For the following:
i) H3PO4 > H3AsO4 > H3SbO4
ii) H2Te > H2Se > H2S > H2O
iii) HCl > HBr > HI
iv) SbH3 > AsH3 > PH3 > NH3
The order of acidity is correct for which series?
1. ) all are correct
2. ) i and ii
3. )i, ii and iv
4. ) ii, iii
5. ii, iv
I know the ii and iv are right....but i dunno about number i ? :S
can someone help me and confirm my answers?
You are correct that ii and iv are correct. i is also correct.
To determine the correctness of the order of acidity in the given series, you need to understand the trends in acidity for the compounds mentioned. Here's an explanation of each series:
i) H3PO4 > H3AsO4 > H3SbO4: In this series, the acidity increases as we move from left to right. This is because the electronegativity of the central atom increases, leading to stronger polarization of the O-H bond and easier dissociation of the proton (H+). Therefore, H3PO4 is more acidic than H3AsO4, and H3AsO4 is more acidic than H3SbO4.
ii) H2Te > H2Se > H2S > H2O: In this series, the acidity decreases as we move from left to right. This is because the size of the central atom increases, leading to weaker polarization of the O-H bond and less efficient dissociation of the proton. Therefore, H2Te is the most acidic, followed by H2Se, then H2S, and finally H2O.
iii) HCl > HBr > HI: In this series, the acidity increases as we move from left to right. This is because the strength of the bond between the central atom and the hydrogen decreases as we move down the periodic table. Therefore, HCl is less acidic than HBr, and HBr is less acidic than HI.
iv) SbH3 > AsH3 > PH3 > NH3: In this series, the acidity decreases as we move from left to right. This is because the size of the central atom increases, leading to weaker polarization of the N-H bond and less efficient dissociation of the proton. Therefore, SbH3 is the most acidic, followed by AsH3, then PH3, and finally NH3.
Based on the above explanations, the correct order of acidity for the given series is:
- ii) H2Te > H2Se > H2S > H2O
- iv) SbH3 > AsH3 > PH3 > NH3
Therefore, the correct answer is option 5. ii, iv.
To determine the correctness of statement i) "H3PO4 > H3AsO4 > H3SbO4" in the order of acidity, we need to examine the acidic strengths of each compound.
In general, the acidity of oxyacids increases with an increase in the electronegativity of the central atom. Here, we have phosphorus (P), arsenic (As), and antimony (Sb) as the central atoms.
Comparing the electronegativity, phosphorus (P) has the lowest electronegativity, followed by arsenic (As), and then antimony (Sb).
Based on this, we can deduce that the order of acidity is as follows:
H3PO4 < H3AsO4 < H3SbO4
Therefore, statement i) "H3PO4 > H3AsO4 > H3SbO4" is not correct.
Hence, the correct answer is option 4) ii, iii, where only statement ii) (H2Te > H2Se > H2S > H2O) and iii) (HCl > HBr > HI) are correct.