Textbook Question
Show the dipole arrow for each of the following bonds:
a. Si―Cl
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4. Molecular Compounds
Dipole Moment (Simplified)
Multiple Choice
Arrange the following elements in order of decreasing electronegativity: P, Na, N, Al
A
P > Na > N > Al
B
N > P > Na > Al
C
Na > Al > P > N
D
N > P > Al > Na
E
P > N > Na > Al
Verified step by step guidance1
Understand the concept of electronegativity: Electronegativity is a measure of an atom's ability to attract and hold onto electrons. It generally increases across a period from left to right and decreases down a group in the periodic table.
Identify the position of each element in the periodic table: Phosphorus (P), Sodium (Na), Nitrogen (N), and Aluminum (Al) are located in different groups and periods. Nitrogen is in Group 15, Period 2; Phosphorus is in Group 15, Period 3; Sodium is in Group 1, Period 3; and Aluminum is in Group 13, Period 3.
Compare electronegativity values: Nitrogen, being in the second period and further to the right, has a higher electronegativity than Phosphorus. Sodium, being in Group 1, has a lower electronegativity compared to Aluminum, which is in Group 13.
Arrange the elements based on their electronegativity values: Start with the element with the highest electronegativity and proceed to the lowest. Nitrogen has the highest electronegativity, followed by Phosphorus, then Aluminum, and finally Sodium.
Select the correct option: Based on the arrangement of electronegativity values, the correct order is N > P > Al > Na.
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