Open Question
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Ch.22 - The Main Group Elements
Chapter 22, Problem 158
In the early 1960s, krypton was found to react with fluorine gas in an electrical discharge tube at -183 °C. The compound formed was KrF2. What are the oxidation states of Kr and F in this compound? What is the electron-dot structure and geometry?
Verified step by step guidance1
Step 1: Determine the oxidation states of Kr and F in KrF_2. Start by knowing that fluorine (F) is more electronegative and typically has an oxidation state of -1.
Step 2: Since there are two fluorine atoms, the total oxidation state contributed by fluorine is 2(-1) = -2.
Step 3: The compound KrF_2 is neutral, so the sum of the oxidation states must be zero. Therefore, the oxidation state of Kr must be +2 to balance the -2 from the fluorine atoms.
Step 4: Draw the electron-dot structure for KrF_2. Krypton (Kr) is a noble gas with a full valence shell, but in KrF_2, it forms bonds with two fluorine atoms. Each fluorine atom shares one pair of electrons with krypton.
Step 5: Determine the geometry of KrF_2. With two bonding pairs and no lone pairs on the central atom (Kr), the geometry is linear according to VSEPR theory.
Related Practice
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