1 / 14

Subatomic Particles

Learn about subatomic particles, atomic numbers, mass numbers, isotopes, and atomic mass. Understand the role of protons, neutrons, and electrons in atoms.

alicesalazar
Download Presentation

Subatomic Particles

An Image/Link below is provided (as is) to download presentation Download Policy: Content on the Website is provided to you AS IS for your information and personal use and may not be sold / licensed / shared on other websites without getting consent from its author. Content is provided to you AS IS for your information and personal use only. Download presentation by click this link. While downloading, if for some reason you are not able to download a presentation, the publisher may have deleted the file from their server. During download, if you can't get a presentation, the file might be deleted by the publisher.

E N D

Presentation Transcript

  1. Subatomic Particles

  2. 1. Subatomic Particles

  3. Special notes on subatomic particles • In a neutral atom # of protons=#of electrons. • If the number of protons does not equal the number of electrons you have a charged atom known as an ion. • # protons > # electrons forms a + ion (cation) • # electrons > # protons forms a – ion (anion) • Most of the mass of an atom is in nucleus.

  4. Atomic Number (z) • 1913—Henry Mosley • Used to identify an atom • Indicates the number of protons • In a neutral atoms also gives the number of electrons

  5. 3. Mass Number (A) • Total number of protons and neutrons in the nucleus of an atom. (nucleons) • Notation: AXZ • Mass # = #protons + # neutrons • # neutrons = Mass # - # protons

  6. Try the following:

  7. 19F9 9 protons 19-9=10 neutrons 9 electrons 19F9-1 9 protons 10 neutrons 10 electrons 24Mg12 12 protons 24-12=12 neutrons 12 electrons 24Mg12+2 12 protons 12 neutrons 10 electrons Determine the # of protons, neutrons, and electrons for these added examples:

  8. Isotopes • Thomson (1912) found 2 types of neon atoms and Soddy (1910) found 2 types of uranium atoms. • 2 elements that have the same atomic number but different mass numbers • Based on atomic structure: 2 elements that have the same number of protons but different number of neutrons. • For example: Cl-35 and Cl-37

  9. 5. Atomic Mass • Decimal number • Average of all the naturally occurring isotopes for a particular element • If you round the atomic mass it gives you the mass number for the most common isotope. • Unit is amu (atomic mass unit) • 1 amu is 1/12 the mass of C-12 • Gram atomic mass= amu but in grams

  10. Try the following: • Determine the number of protons, neutrons, and electrons for the following isotopes of hydrogen: Solution: Hydrogen-1 (protium) 1H1 1p,0n,1e Hydrogen-2 (deuterium)2H1 1p,1n,1e Hydrogen-3 (tritium) 3H1 1p,2n,1e

  11. Naturally occurring chlorine consists of 75% Cl-35 and 25% Cl-37. Find the average atomic mass. • .75(35) + .25(37)= 35.50 amu or • 75(35) + 25(37) =35.50 amu 100

  12. 3. Calculate the atomic mass of an element with isotope A occurring 70.0% of the time with a mass of 13.0 amu and isotope B occurring 30.0% of the time with a mass of 15.0 amu. • .70 (13.0) +.30 (15.0) =13.6 amu

  13. An element X has three isotopesX-30 has a 50.0% abundance, X-28 has a 30.0% abundance and X-31 has a 20.0% abundance. • .500(30) + .300(28) + .200 (31) = 29.6 amu

  14. 5. There are two isotopes of element Z, 60.0% of the atoms have a mass of 58.0 amu and 40.0% have a mass of 57.0 amu. Calculate theatomic mass of element Z. • .600(58.0) + .400(57) = 57.6 amu

More Related