Periodic Table-Chapter 6
Resources and Activities
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Good video song and animation Periodic table:
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http://www.youtube.com/watch?v=zGMwSKFBpo&feature=related
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Animations – metal character, ionization
energy and metal reactivity
Reaction of Alkali Metals with Water
Brainiac Videos on You Tube:
http://www.youtube.com/watch?v=m55kgyAp
YrY
•
TB and Chapter 6 reading and study guide
•
Dynamic periodic Table:
http://www.ptable.com/
•
What can you discover and conclude about
periodic trends ?
•
Regents reference tables- S and Periodic Table
and table S
•
Periodic Table Lab Activities
•
(1) Color Coded Periodic Table
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(2) POGIL on Periodicity of Elements
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What do the elements look like?
http://www.periodictable.com/
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(3) Graphing of Periodic Properties versus
Atomic Number – “Periodic Trends-Student
Sheet”
(4) “Overview of Periodic Properties”
Dmitri Mendeleev
(1869)
In 1869 Mendeleev and Lothar Meyer (Germany)
published nearly identical classification schemes for
elements known to date. The periodic table is base
on the similarity of properties and reactivities
exhibited by certain elements. Later, Henri Moseley
( England,1887-1915) established that each elements
has a unique atomic number, which is how the
current periodic table is organized.
http://www.chem.msu.su/eng/misc/mendeleev/welcome.html
Periodic Table- Historical Development
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Dmitri Mendeleev’s Periodic Table (late 1800’s)
Elements were arranged according to increasing
atomic mass. Other chemists? Lothar Meyer
He predicted the physical and chemical properties of
missing elements by averaging the properties of the
known elements.
Henry Moseley – in 1913 he determined the nuclear
charge (atomic number of the element). He
arranged the periodic table by order of increasing
atomic number.
Periodic law states that when the elements are
arranged by atomic number, their physical and
chemical properties vary periodically.
Modern Periodic Table
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Modern periodic Table is organized based on atomic number
of the elements and their chemical properties
Vertical columns – groups or families
 similar chemical and physical properties
 Same number of valence electrons
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Valence Electrons are the electrons in the highest occupied
energy level of an element’s atom; outer-most electrons
Valence electrons determine the chemical properties of the
element.
7 horizontal rows – periods – contain elements with valence
electrons in the same principle energy level
 Properties within a period change
Characteristics of Metals, Nonmetals, and Metalloids
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Metals are good conductors of heat
and electricity, are malleable, ductile,
and make up most of the periodic
table. They also have luster. Most
metals are solids are room temp
(except Hg which is a liquid).
Metals have low ionization energies
and electronegativities. Metals tend to
lose electrons to form positive ions
(cations) with smaller radii. Metallic
character increases as you go down
(descend) the group 1 alkali metals
and the group 2 alkaline earth metals.
Francium and Cesium are highly
reactive metals.
Reaction of Alkali Metals with Water
Brainiac Videos on You Tube:
http://www.youtube.com/watch?v=m
55kgyApYrY
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Nonmetals are found in upper right
hand corner of the periodic table. They
can be gases or molecular or network
solids at room temperature (bromine is
an exception and is a liquid at room
temperature). They are poor
conductors, dull, brittle; only carbon
(graphite) conducts.
Nonmetals have high ionization
energies and high electronegativities.
Nonmetals tend to gain electrons to
become negative ions with larger radii
than their atoms. Fluorine is a highly
reactive nonmetal.
Metalloids– have properties that
are similar to metals and nonmetals;
found along the diagonal (ex:Si,Ge)
Noble Gases or Inert Gases- Group
18, are chemically inert (with some
rare exception).
Reading the Periodic Table: Classification
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Nonmetals, Metals, Metalloids, Noble gases
Periodic Table trends and Metallic character
Metallic Character
Elements with low ionization energies
tend to be metals. Those with high
ionization energies tend to be nonmetals.
This can vary within a group as well as
within a period.
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Periodic Table
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Group 1 – Alkali Metals, most reactive metals (one valence electron).
Groups with either nearly empty or nearly full valence shells tend to
be particularly reactive. Group 2 - Alkaline Earth Metals, second most
reactive group of metals (2 valence electrons)
Note that Hydrogen is a Non metal and is NOT an alkali metal.
Group 17 – Halogens, F, Cl, Br, I, most reactive nonmetals (recall groups with either nearly empty or nearly full valence shells tend to
be particularly reactive). Group 17 : Halogens (have 7 valence
electrons), are the most reactive nonmetals; undergo chemical
reactions to gain 1 e- to get to a Noble gas configuration.
Video of reaction of chlorine gas with sodium metal
http://jchemed.chem.wisc.edu/jcesoft/cca/cca0/movies/nacl1.html
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Group 18 – Noble Gases, Inert, Ne, Ar, Kr, Xe, He,
Periodic Table
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s block : Groups 1,2 and He
p block : Groups 13-18 Main Group Elements
d block: Transition Elements – outermost electrons
are in the d orbitals. (d block metals; the d orbitals
have a numeric label that is 1 less than the period
number . Example:
Electron configuration of elements
Dynamic periodic Table: http://www.ptable.com/
Ionization Energy of Elements
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The energy needed to remove an electron
from a gaseous atom is called the Ionization
Energy. Ex. K  K+ + eGroup Trends – Ionization Energy decreases as
you move down a group. Size of the atom
increases as you move down a group and the
valence electrons are further from the
nucleus, and therefore more weakly held (by
their attraction to the nucleus) and are easier
to remove
Periodic Table
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Electronegativity – is the tendency for atoms of
the element to attract electrons when they are
chemically combined with another element.
F has the highest electronegativity, Fr has the
lowest electronegativity and cesium has the next
lowest electronegativity.
Periodic Trends – Electronegativity increases
from left to right. Nonmetals attract electrons
Group Trends- Electronegativity increases from
bottom to top. F has the highest
electronegativity of the halogens.
Periodic Table
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Periodic trends in ionization energy- ionization increases as you
move from left to right across the period. As you move towards
the right, there is a greater attraction of the nucleus for its
outer electrons. Electrons are less likely to be lost.
Electrons in the outermost shell available to be lost, gained or
shared in the formation of chemical compounds are called
Valence electrons.
K  K+ + eCations are smaller than their neutral atoms, anions are larger
than their neutral atoms.
P. Table - Atomic Size/Atomic Radius
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Periodic Trends in Atomic Size – X-Ray diffraction is
used to determine size of solid atoms. Atomic Radius
– half the distance between the nuclei of two like
atoms.
Group Trends- Atomic size increases as you move
down a group on the periodic table. You add more
protons, neutrons, electrons, and energy levels
overall.
Atomic Size decreases as you move from left to right
across a period. As more electrons are added to
the same energy level, they are pulled in tighter to
the nucleus (with increasing nuclear charge).
Periodic Table (what about
transition elements?)
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Properties of the d-block elements vary with less
regularity than the main-group elements. Their
atomic radii generally decrease across a period.
Ionization Energy and electronegativity also shows
the same trends for the d-block.
D-block elements remove electrons from the outer s
shell before d electrons are removed from the outer
shell.
Copyright © Houghton Mifflin Company. All
8 | 15
Periodic Table-Chapter 6
Resources and Activities
•
Good video song and animation Periodic table:
•
http://www.youtube.com/watch?v=zGMwSKFBpo&feature=related
•
•
•
•
TB and Chapter 6 reading and study guide
WB – Periodic Table Unit for content and
practice problems
•
•
Dynamic periodic Table:
http://www.ptable.com/
•
•
Regents reference tables- S and Periodic Table
and table S
•
•
•
•
What do the elements look like?
http://www.periodictable.com/
•
Animations – metal character, ionization
energy and metal reactivity
Reaction of Alkali Metals with Water
Brainiac Videos on You Tube:
http://www.youtube.com/watch?v=m55
kgyApYrY
What can you discover and conclude
about periodic trends ?
Periodic Table Lab Activities
(1) Color Coded Periodic Table
(2) POGIL on Periodicity of Elements
(3) Graphing of Periodic Properties
versus Atomic Number – “Periodic
Trends-Student Sheet”
(4) “Overview of Periodic Properties”