ATOMIC_STRUCTURE_AHL(MAH)_(NXPowerLite) Opp

ATOMIC_STRUCTURE_AHL(MAH)_(NXPowerLite) Opp - 100s of free...

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1 ATOMIC STRUCTURE Advanced Higher Level 100’s of free ppt’s from www.pptpoint.com library
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2 Topic 12: Atomic Structure(3h) 12.1 Electron Configuration State the relative energies of s, p, d and f orbitals in a single energy level.
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3 Topic 12: Atomic Structure(3h) 12.1.1 Explain how evidence from first and successive ionization energies across periods accounts for the existence of the main energy levels and sub-levels in atoms. Interpretation of graphs of first ionization and successive ionization energies versus atomic number provides evidence for the existence of the main energy levels and sub-levels. Aim 7: Spreadsheets, databases and modeling software can be used here.
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4 12.1.4 State the maximum number of orbitals at each energy level. 12.1.5 Draw the shape of an s orbital and the shapes of the px, py and pz orbitals. 12.1.6 Apply the Aufbau principle, Hund’s rule and the Pauli exclusion principle to write electron configurations for atoms and ions up to Z=54 For Z = 23 the full electronic configuration is 1s 2 2s 2 2p 6 3s 2 3p 6 4s 2 3d 3 or [Ar] 4s 2 3d 3 or [Ar] 3d 3 4s 2 . Exceptions to the principle for copper and chromium should be known. Students should be familiar with the representation of the spinning electron in an orbital as an arrow in a box.
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5 FIRST IONIZATION ENERGIES OF SUCCESSIVE ELEMENTS The first ionization energy IE1 is the energy required to remove the one electron from a gaseous atom or one mole of electrons from one mole of isolated gas atoms. Write down the chemical equations that describe the first ionization energy of helium and sodium. In the plot on the next slide it is apparent that there are periodic patterns to the first ionization energies. Learning check: Can you remember the definition of “periodicity” in chemistry?
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6 Can you describe the general trend across a single period? Can you describe the “fine structure” of the general trend within a period? After a class discussion, and reading the information below, can you explain in your own words, how evidence from first and successive ionization energies across periods accounts for the existence of the main energy levels and sub-levels in atoms.
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7 First Ionization Energy
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8 The periodic trends can be used as evidence for electrons in main shells and sub-shells When a singly positively charged ion is formed, the effective nuclear charge increases (i.e. the ratio of the number of protons to the number of electrons) and thus it takes more energy to remove the next electron. IE2 is always greater than IE1. Each subsequent electron becomes harder to remove as the effective nuclear charge increases still more.
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9 Within a given row the ionization energy increases with increasing atomic number. Atoms with filled or half-filled subshells have higher
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This note was uploaded on 11/17/2011 for the course PHYS 121 taught by Professor Burgeson during the Fall '11 term at BYU.

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ATOMIC_STRUCTURE_AHL(MAH)_(NXPowerLite) Opp - 100s of free...

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