Slideshare uses cookies to improve functionality and performance, and to provide you with relevant advertising. If you continue browsing the site, you agree to the use of cookies on this website. See our User Agreement and Privacy Policy.

Slideshare uses cookies to improve functionality and performance, and to provide you with relevant advertising. If you continue browsing the site, you agree to the use of cookies on this website. See our Privacy Policy and User Agreement for details.

Like this presentation? Why not share!

No Downloads

Total views

4,949

On SlideShare

0

From Embeds

0

Number of Embeds

17

Shares

0

Downloads

39

Comments

0

Likes

2

No embeds

No notes for slide

- 1. Counting Atoms<br />Chapter 3.3<br />
- 2. Objectives<br />Explain what isotopes are<br />Define atomic number and mass number, and describe how they apply to isotopes.<br />Given the identity of a nuclide, determine its number of protons, neutrons, and electrons.<br />Define mole in terms of Avogadro’s number, and define molar mass.<br />Solve problems involving mass in grams, amount in moles, and number of atoms of an element<br />
- 3. Atomic Number<br />Symbol – Z<br />Number of protons in nucleus of atom<br />Determines the identity of the atom!!!!!<br />C - 6<br />He - ___<br />F - ___<br />Pb - ___<br />Use periodic table to find these!<br />Since atoms are neutral atomic number is also number of electrons<br />So C also has 6 electrons<br />He - ____ electrons<br />
- 4. Isotopes<br />All Hydrogen atoms contain 1 proton<br />Many naturally occurring elements can contain different numbers of neutrons.<br />Isotope – at0ms of the same element that have different masses.<br />n<br />n<br />n<br />Protium<br />99.985 %<br />Deuterium<br /> 0.015 % <br />Tritium<br />Trace<br />Three isotopes of Hydrogen<br />
- 5. Mass Number<br />Mass number – total number of protons and neutrons in the nucleus of an isotope<br />Symbol – A<br />Protium has 1 proton and 0 neutrons <br />Mass number = #p + #n<br /> = 1 + 0<br /> = 1<br /><ul><li>What is the mass number deuterium and tritium?
- 6. Find on periodic table</li></li></ul><li>Designating Isotopes<br />Hyphen Notation <br />Name of atom – mass number<br />Uranium - 235<br /><ul><li>Nuclear symbol
- 7. A X A : mass number, Z : atomic number, X : symbol of element
- 8. 235U</li></ul>Z<br />92<br /><ul><li>Number of protons Neutrons Electrons</li></ul> 92 143 92<br /><ul><li>Nuclide – general term for any isotope of any element</li></li></ul><li>Relative Atomic Mass<br />Oxygen – 16 , mass of 2.657 x 10-23 g<br />Easier to use relative scale<br />Need arbitrarily chosen standard<br />All others are compared to carbon - 12<br /><ul><li>One atomic mass unit (1 amu) – exactly 1/12 the mass of a carbon – 12 atom.
- 9. All others are compared to carbon -12
- 10. Hydrogen – 1 , about 1/12 the mass of carbon -12
- 11. Precise value is 1.007825 amu
- 12. Magnesium – 24 , Slightly less than twice that of carbon -12
- 13. Precise value is 23.985042 amu</li></li></ul><li>Average Atomic Mass of Elements<br />Most elements occur naturally as mixtures of isotopes<br />Average atomic mass : weighted average of the atomic masses of the naturally occurring isotopes of an element<br />Ex. of weighted average<br />Box contains two types of marbles, 25% have mass of 2.00g, and 75% have a mass of 3.00 g.<br />25 marbles x 2.00 g = 50 g<br /> 75 marbles x 3.oo g = 225 g<br />so 50 g + 225 g = 275 g (TOTAL MASS)<br /> 275 g ÷ 100 = 2.75 g average marble mass <br />
- 14. Calculating average atomic mass<br />Or<br />(2.00 g x 0.25) + (3.00 g x .75) = 2.75 g<br /><ul><li>Calculate the average atomic mass of copper
- 15. Use table 3-4 pg. 80 in text
- 16. Copper - 63 69.17% with mass of 62.929599 amu</li></ul> Copper – 65 30.83% with mass of 64.927793 amu<br />(0.6917 x 62.929599 amu) + (0.3083 x 64.927793 amu)<br />=63.55<br />Match with atomic mass on periodic table <br />Round to two decimal places in calculations<br />
- 17. Relating Mass to Numbers of Atoms<br />The MOLE<br />SI base unit for amount of a substance<br />Abbreviated as mol<br />Defined as : amount of substance that contains as many particles as there are atoms in exactly 12 g of carbon – 12<br />Counting unit just like a dozen<br />We don’t order 12 or 24 eggs, we order 1 or 2 dozen<br />In same way, a chemist may want 1 mol of carbon or 2 mol of iron.<br />63.55 g of copper or 1 mol of copper<br />
- 18. Avogadro’s Number<br />The number of particles in a mole – AVOGADRO’S NUMBER<br />6.022 x 1023particles in exactly one mole of a pure substance<br /><ul><li>How big is this number?
- 19. If every person on earth (5 billion people) counted 1 atom per second, it would take 4 million years to count all the atoms.</li></li></ul><li>Molar Mass<br />Molar mass – mass of one mole of a pure substance<br />Units : g/mol<br />Numerically equal to atomic mass of element<br />Mass of 6.02 x 1023 atoms of element<br />One mole He 6.02 x 1023atoms 4.oo g<br />One mole Li 6.02 x 1023atoms6.94 g<br />One mole Cu 6.02 x 1023atoms63.5o g<br />One mole Fe 6.02 x 1023 atoms 55.78 g<br />
- 20. Gram/Mole Conversions<br />Mass <br />In grams<br />Moles <br />In mol<br />Atoms <br />In atoms<br />Avogadro’s Number<br />Molar mass<br />What is the mass in grams of 3.50 mol of the element copper, Cu?<br />A chemist produced 11.9 g of Aluminum, Al. How many moles of aluminum were produced? <br />How many moles of silver, Ag, are in 3.01 x 1023 atoms of silver?<br />What is the mass in grams of 1.20 x 1023 atoms of copper, Cu?<br />
- 21. The Ten Commolements<br />(found at http://members.tripod.com/~smalls42/commolements.html)<br />Thou shalt not use 6.02 x 1023 in vain. <br />Thou shalt not use the term mole if thou has no true knowledge of the term mole. <br />Thou shalt not kill a mole. <br />Thou shalt not covet your neighbor's mole. <br />Thou shall always remember to celebrate Mole Day. <br />Thou shalt not disparage Mole Day. <br />Thou shalt not use a mole out of season. <br />Thou shalt always honor the one who introduced thou to Mole Day. <br />You shalt always keep sacred 10/23. <br />Thou shalt always remember these commolments or thou will never properly celebrate Mole Day. <br />

No public clipboards found for this slide

×
### Save the most important slides with Clipping

Clipping is a handy way to collect and organize the most important slides from a presentation. You can keep your great finds in clipboards organized around topics.

Be the first to comment