Topic 2 – Atomic Structure

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Presentation transcript:

Topic 2 – Atomic Structure The Atom

The Atom The atom is the smallest particle of matter.

Element Notation Atomic Number (AN) – Number of Protons = Number of Electrons Mass Number (MN) – Protons + Neutrons n = MN - AN Example: P= N= E=

Composition Consists of Protons, Neutrons and Electrons. Mass (amu) Charge Where? Protons 1 +1 nucleus Neutrons Electrons 5x10-4 -1 Energy shells

Notation Mass Number Atomic Number Charge Mass Number Atomic Number Mass Number: Number of Protons and Neutrons in the Nucleus Atomic Number: Number of Protons and the number of Electrons Charge: The losing or gaining of electrons results in a charge ± n

Isotopes Different atoms of the same element containing the same number of protons but a different number of neutrons. Thus they have different mass numbers but have identical chemical properties. Physical properties differ.

Exercise: 6 6 6 #P _______ _______ _______ #N _______ _______ _______ Naturally occurring carbon consists of three isotopes, 12C, 13C, and 14C. State the number of protons, neutrons, and electrons in each of these carbon atoms. 12C 13C 14C 6 6 6 #P _______ _______ _______ #N _______ _______ _______ #E _______ _______ _______ LecturePLUS Timberlake

Radioactive Isotopes Many isotopes are radioactive once their nucleus breaks down spontaneously. 60Co => 60 Ni + β There are three forms of radiation: Alpha - α Beta - β or 0 e Gamma - γ

Relative Atomic Mass The mass of an atom when compared to the mass of 1/12 Carbon. Find the Relative Atomic Mass of Oxygen: