1. A Little Periodic Table History…

2. History of the Periodic Table
Dmitri Mendeleev, a Russian scientist born in Siberia in 1834, is known as the father of the periodic table of the elements
The periodic table is designed to help you predict chemical and physical properties of elements

3. Method Behind the Madness
Mendeleev set out to find a pattern in the elements
He wrote facts on paper cards for each element
Melting Point
Density
Colors
Atomic Masses

4. Method Behind the Madness (cont)
After laying all of his cards out he noticed that by arranging them according to their properties they were arranged in order of increasing atomic mass
Mendeleev was even able to use the patterns in his table to predict the properties of undiscovered elements
The first periodic table was published in 1869
The Genious of Mendeleev's Periodic Table - TedEd
Mendeleev Song

5. Today, elements are arranged in order of increasing atomic number on the periodic table
Big Science Idea

6. Element Location
Elements are located in three main categories on the periodic table based on their physical properties
Metals
Nonmetals
Metalloids

7. Physical Properties
Physical Property - a property of matter that can be observed or measured WITHOUT CHANGING the substance

8. Examples of Physical Properties
Color/Texture
Mass – How much matter is in an object
Malleable – Can be pounded/rolled into a shape
Ductile – Can be stretched into a long wire
Density – How tightly mass is packed into an object

9. Metals, Nonmetals, & Metalloids

10. Metals
Most elements are metals. The 88 elements to the left of the stair-step line are metals or metal-like elements.
Physical Properties of Metals:
high luster (shininess)
good conductors of heat and electricity
high density (heavy for their size)
high melting point
ductile
malleable

11. Metals

12. Non-Metals
Non-metals are found to the right of the stair-step line. Their characteristics are opposite those of metals.
Physical Properties of Nonmetals:
no luster (dull appearance)
poor conductor of heat and electricity
brittle (breaks easily)
not ductile
not malleable
low density
low melting point

13. Non-Metals

14. Metalloids
Elements on both sides of the zigzag line have properties of both metals and nonmetals. These elements are called metalloids.
Physical Properties of Metalloids:
solids
can be shiny or dull
ductile
malleable
conduct heat and electricity, but not as well as metals
Antimony (Sb)

15. Metalloids

16. Scientists organize elements according to their physical and chemical properties
Big Science Idea

17. How to Read the Periodic Table
The Periodic table is designed to help you predict what an element's physical and chemical properties are
You can also predict what elements will bond with each other

19. Elements are arranged:
Vertically into Groups (also called Families)
Periodic Table Bitesize (only show part 1)
Horizontally Into Periods

20. Periodic Table Arrangement
Groups or Families
Vertical columns on the periodic table
Periods
Horizontal rows of the periodic table

21. Why?

22. If you looked at one atom of every element in a group you would see…

23. Each atom has the same number of valence electrons (the electrons in its outermost shell). Think back to the Bohr Model
An example…

24. The group 2 atoms all have 2 electrons in their outer shells
Be (Beryllium) Atom
Mg (Magnesium) Atom

25. Valence Electrons
Effect the way an atom bonds, which determines many of the chemical properties of the element
Atoms can have anywhere between 1 and 8 valence electrons
This is why elements within a group usually have similar chemical properties

26. Chemical Properties
A chemical property is a characteristic that is observed when a substance changes into a different substance

27. Examples of Chemical Properties
Combustible – capable of igniting at higher temps
Corrosion
Reactivity
Flammable – capable of igniting
Oxidation – rusting or tarnishing

28. Reactivity decreases from left to right
Metals – Reactivity
Reactivity decreases from left to right
Metal Reactivity

29. Nonmetals – Reactivity
Reactivity increases from left to right
Not Reactive X

30. If you looked at an atom from each element in a period
you would see…

31. Each atom has the same number of electron holding shells.
An example…

32. The period 4 atoms each have 4 electron containing shells
4th Shell
K (Potassium)
Atom
Kr (Krypton)
Atom
Fe (Iron) Atom

34. Each group has distinct properties
The periodic Table is divided into several groups based on the properties of different atoms
For example…

35. The periodic table tells us several things…

36. Periodic Table Information on the periodic table: Atomic number
Atomic symbol
Mass number (Atomic Mass)
Element name
Group and period numbers

37. O Think Inside the Box Oxygen 8 16
Atomic Number: Number of protons (also the number of electrons) in an atom of an element. O
Oxygen 16 8
Element’s Symbol: An abbreviation for the element.
Element’s Name
Atomic Mass:
Number of protons + neutrons.

38. Chemical Symbols Shorthand way of representing the elements
Usually one or two letters
Usually taken from the name of the element
Carbon-C, Calcium-Ca, Hydrogen-H, Iodine-I, Oxygen-O, Chlorine-Cl

39. Chemical Symbols Some symbols come from their Latin name:
Gold-Au--aurum
Silver-Ag--argentum
Iron-Fe--Ferrum
Mercury-Hg--hydrogyrum

40. How do we know the number of subatomic particles in an atom?
Atomic number: this number indicates the number of protons in an atom of a particular element
Ex: Hydrogen’s atomic number is 1
So hydrogen has 1 proton
Ex: Carbon’s atomic number is 6
So carbon has 6 protons
**The number of protons is a unique property that identifies an element.
Ex. 2 protons = He, 29 protons = Cu

41. Atomic Mass
Atomic Mass Unit (amu) is used to measure the particles in atoms
Protons & Neutrons are about 1 amu
Electrons are MUCH smaller
It takes about 2,000 electrons to equal 1 amu
Atomic Mass = Protons + Neutrons

42. Li 6.941 3 Mass # Atomic # Symbol
Pick an element off the Periodic Table and draw and label it just like this one!

43. Group and Period Numbers
Group Numbers

44. APEMAN

45. How Can I Find Out the Number of Protons and Electrons?
Atomic No. = # of protons
Since protons & electrons are EQUAL...the atomic no. also tells you the # of electrons
*Atomic # = # of Protons = # of electrons*

46. Atomic # = # of Protons = # of electrons
APE
Let’s take a look:
A = Atomic number
P = Number of protons
E = Number of electrons
These are all the same number!! So
Atomic # = # of Protons = # of electrons

47. Neutrons = Mass Number – Atomic Number
Then How Can I Find Out the Number of Neutrons?
Mass Number = number of protons + number of neutrons So
Neutrons = Mass Number – Atomic Number

48. MAN Now let’s look at MAN: M= Atomic Mass - A= Atomic Number
N= # of Neutrons
Simple math!
Mass minus atomic number gives you the number of neutrons!!!

49. APEMAN
Let’s work a couple together
Let’s try Nitrogen!

50. Nitrogen
Boron 5 7 A= P= E= M=
-A= N=
A= P= E= M= -A= N= 5 7 5 7 11 14 5 7 6 7

51. Now that we know how to figure out protons, electrons, and neutrons…
Let’s try to create a Bohr Model

52. Lithium Li Lithium Electrons =
Atomic Structure
Electrons =
3 (2 in the 1st shell, 1 in the 2nd shell) - + 3 Li
Lithium 7
Protons
= 3
Neutrons =
4 (7-3 = 4)

53. Protons determine an element’s identity and valence electrons determine its chemical properties
Big Science Idea

54. SUMMARY The Atomic Number of an atom = number of
protons in the nucleus.
The Atomic Mass of an atom = number of
Protons + Neutrons in the nucleus.
The number of Protons = Number of Electrons.
Electrons orbit the nucleus in shells.
Each shell can only carry a set number of electrons.