# of Subatomic particles Atomic Mass - calculate

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# of Subatomic particles Atomic Mass - calculate What’s inside? Properties The Atom Periodic Table # of Subatomic particles Atomic Mass - calculate

Contains 99.9% of the mass of the atom. WHAT’S INSIDE NUCLEUS The “core” of the atom. Contains 99.9% of the mass of the atom. ELECTRON CLOUD Area around the nucleus.

SUBATOMIC PARTICLES PROTON Located in the nuceus Charge – positive Mass = 1 amu (atomic mass unit) Neutron Located in the nucleus Charge – neutral Mass – 1 amu (atomic mass unit) ELECTRON Located outside the nucleus in the “electron cloud” Charge – negative Have very little mass - 9.11 x 10⁻28 g/ 0 amu

PROPERTIES OF ATOMS OF DIFFERENT ELEMENTS What makes one atom different from another? The number of subatomic particles in the atom. Gold Mercury

PERIODIC TABLE INFORMATION ATOMIC NUMBER: The number of protons located in the nucleus of the atom. Identifies the element Will never change!!! MASS NUMBER: How many protons and neutrons are in the nucleus of the atom. Protons + Neutrons = Mass #

DETERMINING NUMBER OF SUBATOMIC PARTICLES Element Number of Protons Number of Electrons Number of Neutrons Atomic Number Mass Number Manganese 25 30 Sodium 11 12 Bromine 35 45 Yttrium 39 89 Arsenic 33 75 Actinium 227 Protons: Same as the atomic #. Neutrons : Mass # - Atomic # Electrons: Same as the # of protons

Number that shows on the periodic table. AVERAGE ATOMIC MASS Number that shows on the periodic table. Average of all the isotopes of an element. An isotope is an atom that has the same number of protons but differing numbers of neutrons, changing the mass of the atom.

CALCULATING ATOMIC MASS Determine the mass contribution of each isotope of the element. (relative abundance x mass of isotope) Add the mass contributions together. Note that you do not divide!! Use significant figures in rounding answer.