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The Atomic Nature of Matter: Exploring the Building Blocks of the Universe

This text provides an introduction to the atomic nature of matter, exploring the concept of atoms as the fundamental building blocks of everything. It covers topics such as elements, compounds, isotopes, and the structure of atoms, including the nucleus, protons, neutrons, and electrons. The text also discusses the periodic table, phases of matter, and the fourth state of matter, plasma. Discover the fascinating world of atoms and their role in shaping the universe.

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The Atomic Nature of Matter: Exploring the Building Blocks of the Universe

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  1. Conceptual Physics The Atomic Nature of Matter

  2. Atoms • Building blocks of matter • Everything is composed of atoms

  3. Elements • atoms of the same kind • there are 115 known elements to date • Every element is unique, and has its own set of properties • All atoms of the same element have the same # of protons.

  4. Atoms are recyclable • the same atoms have been here since the beginning of time • Combine w/ other elements, then go back to original form and back again • You may be breathing the same air as Julius Caesar or George Washington….

  5. Atoms are very small • Cannot view individual atoms w/ visible light • Only way to “see” atoms is w/ Scanning Tunneling Microscope • About 1023 (or 1000000000000000000000000000) atoms in one thimble-full of water

  6. Brownian Motion • Jiggling of atoms • Atoms are constantly moving • Molecular motion never stops unless a substance is at a temperature of (-273˚ C) a.k.a. absolute zero

  7. Molecules • combinations of atoms ex. H2, H2O, NaCl, N2 • Can be combinations of the same atom, or of different types of atoms

  8. Compounds • combinations of atoms of different elements ex. NaCl, H2O, HCl • A compound is always a molecule, but a molecule may not necessarily be a compound (examples …. H2 , N2 )

  9. Rutherford Experiment • Gold Foil - showed atoms are largely empty space, very dense nucleus that reflected charged particles backwards • Like a “shooting a 15-inch artillery shell at a piece of tissue paper and having it come back and hit you”

  10. Nucleus • very dense……. Composed of Protons & Neutrons • Almost all of the mass of an atom is concentrated in the nucleus • A teaspoonful of nuclei packed together would weigh a billion tons

  11. Neutrons & Protons • Nuetrons- Nuetral charged particle found in nucleus • Protons- Positively charged particle found in nucleus, atoms of the same number of protons are atoms of the same element

  12. Isotopes • for a given element, the number of neutrons may vary. Isotopes of an element are atoms of the same element having different numbers of neutrons • Example - Uranium-238 (atomic mass 238) has isotope Uranium -235 • This was used to make the atomic bomb dropped on Hiroshima

  13. Electrons (e-) • negatively charged particle not found in the nucleus. • Orbits the nucleus in various energy levels. • In a neutral atom, the number of electrons will match the number of protons • # of electrons in a neutrally charged atom is equal to the # of protons, which is given with the atomic number. • Mass of 1 electron is about 1800 times less than the mass of a proton or neutron

  14. Ions • Charged Particle • Positively charged (less electrons than protons) • Negatively charged (more electrons than protons) • not all atoms are neutral. This happens when the number of electrons is more than, or less than the number of protons. • The number of protons never changes, • however the number of electrons can change often.

  15. Shell Model of an Atom • Electrons occupy different shells. • 2 maximum electrons may fit in the first shell • The next shell holds 8 electrons, and the largest shell will hold 32 electrons. • For example, if an atom has 13 electrons, it will have 2 in the first shell, 8 in the second shell, and the remaining 3 will go in the third shell.

  16. Periodic Table • chart that lists atoms by their atomic number and by their electron arrangement. • As you move from left to right on chart each element gains one proton and electron . • As you go down each column each element has one more shell filled than the element above. • Elements in the same column are in a Group. Groups have similar properties.

  17. Atomic Number - number of protons in the nucleus • Atomic Mass – equals the average mass (in atomic mass units) of the nucleus • # of Protons = Atomic Number • # of Electrons = # of Protons, (if molecule has no charge) • # of Neutrons = (Atomic mass(rounded))- (atomic number)

  18. Phases of Matter • Solid, Liquid, Gas – three familiar states of matter. In all phases, atoms are in constant motion. • The more the molecules move the more fluid they become, • Solid – molecules have least energy, stay fixed relative to each other • Liquid- molecules have more energy, molecules move relative to one another • Gas – molecules have most energy, move with large distances between each other

  19. Plasma – the 4th State of Matter • Consists of positive ions and free electrons. Exists only at high temperatures. • What sun and stars are made of. Can be seen here on Earth in the glowing gas of fluorescent lamps.

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