1. Periodic Table

2. first arranged the periodic table
Demtri Mendeleev
first arranged the periodic table
arranged them by atomic mass
he noticed that they had similar chemical and physical properties but some elements were out of order

3. Henry Mosley
Arranged the elements by atomic number
modern table is arranged this way
periodic law: the properties of the elements are periodic functions of their atomic number
Patterns

4. B Si As Ge Sb Te non metals Transition metals Inner transition
Noble Gases
Transition As
Alkaline Earth Metals
Halogens Ge
Alkali Metals Sb Te
metals
Inner transition
Periods
Groups or Families
•vertical columns
• members have the same number of
valance electrons
•members of the group have similar
chemical properties
•horizontal rows
•members have the same # of principal energy levels

5. B, Si, As, Ge, Sb, Te ONLY!!! • Luster • ductile • malleable
Metals
Metalloids
Nonmetals
• Luster
• ductile
• malleable
• good conductors of heat and electricity
• high melting and boiling pt.
• semi-metals
• touch a side of the staircase
Has properties of both metals and nonmetals
• dull
• brittle solids
• poor conductors of heat and electricity
• low melting and boiling pt.
B, Si, As, Ge, Sb, Te
ONLY!!!

6. Group 1 - Alkali Metals valance electron(s) 1 +1 ion
• most active metals
• not found in nature by themselves
• form stable compounds
• can be obtained by electrolysis of fused salt.

7. Group 2 - Alkaline Earth Metals
valance electrons ion
• second most active metal
• some are not found in nature by themselves

8. Group 17 - Halogens •valance electrons 7 •most common ion -1
• have all states of matter at room temp.
F2, Cl2 gases
Br2, liquid
I2, solids
• are the most reactive non metals

9. Group 18 - Noble Gases valance electrons 8 •Inert gases (non reactive)
•have the most stable electron configuration- 8 e in the valence shell
•Kr and Xe can react with fluorine-they have an oxidation number other than 0

10. Transition Elements • many positive oxidation numbers
• valance electrons are in various energy levels --can lose electrons from more than one energy level
• form colored ions in solutions

11. same element in various forms
Diatomic Elements
Allotropes
Liquids
Radioactive
same element in various forms
Different physical and chemical properties
O2 O3
C- graphite diamond
I Bring Clay From
Our New Home
All elements over #82
have no stable
isotopes
Br nonmetal
Hg metal
I2, Br2, Cl2, F2, O2,
N2, H2
all other elements are
monatomic

12. TABLE S NOTE: Leave Room in each box. We will revisit in detail
Ionization Energy
Electronegativity
• amount of energy needed to remove an electron
• the ability of an atom to attract an electron
TABLE S
Periodic Trends
patterns on the
periodic table
Atomic Radius
Reactivity
• distance from the nucleus to the outer most energy level
the ability of a substance to undergo a change

13. •lower the energy -easier to remove • across periods value increases
Ionization Energy
•lower the energy -easier to remove
• across periods value increases
-harder to remove e-’s from non-metals they need more to be stable; easier to remove from metals- they want to get rid of them.
• move down a family (group) decrease
-harder to remove e-’s closer to the (+) nucleus
-(Opposites attract!); easier to remove e-’s farther away shielding by other e-’s

14. • move across a period increases
Electronegativity
• range (4.0 is highest)
• move across a period increases
-non metals want e-’s so they will be
attracted to them; metals want to get
rid of e-’s so they will not be attracted
to them.
• move down a family decreases
-Harder to attract e-’s when there are other e-’s
blocking the pull from the nucleus and repelling
the e-’s.

15. Atomic Radius
• period: decrease as you move across because increase in nuclear charge(+)
•group: increase as we go down
because increasing number of energy levels in an atom

16. Reactivity
• metals: left and down
• most active metal Fr
• nonmetals; right and up
• most active non metal F

17. IE increases
EN increases
Radius decrease
IE decreases
EN decreases
Radius increase
nonmetal
metal
Reactivity

18. Atomic vs. Ionic Size Nonmetals Metals gain electrons lose electrons
become negative ions
Ion is larger than atom
lose electrons
become positive ion
ion is smaller than atom
Cl + 1e Cl-
Na Na+ + 1e