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The properties of the elements such as a...

The properties of the elements such as atomic or ionic radii ionisation enthalpy, electron gain enthalpy and electronegativity are directly or indirectly related to their electronic configuration and are called periodic properties. A part the periodic table is given below :
`{:(C, N, O, F),(, P, S, Cl),(,,Se, Br), (,,,I):}`
Which of the following has the largest size ?

A

N

B

O

C

S

D

P

Text Solution

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The correct Answer is:
To determine which element has the largest size among the given options (Nitrogen, Phosphorus, Oxygen, and Sulfur), we need to analyze their positions in the periodic table and understand the trends in atomic size. ### Step-by-Step Solution: 1. **Identify the Elements and Their Groups:** - The elements given are Nitrogen (N), Phosphorus (P), Oxygen (O), and Sulfur (S). - Nitrogen and Phosphorus belong to Group 15 (Pnictogens). - Oxygen and Sulfur belong to Group 16 (Chalcogens). 2. **Understand the Trend in Atomic Size:** - Atomic size generally increases as you move down a group in the periodic table because additional electron shells are added. - Conversely, atomic size decreases as you move from left to right across a period due to increasing nuclear charge, which pulls the electrons closer to the nucleus. 3. **Compare the Elements:** - **Nitrogen (N)** is in Period 2, while **Phosphorus (P)** is in Period 3. Therefore, Phosphorus will be larger than Nitrogen due to having an additional electron shell. - **Oxygen (O)** is also in Period 2, while **Sulfur (S)** is in Period 3. Thus, Sulfur will be larger than Oxygen for the same reason. - Now, we need to compare Nitrogen and Oxygen (both in Period 2) with Phosphorus and Sulfur (both in Period 3). 4. **Determine the Largest Size:** - Between Nitrogen and Phosphorus, Phosphorus is larger. - Between Oxygen and Sulfur, Sulfur is larger. - Therefore, comparing the largest from each group, Phosphorus (P) is larger than Sulfur (S). 5. **Conclusion:** - The element with the largest atomic size among the given options is **Phosphorus (P)**. ### Final Answer: **Phosphorus (P) has the largest size among the given elements.**
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The properties of the elements such as atomic or ionic radii ionisation enthalpy, electron gain enthalpy and electronegativity are directly or indirectly related to their electronic configuration and are called periodic properties. A part the periodic table is given below : {:(C, N, O, F),(, P, S, Cl),(,,Se, Br), (,,,I):} Bromine belongs to period

The properties of the elements such as atomic or ionic radii ionisation enthalpy, electron gain enthalpy and electronegativity are directly or indirectly related to their electronic configuration and are called periodic properties. A part the periodic table is given below : {:(C, N, O, F),(, P, S, Cl),(,,Se, Br), (,,,I):} The highest ionisation enthalpy is of

The properties of the elements such as atomic or ionic radii ionisation enthalpy, electron gain enthalpy and electronegativity are directly or indirectly related to their electronic configuration and are called periodic properties. A part the periodic table is given below : {:(C, N, O, F),(, P, S, Cl),(,,Se, Br), (,,,I):} The highest negative electron gain enthalpy is of

Periodic Trend |Atomic Radii |Ionic Radii|Ionisation Enthalpy |Electron Gain Enthalpy|Electronegativity |OMR|Summary

The properties of the elements (atomic/ionic radii, electron gain enthalpy, ionization enthalpy, electronegativity, valence, oxidising/reducing power, acid/base character, etc.) which are directly or indirectly related to their electronic configirations are called periodic properties. These properties show a regular gradation on moving from left to right in a period or form top to bottom in a group. Down a group, the atomic/ionic radii, metallic character and reducing character increase while ionization enthalpy and electronegativity decrease. Along a period from left to right, atomic/ionic and metallic character decrease while ionization enthaloy, electronegativity, non-metallic character and oxiding power increase. However, electron gain enthalpy becomes less negative down a group butmore negative along a period. In contrast, inert gases have positive electron gain enthalpies which do not show may regular trend. The outermost electronic configuration of the most electronegative elements is:

The properties of the elements (atomic/ionic radii, electron gain enthalpy, ionization enthalpy, electronegativity, valence, oxidising/reducing power, acid/base character, etc.) which are directly or indirectly related to their electronic configirations are called periodic properties. These properties show a regular gradation on moving from left to right in a period or form top to bottom in a group. Down a group, the atomic/ionic radii, metallic character and reducing character increase while ionization enthalpy and electronegativity decrease. Along a period from left to right, atomic/ionic and metallic character decrease while ionization enthaloy, electronegativity, non-metallic character and oxiding power increase. However, electron gain enthalpy becomes less negative down a group butmore negative along a period. In contrast, inert gases have positive electron gain enthalpies which do not show may regular trend. Which of the following isoelectronic ions has the lowest first ionization enthalpy?

The properties of the elements (atomic/ionic radii, electron gain enthalpy, ionization enthalpy, electronegativity, valence, oxidising/reducing power, acid/base character, etc.) which are directly or indirectly related to their electronic configirations are called periodic properties. These properties show a regular gradation on moving from left to right in a period or form top to bottom in a group. Down a group, the atomic/ionic radii, metallic character and reducing character increase while ionization enthalpy and electronegativity decrease. Along a period from left to right, atomic/ionic and metallic character decrease while ionization enthaloy, electronegativity, non-metallic character and oxiding power increase. However, electron gain enthalpy becomes less negative down a group butmore negative along a period. In contrast, inert gases have positive electron gain enthalpies which do not show may regular trend. Tick the correct order of second ionization enthalpy in the following:

The properties of the elements (atomic/ionic radii, electron gain enthalpy, ionization enthalpy, electronegativity, valence, oxidising/reducing power, acid/base character, etc.) which are directly or indirectly related to their electronic configirations are called periodic properties. These properties show a regular gradation on moving from left to right in a period or form top to bottom in a group. Down a group, the atomic/ionic radii, metallic character and reducing character increase while ionization enthalpy and electronegativity decrease. Along a period from left to right, atomic/ionic and metallic character decrease while ionization enthaloy, electronegativity, non-metallic character and oxiding power increase. However, electron gain enthalpy becomes less negative down a group butmore negative along a period. In contrast, inert gases have positive electron gain enthalpies which do not show may regular trend. Amomgst the following elements (whose electronic configurations are given below) the one having the highest ionization enthalpy is :

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P Block Elements|Periodic Table|Electronic Configuration|Atomic Radii|Ionisation Enthalpy|Electron Gain Enthalpy|Electronegativity|Mass | Density | Boiling & Melting Point|OMR