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Atoms and Elements - Survey of Chemistry I | CHEM 1151K, Study notes of Chemistry

Material Type: Notes; Professor: Osborne; Class: Survey of Chemistry I; Subject: Chemistry; University: Gordon College; Term: Spring 2010;

Typology: Study notes

2009/2010

Uploaded on 05/03/2010

ewhaley
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General, Organic, and Biological Chemistry Copyright© 2010 Pearson Education, Inc.
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Chapter 3 Atoms and Elements
3.6
Electron Energy Levels
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Chapter 3 Atoms and Elements

Electron Energy Levels

Electromagnetic Radiation

Electromagnetic radiation  (^) is energy that travels as waves through space  (^) is described in terms of wavelength and frequency  (^) moves at the speed of light in a vacuum speed of light = 3.0 x 10 8 m/s

Learning Check

  1. Which of the following has the shortest wavelength? A. microwaves B. blue light C. UV light
  2. Which of the following has the lowest energy? A. red light B. blue light C. green light

Solution

  1. Which of the following has the shortest wavelength? C. UV light
  2. Which of the following has the lowest energy? A. red light

Atomic Spectrum

An atomic spectrum consists of  (^) lines of different colors formed when light from a heated element passes through a prism  (^) photons emitted when electrons drop to lower energy levels

Example of Atomic Spectra

Energy Level Changes

 (^) An electron absorbs energy to “jump” to a higher energy level.  (^) When an electron falls to a lower energy level, energy is emitted.  (^) In the visible range, the emitted energy appears as a color.

In each of the following energy level changes, indicate if energy is

  1. absorbed 2) emitted 3) not changed A. An electron moves from the first energy level ( n =
  2. to the third energy level ( n = 3). B. An electron falls from the third energy level to the second energy level. C. An electron moves within the third energy level.

Learning Check

Sublevels

Sublevels  (^) contain electrons with the same energy  (^) are found within each energy level.  (^) are designated by the letters s, p, d, and f The number of sublevels is equal to the value of the principal quantum number (n ).

Number of Sublevels

Orbitals

An orbital  (^) is a three-dimensional space around a nucleus where an electron is most likely to be found  (^) has a shape that represents electron density ( not a path the electron follows)  (^) can hold up to 2 electrons  (^) contains two electrons that must spin in opposite

s Orbitals

An s orbital  (^) has a spherical shape around the nucleus  (^) increases in size around the nucleus as the energy level n value increases  (^) is a single orbital found in each s sublevel

Sublevels and Orbitals

Each sublevel consists of a specific number of orbitals_._  (^) An s sublevel contains one s orbital.  (^) A p sublevel contains three p orbitals.  (^) A d sublevel contains five d orbitals.  (^) An f sublevel contains seven f orbitals.

Electrons in Each Sublevel