1. Atomic Structure and development of the atom

2. Engager Think, Pair and Share… True or False…?
Atoms cannot be split up into anything smaller.
Atoms are solid objects and nothing can pass through them.
There are millions of different kinds of atoms.
No-one has ever seen an atom.
False!
False!
False!
False!

3. To understand how the structure of the atom has changed
To evaluate the different types of models of the atom.
To suggest why models have changed in science.
To explain the different sub atomic particles.
Progress

4. To demonstrate good progress in this lesson
Name
Will…
To suggest why models have changed in science.
To explain the different sub atomic particles
The Honley Learning Mindset Advocate for this lesson is…
Matthew – will show resilience by not giving up if he finds something difficult.

5. Recap - The Structure of the Atom
There are many different models used to describe the structure of an atom.
In this model the electrons are shown orbiting around a central nucleus.
However, electrons also possess properties typical of waves.

6. The Structure of the Atom
There are many different models used to describe the structure of an atom.
In this model the electrons are shown orbiting around a central nucleus.
However, electrons also possess properties typical of waves.

7. Atomic structure definition
Click on the You tube link if needed

8. Atomic number Number of protons Number of electrons
Mass Number Number of protons +
Number of neutrons
ALWAYS THE BIGGER ONE! 4 2 He
Atomic number Number of protons Number of electrons
Segway ito information on the periodic table, students must be able to identify these numbers.
Hand out periodic tables and have students find the correct number of sub atomic particles in 5 elements

9. H H H What is going on here? 1 2 1 3 1 1 proton 1 proton 1 proton
1 electron
Refer to the balance needed between the numbers of protons and neutrons for an atom to be stable, they don’t have to be equal numbers but there is a ‘required mix for stability line’. The further away from this ‘line’ the isotope is the more radioactive it is likely to be.
1 electron
1 electron
0 NEUTRONS
1 NEUTRON
2 NEUTRONS

10. Can you and your partner come up with a definition for an isotope?
What’s an isotopes?
Link in the baseball team from the simpsons and why it is called the isotopes
Can you and your partner come up with a definition for an isotope?

11. Definition of an Isotopes
Talk through the idea that the further away from the ídeal’ they are.. The more unstable they will be and thus radioactive
Same number of protons and electrons, different neutrons

12. Sub Atomic Particles - Check What You Know
For each particle drag and drop the correct answers into the table.

13. Connector -Why do models in Science change ?

14. Plum pudding model of the atom
One of the first models of the atom was by J J Thompson and he knew the atom was neutral and had no charge and he also showed that they contain electrons which were negatively charged
Positively charged sphere
Negatively charged electron
This became known as the ‘plum pudding’ model.

15. Earnest Rutherford
E. Rutherford ( )
In 1910, Earnest Rutherford’s team carried out experiments in which particles were fired at a thin sheet of gold.
Rutherford expected all of the particles to pass straight through...

16. Earnest Rutherford
Press ‘Start’ to take a closer look at Rutherford’s experiment...
Rutherford also predicted the existence of neutrons in the nucleus, and named the three types of nuclear radiation alpha (), beta () and gamma ().

17. Earnest Rutherford experiment
Click on the You tube link for explanation

18. What Rutherford’s team observed……..
Most of the alpha particles went straight through the foil.
Some alpha particles were deflected through large angles.
3. A very few alpha particles were reflected straight back.

19. Rutherford’s conclusions
Observation
Conclusion
Most alpha particles went straight through the foil.
A few were deflected through large angles.
A very few were reflected straight back.
Atoms are mostly space.
The nucleus is very small compared to the size of the atom and it contains most of the mass and all the positive charge.

20. Comprehension exercise – Complete the sheet given by going around the room and finding the information. Teacher another student an aspect of what you have found out

21. Atomic structure (Physics) Relative charges;
Keywords; proton, neutron, electron, nucleus, orbital/shell, plum pudding model, Niels Bohr, alpha particle, positive, negative, models
James Chadwick, relative mass, relative charge, isotope, atomic number, mass number, electronic configuration,
Atoms, elements & compounds
Relative charges;
Compounds;
Are formed by elements in chemical reactions
Are 2 or more elements that are chemically combined
Atoms;
Atomic number;
The proton number, it is different for every element
Atoms;
Elements;
There are about 100 different elements, each with a symbol
Isotopes;
Size and mass;
Very small, radius is 0.1nm (1x10-10m)
Mass is mainly in the nucleus
Mass Number;
Early ideas;
Before the discovery of the electron atoms were tiny spheres, they couldn’t be divided
Development of the model of the atom;
Electronic configurations;
Nucleus development;
Experiments now show nucleus is made of smaller particles of positive charge
Relative Atomic Mass;
This is the mass of the element that takes into account the relative abundance of isotopes,
Calculated by=
(mass x abundance) + (mass x abundance)
100
Plum pudding;
Niels Bohr;
Adapted the nuclear model suggesting electrons in orbitals at set distance
James Chadwick;
Evidence to show the existence of neutrons in the nucleus
Atomic structure
(Physics)
Alpha particle scattering;
Showed that the mas of an atom was concentrated in the centre, it was charged too

22. Atomic structure (Physics) Relative charges;
Keywords; proton, neutron, electron, nucleus, orbital/shell, plum pudding model, Niels Bohr, alpha particle, positive, negative, models
James Chadwick, relative mass, relative charge, isotope, atomic number, mass number, electronic configuration, percentage abundance, periodic table,
Atoms, elements & compounds
Relative charges;
Compounds;
Are formed by elements in chemical reactions
Are 2 or more elements that are chemically combined
Atoms;
An atom has no overall charge, the number of protons = the number of electrons
Atomic number;
The proton number, it is different for every element
Atoms;
Everything is made of atoms, it is the smallest part of an element
Elements;
There are about 100 different elements, each with a symbol
Isotopes;
Atoms that have the same number of protons (element), but different numbers of neutrons
Size and mass;
Very small, radius is 0.1nm (1x10-10m)
Mass is mainly in the nucleus
Mass Number;
The number of protons & neutrons in the nucleus
Early ideas;
Before the discovery of the electron atoms were tiny spheres, they couldn’t be divided
Development of the model of the atom;
New experimental evidence may lead to the model being changed or replaced
Electronic configurations;
Electrons fill the lowest energy levels first
This starts from the nucleus, following a set pattern up to the following maximum
1st shell – 2 electrons
2nd shell – 8 electrons
3rd shell – 8 electrons
4th shell – 2 electrons
Nucleus development;
Experiments now show nucleus is made of smaller particles of positive charge
Relative Atomic Mass;
This is the mass of the element that takes into account the relative abundance of isotopes,
Calculated by=
(mass x abundance) + (mass x abundance)
100
Plum pudding;
After the electron was discovered the atom became a ball of positive charge with negative electrons scattered in it
Niels Bohr;
Adapted the nuclear model suggesting electrons in orbitals at set distance
James Chadwick;
Evidence to show the existence of neutrons in the nucleus
Atomic structure
(Physics)
Alpha particle scattering;
Showed that the mas of an atom was concentrated in the centre, it was charged too

23. Homework – GCSE Question on Ernest Rutherford's experiment