1. Atoms and Elements: Are they Related?
Fall 2011

2. ATOMS ALL MATTER IS MADE OF ATOMS
Definition: ATOMS ARE THE SMALLEST PIECE OF MATTER and CANNOT BE BROKEN DOWN INTO A SIMPLER SUBSTANCE.

3. ATOMS HAVE 3 BASIC PARTS
(Subatomic Particles)
PROTONS
NEUTRONS
ELECTRONS

4. PROTONS (POSITIVE CHARGE)
ARE FOUND IN THE NUCLEUS AND MAKE UP MOST OF THE MASS OF THE ATOM.
VERY IMPORTANT!!! The number of protons an atom has tells you what kind of atom it is!!!!

5. The Atomic Number is the number of Protons
Pg. 158

6. NEUTRONS (NO CHARGE)
ARE FOUND IN THE NUCLEUS
MAKE UP PART OF THE MASS OF THE ATOM

7. Finding the Number of Neutrons for an Atom
The protons and neutrons make up the mass of an atom.
If you know the protons (atomic number) then you can find the number of neutrons by subtracting the atomic mass from the # of protons (atomic number).
atomic mass - # of protons = # of neutrons

8. ELECTRONS (NEGATIVE CHARGE - )
FOUND IN THE ELECTRON SHELL (cloud) ORBITING THE NUCLEUS.
TAKES UP MOST OF THE SPACE IN AN ATOM.
The # of electrons = the # of protons

9. Label the atom below on your packet!
What type of atom is this?
How do you know?

10. Let’s Break for Questions???
How many protons should Hydrogen have?
How about Oxygen?
Which particles are located in the nucleus of an atom?
Where are the electrons located?

11. Atomic Size
-A typical atom is about one ten-billionth of a meter in diameter. (THAT’S REALLY, REALLY SMALL AND WHY WE CAN’T SEE THEM WITH A REGULAR MICROSCOPE)
-ATOMIC MASS = Protons + Neutrons.
-Most of the atomic mass comes from the nucleus.
-Electrons weigh very little. That is why they do not add to the mass of the atom. -They DO contribute to the SIZE.

12. Discovery of the Atom (pg. 80)
By the early 1800’s, John Dalton proposed that all substances are made up of atoms.
In 1898, J.J. Thomson, proposed that atoms are made up of smaller parts.
In 1911, Ernest Rutherford,
proposed that atoms have
electrons and a positively charged nucleus.

13. Dalton’s Atomic Theory
All matter is made of atoms. Atoms are indivisible and indestructible.
2) All atoms of a given element are identical in mass and properties
3) Compounds are formed by a combination of two or more different kinds of atoms.
4) A chemical reaction is a rearrangement of atoms.

14. Niels Bohr’s model of the atom
Electrons revolved around the nucleus in circular paths called orbits.

15. Electron Cloud Model Current Atomic Theory:
Electrons travel in regions of various thicknesses called clouds.

16. ELEMENTS DEFINITION: PURE SUBSTANCES MADE OF ONLY 1 KIND OF ATOM.
ARE THE BUILDING BLOCKS OF MATTER.
CANNOT BE BROKEN DOWN INTO A SIMPLER SUBSTANCE.
HAVE THEIR OWN UNIQUE SET OF PROPERTIES THAT NO OTHER ELEMENT HAS.

17. ELEMENTS
There are 92 naturally occurring elements on the periodic table. This means they are in nature and not made in a laboratory by scientists.
As of this year (2011) there are 118 confirmed elements. There are 4 more under investigation and scientific testing.

18. Let’s Stop for Questions!
What type of atoms make up the element Lithium? Carbon? Sodium?

19. ELEMENTS ARE MADE OF ONLY 1 KIND OF ATOM.
SOME COMMON ELEMENTS
HYDROGEN (H), HELIUM (He), OXYGEN (0),
Notice that the first letter is capital and the next letter is lower case.

20. Atoms and Elements Activity
As a group, look at the food labels on the items at your table. Make a list of the items in the left hand side column and in the right hand side column make a list of any elements found in that substance.
You may use your periodic table to help you identify the elements.

21. The food item would be: Cooked Ham
What are the elements that are found on this food label?

22. QUESTIONS????
What are the most commonly occurring elements in the food labels?
What items seemed to have the most amount of elements in them?
Can you predict what that means about the food item?
Why do you think the baby formula has such a variety of elements?
Can you predict what the other items on the food label are if they are not elements?

23. Wrap Up Use your dry erase boards to write answers and hold them high!!!
Protons have what charge?
Electrons have what charge?
Which parts of an atom make up the mass of the atom?
Elements are made up of?
The element lead is made up of what kind of atoms?

24. Periodic Table
The periodic table is an organized table of each element.
Each box gives information about each type of element found on Earth.

25. ELEMENTS ARE ORGANIZED IN THE PERIODIC TABLE ACCORDING TO ATOMIC NUMBER.

26. ELEMENTS ARE ORGANIZED IN THE PERIODIC TABLE OF ELEMENTS ACCORDING TO THEIR SIMILAR CHARACTERISTICS
3 major groups: metals, nonmetals and metalloids
See pg. 57 in book

27. Element Info in Each Box
Atomic weight
Atomic Number
Symbol
Name

28. Atomic Number- Number of Protons in an atom Silver = 47 protons
Information from the periodic table
Atomic Number- Number of Protons in an atom
Silver = 47 protons

29. Elements & their symbols
Iron- Fe (Ferrum)
Lead- Pb (Plumbum)
Elements & their symbols
SOME COMMON ELEMENTS
HYDROGEN (H), HELIUM (He), OXYGEN (0),
Notice that the first letter is capital and the next letter is lower case.
Gold- Au (Aurum)

30. Arrangement of the Periodic table
Periods – Rows are called periods. The elements in these rows change conductivity and number of electrons as you move across the table.
Groups – Columns are called groups or families. These elements have the same properties because of the number of electrons.

31. How is the Periodic Table Organized?
Periods
Even though they skip some squares in between, all of the rows go left to right. When you look at a periodic table, each of the rows is considered to be a different period

32. When a column goes from top to bottom, it's called a group or family.
Groups
Groups are often called families because these elements seem to be related.
**Elements in the same group show similarities in their chemical and physical properties.

33. Elements are classified: *Metals *Nonmetals *Metalloids
The Periodic Table Of Elements
Elements are classified:
*Metals
*Nonmetals
*Metalloids
Xenon
Scandium

34. Properties of a metal *Malleable - flattened
*Good conductors – conducts heat or electricity
*Malleable - flattened
*Ductile – can be made into wires
*Shiny- you can see you reflection
Gold
Iron
Magnesium

35. Properties of a Nonmetal
*Not malleable – cannot be flattened
*Not shiny
*Poor conductors
Chlorine
Helium
Bromine

36. Silicon Arsenic Properties of Metalloids
Semiconductors – Average conductors
Shiny but brittle
Silicon
Arsenic
Boron

37. Sulfur
GOLD (AU)
Silver

38. ELEMENTS IN OUR BODIES
IODINE

39. 1.Oxygen (65%) 2.Carbon (18%) 3.Hydrogen (10%) 4.Nitrogen (3%)
5.Calcium (1.5%)
6.Phosphorus (1.0%)
7.Potassium (0.35%)
8.Sulfur (0.25%)
9.Sodium (0.15%)
10.Magnesium (0.05%)
11.Copper, Zinc, Selenium, Molybdenum, Fluorine, Chlorine, Iodine, Manganese, Cobalt, Iron (0.70%)
12.Lithium, Strontium, Aluminum, Silicon, Lead, Vanadium, Arsenic, Bromine (trace amounts)
99% of the mass of the human body is made up of only six elements: oxygen, carbon, hydrogen, nitrogen, calcium, and phosphorus. Every organic molecule contains carbon. Since 65-90% of each body cell consists of water (by weight), it isn't surprising that oxygen and hydrogen are major components of the body

40. Elements in the body Oxygen Carbon Hydrogen Nitrogen Calcium
Phosphorus
Potassium
Sodium
Chlorine
Magnesium
Sulfur

41. GASES
FLUORINE
KRYPTON
NITROGEN
NEON

42. Atoms to Elements to ???

43. ELEMENTS & COMPOUNDS ARE THE BASIC BUILDING BLOCKS OF MATTER
EACH ELEMENT & COMPOUND HAS SPECIFIC PROPERTIES

44. COMPOUNDS ARE MADE OF 2 OR MORE DIFFERENT KINDS OF ATOMS/Elements BONDED TOGETHER

45. COMPOUNDS ARE MADE OF 2 OR MORE DIFFERENT KINDS OF ATOMS BONDED TOGETHER

46. Compounds

47. COMPOUNDS ARE MADE OF 2 OR MORE DIFFERENT KINDS OF ATOMS BONDED TOGETHER
FOR A COMPOUND TO FORM, A CHEMICAL CHANGE MUST TAKE PLACE (A REACTION)
THE ELEMENTS THAT COMBINE MAKE A NEW SUBSTANCE WITH NEW PHYSICAL PROPERTIES
COMPOUNDS CANNOT BE BROKEN DOWN PHYSICALLY. REQUIRES A CHEMICAL CHANGE
MORE COMMON THAN ELEMENTS
NaCl
TABLE SALT + =

48. + = COMPOUNDS ARE IDENTIFIED BY A CHEMICAL FORMULA
THE ELEMENTS THAT COMBINE TO MAKE THE COMPOUND CHANGE PROPERTIES
NaCl
TABLE SALT + =

49. A way of writing how many atoms are in a compound.

50. Chemical Formulas
Written as: C4H10
Butane
Written as: CH4
Methane

51. Subscripts= how many atoms
= how many total molecules
Subscripts= how many atoms

52. FeO2
H2O
C6H12O6
2Li + 2O2

53. Chemical Changes Through Chemical Reactions
A chemical reaction – Process in which the physical and chemical properties of the original substance change as new substances with different properties are formed

54. A burning match is a good example of a chemical reaction.
Application of a spark to the chemicals on the match head start the chemical reaction.
Signs of a chemical change – heat given off, light given off, new substance formed – black material on the match head when the fire is extinguished.

55. Parts of a Chemical Reaction REACTANTS CHANGE INTO PRODUCTS
Products – Substances produced in the reaction (black material on match)
Reactants – Substance that begins the chemical reaction (chemicals on match head)
In other words:
REACTANTS CHANGE INTO PRODUCTS

56. takes the place of an = sign Shows substances combine
CHEMICAL EQUATIONS
Chemical equations are symbols used to describe the details of a chemical reaction and how the reactants changed into the product. This involves indicating all the atoms involved in the reaction.
Fe + O FeO2
Arrow:
Means “yields”
takes the place of an = sign
Reactants:
Iron and oxygen
Product:
Ferrous oxide
(rust)
Plus Sign:
Shows substances combine

57. Law of Conservation of Mass
Matter cannot be created or destroyed, it just changes forms.
The total mass of the reactants must equal the total mass of the product.

58. Examples: H2O, NaCl. MOLECULES ARE 2 OR MORE ATOMS ATTACHED TOGETHER
THEY CAN BE THE SAME KIND (ELEMENTS)
THEY CAN BE DIFFERENT KINDS (COMPOUNDS)
Examples: H2O, NaCl.

59. CAN YOU TELL WHICH IS A MOLECULE OF AN ELEMENT OR A COMPOUND
CAN YOU TELL WHICH IS A MOLECULE OF AN ELEMENT OR A COMPOUND? WHICH SHOWS AN ATOM?

60. Hg + O2 HgO H2 + Cl HCl Mg + O2 MgO O2 + H2 H2O CH4 + O2 CO2 + H2O
Balancing Chemical Equations
Hg + O HgO
H2 + Cl HCl
Mg + O MgO
O2 + H H2O
CH4 + O CO2 + H2O
Fe + Cl FeCl3