What are the chemical properties of Group 15?
What are the chemical properties of Group 15?
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 factors influence the properties of p-block elements?
The properties of p-block elements like that of others are greatly influenced by atomic sizes, ionisation enthalpy, electron gain enthalpy and electronegativity.
What are the chemical properties of Group 16 elements?
Oxygen shows anomalous behaviour. This is due to its small size, high electronegativity, high ionisation enthalpy and absence of d-orbitals in its valence shell. Due to the absence of d-orbitals in oxygen, its covalency is limited to four.
What are the properties of Group 17 elements?
Physical properties of Group 17 elements
| Element | Fluorine | Chlorine |
|---|---|---|
| Atomic radius (nm) | 0.071 | 0.099 |
| Density (g cm-1) | 0.0017 | 0.0032 |
| Melting point (°C) | -220 | -101 |
| Boiling point (°C) | -188 | -35 |
Which of the following properties of p-block elements increase as we move from left to right?
The first ionization enthalpy of the p-block elements generally increases on moving from left to right along a period.
Why p-block elements have high ionisation enthalpy?
It is because in case of group 15 elements, the electron is to be removed from the half-filled p-orbitals. In general, In P-Block elements, the first ionization enthalpy decreases in a regular way on a descending group. It is because on a descending group, the atomic size increases.
Why some elements are called P block elements?
The s-block and p-block elements are so called because their valence electrons are in an s orbital or p orbital respectively. They are also called Typical Elements to distinguish them from the transition and inner transition series.
What are the atomic and physical properties of group 16 elements?
Metallic character increases down the group, with tellurium classified as a metalloid and polonium as a metal. Melting point, boiling point, density, atomic radius, and ionic radius all increase down the group. Ionization energy decreases down the group.
What are the properties of Group 18?
The members of the group have eight electrons in their outermost orbit (except helium which has two electrons). Thus, they have a stable configuration. Group 18 elements are gases and chemically unreactive, which means they don’t form many compounds. Thus, the elements are known as inert gases.
What are the physical and chemical properties of halogens?
In general, halogens have low melting and boiling points, high electronegativities, and are sparingly soluble in water. Their properties show trends as you move down the group. For example, atomic radius and melting and boiling points increase down the group whilst reactivity and electronegativity decrease.
Why metallic character increases down the group in p-block?
Metallic character increases as you move down an element group in the periodic table. This is because electrons become easier to lose as the atomic radius increases, where there is less attraction between the nucleus and the valence electrons because of the increased distance between them.
Why p-block elements are Electronegative?
The tendency of an atom in a molecule to attract the shared pair of electrons towards itself is known as electronegativity. It is a dimensionless property because it is only a tendency. It basically indicates the net result of the tendencies of atoms in different elements to attract the bond-forming electron pairs.
