1. Organization of Matter
7. P.2: The student will demonstrate an understanding of the structure and properties of matter and that matter is conserved as it undergoes changes.

2. Section 1
7. P.2A.1: Develop and use simple atomic models to illustrate the components of elements (including the relative position and charge of protons, neutrons, and electrons).

3. The Atom
SKETCH TO LEARN: USE A DESCRIPTION WHEEL TO DESCRIBE ATOMS
ATOM- THE SMALLEST PART OF ANY ELEMENT THAT HAS THE CHEMICAL PROPERTIES OF THAT ELEMENT
ATOMS ARE PARTICLES MUCH TOO SMALL TO BE SEEN WITH A CLASSROOM MICROSCOPE ​
EVEN THOUGH ATOMS ARE SMALL, THEY HAVE MASS AND TAKE UP SPACE
Atom

4. The Atom Atom – composed of subatomic particles
Protons (+)
Neutrons
Electrons (-)
These particles affect the properties of an atom
Once you understand these particles and their importance in atoms, you will be able to describe and explain all types of atoms

5. Protons(+) and Neutrons
Protons have a positive charge
(+) and blue in the picture
Neutrons have NO charge
Red in the picture
They are tightly bound in a tiny nucleus
The nucleus is the tiny cluster in the center of an atom
About the same mass
An example of an atomic model of Carbon

6. Electrons (-) Electrons have a negative charge
Electrons move in random patterns in an orbital around the nucleus (in the center)
1st orbit can hold up to 2 electrons
2nd orbit can hold up to 8 electrons

7. What atom is it?
This depends on the number of protons (+) in the nucleus
Usually, the same number of electrons (-) exist floating around the nucleus as protons exist in the nucleus (Usually, but not always)

8. Element Symbol Hydrogen H Silicon Si Carbon C Copper Cu Nitrogen N
Aluminum Al
Oxygen O
Silver Ag
Chlorine Cl
Gold Au
Magnesium Mg
Iron Fe
Zinc Zn
Helium He
Calcium Ca
Potassium K
Phosphorus P
Sodium Na

9. Section 2
7. P.2A.2: Obtain and use information about elements (including chemical symbol, atomic number, atomic mass, and group/family) to describe the organization of the periodic table.

10. Periodic Table of Elements (PTE)

11. Periodic Table of Elements (PTE)
Used to organize all of the elements in a visual way
Every periodic table will have a square for each element with the:
element name
chemical/element symbol
atomic number
atomic mass
You should be able to and will be
expected to locate each element on the PTE
Once you understand the above vocab

12. Element Name and Chemical Symbol
Each element has a different symbol
Symbols are written with one, two, or three letters
The first letter is always capitalized
***Be familiar with the element names and symbols in the chart!!!
Quiz Thursday, September 1
Element
Symbol
Hydrogen H
Silicon Si
Carbon C
Copper Cu
Nitrogen N
Aluminum Al
Oxygen O
Silver Ag
Chlorine Cl
Gold Au
Magnesium Mg
Iron Fe
Zinc Zn
Helium He
Calcium Ca
Potassium K
Phosphorus P
Sodium Na

13. Atomic Number The atomic number of an element = the number of protons
The atomic number is a whole number
The atomic number is always the same for a given element
The elements on the periodic table are arranged numerically by increasing atomic number

14. Atomic Mass
The atomic mass is an average sum of the number of the protons and the number of neutrons in the nucleus of the atom
Since the atomic mass of an element is an average, it is usually not a whole number

15. Periodic Table Organization
Families/Groups
A horizontal row on the periodic table is called a period
There are 7 periods (rows)
Left to Right
Families, also called groups, are vertical columns of elements on the periodic table
There are numbered 1-18
Top to Bottom
Elements in the same family have similar properties

16. Periods

17. Families/Groups

18. Metals, Nonmetals, and Metalloids
Where are the metals, nonmetals, and metalloids?

19. Metalloids
There is a zigzag line on the right side of the periodic table that separates the metals from the nonmetals. Metalloids are found on the zigzag line.
Yellow in the picture
Elements identified as metalloids have properties (characteristics) of both metals and nonmetals.

20. Metals
Metals are generally located on the left side of the zigzag line
Gray in the picture
Examples of metals are: Sodium (Na), Calcium (Ca), Iron (Fe), and Aluminum (Al)
The majority of elements are metals

21. Nonmetals
Nonmetals, with the exception of Hydrogen (H), are located on the right side of the zigzag line
Red in the picture
Examples of nonmetals are: Chlorine (Cl), Oxygen (O), Sulfur (S), and Iodine (I)

22. Section 3 and 4
7. P.2A.3: Analyze and interpret data to describe and classify matter as pure substances (elements or compounds) or mixtures (heterogeneous or homogeneous) based on composition.
7. P.2A.4: Construct explanations for how compounds are classified as ionic (metal bonded to nonmetal) or covalent (nonmetals bonded together) using chemical formulas

23. What is matter made of?
Matter can be classified on the basis of its composition (what it is made of)

25. Elements
Elements are pure substances that cannot be changed into simpler substances
Elements are composed of one kind of atom
Examples: Hydrogen, Oxygen, Carbon

26. Compounds
Compounds are pure substances that are composed of two or more atoms that are chemically combined
Compounds can only be changed into simpler substances called elements by chemical changes

27. You should know this chart!!!
If you don’t, then you need to put some time in learning it!!!

28. Bonds
Elements are made up of one kind of atom and the symbol for each element is unique.
Compounds are composed of more than one atom chemically bonded, and their formulas show the different atoms that compose the compound.

29. Ionic Bonds An ionic bond is formed when metals react with nonmetals
Electrons are transferred from the metals to the nonmetals.
React means combine or bond)

30. Covalent Bonds
Covalent bonds are formed when two or more nonmetals react (combine or bond) with each other
Covalent bonds SHARE electrons and are called covalent compounds

31. Chemical Formulas
Chemical formulas use element symbols from the periodic table and numerical subscripts to depict the name and number of atoms of each element in the compound;
Examples include: Water (H2O), Glucose or sugar (C6H12O6), and Table Salt (NaCl).

32. Subscripts in Chemical Formulas
In a chemical formula, the subscripts (numbers) = number of each kind of atom that appears in the compound. The subscript is written to the lower right of the element symbol.
If no subscript is written, only one atom of that element is part of the compound.
For example, in H2O, the number 2 is the subscript for hydrogen and means that there are 2 atoms of hydrogen in the compound of water; since there is no subscript for oxygen it is assumed to be one atom of oxygen.
N2, O2, F2, Cl2, Br2, I2, and H2 are diatomic molecules where all of the atoms of the molecule are the same element.

33. STOP!!! TIME FOR AN ACTIVITY

34. Mixtures
Mixtures are composed of two or more different substances that retain their own individual properties and are combined physically (mixed together).
Mixtures can be separated by physical means (filtration, sifting, or evaporation).

35. Heterogeneous mixtures
Mixtures can be…
Heterogeneous mixtures
Homogeneous mixtures
Explain in you notes what differences you see between the left side and right side

36. Heterogeneous Mixtures
In a heterogeneous mixture, which is not uniform throughout (doesn’t look the same), the component substances can be visibly distinguished (you can see each different item).
Examples: Salt and pepper mix, cereal and milk, rice and beans

37. Homogeneous Mixture
In a homogeneous mixture, which is uniform throughout, the substances are evenly mixed and cannot be visibly distinguished. The particles of the substances are so small that they cannot be easily seen. Another name for a homogeneous mixture is a solution.
Examples: rock, air, blood, Italian salad dressing, ocean water, Kool-Aid

38. Create a Venn diagram – comparing and contrasting pure substances and mixtures
This is for a grade, so raise your hand when this is completed to be signed off.