Table of Contents
- 1 Why acidic character increases down the group 15?
- 2 Which group 15 oxide is most acidic?
- 3 Why are Tritoxides more acidic than Pentoxides?
- 4 Which is more acidic e2o3 or e2o5 & Why?
- 5 Which oxide is the most acidic?
- 6 Why is P2O5 more acidic than p2o3?
- 7 Why E2O3 is less acidic than E2O5?
- 8 Which has higher oxidation state E2O3 or E2O5?
- 9 Why do group 15 elements have +3 and +5 oxidation states?
- 10 How does the chemical character of oxides change down the group?
Why acidic character increases down the group 15?
This occurs due to many reasons. Namely, increase in the oxidation state. The more the oxidation state of an element more is its acidic property. In this case mentioned in the question, the acidic character of hydrides increases down the group.
Which group 15 oxide is most acidic?
And we know that all of these elements mentioned in the question belong to the same group, in the order phosphorus, arsenic, antimony and bismuth, down the group. So \[{{P}_{2}}{{O}_{5}}\] is the most acidic oxide, among all the given options. Hence the correct option is A.
Why does the acidic character of oxides decrease down the group 15?
As we know that electronegativity is the property of the element to attract electron pairs. Hence, the acidic character of the oxides “decreases down the group” because the electronegativity decreases down the group.
Why are Tritoxides more acidic than Pentoxides?
N2O5 is more acidic because the oxidation state of nitrogen (+5) is more than in N2O3(+3). Greater the oxidation state of the central atom, more is the acidic strength of the oxide.
Which is more acidic e2o3 or e2o5 & Why?
E2O5 is more acidic than E2O3 because higher is the oxidation state of central atom, the more it attracts electrons leading to more acidic nature.
Why does an acidic character increase down the group?
Going down a group the acid strength increases because the bond strength decreases as a function of increasing size of the nonmetal, and this has a larger effect than the electronegativity. Remember, the weaker the bond, the strong the acid strength.
Which oxide is the most acidic?
Therefore Cl2O7 is the most acidic oxide.
Why is P2O5 more acidic than p2o3?
Explanation: Higher the oxidation state of central atom, more is the acidic strength of that compound. thus P₂O₅ has higher oxidation state than P₂O₃, so P₂0₅ is more acidic than P₂O₃.
Does acidity increase or decrease as you go down the periodic table?
Acidity INCREASES as you go from left to right across the periodic table and DECREASES as you go down a group/column. The opposite is true for Basicity: INCREASES as you go up a group/column and DECREASES as you go from right to left across the periodic table.
Why E2O3 is less acidic than E2O5?
As we move down the group, the atomic size increases, electronegativity decreases and metallic character increases. All these elements form two types of oxides: E2O3 and E2O5. The oxide in the higher oxidation state of the element is more acidic than that of lower oxidation state.
Which has higher oxidation state E2O3 or E2O5?
E2O5 has greater oxidation state than E2O3. The oxidation states of the compounds can be calculated as: In both the cases, let us assume the oxidation state of E be x.
Which oxide is more acidic than the other?
The oxide in the higher oxidation state of the elements is more acidic than that of lower oxidation state. Oxides of nitrogen and phosphorus are acidic. Oxides of As and Sb are amphoteric and Bismuth are basic.
Why do group 15 elements have +3 and +5 oxidation states?
This is because of the expansion in nuclear size and metallic character. Group 15 elements additionally indicate positive oxidation states of +3 and +5 by developing covalent bonds. Because of the inert pair effect, the +5 oxidation state stability diminishes down the group, while that of +3 oxidation state increments.
How does the chemical character of oxides change down the group?
Acidic character of oxides of this group decreases and basicity increases down the group. On moving down the group, the atomic size increases, electronegativity decreases and metallic character increases. All these elements form two types of oxides: E 2 O 3 and E 2 O 5.
What are the chemical properties of Group 15 elements?
The s orbital is completely filled and p orbital is half-filled which makes them stable in nature. The chemical properties of these elements are determined by the oxidation states exhibited by them. The elements of group 15 generally exhibit -3, +3 and +5 oxidation states.