Question

Read the given passage and answer the questions 1 to 4 that follows:-
The elements of Group 16 (0,S,Se,Te,Po), commonly known as 'chalcogens' exhibit a number of oxidation
states. The stability of -2 oxidation state decreases down the group. Other elements of the group exhibit +2, +4,
+ 6 oxidation states but + 4 and + 6 are more common. They react with hydrogen to form hydrides of the type
HE and with halogens to form halides of the formula EX2, EX4,EX.
1. Why does the stability of + 6 oxidation state decreases down the group?
2. Arrange H2O, H2S, H Se, H2Te in order of their increasing acidic strength.
3. Why is H20 a liquid and H2S a gas?
4. Draw the structure of SF4.​

Answer 1

Answer:

Explanation:

1. Stability of the chalcogens, i.e., the oxygen family decreases due to inert pair effect, (the tendency of the electrons in the outermost atomic s orbital to remain un-ionized or unshared in compounds of post-transition metals or p- block elements)

2. H2Te > H2Se > H2S > H2O (since the size of tellurium is greater, there will be electron- electron repulsion, causing the faster releasing of H+ ions, and so is the condition for all other elements)

3. H2O is a liquid and H2S is a gas because O is more electronegative than S, thus, O forms hydrogen bonds, thus, making H2O a liquid

4. SF4 will be trigonal bipyramidal with a lone pair..... The attachment might help you....

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