Subatomic Particles. Atomic Particles ParticleChargeMass (kg)Location Electron9.109 x 10 -31 Electron cloud Proton+11.673 x 10 -27 Nucleus Neutron01.675.

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Presentation transcript:

Subatomic Particles

Atomic Particles ParticleChargeMass (kg)Location Electron9.109 x Electron cloud Proton x Nucleus Neutron x Nucleus

Atomic Number Atomic number (Z) of an element is the number of protons in the nucleus of each atom of that element. Identifies the element Element# of protonsAtomic # (Z) Carbon66 Phosphorus15 Gold79

Isotopes Isotopes are atoms of the same element having different masses due to varying numbers of neutrons. IsotopeProtonsElectronsNeutronsNucleus Hydrogen–1 (protium) 110 Hydrogen-2 (deuterium) 111 Hydrogen-3 (tritium) 112

Mass Number Mass number is the number of protons and neutrons in the nucleus of an isotope. Mass # = p + + n 0 Isotopep+p+ n0n0 e-e- Mass # Oxygen Arsenic Phosphorus153116

Calculating Average Atomic Mass expressed in atomic mass units (amu) –done because actual masses so small and hard to work with –based on carbon-12 assigned mass of exactly 12 amu weighted average of all naturally occurring isotopes.

change % abundances to decimals for each isotope Multiply abundance by atomic mass of isotope Add products to get average atomic mass for element Example Chlorine has two isotopes. The isotope with a mass of amu has a relative abundance of 75.77%. The isotope with a mass of amu has a relative abundance of24.33%. Calculate the atomic mass of chlorine. x = amu x = amufor 24.33% = for 75.77% = for Clatomic mass = = amu