Polarity Is the separation of an electric charge which leads a molecule to have a p o s i t i v e an d negative end. - The distribution of electrical charge over the atoms joined by the bond. Charge is evenly distributed in a nonpolar, but unevenly distributed in a polar molecule. POLAR MOLECULE- Unequal distribution of charges, one is more positive and the other is more negative. - Dissolves in water. -Asymmetrical in shape NONPOLAR MOLECULE- Equal distribution of charges, no dipole (+/-). - Does not dissolve in water. - Symmetrical in shape Can be determined by two factors: 1. electronegativity difference 2. molecular geometry through the VSEPR ( Valence Shell E l e c tron Pair Repulsion) theory FIRST STEP: Determine the total number of electrons of the given molecule. SECOND STEP: Draw lines to bond the atoms (one line means two electrons). THIRD STEP: Check if the OCTET RULE is followed. Eight electrons should should be around the element. Except for hydrogen which only needs two electrons. FOURTH STEP: Rearrange the electrons of the bonded atom. You may create double or triple bond if necessary. FIFTH STEP: Generic Check Formula and and compare Molecular to the shape. SIXTH STEP: answer the following questions: -Bonded elements are the same? (If no, it's POLAR) (If YES, answer the following question: With lone pairs?) (If without lone pair, it's NONPOLAR); (If with lone pairs, is it asymmetric or symmetric?--- Asymmetric= Polar; Symmetric= Nonpolar)

1. Polarity of
Molecules
(Polar and Nonpolar)
11th grade

2. Polarity
Is the separation of an
e l e c t r i c c h a r g e
w h i c h l e a d s a
molecule to have a
p o s i t i v e a n d
negative end.

3. POLARITY
The distribution of electrical charge over the
atoms joined by the bond.
Charge is evenly distributed in a nonpolar, but
unevenly distributed in a polar molecule.

4. CHEMICAL BONDING
- A force that holds atoms together in a
molecule or compound.
- Formed when atoms lose, accept or share
electrons

5. Why does atom bonds?
-
-
Atoms form bonds so each atom has 8
valence electrons.
This makes the atom stable.
- Ions formed as a result of electron
transfer.

6. CHEMICAL BONDING
Metallic
is a term used to describe the
collective sharing of a sea of
valence electrons between
several positively charged
metal ions.
Covalent
Ionic
In ionic compounds, ions
are h el d to g eth er b y
el ectrostatic forces –
forces between oppositely
charged ions.
Bonds
A bond created by the
sharing of el ectrons
between atoms (in pairs)

7. In ionic compounds, ions are held
together by electrostatic forces –
forces between oppositely
charged ions.
Electrons transferred between
the cation (positively charged ion)
and the anion (negatively
charged ion)
IONIC BOND

8. -Occurs between a metal and a nonmetal.
Metal Atom loses e-: gets a positive charge.
Nonmetal Atom gains e-: gets a negative charge.

9. COVALENT BOND
-
-
A bond created by the
s h a r i n g o f e l e c t ro n s
between atoms (in pairs)
Oc c urs b e t w e e n t w o
nonmetals (resulting in a
neutral overall charge).
- Electrons not transferred in
t h i s c a s e E l e c t r o n s
typically shared in pairs

10. TYPES OF COVALENT BONDS
POLAR COVALENT
BOND
NONPOLAR
COVALENT BOND
e- shared equally
e- shared unequally,
so there’ll be no
chance to have a
partial positive
a n d p a r t i a l
negative end.

11. TYPES OF COVALENT BONDS
POLAR COVALENT BOND
e- shared unequally,
so there’ ll be no
chance to have a
partial positive and
partial negative end.

12. TYPES OF COVALENT BONDS
NONPOLAR
COVALENT BOND
e- shared
equally

13. POLAR
MOLECULE
NONPOLAR MOLECULE
- Unequal distribution of
charges, one is more
positive and the other is
more negative.
Equal distribution of
charges, no dipole (+/-).
Dissolves in water. - Does not dissolve in water.
- Asymmetrical in shape - Symmetrical in shape

14. POLARITY
01
- separation of an electric charge which
leads a molecule to have a positive and
negative end
01

15. Can be determined by two factors:
molecular geometry
through the VSEPR
( V a l e n c e S h e l l
E l e c t r o n P a i r
Repulsion) theory
electronegativity
difference
01 02

16. VALENCE ELECTRON AND
LEWIS DOT SYMBOL
●
●
Valence shell- Outer
shell of an atom
Valence electrons are
t h e “ o u t e r m o s t
electrons” of the atom
involved in chemical
bonding.

17. VALENCE ELECTRON AND
LEWIS DOT SYMBOL
● Octet Rule states that
atoms tend to form
compounds in ways
that give them eight
valence electrons and
t h u s t h e e l e c t r o n
configuration of a noble
gas.

18. Rules for writing shell electron configurations of the
representative elements:
1.
2.
3.
The number of electrons in an atom of a given
element is the same as the element’s atomic
number.
Number of shells that contains electrons will be
the same as the period number.
For the representative (Group A) elements, the
number of valence electrons is the same as the
group number.

19. Recall:
Period 1
Period 2
Period 3
Period 4
Period 5
Period 6

20. Lewis Structures
Gilbert Newton Lewis (1875-1946) an American
chemist who developed in 1916 the electron dot
symbols to help explain chemical bonding.
Lewis symbol, the nucleus and the inner
electrons of an atom or ion are represented by
the element’s symbol.

21. Lewis Structures
●
●
●
Lewis structures use Lewis symbol
to show valence electrons in
molecules and ions of compounds.
The pair of dots representing the
shared pair of electrons in a
covalent bond is often replaced by
a long dash.
An unshared pair, also called a lone
pair, is a pair of electrons that is not
in volved in bon din g an d th at
belongs exclusively to one atom.
Shared pair
(covalent bond)
•
•
Lone
pair

22. Lewis symbols for the first three periods of
representative elements
1A 2A 3A 4A 5A 6A 7A 8A
Li●
●Be●
●
●B●
●
●C●
●
●●
●N●
●
Na● ●Mg●
●
●Al●
●
●Si●
●
●●
●P●
●
H● He
●
●

23. STEPS FOR DRAWING LEWIS DOT SYMBOLS:





Count all the valence electron.
Determine the central atom (the element
there is only one of).
Draw a single bonds to the central atom.
Put all the valence electron on atoms as
lone pairs.
Turn lone pairs into double or triple bonds to
give every atom an octet.

24. ELECTRONEGATIVITY
●
●
Electronegativity is a measure of how
strongly atoms attract bonding
electrons to themselves.
The higher the electronegativity, the
greater an atom’s attraction for
electrons.

25. ELECTRONEGATIVITY
Increasing
Decreasing

26. ELECTRONEGATIVITY

27. PAULING ELECTRONEGATIVITY VALUES
Type of Bond Electronegativity
Difference (ΔEN)
Ionic ≥1.7
Polar Covalent 0.5 to 1.6
Nonpolar Covalent ≤0.4

28. Molecules Electronegativity Difference (ΔEN)
Po
lar
Nonp
olar
Example
S02
EN of S = 2.5
EN of O = 3.5 √
Predict the type of polarity using electronegativity (EN)
values in the following molecules.

29. Predict the type of polarity using electronegativity (EN) values in
the following molecules.
Molecules Electronegativity Difference (ΔEN)
Po
lar
Nonp
olar
Example
S02
EN of S = 2.5
EN of O = 3.5 √
1. NH3
2. CCl4
3. H20
4. CH4
5. BH3
ΔEN=3.5-2.5 = 1.0

30. Molecules Electronegativity Difference (ΔEN)
Po
lar
Nonp
olar
Example
S02
EN of S = 2.5
EN of O = 3.5 √
Predict the type of polarity using electronegativity (EN)
values in the following molecules.
1st Step:
SO2
2nd Step:

31. 3rd Step: Check if the octet rule is
followed. 8 electrons should be
around the element. Except for
hydrogen which only needs two
electrons.
8 electrons around it
6 electrons around it
8 electrons around it 8 electrons around it 8 electrons around it
8 electrons around it
4th Step: Rearrange the electrons of
the bonded atom. You may create
double or triple bond if necessary.

32. Legend:
A – Central atom
X - Number of
bond
E – Lone pair
Generic Formula Molecular Shape
AX Linear
AX2 Linear
AXE Linear
AX3 Trigonal Planar
AX2E Bent
AXE2 Linear
AX4 Tetrahedral
AX3E Trigonal Planar
AX2E2 Bent
AXE1 Linear

33. Generic
Formula
Molecular
Shape
AX Linear
AX2 Linear
AXE Linear
AX3 Trigonal Planar
AX2E Bent
AXE2 Linear
AX4 Tetrahedral
AX3E Trigonal Planar
AX2E2 Bent
AXE1 Linear
Bonded
atom
Bonded
atom
Lone pair
AX2E
No. of Bonded Atoms : 2
Lone Pair : 1
Legend:
A – Central atom
X - Number of bond
E – Lone pair

34. Generic
Formula
Molecular
Shape
AX Linear
AX2 Linear
AXE Linear
AX3 Trigonal Planar
AX2E Bent
AXE2 Linear
AX4 Tetrahedral
AX3E Trigonal Planar
AX2E2 Bent
AXE1 Linear
Bonded
atom
Bonded
atom
Lone pair
AX2E
No. of Bonded Atoms : 2
Lone Pair : 1

35. Generic
Formula
Molecular
Shape
AX Linear
AX2 Linear
AXE Linear
AX3 Trigonal Planar
AX2E Bent
AXE2 Linear
AX4 Tetrahedral
AX3E Trigonal Planar
AX2E2 Bent
AXE1 Linear
Bonded
atom
Bonded
atom
Lone pair
AX2E - BENT
No. of Bonded Atoms : 2
Lone Pair : 1
5th Step: Check and compare to the
Generic Formula and Molecular
shape.

37. 5th Step: Draw the molecular shape.

38. Check the table in the next slide

39. VSEPR-predicted
molecular and
electron-pair
geometries. The
m o l e c u l a r
geometries are
identical to the
electron-pair
geometries when
there are no lone
pairs present. A,
central atom; X,
peripheral atom;
E , u n s h a r e d
electron pair.

41. Figure 8. VSEPR-predicted molecular and electron-pair geometries. The molecular geometries are identical to the
electron-pair geometries when there are no lone pairs present. A, central atom; X, peripheral atom; E, unshared electron
pair.

42. V S E P R - p r e d i c t e d
molecular and electron-
pair geometries. The
molecular geometries are
identical to the electron-
pair geometries when there
are no lone pairs present.
A , c e n t r a l a t o m ; X ,
p e r i p h e r a l a t o m ; E ,
unshared electron pair.

43. 6th Step: Answer the question from this diagram.
Bonded elements are the same?
No
POLAR
Asymmetri
c
Symmetric
Yes
Yes
With lone pairs?
No
NONPOLAR

44. Answer: Polar

45. FIRST STEP: Determine the total number of electrons of
the given molecule.
SECOND STEP: Draw lines to
bond the atoms (one line
means two electrons).
CH4
CH4
C 1 x 4 = 4
H 4 x 1 = 4
8

46. THIRD STEP: Check if the OCTET RULE is followed. Eight electrons
should should be around the element. Except for hydrogen which only
needs two electrons.
FOURTH STEP: R earrang e the
electrons of the bonded atom. You
may create double or triple bond if
necessary.
CH4
No need since it already
follows the octet rule.

47. Generic
Formula
Molecular
Shape
AX Linear
AX2 Linear
AXE Linear
AX3 Trigonal Planar
AX2E Bent
AXE2 Linear
AX4 Tetrahedral
AX3E Trigonal Planar
AX2E2 Bent
AXE1 Linear
AX4 - TETRAHEDRAL
No. of Bonded Atoms : 4
Lone Pair : 0
FIFTH STEP: Check and compare to the
Generic Formula and Molecular shape.

48. 6th Step: Answer the question from this diagram.
Bonded elements are the same?
No
POLAR
Asymmetri
c
Symmetric
Yes
Yes
With lone pairs?
No
NONPOLAR

49. A n s w e r :
Nonpolar

50. Single Double Triple
Examples:
H2
F2
HCl
●
●
●
Examples: Examples:
Write some examples of the following covalent bonds having in mind the information learned
Covalent bonds
A B
A B
A B
A B A B
A B

51. Complete the table below with examples of ionic compounds
Ionic bonds and atoms
Name Symbol Atoms Formula
Potassium oxide K2O
2 potassium
1 oxygen
●
●
K2O2 + 2K → 2K2O

52. Write the number of atoms in the following formulas
Number of atoms
H2SO4
CaCl2
NaCl
C2H6
KNO3
H2O2
KMnO4
H3PO4

53. O
Drag the electrons into each atom to
create the formation of water
H
H
+ + + + + + + + - - - - - - - -

54. Single Double Triple
Examples:
H2
F2
HCl
●
●
●
Examples: Examples:
Write some examples of the following covalent bonds having in mind the information learned
Covalent bonds
A B
A B
A B
A B A B
A B

55. Categorize the components of each bonding using your periodic table
Determine each compound
Formula Metal Non-metal Bond
NO2
NaCl
C4H10
Na2S
H2S

56. Explain the water splitting process observing the separation of water molecules into hydrogen
and oxygen in the infographic below
Water splitting
O2
2H2O 2H2 +
Explain the process here
+

57. Chemical bonding process
Valences
Octet rule
Structures
Geometry

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