Section 3.3 Atomic Structure

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Presentation transcript:

Section 3.3 Atomic Structure To learn about the internal parts of an atom To understand Rutherford’s experiment To describe some important features of subatomic particles To learn about the terms isotope, atomic number, and mass number To understand the use of the symbol to describe a given atom

The Structure of the Atom Dalton’s atomic theory answered many questions It did not answer them all What causes atoms to stick together to form compounds? What is an atom like?

The Structure of an Atom J.J. Thomson, British physicist, 1890s First to recognize that atoms contained negatively charged particles called electrons William Thomson (Lord Kelvin) Plum pudding model – an atom is like plum pudding. The atom (pudding) is positively charged. The electrons (raisins) are spread randomly throughout. The positive and negative balance each other out so that the atom is neutral

Rutherford’s Experiment New Zealand, physicist, Ernest Rutherford Proved that plum pudding model was incorrect He studied alpha particles Particles containing 2 protons and 2 neutrons Alpha particles can be emitted by radioactive material and travel through the air Rutherford’s experiment – he bombarded a piece of gold foil with alpha particles. The gold foil was surrounded by a detector that produced tiny flashes whenever an alpha particle collided with it

Rutherford’s Experiment He was surprised by his results He expected all of the particles to pass directly through Some were deflected Rutherford concluded there must be dense positively charged nucleus in the center of the gold atoms that deflected the α particles.

Rutherford’s Experiment Rutherford theorized that the nucleus is made of two particles Proton -- positive particle with an equal but opposite charge of an electron. Significantly more massive than an electron. Neutron -- a particle with no charge but similar in mass to a proton

Modern Concept of Atomic Structure Question: If all atoms are composed of the same components, why do different atoms have different chemical properties? Number and arrangement of electrons

Isotopes James Chadwick – discovered that atoms contain neutrons Dalton’s theory had to be modified: “All atoms of the same element contain the same number of protons and electrons, but atoms of a given element may have different numbers of neutrons”

Na Na Isotopes 23 11 24 11 number of protons number of neutrons number of electrons Atomic number Mass number 11 Na 23 11 12 11 11 23 Sodium-23 number of protons number of neutrons number of electrons Atomic number Mass number 11 13 Na 24 11 11 11 24 Sodium-24

Practice Use your periodic table. Give the number of protons, neutrons and electrons for the following: Nitrogen-15 Lithium-9 Protons 7 Electrons 7 Neutrons 8 Protons 3 Electrons 3 Neutrons 6 Barium-136 Carbon-14 Protons 6 Electrons 6 Neutrons 8 Protons 56 Electrons 56 Neutrons 80