1. Lesson 083 Learning Goal: You should be able to
Explain patterns relationships etc. in the PT.
Success criteria: Can you …
Answer questions about the PT?

2. Vocabulary Valence electron Period Group or Family Molecule Compound
Atom
Atomic number
Atomic mass
Element
Proton
Neutron
Electron
Electron orbit or shell
Nucleus
Isotope
Valence electron
Period
Group or Family
Molecule
Compound

3. Write To Think 083 Obtain correct laptop, log in and …
When a candle burns is it a physical change or a chemical reaction? Explain.
A liquid that has a pH of 1 has a high or low amount of hydrogen ions?
How many more or less hydrogen ions would a solution of pH 3 have?
Why do you think group one elements are called “alkali” “metals”?
Where are the metalloids?

6. ON A DATE !

7. To Do Go to google classroom. Find “periodic table patterns …. “
Open attempt to answer questions and/or use the URLs to add to your organizer!

8. End of lesson.
Any slides after here are resources for the teacher .. But feel free to use them!

9. Periodic table orientation
Period = row = Horizontal = across the periodic table
Periods have numbers 1 to 7
Family/Group = column =Vertical = up or down the periodic table
Groups have numbers 1 to 18
They also have names

10. Summarizer How are atoms neutral?
What makes the atomic number of any atom?
If the number of protons is changed in an atom then the atom will be a different type. Why?

11. Whiteboard Review:
What is the charge of a proton? (Write a sign or symbol)
Which sub atomic particle is neutral?
Which particles orbit the nucleus?
If a model of an atom makes the nucleus the size of a soccer ball … how far away would the closest electrons be?
Which number of particles is the atomic number?
Which number of particles always equal the number of protons in an atom?
Which particles have almost zero mass?
Which particles are the ‘id’ of an atom?
Which particles make up the nucleus?
Which particles travel at the speed of light?
How many electrons can be in the 2nd shell?
Which particles make up the atomic mass?
If the atomic mass is 60 and the atomic number is 40 how many neutrons are there?
Does adding a proton change the type of atom?
Does adding a neutron change the type of atom?
If an electron is added to an atom is it still an atom?
Draw a model of an atom with mass 14 and 8 electrons.

12. Helpful information … Atoms are neutral, with balanced charges
Atoms have equal numbers of protons (+) and electrons (-)
Atomic number = number of protons (p)
The id or type of atom is its atomic number
Atomic mass or mass number = number of protons + number of neutrons (Why?)
Atomic mass (n & p) - Atomic number (p) = number of neutrons (n)
Electron shells ALWAYS fill up from the inside to the outside shells. (2, 8, 8 or 18 etc.)

13. Definitions/Characteristics/Properties etc. of sub atomic particles
Atom: Smallest possible unit into which matter can be divided, while still maintaining its properties. Made of protons ,electrons and neutrons. Atoms are always NEUTRAL!
Nucleus: Small, dense center of the atom. Contains protons and neutrons.
Protons: Carry a positive charge. Determines the properties/identity of the atom.
Electrons: Carry a negative charge. Gives atoms their ‘surface’ or ‘edge’. React or not react with other atoms.
Electron orbits or shells or clouds: The area around the nucleus that contains the electrons.
Number of electrons = number of protons because an atom is always neutral!
Neutrons: Carry a neutral charge. Make atoms stable (or not).
Atomic number: The number of protons in the nucleus of the atom, which determines its chemical properties and its position in periodic table. Examples: Oxygen has 8 protons, atomic # 8. Gold has 79 protons, atomic # 79.
Mass number: The number of protons AND neutrons in the nucleus of the atom. Determine the mass of the atom. Examples: Carbon has 6 protons and can have 6 neutrons, mass number # 12. Chlorine has 17 protons, and can have 19 neutrons, mass number # 36.
Isotopes: Two or more forms of the same element that has equal number of protons but different number of neutrons and differ in relative atomic mass and have same chemical properties