Multiple Choice
Which of the following correctly describes the Lewis dot structure for the copper(II) chloride ion, CuCl2?
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11. Bonding & Molecular Structure
Lewis Dot Structures: Ions
Multiple Choice
Which of the following correctly represents the Lewis dot structure for the ions in potassium oxide (K2O)?
A
Each K atom loses one electron to become K^+, and the O atom gains two electrons to become O^{2-}, resulting in [K^+] [O^{2-}] [K^+]
B
The O atom loses two electrons to each K atom, forming O^{2+} and two K^- ions
C
Both K atoms and the O atom retain their valence electrons, with no electron transfer
D
Each K atom shares one electron with the O atom, forming covalent bonds between K and O
Verified step by step guidance1
Identify the elements involved and their typical ionic behavior: Potassium (K) is an alkali metal that tends to lose one electron to form K^+ ions, while oxygen (O) is a nonmetal that tends to gain two electrons to form O^{2-} ions.
Determine the total number of valence electrons before ion formation: Each K atom has 1 valence electron, and the O atom has 6 valence electrons, so for K_2O, total valence electrons = 2(1) + 6 = 8 electrons.
Consider electron transfer based on typical ionic bonding: Each K atom loses one electron (becoming K^+), and the O atom gains two electrons (becoming O^{2-}), resulting in a transfer of electrons rather than sharing.
Represent the ions with their charges and electron configurations: Write the potassium ions as K^+ (no valence electrons shown in the Lewis structure) and the oxide ion as O^{2-} with a full octet of electrons represented as dots around the oxygen symbol.
Combine the ions to form the ionic compound: The Lewis structure is shown as [K^+] [O^{2-}] [K^+], indicating that the compound consists of two potassium cations and one oxide anion held together by ionic bonds.
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