S

The Periodic TableJ. Bishop

History of the Periodic Table

Dmitri Mendeleev : Father of the Periodic

Table

S 1st Periodic Table

S Organized PT by increasing atomic mass

S Left spaces

S Predicted properties of unknown elements

Mendeleev’s Table

History of the Periodic Table

Henry Moseley: Modern Periodic Table

S Put elements in order by atomic number

Periodic Table Organization

Columns

S Vertical Groups/Families

S Same number of valence electrons

S Similar Properties

Each element in

group 2 has 2 valence

electrons

Periodic Table Organization

Periods

S Horizontal rows

S Same number of energy levels.

Each element in

period 4 has four

energy levels

Periodic Table Organization

The Periodic Table is divided into regions

based on general properties

S Metals

S Non-metals

S Metalloids

Metals

S Left side of the stairs

S Forms cations by losing electrons

S High Melting Points

S Metallic luster (shiny)

S Malleable (bendable) and ductile (makes wires)

S Good conductors of heat and electricity

Non-metals

S Right side of the stairs

S Form anions by gaining electrons

S Low Melting Points

S Insulators (poor conductors or heat & electricity)

Metalloids

S Have properties of both metals and non-metals

S Semi-conductors

S

Groups

Hydrogen

SBelongs to a family of its

own.

S Is a diatomic, reactive gas.

S It is a NONMETAL!!

SWas involved in the

explosion of the

Hindenberg.

S Is promising as an

alternative fuel source for

automobiles

S Group 1

S 1 valence electrons

S Soft, Silvery

S Most reactive group of metals

Alkali Metals

S What trend in reactivity is seen

amongst the alkali metals?

SWhat would you expect from

Francium?!?!

Alkali Metal Video

S Group 2

S 2 valence electrons

S Silvery

S Fairly reactive

Alkaline Earth Metals

S d sublevel

S Most are good

conductors of

heat &

electricity

S Malleable

(easily bent or

hammered into

wires or sheets)

Transition Metals

Halogens

S Group 17

S 7 valence electrons

S Most reactive group of nonmetals

Halogens

SWhat trend in reactivity is seen

amongst the Halogens?

Noble Gases

S Group 18

S 8 valence electrons

S Unreactive

S Gases at room temperature

Jellyfish lamps

Lanthanides & Actinides

S Located at the bottom of the Periodic Table

S Rare Earth Metals

ALIEN PERIODIC TABLE

S

Periodic Trends

Periodicity

S Periodicity refers to the recurring trends

that are seen in the element properties.

S Trends move left, right, up, and down

across the periodic table.

Reactivity of Metals

S Describes the reactivity of metals.

S Reactivity of metals increases down the columns and to

the left across the periods on the periodic table.

Why?S Increase in the size of the atom (value of n)

S Weaker nuclear charge (# protons)

S Low electronegativity & low ionization energy

Fr

Reactivity of Nonmetals

S Describes the reactivity of nonmetals.

S Reactivity of nonmetals increases up the columns and to

the right across the periods on the periodic table.

Why? S Decrease in the size of the atom (value of n)

S Stronger nuclear charge (# protons)

S High electronegativity & high ionization energy

F

Atomic Radius

S Atomic radius is ½ the distance between two adjacent

nuclei. (size of the atom)

S Atomic radius increases down the columns and to the

left across the periods on the periodic table.

Why? S Increase in energy levels

S Weaker nuclear charge(# protons)

S Low electronegativity &low ionization energy

Reactivity of Metals

Fr

Which element is the biggest?

Atomic Radii

Learning Check

Out of each pair pick which metal is most reactive

1. Mn & Ca

2. Zn & Cd

3. Rb & Sr

Out of each pair pick which nonmetal is most reactive

4. F & Cl

5. C & N

6. P & O

Out of each pair pick which element has the greatest atomic

radius.

7. He & Ne

8. Ru & Co

9. Hf & Ta

Ionic Radius

S Ionic Radius is the size of the ion

S Positive Ions (cations) The more electrons an atom loses the smaller the ion

S Negative Ions (anions) The more electrons an atom gains the larger the ion

S

cations anions

Ca atom Ca+2 ion Cl atom Cl-1 ion

the size of an ion

20 p+

20 e–

20 p+

18 e–

17 p+

17 e–

17 p+

18 e–

Ca Ca2+ Cl Cl1–

cations lose electrons-

smaller

Anions gain electrons

larger

Ionic Radius

Ionization Energy

S Ionization Energy is the energy need to remove a

valence electron from an atom.

S Ionization energy increases up the columns and to the

right across the periods on the periodic table.

Why? S Size of atom decreases

S Increase in nuclear charge

He

Electronegativity

S Electronegativity is the tendency for an atom to attract

electrons to itself in a chemical bond.

S Electronegativity increases up a column and to the right

across a period on the periodic table.

Why? S Size of atom decreases.

S Increase in number of valence electrons

F

Vocabulary

1. Mendeleev

2. Moseley

3. Period

4. Group

5. Metals

6. Nonmetals

7. Metalloids

8. Alkali Metals

9. Alkaline Earth Metals

10. Transition Metals

11. Halogens

12. Noble Gases

13. Lanthanides

14. Actinides

For the following you must

define the trend and explain

WHY!!!

15. Reactivity of Metals

16. Reactivity of Nonmetals

17. Atomic Radius

18. Ionic Radius

19. Ionization Energy

20. Electronegativity