Mary J Bojan Chem 110 3 Structure of the atom Properties of the atom Atoms

Mary j bojan chem 110 3 structure of the atom

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Mary J. Bojan Chem 110 3 Structure of the atom Properties of the atom Atoms combine to form molecules Molecules react Energy in chemical reactions Matter & Energy Identity and structure of atom Components of atom Atomic number Average atomic mass isotopes Intro to energy Kinetic energy Potential energy Electrostatic energy Heat and work System & surroundings Exothermic & endothermic enthalpy State function light Electromagnetic spectrum Wavelength and frequency Avogadro’s number Ebook Chapter 1 Mary J. Bojan Chem 110 4
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5 Lessons 01-1-3 Learning Objectives Upon completion of Lessons 01-1-3, you should be able to: Apply the technique of dimensional analysis to various chemical problems. Define the term isotope. Calculate the number of protons, neutrons, and electrons for different isotopes and ions. Calculate the average atomic mass for an element, given its isotopes and percent abundances. Using knowledge of Avogadro’s Number and the mass-mole relationship, calculate masses of individual atoms or molecules, mole quantities from mass amounts, mass quantities from mole amounts, and particle quantities from mass or mole amounts. Mary J. Bojan Chem 110 6 We will use SI (= metric) base units, derived SI units, and common prefixes See the Metric Unit Skill Check for details and practice. The common base units and important prefixes are given below. Review: Scientific Measurement: All measured quantities consist of a number and a unit. SI Base Unit Mass Kilogram (kg) Length Meter (m) Time Second (s) Temperature Kelvin (K) Important Prefixes mega- (M) 10 6 Kilo- (k) 10 3 centi- (c) 10 –2 milli- (m) 10 –3 micro- (μ) 10 –6 nano- (n) 10 –9 You must be able to fluently convert within metric units. Prefixes and conversions will not be given on an exam. Mary J. Bojan Chem 110
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Review: Pure substances can be elements or compounds. Mary J. Bojan Chem 110 7 Elements : Smallest units of matter that still preserve their chemical identity. Examples: Ar (g), Fe (a metal), O 2 (g) Compounds : Substances composed of two or more elements that are chemically combined (bonded) in fixed proportions. Examples: H 2 O( ), NaCl(s) Mixture: Substances are physically present in the same place, but are not chemically bonded. They can be separated into pure substances by physical means (without changing the identity of the components).
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  • Fall '17
  • Joseph Houck
  • Atom, Chem, Mary J. Bojan

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