ATOMIC STRUCTURE.

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Presentation transcript:

ATOMIC STRUCTURE

Label the following: Nucleus protons neutrons electrons

Simplified view of the atom

Protons = positive charge + electrons= negative charge - neutrons= no charge 0

ATOMIC MASS Inside the nucleus (mainly) protons + neutrons unit is AMU find on periodic table (round to whole #)

ATOMIC NUMBER Number of protons cannot change! Identifies element

IONS Charged atoms: NOT neutral p> e positive p< e negative example: 11p 11e 12 n neutral Na 11p 10 e 12n ion Na+

ISOTOPES Different number of neutrons than stable atom usually radioactive atomic mass is different than stable atom example: 234U

History of atomic stucture ttp://atomictimeline.net/index.php Rutherford’s experiment

Can we see atoms? STM- scanning tunneling microscope Invented 1981 Shows arrangement of atoms Gold

element- same atoms bonded together Compound- two (or more) different atoms bonded Mixtures- two (or more) different materials NOT bonded Minerals?-

WORKSHEET P= e= n= atomic mass= atomic number= how to recognize an ion? How to recognize an isotope?

TO CALCULATE # OF NEUTRONS Atomic mass (p+n) atomic number (p) SUBTRACT!

Sample problems 11 p 12 n 10 e 19 p 21n 19 e 25 p 30 n 21 e Cr+3 234 Pu