 2,7. Clearly, chlorine requires one electron to attain its nearest noble gas configuration (argon).
Cl + e− → Cl−
The complete reaction may be written as :
Na+ + Cl− → NaCl or Na+Cl−
Sharing of electrons
The bond formed by sharing of electrons is called a covalent bond. Sharing of electrons can be understood using the example of Cl2.
Formation of dichlorine (Cl2) : The atomic number of chlorine is 17 and has 7 valence electrons, which means Cl needs one more electron to complete its octet. In order to complete its octet , each chlorine atom contributes one electron to the shared pair. By doing this, both the chlorine atoms attain their nearest noble gas configuration (which is argon).
Single covalent bond : When one pair of electrons takes part in bond formation, the bond is known as single covalent bond.
Example : In H2O molecule, each hydrogen-oxygen bond is formed by sharing a pair of electrons.
Double covalent bond : When two pairs of electrons are involved in bond formation, the bond is known as double covalent bond.
Example : In CO2 molecule, each carbon-oxygen bond is formed by sharing two pairs of electrons.
Triple covalent bond : A triple covalent bond is formed when three pair of electrons are shared.
Example : In N2 molecule, three pair of electrons are shared between nitrogen atoms.
Dashes −, = and ≡
For simplicity, each shared pair of electrons can be represented by a dash (−) i.e., one dash is used to represent a single bond, two dashes are used for double, and three for triple bond. Example : the above structure of N2 can be simplified as :N≡N:.
Steps involved for writing Lewis structures
Count the total number of valence electrons of combining atoms. In case of ions, add one electron for each -ve charge and subtract one electron for each +ve charge.
In general, the least electronegative atom occupies the central position while other atoms are placed at the terminal.
Draw a single bond between atoms and check if all the atoms have complete octets. If each atom has complete octet then our structure is complete.
If some atoms have incomplete octets then use multiple bonds until they have complete octets. (Note : the number of dots i.e., valence electrons must not change
Sodium has 1 electron in its outermost shell. It transfers one electron to chlorine so it has now ten electrons which is the same as that of inert gas neon.
Explanation:
bad diagram but hope it help you
