Chemistry - The Central Science Chapter 2

Chemistry - The Central Science Chapter 2 - Isotope All...

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Chapter 2 Atoms, Molecules and Ions I. Chemical Elements II. Atomic Particles III. Isotopes IV. Atomic Mass and Molecular Mass V. Nomenclature HW #P1 – 1.10, 1.13, 1.41, 1.49, 2.5, 2.8, 2.43, 2.48, 2.62, 2.91 P1 is covered on Q1.
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Chapter 2 I. Chemical Elements and Periodic Table Chemical Elements – 90 naturally occurring Everything is composed of these elements. Elements combine to form compounds. If one divides an element to the smallest unit, which retains identity " atom? Atoms combine to form molecules. H + H + O macroscopic scale atomic scale elements atoms compounds molecules
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II. Atomic Particles Each atom is composed of particles. Particle Charge Mass proton + 1.67 × 10 g -24 neutron none 1.67 × 10 g -24 electron --- 9.11 × 10 g -28 Protons and neutrons are the nucleus. Atom diameter is - 1Å; nucleus is 10 Å -4 Mass is in nucleus – nuclear density is 10 g/cm . 13 3 The number of protons gives the Atomic Number. The number of neutrons gives the
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Unformatted text preview: Isotope. All chemical changes are electronic involving a charge in the electrons (nuclear chemistry is the exception!) III. Isotopes Atomic number (the # of protons) specifies the atom. Atomic mass is the sum of protons and neutrons. 6 C Atomic number = 6 12 Atomic mass = 12 How Many Neutrons? How Many Electrons? Examples: 25 1) Mn How many protons, 55 neutrons, electrons? 25 2) Mn How many protons, 55 2+ neutrons, electrons? 3) (a) How are Cl and Cl different? 35 37 (b) If Cl is present in 75.5% and Cl is 35 37 present in 24.5%, what would atomic weight be for a natural mixture of Cl atoms? IV. Atomic Mass and Molecular Mass Atomic mass is obtained from periodic table or other source. H = 1.008 C = 12.01 O = 16.00 Molecular mass is the sum of atomic masses which make up the molecule. Examples: 2 (1) H O 2 (2) CO V. Nomenclature ( read 60-67)...
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