Chapter%203Chemical%20Periodicity%20and%20The%20Formation%20of%20Simple%20Compounds

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Chapter 3 Chemical Periodicity and The Formation
of Simple Compounds 3.1 Groups of
Elements 3.2 The Periodic Table 3.3 Ions and
Ionic Compounds 3.4 Covalent Bonding and Lewis
Structures 3.5 Drawing Lewis Structures 3.6 Nami
ng Compounds in Which Covalent Bonding
Occurs 3.7 The Shapes of Molecules 3.8 Elements
Forming More than One Ion Topics to be
emphasized in Exam 1
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Chapter 3 Chemical Periodicity. Formation of
Simple Compounds. Molecular Structure. Section
3.2 The Periodic Table Section 3.3 Covalent
Bonding Section 3.3 Lewis Structures Section
3.4 Shapes of Molecules
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• Section 3.2 Periodic Table
• Classic exemplar of the scientific process
  Mendeleev
• Atomic mass and atomic number as atom identifiers
• Periodic properties along rows and down columns
• Electronegativity (ability of an atom to hold
  electrons)
• Chemical reactivity (kinds of reactions atoms
  undergo)
• Valence (the number of bonds to other atoms)
• (4) Underlying structure of the Periodic Table is
  the electronic structure of atoms not their
  masses.

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Dmitri Mendeleev
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Biological Periodic Table http//umbbd.ahc.umn.ed
u/periodic/spiral.html
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Alternate forms of the periodic table
http//www.wou.edu/las/physci/ch412/alttable.htm
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• The Periodic Table
• The chemical and physical properties of the
  element are periodic functions of their atomic
  masses.
• The chemical and physical properties of the
  elements are periodic functions of the atom
  number (number of protons in the nucleus number
  of electrons in the neutral atom).
• The elements can be arranged in groups (columns)
  of elements that possess related chemical and
  physical properties.
• (4) The elements can be arranged in periods
  (rows) of elements that possess progressively
  different physical and chemical properties.

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The Table by groups
I II
III IV V VI VII VIII
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Groups of Elements in the Periodic Table Eight
Groups (the representative elements) I. Alkali
metals (H), Li, Na, K, Rb, Cs II. Alkali earth
metals Be, Al, Ca, Sr, Ba, Ra III. Boron
family B, Al, Ga, In, Tl IV. Carbon family C,
Si, Ge, Sn, Pb V. Nitrogen family N, P, As, Sb,
Bi VI. Chalcogens O, S, Se, Te,
Po VII. Halogens F, Cl, Br, I, At VIII. Noble
gases (He), Ne, Ar, Kr, Xe, Rn
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The Table by kinds of elements
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The Table by sizes of atoms
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The Table by atomic radius
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The connection between the Periodic Table and
atomic structure. Valence electrons The
electrons which are furthest from the positive
nucleus and are most loosely held. These
electrons determine chemical properties of
elements and molecules. Periodic Table The
group number of the group of a column for the
main group elements in the periodic table is the
number of valence electrons possessed by the
neutral atom atomic number number of protons
in the nucleus of an atom. Group number (GN for
main group elements) number of valence
electrons Valence electrons for elements
1-18 I II III IV V VI VII VIII 1H 2He 3Li
4Be 5B 6C 7N 8O 9F 10Ne 11Na 12Mg 13Al 14Si 15P
16S 17Cl 18Ar
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The Table by electron affinity (energy released
when an electron is added to an atom
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Electronegativity and electron affinity are two
key features which determine the nature of the
chemical bond. More later.