Periodic Table Notes
Name _____________________________________
4.1, 4.2, 4.3
Period ________ Date _______________________
4-1: Development of the Periodic Table
1) History of the Periodic Table – By the end of the 1700’ scientists had identified only 30 elements
(ex. Cu, Ag, Au, H2, N2, O2, C). By the mid 1800’s by using
spectroscopy additional elements were identified by using their line
spectra and about 65 elements had been identified.
A. J.W. Dobereiner: Organized the elements into ______________ with similar _____________.
He called these groups ________________.
The middle element is often the
____________________ of the other two.
Ex)
B. J.A.R. Newlands: Law of _______________________.
He said properties repeated every
_________________ element.
C. Mendeleev:
1. Organized the 1st periodic table according to increasing ________________________
and put elements with similar properties in the same ___________________.
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2. He rearranged some elements out of atomic mass _______________ to keep them
together with other elements with similar _____________________. He also left
three ________________ in his table and correctly __________________ the properties
of these 3 unidentified elements that were later identified and matched his predictions.
D. Moseley: Each element has a certain amount of positive charge in the nucleus which are
called _________________.
1. Moseley reorganized the periodic table by _________________ __________________.
2. The Periodic Law:
When elements are arranged in order of increasing _______________
___________________, their physical and chemical ________________________
show a ________________________ pattern.
4-2: Reading the Periodic Table
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A. Information in each square:
Al
Aluminum
26.9815
B. Organizing the Squares
1. Vertical Columns –
2. Horizontal Rows –
C. Electron Configuration & Families
1. Valence electrons - _____________________ electrons responsible for bonding.
2. Elements in the same ____________ have the same number of valence electrons.
D. Family Names – See colored periodic table
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E. Metal, Nonmetals, and Metalloids (Semimetals):
1. Metals
2. Nonmetals
3. Metalloids
4-3: Trends in the Periodic Table
A. Atomic Radius
1. The distance from ________________________________________________
____________________________________________________________
2. Atoms get ______________________ going down a group and
______________________ going across a period.
Ex)
B. Ionic Size
1. When atoms _________ electrons, they become _______ and get _______________.
2. When atoms _________ electrons, they become _______ and get _______________.
3. Ions get _____________________ as you go down a group.
Ex)
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C. Ionization Energy:
1. The energy need to __________________ one electron from an atom.
2. Elements that do not want to lose their electrons have ______________ ionization
energies.
3. Elements that easily lose electrons have ___________ ionization energies.
4. I.E. _____________________ down a group. (opposite of atomic radius)
5. I.E. _____________________across a period. (opposite of atomic radius)
Ex)
D. Successive Ionization Energies:
1. Energy required to ___________________ electrons beyond the 1st electron.
2. Ionization energies will _______________ for every electron removed.
3. Na [Ne]3s1
Na•
1st = ______ kJ
4. Mg [Ne]3s2
Mg:
1st = ______ kJ 2nd = ______ kJ 3rd = ______kJ
5. Al [Ne]3s23p1
2nd = ______ kJ
Al: 1st = _____kJ 2nd = _____kJ 3rd = _____kJ 4th = _____kJ
E. Electron Affinity:
1. Energy change that occurs when an atom ___________ an electron.
2. A highly __________________ electron affinity attracts electrons. (nonmetals)
3. A __________________ electron affinity does not attract electrons. (metals)
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F. Electronegativity:
1. Reflects an atom’s ability to _______________ electrons in a chemical bond.
2. E.N. ____________________ going down a group.
6. E.N. ___________________ going across a period.
7. Examples: NaCl and H2
G. Octet Rule:
1. An atom will tend to ______________, ______________ or _______________
electrons in order to acquire a full set of valence electrons.
2. “Octet” = 8 = s2p6 configuration
H. Oxidation Number:
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