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by: Nick Manning

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# General Chemistry I Exam 1 Study Gide CHEM - 10060 - 001

Marketplace > Kent State University > Chemistry > CHEM - 10060 - 001 > General Chemistry I Exam 1 Study Gide
Nick Manning
KSU
GPA 4.0

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An updated spin-off of Dr. Leslie's posted study guide, includes important formulas, comments, valuable concepts, and explanations.
COURSE
GENERAL CHEMISTRY I
PROF.
TBA
TYPE
Study Guide
PAGES
4
WORDS
CONCEPTS
Chemistry
KARMA
50 ?

## 3

1 review
"Better than the professor's notes. I could actually understand what the heck was going on. Will be back for help in this class."
Cassie Legros PhD

## Popular in Chemistry

This 4 page Study Guide was uploaded by Nick Manning on Wednesday January 27, 2016. The Study Guide belongs to CHEM - 10060 - 001 at Kent State University taught by TBA in Fall 2015. Since its upload, it has received 71 views. For similar materials see GENERAL CHEMISTRY I in Chemistry at Kent State University.

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## Reviews for General Chemistry I Exam 1 Study Gide

Better than the professor's notes. I could actually understand what the heck was going on. Will be back for help in this class.

-Cassie Legros PhD

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Date Created: 01/27/16
General Chemistry I Study guide for Exam 1 in Chem-10060 on Friday, th February 19 over Chapters 1-4. CHAPTER 1  Important to know:  SI units- conversion, prefixes, (factors not given!)  Convert between volume, mass, and density o D=m/v o Volume and Density with displacement  = putting an item in a graduated cylinder of water and measuring how much the water moves up  Convert between temperature units o F=(9/5)*C + 32 o C= (F-32)*5/9  SIGNIFICANT FIGURES & SIG FIG RULES o Addition/ Subtraction- # of places after the decimal o Multiplication/ Division- # of digits after the first nonzero digit  Ex: 13.41 = 4 sig figs  15 = 2 sig figs  13.00 = 4 sig figs CHAPTER 2  Atomic structure o Dalton & Rutherford models  Element Info o Name from symbol o Symbol o # of protons, neutrons, electrons o Atomic mass o Relative atomic mass from isotopic abundance  = Average atomic weight from table  Ion info o # of protons, neutrons, electrons o Charge  Periodic Table o Groups = vertical columns o Period = horizontal rows o ID elements from table o Charge/ covalent bonds element will form  Number of columns away from Noble Gas  Ionic/Covalent Compounds o POLYATOMIC IONS o Which Metals need Roman Numerals & which don’t  ALL Transitions except Ni, Ag, Zn, Cd, Pb, Sn o Name any ionic/covalent compound given formula CHAPTER 3  Write a balanced/ be able to balance a chemical equation  Find molar mass and % composition given chemical formula o Use periodic table!  Empirical Formula o What it is and how to find it from  Mass or % composition  Molecular Formula o What it is and how to find it from given mass data and molar mass  Convert between moles, mass, or # of particles o Molar Mass = g/mol, symbol = M o Avogadro’s Number: 1 mole= 6.022x10^23 entities  Only use when question asks for number of  Atoms  Molecules  Particles  Entities  Find amount of reactant and product used or formed based on a balanced equation o Ratio of moles (Example 2 mols Ca/1 mol C; found in the numbers in front of the symbols of elements in a reaction)  Know to find limiting/excess reagents o Calculate mass of product that could possibly be formed in this scenario  Know % Yield o (Actual yield/ Theoretical yield) x 100%  Combine a series of reactions into one all-inclusive reaction o use this for mass/mole calculations  Molar concentration, given mass of solute & volume of solution o M= Moles solute/Liters of solution o MOLARITY, formula above o Convert between moles, mass, volume, molarity o Dilution Calculations  M1V1=M2V2 CHAPTER 4  Understand why ionic substances conduct electricity when dissolved in solution but not when solid o When the substance is put in a solution, the structure breaks down and electricity can be conducted  Why molecular substances are non-electrolytes in solution o Molecular structures are fixed so the H2O cannot tear them apart  Find out if an ionic substance is soluble or insoluble (solid) based on solubility rules o Know the solubility rules  Write a balanced equation to depict dissociation of a soluble ionic substance  Balanced equation for mixing two ionic substances o Identify precipitates o Molecular, total ionic, and net ionic equations  Molecular- basic equation, shows two solutions as two solutions  Total Ionic- separates the components of each solutions  Net Ionic- equation without spectator ions  Spectator Ions- Ions that are present in the same form in both the reactant equation and the product equation

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