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Chemistry 111 EXam 1 Study Guide

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Chemistry 111 EXam 1 Study Guide 20002

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About this Document

Includes review from week of Jan 19 to Feb 10
Principles of Chemistry I
Charles Lake
Study Guide
Chemistry, General Chemistry
50 ?




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This 4 page Study Guide was uploaded by Notetaker on Sunday February 14, 2016. The Study Guide belongs to 20002 at Indiana University of Pennsylvania taught by Charles Lake in Spring 2016. Since its upload, it has received 27 views. For similar materials see Principles of Chemistry I in Chemistry at Indiana University of Pennsylvania.


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Date Created: 02/14/16
Chemistry 111 Exam 1 February 17, 2016 Define Element: Compound: Substance: Mixture: Physical change: Chemical change: Solid: Liquid: Gas: Intensive: Extensive: Name the compounds and the elements. 1) CO 2 2) Hg 3) CH 3CH 2OH 4) CH 4 5) Fe 6) H 2 What two measurements can or cannot be found based on something’s state of matter? List the changes of state and their relations to each other. True or False: Density is an intensive property of matter. Define Exact Number: Inexact Number: Accuracy: Precision: Mass: Weight: Energy: Heat: Specific Heat: Temperature: Explain the difference between accuracy and precision. How many significant figures are in each? 1) 67,000 mi 2) 6.0340 L 3) 100cm=1 m 4) 12 pencils 5) 250 m Which of the above has the most error? How many sig figs would be in the answer? 2.04m+34.1m (2.85)(67.45)/4.390 True or False: A percent is (x) out of whatever the total measurement. Solve: An ore of tin contains 35.67% tin (m/m). If you need to obtain 45. 3 g of tin, how many kg of tin ore must be purchased? Solve: An empty Erlenmeyer flask weighs 241.3g. When filled with water at 30 C 0 (d=0.99565 g/cm ), the flask and its contents weigh 489.1 g. a) What is the volume of water in the flask? b) How much does the flask weigh when filled with an equivalent volume of mercury (d=13. 534 g/mL)? What are the relative and absolute temperatures of the English and Metric systems? Define Absolute temperature: Density: Specific gravity: Atom: Ion: Cation: Anion: Protons: Neutrons: Electrons: Atom: Explain Dalton’s Atomic Theory. Explain what Rutherford’s experiment showed. True or False: You must know the temperature of what you are measuring to calculate specific gravity. Explain the characteristics of protons, neutrons, and electrons. Include charges and locations. True or False: Cations lose electrons. True or False: Anions gain electrons. True or False: All atoms are ions. 56 Fe 2+ 26 56 represents: 26 represents: Fe represents: 2+ represents: How many neutrons are found in this cation? List the nuclear particles. What are the elements found naturally? List the titles of the sections of the Periodic Table. What is the difference between a group and a period? What are the different groups? What are the different periods? Explain the differences between core and valence electrons. Define isotopes and give an example. Explain the difference between an average and a weighted average. How does the number of electrons an element needs to be stable affect its placement on the Periodic Table? What is Oxygen’s charge? Nitrogen? Carbon? True or False: Noble gases are not stable because they have low electronegativity. Place elements in order from highest to lowest EN P, Al, O, Ca, Rb Explain the relationship between oxidation and cations. Explain the relationship between reduction and anions.


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