1. Periodic Table of Elements

2. Periodic Table
The Periodic Table of the Elements is a chart that displays all of the known elements and contains a great deal of information

3. PToE Organization Metals – left side of PToE Conduct electricity
Malleable
Ductile
Luster
Lose electrons and form cations

4. PToE Organization Nonmetals – right side of PToE and H
Gain electrons and form anions
Lack the properties of metals
Brittle
Dull
Form covalent bonds
Metalloids/Semi-Metals - Stairs
Have properties of both metals and nonmetals

5. PToE Organization
Groups – the vertical columns on PToE; have similar chemical properties
Alkali metals – Group 1
Very active elements
Form ions readily with 1+ charge
Alkaline Earth Metals – Group 2
From ions with 2+ charge
Group 15 & 16
Have all 3 classes of elements (nonmetal, metalloid, metal)
Shows trend in increasing metallic character as you go down a group

6. PToE Organization Halogens – Group 17 Noble Gases – Group 18
All form diatomic molecules
React with metals to form salts
Have all 3 phases of matter at room temperature
Form 1- anions
Noble Gases – Group 18
Exist, under normal conditions, as monatomic gases
Have little chemical reactivity, stable, inert

7. PToE Organization Transition Metals – Groups 3-12
Form multiple cations
Form colored solutions
Periods – horizontal rows of elements
Represent outermost energy level in which there are electrons

8. Periodic Trends Atomic Radius
Half the distance between the nuclei of a diatomic molecule
From left to right across a period, atomic radius decreases (stronger nuclear charge, tighter hold on the electrons)
From top to bottom down a group, atomic radius increases (increase in principle energy levels, another “shell”)

9. Periodic Trends
Ionization Energy – the amount of energy needed to remove the outermost valence electron
Energy is ALWAYS absorbed to lose electrons
Higher IE, less likely to lose an electron
Lower IE, more likely to lose an electron
Lt to Rt across a period, IE will increase (because the electrons are held tighter by the nucleus)
Atoms get smaller, higher attraction for electrons
He will have highest
Top to Bottom down a group, IE will decrease (because the electrons are held less tightly by the nucleus)
Atoms get bigger, lower attraction for electrons
Fr will have lowest

10. Periodic Trends
Electronegativity – the measure of an atom’s attraction for electrons
Noble Gases DO NOT have EN values
Full outer energy level
Stable, do not want to gain or lose electrons
Lt to Rt across a period, EN will increase
Atoms get smaller, greater attraction for electrons
F will have highest EN value at 4.0
Top to Bottom down a group, EN will decrease
Atoms get bigger, lower attraction for electrons

11. Periodic Trends Ionic Radius
Add or lose electrons to gain a noble gas electron configuration
Metals lose electrons, become + (cations) & smaller
When they form ions, the radius gets smaller, nuclear charge remains the same, pulls electrons in tighter
Nonmetals gain electrons, become – (anions) & bigger
When they form ions, the radius gets bigger, nuclear charge remains the same, greater electron repulsion, electrons pull away from nucleus

12. Periodic Trends
Reactivity – how easily an element will form a compound
Most reactive METAL – Fr
Most reactive NONMETAL – F
Metals, as you go down a group, reactivity will increase; across a period, reactivity will decrease – based on Ionization Energy
Nonmetals, as you go down a group, reactivity decreases; across a period, reactivity increases – based on Electronegativity