Physical Science Grade 11 or 12 ABM Strand K-12 Senior High School (Curriculum Guided)

1. Types of Chemical Bonds
Prepared by: Jerome A. Bigael, Leyte Progressive High School

2. What is Chemical Bonds?
•A chemical bond is a lasting
attraction between atoms that
enables the formation of chemical
compounds.

3. Types of Bonds
• Covalent bond (share electrons)
bonds that involve the sharing of a pair of valence
electrons by two atoms.
• Ionic Bond (transfer electrons)
bond in which one or more electrons from one atom
are removed and attached to another atom, resulting
in positive and negative ions which attract each other.

4. Other types of Bonds
• Metallic bonds
is the force of attraction between valence electrons and the
metal atoms.
• Hydrogen bonding
it is a force of attraction between a hydrogen
atom in one molecule and a small atom of
high electronegativity in another molecule.

5. Covalent Bonds
•Covalent bonding can be
visualized with the aid of Lewis
diagrams.

7. •How does this sharing of
electrons affect the structure
and the properties of
substance?

8. Electronegativity
•The extent of sharing of electrons
between atoms in a molecule is
dependent on the electronegativity.
•Electronegativity is the ability of
each atom in a chemical bond to
attract electrons toward it.

9. •This affects a substance’s polarity
and interaction with other
substances.
•Recall that each atom has its own
electronegativity value (eV).

10. • The Higher the electronegativity value,
the higher the tendency of the atom to
attract electrons toward it.
• In the case of H2, O2, and N2, there is
equal sharing of electrons in the covalent
bond of each molecule because the
bonded atoms are of the same kind.

11. •Thus, they have the same
electronegativity value.
•The Bond that exist between these
kind of atom is called nonpolar
covalent bond.
•These kind of bond forms non-polar
molecules.

12. •On the other hand, Let us look at
hydrogen Chloride (HCl), which has
different atoms involved in the
covalent bond.
•Hydrogen has an electronegativity of
2.1 while chlorine has an
electronegativity of 3.0.

13. • Because chlorine has a higher
electronegativity value, electrons tend to
lean toward chlorine; thus, electrons in
two different atoms involved in the bond
are unequally shared and a polar
covalent bond is formed.
• This kind of bond forms a polar molecule.

14. •Due to unequal sharing of
electrons, the electron cloud leans
toward the more electronegative
element.
•This forms partial positive and
partial negative charges.

15. • Because the
electrons are
residing more on
the chlorine atom,
the electron cloud
of chlorine is larger
than that of
hydrogen.

16. • In this case, the hydrogen atom has lower
electronegativity value; thus, it acquires the
partial positive charge, and the shared
electrons are pulled away from it.
• On the other hand, the chlorine atom, which
has a higher electronegativity value, acquires
the partial negative charge; the electrons are
residing more on its side.

17. •Therefore, the
dipole moment
(symbolized by a
crossed arrow) is
directed toward
the chlorine atom.

18. Dipole moment
•Dipole moments occur when there
is a separation of charge.
•The dipole moment is a measure of
the polarity of the molecule.

19. Electronegativity Difference
What is Electronegativity?
•It is the ability of an atom in a
chemical bond to attract electrons
toward it.
Electronegativity values are found in
your periodic table.

20. •Based on Linus Pauling’s scale,
fluorine is the most electronegative
element, while francium is the least
electronegative.

22. •The difference in the
electronegativity values of the
atoms in a molecule or a
compound determines the type and
polarity of bond that is formed.

23. •An ionic bond is formed when the
difference in electronegativity values
(∆EN) of the element is greater than or
equal to 2.0 eV.
Electronegativity difference Type of Bond
∆EN≥2.0 Ionic
0.5<∆EN<2.0 Polar Covalent
0<∆EN≤0.5 Non polar Covalent

24. • A nonpolar covalent bond is formed
when the difference in electronegativity
value is equal to or less than 0.5 eV.
Electronegativity difference Type of Bond
∆EN≥2.0 Ionic
0.5<∆EN<2.0 Polar Covalent
0<∆EN≤0.5 Non polar Covalent

25. • On the other hand, a polar bond is
formed when the difference in
electronegativity values is greater than
0.5 eV but is less than 2.0 eV.
Electronegativity difference Type of Bond
∆EN≥2.0 Ionic
0.5<∆EN<2.0 Polar Covalent
0<∆EN≤0.5 Non polar Covalent

27. Classify each molecule as having a polar or a nonpolar
covalent bond. Then draw the dipole moment for each
molecule. Indicate the partial positive side a d the partial
negative side.
1. CO2
2. H2O
3. CH4
4. HBr
5. NH3

28. Electronegativity Difference and Type of Bond
Electronegativity difference Type of Bond
∆EN≥2.0 Ionic
0.5<∆EN<2.0 Polar Covalent
0<∆EN≤0.5 Non polar Covalent