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AU / Chemistry / CHEM 1030 / How can a mixture be separated?

How can a mixture be separated?

How can a mixture be separated?

Description

School: Auburn University
Department: Chemistry
Course: FUNDAMENTALS CHEMISTRY I
Professor: Yngard
Term: Spring 2017
Tags: General Chemistry
Cost: 50
Name: CHEM 1030 study guide
Description: Chapters 1-3
Uploaded: 09/18/2017
5 Pages 131 Views 1 Unlocks
Reviews


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Test If you want to learn more check out Who claimed that athens’ clean air and atmosphere contributed to the keenness of the attic mind?

9/22/17If you want to learn more check out What is the meaning of fidelity?

CHEM 1030

Ch. 1-3 Study Guide

Ch. 1 Scientific Method: (page 7)If you want to learn more check out What is the main question of management?

        Observe phenomena → create hypothesis → Test the hypothesis → Analyze results → Draw conclusions/Establish a theory

COAST Method for Problem Solving: (page 8)We also discuss several other topics like What are the different theories of child developement?

Collect and Organize, Analyze, Solve, and Think

Don't forget about the age old question of What is nosological system?

Mixture vs. Pure Substance (page 12)

       ↙  ↘                              ↘

              heterogeneous          CANNOT be separated easilyWe also discuss several other topics like What are the effects of abiotic and biotic factors?

homogeneous       ↓

↳ (Mixtures CAN be

separated by physical

processes)                

States of Matter (page 15)

  • solid - definite volume / shape
  • liquid - definite volume, not a definite shape
  • gas - neither definite volume nor definite shape

gases expand to occupy the entire volume of the available space

Melting       →            ←         condensation

SOLD←  freezing        LIQUID        vaporization → GAS

                        sublimation     →

                           ←        deposition

Forms of Energy (page 17)

  • energy - capacity to do word
  • work - exertion of force through a distance

W = F × d

  • Potential v. Kinetic Energy (page 18)

KE = ½ mu2 (m = mass, u = speed)

  • Law of conservation of energy - energy cannot be created or destroyed, but converted from form to form.

KNOW: molecular formula, structural formula, and the various types of models (Ch. 1 notes)

KNOW: how to express sigfigs, SI unit prefixes, precision v. accuracy, how to use SI units in conversions

Mean & Standard Deviation (page 33)

  • Mean - calculated average

mean =

  • standard deviation - measure of dispersion in the set of values

s =

  • Confidence interval - range of values around the calculated mean that probably contains the true mean value, μ

        μ = mean ± (values of t in table 1.5)

* Outlier - value that is unusually far from the mean value - not to  be ignored in a correctly-done experiment

Ch. 2 SubAtomic Particles (page 48)

  • electrons (e-) - negatively charged - located on orbitals around nucleus (same # as p+)
  • protons (p+) - positively charged - located in nucleus
  • neutrons (n) - neutral / no charge - in nucleus

        

        Atomic Structures through the Years (page 48)

  • Thomson - discovered e- exist & ratio of mass is consistent
  • Millikan - determined the charge of e- and its mass

*Note their theorized structures from the Chapter 1 powerpoint

↳ Rutherford later theorized the nucleus

Radioactivity (page 50)

  • term used to describe the spontaneous emission of high-energy radiation & particles by radioactive materials
  • radioactive particle : beta (ß) penetrates better (Beta = Betta!) alpha (α) doesn’t penetrate as well.
  • ß particles = high energy e-
  • radioactivity experiments done under Rutherford assisted in the discovery of the nucleus

Nuclear Atom (page 52)

  • protons & neutrons are centrally located in the “nucleus” of the atom and they make up most of the mass of the atom
  • atomic mass units = mass of carbon - 12
  • annu aka Daltons (Da) aka unified atomic mass units
  • p+ & n have much larger masses than e-

Review: A        Symbol format from

          Z ✖️        Ch. 2 Notes

KNOW : how to navigate the periodic table (Ch. 2)

Moles & Molar Masses (page 62)

  • mole-base unit for expressing quantity of substances
  • Avogadro’s Number (6.0221 ✖️ 1023) allows to convert from mols to atoms and vice versa (NA)
  • Molar Mass (μ) has exactly the same number value as the mass of one atom of the element expressed in annu

✖️ ✖️ ✖️ =

Mass Spectometry & Molecular Mass (page 69)

  • Molecular Ions -  molecules that have lost/gained e-, giving them a charge
  • Mass spectrum - when these ions are organized based on mass (m) and electrical charges (z) in an m/2 ratio.

* can be used to find isotopic abundances of elements (review page 71 & Ch. 2 Notes)

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