Download File - Science with Mr Thompson

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?
Vocabulary
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Atom
Atomic number
Atomic mass
Element
Proton
Neutron
Electron
Electron orbit or shell
Nucleus
Isotope
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Valence electron
Period
Group or Family
Molecule
Compound
Write To Think 083
Obtain correct laptop, log in and …
1. When a candle burns is it a physical change
or a chemical reaction? Explain.
2. A liquid that has a pH of 1 has a high or
low amount of hydrogen ions?
3. How many more or less hydrogen ions
would a solution of pH 3 have?
4. Why do you think group one elements are
called “alkali” “metals”?
5. Where are the metalloids?
ON A DATE !
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!
End of lesson.
• Any slides after here are resources for the
teacher .. But feel free to use them!
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
Summarizer
1. How are atoms neutral?
2. What makes the atomic number of any atom?
3. If the number of protons is changed in an
atom then the atom will be a different type.
Why?
Whiteboard Review:
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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.
Helpful information …
1. Atoms are neutral, with balanced charges
2. Atoms have equal numbers of protons (+) and
electrons (-)
3. Atomic number = number of protons (p)
4. The id or type of atom is its atomic number
5. Atomic mass or mass number = number of
protons + number of neutrons (Why?)
6. Atomic mass (n & p) - Atomic number (p) =
number of neutrons (n)
7. Electron shells ALWAYS fill up from the inside to
the outside shells. (2, 8, 8 or 18 etc.)
Definitions/Characteristics/Properties etc.
of sub atomic particles
1.
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!
2. Nucleus: Small, dense center of the atom. Contains protons and neutrons.
3. Protons: Carry a positive charge. Determines the properties/identity of the atom.
4. Electrons: Carry a negative charge. Gives atoms their ‘surface’ or ‘edge’. React or not react
with other atoms.
5. Electron orbits or shells or clouds: The area around the nucleus that contains the
electrons.
6. Number of electrons = number of protons because an atom is always neutral!
7. Neutrons: Carry a neutral charge. Make atoms stable (or not).
8. 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.
9. 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.
10. 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