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CHM 115 Week 1 Notes

by: Jasmine Padgett

CHM 115 Week 1 Notes CHM 11500 - 001

Jasmine Padgett
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About this Document

These notes are over atoms
General Chemistry
Cynthia A Harwood
Class Notes




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This 2 page Class Notes was uploaded by Jasmine Padgett on Sunday January 24, 2016. The Class Notes belongs to CHM 11500 - 001 at Purdue University taught by Cynthia A Harwood in Fall 2015. Since its upload, it has received 193 views. For similar materials see General Chemistry in Chemistry at Purdue University.

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Date Created: 01/24/16
Chemistry 111 Lecture 1 SI Base Units (can see on pg. 2 Table 1.2 of review packet) Physical Quantity Unit Name Unit Abbreviation Mass kilogram kg Length meter m Time second s Temperature kelvin K Electric current ampere A Amount of substance mole mol Luminous intensity candela cd  The structure of a neutral atom is mainly just empty space with a nucleus of a positive - - charge and negative electrons (e ) surrounding the nucleus in the e cloud  Compared to the entirety of the atom, the nucleus is extremely tiny Isotopes  Every and all atoms of a specific element will always have the same number of protons (p ) o The number of protons determines the atomic number  Isotopes are atoms of an element that have the same number of p but a different number of neutrons (n ) + 0 o To find the mass number you add together the amounts of p and n in an atom + 0 A (p + n ) X Z: X=Atomic Symbol, A=Mass Number, Z=Atomic Number Ion Structure  If e are removed from an atom that is neutral, it becomes a positive ion, also known as a cation  If e are added to a neutral atom, it becomes a negative ion, also known as an anion Atoms and Molecules  Molecules are formed from combinations of atoms o “an independent structure of two or more atoms bound together” (see pg. 42 of textbook)  Law of Multiple Proportions: “a mass law stating that if elements A and B react to form two or more compounds, the different masses of B that combine with a fixed mass of A can be expressed as a ratio of small whole numbers” (see pg. 46 of textbook) *In order to have a properly balanced equation, you must have the same number and types of atoms in both the reactants as well as the products*


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