Group 5A (15)
Express your answer as an integer.
The Correct Answer and Explanation is:
The elements in Group 5A of the periodic table are nitrogen (N), phosphorus (P), arsenic (As), antimony (Sb), and bismuth (Bi). These elements are part of the nitrogen group and have five valence electrons in their outermost electron shell. To address your question properly, it is essential to understand their position in the periodic table and the implications of their electron configurations.
Understanding Group 5A:
- Nitrogen (N) has an atomic number of 7. Its electron configuration is 1s² 2s² 2p³, meaning it has five valence electrons in its second shell.
- Phosphorus (P) has an atomic number of 15. Its electron configuration is 1s² 2s² 2p⁶ 3s² 3p³, meaning it has five valence electrons in its third shell.
- Arsenic (As) has an atomic number of 33. Its electron configuration is 1s² 2s² 2p⁶ 3s² 3p⁶ 4s² 3d¹⁰ 4p³, with five valence electrons in its fourth shell.
- Antimony (Sb) has an atomic number of 51. Its electron configuration is 1s² 2s² 2p⁶ 3s² 3p⁶ 3d¹⁰ 4s² 4p⁶ 4d¹⁰ 5s² 4d¹⁰ 5p³, showing five valence electrons in its fifth shell.
- Bismuth (Bi) has an atomic number of 83. Its electron configuration is 1s² 2s² 2p⁶ 3s² 3p⁶ 3d¹⁰ 4s² 4p⁶ 4d¹⁰ 5s² 5p⁶ 4d¹⁰ 5s² 6p³, with five valence electrons in its sixth shell.
Why the Number of Electrons Matters:
The number of valence electrons dictates how an element behaves in chemical reactions. In the case of Group 5A elements, they typically form compounds by gaining three electrons (to complete their octet) or sharing electrons to form covalent bonds.
Conclusion:
These five elements in Group 5A all have five valence electrons, which is why they are grouped together. If your question is about finding an integer related to this group, a common reference would be their oxidation states. These elements often exhibit an oxidation state of -3 when gaining electrons or +5 when forming covalent bonds.
Thus, Group 5A elements are significant for their electron configurations and common oxidation states, influencing both their chemical and physical properties.