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Bellringer 1.Who is credited with the development of the periodic table? 2.What is the difference between Mendeleev’s version of the periodic table and.

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Presentation on theme: "Bellringer 1.Who is credited with the development of the periodic table? 2.What is the difference between Mendeleev’s version of the periodic table and."— Presentation transcript:

1 Bellringer 1.Who is credited with the development of the periodic table? 2.What is the difference between Mendeleev’s version of the periodic table and the current version of the periodic table?

2 How Atoms Differ Objectives: 3.2 Calculating the number of protons, neutrons, and electrons in an isotope

3 Atomic Number Def.: the number of PROTONS in an atom What is the atomic number of: –Hydrogen? –Lead? –Chlorine? How many protons are in an atom of: –Hydrogen? –Lead? –Chlorine?

4 Atomic Number (cont.) What is the charge of a proton? Where are protons found? What else is in the nucleus? What would be the charge of the NUCLEUS of the following elements: –Hydrogen? –Lead? –Chlorine?

5 Atomic Number (cont.) What is needed to BALANCE this positive nuclear charge, so the atom is neutral? So how many electrons? Atomic number = number of protons = number of electrons How many electrons are in an atom of: –Hydrogen? –Lead? –Chlorine?

6 Practice & Assignment P.99: Study Guide workbook: p.21 (1-12)

7 Isotopes and Mass Number How Dalton’s atomic theory was wrong: –Atoms ARE divisible. (Who is credited with first splitting an atom?) –All atoms of a particular element are NOT identical. All atoms of an element do have the same number of protons and electrons, so what could differ?

8 Isotopes and Mass Number (cont.) Isotopes: atoms with the same number of protons (same element), but with different numbers of neutrons. Examples: –Potassium (K): K-39, K-40, K-41 –Chlorine (Cl): Cl-35 and Cl-37 –Uranium: U-235 and U-238

9 Isotopes and Mass Number (cont.) If atoms have the same number of protons and electrons, but different numbers of neutrons, what else will be different? Answer: MASS Mass number = number of protons + number of neutrons

10 Isotopes and Mass Number (cont.) Examples: –K-39 = 19 protons + 20 neutrons –K-40 = ___ protons + ___ neutrons –K-41 = ___ protons + ___ neutrons Isotope symbolic notation: mass number Element Symbol = 39 K atomic number 19 Isotope name is potassium-39

11 Isotopes and Mass Number (cont.) Review: 1.Number of protons is the same for all atoms of a particular element 2.Number of neutrons can vary ( = isotopes) What is the mass number? What is the atomic number? Number of neutrons = ?

12 Isotopes and Mass Number (cont.) Number of neutrons = mass number – atomic number Example: If an atom of neon has an atomic number of 10, and a mass number of 22: 1.How many protons? Neutrons? Electrons? 2.What is the NAME of the isotope? 3.What is the SYMBOL of the isotope?

13 Practice & Assignment Practice: p.101 (14) Study Guide Workbook: pp (13-23)

14 Mass of Individual Atoms Review: –Mass of proton = x g –Mass of neutron = ? –Mass of electron = 9.11 x g An atom of K-39, has ____ protons, _____ neutrons, and ______ electrons. Who wants to add up that actual mass?!?!

15 Mass of Individual Atoms (cont.) We ALL want to work with whole numbers, so scientists came up with the atomic mass unit (amu). Def.: 1/12 the mass of a carbon-12 atom (ALMOST equal to the mass of 1 proton or 1 neutron)

16 Mass of Individual Atoms (cont.) Review: What does the mass number of an element tell you? The mass recorded on the periodic table for an element is called atomic mass. Atomic mass is determined by the weighted average mass of the isotopes of that element.

17 Mass of Individual Atoms (cont.) What is the atomic mass for chlorine? Chlorine exists naturally as a mixture of % Cl-35 and % Cl-37. What do Cl-35 and Cl-37 mean? The ACTUAL masses of these isotopes would be amu and amu. The math: (75.770% x ) + (24.230% x ) = amu What was the atomic mass of chlorine?

18 Practice & Assignment Remember, to calculate atomic mass: 1.Calculate mass contribution of each isotope by multiplying its mass x its % abundance. 2.Add together all the mass contributions. P.104: (Practice) Assignment: P. 113 (59-68)


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