1. Atomic Theory
Chem. 11

2. Dalton’s Atomic Theory
1 All matter is made up of invisible particles called atoms
2 All atoms of one element are identical. The atoms of any one element are different from those of all other element.
3 Chemical change is the union or separation of atoms
4 Atoms combine in small whole number ratios to form compounds.

3. Thomson’s Model
Joseph Thomson realized that the accepted model, of his time, did not take into account electrons and protons.
Thomson created a new model, known as the “plum pudding atom.”

4. Thomson’s Model
His model contains negatively charged electrons, raisons, which are stuck into a lump of positively charged protons, dough.
The model does not contain any neutrons as they were not discovered during Thomson’s time.

5. Thomson’s Model
Fails to explain about the number of protons, their arrangement in the atom, or the ease with which atoms are stripped of electrons to form ions

6. Rutherford’s Model
Ernest Rutherford performed the Gold Foil experiment, which led to his discovery of the nucleus
Rutherford proposed the nuclear atom in which electrons surround a dense nucleus.

7. Rutherford’s Model
The Gold foil experiment involved the firing of radioactive particles through a thin gold foil and detecting the particles using screens coated with zinc sulfide.
Rutherford discovered that though most of the particles travelled straight through the foil, some particles were deflected.

8. Rutherford’s Model
He concluded that the atom is mainly empty space with all the positive charge and mass being located in the center known as the nucleus.
An argument with Rutherford’s model is what is keeping the negatively charged electrons from being attracted to the positively charged nucleus?
Later experiments showed that the nucleus was composed of protons and neutrons

9. Bohr’s Model
Niels Bohr developed a new atomic model to answer the question of why electrons do not collapse into the nucleus in Rutherford’s model.
He proposed that electrons are arranged in concentric circular paths, know as orbits, around the nucleus.

10. Bohr’s Model
His model is fashioned after the motions of the planets around the sun.
It is often referred to as the planetary model.
Bohr proposed that the electrons in a particular path have a fixed energy; the electrons do not lose energy and do not fall into the nucleus

11. Energy Levels
The Energy Level of an electron is the region around the nucleus where it is likely to be moving.
The lowest rung of the ladder corresponds to the lowest energy level
An electron can move from one energy level to another, but it cannot stop between levels

12. Energy Levels
An electron must lose or gain just the right amount of energy to move from one energy level to another.
The amount of energy gained or lost by every electron is not the same.
The energy levels in an atom are not equally spaced.

13. Energy Levels
A Quantum of energy is the amount of energy required to move an electron from its present energy level to the next higher level.
The energies of electrons are said to be quantized
In general, the higher an electron is placed on the energy ladder, the larger the diameter of the circular path of that electron

14. Quantum Mechanical Model
The Quantum Mechanical Model is the modern description of the electrons in atoms
The model leads to quantized energy levels for an electron, but it does not define the exact path an electron takes around the nucleus

15. Quantum Mechanical Model
The model is concerned with the likelihood of finding an electron in a certain position.
It is similar to a cloud; the most dense portion is where the probability of finding an electron is larger.