Modeule 4 Elctrons in Atoms_Module 3.ppt

everything about matter and its classification

2. •Unit 1 Structure and Properties of Matter
•Module 4 Electrons in Atoms
Lesson 3 Electron Configuration (The Bohr Model)

3. Learning outcomes
3
Thermodynamics I
•explain the arrangement of electrons in discrete energy levels around the
nucleus.
•Create and label diagrams of atoms using the Bohr Model for various
elements up to atomic number 20.
•Describe how electrons can move between energy levels by absorbing or
emitting specific amounts of energy (quantum leaps).

4. Bohr's Model of the Atom
Niels Bohr (1913):
Proposed a revolutionary
model of the atom where
electrons orbit the nucleus in
discrete energy levels or
shells.
•Proposed a revolutionary model of the atom where electrons orbit the nucleus in discrete energy levels or shells.

5. Bohr's Model of the Atom
Bohr's model:
- electrons orbit the nucleus like planets
orbit the sun

6. 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

7. 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
2 8
3 8

8. 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.

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

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

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

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

13. Bohr's Model of the Atom
e.g. fluorine:
#P = 9
#e
-
= 9
#N = 10
draw the nucleus with
protons & neutrons
9P
10N

14. 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

15. 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

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

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

18. 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

19. 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

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

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

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

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

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

25. Bohr's Model of the Atom
Niels Bohr also studied the
light produced when atoms
were excited by heat or
electricity.

26. Bohr's Model of the Atom
Niels Bohr (1913):
-studied the light produced when atoms
were excited by heat or electricity

27. 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 colors were obtained by atoms of
different elements

28. 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

30. 30
 THANK YOU 