NEET Exam > NEET Videos > Chemistry Class 12 > Trends in Group-15 Elements - 1
Trends in Group-15 Elements - 1 Video Lecture | Chemistry Class 12 - NEET
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FAQs on Trends in Group-15 Elements - 1 Video Lecture - Chemistry Class 12 - NEET
| 1. What are the group-15 elements? |  |
Ans. The group-15 elements, also known as the nitrogen group, are a group of elements in the periodic table that includes nitrogen (N), phosphorus (P), arsenic (As), antimony (Sb), and bismuth (Bi). These elements share similar chemical properties due to their same outer electron configuration.
| 2. What are the trends observed in the group-15 elements? | |
Ans. The group-15 elements exhibit certain trends as we move down the group. Some of these trends include an increase in atomic radius, an increase in metallic character, a decrease in electronegativity, and a decrease in ionization energy. Additionally, the oxidation states of these elements become more negative as we move down the group.
| 3. How does the atomic radius change in group-15 elements? | |
Ans. The atomic radius generally increases as we move down the group-15 elements. This is because each successive element has an additional electron shell, which increases the distance between the nucleus and the outermost electrons. As a result, the atomic radius increases, leading to larger atomic sizes.
| 4. What is the trend in the electronegativity of group-15 elements? | |
Ans. The electronegativity of group-15 elements generally decreases as we move down the group. This is due to the increase in atomic size and the shielding effect of inner electron shells. As the atomic size increases, the attraction between the nucleus and the outermost electrons decreases, resulting in lower electronegativity values.
| 5. How does the ionization energy change in group-15 elements? | |
Ans. The ionization energy, which is the energy required to remove an electron from an atom, generally decreases as we move down the group-15 elements. This is because the outermost electron is farther from the nucleus due to the increasing atomic size, making it easier to remove. Therefore, the ionization energy decreases as we move down the group.
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Nov 24, 2024 Last updated |
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