Atoms and Molecules.

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Atoms: Development of the Atomic Theory

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Presentation transcript:

Atoms and Molecules

Atom The smallest particle of an element Examples: Hydrogen Carbon Chlorine Titanium

The Atomic Model Democritus (450 B.C.) John Dalton (1800) If you kept cutting a substance in half forever, eventually you would end up with an “uncuttable” particle. John Dalton (1800) All substances are made of atoms Atoms of the same element are exactly alike, and atoms of different elements are different. JJ Thompson (1897) Discovered electrons Developed “plum pudding” model

The Atomic Model Ernest Rutherford (1911) Neils Bohr (1913) Most of the atom’s mass is found in a region in the center called the nucleus Neils Bohr (1913) Electrons travel around the nucleus in definite paths. Erwin Schrodinger There are regions inside the atom where electrons are likely found

Nucleus The central core of an atom, contains protons and usually neutrons

Proton Small positively charged particles found in the nucleus of an atom

Neutron Small uncharged particles found in the nucleus of an atom

Nuclear Energy Fission Fusion The potential energy stored in the nucleus of an atom Fusion Fission

Electron Tiny, negatively-charged, high-energy particles that move around the outside of the nucleus

Electrical Energy The energy of moving electrical charges Charge- A definite amount of electricity, positive or negative

Element A substance that cannot be broken down into any other substances

Atoms continued Atomic Number= number of protons Atomic Mass= number of protons + neutrons # Electrons = # Protons

Calculations Magnesium Oxygen 12 protons 12 electrons 12 neutrons (24-12=12) Oxygen 8 protons 8 electrons 8 neutrons (16-8=8)

Molecule A particle made of two or more atoms bonded together

Chemical Bond The force that holds the atoms together

Chemical energy The potential energy stored in chemical bonds