Periodic Table - Gov 421... · Th90 Pa91 92U Np93 Pu94 Am95 96Cm Bk97 Cf98 Es99 Fm100 Md101 No102...

Periodic Table

All of the elements are listed in the periodic table.

There are about 120 known elements, although many of these are very uncommon, and some do not occur naturally.

There is a great variety of properties among the elements.

Most are solid at room temperature, some are a gas at room temperature, and only two (Bromine and Mercury) are liquid at room temperature.

The elements can be divided into groups based on their properties.

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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

Periodic Table of the Elements

The periodic table contains information about each of the elements.

Title: Periodic table (2 of 46)

Atomic Structure

Every element is made up entirely of atoms with a specific number of protons, neutrons, and electrons.

All of the atoms of any element will have the same structure...in other words, the same number of protons, neutrons, and electrons.


Reading the Periodic Table

Cl17

35.453Chlorine

Atomic number

Element name

Symbol

Relative atomic mass



Atomic number

The number of protons in the nucleus. This number will not changefor any element. (If there is a different number of protons, it isn'tthe same element anymore!)

Electrons

The number of electrons will be the same as the number of protons.

Why is this?



Relative Atomic Mass

The atomic mass is the average mass for an atom of the element listed.Not all atoms of the same element have identical atomic mass.

Why?

What do we call atoms of the same element with different atomic mass?



Neutrons

The atomic mass is approximately equal to the total number of protonsand neutrons. So, the number of neutrons can be found by subtracting the atomic number from the atomic mass.

(Unless a specific isotope mass number is given, just round the atomicmass for this)



Cl17

35.453Chlorine

For example, in chlorine, the atomic number is 17. This means there are 17 protons.

How many electrons are there?

The atomic mass is 35.453

This rounds to 35. How many neutrons are there in an average chlorine atom?

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Isotopes are written with the specific mass number of the isotope given.

For example, an some chlorine atoms have 19 neutrons, instead of 18. This isotope is written as Chlorine36.

*Mass number is the total number of protons and neutrons...so an atom of Chlorine36 would have:

36 17 = 19Mass number protons neutrons

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Arrangement of the Periodic Table

Remember that elements are arranged on the table according to their properties, both physical and chemical.

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Metals and Nonmetals

Two major groups of elements are the metals and the nonmetals .

Look at the examples below. Which ones are metals? Nonmetals?How can you tell?

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Properties of Metals and Nonmetals

You can tell the difference between metals and nonmetals by their properties.

Metals Nonmetals

Shiny (lustrous)

Malleable and ductile

Most are good conductors of heat and electricity

Most are solid at room temperature

Form positive ions

React with acids

Dull in color (not shiny)

Brittle (break instead of bending)

Most are poor conductors of heat and electricity

May be solid, gas, or liquid at room temperature

Most form negative ions

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98Cf


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




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





Helium


Periodic Table of the ElementsMost of the elements are metals. They are listed on the left side of the table. Nonmetals are on the right side.The far right are a special group called the inert gases, or noble gases .

The noble gases are special nonmetals that are very unreactive ...in other words, they almost never react with other elements.


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Homework

Read Section 5.5, pages 184187 in your text.

Complete Questions #14 on page 187

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Homework

#1)Metals NonmetalsProperty

Lustre

Conductivity

Location

State

Valence e

Gain/lose

Ionic charge

Other

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Homework

#2) What element is located in the metallic area of the periodic table, but has mainly nonmetallic properties

#3) How many electrons are found in each of the first three orbits for the first twenty elements?

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Arrangement of the Periodic Table

The arrangement of the periodic table also gives information about the structure of the atoms. This reflects the fact that electrons are not just swirling around the nucleus randomly; they are arranged in levels, also called shells or orbits.

Horizontal rows, or periods, on the table contain elements with the same number of electron levels.

Vertical columns, or groups, contain elements with similar electron arrangement, particularly in their outer electron shells.

The outer shell is called the valence shell, and it is this shell which primarily controls how the element behaves during chemical reactions.

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Electron Arrangement into Shells

Each electron shell, or orbit, holds a limited number of electrons:

The first orbit holds up to two electrons

The second orbit holds up to eight electrons

The third orbit holds up to eight electrons

The fifth and sixth orbit can hold up to 18 electrons each, while the sixth and seventh can hold up to 32 electrons each. However, the arrangement of electrons in these levels get a bit more complicated...for our purposes, we'll be sticking mostly to elements with 20 or fewer electrons.

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98Cf


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




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





Helium


Groups and Periods

The each group (the horizontal columns) in the periodic table holds elements which have the same number of valence electrons .



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98Cf


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




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





Helium


Groups and Valence ElectronsFor example, group 1 elements all have a single

valence electron. Group 17 elements are a

single electron short of a full valence shell.


Bohr Diagrams

Chemical reactions between atoms involves movement of electrons; either electrons are exchanged between atoms, or they are shared by atoms.

Only electrons in the outer orbit are involved in chemical reactions. What is the term for electrons in the outer orbit?

When working out how elements combine in chemical reactions, it is helpful to use a model for showing the electron arrangement. Bohr diagrams, developed by Niels Bohr, are a simple way to represent the atoms.

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Bohr Diagrams

Drawing Bohr diagrams is fairly simple, just follow three steps:

1) Draw a circle to represent the nucleus, and write the number ofprotons and neutrons in the circle. (This is different from the waythey are done in your book.)

2) Draw circles to represent the electron orbits. The period inwhich the element is located tells you how many orbits youwill need.

3) Arrange electrons in the orbits, following the 288 rule.Another difference between the way your book shows thesediagrams and the way we will draw them is the arrangementof electrons in the second and third orbits. Draw the first fourelectrons at the top, bottom, left, and right; then, draw thenext four by pairing up the first four.

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Bohr Diagrams

For example, draw the Bohr model to represent a Fluorine atom.

FluorineP: 9N:10E: 9

P: 9N:10

9 protons and 10 neutrons written in the nucleus

2 electrons in the first orbit

7 electrons in the second orbit; four arranged at the top, bottom, left, and right; the next three pairing with the first four

*Note that there are 9 electrons in total...the same as the number of protons

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, #4

From the homework: Draw Bohr diagrams to represent atoms of boron, chlorine, nitrogen, and beryllium.

Boron

P:

N:

E:

P: N:

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, #4


Chlorine

P:

N:

E:

P: N:

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, #4


Nitrogen

P:

N:

E:

P: N:

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, #4


Beryllium

P:

N:

E:

P: N:

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Ions and Ionic Charges

The most stable arrangement of electrons in any orbit occurs when the orbit is full...in other words, when it contains the maximum number of electrons.

When a valence orbit is full, the entire atom has achieved a stable electron arrangement. During a chemical reaction, atoms tend to either gain or lose electrons, moving towards the stable arrangement of a full valence orbit.

What determines whether an atom will gain electrons or lose them? If an orbit is nearly full, it will gain the final few electrons to fill it up.

However, if an orbit is nearly empty, it will let those few electrons go easily, eliminating the orbit completely...and leaving the full lower orbit.

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Ions and Ionic Charge

For example, Fluorine is one electron short of a full valence orbit.


P: 9N:10

Fluorine will pick up the extra electron, filling its valence orbit.

Since the number of protons and electrons is no longer equal, the atom now has an overall charge, and is called an ion


P: 9 +E: 10

Charge: 1 Like Fluorine, most nonmetals gain electrons, and form negative ions

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P: N:

Ions and Ionic Charge

Sodium, on the other hand, has only one valence electron.

SodiumP: 11N:12E: 11

Sodium will lose its valence electron, emptying the orbit and leaving the full orbit below.

Since the number of protons and electrons is no longer equal, the atom now has an overall charge, and is called an ion

SodiumP: 11N:12E: 10

P: 11 +E: 10

Charge: 1+

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Examples:

Draw the stable ion formed by an atom of:

P: N:

Element:

P:

N:

E:

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Examples:


P: N:

Element:

P:

N:

E:

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Examples:


P: N:

Element:

P:

N:

E:

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Examples:


P: N:

Element:

P:

N:

E:

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Noble Gases

What do you notice about the electron arrangement of the noble gases?

How does this relate to their chemical properties?

Two atoms with the same electron arrangement are said to be isoelectronic. When atoms form ions, they gain a full valence orbit, and become isoelectronic with one of the noble gases.

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Homework

Review Section 5.5 (pages 184187) in your text.

Complete Questions #58 on page 187

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Title: Feb 188:36 PM (44 of 46)


66Dy



98Cf


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




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





Helium


Groups and Periods

Some of the groups on the table are given specificnames; elements in these groups share similarchemical properties.


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Periodic Table - Gov 421... · Th90 Pa91 92U Np93 Pu94 Am95 96Cm Bk97 Cf98 Es99 Fm100 Md101 No102...

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