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The Atom

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

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The Atom

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

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

  3. 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

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

  5. 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 #

  6. DETERMINING NUMBER OF SUBATOMIC PARTICLES Protons: Same as the atomic #. Neutrons : Mass # - Atomic # Electrons: Same as the # of protons

  7. 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.

  8. 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.

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