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The pronounced change from non-metallic ...

The pronounced change from non-metallic behaviour and also increase in the basicity of oxides from nitrogen to bismuth in group `15` is principally due to incresing size of the atoms. The ionisation potential of nitrogen is very high on account of its small size. However, ionisation potential decreases regularly on descending the group.
The most unstable hydride is.

A

`NH_3`

B

`SbH_3`

C

`BiH_3`

D

`PH_3`

Text Solution

Verified by Experts

The correct Answer is:
C
Due to weakest `Bi-H` bond strength, `BiH_3` is least stable.
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The pronounced change from non-metallic behaviour and also increase in the basicity of oxides from nitrogen to bismuth in group 15 is principally due to incresing size of the atoms. The ionisation potential of nitrogen is very high on account of its small size. However, ionisation potential decreases regularly on descending the group. Among the trihalides of nitrogen, which one is least basic ?

The pronounced change from non-metallic behaviour and also increase in the basicity of oxides from nitrogen to bismuth in group 15 is principally due to incresing size of the atoms. The ionisation potential of nitrogen is very high on account of its small size. However, ionisation potential decreases regularly on descending the group. In all the group 15 elements, the number of unpaired electrons in the valence shell is.

The pronounced change from non-metallic behaviour and also increase in the basicity of oxides from nitrogen to bismuth in group 15 is principally due to incresing size of the atoms. The ionisation potential of nitrogen is very high on account of its small size. However, ionisation potential decreases regularly on descending the group. Which trihalide is most ionic among the following ?

The pronounced change from non-metallic behaviour and also increase in the basicity of oxides from nitrogen to bismuth in group 15 is principally due to incresing size of the atoms. The ionisation potential of nitrogen is very high on account of its small size. However, ionisation potential decreases regularly on descending the group. Which one of the following is a strongest base ?

The pronounced change from non-metallic behaviour and also increase in the basicity of oxides from nitrogen to bismuth in group 15 is principally due to incresing size of the atoms. The ionisation potential of nitrogen is very high on account of its small size. However, ionisation potential decreases regularly on descending the group. Which one of the following fluorides does not exist ?

The pronounced change from non-metallic behaviour and also increase in the basicity of oxides from nitrogen to bismuth in group 15 is principally due to incresing size of the atoms. The ionisation potential of nitrogen is very high on account of its small size. However, ionisation potential decreases regularly on descending the group. Which one of the following fluorides does not exist ?

It is not possible to measure the atomic radius precisely since the electron cloud surrounding the atom does not have a sharp boundary. One practical approach to estimate the size of an atom of a non-metallic element is to measure the distance between two atoms when they are bound together by a single bond in a covalent molecule and then dividing by two. For metals we define the term "metallic radius" which is taken as half the inter nuclear distance separating the metal cores in the metallic crystal. Then van der waal's radius represents the over all size of the atoms which includes its valence shell in a non bonded situation. It is the half of the distance between two similar atoms in separate molecules in a solid. The atomic radius decreases across a period and increases down the group. Same trends are observed in case of ionic radius. Ionic radius of the species having same number of electrons depends on the number of protons in their nuclei. Sometimes, atomic and ionic radii give unexpected trends due to poor shielding of nuclear charge by d -and f- orbital electrons. Now answer the following three questions: K^(+), CI^(-), Ca^(2+), S^(2-) ions are isoelectronic. The decreasing order of their size is:

It is not possible to measure the atomic radius prectsely since the electron cloub surrouding the atom does not have a sharp boundary. One practial approach to estimate the size of an atom of a non-metallic element is to measure the distance between two atoms when they are bound togther by a signle bond in a covalent molecule and then dividing by two. For metals we define the term "matellic radius" which is taken as half the internuclear distance separating the metal cores in the metallic crystal. Then van der waal's radius represents the over all size of the atoms which includes its valence shell in a non bonded situation. It is the half of the distance between two similar atoms in separate molecules in a solid. The atomis radius decreases across a period and increases down the group. Same trends are observed in case of ionic radius. Ionic radius of the species having same number of electrons depends on the number of protons in their nuclei. Sometimes, atomic and ionic radii give unexpected trends due to poor shielding of nuclear charge by d -and f- orbital electrons. Now answer the following three questions: Select the INCORRECT option regarding atomic//ionic sizes:

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Both alkali metals and alkaline earth metals are s- block elements. They resemble each other in many respects but still there are certain dissimilarities in their properties due to different number of electrons in the valence shell, different atomic radii, ionisation enthalpy, electronegativity, etc. Like lithium, Be also differs from rest of the alkaline earth metals on account of its small atomic size and high electronetativity. Be^(2+) ion is very small and exerts a high polarising effect on any anion associated with it. The correct sequence of increasing covalent character is

CENGAGE CHEMISTRY ENGLISH-P-BLOCK GROUP 15 ELEMENTS - THE NITROGEN FAMILY-Exercises (Linked Comprehension)
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  12. Which of the following oxides is most acidic ?

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