Electronic Configuration and Oxidation States of Transition Metals

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Anonymous
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191367
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Electronic Configuration and Oxidation States of Transition Metals
Updated:
2013-01-04 10:12:10
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Chemistry
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Advanced Higher Chemistry - Unit One - Electronic Configuration and Oxidation States of Transition Metals
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  1. The d block transition metals are metals with an incomplete _ subshell in at least one of their ions?
    d
  2. Which two transition metals are the exception to the Aufbau principle and why?
    Chromium and copper atoms because the atoms are more stable with a half filled d block of electrons
  3. When transition metals form ions are electrons first lost from the s or d block?
    The s block
  4. An element is said to be in a specific oxidation state when it has a specific oxidation...?
    number
  5. What is the oxidation number of an uncombined element?
    0
  6. In most compounds, what oxidation number does hydrogen have?
    +1
  7. In metallic hydrides what is the oxidation number of hydrogen?
    -1
  8. What oxidation number does fluorine have in all its compounds?
    -1
  9. What oxidation number does oxygen have in most of its compounds?
    -2
  10. For ions, what is the general rule about oxidation numbers?
    The oxidation number of an ion is the same as the charge on the ion eg the oxidation number of Na+ is +1, Cl - is -1, ect
  11. The sum of all the oxidation numbers of all the atoms in a molecule or neutral compound must add up to...?
    0
  12. The sum of all the oxidation numbers of all the atoms in a polyatomic ion must add up to...?
    the charge on the ion
  13. Is oxidation defined as an increase or decrease in oxidation number?
    Increase
  14. Is reduction defined as an increase or decrease in oxidation number?
    Decrease
  15. Do compounds containing metals in high oxidation states tend to be oxidising or reducing agents?
    Oxidising
  16. Do compounds containing metals in low oxidation states tend to be oxidising or reducing agents?
    Reducing

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