"Brief" History of the Atom About two thousand years in under 15 minutes

Transcription

1 "Brief" History of the Atom About two thousand years in under 15 minutes Chemistry C2 Structure and properties of atoms Atom: Smallest particle of an element that retains its identity in a chemical reaction Protons + Neutrons 0 Electrons

2 The ATOM The smallest piece of matter that still keeps the properties of the element Elements are made of atoms that are all the same Atoms can be divided into smaller parts, but these parts do not keep the properties of the elements Protons The atomic number determines the number of protons Protons are positively charged Number of protons determines number of electrons Contributes to most of the atom s mass Inside the Nucleus

3 Neutrons Inside the Nucleus Neutral charge Same mass as protons Atomic Mass Number Atomic number Number of Neutrons Quarks Make up neutrons and protons 6 have been confirmed Smallest particle yet discovered Inside the Nucleus

4 Electrons Outside the Nucleus Negative Charge Surround the nucleus in the form of a cloud Have very little mass Same number as number of protons to make stable atoms electrically neutral Atomic Models Bohr model. In this model, the nucleus is orbited by electrons, which are in ordered energy levels.

5 A Some What Brief History of the Atom The idea of atoms began 2400 years ago with Greek thinkers who defined atoms as the smallest parts of matter. Democritus: 458 BC Grew up right after the end of the Persian Wars Taught by Leucippus who first thought of the world being made of smaller things. Lived through the civil war in which Athens was eventually defeated by Sparta (Peloponnesian War) War and thought was his everyday life

6 Dalton s Model In the early 1800s, the English Chemist John Dalton performed a number of experiments that eventually led to the acceptance of the idea of atoms.

7 Ernest Rutherford Worked under JJ Thomson He developed a theory of the nucleus All the atom s mass was centralized into a nucleus Rutherford s Gold Foil Experiment Rutherford s experiment Involved firing a stream of tiny positively charged particles at a thin sheet of gold foil

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9 This could only mean that the gold atoms in the sheet were mostly open space. Atoms were not a pudding filled with a positively charged material. Rutherford concluded that an atom had a small, dense, positively charged center that repelled his positively charged bullets. He called the center of the atom the nucleus The nucleus is tiny compared to the atom as a whole.

10 Bohr Model In 1913, Bohr proposed an improvement. In his model, he placed each electron in a specific energy level. Bohr Model According to Bohr s atomic model, electrons move in definite orbits around the nucleus, much like planets circle the sun. These orbits, or energy levels, are located at certain distances from the nucleus.

11 The Wave Model or Quantum Mechanical Model Today s atomic model is based on the principles of wave mechanics. According to the theory of wave mechanics, electrons do not move about an atom in a definite path, like the planets around the sun. The Wave Model In fact, it is impossible to determine the exact location of an electron. The probable location of an electron is based on how much energy the electron has. According to the modern atomic model, at atom has a small positively charged nucleus surrounded by a large region in which there are enough electrons to make an atom neutral.

12 Electron Cloud: A space in which electrons are likely to be found. Electrons whirl about the nucleus billions of times in one second They are not moving around in random patterns. Location of electrons depends upon how much energy the electron has. The Wave Model Depending on their energy they are locked into a certain area in the cloud. Electrons with the lowest energy are found in the energy level closest to the nucleus Electrons with the highest energy are found in the outermost energy levels, farther from the nucleus.