Chem-01-Atoms ElectronicStructure Lecture Notes

7/25/2019 Chem-01-Atoms ElectronicStructure Lecture Notes

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Atoms and

Electronic Structure

Atomic Structure and

Subatomic Particles

Protons and neutrons in

nucleus

Electrons move about

is the remaining space

of the atom.

1

Protons Neutrons Electrons

Note:

atomic mass unit (amu)

Relative

Charge

Charge

(C)

Mass

(amu)

Mass

(g)

Proton +1 +1.602181019 1.00727 1.672611024

Neutron 0 0 1.00866 1.674931024

Electron -1 1.602181019 0.00055 0.000911024


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Elements: Defined by their

number of protons

Atomic number (Z)

This number identifies the element. (See the

numbers on the periodic table.)

Mass number (A)

So, if given the Z and A, how will you determine

the number of neutrons?

Some questions.

What is the atomic number of Chlorine?

How many protons does chlorine have?

11A

188A

1H

1.008 22A

133A

144A

155A

166A

177A

2He

4.003

3Li

6.941

4Be

9.012

5B

10.81

6C

12.01

7N

14.01

8O

16.00

9F

19.00

10Ne

20.18

11Na

22.99

12Mg

24.31 3

3B4

4B5

5B6

6B7

7B 89

8B1 0 11

1B122B

13Al26.98

14Si

28.09

15P

30.97

16S

32.06

17Cl

35.45

18Ar39.95

19K

39.10

20Ca

40.08

21Sc

44.96

22Ti

47.87

23V

50.94

24Cr

52.00

25Mn

54.94

26Fe

55.85

27Co

58.93

28Ni

58.69

29Cu

63.55

30Zn

65.39

31Ga

69.72

32Ge

75.59

33As74.92

34Se

78.96

35Br

79.90

36Kr

83.80

37Rb

85.47

38Sr

87.62

39Y

88.91

40Zr

91.22

41Nb

92.91

42Mo

95.96

43Tc

(98)

44Ru

101.1

45Rh

102.9

46Pd

106.4

47Ag

107.9

48Cd

112.4

49In

114.8

50Sn

118.7

51Sb

121.8

52Te

127.6

53I

126.9

54Xe

131.3

55Cs

132.9

56Ba

137.3

57La

138.9

72Hf

178.5

73Ta

180.9

74W

183.8

75Re

186.2

76Os

190.2

77Ir

192.2

78Pt

195.1

79Au197.0

80Hg

200.6

81Tl

204.4

82Pb

207.2

83Bi

209.0

84Po

(209)

85At(210)

86Rn(222)

87Fr

(223)

88Ra

(226)

89Ac(227)

104Rf

(261)

105Db(262)

106Sg

(266)

107Bh

(264)

108Hs

(269)

109Mt

(268)

110Ds

(271)

111Rg

(272)

112Cn

(285)

113 114Fl

(289)

115 116Lv

(292)

117 118

Lanthanide series

58Ce

140.1

59Pr

140.9

60Nd

144.2

61Pm(145)

62Sm150.4

63Eu

152.0

64Gd

157.3

65Tb

158.9

66Dy

162.5

67Ho

164.9

68Er

167.3

69Tm168.9

70Yb

173.0

71Lu

175.0

Actinide series

90Th

232.0

91Pa

231.0

92U

238.0

93Np

(237)

94Pu

(244)

95Am(243)

96Cm(247)

97Bk

(247)

98Cf

(251)

99Es

(252)

100Fm(257)

101Md(258)

102No(259)

103Lr

(262)


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If the mass number is 37, how

many neutrons does the atom

have?1. 372. 17

3. 20

4. 27

5. 30

How many electrons does an atom of chlorine

have?

What element has an atomic number of 12?

Isotopes

Isotopes

Most elements have two or more isotopes. Symbols can be used to distinguish the different

isotopes:


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Isotope symbols

XA

Z

Determine the number of

protons, neutrons and electrons.

1. p=5, n=6, e=6

2. p=5, n=6, e=5

3. p=6, n=5, e=5

4. p=5, n=11, e=5

5. p=6, n=5, e=5

B115

Example

B115

Is the 5 necessary ?


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More about isotopes:

Hydrogen is the only element in which the

different isotopes has their own names.

1H

2H

3H

Ions: Losing and Gaining

Electrons

Ions -

Cation - positive charged ion.

Anion - negative charged ion.

Symbol electrons protons neutrons

24Mg

23Na+

35Cl

35Cl-

56Fe3+

15N

16O2-

27Al3+


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Give the number of electrons and

neutrons for 35Cl

1. e = 16, n = 20

2. e = 18, n = 18

3. e = 17, n = 20

4. e = 18, n = 20

5. None of the above

The Periodic Law

and the Periodic Table

11A

188A

1H

1.008

22A

133A

144A

155A

166A

177A

2He

4.003

3Li

6.941

4Be

9.012

5B

10.81

6C

12.01

7N

14.01

8O

16.00

9F

19.00

10Ne

20.18

11Na

22.99

12Mg

24.31

33B

44B

55B

66B

77B 8

98B

10 111B

122B

13Al26.98

14Si

28.09

15P

30.97

16S

32.06

17Cl

35.45

18Ar39.95

19K

39.10

20Ca

40.08

21Sc

44.96

22Ti

47.87

23V

50.94

24Cr

52.00

25Mn

54.94

26Fe

55.85

27Co

58.93

28Ni

58.69

29Cu

63.55

30Zn

65.39

31Ga

69.72

32Ge

75.59

33As74.92

34Se

78.96

35Br

79.90

36Kr

83.80

37Rb

85.47

38Sr

87.62

39Y

88.91

40Zr

91.22

41Nb

92.91

42Mo

95.96

43Tc(98)

44Ru

101.1

45Rh

102.9

46Pd

106.4

47Ag107.9

48Cd

112.4

49In

114.8

50Sn

118.7

51Sb

121.8

52Te

127.6

53I

126.9

54Xe

131.3

55Cs

132.9

56Ba

137.3

57La

138.9

72Hf

178.5

73Ta

180.9

74W

183.8

75Re

186.2

76Os

190.2

77Ir

192.2

78Pt

195.1

79Au197.0

80Hg

200.6

81Tl

204.4

82Pb

207.2

83Bi

209.0

84Po

(209)

85At(210)

86Rn

(222)

87Fr

(223)

88Ra

(226)

89Ac(227)

104Rf

(261)

105Db(262)

106Sg

(266)

107Bh(264)

108Hs

(269)

109Mt

(268)

110Ds

(271)

111Rg(272)

112Cn(285)

113 114Fl

(289)

115 116Lv

(292)

117 118

Lanthanide series58Ce

140.1

59Pr

140.9

60Nd

144.2

61Pm(145)

62Sm

150.4

63Eu

152.0

64Gd

157.3

65Tb

158.9

66Dy

162.5

67Ho

164.9

68Er

167.3

69Tm168.9

70Yb

173.0

71Lu

175.0

Actinide series90Th

232.0

91Pa

231.0

92U

238.0

93Np(237)

94Pu

(244)

95Am(243)

96Cm(247)

97Bk

(247)

98Cf

(251)

99Es

(252)

100Fm(257)

101Md(258)

102No(259)

103Lr

(262)

Elements with

similar

properties have

a repeating

pattern and are

aligned in

columns

Understanding Light

Classical Physics viewed energy as

continuous.ie. Any amount of energy could be

released. This was found to be false by Max Planck when

concerning the radiation emitted by a heated solid.

2


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Properties of Waves

Waves - a vibrating disturbance by which energy

is transmitted.

Waves are characterized by

Wavelength ()

Amplitude

Frequency ()

The speed (u) of the wave =

Propert ies of Waves


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Visible light consists of electromagnetic waves.

Electromagnetic

radiation

Energy

Units Joule

1 J = 1 kg m2/s2

Electric field component

Magnetic field component

c =

For electromagnetic radiation:

Speed of light in a vacuum: 3.00 10 8 m/s


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A photon has a frequency of 3.5 105 Hz.

Convert this frequency into wavelength (nm).

Does this frequency fall in the visible region?

What is the frequency (in Hz) of

light with a wavelength of 490 nm?

1. 6.12 1023

2. 6.12 105

3. 6.12 1014

4. 1.63 10-15

5. 1.63 10-6

Interactions of Waves

Interference

Constructive Interference


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Destructive Interference

Wave versus particle behavior

Diffraction -

Slit must be a

comparable size to

the wavelength

Interference Pattern


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Plancks Quantum Theory

When solids are heated they emit electromagnetic

radiation.

It was determined that the amount of radiation

energy emitted was related to its wavelength.

Classical physics could not account for this fact.

Planck solved the problem...

3

Plancks Quantum Theory

Plancks assumption: atoms and molecules could

emit (or absorb) energy only in discrete quantities.

These bundles of energy were called quantum -

the smallest quantity of energy that can be emitted.

E = h


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The Particle Nature of Light

Planck did not know the why of his discovery.

Einstein used Plancks Quantum Theory to help

explain something called the photoelectric effect

and then explained the why of Plancks theory.

The Photoelectic Effect

Light strikes the metal and ejects electrons.

What They Found

There was a certain

frequency where

below this frequencyno electrons were

ejected, no matter

how intense the light

was.


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What They Found

What They Found

Einsteins Explanation of the

Photoelectric Effect

Light is made of a stream of particles (called

photons).

Each photon has energy- Each photon, if it has enough energy, can knock

off one electron. (It must overcome the binding

energy ( BE ) of the electron.)


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h = KE + BE

Dual Nature of Light

1. Waves

2. Particles

Depending on the experiment, light behaves one

way or the other.

We will see later that matter has this nature also.

Calculations

So now you have these two equations:

c=

E=h

With these two equations if you know one of the

following, you can calculate the other two:


15/35

When copper is bombarded with high-energy electrons, X rays

are emitted. Calculate the frequency and energy (in joules)

associated with the photons if the wavelength of the X rays is

0.154 nm.

1. 1.96 10181/s 1.29 10-15 J

2. 1.96 109 1/s 1.29 10-24 J

3. 4.62 107 1/s 3.03 10-26 J

4. 4.62 10-2 1/s 3.06 19-34 J

Frequency Energy

Bohrs Model of the

Hydrogen atom

4

Emission Spectra

The continuous or line spectra of radiation emitted

by substances.

Obtained by energizing a sample until it produces light

the light is passed through a prism

the rainbow produced is the spectrum

The spectrum is not necessarily in the visible region

of electromagnetic radiation.


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1. e- can only have specific (quantized) energy values

2. light is emitted as e- moves from one energy level to

another

Bohrs Model of the Atom (1913)


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The Dual Nature of Electrons

Electron only occupies certain fixed

distances.Why?

Louis de Broglie provided a solution.

5

Expected behavior of particles

Actual electron behavior


18/35

h

mv

This equation is typically used to calculate the

wavelength

of a particle when the mass and velocity are

known.

Watch your units!

What is the de Broglie wavelength (in nm)

associated with a 2.5 g Ping-Pong ball traveling at

15.6 m/s?

h

mv

The Uncertainty Principle

We know electrons

have a wave nature.

We know electronshave a particle

nature.

6


19/35

Heisenbergs Uncertainty

Principle

4hvmx

Uncertainty in position = x

Uncertainty in velocity = v

Quantum Mechanics and the

Atom

Electrons do not move as orbits about the nucleus.

Due to Heisenbergs Uncertainty Principle we can

only define regions in space where we have a high

probability of finding an electron.

Schrdinger equations -

These equations take into account the particle and

wave nature of the electron

These equations launched quantum mechanics.


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Solutions to the Schrdinger

Equation for the Hydrogen Atom

Complex mathematical functions but they give us

quantum numbers which define the orbitals.

The four quantum numbers:

The principal quantum number (n)

The angular momentum quantum number (l)

The magnetic quantum number (ml)

The spin quantum number (ms)

7

Principal Quantum number,n

n = 1, 2, 3, 4

The farther out the electron is, the larger, higher in

energy and more unstable the orbital.

All electrons with the same n value are in the same

(principal) shell.

Energy of an electron in hydrogen:

21

nRE Hn

RH= 2.181018 J

Rydberg constant

for Hydrogen


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The Angular Momentum Q.N., (l)

l= 0, 1, .(n-1)

Usually we call the subshells by the following

names.

Orbital or subshell names

l Name of

Orbital/Subshell

0

1

2

3

4

Note: Each principal quantum number has its ownallowable values of (l) because l goes up to (n-1)

In the shelln=4, what are the

names of the subshells it has?

1. s only

2. s and p3. s, p and d

4. s, p, d and f


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Magnetic Quantum Number, ml

ml= -l, .0..+

l

All electrons with the same n,l, ml are said to bein the same orbital.

Lets stop and derive a table of quantum numbers[n, l, ml].

Connections between Q.N.s

n l ml

Which of the following is not an

allowable set of quantum numbers

[n, l, ml]1. [1,0,0]

2. [2,2,-2]

3. [3,2,0]

4. [4,1,-2]

5. Both 1 and 2

6. Both 2 and 4


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Which set of quantum numbers

will identify an electron in a 4p

subshell?

1. [4, 3, 2]

2. [4, 1, 0]

3. [4, 1, -1]

4. [4, 2, 0]

5. Both 2 and 3

Atomic Spectroscopy Explained

Atom absorbs energy, electron promoted to

higher energy level. (Excited state.)

Electron emits photon of light. (Returns to

the ground state.

8


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For

Hydrogen

Notice how the levels

get closer together as

they go farther away

from the nucleus.

E = RH( )1 1n2f n

2i

This equation can onlybe used for

the Hydrogen atom

Connection between energy of the

electron and energy of the photon.

c

hEphoton


25/352

Calculate the E of the electron of a hydrogen

atom as the electron drops from then = 5 state to

then = 3 state.

1. +2.91 x 10-20

2. -2.91 x 10-20

3. +1.55 x 10-19

4. -1.55 x 10-19

Calculate the wavelength (in nm) of a photon

emitted by a hydrogen atom when its electron

drops from then = 5 state to then = 3 state.

1. 323

2. 456

3. 646

4. 811

5. 1280

Atomic Orbitals

Orbitals are defined by

the Schrdinger

equations.

Regions in space where

there is a high

probability of finding

an electron.

9


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p orbital l= 1

d orbitals l= 2

f orbitals l= 3


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The Phase of Orbitals

Phase

Two dimensional waves.

Three dimensional waves

1s

2s 2p

3s 3p

4s 4p 4d

3d

Energy

Energy Levels in a Hydrogen Atom

1s

2s 2p

3s3p

4s

4p

4d

3d

Energy

Energy Levels in a Multi-electron Atom

Orbital Diagram

Shows what subshells (orbitals) are occupied by

electrons.

Ground state

10


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Electron Spin and the Pauli

Exclusion Principle

Electrons spin, either one way or the other.

All electrons have the same amount of spin.

Spin Quantum number (ms)

Example of an orbital diagram for hydrogen

Arrow shows the spin

Up arrow = +; down arrow =

1s

Pauli Exclusion Principle

No two electrons in an atom can have the same

four quantum numbers.

Result

Helium has two electrons in the atom

Orbital diagram:

1s

Quantum Numbers and

Orbital Diagrams

Each electron has a set of four quantum numbers

associated with it.

The first three, give the electrons location The forth gives the spin

1s


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Electron Configuration for

Multielectron atoms

We will learn to write the configuration for

ground state atoms.

Electrons are in their lowest energy state

possible.

Aufbau principle building up from lowest to

highest energy

11

For a many electron atom:E(s orbital) < E(p orbital) < E(d orbital) < E(f orbital)

1s

2s 2p

3s 3p

4s 4p 4d

3d

Energy

Energy Levels in a Hydrogen Atom

1s

2s 2p

3s3p

4s

4p

4d

3d

Energy

Energy Levels in a Multi-electron Atom

It will be necessary for you to know the

order of orbitals from lowest in energy to

highest energy.

The following is one way to learn the order.


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Element Orbital Diagram Electron Config. Q.N.

H

He

Li

Be

B

What are the quantum numbers

of the last two electrons of Be

electron configuration?

1. [2, 0, 0, ] [2, 0, 1, ]

2. [2, 0, 0, ] [2, 0, 0, ]

3. [2, 0, 0, ] [2, 0, 0, -]

4. [2, 0, 0, ] [3, 0, 0, ]

Hunds Rule

The most stable arrangement of electrons insubshells is the one with the greatest number of

parallel spins.

Result:


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Element Orbital Diagram Electron Config. Q.N.

C

N

O

F

Ne

Q

Which Q.N.s are different for the

last two electrons placed in

oxygen?1. n

2. l

3. ml

4. ms

5. l and ms

6. ml and ms

k3

Be able to duplicate this breakdown of the Periodic Table and

you can do the configuration of any element.

11A

188A

1H

1.00

8

22A

133A

144A

155A

166A

177A

2He4.00

3

3Li

6.94

1

4Be9.01

2

5B

10.8

1

6C

12.0

1

7N

14.0

1

8O

16.0

0

9F

19.0

0

10Ne20.1

8

11Na22.9

9

12Mg24.3

1

33B

44B

55B

66B

77B 8

98B

10 111B

122B

13Al26.9

8

14Si

28.09

15P

30.97

16S

32.06

17Cl

35.45

18Ar39.9

5

19K

39.10

20Ca40.0

8

21Sc44.9

6

22Ti

47.87

23V

50.94

24Cr52.0

0

25Mn54.9

4

26Fe55.8

5

27Co58.9

3

28Ni

58.69

29Cu63.5

5

30Zn65.3

9

31Ga69.7

2

32Ge75.5

9

33As74.9

2

34Se78.9

6

35Br79.9

0

36Kr83.8

0

37Rb

85.47

38Sr

87.62

39Y

88.91

40Zr

91.22

41Nb

92.91

42Mo

95.96

43Tc

(98)

44Ru

101.1

45Rh

102.9

46Pd

106.4

47Ag

107.9

48Cd

112.4

49In

114.8

50Sn

118.7

51Sb

121.8

52Te

127.6

53I

126.9

54Xe

131.3

55Cs132.

9

56Ba137.

3

57La138.

9

72Hf

178.

5

73Ta180.

9

74W

183.

8

75Re186.

2

76Os190.

2

77Ir

192.

2

78Pt

195.

1

79Au197.

0

80Hg200.

6

81Tl

204.

4

82Pb207.

2

83Bi

209.

0

84Po

(209)

85At(210)

86Rn(222)

87Fr

(223)

88Ra

(226)

89Ac(227)

104Rf

(261)

105Db

(262)

106Sg

(266)

107Bh(264)

108Hs

(269)

109Mt

(268)

110Ds

(271)

111Rg(272)

112Cn(285)

113 114Fl

(289)

115 116Lv

(292)

117 118

Lanthanide series

58Ce140.

1

59Pr

140.9

60Nd144.

2

61Pm(145)

62Sm150.

4

63Eu152.

0

64Gd157.

3

65Tb158.

9

66Dy162.

5

67Ho164.

9

68Er

167.3

69Tm168.

9

70Yb173.

0

71Lu175.

0

Actinide series

90Th232.

0

91Pa

231.0

92U

238.0

93Np(237)

94Pu

(244)

95Am(243)

96Cm(247)

97Bk

(247)

98Cf

(251)

99Es

(252)

100Fm(257)

101Md(258)

102No(259)

103Lr

(262)


32/35

Slide 92

k3 diagram used for the question has points to the the two paramagnetic electrons of oxygenkwoodru, 10/29/2007


33/35

Procedure for writing the

Electron Configuration

Find the nearest noble gas which comes before the

element. Place the noble gas symbol in square brackets.

This is called the noble gas core.

Example: [He]

Now use the breakdown of the periodic table that

you learned to add electron in until you have

reached the element of interest.

Write the electron configuration of Cl.

11A

188A

1H

1.008

22A

133A

144A

155A

166A

177A

2He4.00

3

3Li

6.941

4Be9.01

2

5B

10.81

6C

12.01

7N

14.01

8O

16.00

9F

19.00

10Ne20.1

8

11Na22.9

9

12Mg24.3

1

33B

44B

55B

66B

77B 8

98B

10 111B

122B

13Al26.9

8

14Si

28.0

9

15P

30.9

7

16S

32.0

6

17Cl

35.4

5

18Ar39.9

5

19K

39.10

20Ca40.0

8

21Sc44.9

6

22Ti

47.87

23V

50.94

24Cr52.0

0

25Mn54.9

4

26Fe55.8

5

27Co58.9

3

28Ni

58.69

29Cu63.5

5

30Zn65.3

9

31Ga69.7

2

32Ge75.5

9

33As74.9

2

34Se78.9

6

35Br79.9

0

36Kr83.8

0

37Rb85.4

7

38Sr

87.62

39Y

88.91

40Zr

91.22

41Nb92.9

1

42Mo95.9

6

43Tc(98)

44Ru101.

1

45Rh102.

9

46Pd106.

4

47Ag107.

9

48Cd112.

4

49In

114.8

50Sn118.

7

51Sb121.

8

52Te127.

6

53I

126.9

54Xe131.

3

55Cs132.

9

56Ba137.

3

57La138.

9

72Hf

178.5

73Ta180.

9

74W

183.8

75Re186.

2

76Os190.

2

77Ir

192.2

78Pt

195.1

79Au197.

0

80Hg200.

6

81Tl

204.4

82Pb207.

2

83Bi

209.0

84Po

(209)

85At(210)

86Rn

(222)

87Fr

(223)

88Ra

(226)

89Ac(227)

104Rf

(261)

105Db(262)

106Sg

(266)

107Bh(264)

108Hs

(269)

109Mt

(268)

110Ds

(271)

111Rg(272)

112Cn

(285)

113 114Fl

(289)

115 116Lv

(292)

117 118

Lanthanide series

58Ce140.

1

59Pr

140.9

60Nd144.

2

61Pm(145)

62Sm150.

4

63Eu152.

0

64Gd157.

3

65Tb158.

9

66Dy162.

5

67Ho164.

9

68Er

167.3

69Tm168.

9

70Yb173.

0

71Lu175.

0

Actinide series

90Th232.

0

91Pa

231.0

92U

238.0

93Np(237)

94Pu

(244)

95Am(243)

96Cm(247)

97Bk

(247)

98Cf

(251)

99Es

(252)

100Fm(257)

101Md(258)

102No(259)

103Lr

(262)

Sn:

V: 1

1A188A

1H

1.008

22A

133A

144A

155A

166A

177A

2He4.00

3

3Li

6.941

4Be9.01

2

5B

10.81

6C

12.01

7N

14.01

8O

16.00

9F

19.00

10Ne20.1

8

11Na22.9

9

12Mg24.3

1

33B

44B

55B

66B

77B 8

98B

10 111B

122B

13Al26.9

8

14Si

28.09

15P

30.97

16S

32.06

17Cl

35.45

18Ar39.9

5

19K

39.1

0

20Ca40.0

8

21Sc44.9

6

22Ti

47.8

7

23V

50.9

4

24Cr52.0

0

25Mn54.9

4

26Fe55.8

5

27Co58.9

3

28Ni

58.6

9

29Cu63.5

5

30Zn65.3

9

31Ga69.7

2

32Ge75.5

9

33As74.9

2

34Se78.9

6

35Br79.9

0

36Kr83.8

0

37Rb85.4

7

38Sr

87.6

2

39Y

88.9

1

40Zr

91.2

2

41Nb92.9

1

42Mo95.9

6

43Tc(98)

44Ru101.

1

45Rh102.

9

46Pd106.

4

47Ag107.

9

48Cd112.

4

49In

114.

8

50Sn118.

7

51Sb121.

8

52Te127.

6

53I

126.

9

54Xe131.

3

55Cs132.

9

56Ba137.

3

57La138.

9

72Hf

178.5

73Ta180.

9

74W

183.8

75Re186.

2

76Os190.

2

77Ir

192.2

78Pt

195.1

79Au197.

0

80Hg200.

6

81Tl

204.4

82Pb207.

2

83Bi

209.0

84Po

(209)

85At(210)

86Rn

(222)

87Fr

(223)

88Ra

(226)

89Ac(227)

104Rf

(261)

105Db(262)

106Sg

(266)

107Bh(264)

108Hs

(269)

109Mt

(268)

110Ds

(271)

111Rg(272)

112Cn

(285)

113 114Fl

(289)

115 116Lv

(292)

117 118

Lanthanide series

58Ce140.

1

59Pr

140.9

60Nd144.

2

61Pm(145)

62Sm150.

4

63Eu152.

0

64Gd157.

3

65Tb158.

9

66Dy162.

5

67Ho164.

9

68Er

167.3

69Tm168.

9

70Yb173.

0

71Lu175.

0

Actinide series

90Th232.

0

91Pa

231.

0

92U

238.

0

93Np(237)

94Pu

(244)

95Am(243)

96Cm(247)

97Bk

(247)

98Cf

(251)

99Es

(252)

100Fm(257)

101Md(258)

102No(259)

103Lr

(262)


34/35

The electron configuration of

Antimony is1. [Kr]5s25d105p6

2. [Kr]5s2

4d10

5p3

3. [Xe]5s24d105p3

4. [Xe]5s25d105p2

A few other points to know. Transition metals - have incompletely filled d

subshells or readily give rise to cations that have

incompletely filled d subshells.

Exception to learn:

This is due to the stability achieved with half filled

or filled subshells.

Examples of the Exceptions

chromium

[Ar] 4s23d4

silver

[Kr]5s24d9


35/35

Lanthanides (rare earths) - incompletely filled

4f subshells or readily give rise to cations that

have incompletely filled 4f subshells.

Actinide series - most of these not found in nature

but have been synthesized.

Chem-01-Atoms ElectronicStructure Lecture Notes

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Transcript of Chem-01-Atoms ElectronicStructure Lecture Notes