Bohr's Model of the Atom

Bohr's Model of the Atom Niels Bohr (1913):

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

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

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

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 orbit maximum # electrons 1 2 8 3 4 18

used to predict the reactivity of an element Bohr's Model of the Atom used to predict the reactivity of an element Reactivity- how likely an element will form a compound with another element. electrons fill orbits closest to the nucleus first. (later known as Aufbau principle) Electrons in outermost orbit are called valence electrons, involved in chemical reactions

Drawing Bohr Models Draw the nucleus. Write the number of neutrons and the number of protons in the nucleus. Draw the first energy level. Draw the electrons in the energy levels according to the rules below. Make sure you draw the electrons in pairs. Draw the pairs as far apart from other pairs Keep track of how many electrons are put in each level and the number of electrons left to use.

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 = 10 draw the nucleus with protons & neutrons 9P 10N

Bohr's Model of the Atom e.g. fluorine: #P = 9 #e- = 9 #N = 10 how many electrons can fit in the first orbit? 9P 10N

Bohr's Model of the Atom e.g. fluorine: #P = 9 #e- = 9 #N = 10 how many electrons can fit in the first orbit? 2 9P 10N

Bohr's Model of the Atom e.g. fluorine: #P = 9 #e- = 9 #N = 10 how many electrons are left? 9P 10N

Bohr's Model of the Atom e.g. fluorine: #P = 9 #e- = 9 #N = 10 how many electrons are left? 7 9P 10N

Bohr's Model of the Atom e.g. fluorine: #P = 9 #e- = 9 #N = 10 how many electrons are left? 7 how many electrons fit in the second orbit? 9P 10N

Bohr's Model of the Atom e.g. fluorine: #P = 9 #e- = 9 #N = 10 how many electrons are left? 7 how many electrons fit in the second orbit? 8 9P 10N

Bohr's Model of the Atom e.g. fluorine: #P = 9 #e- = 9 #N = 10 9P 10N

Bohr's Model of the Atom try these: hydrogen boron magnesium

Bohr's Model of the Atom try these: hydrogen 1P 0N

Bohr's Model of the Atom try these: boron 5P 6N

Bohr's Model of the Atom try these: magnesium 12P 12N