the periodic table - welcome students · intro to the periodic table ... developed a version of the...
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The Periodic Table
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Intro to the Periodic Table
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Intro to the Periodic Table
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Intro to the Periodic Table
Dobereiner:
Developed ‘triads’ that
groups elements based on
common characteristics.
No arrangement between
triads, however.
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Dmitri Mendeleev
Mendeleev:
Developed a version of the periodic table of elements that reflected patterns and properties.
Biggest contribution: leaving blank spaces predicting elements (and their properties) that had yet to be discovered!
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Intro to the Periodic Table
In 1913 Henry Mosely (along with Rutherford)discovered the idea of positive charge within thenucleus. Discovered each element had a certain
amount of positive charge in the center. Called these whole number positive charges
atomic number. Determined the atomic number of all known
elements at that time.
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B. Moseley
Mosely: Arranged the periodic table in order of
increasing atomic number.
- This is the way the table is
currently arranged.
- Remember # of protons =
atomic #
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Intro to the Periodic Table
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Periodic Law: The properties of elements are
periodic – that is a repeating pattern of chemical
and physical properties. (they repeat in a
systematic way)
Key Idea
For example, which elements are similar to sodium?
Elements in the same group have similar properties.
This is because they have the same # of valence
electrons!
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Intro to the Periodic Table
Valence Electrons:
Outermost electrons in an atom (responsible for
properties of an element).
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Intro to the Periodic Table
Example: State the valence electrons for the
Following elements.# of valence electrons
Li Mg Al O Cl Ne
Lewis Dot Diagram
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Periodic TrendsValence electrons and group properties:Each element in a group has similar properties, due to all members
having the same number of valence electrons.
Metals: Nonmetals:
Form (+) ions Form (-) ions
Lose electrons Gain electrons
Group 1 Group 2 Groups 3-12 Group 13 Group 14 Group 15 Group 16 Group 17 Group 18
1 Valence Electron
2 Valence Electrons
Varies 3 Valence Electrons
4 Valence Electrons
5 Valence Electrons
6 Valence Electrons
7 Valence Electrons
8 Valence Electrons
+1+2 Varies +3 +/- 4 -3 -2 -1 No Ions
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Ever wonder what people who like science and
music do in their spare time?
https://www.youtube.com/watch?v=VgVQKCcfwnU
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Groups of the Periodic Table
http://periodictable.com/index.html
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Groups of the Periodic Table
Hydrogen:
Has 1 valence electron, so it
is placed with
group1 but it is NOT a
metal. One of the more
common elements in the
universe.
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Groups of the Periodic Table
Alkali Metals:
Very reactive, explosive metals (often grey, soft).
1 valence electron and forms +1 ions.
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Alkali Metal Reactivity
Reactivity with air & water:
http://www.youtube.com/watch?v=uixxJtJPVXk&safety_mode=true&persist_safety_mode=1&safe=active
Brainiac’s play with alkali metals:
http://www.youtube.com/watch?v=m55kgyApYrY&safety_mode=true&persist_safety_mode=1&safe=active
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Groups on the Periodic Table
Alkaline Earth Metals:
Reactive metals, tend to be found in compounds
in nature. 2 valence electrons and forms +2 ions.
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Groups on the Periodic Table
Transition Metals:
Stable metals. Can form
more than one (+) ion
b/c they can change the #
of electrons lost. They
form colorful (+) ions
when in a solution.
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Groups on the Periodic Table
Lanthanide Series:
4f block of elements
Actinide Series: 5f block of
elements. Almost all
are man-made, all are
radioactive.
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Groups of the Periodic Table
Halogens:
Reactive nonmetals.
Group contains all 3 states
of matter (s,l,g). Mainly
form -1 ions b/c they
only need 1 valence
electron to achieve octet.
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Reactivity of Halogens:
http://www.youtube.com/watch?v=u2ogMUDBaf4
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Groups of the Periodic Table
Noble Gases:
Stable valence electron configuration, which
means they are nonreactive – they have a full
octet (remember that # is 2 for He, but 8 for the
rest of the group.)
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Group 13
+3 Ion
Group 14
+/- 4 Ion
Group 15
-3 Ion
Group 16
-2 Ion
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Groups of the Periodic Table
Metals SemimetalsMetalloids
Nonmetals
Malleable, ductileShiny (luster)Lose electrons = (+) ionsGood conductorsOnly liquid: Hg (rest are solid)
7 total (on step line)B, Si, Ge, As, Sb, Te, At
Properties are in between metals and nonmetals
BrittleNonconductorsGases, liquid (Br), and solidsGain electrons = (-) ions
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The Octet Rule:
Atoms will lose, gain or
share electrons to achieve
stability – a full octet of 8
valence electrons.
Metals accomplish this by
losing electrons.
Nonmetals gain electrons
to fill the valence shell.
Exception: 1st PEL only
holds 2 electrons.
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As you move across a period:
- # of PEL’s stays the same
- # of protons increases
- # of e- in the valence shell increases
which increases attraction.
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Coulombic attraction increases b/c
atomic radius decreases.
As you move across a period the # of
protons increases & the # of e- in the
valence shell increases, which
increases attraction.
Coulo
mbic
att
ract
ion d
ecre
ases
b/c
ato
mic
rad
ius
incr
ease
s. I
ncr
ease
in #
of
PE
L’s
cau
ses
e-to
be
fart
her
fro
m
the
nucl
eus
dec
reas
ing a
ttra
ctio
n.
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Coulo
mbic attractio
n in
creases b/c
atom
ic radiu
s decreases.
As y
ou m
ove acro
ss a perio
d th
e # o
f
pro
tons in
creases & th
e # o
f e-in
the
valen
ce shell in
creases, which
increases attractio
n.
Coulombic attraction decreases b/c
atomic radius increases. Increase in #
of PEL’s causes e- to be farther from
the nucleus decreasing attraction.
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Periodic TrendsPeriodic Trends:
Predictable patterns across the periodic table
(atomic radius, metallic character, ionization
energy, electronegativity) and down the groups.
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Atomic Radius:
Across a period:
Get Smaller
Down a group:
Get Larger
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Metallic Character:
How much an atom acts
metallic – i.e. how easily it
loses electrons.
Across a period:
Decreases ( you are heading
towards the nonmetals)
Down a group:
Increases (easier to lose an
electron if the atom is
bigger).
* Most metallic elements are in the lower left corner.
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+ ion:
Loss of an electron
reduces the electron cloud
size. Radius decreases.
- ion:
Gain of an electron
increases electron cloud
size. Radius increase.
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Ionization Energy:
Energy to remove
outermost electron
Across a period:
Increase
Down a group:
Decrease
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Electronegativity:
Ability to attract an electron
(“affinity for electrons”)
Across a period:
Increase
Down a group:
Decrease
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