A Guided Tour of the Periodic Table

Section 3.2

Using the Periodic Table

Atomic number – the number of protons in the nucleus of an atom or the number of electrons in the nucleus of an atom.

ALWAYS TRUE!!!!!

The elements are inorder of Periodic Tableby the # of protons presentin the nucleus.

Using the Periodic Table

Mass number – the TOTAL number of protons and neutrons in the nucleus of an atom; may change.

Using the Periodic Table

Ions: 1. Ionization – the process of adding electrons

to or removing electrons from an atom or group of atoms.

2. Ion – an atom or group of atoms that has lost or gained one or more electrons and therefore has a net electric charge.

Using the Periodic Table

Ions:Cation – an ion with a positive charge. (Lithium, Li)

Li+

IonsAnion – an ion with a negative charge (Flourine, F)

F-

Using the Periodic Table

Isotopes- any atoms having the same number of protons but DIFFERENT number of neutrons.

See fig 3-17 on pg 84 in textbook

SymbolAtomic Mass

Atomic Number

Charge (if ion)

HHydrogen

1

1

Protons: 1Neutrons: 0Electrons: 1

NaSodium

23

11

Protons: 11Neutrons: 12Electrons: 11

EXAMPLEHow many protons, neutrons and electrons are found in an atom of

13355 Cs

Atomic number = protons and electronsThere are 55 protons and 55 electrons

Mass number = sum of protons and neutrons133 – 55 = 78

There are 78 neutrons

Atomic Mass Unit (AMU) – a quantity equal to 1/12 of the mass of a Carbon-12 atom

Average Atomic Mass- the weighted average of the masses of all naturally occurring isotopes of an element.

Organization of the P.T.

Periodic Law: properties of elements tend to change in a regular pattern when elements are arranged in order of increasing atomic number, or number of protons in their atoms.

The Periodic Table

Over 100 years ago, the chemist Mendeleev arranged the known elements in order of increasing atomic mass.

He noticed a repeating pattern in theproperties of the elements.He designed a table with rows and columns toshow the repeating patterns.

Mendeleev left blank spaces in his table when the properties of the elements above and below did not seem to match.

The existence of unknown elements was predicted by Mendeleev on the basis of the blank spaces.

When the unknown elements were discovered, it was found that Mendeleev had closely predicted the properties of the elements as well as their discovery.

The Periodic Table

In the Modern Periodic Table . . .

Elements are arranged by increasing atomic numbers.

The term “periodic” part means that similar properties repeat every so often.

There are currently 118 known elements.

Rows of the Periodic Table

The beginning of the row is where the patterns that Mendeleev discovered begin repeating again.

What the table tells you . . .

Each box contains information about one of the elements.

- Atomic Number- Chemical Symbol- Name of Element- Atomic Mass

Some tables give more information for each element.

Periodic Table

The color of the box tells you if the state of the element at room temperature and pressure is a solid, liquid, or gas.

Most are solids, some are gases, and two are liquids.

The stair-step line separates metals from non-metals.

Metals are to the left of the stair-step line; non-metals are to the right.

Using the Periodic Table 1. Period a horizontal row of elements in

the periodic table

2. Determines electron arrangement

Using the Periodic Table

Groups (family) – a vertical column of elements in the periodic table.

Same number of valence electrons in each group therefore they have similar properties.

Examples: Cl (Chlorine) and F (Flourine)These are both Halogens and have very similar properties.

Columns on the Periodic Table

There are 18columns orgroups.

The elements ineach group resemble eachother – the react similarly to other substances.

How are elements classified?

A: Metals vs. Nonmetals

1: Elements can be put in various types of categories based on their physical and chemical properties.A common physical property used to classify elements are metallic and nonmetallic properties.

Periodic Table: Metallic arrangement

Layout of the Periodic Table: Metals vs. nonmetals1

IA18

VIIIA

1 2IIA

13IIIA

14IVA

15VA

16VIA

17VIIA

2

3 3IIIB

4IVB

5VB

6VIB

7VIIB

8 9VIIIB

10 11IB

12IIB

4

5

6

7

MetalsNonmetals

Periodic Table: The three broad ClassesMain, Transition, Rare Earth

Main (Representative), Transition metals, lanthanides and actinides (rare earth)

Metals vs Nonmetals

Metallic properties include:A. ShinyB. Conduct Heat/ElectricityC. Ductile/MalleableD. Have a positive Oxidation NumberE. Found on the Left/Middle of the Periodic Table

Metals vs Nonmetals

Nonmetallic properties include:a. Dullb. Poor conductor of Heat/Electricity (INSULATORS)c. Brittled. Have a Negative Oxidation Numbere. Found on the Right Side of P.T.

Metals vs Nonmetals

Some elements have properties of both metals and nonmetals and are referred to as metalloids.

Metalloids are usually nonmetals that can conduct heat and electricity.

The metalloids are located between the metal and nonmetal sides of the periodic table.

Metals vs Nonmetals

There are 109 total elements on the periodic table.

Out of the 109 elements, 84 are metals, 17 nonmetals and 8 metalloids (semiconductors)

Families

FAMILIES OF ELEMENTS

Elements are put into families based on similarities of chemical properties.

Families

Families of Periodic Tablea. ALKALI METALS – 1 (IA)b. ALKALINE EARTH METALS – 2 (IIA)c. TRANSITION METALS – 3-12 (B Groups)d. HALOGEN GROUP – 17 (VIIA)e. NOBLE GASES – 18 (VIIIA)

ALKALIE METALS (IA)

Group IA elements on P.T. With EXCEPTION of Hydrogen (H), they are the

MOST Metallic elements on the table. Best conductors of heat and electricity Most reactive metals on earth Never found free, always found in a

compound.ALL HAVE ONLY 1 VALENCE

ELECTRON

Alkaline Earth Metals (IIA)

Group IIA on P.T. Not as reactive as the group IA metals Still very reactive Never found free in natureALL HAVE 2 VALENCE ELECTRONS

TRANSITION METALS (IIIB – IIB)

A majority of the elements on the periodic table are transition metals.

Names given based on their decreasing metallic characteristics as one moves from the left to the right side of the periodic table.

HALOGENS

Found in group VIIA Known as the Salt Forming elements HALO- means “salt forming” Most reactive nonmetals NEVER found free in nature Usually found in salt compounds containing

a metal from either alkali or alkaline earth metal families.

NOBLE GASES

Group VIIIA ALL Nonreactive Nonmetals Only elements known that have a naturally

FULL Valence Shell (Outer energy level) Since nonreactive, then they will

ALWAYS be found FREE in nature and NEVER in a compound.

Periodic Table e- configuration from the periodic table

(To be covered in future chapters)

B2p1

1IA

18VIIIA

1 2IIA

13IIIA

14IVA

15VA

16VIA

17VIIA

2

3 3IIIB

4IVB

5VB

6VIB

7VIIB

8 9VIIIB

10 11IB

12IIB

4

5

6

7

H1s1

Li2s1

Na3s1

K4s1

Rb5s1

Cs6s1

Fr7s1

Be2s2

Mg3s2

Ca4s2

Sr5s2

Ba6s2

Ra7s2

Sc3d1

Ti3d2

V3d3

Cr4s13d5

Mn3d5

Fe3d6

Co3d7

Ni3d8

Zn3d10

Cu4s13d10

B2p1

C2p2

N2p3

O2p4

F2p5

Ne2p6

He1s2

Al3p1

Ga4p1

In5p1

Tl6p1

Si3p2

Ge4p2

Sn5p2

Pb6p2

P3p3

As4p3

Sb5p3

Bi6p3

S3p4

Se4p4

Te5p4

Po6p4

Cl3p5

Be4p5

I5p5

At6p5

Ar3p6

Kr4p6

Xe5p6

Rn6p6

Y4d1

La5d1

Ac6d1

Cd4d10

Hg5d10

Ag5s14d10

Au6s15d10

Zr4d2

Hf5d2

Rf6d2

Nb4d3

Ta5d3

Db6d3

Mo5s14d5

W6s15d5

Sg7s16d5

Tc4d5

Re5d5

Bh6d5

Ru4d6

Os5d6

Hs6d6

Rh4d7

Ir5d7

Mt6d7

Ni4d8

Ni5d8

Summary

Periodic Table: Map of the Building block of matterType: Metal, metalloid and Nonmetal

Groupings: Representative or main, transition and Lanthanide/Actinides (rare)

Family: Elements in the same column have similar chemical property because of similar valence electronsAlkali Metal, Alkaline Earth Metal, halogens, noble gases

Period: Elements in the same row have valence electrons in the same shell.

Iron Triad

Iron (Fe)Cobalt

(Co)Nickel

(Ni)

Coinage Elements

Copper (Cu)

Silver (Ag)

Gold (Au)

Liquid @ Room Temp

Mercury (Hg) and Bromine (Br)