Practical Chemistry TEST Objectives/Notes: Unit 6: ELECTRONS IN ATOMS Use a periodic table to determine the correct number of protons, neutrons, and electrons in a particular atom. o Atomic # equals # protons and # electrons in an atom o # Neutrons = Mass # minus # Protons Understand the electron configuration as given in the Periodic Table. o Distinguish between ground and excited states. Label a Bohr diagram of an atom including the electron energy shells. o Label the subatomic particles, their symbols, charges, mass, and location. Identify valence electrons and distinguish them from kernel electrons. o Draw Lewis (Electron) Dot structures for atoms. o Know the Octet Rule requiring no more than eight electrons in the valence shell. o Kernel: includes the nucleus and all inner electron shell electrons (NOT valence). Distinguish between isotopes of an element; know isotopic notation. o Remember, isotopes have the same atomic number! (But different # neutrons.) o Isotopic Notation for carbon: C-12 or 126C. Distinguish between the Bohr and the Orbital models of the atom. o Term orbital indicates most likely location of an electron (probability). o Each electron in an atom has a distinct amount of potential energy. Distinguish between ground state and excited state configurations of an atom. o Use the electron configuration given in the Reference Table as the ground state. o Ground State: electrons occupy their lowest possible energy level. o Excited State: electrons occupy higher energy levels while lower levels are vacant. Define the term principal energy level. o The principal energy level (n) is the number of energy levels as shown in the electron configuration on the periodic table. Ex: carbon has a configuration of 2-4. This means there are two principal energy levels, n=1 containing 2 electrons, and n=2 containing 4 electrons. Explain the cause of spectral lines in terms of electrons and energy levels. o State how Bright-Line spectra are produced in terms of energy states of an electron. o Distinguish between continuous and bright-line spectra. o Know that each element has its own unique bright-line spectrum.