CHM103 Class Notes Week 3 (9/5-9/9)
CHM103 Class Notes Week 3 (9/5-9/9) 103
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This 2 page Class Notes was uploaded by askcch on Friday September 9, 2016. The Class Notes belongs to 103 at University of Miami taught by Elliot Atlas in Fall 2016. Since its upload, it has received 8 views. For similar materials see Chemistry for Life Sciences I (Lecture) in Chemistry at University of Miami.
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Date Created: 09/09/16
CHM103 lass Notes Week 3 9/59/9) ________________________________________________________________________________ From revious ections 1.61.10 Units and Scientific Notations, Significant Figures and Rounding, Unit Conversions and Estimating Answers ________________________________________________________________________________ Chapter 1: atter and Measurements 1.11 Temperature, eat, and Energy Energy: the capacity to do work or supply heat 1000cal = 1kcal, 1000J = 1KJ, 1cal = 4.184J, 1kcal = 4.184KJ Heat (cal) = Mass (g) x Temp Change (Δ℃) x Specific Heat (cal/(g*℃) Temperature: ℉, ℃, ℃ and K are the same size (^ 1℃ = ^ 1K), but DIFFERENT in starting point 0℃ = freezing point of water, 273.15℃/ 0K = Absolute Zero 32℉ = 0℃, 212℉ = 100℃, ^ 1℃ ^ .8℉ Professor didn’t finish the whole chapter in class ________________________________________________________________________________ Chapter 2: Atoms and the eriodic Table 2.1 Atomic heory nd he Structure of Atoms Atomic heory: 1. All matter is composed of atoms 2. The atoms of a given element differ from the atoms of allother elements 3. Chemical compounds consist of atoms combined in specific ratios. Only whole atoms an combine 4. Chemical reactions change only the way atoms are combined in compounds Protons: carry a positive lectrical charge Neutrons: have a mass similar to that of a proton, but are electrically neutral Electrons: very small in mass, carry a negative electrical charge All atoms are neutral and have o net charge Number of protons = Number of electrons, to balance out Atomic mass unit (amu) is the unit for describing the mass of an atom 1amu = 1.660539 x 10^24 g = 1/12 wt of 1 C12 atom The protons and neutrons are packed densely together, forming the nucleus Opposite lectrical charges attract ach other Like charges repel each other 2.2 Elements and tomic Number Atomic Number is the number of protons in atoms of a given element Mass Number is the sum of the protons and neutrons in an atom 2.3 Isotopes and tomic Weight Isotopes are toms ith dentical atomic numbers but different mass umbers A specific isotope s epresented by The isotopes of most elements do not have distinctive names The mass number A is given after the name of the element (e.g. Uranium235, Carbon12) Most naturally occurring elements are mixtures of isotopes
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