Table of Contents
- 1 What properties does group 15 have?
- 2 What does Group 15 represent?
- 3 What is Group 15 on the periodic table called?
- 4 Why does boiling point increase in Group 15?
- 5 Why boiling point decreases down the group 15?
- 6 Does boiling point increases down the group?
- 7 What is the electronic setup of Group 15 elements?
- 8 Why does the stability of Group 15 elements decrease?
What properties does group 15 have?
Periodic Trends in Group 15 Elements
| Property | Nitrogen | Phosphorus |
|---|---|---|
| Melting point Boiling point (°C) | – 210 -196 | 44.15 281 |
| Density (g/cm3) at 25°C | 1.15(g/L) | 1.8 |
| Atomic radius (pm) | 56 | 98 |
| First Ionization energy (kJ/mol) | 1402 | 1012 |
What does Group 15 represent?
The nitrogen family includes the following compounds: nitrogen (N), phosphorus (P), arsenic (As), antimony (Sb), and bismuth (Bi).
Which property of Group 15 elements increase on moving down the group?
On moving down the group, the atomic radii increase due to increase in number of shells because of addition of a new principal shell in each succeeding element.
What is Group 15 on the periodic table called?
Summary. Members of group 15 of the periodic table (15th vertical column) are summarised as group 15 elements (or the nitrogen group) consisting of nitrogen (N), phosphorus (P), arsenic (As), antimony (Sb) and bismuth (Bi).
Why does boiling point increase in Group 15?
The elements included in group number 15 are nitrogen, phosphorus, arsenic, antimony and bismuth. While moving down the group the atomic size of the element increases because an extra shell is added as the number of periods increases. So the boiling point of Sb is greater than Bi.
What is the charge of Group 16?
Elements in group 16 have a charge of -2, while all the elements of group 17 are halogens with a charge of -1 each.
Why boiling point decreases down the group 15?
Atomic radii increase in size down the group. Electron affinity (the ability of the atom to accept an electron) decreases down the group. Boiling point (amount of energy required to break bonds to change a liquid phase substance to a gas) increases down the group. Metallic character increases down the group.
Does boiling point increases down the group?
Melting and Boiling Points (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.
What are the chemical properties of Group 15 elements?
All the elements of group 15 form gaseous trihydrides of the formula EH3, (where E=N, P, As, Sb or Bi) such as: The lighter elements also form hydrides of the formula M2H4 such as N2H4 (hydrazine), P2H4 (diphosphine) and As2H4 (diarsine).
What is the electronic setup of Group 15 elements?
In the iotas of p-block elements, the separating electron enters the valence p subshell. In this manner, in these elements, the np subshell is filled step by step. The general valence shell electronic setup of group fifteen elements is ns 2, np 1-6. The electronic design of helium is 1s 2. It has no orbitals.
Why does the stability of Group 15 elements decrease?
The stability of the hydrides of group 15 elements decreases in the order: NH3 > PH3 > AsH3 > SbH3 > BiH3. Explanation: On going down the group, the size of the central atom increases and therefore, its tendency to form stable covalent bond with small hydrogen atom decreases.
What is the reducing character of Group 15 elements?
(iii) Reducing character: The reducing character of the hydrides of group 15 elements increases from NH3 to BiH3. Thus, increasing order of reducing character is as follows : NH3 < PH3 < AsH3 < SbH3 < BiH3 Explanation: The reducing character depends upon the stability of the hydride.