Why melting point increases down the group 16?
Why melting point increases down the group 16?
Why do the melting and boiling points of Group 16 elements increase down the group? The melting and boiling point increase down the group due to the increase size of the element, which increases the Van der Waal’s forces of attraction and hence the melting and boiling point increases down the group.
Why do the melting and boiling points of group 16 hydrides increase?
Group 16 hydride molecules have a bent shape. Weaker intermolecular forces act between other Group 16 hydride molecules. The melting point and boiling point of water (H2O) molecules is unexpectedly high due to the stronger hydrogen bonds acting between water molecules.
What is the melting point of group 16 elements?
Preparation and General Properties of the Group 16 Elements
| Property | Oxygen | Tellurium |
|---|---|---|
| *The configuration shown does not include filled d and f subshells. | ||
| melting point/boiling point (°C) | −219/−183 | 450/988 |
| normal oxidation state(s) | −2 | +6, +4, −2 |
| product of reaction with H2 | H2O | none |
Why melting point increases down the group?
The melting and boiling points increase down the group because of the van der Waals forces. The size of the molecules increases down the group. This increase in size means an increase in the strength of the van der Waals forces.
Which element of GR 16 has the highest melting point?
The element with highest m.p. and b.p. in Group 16 is
- A. Po.
- B. Te.
- C. Se.
- D. S.
- Answer. B.
- Melting point and boiling point of Te are more than Po. m.p. and b.p. increase down the group from O to Te.
Why melting point increases down the group 15?
Ionization energy (the amount of energy required to remove an electron from the atom in its gas phase) decreases down the group. Melting point (amount of energy required to break bonds to change a solid phase substance to a liquid phase substance) increases down the group.
Why does group 16 have higher boiling points than Group 17?
Oxygen as a 1st row element, is far more electronegative than sulfur and tellurium, and the O−H is far more polar as a result. The resultant intermolecular hydrogen bonding between adjacent molecules accounts for the exceptionally high boiling point of water, compared to the lower Group VI hydrides.
Which is most thermally stable in group 16?
Write the order of thermal stability of the hydrides of group 16 elements. Answer: The thermal stability of the hydrides of group 16 elements decreases down the group, i.e., H2O > H2S > H2Se > H2Te > H2Po.
Why is group 16 called Chalcogens?
-Group-16 elements are also called chalcogens. They are called so because most of the copper ores have copper in the form of oxides and sulphides. They also contain small amounts of selenium and tellurium. So, group-16 elements are named chalcogens.
Which of the following is correct order of melting point of 16 group?
Thus, melting point order is H2Te>H2Se>H2S.
What are the boiling points of Group 16 hydrides?
Now, consider the boiling points of Group 16 hydrides as shown in the table below: Boiling point of water is anomalously high! Gradual increase in boiling points down the rest of the group as the relative molecular mass of the molecules increases.
What are the intermolecular forces between group 16 hydrides?
The most significant intermolecular forceacting between water (H2O) molecules is the hydrogen bond. Weaker intermolecular forces act between other Group 16 hydride molecules. The melting point and boiling point of water (H2O) molecules is unexpectedly high due to the stronger hydrogen bonds acting between water molecules.
How are the group 16 elements related to water?
The group sixteen elements react with hydrogen to frame hydrides of the sort H2E, where E could be any element oxygen, sulfur, selenium, tellurium or polonium. Water is an odorless and colorless liquid but the hydrides of the various elements of this group are poisonous gases which are colorless with disagreeable smells.
How many valence electrons in a group 16 hydride?
Trends in Group 16 Hydrides Tutorial Key Concepts Group 16 elementsare: naturally occurring oxygen, sulfur, selenium, tellurium, polonium, and the man-made element livermorium. The atoms of Group 16 elements have 6 valence electrons. An atom of hydrogen has 1 valence electron.