College Chemistry Lesson 3
College Chemistry Lesson 3 CHM 111
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This 2 page Class Notes was uploaded by Kara Nichols on Wednesday May 25, 2016. The Class Notes belongs to CHM 111 at Calhoun Community College taught by Mona Chaudhary in Spring 2016. Since its upload, it has received 18 views.
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Date Created: 05/25/16
College Chemistry 1 – Mona Chaudhary 5/25/2016 Important Words or Important People Important Concepts Definitions Lesson 3 Matter o Has weight, shape, and mass Desk, classroom Composed of atoms Atom o Smallest unit that can be identified as a particular element o Fundamental Particles (building blocks) Proton P or p+ Mass ≈ 1 amu Charge = +1 Location = in the nucleus Neutron n or n0 Mass ≈ 1 amu Charge = +1 Location = in the nucleus Electron e or e Mass ≈ 0 Charge = -1 Location = outside the nucleus o Concentric circles Atomic Number (Z) o Always a whole number o The number of protons in the nucleus + o Z = # p o Identifies element in the periodic table Hydrogen Z = 1 Helium Z = 2 Z = 17? Chlorine (Cl) Z = 76? Osmium (Os) o Neutral atoms The number of protons = the number of electrons + - H is different than H or H Cl Cl- H H+ Li2 + + + + + p = 17 p = 17 p = 1 p = 1 p = 3 e = 17 e = 18 e = 1 e = 10 e = 1 ANION CATION CATION Mass Number o Always a whole number + 0 o A = p + 0 o A-Z = n Isotopes: Isotopes o Atoms of the same element with different masses p = 29 p = 29 o All isotopes have the same number of protons (Z)63 65 29 Cu e = 29 29 Cu e = 29 o May have a different number of neutrons n = 34 n = 36 Atomic Weight / Mass o ALWAYS a decimal number o Weighted average of all the isotopes of a particular element o Round to two places after the decimal Ions o Charges particles formed from a gain or loss of electrons The number of protons stays the same o Cation – positive charge – less electrons than protons o Anion – negative charge – more electrons than protons
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