THE ATOM AND THE PERIODIC TABLE

STATE STANDARD

SPI 0807.9.9 Use the periodic table to determine the properties of an element.

OBJECTIVES

I can identify the parts of an atom I can compare and contrast the relative masses of the

different parts of an atom I can calculate atomic mass

REPRESENTATION OF AN ATOM

ELEMENT TILE

STATE STANDARD

SPI 0807.9.9 Use the periodic table to determine the properties of an element.

OBJECTIVES

I can calculate atomic mass correctly 8 out of 10

Calculating Atomic Mass

APEAtomic# = #of Protons = #of Electrons

For Oxygen, O, the atomic # is 8

So, O has 8 Protons and 8 Electrons.

Calculating Atomic Mass

MAN (Mass #)- (Atomic#)= ( # of Neutrons)

Calculating Atomic Mass

Oxygen has an Atomic # of 8Therefore O has: 8 Protons 8 Electrons

To calculate # of Neutrons: First round the atomic

mass from 15.99 to 16 Then subtract the

number of Protons.

16 Mass # - 8 Atomic # 8 # Neutrons

ISOTOPES

ISOTOPES are atoms that have the same number of protons but different number of neutrons.

ISOTOPES

Isotopes of an element share the same chemical properties and most of the same physical properties.

STATE STANDARD

SPI 0807.9.9 Use the periodic table to determine the properties of an element.

OBJECTIVE

I CAN ACCURATELY DRAW THE BOHR ATOMIC MODEL FOR THE FIRST 20 ELEMENTS

BOHR’S MODEL OF THE ATOM

Niels Bohr (1913): studied the light produced when atoms were excited by heat or electricity.

Bohr proposed that electrons are in orbits & when excited jump to a higher orbit. When they fall back to the original they give off light.

BOHR’S MODEL OF THE ATOM

BOHR’S MODEL OF THE ATOM

BOHR’S ATOMIC MODEL

Bohr's model: -electrons orbit the nucleus like planets orbit the sun

Each orbit can hold a specific maximum number of electronsORBIT (n) MAX # OF

ELECTRONS1 22 83 184 32

BOHR ATOMIC MODEL FOR NEON