1. Monday, May 8th Entry Task Schedule:
Why is a positive ion smaller than a neutral atom? Why is a negative ion larger than a neutral atom?
Schedule:
Isotope practice set Periodic table intro
Objective: I will use the periodic table to solve puzzles and answer questions
Homework
Complete handouts if not finished in class
Read 5.2
Please have on desk:
ISN, Made to Order activity

2. Tuesday, May 9th
Entry Task The most common form of chlorine is chlorine-35. How is chlorine-37 the same? How is it different?
Schedule:
Periodic table organization
Objective: I can describe the organization of the modern periodic table.
Homework
Re-read 5.2
Please have on desk:
ISN open to periodic table puzzles

3. Historical Development and Current Structure
The Periodic Table of the Elements
Historical Development and Current Structure

4. Historical Background
The first scientific discovery of an element was in 1649 by Hennig Brand who discovered phosphorus.
By 1869, a total of 63 elements had been discovered.
As the number of known elements grew, scientists began to recognize patterns in their properties and began to develop classification schemes.

5. Hennig Brand & Phosphorus

6. Historical Breakthroughs
1860 Dmitri Mendeleev began thinking about how he could organize the elements based on their physical and chemical properties.
Mendeleev liked card games so he made a set of card with each element on it and spent hours trying to arrange the cards into a pattern.

7. Dmitri Mendeleev
He figured out a way to organize the elements using the properties of the elements on the cards.
Instead of similar suits (heart, spade, etc) he did similar properties
He used increasing atomic mass-the average mass of all the element’s isotopes.
Mendeleev produced the first periodic table of the elements in 1869.

9. Henry Moseley
Henry Moseley, a British Physicist, was able to determine by 1914 the atomic numbers of all the known elements using an experimental technique.
Moseley then proceeded to rearrange the elements according to increasing atomic numbers.
Moseley's periodic law is now considered the current Periodic Law.

10. Glenn Seaborg
Glenn Seaborg, an American chemist discovered plutonium in 1940.
He discovered all the special state transition metal elements from 94 to 102 in the 1950’s.
He reconfigured the periodic table by placing the actinide series below the lanthanide series.

11. Historical Breakthroughs
Mendeleev Moseley Seaborg

12. Current Structure
The elements are arranged in increasing order of atomic number as you go from left to right across the table.
The horizontal rows are called periods; there is a progression from metals to non-metals across each period.
The vertical rows are called groups or families; elements in each group share similar physical and chemical properties.

13. Current Structure
Examples of elemental families - Alkali metals (1); Alkaline earth metals (2); noble gases (18).
Transition metals: Similar in many ways, they are often used as catalysts.
Lanthanides: (Elements 58 to 71) are found on earth in only very small amounts.
Actinides: (Elements 90 to 103) include most of the well known elements which are found in nuclear reactions.

14. Current Structure
The elements with larger atomic numbers than 92 do not occur naturally. They have all been produced artificially by bombarding other elements with particles.
What is the Periodic Table of The Elements? "It is a huge, efficient resource!"

15. Your turn!
Read pages 150 and What are the trends in the periodic table?

16. Reading Each Element ATOMIC NUMBER - # of protons
CHEMICAL SYMBOL- abbreviation of name
NAME – full name of the element
ATOMIC MASS- average atomic mass of all the isotopes of the element
Atomic Number
Chemical Symbol
Name
Atomic mass

17. Periods Horizontal row
Change from metal to non metals going from left to right
Not much else is similar

18. Trends Atoms form ions by losing or gaining electrons
Group 1 atoms lose an electron to form ions with 1+ charge
Group 2 atoms lose two electrons to form ions with a charge of 2+
Group 18 do not form ions
Group 17 gain an electron to form a 1- ion
Group 16 gain two electrons to form 2- ion
Group 3-12 form ions but they are different and charges can vary

19. More Trends

20. Wednesday, May 10th
Entry Task What is the most common element in the universe? What are the two most common elements in the human body?
Schedule:
Getting to know the periodic table
Objective: I will diagram the periodic table of the elements
Homework:
Complete steps 1-11
Please have on desk:
ISN

21. Turn to page 105 in your journal
Divide the page in half (hamburger).

22. On the top half, draw and complete these two tables
Na-12
Na-20
#p+
#n0
#e-
Se-50
Se-55
#p+
#n0
#e-

23. On the bottom half, draw and label a Be2+ ion And label an O2- ion
Be sure to show the number of protons and neutrons in the nucleus and the electrons in their energy levels outside the nucleus (use your structure of the atom handout to help you.)

24. Thursday, May 11th Entry Task Schedule:
Explain how you would determine the number of protons, neutrons, and electrons in an element.
Schedule:
The periodic table is a map of the elements
Objective: I can classify elements as metals, nonmetals, & metalloids
Homework:
Read 5.3 carefully
Please have on desk:
Getting to know the periodic table sheet

25. The periodic table has distinct regions
An element’s position on the periodic table helps you predict it’s physical and chemical properties as well as it’s chemical behavior.
Metals (except hydrogen) are on the left, nonmetals (except hydrogen) on the right, metalloids are in between.

26. Groups Run vertically Numbered from 1-18
Show similarities in their chemical and physical properties
Can be called a family of elements because they seem to be related
Same number of valence electrons in the outer energy level

27. Metals In general, metals are elements that: form cations
conduct electricity
conduct heat
are shiny
are solid at room temp (except Hg)
are malleable (shaped by pounding)
are ductile (can be drawn into wire)

28. Reactive Metals
The term reactive indicates how likely an element is to undergo a chemical change.
Group 1 is the most reactive of the metals.
Group 2 is the second most reactive of the metals.

29. Group 1: Alkali metals
They have 1 valence electron in the outer energy level.
They readily give up that electron to form a +1 ion.
- solid
- reactive violently with water
- shiny
- low density

30. Group 1: Alkali metals
Na+ and K+ are essential for properly functioning cells

31. Group 2: Alkaline Earth metals
They have 2 valence electrons in the outer energy level.
They readily give up those electrons to form a +2 ion.
- solid
- silver colored
- more dense than alkali metals
- very reactive, less than alkali
metals though

32. Group 2: Alkaline Earth metals
Ca+2 is essential for bones and teeth
Magnesium is light & inexpensive and combined with other metals to make things such as airplane frames, engine blocks, transmission blocks…

33. Groups 3-12: Transition metals
Have 1 or 2 valence electrons
Less reactive than group 1 or 2 metals
Good conductors of heat, electricity
Higher densities
Group 11 metals are easily shaped
Important in industry, construction, and technology

34. Groups 3-12: Transition metals
Au and Ag – coins and jewelry
Cu – pipes, wire
Zn and Ni – coins
W – filiments
Pt – catalytic converters
Fe – used in steel
Brass – alloy of Cu and Zn

35. Lanthanides: Rare Earth Elements
Elements in period 6
3 valence electrons
Very reactive
High luster, tarnish easily
High conductivity for electricity
Very small differences between them

36. Group 13: Boron group Contains 1 metalloid and 4 metals
3 valence electrons in the outer energy level
They are reactive and solid at room temperature

37. Friday, May 12th Entry Task List 5 properties of metals. Schedule:
Nonmetals
Objective: I can describe properties of nonmetals, halogens, noble gases, and chalcogens
Homework
Complete the handout
Please have on desk:
ISN

38. Nonmetals
In general, nonmetals have properties that are opposite of metals.
They also have more variable properties.
Solid, liquid, or gas
Solids are dull, brittle, poor conductors of heat and electricity

39. Group 17: Halogens From Greek words meaning “forming salts”
The most reactive nonmetals
Have 7 valence electrons
Easily gain an electron to form a -1 anion
Never found uncombined in nature

40. Group 17: Halogens React violently with alkali metals to form salts
Chlorine used to clean drinking water, swimming pools
Iodine used to kill germs on skin

41. Group 18: Noble Gases
Have 8 valence electrons (except Helium which has 2)
Least reactive group of elements
Colorless, odorless gases
Found in the atmosphere

42. Group 18: Noble Gases
Inert gases almost never react with other elements
Neon, krypton, xenon, and argon gases are uses in colorful lights
Argon used in tungsten filament bulbs because it is nonreactive
Radon is radioactive and can cause lung damage

43. Hydrogen stands apart
Hydrogen is set apart because its properties does not match any single group
1 valence electron, easily forms a +1 cation.
Properties are similar to nonmetals rather than metals

44. Group 16: Chalcogens Also known as the oxygen group
6 valence electrons, gains 2 electrons to form a -2 anion
Reactive with both metals and nonmetals
All but oxygen are solid at room temperature
Contains: 3 nonmetals, 2 metalloids

45. Group 15: Nitrogen group
5 valence electrons, gains 3 electrons to form a -3 anion
Reactivity varies
All but nitrogen are solid at room temperature
Contains: 2 nonmetals, 2 metalloids, and 1 metal

46. Group 14: Carbon group 4 valence electrons
Carbon and silicon usually do not form ions
Tin and lead form ions
All are solid at room temperature
Contains: 1 nonmetal, 2 metalloids, and 2 metals