Download File - Science with Mr Thompson

Lesson 079
Learning Goal: You should be able to
Describe the structures and functions of three sub
atomic particles
Calculate number of sub atomic particles from their
relationships
Draw a Bohr
Success criteria: Can you …
Vocabulary
•
•
•
•
•
•
•
•
•
•
Atom
Atomic number
Atomic mass
Element
Proton
Neutron
Electron
Electron orbit or shell
Nucleus
Isotope
•
•
•
•
•
Valence electron
Period
Group or Family
Molecule
Compound
Write To Think 079
1. What is the difference between atomic mass and
atomic number?
2. Which one defines the type of atom?
3. If an atom has 16 protons and 10 neutrons …
what’s its mass?
4. What type of atom is it?
5. How many electrons would it have …and how do
you know?
Calculate the number of sub atomic
particles
• 5 minutes
• Check
Being Bohring!
-
-
8p
8n
-
-
-
-
Patterns using Bohr(ing) diagrams
•
•
•
•
•
•
Read salmon sheet
Group = column
Period = row
Valance electrons = electrons in outer shell
Number of shells = count from inside to outside
Instructions and Questions etc.
Whiteboard Review:
1.
2.
3.
4.
5.
6.
7.
8.
9.
10.
11.
12.
13.
14.
15.
16.
17.
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.
Calculating # of sub atomic particles
8
0
Oxygen
15.999
Atomic #
8
16
Element Symbol O
# of Protons
8
# of Neutrons 16 - 8 = 8
# of electrons 8
Atomic Mass
Calculating # of sub atomic particles
79
Au
Gold
196.967
Atomic #
79
Atomic Mass
197
Element Symbol Au
# of Protons
79
# of Neutrons 197
# of electrons
79
- 79 = 118
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
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?