Development of Atomic Models

Bohr's Model of the Atom

Bohr's Model of the Atom

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

Bohr's Model of the Atom

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

Rutherford's model couldn't explain why unique colours were obtained by atoms ofdifferent elements

Bohr's Model of the Atom

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

Rutherford's model couldn't explain why unique colours were obtained by atoms ofdifferent elements

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

Bohr's Model of the AtomBohr's model:-electrons orbit the nucleus like planets orbit the sun-each orbit can hold a specific maximum number of electrons

Bohr's Model of the AtomBohr's model:-electrons orbit the nucleus like planets orbit the sun-each orbit can hold a specific maximum number of electrons

orbitmaximum # electrons122838 4 18

Bohr's Model of the Atom

Bohr's model:-electrons orbit the nucleus like planets orbit the sun-each orbit can hold a specific maximum number of electrons-electrons fill orbits closest to the nucleus first.

Bohr AtomThe Planetary Model of the Atom

Bohrs ModelNucleusElectronOrbitEnergy Levels

Bohr's Model of the Atom

e.g. fluorine:#P =

#e- =

#N =

Bohr's Model of the Atom

e.g. fluorine:#P = atomic # = 9#e- =

#N =

Bohr's Model of the Atom

e.g. fluorine:#P = 9

#e- = # P = 9#N =

Bohr's Model of the Atom

e.g. fluorine:#P = 9

#e- = 9

#N = atomic mass - # P = 10

Bohr's Model of the Atom

e.g. fluorine:#P = 9

#e- = 9

#N = 10draw the nucleus with protons & neutrons

9P10N

Bohr's Model of the Atom

e.g. fluorine:#P = 9

#e- = 9

#N = 10how many electrons canfit in the first orbit?9P10N

Bohr's Model of the Atom

e.g. fluorine:#P = 9

#e- = 9

#N = 10how many electrons canfit in the first orbit?29P10N

Bohr's Model of the Atom

e.g. fluorine:#P = 9

#e- = 9

#N = 10how many electrons are left?9P10N

Bohr's Model of the Atom

e.g. fluorine:#P = 9

#e- = 9

#N = 10how many electrons are left?79P10N

Bohr's Model of the Atom

e.g. fluorine:#P = 9

#e- = 9

#N = 10how many electrons are left?7how many electrons fit in the second orbit?9P10N

Bohr's Model of the Atom

e.g. fluorine:#P = 9

#e- = 9

#N = 10how many electrons are left?7how many electrons fit in the second orbit?89P10N

Bohr's Model of the Atom

e.g. fluorine:#P = 9

#e- = 9

#N = 109P10N

Seatwork #4 :

Sodium

Boron

Magnesium

Oxygen

**Objectives:To describe the Bohr model of the atom.To explain the relationship between energy levels in an atom and lines in an emission spectrum.*