1. Chemical Periodicity Ch.6
Anthony Gates
Chemistry
Unit 4

2. Brief History
Mid-1800’s: only 70 elements were found , but scientist knew many more existed.
Scientists tried to organize the elements by chemical properties, but failed.

3. Dimitri Mendeleev Organized the elements by increasing mass.
Used notecards
Left blank spaces where he knew there was an element, but they weren’t discovered yet.
The result was the first periodic table of elements.

4. Mendeleev cont.
After organizing the table, Mendeleev noticed repeating similarities in chemical and physical properties.

5. The Editing Process
When organizing his table, Mendeleev noticed that Iodine had a smaller mass than Tellurium, but it had more properties in common with bromine and chlorine than tellurium.
Mendeleev switched the places of these elements to match up the properties.
This occurred with a few more elements.

6. Henry Mosely…Rethinking the Table
Discovered that each element has a different number of protons and determined the atomic number for each element.
Arranged the chart according to the atomic number (number of protons) resulting in the Modern Periodic Table.

7. Periodic Law
Periodic Law: when elements are arranged in order of increasing atomic number, there is a periodic repetition of their physical and chemical properties.

8. Parts of the Periodic Table
Periods:
Groups:
Horizontal rows
Side-to-side
7 total
Vertical columns
Up and down
Also called families (share characteristics)

9. Classes of Elements There are three classes of elements: Metals
Nonmetals
Metalloids

10. Metals Majority of the elements
Good conductors of electricity and heat
Shiny/high luster (reflect light)
Ductile
Can be drawn into a wire
Malleable
Can be hammered into thin sheets without breaking

11. Nonmetals Tend to be gasses at room temperature
Poor conductors of heat or electricity
Brittle
Shatter if hit by a hammer

12. Metalloids Stair-step of elements
Individual metalloids tend to share properties of both metals and nonmetals

13. Mission Possible… “Elemental Research”
Your homework is to do a little research:
Pick an element out of the beaker and write down the name of that element on the worksheet. From there you will have to find out information about the element including things like:
Chemical Symbol
Location on the periodic table (group and period number)
Properties (similar to the ones in the last three slides)
Element Class
How is it commonly used in the world?
If you missed this class, I will expect that you will pick any element on the table and fill out the Elemental Research worksheet found on my website.
On my desk will be a beaker with slips of paper that have the names of the elements for students to choose from. If a student complains that they received the same element for their elemental superhero, have them pick a different one.

14. Bellwork
Come up with two properties of metals and two properties of nonmetals with a partner seated near you. (be prepared to share with the class)
Pull out your homework and be prepared to present your finding to the class.

15. Active Metal Group Alkali Metals Alkaline Earth Metals
Very reactive - react violently w/ H2O
Not found freely in nature
Soft metals, silver in color
Alkaline Earth Metals
Reactive Metals < Group 1
Harder, stronger than Group 1

16. Transition Metal Group
Transition Metals:
Outermost s and d orbitals contain electrons
Harder and denser than Active Metal Group (Group 1 & 2)
Less reactive
Found in nature

17. Inner-Transition Metals
Outermost s and f orbitals contain electrons
Lanthanide Series
“Rare” earth metals
Shiny, Reactive
Actinide Series
All unstable and radioactive

18. Halogen Group Halogens Very reactive nonmetals
7e- in outer energy level/shell
Reacts easily to gain 1e- = full shell

19. Noble Gas Group Noble Gases: outer s and p orbitals are full _s2_p6
8e- in outer shell: stable!
Also called the inert gases
They don’t react because they are “happy”
They don’t want to lose or gain electrons

20. Representative Elements
Elements whose s and p orbitals are partially filled
“the 2 towers”

21. Periodic review Which group(s) contain the alkaline earth metals?
Which group(s) contain the noble gases?
Group 18
Which group(s) contain the transition metals?
Groups 3-12

22. Bellwork
With a partner near you, identify where on the periodic table, the following groups of elements are located:
Halogens
Alkaline Earth Metals
Inner Transition Metals
Noble Gases
Alkali Metals
Transition Metals

23. Learning objective
I can describe relative properties of elements based on periodic trends.

24. Periodic Trends
Mendeleev noticed that after creating the periodic table that there was a periodic set of similarities amongst the physical and chemical properties of the elements.

25. Trend: Atomic Size (radius)
One half the distance between the nuclei of two atoms of the same element joined together.

26. Trend: Atomic Radius
Atomic radius increases as you move down the periodic table.
Higher energy levels make the atom larger.

27. Trend: Atomic Radius
Atomic radius decreases as you move to the right on the periodic table.
As you add another proton to the nucleus, the charge pulls the electrons closer to the nucleus, causing a decrease in size.

28. Practice Which of the following pairs has the greater atomic size?
K or Cr
Ga or B
S or Sn

29. Trend: Ionization Energy
The energy required to remove an electron from an atom.
1st ionization energy: energy required to remove the 1st electron from an atom
2nd ionization energy: energy required to remove the 2nd electron from an atom.
3rd, 4th, 5th…

30. Trend: Ionization Energy
Ionization energy decreases as you go down
The attractive force between the nucleus and the electrons is weaker with larger distance.
Less energy is required to overcome this force.

31. Trend: Ionization Energy
Ionization energy increases as you move to the right on the periodic table.
Increased attractive force between nucleus and electrons with more protons.
More energy is required to overcome this force.

32. Practice Which of the following has the greater ionization energy?
Cl or Al
Na or Rb
O or Si

33. Trend: Electronegativity
The ability of an atom to attract electrons when the atom is in a compound.

34. Trend: Electronegativity
Noble Gases are not electronegative because they don’t want to react with other atoms.
Based on a scale from called the Pauling Scale
Fluorine has the highest electronegativity at 4.0

35. Trend: Electronegativity
Electronegativity decreases as you move down a group.
Bonding electrons are farther away; thus the nucleus can’t pull as hard on them.

36. Trend: Electronegativity
Electronegativity increases as you move to the right.
Metals (left): want to lose electrons
LOW electronegativity
Nonmetals (right): want to gain electrons
HIGH electronegativity

37. Practice Which of these has the greater electronegativity? Br or Cu
C or Pb
Ne or N
S or F

38. Bellwork Compare silver and mercury. Which one will have the greater…
Atomic Radius
Ionization Energy
Electronegativity
Discuss with someone near you, why do other elements want to be like the Noble Gases?
Pull out your homework.

39. Learning Objective
I can identify how atoms can become ions and show the correct symbol for a given ion.

40. Atoms vs. Ions
Atoms lose or gain electrons to obtain the electron configuration of a noble gas.
This causes the atom to take on a charge.
Atoms = NEUTRAL
Ions = CHARGED ATOMS

41. Ion Types Positive Ions (Cations): formed by an atom losing electrons
p e charge
Na: 1s22s22p63s none
Na+: 1s22s22p
Ne: 1s22s22p none

42. Ion Types Negative Ions (Anions): formed by an atom gaining electrons
p e charge
O: 1s22s22p none
O-2: 1s22s22p
Ne: 1s22s22p none