1. Starter S-30 How many electrons are found in Carbon Nitrogen Argon
Potassium

2. Chapter 5
Electrons in Atoms

3. Chapter 5
5.1 Models of the Atom

4. 5.1 Models of the Atom
Rutherford – electron moves around the nucleus, like planets
Could not explain the chemical properties of atoms

5. 5.1 Models of the Atom
Niels Bohr – (1913) electrons are found only in specific circular paths, or orbitals, around the nucleus

6. 5.1 Models of the Atom Bohr model has 4 principles
Electrons assume only certain orbits around the nucleus. These orbits are stable and called "stationary" orbits.
Each orbit has an energy associated with it. For example the orbit closest to the nucleus has an energy n1, the next closest n2 and so on.
Light is emitted when an electron jumps from a higher orbit to a lower orbit and absorbed when it jumps from a lower to higher orbit.
The energy and frequency of light emitted or absorbed is given by the difference between the two orbit energies.

7. Energy Level Simulation
5.1 Models of the Atom
Quantum – the amount of energy required to move an electron from one energy level to another energy level
The levels for hydrogen were first determined by what frequencies of light were given off
Energy Level Simulation

8. 5.1 Models of the Atom Quantum Mechanical Model
1926 Erwin Schrödinger – no longer a circular pathway, but an area of probability
The energy of electrons in atoms is quantised.
The number of possible energy levels for electrons in atoms of different elements is a direct consequence of wave-like properties of electrons.
The position and momentum of an electron cannot both be determined simultaneously.
The region in space around the nucleus in which an electron is most probably located is what can be predicted for each electron in an atom. Electrons of different energies are likely to be found in different regions. The region in which an electron with a specific energy will most probably be located is called an atomic orbital.

9. 5.1 Models of the Atom Atomic Orbitals
First electrons are listed by energy levels (principle quantum number)
The values are n=1,2,3,4,5,6,7
There are sublevels in each level,
if n=1, there is one sublevel
if n=2, there are two sublevels

10. 5.1 Models of the Atom The first sublevel is always called s
Holds a maximum of 2 electrons
It represents the area where electrons will be 90% of the time

11. 5.1 Models of the Atom The second sublevel is p
Holds a maximum of 2 electrons per shape
Total maximum is 6 electrons

12. 5.1 Models of the Atom The third sublevel is d
Holds a maximum of 2 electrons per shape
Total maximum is 10 electrons

13. 5.1 Models of the Atom The fourth sublevel is f
Holds a maximum of 2 electrons per shape
Total maximum is 14 electrons

14. 5.1 Models of the Atom
More, but none in the ground (lowest energy) state
The orbital names s, p, d, and f stand for names given to groups of lines in the spectra of the alkali metals. These line groups are called sharp, principal, diffuse, and fundamental. So 1s
2s 2p
3s 3p 3d
4s 4p 4d 4f

15. Starter S-34
What is the shape of an s orbital? How many electrons will it hold?
What is the shape of
a p orbital? How
many electrons will
it hold?

16. 5.2 Electron Arrangement in Atoms
Chapter 5
5.2 Electron Arrangement in Atoms

17. 5.2 Electron Arrangements in Atoms
Electron Configuration – the way electrons are arranged around a nucleus
Aufbau Principle – electrons occupy the orbitals of lowest energy first
-First draw the following
-Now draw these arrows
Remember 7s
6s 6p 6d
5s 5p 5d 5f
4s 4p 4d 4f
3s 3p 3d
2s 2p 1s
s holds 2
p holds 6
d holds 10
f holds 14

18. 5.2 Electron Arrangements in Atoms
To write a configuration
Calculate the number of electrons
Place electrons in orbitals by following diagonal lines
Continue until no
electrons remain 7s
6s 6p 6d
5s 5p 5d 5f
4s 4p 4d 4f
3s 3p 3d
2s 2p 1s

19. 5.2 Electron Arrangements in Atoms
Example: Titanium
Electrons? 22 7s
6s 6p 6d
5s 5p 5d 5f
4s 4p 4d 4f
3s 3p 3d
2s 2p 1s

20. 5.2 Electron Arrangements in Atoms
Example: Titanium
Electrons? 22
2 go in 1s 7s
6s 6p 6d
5s 5p 5d 5f
4s 4p 4d 4f
3s 3p 3d
2s 2p 1s

21. 5.2 Electron Arrangements in Atoms
Example: Titanium
Electrons? 22
2 go in 1s
20 remain 7s
6s 6p 6d
5s 5p 5d 5f
4s 4p 4d 4f
3s 3p 3d
2s 2p
1s2

22. 5.2 Electron Arrangements in Atoms
Example: Titanium
Electrons? 20
2 go in 2s
18 remain 7s
6s 6p 6d
5s 5p 5d 5f
4s 4p 4d 4f
3s 3p 3d
2s22p
1s2

23. 5.2 Electron Arrangements in Atoms
Example: Titanium
Electrons? 18
6 go in 2p
12 remain 7s
6s 6p 6d
5s 5p 5d 5f
4s 4p 4d 4f
3s 3p 3d
2s22p6
1s2

24. 5.2 Electron Arrangements in Atoms
Example: Titanium
Electrons? 12
2 go in 3s
10 remain 7s
6s 6p 6d
5s 5p 5d 5f
4s 4p 4d 4f
3s23p 3d
2s22p6
1s2

25. 5.2 Electron Arrangements in Atoms
Example: Titanium
Electrons? 10
6 go in 3p
4 remain 7s
6s 6p 6d
5s 5p 5d 5f
4s 4p 4d 4f
3s23p63d
2s22p6
1s2

26. 5.2 Electron Arrangements in Atoms
Example: Titanium
Electrons? 4
2 go in 4s
2 remain 7s
6s 6p 6d
5s 5p 5d 5f
4s24p 4d 4f
3s23p63d
2s22p6
1s2

27. 5.2 Electron Arrangements in Atoms
Example: Titanium
Electrons? 2
2 go in 3d
0 remain
4s2
3s23p63d2
2s22p6
1s2

28. 5.2 Electron Arrangements in Atoms
Example: Carbon
Electrons 7s
6s 6p 6d
5s 5p 5d 5f
4s 4p 4d 4f
3s 3p 3d
2s 2p 1s

29. 5.2 Electron Arrangements in Atoms
Example: Carbon
Electrons 6 7s
6s 6p 6d
5s 5p 5d 5f
4s 4p 4d 4f
3s 3p 3d
2s 2p 1s

30. 5.2 Electron Arrangements in Atoms
Example: Carbon
Electrons 6
2s22p2
1s2

31. 5.2 Electron Arrangements in Atoms
Example: Argon
Electrons 7s
6s 6p 6d
5s 5p 5d 5f
4s 4p 4d 4f
3s 3p 3d
2s 2p 1s

32. 5.2 Electron Arrangements in Atoms
Example: Argon
Electrons 18 7s
6s 6p 6d
5s 5p 5d 5f
4s 4p 4d 4f
3s 3p 3d
2s 2p 1s

33. 5.2 Electron Arrangements in Atoms
Example: Argon
Electrons 18
3s23p6
2s22p6
1s2

34. 5.2 Electron Arrangements in Atoms
Example: Nickel
Electrons 7s
6s 6p 6d
5s 5p 5d 5f
4s 4p 4d 4f
3s 3p 3d
2s 2p 1s

35. 5.2 Electron Arrangements in Atoms
Example: Nickel
Electrons 28 7s
6s 6p 6d
5s 5p 5d 5f
4s 4p 4d 4f
3s 3p 3d
2s 2p 1s

36. 5.2 Electron Arrangements in Atoms
Example: Nickel
Electrons 28
4s2
3s23p63d8
2s22p6
1s2

37. Starter S-35
Draw the electron configuration for Zirconium (Zr).

38. 5.2 Electron Arrangements in Atoms
Pauli Exclusion Principle – an orbital may only have two electrons. Those electrons must have opposite spins.
Hund’s Rule – electrons occupy orbitals of the same energy so that the number of electrons with the same spin is as large as possible

39. 5.2 Electron Arrangements in Atoms
Orbital Diagrams
Represent orbitals by boxes
1 box for s
3 for p,
5 for d
7 for f
3. each box can hold up to 2 electrons

40. 5.2 Electron Arrangements in Atoms
electrons represented by arrows
a. direction represents spin (1 up, 1 down per box)
5. boxes must be unpaired before they can pair up

41. 5.2 Electron Arrangements in Atoms
Example: Copper
Electrons? 29
Electrons Configuration
4s2
3s2 3p6 3d9
2s2 2p6
1s2

42. 5.2 Electron Arrangements in AtomsCu
4s2
3s2 3p6 3d9
2s2 2p6
1s2

43. 5.2 Electron Arrangements in AtomsCu
4s2
3s2 3p6 3d9
2s2 2p6 1s

44. 5.2 Electron Arrangements in AtomsCu
4s2
3s2 3p6 3d9
2s 2p6 1s

45. 5.2 Electron Arrangements in AtomsCu
4s2
3s 3p6 3d9
2s 2p 1s

46. 5.2 Electron Arrangements in AtomsCu
4s2
3s 3p6 3d9
2s 2p 1s

47. 5.2 Electron Arrangements in AtomsCu
4s2
3s 3p 3d9
2s 2p 1s

48. 5.2 Electron Arrangements in AtomsCu 4s
3s 3p 3d9
2s 2p 1s

49. 5.2 Electron Arrangements in AtomsCu 4s
3s 3p 3d
2s 2p 1s

50. 5.2 Electron Arrangements in Atoms
Write the electron configuration for Carbon
2s22p2
1s2

51. 5.2 Electron Arrangements in Atoms
2s 2p 1s
Draw the orbital filling diagram for Carbon
2s22p2
1s2

52. 5.2 Electron Arrangements in Atoms
Write the electron configuration for Titanium
4s2
3s23p63d2
2s22p6
1s2

53. 5.2 Electron Arrangements in AtomsTi 4s
3s 3p 3d
2s 2p 1s
Draw the orbital filling diagram Titanium
4s2
3s23p63d2
2s22p6
1s2

54. 5.2 Electron Arrangements in Atoms
Lewis dot diagrams
Show only Valence Electrons
Valence – highest energy level electrons
Pick out the highest energy level from the orbital filling diagram
Write the symbol for the element
Imagine a box around the symbol
Placed paired and unpaired electrons around the symbol

55. 5.2 Electron Arrangements in Atoms
Carbon
2s 2p 1s C

56. 5.2 Electron Arrangements in Atoms
3s 3p 3d
2s 2p 1s
Titanium Ti

57. 5.2 Electron Arrangements in Atoms
Never
More than 4 pair of dots around a symbol

58. Starter S-36
4s p
3s 3p 3d
2s 2p 1s
Draw the electron configuration, orbital filling diagram, and Lewis dot diagram for Arsenic (As).
4s24p3
3s23p63d10
2s22p6
1s2

59. Rb Starter S-37 5s1 4s24p6 3s23p63d10 2s22p6 1s2 5s 4s 4p 3s 3p 3d
Draw the electron configuration, orbital filling diagram, and Lewis dot diagram for Rabidium, (Rb).
5s1
4s24p6
3s23p63d10
2s22p6
1s2

60. 5.2 Electron Arrangements in Atoms
Exceptions
Sometimes the electron configuration pattern is not followed
Because, although a filled orbital is the most stable, a half filled orbital is more stable than other arrangements
For example Copper seems like it should be

61. 5.2 Electron Arrangements in AtomsCu 4s
3s 3p 3d
2s 2p 1s
The 3d is not stable
If 1 electron is moved from the 4s to the 3d

62. 5.2 Electron Arrangements in AtomsCu 4s
3s 3p 3d
2s 2p 1s
4s is half full – stable
3d is full - stable

63. 5.3 Physics & the Quantum Mechanical Model
Chapter 5
5.3 Physics & the Quantum Mechanical Model

64. 5.3 Physics & the Quantum Mechanical Model
The Quantum Mechanical Model grew out of the study of light
Wavelength (l) – distance from one wave to the next
Frequency (n) – number of cycles per second
measured in hertz (hz)

65. 5.3 Physics & the Quantum Mechanical Model
The study of light includes the entire Electromagnetic Spectrum
From lowest energy to greatest
Radio
Microwave
Infrared
Visible Light
Ultraviolet
X-Ray
Gamma Ray

66. 5.3 Physics & the Quantum Mechanical Model
Two Equations
c = 3 x 108 m/s (speed of light) or 300,000,000
f = frequency (hz)
l = wavelength (m)

67. 5.3 Physics & the Quantum Mechanical Model
Energy Equation
E = energy (J)
f = frequency (hz)
h = x Js

68. Starter S-39 A. Draw the electron configuration, orbital filling
diagram, and Lewis dot
diagram for Phosphorus (P).
B. What is the frequency of a light with a wavelength of 435 nm?
C. What is the energy of that photon?

69. 5.3 Physics & the Quantum Mechanical ModelAt
5.3 Physics & the Quantum Mechanical Model
Atomic Spectra
When an electron is given energy, it is excited.
The atom then drops back to its ground state and gives off a photon.

70. 5.3 Physics & the Quantum Mechanical ModelAt
5.3 Physics & the Quantum Mechanical Model
Different frequencies of light are produced
some are visible

71. 5.3 Physics & the Quantum Mechanical ModelAt
5.3 Physics & the Quantum Mechanical Model
If a spectroscope is used to view the results we get either an emission spectrum (what light comes off)
or an absorption spectrum

72. 5.3 Physics & the Quantum Mechanical ModelAt
5.3 Physics & the Quantum Mechanical Model
Elements can be identified by their spectrum
Argon
Helium
Mercury
Sodium
Neon

73. 5.3 Physics & the Quantum Mechanical ModelAt
5.3 Physics & the Quantum Mechanical Model
Atomic Spectra are produced using a spectroscope.

74. Starter S-38 What is the wavelength of a green laser if it has a
frequency of
5.17x1014 hz?
B. How much energy
is in one photon of that laser light?

75. Ir Starter S-39 6s2 5s25p65d7 4s24p64d104f14 3s23p63d10 2s22p6 1s2
Complete the electron configuration, orbital
filling diagram, and
Lewis dot diagram
for Iridium (Ir) 6s
5s p d Ir
6s2
5s25p65d7
4s24p64d104f14
3s23p63d10
2s22p6
1s2

76. 5.3 Physics & the Quantum Mechanical ModelAt
5.3 Physics & the Quantum Mechanical Model
The light emitted by an electron moving from a higher energy level to a lower level has a frequency directly proportional to the energy change of the atom.

77. Starter S-42
Complete the electron configuration, orbital
filling diagram, and
Lewis dot diagram
for Iron (Fe) 4s
3s p d Fe
4s2
3s23p63d6
2s22p6
1s2

78. Starter S-44
These pigs are very happy that you are taking a test!