Atoms – The Building Blocks of EVERYTHING

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Presentation transcript:

Atoms – The Building Blocks of EVERYTHING Foothill Chemistry

Law of Conservation of Mass

Law of Definite Proportions

Law of Multiple Proportions Sample of CO2 Mass of Carbon – 1 g Mass of Oxygen – 2.66 g Sample of CO Mass of Oxygen – 1.33 g Ratio of Mass of Oxygen in CO2 to Mass of Oxygen in CO – 2:1 Ratios are Small Whole Numbers

Dalton’s Atomic Theory All matter is composed of extremely small particles called atoms. Atoms of a given element are identical in size, mass, and other properties; atoms of different elements differ in size, mass, and other properties. Atoms cannot be subdivided, created, or destroyed. Atoms of different elements combine in simple whole-number ratios to form chemical compounds. In chemical reactions, atoms are combined, separated, or rearranged.

Dalton Was Good, but Not Perfect Isotopes of the Same Atom Differ in Mass Atoms are Divisible Into Smaller Particles

Cathode Ray Tube Experiment

Rutherford Experiment

Atomic Structure

Subatomic Particles Put it in perspective – If an atom is the size of the Houston Astrodome, the nucleus is a marble on the 50 yard line.

Isotope Notation (Element Symbol) 1H 1H 12C 6C 13C 6C 14C 6C Mass Number Charge (Element Symbol) Atomic Number 1H 1H 12C 6C 13C 6C 14C 6C Atomic Number = Number of Protons (the element # on the Periodic Table) Mass Number = Number of Protons + Number of Neutrons Charge = Number of Protons – Number of Electrons How Many Protons, Neutrons and Electrons are there in the Isotopes Listed Above?

Atomic Mass Unit Carbon-12 is the basis for the atomic mass unit (amu) An amu is defined as 1/12 of the mass of a carbon-12 atom Because there are 6 protons and 6 neutrons, the mass of one proton and one neutron are considered equal (1 amu)

Atomic Mass Weighted average mass of the atoms in a naturally occurring sample of the element

Mass, Mass, and More Mass Mass Number – Protons + Neutrons Atomic Mass Unit – 1/12 of carbon-12 mass Atomic Mass – Weighted average mass of the atoms in a naturally occurring sample of an element To be continued with … Molar Mass