Download Unit 4 - The Periodic Table

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UNIT
THE PERIODIC TABLE
(THESE ARE YOUR NOTES)
The PERIODIC TABLE is a chart that organizes all known elements into a grid of horizontal rows (periods) and
vertical columns (groups) arranged by increasing atomic number.
Periodic: appearing or occurring at regular intervals.
Periodic Law: The Periodic Law states that the physical and chemical properties of the
elements recur in a systematic and predictable way when the elements are arranged in order
of increasing atomic number.
Mendeleev: developed a periodic table in the 1870’s
He arranged the elements that were known at the time by increasing atomic mass.
He grouped elements together by similar properties.
Using his periodic table, he was able to predict the properties of unknown elements.
Groups: Vertical columns of elements on the periodic table.
Elements from the same group have the same number of valence electrons.
Elements from the same group will react similarly; an element from the same group
would be the best replacement for a given element in an experiment.
Periods: Horizontal rows of elements on the periodic table
Each period represents an added electron energy level
Definitions
IONIZATION ENERGY
The amount of energy needed to remove the outermost electron of an atom.
ELECTRONEGATIVITY
An atom’s ability to attract electrons to itself when bonded to another element.
Other Nonmetals
Other Nonmetals
Alkali Metals
Alkali Metals
Alkaline Earth
Metals
Alkaline
Earth Metals
Transition Transition
Metals Metals
Rare EarthInner
Metals
Transition Metals
Inner Transition
Other Nonmetals
Metals
Alkali Metals
Alkaline Earth Metals
Transition Metals
Rare Earth Metals
Other Nonmetals
Alkali Metals
Alkaline Earth Metals
Transition Metals
Rare Earth Metals
Other Nonmetals
Alkali Metals
Alkaline Earth Metals
Transition Metals
Rare Earth Metals
Other Nonmetals
Alkali Metals
Alkaline Earth Metals
Transition Metals
Rare Earth Metals
Noble Gases
Metalloids
Halogens
Other Metals
Stair-Step Line
Make sure you can identify the following sets of elements by their location on the Periodic Table!
1.
The Alkali Metals in Group 1 (1A on your periodic table)
2.
The Alkaline Earth Metals in Group 2 (2A on your periodic table)
3.
The Transition Metals in the d orbital block
4.
The Metalloids along the Stair-Step Line that divides Metals from Nonmetals
5.
The Halogens in Group 17 (7A on your periodic table)
6.
The Noble Gases in Group 18 (8A on your periodic table)
Noble Gases are extremely stable and generally nonreactive.
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Atomic Radius: Increases down and to the left on the periodic table
smallest
largest
As you go down a group (column), atomic radius INCREASES
The number of energy levels increases as you move down a group.
Each successive energy level is further from the nucleus than the last.
From Left to Right across a period (row), atomic radius DECREASES
As you go Left to Right across a period, each element has one more electron (-) in the
same energy level. Each element also has one more proton (+) in the nucleus.
The electrons are pulled closer to the nucleus which results in a smaller atomic radius.
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ION: an atom that has a negative or positive charge
an ion is an atom that has either gained or lost electrons
e-
e-
e-
Has a negatively charged ion lost electrons or gained electrons?
electrons have a
negative charge
Has a positively charged ion lost electrons or gained electrons?
Size of a Neutral Atom vs. Size of an Ion
The size of an atom will change as it gains or loses electrons to become an ion.
A negatively charged ion is called an Anion.
Negative ions (anions) are LARGER than their respective atoms.
Atom / Ion Size
A positively charged ion is called a Cation.
Positive ions (cations) are Smaller than their respective atoms.
Atom / Ion Size
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Ionization Energy
The amount of energy needed to remove the outermost electron of an atom.
Electronegativity
An atom’s ability to attract electrons to itself when bonded to another element.
Both Ionization Energy and Electronegativity
increase going up and to the right on the periodic table.
Fluorine has the
highest electronegativity
of all the elements
lowest
These are your UNIT 3 YELLOW NOTES. These are yours to keep.
They are NEVER DUE and are therefore never to be turned in.
You are to have these notes in class every day. Do not lose them.
This is an outline of the topics we are studying in this Unit.
The idea is that you will follow along as we discuss these topics
and YOU WILL TAKE YOUR OWN NOTES on this document.
THIS IS NOT MEANT TO BE A COMPLETE SET OF NOTES!
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Reactivity: the tendency of an element to react with other elements.
Reactivity increases going down for metals, but going up for nonmetals.
What is the most reactive metal?
What is the most reactive nonmetal?
This graph shows the ionization energies of the first 19 elements.
Ionization Energy
The amount of energy needed
to remove the outermost
electron of an atom.
He, Ne and Ar are much higher on the graph because it takes more energy to
remove an electron from these atoms (noble gasses are very stable).
Li, Na and K are much lower on the graph because they have a single valence
electron that is easier to remove.
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Yo, here is like everything!
Periodic Trends
Element Families
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