2. Warm Up Activity
• Provide the Electron Configurations for the
following elements:
– H
– Li
– Na
– K
– Rb
– Cs
– Fr
• Do you notice any patterns/trends/similarities in
their electron configurations?
• Do you notice any patterns/trends/similarities in
their location on the periodic table?
3. Periodicity
• Periodicity: Refers to the inherent reoccurring
nature of certain properties within the elements
at specific predictable intervals.
• There are repeating patterns within the elements.
• Certain elements have many properties in
common and can be grouped together into
specific families.
• Has Everything to do with the number and
location of electrons.
4. The Periodic Table
• The periodic table is a invaluable tool that
arranges the elements in a very specific way.
• It groups “like” elements together by their
properties.
• The periodic table has a number of trends
within in it.
• ESSENTIAL organizational tool for chemists
5. Early Attempts
• Believe it or not chemists did not immediately
stumble upon the current periodic table.
– There were many many attempts at creating a
working model, that met with varying degrees of
success, before the modern periodic table we all
recognize was developed.
10. Mendeleev
• Our modern periodic table is based
on the work of Dimitri Mendeleev
who was the first scientist to publish
an functioning organized table of the
known elements.
• Based his table on 2 factors:
similarities in chemical and physical
properties and atomic mass.
• Mendeleev even went out on a limb
and predicted the properties of 2 at
the time undiscovered elements.
• He was very accurate in his
predictions, which led the world to
accept his ideas about periodicity
and a logical periodic table.
11. “Periodic Law”
• Mendeleev’s Table was very
good but not perfect.
• Moseley proposed the idea of
a Periodic Law which states:
– When arranged by increasing
atomic number, the chemical
elements display a regular and
repeating pattern of chemical
and physical properties.
– Focuses on atomic number
instead of atomic mass
12. The Periodic Law
• The periodic table organizes the elements into
Groups/Families and Periods.
• Groups or Families: Atoms with similar properties
appear in vertical columns on the periodic table.
– We now know they are similar because they all have
the same number of valence (outer shell) electrons,
which governs their chemical behavior.
• Periods: Contain elements within the same
energy level or shell.
– The elements within a period all have the same n
(Primary Quantum Number).
14. Periodic Table
e- configuration from the periodic periodic table
1 18
IA VIIIA
2 13 14 15 16 17
1 H IIA IIIA IVA VA VIA VIIA He
1s1 1s2
2 Li Be B •B
C N O F Ne
•2p2 1 2p3 2p5
2s1 2s2 2p1 2p 2p4 2p6
Na Mg 3 4 5 6 7 8 9 10 11 12
3 IIIB IVB VB VIB VIIB VIIIB IB IIB Al Si P S Cl Ar
3s1 3s2 3p1 3p2 3p 3 3p4 3p5 3p6
4 K Ca Sc Ti V Cr Mn Fe Co Ni Cu Zn Ga Ge As Se Be Kr
4s1 4s2 3d1 3d2 3d3 4s13d5 3d5 3d6 3d7 3d8 4s13d10 3d10 4p1 4p2 4p3 4p4 4p5 4p6
5 Rb Sr Y Zr Nb Mo Tc Ru Rh Ni Ag Cd In Sn Sb Te I Xe
5s1 5s2 4d1 4d2 4d3 5s14d5 4d5 4d6 4d7 4d8 5s14d10 4d 10
5p1 5p2 5p3 5p4 5p5 5p6
6 Cs Ba La Hf Ta W Re Os Ir Ni Au Hg Tl Pb Bi Po At Rn
6s1 6s2 5d1 5d2 5d3 6s15d5 5d5 5d6 7
5d 5d8 6s15d10 5d10 6p1 6p2 6p3 6p4 6p5 6p6
7 Fr Ra Ac Rf Db Sg Bh Hs Mt
7s1 7s2 6d1 6d2 6d3 7s16d5 6d5 6d6 6d7
16. Major Categories
• Metals: are conductors of heat and
electricity, lustrous (shiny), malleable,
ductile, and generally solid.
• Nonmetals: may be solids, liquids, or
gases, and are poor conductors of heat
and electricity. When solids, they are
brittle, non-lustrous materials.
• Metalloids: are solids at standard
conditions, and are semiconductors of
electricity, making them handy for use in
the electronics field. Metalloids have
properties between that of metals and
nonmetals, causing them to have the
nickname of "semimetals."
17. Location on Periodic Table
• The periodic table tells you
where the metallic,
nonmetallic, and
semimetallic elements are.
• Look for the line that looks
like a staircase.
– Elements left of this line are
metals.
– Elements to the far right of
this line are nonmetals
– Elements touching the line
on either side are
semimetals, or metalloids
19. Other Locations
• Main block elements: These are the s- and p-
sections of the periodic table (groups 1,2, 13-18)
• Transition elements: These are the elements in
•
the d- and f-blocks of the periodic table.
– The term “transition element”, while technically
referring to the d- and f-blocks, usually refers only to
•
the d-block.
– Technically, the d-block elements are the “outer
•
transition elements”
– Technically, the f-block elements are the “inner
transition elements”
20. Group 1: Alkali Metals
All Alkali Metals have 1 Valence
Electron.
Highly Reactive!
• Alkali metals are NEVER found pure in
nature; they are too reactive.
Potassium, K
Flammable in air and water. reacts with water
Reactivity of these elements and must be
stored in
increases down the group. kerosene
Low melting (MP of Li = 181° C, Na
= 98° C) and Boiling Points.
They are light, low-density (Li =
0.535, Na = 0.968 g/ml), soft
metals.
21. Group 2: Alkaline Earth Metals
• All alkaline earth metals have 2 valence electrons
• They are also reactive, but less so than the alkali metals.
• They are light, soft metals, but stronger and denser than
the alkali metals. (Density of Ca = 1.55, Mg = 1.74 g/ml).
• Alkaline earth metals are not found pure in nature; they
are too reactive.
• Low MP and BP, but higher than alkali metals (MP of Ba=
302 °C, Mg = 649 °C)
• The word “alkaline” means “basic”
– common bases include salts of the metals
• Ca(OH)2
• Mg(OH)2
22. Groups 3-12: Transition
Metals
They are less reactive than
the alkali and alkaline earth
metals, but vary greatly
among themselves in
reactivity- generally stable.
Most are hard solids with
high melting and boiling
points. (Fe = 1535° C, Ti =
1660° C).
Typically High density (Fe =
7.87, Ir = 22.4 g/ml)
Share many of the general Copper, Cu, is a
relatively soft Mercury, Hg, is the
characteristics of all metals metal, and a very only metal that
good electrical exists as a liquid at
conductor. room temperature
23. Inner Transition Metals
• Lanthanides (4f section)
•
– Also called the rare earth metals, because they’re rare.
– Usually intermediate in reactivity between alkaline earth metals and transition
metals.
– High MP and BP
– Used in light bulbs and TV screens as phosphors.
• Actinides (5f section)
•
– Many have high densities
– Most are radioactive and manmade
– Melting points vary, but usually higher than alkaline earth metals.
– Reactivity varies greatly
– Used for nuclear power/weapons, radiation therapy, fire alarms.
24. Properties of
Metalloids
They have properties of
both metals and nonmetals.
Metalloids are more brittle
than metals, less brittle than
most nonmetallic solids
Metalloids are
semiconductors of electricity
Some metalloids possess
metallic luster
25. Nonmetals
Nonmetals are poor
conductors of heat and
electricity
Nonmetals tend to be
brittle
Many nonmetals are gases
at room temperature
Carbon, the graphite in “pencil
lead” is a great example of a
nonmetallic element.
26. Group 17: Halogens
Halogens all have 7 valence electrons.
These elements are highly reactive.
Halogens are never found pure in nature; they
are too reactive.
Highly volatile – F and Cl are gases, Br is a
volatile liquid, and I is an easily sublimed solid.
Strong oxidizers – they readily pull electrons
from other atoms.
All are also extremely dangerous, especially
when inhaled.
Halogens in their pure form are diatomic
molecules (F2, Cl2, Br2, and I2)
Chlorine is a yellow-green
poisonous gas
27. Group 18: Noble Gases
Have full electron shells
Noble gases have 8 valence electrons
(except helium, which has only 2)
Noble gases are ONLY found pure in nature
– they are chemically unreactive.
Colorless, odorless, and unreactive; they
were among the last of the natural
elements to be discovered
Used to provide the atmosphere in
situations where you don’t want chemical
reactions to occur (light bulbs, glove boxes,
etc).
28. Hydrogen
• Hydrogen – “The Weirdo”
•
– Has properties unlike any
other element
– Diatomic – H2
– Can form either a +1 or -1
charge
– Relatively unreactive
unless energy is added
(under most conditions) –
it can form explosive
mixtures with oxygen (as it
did in the Hindenburg
explosion)
