Atomic Mass Agenda Review (whiteboards) Read 4.7 & 4.8 Notes Homework.

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Presentation transcript:

Atomic Mass Agenda Review (whiteboards) Read 4.7 & 4.8 Notes Homework

Parts of Atomic Theory Atoms of the same element are identical Atoms can rearrange – reactions Atoms can mix in whole number ratios – compounds Atoms are indivisible – no subatomic particles according to Dalton

How do isotopes differ? Number of neutrons in nucleus

How do ions differ? Number of electrons Cations have lost electrons to gain positive charge Anions have gained electrons to have negative charge

146C ____ p+ ____ e- ____ no 6 8

94Be+2 ____ p+ ____ e- ____ no 4 2 5

3617Cl- ____ p+ ____ e- ____ no 17 18 19

Read section 4.7 & 4.8 w/ partner Six inch voices Grab book Read section 4.7 & 4.8 w/ partner Six inch voices

Average Atomic Mass date

Average atomic mass A WEIGHTED average dependent on the percent abundance of each isotope. If all isotopes were in a bag, how frequently would you pull out each separate isotope. Measured in amu’s

Atomic Mass Unit An amu is the mass of a single proton. 1 amu = 1.67*10-24 g

Determining Average Mass Multiply Mass number by Percent abundance. Add the answers. Answer should be close to most abundant isotope.

Example Cesium is 75% 133Cs, 20% 132Cs, 5% 134Cs. What is the average atomic mass? 133*.75 132*.20 134*.05 132.85 amu Closest to the most abundant isotope

Example Chromium has four istopes. 4.35% 50Cr, 83.79% 52Cr, 9.5% 53Cr, 2.36% 54Cr. What is the average atomic mass of Cr? 50*.0435 52*.8379 53*.095 54*.0236 52.0552 amu

Determining % abundance Create an equation equaling average atomic mass Mass1 * %X + Mass2 * %Y = average atomic mass Create an equation equaling 100% X + Y = 1 Use substitution to solve for x. Mass1 * %X + Mass2 * %(1-X) = average atomic mass

Let one isotope be X and the other 1-X 10.013X + 11.009(1-x) = 10.812 The average atomic weight of boron is 10.812amu. Boron has two isotopes: boron-10 with a mass of 10.013 and boron-11 with a mass of 11.009. What are the % abundances of each isotope? Let one isotope be X and the other 1-X 10.013X + 11.009(1-x) = 10.812 10.013X + 11.009 – 11.009X = 10.812 0.197 = 0.996X 0.1978 = X Boron-10 is 19.78% abundant Boron-11 is 80.22% abundant

What are the % abundances of the two isotopes of rubidium What are the % abundances of the two isotopes of rubidium? Average atomic mass 85.4678 amu Rb-85, 84.9918 amu Rb-87, 86.9092 amu Let X be for Rb-85 and 1-X for Rb-87 84.9918X + 86.9092(1-X) = 85.4678 84.9918X + 86.9092 – 86.9092X = 85.4678 1.4414 = 1.9174X 0.7517 = X Rb-85 is 75.17% abundant Rb-87 is 24.83% abundant

Homework Complete isotopes and average atomic mass worksheet Review scientists and discoveries. Lab report due Rough draft Wednesday Final draft Friday