The document discusses the arrangement and trends of the periodic table, explaining its structure, including periods and groups, and the properties of different families of elements. It highlights the behavior of metals, non-metals, and metalloids, as well as key concepts such as atomic radius, ionization energy, and reactivity. Furthermore, it notes the specific characteristics of various groups, including alkali metals, alkaline earth metals, halogens, and noble gases.

2. The Arrangement and
Periodic Trends
PERIODIC
TABLE

3. Objectives:
 Explain the arrangement in the
periodic table and it’s patterns.
 Classify the elements by the
arrangement of the elements in the
periodic table.
 Determine the properties of the
elements by the periodic table and
its trends.

4. ARRANGEMENT OF THE
ELEMENTS

5. Henry Moseley developed a modern period law.
- states that the properties of elements vary periodically with
atomic number.
- Atomic number (Moseley), atomic mass or weight
(Mendeleev).
- the organization of the table showed more consistent
periodic patterns of the physical properties and solved the
anomalies (metalloids have been found).

6. Periods and Groups
A period is a
horizontal row of
the periodic table.
There are seven
periods in the
periodic table, with
each one beginning
at the far left. A new
period begins when
a new principal
energy level begins
filling with
electrons. Also have
electron shells.
Vertical columns in
the periodic table
starting from top to
bottom are
called groups. There
are 18 groups in the
modern periodic
table. The elements
of same group have
same number of
valence electrons.

7. Neuron
Electron Shells
Valence Electrons
Electron
Proton

8. Periodic Table Groups (Families)
The families in the periodic table
were arranged by same
properties. The Lanthanides and
Actinide series known as Inner
transition metals. The families
have a difference reactivity
based on their properties.

9. The alkali metals consist of all of the elements in group one with the exception of hydrogen.
These elements are extremely reactive and for this reason, are usually found in compounds.
The alkaline earth metals are the second most reactive family on the periodic table
(following behind the alkali metals).
The name halogen means “salt formers” in greek. This is evident in nature as halogens
interact with metals to form various salts. On another note, the halogens are a unique group
of elements. They are the only periodic family that contains elements in the three states of
matter at standard temperature.
The noble gases, also called aerogens, are inert gases. Some examples include argon, krypton,
and neon. They can be found in group eighteen on the periodic table. Likewise, this means they
have a complete valence shell. For this reason, they are stable and relatively unreactive.

10. The transition metals typically form two or more oxidation states. They have low ionization
energies and high conductivity.
Lanthanides are a family of rare earth
metals that contain one valence electron in
the 5d shell. They are highly reactive and a
strong reducing agent in reactions.
Actinides are another family of rare earth
metals. Like the lanthanides, these
elements are highly reactive.

11. Metals, Non-metal, Metalloids
Metal
(Physical
Properties)
-Luster
-Malleable
-Ductility
-Hardness
(Chemical
Properties)
-Electropositive
Character
-tend to lose an
electron and
become positively
charged.
Non-metal
(Physical Properties)
-Non-malleable and ductile
-Luster
(Chemical Properties)
-Electronegative Character
-tend to acquire and
become negatively charged.
Metalloids
-the intermediate of metal
and non-metal.

12. The Periodic Trends

13. Metallic and Non-Metallic Character
Metallic character is strongest
for the elements in the leftmost
part of the periodic table and
tends to decrease as we move
to the right in any period.
Non metallic character
increases bottom to top and left
to right with the most nonmetal
element in the top right corner.

14. Atomic Radius and Atomic Size
Measure the distance between
the nuclei of two identical
atoms bonded together and
divide the distance by 2.
Atomic size is the distance
between the centre of the
nucleus of an atom and its
outermost shell.

16. Ionization Energy and Electron Affinity
The energy required
to remove one
electron from the
outer shell of a
neutral atom.
The energy change
that occurs when a
neutral atom gains
an electron.

18. Electronegativity
Measures the ability of
an atom in a chemical
compound to attract
electrons from another
atom in the compound.

19. Reactivity describes the ability of a molecule or atom
to undergo a chemical reaction, followed by a release
in energy. This property is dependent on
characteristics such as electronegativity and ionization
energy. These are factors that affect the interactions of
electrons that chemical reactions undergo. Reactivity
is dependent on the classification of an element
(metals and non-metals), as they both have differing
periodic trends. The reactivity of metals increases
further left along a period, and further down a group.
On the other hand, reactivity in non-metals increase
further right down a period, and further up a group.
The most highly reactive element to be observed is
cesium, as it spontaneously reacts with air and water!