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.