THE ATOM AND THE PERIODIC TABLE

STATE STANDARD  SPI 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 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 APE Atomic# = #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 8 Therefore O has:  8 Protons  8 Electrons To calculate # of Neutrons:  First round the atomic mass from 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 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 ATOMIC MODEL  Bohr's model: -electrons orbit the nucleus like planets orbit the sun  Each orbit can hold a specific maximum number of electrons ORBIT (n)MAX # OF ELECTRONS

BOHR ATOMIC MODEL FOR NEON