Objectives: to learn about atomic structure: 1) how the elements are organized
2)
basic atomic structure
3)
how the structure of atoms differ
Periodic Table
·
Symbols & elements
·
Groups and periods of elements
·
Metals vs. non-metals
Organization of the Periodic Table
·
Groups of elements (families)
·
Periods of elements (series)
Groups of Elements (families)
·
Column of elements on the tables
·
Members have similar physical & chemical
properties
Periods of Elements (series)
·
Rows of elements
·
Members have electrons in the same valence shell
-Metals
·
Good conductors of heat & electricity
·
Ductile- can be drawn into wires
·
Malleable-pounded into shapes
·
Lustrous- reflect light
·
Form “+” ions
·
Contain a metallic bond
·
“sea” of de-localized electrons
·
Examples: Ag, Fe, Hg, Ti, Pb
-Non-metals
·
Poor conductors “insulators”
·
Brittle
·
Dull
·
Form “-“ ions
·
Examples: Se, P, C, I, Br
-Metalloids
·
Have properties of both metals and non-metals
·
Semi-conductors
·
Examples: B, Te, Ge, As, Si
Relation to the Periodic Table
·
Atomic number (Z)
·
Number of protons in an atom whole number on the
periodic table
·
Mass number (Mn)
o
Mn= P+ + N°
o
Integer closest to atomic mass is protons +
neutrons
·
Atomic Mass
o
Relative mass of the atom (the other number on
the periodic table)
·
Isotopes
o
Atom of same elements with a different number of
neutrons in a nucleus (2 or more atoms)
§
Protium: Hydrogen-1
§
Daterium: Hydrogen-2
§
Tritium: Hydrogen- 3
o
The number stands for the mass number of the
isotopes
|
Isotopes
|
Protons
|
Neutrons
|
Electrons
|
|
Hydrogen-1
|
1
|
0
|
1
|
|
Hydrogen-2
|
1
|
1
|
1
|
|
Hydrogen-3
|
1
|
2
|
1
|
Assuming neutral atoms protons=electrons
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