Upload
katherine-jefferson
View
216
Download
0
Embed Size (px)
DESCRIPTION
Important Vocabulary Electromagnetic spectrum Emission spectrum Energy level Electron cloud Valence electrons Lewis dot diagrams Wavelength Frequency
Citation preview
Electrons in AtomsChapter 2 Section 2
Objectives How does the electron relate to the
modern atomic theory? How do electron energy levels in an atom
differ from one another? How are Lewis electron dot diagrams used
to illustrate valence electrons?
Important Vocabulary Electromagnetic spectrum Emission spectrum Energy level Electron cloud Valence electrons Lewis dot diagrams Wavelength Frequency
Electrons Motion & Energy Electrons have enough energy to keep
them in constant motion around the nucleus
This enables them to overcome the attraction of the positive nucleus
Electrons occupy orbitals of only certain amounts of energy
For them to move up a level of energy, energy must be added
For them to move down a level of energy, energy must be released in the form of light or heat
Waves Transfer Energy Energy is the ability to exert a force over a certain
distance It is also the ability to do work Waves carry energy because they can do work For example:
Water waves can transfer energy to a leaf, to a boat, or onto a beach
Sound waves can transfer energy to your eardrum
Light waves can transfer energy to your eye The bigger the wave the _______ energy it carries
Electromagnetic Radiation Electromagnetic radiation travels
in the form of waves that have both electric and magnetic properties
Electromagnetic waves travel through a vacuum at the speed of light (300 million m/s)
Two properties of waves are frequency and wavelength
Wavelength & Frequency• Wavelength is the distance from one crest to
the next• Frequency is the number of waves per second• A low frequency results in a long
wavelength and a high frequency results in a shorter wavelength
Electromagnetic Spectrum
The electromagnetic spectrum consists of electromagnetic radiation waves at all possible energies, frequencies, and wavelengths
The spectrum ranges from 103 m to 10-12 meters
Each part of the electromagnetic spectrum has unique properties
Radio Waves
Heinrich Hertz proved the existence of radio waves in the late 1880s
Radio waves have wavelengths that range from 200 to 600 m
Have the longest wavelengths and the lowest energy
They are used as TV signals, AM and FM radio signals, and for radar equipment
Radio telescopes view planets, comets, giant clouds of gas and dust, stars, and galaxies
Microwaves
Are low energy, low frequency radiation waves
They are used in Doppler radar for weather forecasting and to cook your food
Microwaves are also used to carry telecommunication signals
Most mobile phones use microwaves to transmit information, and space probes transmit signals back to Earth with microwaves
Different wavelengths of microwaves (grouped into "sub-bands") provide different information to scientists.
Infrared Waves In 1800, William Herschel discovered
them Have less energy than visible light Are given off by the human body
and other warm objects We experience infrared rays as heat
from fires and electric heaters Through night-vision goggles and
infrared thermal cameras we can see infrared waves
Visible Spectrum Cone-shaped cells in our eyes act as
receivers tuned to the wavelengths in this narrow band of the spectrum
A typical human eye will respond to wavelengths from about 380 to 750 nm
The spectrum does not contain all the colors that the human eye and brain can distinguish
Unsaturated colors such as pink, and purple colors such as magenta, are absent because they can only be made by a mix of multiple wavelengths
When white light shines through a prism, the white light is broken apart into the colors of the visible light spectrum
Water vapor in the atmosphere can also break apart wavelengths creating a rainbow
Ultraviolet Waves In 1801, Johann Ritter discovered them Have shorter wavelengths than visible
light UV waves are invisible to the human
eye, but some insects, such as bumblebees, can see them.
The Sun is a source of the full spectrum of ultraviolet radiation, which is commonly subdivided into UV-A, UV-B, and UV-C
X-rays X-rays were first observed and documented in
1895 by German scientist Wilhelm Conrad Roentgen
X-rays have very small wavelengths, between 0.03 and 3 nanometers
X-rays are used by doctors to see the internal structures of the body
X rays have very high energies, so they may kill living cells or turn them into cancer cells when exposed to too much of this type of radiation
Gamma Rays Have the highest energy and shortest
wavelengths They are produced by the hottest and
most energetic objects in the universe, such as neutron stars and pulsars, supernova explosions, and regions around black holes
On Earth, gamma waves are generated by nuclear explosions, lightning, and the less dramatic activity of radioactive decay
Gamma rays can be used to treat cancer by killing the diseased cells
Electrons and Light When electrons become excited they give
off light The spectrum of light released is called the
emission spectrum Each element has a different emission
spectrum So it serves as evidence of energy levels
within atoms
Energy Levels There are seven levels of energy
available for electrons to occupy Electrons can move between energy
levels like the rungs of a ladder absorbing or releasing energy
The number of filled energy levels depends on the number of electrons
Lower levels are filled first
Energy Levels 1st energy level = 2 electrons 2nd energy level = 8 electrons 3rd energy level = 8 electrons 4th energy level = 18 electrons
For example: Na has 11 electrons 2 in level 1 8 in level 2 1 in level 3
Valence Electrons Every atom has between 1 and 8 valence electrons Valence electrons are electrons in the outermost
energy level of an atom They determine an atom’s chemical properties and
its ability for form bonds For example: Neon
Has 10 electrons2 electrons in the lowest level8 electrons in the 2nd level
Thus, it has 8 valence electrons!
Lewis Dot Diagrams Valence electrons are usually the only
electrons used in chemical reactions We represent valence electrons as
Lewis dot diagrams, which illustrate the valence electrons of an element as dots
Normally, all the elements within a group have the same electron dot structure with the exception of Helium
Lewis Dot Diagrams