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ATOMIC STRUCTURE

ATOMIC STRUCTURE. ATOMIC STRUCTURE P + = PROTON N o = NEUTRON E --- = ELECTRON DIFFERENT WAYS TO WRITE ELEMENTS & THEIR SYMBOLS Phosphorus—31 AND 31 15 P ***NEUTRONS = mass # -- atomic #

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ATOMIC STRUCTURE

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  1. ATOMIC STRUCTURE

  2. ATOMIC STRUCTURE • P+ = PROTON • No = NEUTRON • E--- = ELECTRON • DIFFERENT WAYS TO WRITE ELEMENTS & THEIR SYMBOLS • Phosphorus—31 AND 3115P • ***NEUTRONS = mass # -- atomic # • ***isotopes--- atoms of the same element but with different numbers of neutrons (different mass #s) • Ex: P—32 and P—30

  3. Ex: phosphorus—31 Protons = 15 Electrons = 15 Neutrons = 16

  4. NUMBER THESE COLUMNS ON YOUR PERIODIC TABLE: • 1 2 13 14 15 16 17 18 • (1A) (2A) (3A) (4A) (5A) (6A) (7A) (8A) • Vertical columns—groups or families • --- there are 18 total (8A groups and 10B groups) • Horizontal rows—periods or series • ---there are 7 rows total

  5. VALENCE ELECTRONS-- the outermost electrons having the highest amount of energy and are farthest from the nucleus and the ones involved in chemical reactions • ** # of valence electrons = “A” column # on the periodic table • (“A” group #) • ** # of energy levels = row # on the periodic table • Ex: Beryllium (Be): column 2A= 2 valence electrons • Row 2 = 2 energy levels • Ex: Phosphorus (P): column 5A = 5 valence electrons • Row 3 = 3 energy levels

  6. ATOMIC MATH PROBLEM • 1. Take the # of protons in oxygen X the # of electrons in fluorine = _______________ • 2. Take this number --- # of neutrons in chlorine = _________________ • 3. Take this number + silicon’s atomic # = ____________ • 4. Take this number / # of neutrons in helium = _____________ • 5.Take this number --- aluminum’s mass # = _____________

  7. Calculating average atomic mass using % abundance information • atomic mass-the average mass of all of an element's isotopes; you round this to actually get the mass number ***every element has at least 2 isotopes * **the most abundant isotope matches the mass # from the periodic table!! Ex: Which is most common? O-16 O-17 O-18

  8. Hydrogen has 3 known isotopes: H-1 (protium) occurs 99.9885% of the time with an atomic mass of 1.0078 amu H-2 (deuterium) occurs 0.0115% of the time with an atomic mass of 2.0141 amu H-3 (tritium) is synthetically made MASS OF EACH ISOTOPE X DECIMAL FORM OF THE % OF THE TIME IT OCCURS

  9. (1.0078 X 0.999885 ) + (2.0141 X 0.000115) 1.007684103 + 0.000231622 1.007915725 amu

  10. Calculate avg. atomic mass for “element Z” Z—10 occurs 75.5% of the time Z—11 occurs 20.5 % of the time Z—12 occurs 4.0 % of the time (10 x 0.755) + (11 x 0.205) + (12 x 0.040) 10.285 amu

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