1. A Guided Tour of the Periodic Table
Section 3.2

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 in
order of Periodic Table
by the # of protons present
in the nucleus.

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

4. 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.

5. Using the Periodic Table
Ions:
Cation – an ion with a positive charge. (Lithium, Li)
Li+

6. Ions
Anion – an ion with a negative charge (Flourine, F) F-

7. 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

8. Charge (if ion)
Atomic Mass
Symbol
Atomic Number

9. Hydrogen
Protons: 1
Neutrons: 0
Electrons: 1 H 1 1

10. Sodium
Protons: 11
Neutrons: 12
Electrons: 11 Na 23 11

11. Cs 133 55 EXAMPLE How many protons, neutrons and
electrons are found in an atom of
133 55 Cs
Atomic number = protons and electrons
There are 55 protons and 55 electrons
Mass number = sum of protons and neutrons
133 – 55 = 78
There are 78 neutrons

12. 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.

13. 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.

14. 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 the
properties of the elements.
He designed a table with rows and columns to
show the repeating patterns.

15. The Periodic Table
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.

16. 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.

17. Rows of the Periodic Table
The beginning of the row is where the patterns that Mendeleev discovered begin repeating again.

18. 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.

19. 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.

20. Using the Periodic Table
1. Period  a horizontal row of elements in the periodic table
2. Determines electron arrangement

21. 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.

22. Columns on the Periodic Table
There are 18
columns or
groups.
The elements in
each group
resemble each
other – the react
similarly to other
substances.

23. 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.

24. Periodic Table: Metallic arrangement
Layout of the Periodic Table: Metals vs. nonmetals
Nonmetals
Metals

25. Periodic Table: The three broad Classes Main, Transition, Rare Earth
Main (Representative), Transition metals, lanthanides and actinides (rare earth)

26. Metals vs Nonmetals Metallic properties include: A. Shiny
B. Conduct Heat/Electricity
C. Ductile/Malleable
D. Have a positive Oxidation Number
E. Found on the Left/Middle of the Periodic Table

27. Metals vs Nonmetals Nonmetallic properties include: a. Dull
b. Poor conductor of Heat/Electricity (INSULATORS)
c. Brittle
d. Have a Negative Oxidation Number
e. Found on the Right Side of P.T.

28. 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.

29. 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)

30. Families FAMILIES OF ELEMENTS
Elements are put into families based on similarities of chemical properties.

31. Families Families of Periodic Table a. 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)

32. ALKALIE METALS (IA) ALL HAVE ONLY 1 VALENCE ELECTRON
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

33. Alkaline Earth Metals (IIA)
Group IIA on P.T.
Not as reactive as the group IA metals
Still very reactive
Never found free in nature
ALL HAVE 2 VALENCE ELECTRONS

34. 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.

35. 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.

36. 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.

37. Periodic Table e- configuration from the periodic table (To be covered in future chapters)Li
2s1 Be
2s2 B
2p1 C
2p2 B
2p1 N
2p3 O
2p4 F
2p5 Ne
2p6 Na
3s1 Mg
3s2 Al
3p1 Si
3p2 P
3p3 S
3p4 Cl
3p5 Ar
3p6 K
4s1 Ca
4s2 Sc
3d1 Ti
3d2 V
3d3 Cr
4s13d5 Mn
3d5 Fe
3d6 Co
3d7 Ni
3d8 Cu
4s13d10 Zn
3d10 Ga
4p1 Ge
4p2 As
4p3 Se
4p4 Be
4p5 Kr
4p6 Rb
5s1 Sr
5s2 Y
4d1 Zr
4d2 Nb
4d3 Mo
5s14d5 Tc
4d5 Ru
4d6 Rh
4d7 Ni
4d8 Ag
5s14d10 Cd
4d10 In
5p1 Sn
5p2 Sb
5p3 Te
5p4 I
5p5 Xe
5p6 Cs
6s1 Ba
6s2 La
5d1 Hf
5d2 Ta
5d3 W
6s15d5 Re
5d5 Os
5d6 Ir
5d7 Ni
5d8 Au
6s15d10 Hg
5d10 Tl
6p1 Pb
6p2 Bi
6p3 Po
6p4 At
6p5 Rn
6p6 Fr
7s1 Ra
7s2 Ac
6d1 Rf
6d2 Db
6d3 Sg
7s16d5 Bh
6d5 Hs
6d6 Mt
6d7

38. Summary Periodic Table: Map of the Building block of matter
Type: 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 electrons
Alkali Metal, Alkaline Earth Metal, halogens, noble gases
Period: Elements in the same row have valence electrons in the same shell.

39. Iron Triad
Iron (Fe) Cobalt (Co) Nickel (Ni)

40. Coinage Elements
Copper (Cu) Silver (Ag) Gold (Au)

41. Mercury (Hg) and Bromine (Br)
Room Temp
Mercury (Hg) and Bromine (Br)