September 30, 2014

So, here's the order and you will have to memorize the order!

58 59 60 61 62 6463 65 67 68 69 70 71Ce Pr Nd Pm Sm Eu Gd Tb Ho Er Tm Yb Lu

66Dy

Cerium Praseodymium Neodymium Promethium Samarium Europium Gadolinium Terbium Dysprosium Holmium Erbium Thulium Ytterbium Lutetium

90 91 92 93 94 9695 97 99 100 101 102 103Th Pa U Np Pu Am Cm Bk Es Fm Md No Lr

98Cf

Thorium Protactinium Uranium Neptunium Plutonium Americium Curium Berkelium Californium Einsteinium Fermium Mendelevium Nobelium Lawrencium

Ru

Ti

Rhenium

Ruthenium Rhodium

H

Li Be

Na Mg

K Ca

Rb Sr

Cs Ba

Fr Ra

Sc

Y

La

Ac

Zr

Hf

Rf

V

Nb

Ta

Db

Cr

Mo

W

Sg

Mn

Tc

Re

Bh

Fe

Os

Hs

Co

Rh

Ir

Mt

Ni

Pd

Pt

Cu

Ag

Au

Zn

Cd

Hg

Hydrogen

Lithium

Sodium

Potassium

Rubidium

Cesium

Beryllium

Magnesium

Calcium

Strontium

Barium

Radium

Scandium

Yttrium

Lanthanum

Actinium

Vanadium

Niobium

Tantalum

Dubnium

Chromium

Molybdenum

Tungsten

Manganese

Technetium

Iron Cobalt Copper Zinc

Palladium Silver Cadmium

Iridium Platinum Gold Mercury

Hassium Meitnerium

B

Al

Ga

In

Tl

C

Si

Ge

Sn

Pb

N

P

As

Sb

Bi

O F

Cl

Br

I

At

He

Ne

Ar

Kr

Xe

Rn

S

Se

Te

Po

Francium

Titanium

Rutherfordium

Zirconium

Hafnium

Seaborgium

Osmium

Bohrium

1

3 4

11 12

Nickel

19 20

37 38

55 56

87 88

21 22 23 24 25 26 27 28 29 30

39 40 41 42 43 44 45 46 47 48 49

57 72 73 74 75 76 77 78 79 80

89 104 105 106 107 108 109

5 6 7 8 9 10

13 14 15 16 17 18

31 32 33 34 35 36

50 51 52 53 54

81 82 83 84 85 86

2

Gallium Germanium Arsenic Selenium Bromine Krypton

Indium Tin Antimony Tellurium Iodine Xenon

ArgonChlorineSulfurPhosphorusSiliconAluminium

Boron Carbon Nitrogen Oxygen Fluorine Neon

Helium

Thallium Lead Bismuth Polonium Astatine Radon

But we can also use the periodic table!

IB Syllabus

?

Application of the Aufbau principle, Hund’s rule and the Pauli exclusion principle to write electron configurations for atoms and ions up to Z = 36.

September 30, 2014

Review: Let's try this one.

State the electron configuration of tellurium.

What about ions?

Ba 2+

Cl-

What about Cr?What about Cr?

September 30, 2014

?Another one:Exceptions:

Here are some questions for you to try!How do we know if the sub orbitals are actually there?

Well, from the ionization energy patterns!

So, what's ionization energy?

The first electron to be removed is one that already has a high energy and is least strongly attracted to the nucleus; that is, one in the valence shell. This will require the lowest ionization energy. If there are more electrons in this outer shell, then they will be removed next, with the ionization energy gradually increasing. When the outermost electron shell is empty, the next electron to be lost will come from the next closest shell to the nucleus. But since this shell is full, and therefore stable, a great deal more energy will be required to remove one electron from this shell than was needed to remove the previous electron.

September 30, 2014

A graph of first ionization energies of the first 54 elements shows distinct patterns that lead us to a greater understanding of the electron structure of an atom.

The most obvious feature of this graph is the periodic series of peaks corresponding to the first ionization energy of the noble gases (He, Ne, Ar, Kr, Xe). These elements have high first ionization energies because they have a full electron shell and an associated high degree of energetic stability.

The next most obvious feature of the graph is the lowest point of each periodic series. These troughs correspond to the group 1 elements (Li, Na, K, Rb). These elements have only one electron in the outer shell and so the first ionization energy is small, as little energy is required to remove this electron from the atom.

But, let's examine further...

If the second energy level is like the first energy level, then we would expect a gradual increase in ionization energy as we remove the electrons one by one

However, that's not the case!

September 30, 2014

This suggests the presence of sub-levels (subshells) within the main energy levels. The first sub-level in the 2nd energy level is filled with 2 electrons. The second sub-level appears to be filled by 3 electrons, with a third sub-level filled with a further 3 electrons.

The other possibility, is that the second sub-level gains some stability in becoming half-full, and its greatest stability is when it is completely full with 6 electrons in it.

So, what are these s, p, d, f orbitals?

An orbital is a region of space in which an electron or electrons may be found.

12.1.5Draw the shape of an s orbital and the shapes of the px, py and pz orbitals.

s orbitals

What about d?

P orbitals

September 30, 2014