Are group 16 hydrides polar?
[2 marks] Some physical properties of molecular substances result from the different types of forces between their molecules. Explain why the hydrides of group 16 elements (H2O, H2S, H2Se and H2Te) are polar molecules. These hydrides all have a bent shape due to the two lone pair of electrons on the central atom.
What are the hydrides of group 16?
The Group 16 hydrides are: O: water, H2O; hydrogen peroxide, H2O2; trioxidane H2O. S: hydrogen sulfide, H2S; hydrogen disulfide, H2S. Se: hydrogen selenide, H2Se.
Why do hydrides of group 16 increase down the group?
Acidic nature: Due to the decreasing bond dissociation enthalpy, acidic character of group 16 elements increases down the group. H2O < H2S < H2Se < H2Te Reducing character: The reducing character also decreases down the group due to the decreasing bond dissociation enthalpy.
Which hydrides of group 16 does not show reducing property?
All hydrides of group 16 elements, except H2O, are reducing agent. The reducing power of these hydrides increase in going from H2S to H2Te, which may be due to increase in the size of the atom and hence decrease in the M-H bond energy.
Why is group 16 polar?
The difference in the electronegativities of Group 16 elements and hydrogen results in a polar covalent bond, that is, compared to the hydrogen atoms the Group 16 atom generally has a greater attraction for the shared electrons so the electrons of the shared electron pair spend more time around the nucleus of the Group …
What is the general electronic configuration of group 16 elements?
Group 16 elements have 6 electrons in their valence shell and their general electronic configuration is ns2np4.
What are the properties of group 16 elements?
Preparation and General Properties of the Group 16 Elements
| Property | Oxygen | Sulfur |
|---|---|---|
| atomic mass (amu) | 16.00 | 32.07 |
| valence electron configuration* | 2s 22p 4 | 3s 23p 4 |
| melting point/boiling point (°C) | −219/−183 | 115/445 |
| density (g/cm 3) at 25°C | 1.31 | 2.07 |
What do group 16 elements have in common?
The oxygen family consists of the elements that make up group 16 on the periodic table: oxygen, sulfur, selenium, tellurium, and polonium. These elements all have six electrons in their outermost energy level, accounting for some common chemical properties among them.
Which of the following atomic numbers belong to group 16 elements?
Group 16 Elements Of Modern Periodic Table
| Period | Element | Atomic Number |
|---|---|---|
| 2 | Oxygen | 8 |
| 3 | Sulphur | 16 |
| 4 | Selenium | 34 |
| 5 | Tellurium | 52 |
Are all group 16 oxides acidic?
Acid-base properties:The acidic character of oxides of group 16 elements decreases as we move down the group. Reducing-oxidising properties: Since +6 oxidation state of sulphur is more stable than +4 oxidation state, therefore, SO2 acts as a reducing agent.
Which of the following has lowest reducing character in group 16?
– All the given options are group 16 hydrides. – On going down the group, the reducing character of group 16 hydrides increases. – This implies that H2O is the least reducing among the following. – It only acts as a reducing agent in the presence of a very strong oxidising agent.
Are group 16 elements metals?
The chalcogens are the first group in the p block to have no stable metallic elements. All isotopes of polonium (Po), the only metal in group 16, are radioactive, and only one element in the group, tellurium (Te), can even be described as a semimetal.