ATOMIC PRESENTATION

by Daman

the atomic evolution

INDEX

14. Thanks

13. Work Cited

12. Timeline

11. Quarks, leptons & bosons

10. James Chadwick

9. Erwin Schrodinger

7. Neil Bohr

6. Ernest Rutherford

5. J.J Thomson

4. Eugen Goldstein

3. Jhon Dalton

2. Antoine Lavoisier

8. Werner Heisenberg

1. Leucippus

Leucippus' discovery

• He came up with the concept of tiny particles making up matter
• if purticles are cut in half again and again there will be a point when you can't cut anymore

• atoms = uncuttable/indivisible

Leucippus' discovery

Antoine lavoisier

antoine lavoisier

Antoine was known for his experimantation and love for dividing oxygen molecules from HgO. This led to the Law od Conservation which says matter cannot be made or destroyed.

Dalton's atomic theory

WRITE A TITLE HERE

The number and kind of atoms in a compound is constant.

They compine in a ratio of whole numbers to form compounds.

Atoms of different chemicals have different masses + properties.

Atoms of a given chemical are identical in mass + chemical properties.

They're indivisible particles which cannot be created nor destroyed in a chemical reaction.

All matter is made of tiny particles called atoms.

John Dalton

"This paper will no doubt be found interesting by those who take an interest in it."

goldstein'sstudy

eugen goldstein

In 1870 scientists began using gas filled tubes with electrodes in each end which emit light when an electrical current passes through them and called them cathode ray. In 1886 Eugen Goldstein found that the tubes also emitted light from the positive electrode which meant there must be a positive charge in matter. These were named protons later in 1920.

J.J THOMSON

In 1904 he suggested the plum pudding model. The way he viewed it was a positive atom composed of random negative electrons or "corpuscles"

J.J Thomson also researched cathode rays but his resercg lead to the discovery of electrons. Hefigured the mass of the rays (1000 times lighter than hydrogen) by measuring how much heat the cathode rays generated, how much they could be bent by magnets and other things. In conclusion rays = small negatively charged particles aka electrons.

j.j thomson

ernest rutherford

ernest rutherford

In 1911 Rutherford conducted the gold foil experiment with Hans Gaigner and Ernest Marsden to better understand the structure of an atom. For his setup he used alpha particles in a lead container with a small opening, a very thin gold foil and a circular fluorescent screen around the foil.

Many particles passed straight through but some went sideways and some bounced almost straight back.

The particles hit the gold foil.

Step 3

Step 2

The alpha particles travelled outside the lead box in a straight direction.

Step 1

gold foil experiment

After the experiment they were shocked . They thought that if an atom is a sphere of positive charge with the electrons embedded in it it's expected that the atoms will pass right through the gold foil and hit the detector straight because the mass of alpha particle is heavier than the mass of positive charges and it has higher energy.

gold foil experiment

The electrons revolve around the nucleus in circular path and the size of the nucleus is very small compared to the size of the atom.

Most of the other particles passed straight through the foil and hit the detector. Some particle got deflected by small angles and few particles almost rebounded. Rutherford's experiment concluded with the discovery of the nucleus. The center is denser so allows particles to bounce and reflect and most of the space inside the atom is empty. The positive charge is all in the middle .

gold foil experiment

ernest rutherford

neil's bohr model

• in 1913 Bohr figured that only certain special orbits called discrete orbits of electrons are allowed inside the atom and that electrons don't radiate energy.
• Each shell of electrons has a defined energy level.

neil bohr

werner heisenberg

In 1925 Heisenberg used math to discover that it's impossible to calculate the exact momentum and the exact position of a subatomic particle at the same time. So he proposed the quantum theory which says that electrons have properties of both particles and waves. By probability they said they’re found in orbitals

werner heisenberg

erwin schrodinger

In 1926 Schrodinger came up with an equation to calculate everything we can possibly know about the quantum system. His equation says we can't know both momentum and position but we can know things like the energy levels and the wave function.

erwin schrodinger

james chadwick

These particles have a mass similar to protons and zero charge. He called them neutrons.

In 1932 Chadwick conducted an experiment using alpha particles and baryllium. He did so because when they compared the mass of two elements and tried to balence them, something was always off. During his experiment he bombarded alpha particles to baryllium and was shocked when he found that there were other particles in an atom beside protons and electrons.

james chadwick

quarks, leptons and bosons

A proton is made up of three quarks including two "up" quarks and one "down" quark and a neutron is made up of three quarks including two "down" quarks and one "up" quark

Quarks, leptons and bosons play a very big role in the world of radiation oncology. An atom is formed of protons, neutrons and electrons but these are also formed of other smaller fundamental blocks called quarks. These can go by names of up, down, strange, charmed, bottom, and top, arranged from least to most massive.

quarks, leptons & bosons

quarksleptons bosons

neutrons

planetary model

electrons

cathode ray- protons

dalton's theory

Timeline

5th century - atom

• https://findanyanswer.com/when-did-eugen-goldstein-discover-the-proton?msclkid=2a638aa3cf2c11eca98563041d7198a6
• https://www.ducksters.com/science/physics/elementary_particles_quarks.php
• https://theoncologist.onlinelibrary.wiley.com/doi/full/10.1634/theoncologist.11-1-62

• "Crash Course Chemestry" youtube
• "Don't Memorise- chemestry" youtube.

work cited

work cited

ThankYou!