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chemistry 135

by: Esraa Hagag

chemistry 135 chem135

Esraa Hagag
Northampton Community College

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these notes cover the week of September 26 and first Monday of October
chemistry of life
edward s fleming
Class Notes
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This 3 page Class Notes was uploaded by Esraa Hagag on Tuesday October 4, 2016. The Class Notes belongs to chem135 at Northampton Community College taught by edward s fleming in Fall 2016. Since its upload, it has received 4 views. For similar materials see chemistry of life in Chemistry at Northampton Community College.

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Date Created: 10/04/16
Chapter 7 Chemical reactions In a chemical reactions one or more pure substances are changed or transformed into  new and different substances  reactants products  reactants and products are given by chemical symbols and formulas  all chemical reactions involve release or absorption of energy formula weight:  every chemical formula stands for two things  the smallest particles of compound (nanoscale)  an large aggregated of small particles that can be handled (macroscale) molecular compounds: 1. nanoscale  formula tells us kind and number of atoms in “molecule”  give us the weight or mass of a “molecule” e.g. H 2:   1 molecule of water consists of two atoms of hydrogen and one atom of  oxygen  Tells us the mass of one molecule of water is 2x mass of H plus mass of  oxygen Mass (1 H O2molecule) = (2x) mass of H + (1x) mass of O                          = 2(1) + 1(16) = 18 amu Ionic compounds:  Formula gives us the ratio of + to – ions in crystal  Also gives formula weight  e.g. CaI 2: 1 Ca  for every 2 i­ mass of Cai  2 mass of Ca  + (2x) mass of i ­ Cai 2= 40 + 2(127) = 294 amu 2. Macroscale:   Individual atoms, ions, molecules too small to be dealt with  Need to have a large quantity of small particles so we can deal with them  on macroscale  To overcome this problem, the unit used for small particles, is the mole, mole  23 is equal to 6.02*10  units (Avogadro’s number: number in front of chemical  formula is coefficient: tells us the number of moles that compound N S Al So 4 O 1 3 2 3 12 2 6 4 6 24 0.5 1.5 1 1.5 6 On macroscale a chemical formula or element symbol stand for one mole Molar mass:  Chemical formula also gives the mass in grams of the substance   Molar mass= sum of atomic weight of substituent elements   e.g. H 2  nanoscale: 18 atomic mass unit (amu)   macroscale: 18 grams (the weight of one mole of H2O  molar mass of water is 18 grams/mole  e.g. CaI 2  nanoscale: 294 amu  macroscale: 294 g/mole (weight of 1 mole of CaI2)  molar mass of CaI =2294 g/mole  one mole of any substance contains Avogadro’s number of particles (atoms, ions, or  molecules) but they have different molar masses (mm) molar/grams interconversion:  number of moles of particular substance equals mass of substance over molar mass moles= mass/molecular mass moles=g*moles/g mass =number of moles * mm g= moles*g/mole Page 216 no. 7.4 a. number of Li atoms in 4.5 moles Li 23 24 atoms= 4.5*(6.02*10 ) atoms/mole= 2.71*10  atoms


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