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Welcome to Chemistry! Oct 14, 2015 Wednesday Do now: if you clearly have a Agenda: –Finish Work on st4 hetrogenous mixture what are classwork #2 Look at st 3 some ways you can separate assessment it? (Pick up periodic table up front) Objectives: St 4: Matter: Understand the structure of an atom in terms of its subatomic particles; isotopes and ions; differentiate between the classification and separation of matter (mixtures, pure substances…) IONS: LEARN EM! Atomic Structure introduction Assignments: Mass volume lab final report due Thursday St 4 cw 1 and 2 check off thursday The Week: Thursday Atomic practice Periodic table • This is your copy to use for any assessement (except the ion assessment) • You make make any handwritten notes on it you want. ( I will give some hints on that through out the year) • Find a safe and easily accessible place for it. – If you don’t have a pocket you can make one out of the provided cardstock later today in your notebook. Right hand side!!!!! If you have mystery substance consider putting the substance through these steps * Can it physically be separated? See 1 and 2 2. If your sample looks uniform, and you get a result for Distillation and Chromotography Then yes for homo.mixture I. If you get a result (solids) with Filtration , Decanting and Centrifuging then you have a hetro.mixture 3. Electrolysis Also here here Standard 3 check in • • • • • Retake will be next week St 3 classwork is due Friday if not done? DPSE solving method Sample problem? If you know that gold has a density of 19.6 g/mL and you have 354ML of Gold ( a pop can!) then how many grams is that? How much money is that worth 37 dollar/gram Right hand side!!!!! 10/14/15 EQ: What is the landscape of an atom? Matter Matter: Anything that has mass and takes up space. Atoms Building blocks of matter. Contains subatomic particles: abbreviations Electrons E Neutrons N Protons P Subatomic Particles Protons and electrons are the only particles that have a charge. Protons and neutrons have essentially the same mass. The mass of an electron is so small we ignore it. Symbols of Elements Mass number (number of protons plus neutrons) Atomic number (number of protons) C 12 6 Resulting Charge Symbol of the Element Elements are symbolized by one or two letters. Atomic Number Mass number (number of protons plus neutrons) Atomic number (number of protons) C 12 6 Resulting Charge Symbol of the Element All atoms of the same element have the same number of protons Atomic Mass Mass number (number of protons plus neutrons) Atomic number (number of protons) C 12 6 Resulting Charge Symbol of the Element The mass of an atom in atomic mass units (amu) is the total number of protons and neutrons in the atom. Determining Electrons Mass number (number of protons plus neutrons) Atomic number (number of protons) Resulting Charge C 12 6 Symbol of the Element In elements the # of protons = the # of electrons, so the element is electrically neutral and no charge is shown. However atoms can gain or lose electrons to become ions and the resulting charge is shown. Isotopes •Atoms of the same element with different masses. •Isotopes have different numbers of neutrons. Carbon actually has 15 different isotopes! 11 C 6 12 C 6 13 C 6 14 C 6 • Protons = electrons in Atoms • Protons ≠ electrons in Isotopes Isotopes •Your periodic tables show an AVERAGE atomic mass. •Round this to the nearest whole #. •On our tables, atomic mass of carbon is 12.01 •IRL: •98.9 % is Carbon-12 It averages to 12.01 •1.1% is Carbon-13 •.0001% is Carbon-14 11 C 6 12 C 6 13 C 6 14 C 6