1. A Guided Tour of the Periodic Table
Chapter 3 Section 2 Notes
A Guided Tour of the Periodic Table

2. Who is Dmitri Mendeleev? (1834-1907)
In 1869, Dmitri Ivanovitch Mendeléev created the first accepted version of the periodic table.

3. What is the Periodic Table?
Shows all known elements in the universe
Organizes elements by chemical properties

4. The Periodic Table
The periodic table groups similar elements together. This organization makes it easier to predict the properties of an element based on where it is in the periodic table.

5. Cu C Carbon Copper Elements
Elements in the periodic table are represented by their symbols.
The first letter is ALWAYS capital
If there is a second letter, it is ALWAYS lowercase
Every element has its own unique symbol Cu C
Carbon
Copper

6. How is the Periodic Table Organized?
The elements are arranged based on the number of protons in the nucleus.
Periodic Law: states that when elements are arranged in order of increasing atomic number, similarities in their properties will occur in a regular pattern.

7. Periods in the Periodic Table
Period: a horizontal row of elements in the periodic table
As you move from left to right in a period, the number of protons and electrons increases by one
Elements in the same period DO NOT have similar properties; in fact, they change greatly across the row
The first element in a period is always an extremely active solid. The last element in a period, is always an inactive gas.

9. Groups or Families in the Periodic Table
Group or family: a vertical column of elements in the periodic table
All elements in a family have the same number of valence electrons, so they have similar properties
For example, lithium (Li), sodium (Na), potassium (K), and other members of group 1 are all soft, white, shiny metals.
These elements are NOT exactly alike because they have different numbers of protons

11. Ions
Ionization: the process of adding electrons to or removing electrons from an atom
Ion: an atom that has lost or gained one or more electrons and has a net electric charge
Cation: an ion with a positive charge
Anion: an ion with a negative charge

12. Goal of Atoms All atoms want to have a FULL outermost energy level
They do this by gaining, losing, or sharing electrons

13. Metals and Electrons 3 p+ 3 p+ 4 n0 4 n0
Metals LOSE electrons to form cations
Example: Lithium loses one electron to become a lithium ion, written as Li+
Second energy level can hold up to 8 e-. It is easier to lose 1 e- than gain 7 more.
3 p+
4 n0
3 p+
4 n0
After lithium loses an electron, it has a full outermost energy level.
2 electrons
3 electrons

14. Nonmetals and Electrons
Nonmetals GAIN electrons to form anions
Example: Fluorine gains one electron to become a fluoride ion, written as F-
Second energy level can hold up to 8 e-. It is easier to gain 1 e- than lose 7 more.
9 p+
10 n0
9 p+
10 n0
After fluorine gains an electron, it has a full outermost energy level.
9 electrons
10 electrons

15. So, how do compounds form?

16. So, how do compounds form?

17. So, how do compounds form?

18. Atomic Number
Atomic Number: how many protons are in the nucleus of an atom
Remember that ATOMS are neutral, so they have equal numbers of protons and electrons
Therefore, atomic number also tells the number of electrons for atoms only

19. Mass Number (Atomic Mass)
Mass Number: the number of protons and neutrons in an atom
Mass number is ONLY protons and neutrons because they provide most of an atoms mass
The same element can have different mass numbers because they may have different numbers of neutrons.

20. Isotopes
Isotopes: atoms of the same element having the same number of protons but different numbers of neutrons
Each “version” of the atom has the same number of protons and electrons

21. Isotopes Some isotopes are more common than others
For example, protium is found most often

22. Calculating Neutrons in an atom
To calculate the number of neutrons in an atom, take mass number minus atomic number.
Mass Number
- Atomic Number
# of Neutrons

23. Average Atomic Mass
In the periodic table, the atomic mass is a decimal because it is an average of all the naturally occurring isotopes
When calculating neutrons from average atomic mass, round to the nearest whole number
Example: How many neutrons are in Zinc? (Atomic Number 30; Average atomic mass 65.39)
65-30 = 35 neutrons

24. How do you read the Periodic Table?