Multiple Choice
Which of the following ions will form a compound with the bicarbonate ion (HCO_3^-) in a 1:1 cation to anion ratio?
2. Atoms & Elements
Ions
Struggling with General Chemistry?
Join thousands of students who trust us to help them ace their exams!Watch the first videoMultiple Choice
Which of the following ions is isoelectronic with the oxide anion O^{2-}?
A
N^{3-}
B
F^{-}
C
Cl^{-}
D
Na^{+}
Verified step by step guidance1
Step 1: Understand the term 'isoelectronic.' Isoelectronic species have the same number of electrons, regardless of their element or charge.
Step 2: Determine the number of electrons in the oxide anion $O^{2-}$. Oxygen has an atomic number of 8, so neutral oxygen has 8 electrons. The $2-$ charge means it has gained 2 extra electrons, totaling $8 + 2 = 10$ electrons.
Step 3: Calculate the number of electrons for each ion given in the options:
- $N^{3-}$: Nitrogen has 7 electrons, plus 3 extra electrons from the charge, total $7 + 3 = 10$ electrons.
- $F^{-}$: Fluorine has 9 electrons, plus 1 extra electron from the charge, total $9 + 1 = 10$ electrons.
- $Cl^{-}$: Chlorine has 17 electrons, plus 1 extra electron, total $17 + 1 = 18$ electrons.
- $Na^{+}$: Sodium has 11 electrons, minus 1 electron due to positive charge, total $11 - 1 = 10$ electrons.
Step 4: Compare the total electrons of each ion to the oxide anion's 10 electrons to identify which ions are isoelectronic with $O^{2-}$.
Step 5: Conclude which ion(s) share the same electron count as $O^{2-}$, confirming the correct answer.
Related Videos
Related Practice
