Explore the types of chemical bonding

3. HOW TO
MAKE THE
ATOMS
STABLE?

5. IONIC BONDING • Metal loses electrons and
becomes positive (+) ion,
called CATION.
• Nonmetal accepts the
electron and becomes
negative (-) ion, called
ANION.
• FORMULA UNIT- it is a pair of
cation and anion.
• BOILING POINT: High
• MELTING POINT: High
• ELETCRONEGATIVITY: 1.8
and above

7. EXERCISES
FORMULA
UNIT
LEDS OF
EACH
ELEMENT
IONIC BOND
FORMATION
KBr
CaF2

8. COVALENT BONDING
• Two nonmetal atoms share
electrons and forms Covalent
Bonding.
• MOLECULES- covalent
bonded atoms.
• This forms single, double, and
triple bonds.
• BOILING POINT: Average
• MELTING POINT: Average

10. POLAR COVALENT
BOND- Unequal
sharing of electrons
ELECTRONEGATIVITY:
0.5 - 1.7
NONPOLAR
COVALENT BOND-
Unequal sharing of
electrons
ELECTRONEGATIVITY:
0 - 0.4

11. REAL LIFE APPLICATION OF IONIC COMPOUNDS
Sodium chloride (table salt) is used to season
food.
Note: Consuming large amounts of sodium ion
(regardless if it is from sodium chloride, sodium
glutamate, or sodium benzoate) can lead to
cardiovascular and kidney problems.
Calcium carbonate- This compound is also
known as chalk and is contained in antacids like Tums
and Rolaids.
The carbonate portion of this formula helps to
neutralize excess stomach acid to help soothe the
stomach.

12. REAL LIFE APPLICATION OF IONIC COMPOUNDS
Derivatives of ammonia are used as fertilizers and
smelling salts (stimulant)
Sodium hypochlorite (bleach)- This chemical is
used to remove stains from clothing and can be used
to disinfect water.

13. REAL LIFE APPLICATION OF COVALENT COMPOUNDS

14. BONDING CHARADES
FOUR TYPES OF BONDS =
FOUR POSSIBLE ANSWERS
IONIC BONDS
POLAR COVALENT BONDS
NONPOLAR COVALENT
BONDS
METALLIC BONDS

16. WHAT IS A MOLECULES?
• A molecule is a group of two or more atoms held together by
chemical bonds.

17. WHAT IS A MOLECULE?
• A molecule is a group of two or more atoms held together by
chemical bonds.

18. POLARITY
• it refers to the distribution of electric charge around atoms, chemical
groups, or molecules.

19. POLARITY of Molecules
• Polarity of the bonds between atoms which can be studied based on
Electrnonegativtity.
• The Geometrical shape of the molecule which can be predicted via the
valence shell electron pair repulsion (VSEPR) theory.

20. ELECTRONEGATIVITY INCREASES
ELECTRONEGATIVITY
DECREASES

23. MOLECULAR GEOMETRY
• The Valence shall electron pair repulsion (VSEPR) theory will help us
to determine the spatial arrangement of atoms in a polyatomic
molecule.

25. METALLIC BONDING
• Is a type of chemical bond that forms when metal atoms share their
pooled valence electrons.

29. are you ready?

30. MISE WHIMS HOOT

31. MY SWIMSUIT

32. DYE FOOL DYE POOL

33. DIPOLE-DIPOLE

34. HIGH DRAW GENE BRANDING

35. HYDROGEN BONDING

36. LAWN DRAWN DISK PERSIAN
FORGE

37. LONDON DISPERSION
FORCE

38. INTERMOLECULAR FORCES
OF ATTRACTION

39. LONDON DISPERSION FORCES
• A temporary attractive force occurs when two adjacent atoms form
temporary dipoles as a result of the positions occupied by their
electrons.

40. DIPOLE-DIPOLE
INTERACTIONS
• Attractive forces between the
positive end of one polar
molecule and the negative end of
another polar molecule.

41. HYDROGEN BONDING
• Strong dipole-dipole interaction
between a hydrogen atom
bonded to a highly
electronegative atom.