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Presented by
Dr. Ujwalkumar Trivedi
Head
Department of Biotechnology
Marwadi University
Rajkot (Gujarat)
Chemical Bonds
Helium
atomElectron
Shell Nucleus
a) Atomic number = number of protons
b) Electrons vary in the amount of energy they
possess, and they occur at certain energy
levels or electron shells.
a) Electron shells determine how an atom
behaves when it encounters other atoms
The octet rule is a simple chemical rule of thumb that
states that atoms tend to combine in such a way that they
each have eight electrons in their valence shells, giving
them the same electronic configuration as a noble gas. The
rule is applicable to the main-group elements, especially
carbon, nitrogen, oxygen, and the halogens, but also to
metals such as sodium or magnesium. In simple terms,
molecules or ions tend to be most stable when the
outermost electron shells of their atoms contain eight
electrons
Octet Rule = atoms tend to gain, lose or share electrons so
as to have 8 electrons
C would like to
N would like to
O would like to
Gain 4 electrons
Gain 3 electrons
Gain 2 electrons
Representation of Valance Electron
Shells
Note: Only valance electrons
are represented
Bonds are formed to attain the Nobel gas
configuration (Octate Rule)
1.Ionic bonds –
2.Covalent bonds –
3.Metallic bonds
Ionic Bonds
Ionic bonds are formed as a result of electrostatic
interactions arising due to ions formed by gaining or
losing the electrons.
Ionic compounds result when metals react with
nonmetals
Metals lose electrons to match the number of
valence electrons of their nearest noble gas
Positive ions form when the number of electrons
are less than the number of protons
Group 1 metals → ion 1+
Group 2 metals → ion 2+
 Group 13 metals → ion 3+
Sodium atom Sodium
ion
Na •
– e−
→ Na +
2-8-1 2-8 ( = Ne)
11 p+
11 p+
11 e-
10 e-
0 1+
Magnesium atom Magnesium ion
•
Mg •
– 2e−
→ Mg2+
2-8-2 2-8
(=Ne)
12 p+
12 p+
12 e- 10 e-
0 2+
Group 1 Group 2 Group 13
H+
Mg2+
Al3+
Li+
Ca2+
Na+
Sr2+
K+
Ba2+
A. Number of valence electrons in aluminum
1) 1 e-
2) 2 e-
3) 3 e-
B. Change in electrons for octet
1) lose 3e-
2) gain 3 e-
3) gain 5
e-
C. Ionic charge of aluminum
1) 3- 2) 5- 3) 3+
A. Number of valence electrons in
aluminum
3) 3 e-
B. Change in electrons for octet
1) lose 3e-
C. Ionic charge of aluminum
3) 3+
Give the ionic charge for each of the
following:
A. 12 p+
and 10 e-
1) 0 2) 2+ 3) 2-
B. 50p+
and 46 e-
1) 2+ 2) 4+ 3) 4-
C. 15 p+
and 18e-
2) 3+ 2) 3- 3) 5-
In ionic compounds, nonmetals in 15,
16, and 17 gain electrons from metals
Nonmetal add electrons to achieve the
octet arrangement
Nonmetal ionic charge:
3-, 2-, or 1-
unpaired electron octet
• • • • 1 -
: F •
+ e−
: F :
• • • •
2-7 2-8 (= Ne)
9 p+ 9 p+
9 e- 10 e-
0 1 -
ionic charge
 Between atoms of metals and nonmetals with very
different electronegativity
 Bond formed by transfer of electrons
 Produce charged ions all states. Conductors and
have high melting point.
 Examples; NaCl, CaCl2, K2O
NaCl formation
Ionic Bonds: One Big Greedy
Thief Dog!
Ionic bond in NaCl – electron from Na is transferred to
Cl, this causes a charge imbalance in each atom. The Na
becomes (Na+) and the Cl becomes (Cl-), charged
particles or ions.
NaClNaCl
Covalent BondsCovalent Bonds
Covalent Bonds are formed by sharing of electrons
between the atoms of similar electronegativity
 Between nonmetallic elements of similar
electronegativity.
 Formed by sharing electron pairs
 Stable non-ionizing particles, they are not
conductors at any state
 Examples; O2, CO2, C2H6, H2O, SiC
H2 or Cl2
Non Polar Covalent bonds-Two atoms share one
or more pairs of outer-shell electrons.
Oxygen AtomOxygen Atom Oxygen AtomOxygen Atom
Oxygen Molecule (OOxygen Molecule (O22))
H2O
Polar Covalent Bonds: Unevenly
matched, but willing to share.
- water is a polar molecule because oxygen is more
electronegative than hydrogen, and therefore electrons
are pulled closer to oxygen.
Structure of H2O
 Formed between atoms of metallic elements
 Electron cloud around atoms
 Good conductors at all states, lustrous, very high
melting points
 Examples; Na, Fe, Al, Au, Co
Metallic Bonds: Mellow dogs with
plenty of bones to go around.
Metals do not combine with metals. They form
Alloys which is a solution of a metal in a metal.
Examples are steel, brass, bronze and pewter.
Thank You
Kindly Reach us at:
Marwadi University
Rajkot-Morbi Highway Road, Gauridad, Rajkot, Gujarat 360003
Website: https://www.marwadieducation.edu.in/

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Chemical Bonds

  • 1. Presented by Dr. Ujwalkumar Trivedi Head Department of Biotechnology Marwadi University Rajkot (Gujarat) Chemical Bonds
  • 3. a) Atomic number = number of protons b) Electrons vary in the amount of energy they possess, and they occur at certain energy levels or electron shells. a) Electron shells determine how an atom behaves when it encounters other atoms
  • 4. The octet rule is a simple chemical rule of thumb that states that atoms tend to combine in such a way that they each have eight electrons in their valence shells, giving them the same electronic configuration as a noble gas. The rule is applicable to the main-group elements, especially carbon, nitrogen, oxygen, and the halogens, but also to metals such as sodium or magnesium. In simple terms, molecules or ions tend to be most stable when the outermost electron shells of their atoms contain eight electrons
  • 5. Octet Rule = atoms tend to gain, lose or share electrons so as to have 8 electrons C would like to N would like to O would like to Gain 4 electrons Gain 3 electrons Gain 2 electrons
  • 6. Representation of Valance Electron Shells
  • 7. Note: Only valance electrons are represented
  • 8. Bonds are formed to attain the Nobel gas configuration (Octate Rule) 1.Ionic bonds – 2.Covalent bonds – 3.Metallic bonds
  • 9. Ionic Bonds Ionic bonds are formed as a result of electrostatic interactions arising due to ions formed by gaining or losing the electrons.
  • 10. Ionic compounds result when metals react with nonmetals Metals lose electrons to match the number of valence electrons of their nearest noble gas Positive ions form when the number of electrons are less than the number of protons Group 1 metals → ion 1+ Group 2 metals → ion 2+  Group 13 metals → ion 3+
  • 11. Sodium atom Sodium ion Na • – e− → Na + 2-8-1 2-8 ( = Ne) 11 p+ 11 p+ 11 e- 10 e- 0 1+
  • 12. Magnesium atom Magnesium ion • Mg • – 2e− → Mg2+ 2-8-2 2-8 (=Ne) 12 p+ 12 p+ 12 e- 10 e- 0 2+
  • 13. Group 1 Group 2 Group 13 H+ Mg2+ Al3+ Li+ Ca2+ Na+ Sr2+ K+ Ba2+
  • 14. A. Number of valence electrons in aluminum 1) 1 e- 2) 2 e- 3) 3 e- B. Change in electrons for octet 1) lose 3e- 2) gain 3 e- 3) gain 5 e- C. Ionic charge of aluminum 1) 3- 2) 5- 3) 3+
  • 15. A. Number of valence electrons in aluminum 3) 3 e- B. Change in electrons for octet 1) lose 3e- C. Ionic charge of aluminum 3) 3+
  • 16. Give the ionic charge for each of the following: A. 12 p+ and 10 e- 1) 0 2) 2+ 3) 2- B. 50p+ and 46 e- 1) 2+ 2) 4+ 3) 4- C. 15 p+ and 18e- 2) 3+ 2) 3- 3) 5-
  • 17. In ionic compounds, nonmetals in 15, 16, and 17 gain electrons from metals Nonmetal add electrons to achieve the octet arrangement Nonmetal ionic charge: 3-, 2-, or 1-
  • 18. unpaired electron octet • • • • 1 - : F • + e− : F : • • • • 2-7 2-8 (= Ne) 9 p+ 9 p+ 9 e- 10 e- 0 1 - ionic charge
  • 19.  Between atoms of metals and nonmetals with very different electronegativity  Bond formed by transfer of electrons  Produce charged ions all states. Conductors and have high melting point.  Examples; NaCl, CaCl2, K2O
  • 21. Ionic Bonds: One Big Greedy Thief Dog!
  • 22. Ionic bond in NaCl – electron from Na is transferred to Cl, this causes a charge imbalance in each atom. The Na becomes (Na+) and the Cl becomes (Cl-), charged particles or ions. NaClNaCl
  • 23. Covalent BondsCovalent Bonds Covalent Bonds are formed by sharing of electrons between the atoms of similar electronegativity
  • 24.  Between nonmetallic elements of similar electronegativity.  Formed by sharing electron pairs  Stable non-ionizing particles, they are not conductors at any state  Examples; O2, CO2, C2H6, H2O, SiC
  • 26. Non Polar Covalent bonds-Two atoms share one or more pairs of outer-shell electrons. Oxygen AtomOxygen Atom Oxygen AtomOxygen Atom Oxygen Molecule (OOxygen Molecule (O22))
  • 27. H2O
  • 28. Polar Covalent Bonds: Unevenly matched, but willing to share.
  • 29. - water is a polar molecule because oxygen is more electronegative than hydrogen, and therefore electrons are pulled closer to oxygen. Structure of H2O
  • 30.
  • 31.  Formed between atoms of metallic elements  Electron cloud around atoms  Good conductors at all states, lustrous, very high melting points  Examples; Na, Fe, Al, Au, Co
  • 32. Metallic Bonds: Mellow dogs with plenty of bones to go around.
  • 33.
  • 34. Metals do not combine with metals. They form Alloys which is a solution of a metal in a metal. Examples are steel, brass, bronze and pewter.
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