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Understanding Chemistry Fundamentals: Atom, Moles, Light, and Periodic Trends

Explore the basics of chemistry, including the atom's structure, mole concept, properties of light, electron configurations, and the periodic table trends in ionization energy and electronegativity.

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Understanding Chemistry Fundamentals: Atom, Moles, Light, and Periodic Trends

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  1. Honors Chem Ch 3 Pg 68The Atom • Nucleus of positive protons and neutral neutrons • Energy levels of negative electrons outside nucleus • Mass = protons + neutrons only Pg 74 • Neutrons = mass – protons • Isotopes – same element with diff neutrons ex: carbon-12 and carbon-14 used in medical imaging

  2. Avogadro’s NumberThe Mole Pg 79 • Mole = 6.02 x 1023particles • Particles can be atoms for elements or molecules for compounds • Mole also = # grams from pd table • Given x wanted/given = wanted ex: Grams x mole/grams = moles ex: Mole x atoms/mole = atoms

  3. Ch 4 Pg 91 Light • Know spectrum from handout • Speed of light C = 3 x 108 m/s • C = wavelength in m x frequency in Hertz c=wf • Light is a photon particle that travels in a wave • Quantum is amt of energy of light given off by electron falling from higher unstable level • Energy = h x frequency E=hf • h = Planck’s constant 6.626 x 10-34J-s

  4. Electron ConfigurationsPg 105 and Pg 130 • Aufbau – fill levels starting with lowest • Pauli – 2 electrons per orbital, spinning in opposite directions • Hund – fill by putting one electron in each orbital in same direction, then put 2nd electron in other direction • Know how to write electron config, orbital notations with arrows, and noble gas notation

  5. Periodic Table Ch 5 Pg 130 • Designed by Russian scientist Mendeleev late 1800’s • Column 1 – alkali metals, lose 1 electron, +1 • Column 2 – alkaline earth metals, lose 2, +2 • Column 7 – halogens, make salts with col 1, gain 1 electron, -1 • Column 8 – noble gas, full outer levels, don’t react • Metalloids – stairstep line • D Block – transition elements, + but varying #+

  6. Trends • Atomic radiiPg 142 – smaller to the right due to more attraction between protons & electrons- larger to the bottomdue to morelevelsof electrons • Ionization energy Pg 145 – energy needed to remove an electron – higher to the right because almost full, lower to the bottom due to farther from nucleus • Electronegativity Pg 153– attraction for electrons – higher to right, lower to bottom

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