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Understanding Isotopes and Atomic Structure: Key Concepts in Chemistry

This guide explores essential concepts in chemistry, focusing on isotopes and atomic structure. It explains isotopic notation, determining mass and atomic numbers, and distinguishing between balanced atoms and isotopes. Key details include the number of neutrons in an isotope, the significance of atomic mass, and the characteristics of valence electrons. The document also covers electron configuration and concepts like Hund's rule and the Aufbau principle. Ideal for students seeking to deepen their understanding of atomic theory and isotopic behavior.

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Understanding Isotopes and Atomic Structure: Key Concepts in Chemistry

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  1. VS MILLIONAIRE!

  2. 234 Pu 94 • Look at the following isotopic notation: • What is the mass number? 234 • What is its atomic number? 94 • Is this a balanced atom or an isotope? isotope • How many neutrons are present in its nucleus? 140 • What is this isotope called? Plutonium 234 • In a balanced state, how many electrons does this element have? 94

  3. Electron dot notation communicates what? The number of valence electrons Look at the following dot notation: Ar • How many valence electrons does this element have? 8 • Is this element stable or unstable? Very stable, it is a noble gas

  4. When an atom has more or less electrons than it has protons it is called a(n) isotope • Atoms that have more electrons than protons are called ions. • Atoms that have more protons than electrons are called ____cations__________. • The weighted average of an element’s isotopes determine its atomic mass. • Electrons in the outermost energy level of an atom are called valence electrons.

  5. Name the particles in an atom in order of least to most massive electron, proton, neutron. • The positively charged, central part of the atom is called the nucleus. • Go to the board and write the isotopic notation of tritium (mass # 3) (see p. 94) • The sum of the number of neutrons and the number of protons is called the atomic mass number. • What does the abbreviation Z stand for? Atomic number • What is Hund’s rule? As electrons fill sublevels, all sublevels will receive one before any receive two.

  6. The Aufbauprinciple describes how electrons fill suborbitals (the high rise hotel analogy). • How does an isotope of an element differ from the balanced atom of the same element? It will have more or less neutrons than protons. • Go to the board and write the correct electron configuration for magnesium Z=12. 1s2 2s2 2p6 3s2

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