The Periodic Table By Ryan Schutte
Dec 22, 2015
The Periodic TableBy Ryan Schutte
Beginnings
Russian Chemist Dmitri Mendeleev produced the first periodic table of elements
He arranged them in order of increasing atomic mass and noticed a periodic repetition of their properties
Mendeleev knew he was not completely correct with his table and left blank spots showing places where he thought an undiscovered element existed
Mendeleev’s Table
What is the Periodic Table?
The Table of Elements is a display of the chemical elements organized on the basis of their properties and presented in increasing atomic number.
Periodic Law
When elements are arranged in order of increasing atomic number, their physical and chemical properties show a periodic pattern
Modern Periodic Table
Has 109 squares, each representing an element
Squares aligned in vertical columns called groups› Elements in these groups have similar
properties Horizontal groups are called periods The Periodic table has 7 periods and
18 labeled groups
Groups
Some groups are given family names Groups on at the far left and right of the periodic
table are very similar within their group and are commonly referred to by their family names
Examples are the alkali metals, alkaline earth metals, halogens, and the noble gases
Metals, Nonmetals, and Metalloids
Metals- on the left side of the table› share many properties and are
characterized by their luster or shine› Good conductors of heat and electricity› Typically solids and room temperature› Malleable and ductile
Metals, Nonmetals, Metalloids cont.
Nonmetals- right side of the table except hydrogen› Do not have metallic luster› Poor conductors of heat and electricity› Neither malleable or ductile› Many are gases at room temperature and
others are solids
Metals, Nonmetals, Metalloids cont.
Metalloids- have properties of metals and nonmetals
Located in between metals and nonmetals in a staircase pattern
Periodic Table Trends- Atomic Radius
Atomic Radius- distance from the center of an atom’s nucleus to its outermost electron
If you go down each group on the periodic table, the atomic radius increases
If you left to right across each period, the atomic radius decreases
Ionization Energy
The energy needed to remove one of its electrons
Think of it as how strongly an atom holds onto its electrons
High ionization energy means atoms hold onto their electrons very tightly
Ionization energy decreases as you go down a group
Increases as you move from left to right across a period
Electronegativity
Ability to attract electrons in a chemical bond
Increase as you move left to right across a period and decrease as you move down a group
GOOD LUCK