Module 2

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Author:
faulkner116
ID:
172843
Filename:
Module 2
Updated:
2012-12-10 17:11:56
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Objective 17 20
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  1. define valence
    is the same as the number of electrons that will be taken to form anions or the number of electrons which will be given away to form cations.
  2. what is the outer shell of electrons called
    valence shell
  3. define covalent bond
    bond formed between two or more atoms that share electrons
  4. because atoms "want" to gain or shed electrons to fill outer shells, valence also describes how many
    positions one moves on the periodic table to reach a noble gas column
  5. define a double covalent bond
    when two electrons are shared equally
  6. Triple covalent bond is when
    three electrons are shared from each atom
  7. define a polar covalent bond
    This kind of bond means that the atoms have a partial charge on them, so it has poles and it's called polar.  Because this kind of bond has characteristics of a polar bond and a covalent bond... polar covalent bond
  8. define ionic bond
    when atoms hang out together because they have opposite charges.
  9. What atoms are in the human body that form polar covalent bonds
    • Oxygen
    • Nitrogen
    • Sulfur
  10. Ionic bonds are formed between
    metal and non-metal ions
  11. In a polar covalent bond the pull on electrons is measured in a quality called
    electronegativity
  12. define hydrogen bonds
    are a special characteristic of compounds that contain hydrogen and oxygen, hydrogen and nitrogen, and hydrogen and sulfur
  13. define a dipole
    more positive charges at one end, more negative charges at the other
  14. what are the most common "electron thieves"
    • Oxygen
    • nitrogen
    • sulfur
  15. electronegative atoms form
    dipoles
  16. dipoles attract
    opposite charges
  17. Hydrogen atoms usually _______ electrons
    lose
  18. Bond strengths...... strongest to weakest
    • Covalent
    • triple
    • double
    • single

    • Ionic
    • Hydrogen

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