Summary: Introduction To Organic Chemistry | William H Brown, et al

Read the summary and the most important questions on Introduction to Organic Chemistry | William H. Brown; Thomas Poon

• 1 Covalent Bonding and Shapes of Molecules

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• 1.1 How do we Describe the Electronic Structures of Atoms?

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• What are the principle energy levels?

  The principle energy levels are the space to which an electron in confined to move within.

• How are electrons further grouped?

  1. The principle energy levels or Shells.
  2. The subshells s, p, d and f.
  3. Orbitals, each containing a maximum of 2 electrons

• How are the orbitals distributed within the shells?

  1. 1 s orbital in each shell
  2. 3 p orbitals in each shell, except the first shell
  3. 5 d orbitals in each shell, except the first two shells
  4. 7 f orbitals in each shell, except the first three shells

• What are the first 10 elements of the periodic table?

  Hydrogen, Helium, Lithium, Berylium, Boor, Carbon, Nitrogen, Oxygen, Fluor, Neon

• What is the element of the periodic table with atomic number 8? And what is the electron configuration?

  Oxygen, 1s2 2s2 2px2 2py1 2pz1

• What is a lewis structure?

  A representation of an electron with it's valence electrons drawn.

• 1.2 What is the Lewis Model of Bonding?

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• How is an ionic bond formed?

  An ionic bond is formed when an electron transfers from the valence shell of an atom with lower electronegativity to one with higher electronegativity.

• When does ionic transfer of electrons occur?

  The guideline is when the difference in electronegativity is 1,9 or greater.

• What is a dipole and how can you display this?

  A dipole is when there is a seperation of charge within a covalent bond or molecule. This can be displayed in a electron density model, with blue showing the more negative part and red the more positive part.

• What is the formal charge and how to derive it?

  The formal charge is the charge on an atom or molecule and can be derived by:
  1. Writing down the Lewis structure.
  2. Assign al unshared electrons.
  3. Compare the number of electrons with the number of electrons in the neutral, unbonded atom.