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Assignment #9 Atomic # = p+ = e- (neutral atom)

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1 9 10 14 15 47 25 55 Assignment #9 Atomic # = p+ = e- (neutral atom)
Mass # = p+ + n0 Atomic number Mass Number of protons p+ neutrons n0 electrons e- Symbol of element 9 10 14 15 47 25 55 19 9 9 F 14 Si 14 29 22 22 - 25 22 Ti 25 = 30 25 Mn Periodic Table of Elements

2 Pb Ch. 5 Practice Problem 11 Calculate Average Mass Mass # = p+ + n0
Lead 82 207.20 Ch. 5 Practice Problem 11 Calculate Average Mass Mass # = p+ + n0 82p 122n 82p 124n 82p 125n 82p 126n % abundance: 1.37% 26.26% 20.82% 51.55% Mass # 204 206 207 208 1.37 100 No amu mass shown. Use mass # instead. x Mass (amu) Relative abundance (% as a decimal) Lead-204 204 x 0.0137 = Lead-206 206 x 0.2626 = Lead-207 207 x 0.2082 = + Lead-208 208 x 0.5155 = 207.21

3 Modern Atomic Theory All matter is composed of atoms.
Atoms of the same element are chemically alike with a characteristic average mass which is unique to that element. Atoms cannot be subdivided, created, or destroyed in ordinary chemical reactions. However, these changes CAN occur in nuclear reactions! Atoms of any one element differ in properties from atoms of another element The exact path of electrons are unknown and e-’s are found in the electron cloud based on probability.

4 Incorrect View Correct View Atomic Theory
Are positive Contains protons Democritus Indestructible particle Extremely Dense Lacked evidence nucleus Atomic Theory Please add other vocabulary or scientists ideas related to atomic theory

5 Isotope Symbol Atomic number Mass number Protons Neutrons Electrons Cobalt-60 Iron-56 66 30 52 28 50 60 Co 27 60 27 27- 60-27= 33 27 56 Fe 26 56 26 26- 56-26= 30 26 42 Ca 20 42 20 20- Calcium-42 42-20= 22 20 66 Zn Zinc-66 30 66-30= 36 30- 30 52 Chromium-52 24 Cr 52-28= 24 24- 24 116 Tin-116 Sn 50 50- 50+66= 116 50 Atomic # Co Cobalt 27 58.93 Fe Iron 26 55.85 Zn Zinc 30 65.39 Cr Chromium 24 52.00 Sn Tin 50 118.71 Atomic mass (average)

6 Isotope Symbol Atomic number Mass number Protons Neutrons Electrons 14 -12 130 -54 11 23 26 12 12 Magnesium-26 Mg 12+14=26 12 75 As 33 75 Arsenic-75 33 33- 75-33= 42 33 130 Xe 54 54 Xenon-130 130-54= 76 54 23 Na Sodium-23 11 23-11= 12 11- 11 22 11 Sodium-22 Na 11- 11+11=22 11 Atomic # Mg Magnesium 12 24.31 As Arsenic 33 74.92 Xe Xenon 54 131.29 Na Sodium 11 22.99 Atomic mass (average)

7 Explain the difference between mass number and average atomic mass.
Mass number refers to the total protons and neutrons in a specific isotope. Atomic mass refers to all the isotopes masses averaged based on their relative abundance. Also called “Average Atomic Mass” or “Atomic Weight”.

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