Chemical bonding occurs through either ionic bonds or covalent bonds. Ionic bonds result from the electrostatic attraction between oppositely charged ions, while covalent bonds form through the sharing of electrons between atoms. The octet rule states that atoms seek to attain a full outer shell of eight electrons to achieve stability. Covalent bonds form when atoms share electrons to attain stable electron configurations of eight electrons. Metallic bonding is characterized by positive metal ions embedded in a "sea" of delocalized valence electrons, giving rise to metallic properties such as conductivity, malleability, and luster.

1. Chemical
Bonding

2. CHEMICAL BONDING
• is a lasting attraction between atoms, ions or molecules that enables
the formation of chemical compounds. The bond may result from
the electrostatic force of attraction between oppositely charged ions
as in ionic bonds or through the sharing of electrons as in covalent
bonds. The strength of chemical bonds varies considerably; there
are "strong bonds" or "primary bonds" such as
covalent, ionic and metallic bonds, and "weak bonds" or "secondary
bonds" such as dipole–dipole interactions, the London dispersion
force and hydrogen bonding.

3. ELEMENTS
are pure substances made up of
one kind of material. Elements
are classifies as metals, non
metals and metalloids.

5. SYMBOL ELEMENTS LATIN NAME
Na Sodium Natrium
K Potassium Kalium
Fe Iron Ferrum
Cu Copper Cuprum
Ag Silver Argentum
Sn Tin Stannum
Sb Antimony Stibium
Hg Mercury Hydrargyyrum
Au Gold Aurum
Pb Lead Plumbum

6. CLASSIFICATION OF ELEMENTS
METALS
metals are mostly solid in form, except for
mercury, they possess luster and they shine
when light falls on them.
Examples:
• Magnesium
• Platinum
• Nickel
• Iron
• Silver

7. •Non metals exist in solids, liquids, and
gases. They are usually light in weight.
They are used as insulators because they
are poor conductors of heat and
electricity.
Examples:
• Carbon
• Phosphorus
• Sulfur
• Iodine
• Bromine
Non
Metals

8. •metalloids are elements that have properties of
both metals and non metals. Metalloids are
solid but lack luster.
Examples: • Boron
• Silicon
• Arsenic
Metalloids

9. COMPOUNDS
• Compounds are the combination of two or more elements that are
chemically combined.
• When elements are combined to form a compound, elements lose their
own identity and characteristics. The new substance formed has different
characteristics and properties from the original elements.
• Example, hydrogen (h) and oxygen (o) are both gases. they combined to
form water (h20). they combine with a definite proportion. water (h2o)
has 2 atoms of hydrogen and 1 atom of oxygen.
• Compounds could be written in a chemical formula, a chemical formula is
an arrangement of symbols and numbers that describe a compound.
H2o is a chemical formula of one molecule of water.

10. KINDS OF COMPOUNDS
ACIDS
Acids are compounds that produce hydrogen ions
when dissolved in water. Some acids are weak and
some are strong.
• Acid can cause certain chemical dyes called
indicators to change color.
• Indicators is a substance that change color at
certain range of Ph values.

11. ACIDS
NAME FORMULA
Nitric HN𝟎𝟑
Perchloric HCL𝟎𝟒
Sulfuric 𝑯𝟐𝐒𝟎𝟒
Hydrobomic HBr
Carbonic 𝑯𝟐𝐂𝟎𝟑
Hydrochloric HCL

12. BASES
• Bases are compounds that produce
hydroxide ions when dissolved in
water.
• Bases usually feel slippery and
have bitter taste.

13. Ionic Bond

14. THE OCTET RULE
• Everyone is seeking for stability. STABILITY refers to the strength to
stand or a resistance to chemical change or physical change. If
humans seek stability, so are the atoms. Stability in atoms involves
the possession of eight (8) electrons in its outermost energy level
or valence electrons. Atoms of all elements, therefore, to become
stable, need to have 8 valence electrons. We call this the OCTET
RULE which was proposed by Gilbert Newton Lewis, an American
Chemist. Lewis spent one year in the Philippines as the
superintendent of the Bureau of Weights and Measures.

16. VALENCE ELECTRON
•The Configuration of electrons and valence electrons are
highly important in the study of chemical bonding.
ELECTRON CONFIGURATION refers to the distribution of
electrons at different positions in an atom. It becomes
more complex as you move along the periodic table due to
an increase of atomic number and, therefore, an increase
of energy level of atoms. On the other hand, VALENCE
ELECTRON are the electrons occupying the highest energy
level in an atom.

18. Electron Configuration of the First 10 Elements
Element Symbol Atomic Number Electron Configuration Number of Valence
Electrons
Group
H 1 1𝒔𝟏 1 1
He 2 1𝒔𝟐 2 8
Li 3 1𝒔𝟐𝟐𝒔𝟏 1 1
Be 4 1𝒔𝟐𝟐𝒔𝟐 2 2
B 5 1𝒔𝟐𝟐𝒔𝟐𝟐𝒑𝟏 3 3
C 6 1𝒔𝟐
𝟐𝒔𝟐
𝟐𝒑𝟐 4 4
N 7 1𝒔𝟐
𝟐𝒔𝟐
𝟐𝒑𝟑 5 5
O 8 1𝒔𝟐
𝟐𝒔𝟐
𝟐𝒑𝟒 6 6
F 9 1𝒔𝟐
𝟐𝒔𝟐
𝟐𝒑𝟓 7 7
Ne 10 1𝑠22𝑠22𝑝6 8 8

19. Lewis Electron Dot Structure (LEDS)
•A system known as LEDS, proposed by Gilbert N. Lewis, is
used to emphasize the atom’s valence electrons. It is a
shorthand method which consists of a symbol of the
element surrounded by dots. The symbol represents the
nucleus of the atom; while the dots represent the valence
electrons of the atom.

22. Covalent
Bond

23. Covalent Bond
•The second type of chemical bond is covalent bond.
Unlike ionic bond, elements involved in covalent
bonds do not transfer electrons but instead they
share electrons. This type of bond exists between
nonmetals.

24. Formation of Covalent Compounds
•When two or more nonmetallic elements combine in a
covalent bonding, a molecule is formed. Gases like O2, H2,
F2, Br2, and I2 always occur as diatomic molecule. As such,
they are more stable than single atoms.

25. Three Types of Covalent Bond
•A single covalent bond, denoted by one short line (-),
is the sharing of one electron pair between two
atoms.
•A double covalent bond, denoted by two short lines
(=), is the sharing of two electron pairs.
•A triple covalent bond, denoted by three short lines,
is the sharing of three electron pairs.

26. Molecular Geometry
•In molecular geometry, the bond lengths and angles
determined experimentally. A simple procedure known as
the VALENCE SHELL ELECTRON REPULSION (VSEPR) can
help predict the geometric arrangement of atoms in
molecules.

27. Linear
• The shaped is produced when two groups try to get as far away
from each other as they can. In HgCl2, molecule, mercury atom
with two electrons in its valance shell is used to form covalent
bond with one electron of chlorine atom producing a linear shape
molecule.
• Cl – Hg – Cl
• As you notice, the HgCl2, molecule adapts a shape where its two
electron pair bonds are as far away from each other as possible.
The shape is linear since the central atom has two bonding electron
pairs in its valence shell. In addition to linear, the angle between
ion pair sand central atom is 180°.

29. Trigonal Planar
• Consider the boron trifluoride
(BF3) molecule. Boron’s three
valence electrons are supplied
with one electron of fluorine to
form single bond BF3. This
shape is formed when three
pairs get as far apart from each
other as possible. The angle
formed by any two bonds in the
molecule is 120°.

30. Tetrahedron
•This structure is a common
one. Many nonmetals and
ions have this structure. One
of which is methane, CH4. In a
methane molecule, carbon
has four bonding pairs of
electrons in its valence shell.
The bond angle for
tetrahedron is 109.5°.

31. Trigonal Bipyramid
• When there are five electron
pairs, trigonal bipyramid structure
is formed. One good example for
this is PCl5 molecule. The five
valence electrons of phosphorus
atom form five boding pairs with
electrons from five chlorine
atoms. Unlike tetrahedron which
bonds are equidistant, the
distance of trigonal bipyramid
bonds are not equal.

32. Octahedron
•Sulfur hexafluoride (SF6) is
one of the few molecules
that have this structure. Six
bonding pairs are present in
which all the positions are
equivalent, all the bond
distances are equal, all the
angles formed by any
adjacent bonds are 90°.

34. Metallic
Bond

35. Metallic Properties
•Metallic solids have special properties that separate them
from other solids. Metallic elements, as what we know, are
located at the left side of the periodic table. A distinct
ladder-like line separates them from the nonmetals. The
position gives an important clue regarding the nature of
how they are bonded together to form solids.
•Metals are malleable, ductile, and have high melting point.
They are good conductors of heat and electricity as well.

36. •Metals have high
melting points. This is
due to the
electrostatic attraction
between the lattice of
metal cation and fluid
of valence electrons in
which they are
immersed.

37. •Metallic compounds are
known to be malleable and
ductile. As you know,
malleability is the ability of
metals to be shaped by
pressure, either by
hammering, rolling into
sheets, or forging. On the
other hand, ductility is the
ability of metals to be drawn
into a wire.

38. •Luster is another distinct
property among metals.
Luster is the ability to
shine and reflect light.
The presence of free
electrons that vibrate
and move are the
reasons why metals
reflect light.