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PERIODIC TABLE
&
ELECTRON CONFIGURATION
Creator of the MODERN Periodic Table
1834 – 1907
Russian scientist
Arranged all of the 63 known elements by their atomic weights
Organized elements into groups possessing similar properties
Left gaps for undiscovered elements predicted a new element would one day be found and deduced its properties.
Group
– column of elements with similar properties.
**8 groups
valence electrons
electrons on the outside ring of the Bohr model
Period
– horizontal row of elements
**7 periods
Same number of
VALENCE electrons
Same number of
electron rings
The stair case or zigzag separates the metals from the nonmetals.
Metals = LEFT of the staircase
Nonmetals = RIGHT of the staircase
Metalloids = located on the staircase
Hydrogen is the exception to the rule
nonmetal on the metal side of the table
Metal ◦ High luster – shiny ◦ Malleable – able to be flattened into sheets ◦ Electronically conductive
Nonmetal ◦ No luster – not shiny ◦ Not conductive ◦ Brittle – breaks apart easily
Metalloids ◦ Elements with the properties of metals and nonmetals ◦ On the staircase
GROUP # NAME # of Valence
Electrons
1 Alkali Metals 1
2 Alkaline Earth Metals 2
3 The Boron Group 3
4 The Carbon Group 4
5 The Nitrogen Group 5
6 The Oxygen Group 6
7 Halogens 7
8 Nobel Gases 8 (except He)
Valence electron
electrons on the outer ring
of an atom
Alkali Metals
Alkaline Earth Metals
Halogens
Nobel Gases
metalloids
Transition Metals
Rare Earth Metals
A statement of where the electrons are on the energy levels (electron rings) in an atom.
Used mathematics to calculate probability of finding electrons within an atom
Called the dense area where electrons have the highest probability the ELECTRON CLOUD
Used to mathematically calculate the positions of electrons within the atom
From Schrodinger’s Equation, four quantum numbers were derived
quantum numbers = describe location of e-
n
◦ principal quantum number
◦ energy level 1-7
FLOOR
l
◦ 2nd quantum number
◦ Sublevel – s, p, d, f, g, h, i
ROOM
m
◦ 3rd quantum number
◦ Orientation in space – which axis it is rotating about (x, y, z)
DESK
s
◦ 4th quantum number
◦ spin – clockwise / counterclockwise
POSITION
No two electrons can have the same set of quantum numbers
The electrons cannot occupy the same space
electron
neutron
proton
•The maximum number of electrons that can fit on an energy level = 2n2
nucleus
1 2 3 4 5 6 7
TOTAL #
of electrons
Ground state -- the lowest possible energy level for an electron
Excited state -- when an electron absorbs energy, and it jumps to a higher level.
Quantum – packet of energy needed for an electron to jump to the next energy level
Photon – energy given off by an electron returning to ground state
Putting energy into the atom moves the electron away from the nucleus ◦ ground state excited state
When the electron returns to ground state it gives off energy light
When electrons absorb or release energy they do so in the one of the forms of energy from the electromagnetic spectrum
The range of frequencies present in light.
White light has a continuous spectrum ALL the colors are possible
rainbow = ROYGBIV RED – ORANGE – YELLOW – GREEN – BLUE – INDIGO - VIOLET
When electrons jump, they only do so in certain ranges
n = 3
n = 4
n = 2
n = 1
Look at the picture and decide if the electron absorbed or released energy
1.
2.
3.