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Chapter 4: Atomic Structure

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Presentation on theme: "Chapter 4: Atomic Structure"— Presentation transcript:

1 Chapter 4: Atomic Structure
Subatomic Particles Symbol Notation Isotopes Average Atomic Mass

2 Democritus Atom: smallest part of an element that retains the identity of that element. Democritus ( B.C.): believed in tiny, indivisible, indestructible particles he called “atomos.” He had NO experimental proof!

3 John Dalton’s Atomic Theory (1803-1807)
All elements are composed of tiny indivisible particles called atoms. Atoms of the same element are identical; atoms of different elements are different. Atoms of different elements can mix in whole number ratios to form compounds. Chemical reactions cause atoms to separate and recombine, NOT change into different atoms.

4 Subatomic Particles

5 Comparing Subatomic Particles
Charge Mass (amu) Location Discoverer proton 1+ 1 nucleus Thomson neutron Chadwick electron 1- 1/1840 outside nucleus The proton gives identity to an atom, the electron gives personality.

6 Mass Number & Atomic Number
Mass Number = Number of protons + neutrons Atomic Number = Number of protons

7 Complete the Table Symbol Atomic Number Mass Number Number of p+
Number of n0 Number of e- 9 10 Na 15 47 25 55 S2- 32 Ga3+ 39

8 Mass of Atoms Mass of atom is very small! Heaviest atom is 4 x 10-22g.
Diameters of atoms: pm (1-5 angstroms) 1 A = 10-10m Both pm and A are commonly used for diameters.

9 Isotopes Have the Same…
Number of protons Atomic Number Number of electrons

10 Isotopes Have Different…
Number of neutrons Mass Number Mass n0

11

12 Isotopes of Hydrogen Hydrogen-1 Hydrogen-2 Hydrogen-3 Protium
Deuterium Tritium

13

14 Atomic Mass Unit (amu) 12 C 6 1 atom of carbon-12 = 12 amu
carbon-12 isotope used as standard 1 atom of carbon-12 = 12 amu carbon-12 has 12 particles with mass mass of proton = 1 amu mass of neutron = 1 amu 12 C 6

15 Average Atomic Mass Weighted average of all isotopes
Seen as mass number on periodic table Units in amu

16 To Calculate Average Atomic Mass You Need…
Number of Isotopes Mass of Isotopes Percent Relative Abundance

17 Calculating Average Atomic Mass
Mass x Rel. Abundance Average Atomic Mass Isotope A Isotope B

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