Atomic models electronic config

Once Upon a Time…Leucippus’ Story

Different Theories of the Atom

Greek Philosophers

• Aristotle: relied on logic-continuous matter.

• Leucippus & Democritus: they introduce the word “atomos” individual particles of matter which could not be subdivided.

Substance were mixtures of different types of atoms.

• Lucretius: Roman poet who wrote about atoms.

Atoms

• The Greeks based their models on logic and speculation, not experiment.

• Several observations led up to the formulation of atomic theory by Dalton.

Dalton’s model of the atom was based on observation and experiment, not

speculation.

• Based on Laws of Nature as discovered by several people.

Dalton’s atomic theory

• All matter is composed of extremely small particles called atoms.

• All atoms of a given element are alike, but atoms of one element differ from

the atoms of any other element.

• Compounds are formed when atoms of different elements combine in fixed

proportion.

Dalton’s Atomic Model:

Solid bowling

ball

J. J Thomson discovered the electron using the cathode ray tube.

Thomson proposed a model of a

spherical atom composed of

diffuse, positively

charged matter, in which

electrons were embedded like

“plum pudding”

Goldstein discovered positive particles, which we now know are protons.

Rutherford proposed the nuclear model of the atom.

Atoms consisted of a central nucleus which had a positive charge and

which had a very small volume, but it also contained most of the mass of the atom. Surrounding the nucleus were electrons, which had very little

mass, but which occupied most of the volume of the atom.

Rutherford set out to test Thomson’s hypothesis.

Microscopic View of the

Alpha Particle

Scattering Experiment

Rutherford's Atomic Model

Discover the

nucleus (proton+ neutron)

and electron flying.

The Bohr Atom

• Bohr was able to accurately predict the energy levels of the one-electron

atom, hydrogen.• He deduced that multi-electron atoms

would have electrons placed in the energy levels described by his theory.

• A certain maximum number of electrons could be in each level.

Bohr’s Atomic model (Energy levels)

Niels Borh Atomic Model“Planetary System”

Electrons flying in energy’s

levels

The charge cloud representations illustrate the regions of high electron probability around a nucleus as calculated using Schrödinger's equations. These complex mathematical equations combine the wave properties and particle nature of an electron with quantum restrictions.

Schrödinger Electron Cloud Model

SommerfeldTalk about Elliptical

orbits and sublevels of

energy

Atomic Models

4 atomic models build the:

“Quantum Mechanical Model of the Atom”

QUANTUM NUMBER

SYMBOL REPRESENTS VALUES PROVIDES INFORMATION ABOUT

First or Principal Quantum Number n Energy Level It can take whole numbers

from 1 to n (1 to 7 most common)

The electron cloud size

Second Quantum Number l Energy Sublevel It can range in values from

0 to n-1 (i.e.: when n=3, values of l are 0, 1, and 2)

The shape of the electron cloud

Third Quantum Number m Orbital (regions

in which 0, 1 or up to 2 electrons are likely to be found)

It can have integral values form -l to +l

m=n2, i.e: when n=2, m= 4, that means that in 2nd level there is one 2s orbital and three 2p orbitals for a total

of four.s= 1 orbital

p= 3 orbitalsd= 5 orbitalsf= 7 orbitals

The orientation in the space of the orbital

Fourth Quantum Number s Spin of the

electronIt can be either +1/2 or -1/2

The rotation direction of the electron, either clockwise or counter-clockwise.

p. 44, 45

Niels Borh Atomic Model“Planetary System”

Electrons flying in energy’s

levels“n”

“s” orbitals,“p” orbitals,“d” orbitals,“f” orbitals.

Sommerfeld talk about Elliptical orbits and sublevels of energy “l” The shape.

s, p, d, and f Orbitals

Charge Cloud Representations of “s” Orbitals

Shapes of “p” Orbitals

Schrödinger Magnetic Zones in the Atom “m”

To know the

orientation of the

e-

3D

px, py, pz orbitals


Dirac-Jordan: Electron’s Spin “s”

counterclockwise clockwise

Electrons in Energy Levels

The maximum number of electrons in any energy level is 2n2.

Level 2n2 max # e-

1 2(1)2 2

2 2(2)2 8

3 2(3)2 18

4 2(4)2 32

Z: Atomic number = # of protonsHe2

A: Atomic mass = # of protons + # of neutrons

He : 4 uma

Isotopes =Same # of protons, lack of neutrons

He: 2p+, 1no

Z: Atomic Number

A: Atomic Mass

Z: Atomic Number

A: Atomic Mass

Z: Atomic Number

A: Atomic Mass

++o

o

e-

e-

Helium atom

2 p+, Z = 22 n0 + 2 p+, A = 4

2 e-

ANION

++o

o

e-

e-

2 p+ = +23 e- = -3

net charge = -1

e- Helium atom

CATION

e-

++o

o

e-

2 p+ = +21 e- = -1

net charge = +1

Helium atom

ISOTOPES

++o

e-

e-

2 p+, Z = 21 n0 + 2 p+, A = 3

2 e-

Helium atom

Elemento Símbolo Número deProtones

(p+)

Número de Neutrones

(no)

Número de Electrones

(e-)

Número Atómico

(Z)

Número de Masa

(A)

Oxígeno O 8 8 8 8 16

Silicio Si 14 14 14 14 28

Aluminio Al 13 14 13 13 27Hierro Fe 26 30 26 26 56

Calcio Ca 20 20

Sodio Na 11 23

Cobre Cu 29 35 29

Magnesio Mg 12 24

Oro Au 79 197

Plata Ag 61 47

Elemento Símbolo Número deProtones

(p+)


(no)


(e-)

Número Atómico

(Z)

Número de Masa

(A)

Oxígeno O 8 8 8 8 16

Silicio Si 14 14 14 14 28

Aluminio Al 13 14 13 13 27Hierro Fe 26 30 26 26 56

Calcio Ca 20 20 20 20 40Sodio Na 11 12 11 11 23

Cobre Cu 29 35 29 29 64Magnesio Mg 12 12 12 12 24

Oro Au 79 118 79 79 197

Plata Ag 44 61 47 108 169

Z: Atomic number = # of protonsHe2

A: Atomic mass (mass number) = # of protons + # of neutrons

He : 4 uma

Isotopes =Same # of protons, lack of neutrons

He: 2p+, 1no

ION: charged atom(+) Cation = lack of electrons

(-) Anion = excess of electrons

Z: Atomic Number

A: Atomic Mass

Nombre y Símbolo del

Elemento

Número deProtones

(p+)


(no)


(e-)

Número Atómico

(Z)

Número de Masa

(A)

Carga Átomo o Ión: Anión o Catión

Zn 30 35 30 30 65 0 Atom

Cl 17 18 18 17 35 -1 Anion

V 23 20 21 23 43 +2 Cation35 34 -1

11 9 -3

12 10 +2

11 23 0

19 20 +1

56 137 0

15 16 -3


Elemento

Número deProtones

(p+)


(no)


(e-)

Número Atómico

(Z)

Número de Masa

(A)


Zn 30 35 30 30 65 0 Atom

Cl 17 18 18 17 35 -1 Anion

V 23 20 21 23 43 +2 Cation

As 33 35 34 33 68 -1 Anion

F 9 11 12 9 20 -3 Anion

Mg 12 12 10 12 24 +2 Cation11 23 0

19 20 +1

56 137 0

15 16 -3


Elemento

Número deProtones

(p+)


(no)


(e-)

Número Atómico

(Z)

Número de Masa

(A)


Zn 30 35 30 30 65 0 Atom

Cl 17 18 18 17 35 -1 Anion

V 23 20 21 23 43 +2 Cation

As 33 35 34 33 68 -1 Anion

F 9 11 12 9 20 -3 Anion

Mg 12 12 10 12 24 +2 Cation

Na 11 12 11 11 23 0 Atom

K 19 20 18 19 39 +1 Cation

Ba 56 81 56 56 137 0 Atom

P 15 16 18 15 31 -3 Anion

Electronic Configuration

• A summary of an orbital diagram.

• The way in which electrons are arranged around the nucleus of the atoms.

There are energy levels

• The energy levels were assigned a

principal quantum number, n, which

could equal 1, 2, 3…

• This quantum number, n designates the

energy and size of the region in space

the electrons might be found.

There are energy sub-levels

• Within an energy level there are

sublevels or subshells, designated s,

p, d, and f.

• This quantum number, l tell the shape of

the region in space the electrons might

be found.

Orbitals

• Each subshell contains one or more orbitals.

• Each orbital can contain one or two electrons.

• Each electron in an orbital must have opposite spins.

Heisenberg Uncertainty Principle

It is impossible to know simultaneously,

both the velocity and the position of a

particle with certainty.

Pauli Exclusion Principle

Two electrons in an atom can not have the

same 4 quantum numbers.

He = 1s2

Hund’s Rule

The most stable arrangement of electrons

in sublevels is the one with the greatest

number of parallel spins.

Short Hand Method

• Write the electron configuration by filling in the number of electrons of each type

in the orbitals: XsaYsbZpc…

Where X, Y, Z are Principle Quantum numbers.

s, p, d, f are the shape of the orbital.

a, b, c are number of electrons.

Examples of short hand electronic configurations

• 2He: 1s2

• 3Li : 1s2 2s1

• 6C: 1s2 2s22p2

1s2s 2p3s 3p 3d4s 4p 4d 4f5s 5p 5d 5f6s 6p 6d 6f7s 7p 7d

Diagram of Aufbau

s=2p=6

d=10f=14

1s 2s 3s 4s 5s 6s 7s2p 3p 4p 5p 6p 7p

3d 4d 5d 6d 7d 4f 5f 6f

Diagram of Aufbau

s=2p=6

d=10f=14

Element Z Electronic Configuration Orbital diagram

s p

Lithium 3

Carbon 6

Oxygen 8

Neon 10

Sodium 11

Aluminium 13

Phosphorus 15

Chlorine 17

Potassium 19

Calcium 20

1s22s1

1s22s22p2

1s22s22p4

1s22s22p6

1s22s22p63s1

1s22s22p63s23p1

1s22s22p63s23p3

1s22s22p63s23p5

1s22s22p63s23p64s1

1s22s22p63s23p64s2

2

2 1

2 1

2 1

3 1

3 2

3 2

3 2

4 2

4 2

Atom or Ion Z or ion

Electronic Configuration

Orbital Diagrams

s p

Nitrogen atom 7

Nitrogen ion -3

Oxygen atom 8

Oxygen ion -2

Fluorine atom 9

Fluorine ion -1

Sodium atom 11

Sodium ion +1

Magnesium atom

12

Magnesium ion +2

Sulphur atom 16

Sulphur ion -2

Chlorine atom 17

Chlorine ion -1

Calcium atom 20

Calcium ion +2

Iodine atom 53

Iodine ion -1

Barium atom 56

Barium ion +2

1s22s22p3

1s22s22p6

1s22s22p4

1s22s22p6

1s22s22p5

1s22s22p6

1s22s22p63s1

1s22s22p6

1s22s22p63s2

1s22s22p6

Atom or Ion Atomic

Number or Charge of

the ion

Electronic Configuration Orbital

Diagram

s

s p

Nitrogen atom 7

Nitrogen ion -3

Oxygen atom 8

Oxygen ion -2

Fluorine atom 9

Fluorine ion -1

Sodium atom 11

Sodium ion +1

Magnesium atom

12

Magnesium ion +2

Sulphur atom 16

Sulphur ion -2

Chlorine atom 17

Chlorine ion -1

Calcium atom 20

Calcium ion +2

Iodine atom 53

Iodine ion -1

Barium atom 56

Barium ion +2

1s22s22p63s23p4

1s22s22p63s23p6

1s22s22p63s23p5

1s22s22p63s23p6

1s22s22p63s23p64s2

1s22s22p63s23p6

1s22s22p63s23p64s23d104p65s24d105p5

1s22s22p63s23p64s23d104p65s24d105p6

1s22s22p63s23p64s23d104p65s24d105p66s2

1s22s22p63s23p64s23d104p65s24d105p6


Charge Cloud Representations of

“s” Orbitals

Shapes of “p” Orbitals

px, py, and pz Orbitals

Valence Electrons

The electrons in the highest occupied energy level of an elements atoms.

The energy level that holds the valence electrons are called Valence shells.

Octet RuleThe most stable arrangement of the atom is

with 8 electrons in the last level like a noble

gas.

Symbol of

element

No.of p+

and e-(Z)

Valence shell

No. of valence

e-

Lewis diagram

e- that can be lost or gained

Charge (+ or -)Cation

o Anion

Electronic configuration of anion or cation

3 Li

11 Na

20 Ca

13 Al

19 K

6 C

15 P

8 O

10 Ne

17 Cl

Symbol of

element

No.of p+

and e-(Z)

Valence shell

No. of valence

e-

Lewis diagram



o Anion


3 Li 3 2 1 1 +1 1s2 2s1

11 Na 11 3 1 1 +1 1s2 2s2 2p6 3s1

20 Ca 20 4 2 2 +2 1s2 2s2 2p6 3s2 3p6 4s2

13 Al

19 K

6 C

15 P

8 O

10 Ne

17 Cl

Li

Na

Ca

Symbol of

element

No.of p+

and e-(Z)

Valence shell

No. of valence

e-

Lewis diagram



o Anion


3 Li 3 2 1 1 +1 1s2 2s1

11 Na 11 3 1 1 +1 1s2 2s2 2p6 3s1

20 Ca 20 4 2 2 +2 1s2 2s2 2p6 3s2 3p6 4s2

13 Al 13 3 3 3 +3 1s2 2s2 2p6 3s2 3p1

19 K 19 4 1 1 +1 1s2 2s2 2p6 3s2 3p6 4s1

6 C 6 2 4 4 ±4 1s2 2s2 2p2

15 P

8 O

10 Ne

17 Cl

Li

Na

Ca

AlK

C

Symbol of

element

No.of p+

and e-(Z)

Valence shell

No. of valence

e-

Lewis diagram



o Anion


3 Li 3 2 1 1 +1 1s2 2s1

11 Na 11 3 1 1 +1 1s2 2s2 2p6 3s1

20 Ca 20 4 2 2 +2 1s2 2s2 2p6 3s2 3p6 4s2

13 Al 13 3 3 3 +3 1s2 2s2 2p6 3s2 3p1

19 K 19 4 1 1 +1 1s2 2s2 2p6 3s2 3p6 4s1

6 C 6 2 4 4 ±4 1s2 2s2 2p2

15 P 15 3 5 3 -3 1s2 2s2 2p6 3s2 3p3

8 O 8 2 6 2 -2 1s2 2s2 2p4

10 Ne 10 2 8 0 0 1s2 2s2 2p6

17 Cl 17 3 7 1 -1 1s2 2s2 2p6 3s2 3p5

Ne

Li

Na

Ca

AlK

C

P

O

Cl

Ne

Education

Atomic models electronic config