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    Chemistry 2
    Chemistry 2
    Chemistry 2
    Ebook53 pages22 minutes

    Chemistry 2

    By BarCharts Publishing, Inc.

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    About this ebook

    Answers at your fingertips to the essentials of a subject that is challenging at best and that many students struggle with. The 6 page laminated guide focuses on physical chemistry with the details and structure of the subject organized and designed to be a key to the answers that are further supported by your texts and lectures. Use as a review before testing, or as a memory companion that keeps your mind focused on the whole course daily, weekly, or as needed before exams.

    Suggested uses:
    o Students – especially relevant for those majoring in engineering, science, or a health care related field
    o Quick Reference – instead of digging into the textbook to find a core answer you need while studying, use the guide to reinforce quickly and repeatedly
    o Memory – refreshing your memory repeatedly is a foundation of studying, have the core answers handy so you can focus on understanding the concepts
    o Test Prep – no student should be cramming, but if you are, there is no better tool for that final review
    LanguageEnglish
    PublisherBarCharts, Inc.
    Release dateMay 1, 2018
    ISBN9781423237501
    Chemistry 2

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      Book preview

      Chemistry 2 - BarCharts Publishing, Inc.

      Table of Contents

      Intermolecular Forces

      Changes in Matter

      Solutions

      Chemical Kinetics

      Acids & Bases

      Thermodynamics

      Electrochemistry

      Radioactivity

      Intermolecular Forces

      Types of Intermolecular Forces

      Intermolecular forces: Forces between molecules, atoms, or particles

      Can be attractive or repulsive

      Are generally weaker than bonding forces

      Relates to Coulomb’s law:

      E =

      =

      Dispersion forces (London forces)

      Occurs in all molecules and atoms

      Created by the variability in the distribution of electrons outside the nucleus

      Electrons are randomly arranged at any one point in time

      The arrangement creates a temporary/instantaneous dipole

      The magnitude is dependent on the ease of polarization of electrons

      Polarize: Form a dipole moment

      Depends on the molar mass and the molecular Shape

      Polarity

      Polarity depends on differences in electronegativity (ΔEN)

      Electronegativity: Ability of an atom to attract electrons

      Nonmetals have higher electronegativity than metals

      ΔEN > 2.0: Ionic bond (nonpolar); electrons are transferred

      ΔEN 0–0.4: Covalent bond (nonpolar); electrons are shared equally or nearly equally

      ΔEN 0.4–2.0: Covalent bond (polar); electrons are shared unequally

      Polar molecules have electron-rich and electron-poor areas

      Polarity helps determine liquids’ miscibility, the ability to mix

      Practical applications

      Water is a polar molecule and grease and oil are nonpolar, so they don’t mix

      One end of a soap molecule is polar and the other nonpolar, so soap can attract both water and grease

      Dipole-dipole force

      Occurs in all polar molecules, which have:

      A permanent dipole

      Dispersion forces

      Higher melting and boiling points

      Hydrogen bonding

      Occurs in polar molecules with hydrogen atoms

      Is the strongest of all intermolecular forces

      Has a strong dipole-dipole attractive force

      Hydrogen atoms bond with fluorine, nitrogen, and oxygen

      Water has hydrogen bonds—without it, all Earth’s water

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