The document provides an overview of chemical bonding, including types such as covalent, ionic, and metallic bonds. It explains the reasons for bond formation, atomic structure, electronic configuration, and valency of elements, particularly from atomic numbers 1 to 20. Also included are definitions and characteristics of various bonds and their formation processes.

1. Introduction
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3. Chemical Bond
 Force of attraction b/w nucleus of one atom & e- of another atom.
 FOA which holds atoms/ions in a molecule
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5. Reason of Bond formation
 No elements exist as an independent atom in nature,except noble gases.
 Noble gas  most stable ; found in independent form
 To attain stability
 Sability ∝ 1/Energy
 Energy releases during bond formation  Bond formation is always
exothermic process.
 To gain electric configuration of nearest noble gas(chemically
inert/stable)
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6.  Water flowing down the hill (looses potential energy)
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7. Basics to learn Chemical
Bonding
Atomic mass/Mass no.(A)  No. of proton + No. of Neutrons
Atomic No.(Z)  No. of proton = No. of electrons
No. of neutrons = Atomic mass – Atomic No. ; (A-Z)
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9. Electronic Configuration
 W.r.t Shell
 W.r.t subshell
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10. w.r.t Shells
 No. of electrons in a shell = 2n2
 n = Shell no.
 K  n = 1 ; 2e-
 L  n = 8e-
 M  n = 18e-
 N  n = 32e-
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11. w.r.t subshell
 Electronic distribution by Aufbau Principles
 1s 2s 2p 3s 3p 4s 3d 4p
 s = 2e-
 p = 6e-
 d = 10e-
 f = 14e-
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12. Electronic configuration of Elements 1
to 20
Atomic No.(Z) Name Symbol w.r.t
shell(K,L)
w.r.t subshell
1 Hydrogen H 1 1S1
2 Helium He 2 1S2
3 Lithium Li 2,1 1S2 2S1
4 Beryllium Be 2,2 1S2 2S2
5 Boron B 2,3 1S2 2S2 2P1
6 Carbon C 2,4 1S2 2S2 2P2
7 Nitrogen N 2,5 1S2 2S2 2P3
8 Oxygen O 2,6 1S2 2S2 2P4
9 Flourine F 2,7 1S2 2S2 2P5
10 Neon Ne 2,8 1S2 2S2 2P6
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13. Atomic No.(Z) Name Symbol w.r.t shell(K,L,M,N) w.r.t subshell
11 Sodium Na 2,8,1 [Ne] 3s1
12 Magnesium Mg 2,8,2 [Ne] 3s2
13 Aluminium Al 2,8,3 [Ne] 3s2 3p1
14 Silicon Si 2,8,4 [Ne] 3s2 3p2
15 Phosphorous P 2,8,5 [Ne] 3s2 3p3
16 Sulphure S 2,8,6 [Ne] 3s2 3p4
17 Chlorine Cl 2,8,7 [Ne] 3s2 3p5
18 Argon Ar 2,8,8 [Ne] 3s2 3p6
19 Potassium K 2,8,8,1 [Ar] 4s1
20 Calcium Ca 2,8,8,2 [Ar] 4s2
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14. Valency
 Combining power of an atom
 Outermost shell  Valence shell
 No. of electrons in valence shell = Valence electrons
 Valence shell completes its 8 electrons by losing,gaining or sharing of
electrons  Valency
 Ex – Cl  2,8,7 ;- have 7 electrons in its valence shell ; needs 1 electron
to complete its octet  Valency 1
 Na  2,8,1 ; - have only 1 electron in its valence shell ; donates 1
electrons  Valency 1
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15. Atomic No.(Z) Name Symbol w.r.t shell(K,L) Valency
1 Hydrogen H 1 1
2 Helium He 2 0
3 Lithium Li 2,1 1
4 Beryllium Be 2,2 2
5 Boron B 2,3 3
6 Carbon C 2,4 4
7 Nitrogen N 2,5 3
8 Oxygen O 2,6 2
9 Flourine F 2,7 1
10 Neon Ne 2,8 0
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16. Atomic No.(Z) Name Symbol w.r.t shell(K,L,M,N) Valency
11 Sodium Na 2,8,1 1
12 Magnesium Mg 2,8,2 2
13 Aluminium Al 2,8,3 3
14 Silicon Si 2,8,4 4
15 Phosphorous P 2,8,5 3
16 Sulphure S 2,8,6 2
17 Chlorine Cl 2,8,7 1
18 Argon Ar 2,8,8 0
19 Potassium K 2,8,8,1 1
20 Calcium Ca 2,8,8,2 2
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17. Types of Chemicval Bond
 Covalent Bond
 Ionic Bond
 Coordinate Bond
 Metallic Bond
 Hydrogen Bond – F/O/N + H
 VanderWaal Bond – b/w inert gases
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19. Ionic Bond
 Complete transfer of electron
 b/w metals & non metals
 Metals (electropositive)  looses electron  Cation
 Non metals (electronegative)  gains electron  Anion
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23. Covalent Bond
 Forms due to sharing of electrons
 Equal sharing
 b/w non metals
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25. Coordinate bond
 Unequal sharing of electrons
 A type of Covalent bond
 One atoms donates 2 electrons/lone pair to other atom
 Represented by headed arrow () Head towards receiver,tail towards
donor.
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27. Metallic bond
 Between metals
 Metals looses electrons & forms electrons cloud/sea
 Metal becomes shiny & good conductor of electricity.
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29. Q.1 – No. of electrons in 1 molecule of
water
A. 18
B. 10
C. 22
D. 32
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30. Q.2-Bond involves when sharing of e
occurs
A. Covalent bond
B. Ionic bond
C. Metallic bond
D. Hydrogen Bond
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31. Q.3-Valency of oxygen is
A. 1
B. 2
C. 3
D. 4
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32. Q.4-Bond between e rich & e deficient
species.
A. Covalent bond
B. Ionic bond
C. Metallic bond
D. Coordinate bond
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33. Q.5-Hydrogen bonding is shown by
A. F
B. O
C. N
D. All of these
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