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In the Periodic Table below, shade all the elements for which the neutral atom has a half-filled p subshell. H Li Be Na Mg K Ca Sc Rb Sr Y Cs Ba La Fr Ra Ac He B CNOF Ne Al Si P S Cl Ar Ti V Cr Mn Fe Co Ni Cu Zn Ga Ge As Se Br Kr Zr Nb Mo Tc Ru Rh Pd Ag Cd In Sn Sb Te I Xe Hf Ta W Re Os Ir Pt Au Hg Tl Pb Bi Po At Rn Rf Db Sg Bh Hs Mt Ds Rg Cn X

In the Periodic Table below, shade all the elements for which the neutral atom has a half-filled p subshell. H Li Be Na Mg K Ca Sc Rb Sr Y Cs Ba La Fr Ra Ac He B CNOF Ne Al Si P S Cl Ar Ti V Cr Mn Fe Co Ni Cu Zn Ga Ge As Se Br Kr Zr Nb Mo Tc Ru Rh Pd Ag Cd In Sn Sb Te I Xe Hf Ta W Re Os Ir Pt Au Hg Tl Pb Bi Po At Rn Rf Db Sg Bh Hs Mt Ds Rg Cn X

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**Title: Understanding Half-Filled p Subshells in the Periodic Table** **Text:** In the Periodic Table below, you are tasked with identifying all the elements for which the neutral atom has a half-filled p subshell. To complete this task, you should shade these elements on your own version of the periodic table. **Explanation of the Diagram:** The image showcases a simplified periodic table, highlighting the arrangement of elements with a focus on the p-block. The table is divided into several sections: - **s-Block:** The left segment includes elements such as Hydrogen (H), Lithium (Li), Beryllium (Be), Sodium (Na), Magnesium (Mg), etc. - **p-Block:** The right segment includes elements such as Boron (B), Carbon (C), Nitrogen (N), Oxygen (O), Fluorine (F), Neon (Ne), and continues downwards with other elements like Aluminum (Al), Silicon (Si), and so forth. - **d-Block and f-Block:** Located in the center and at the bottom respectively in a more complex version of the table but not the focus here. **Focus on Elements with Half-Filled p Subshells:** A half-filled p subshell occurs when there are three electrons in a p orbital. For example, the element Nitrogen (N), which has an atomic number of 7, has the electron configuration 1s² 2s² 2p³, showcasing a half-filled p subshell. To find other elements with a half-filled p subshell, you will need to look for those in similar electronic configurations in subsequent periods. This includes: - **Period 2:** Nitrogen (N) - **Period 3:** Phosphorus (P) - **Period 4:** Arsenic (As) - **Period 5:** Antimony (Sb) - **Period 6:** Bismuth (Bi) By understanding and shading these elements, students can gain insight into electron configurations and the principles behind the periodic table's structure.
Transcribed Image Text:**Title: Understanding Half-Filled p Subshells in the Periodic Table** **Text:** In the Periodic Table below, you are tasked with identifying all the elements for which the neutral atom has a half-filled p subshell. To complete this task, you should shade these elements on your own version of the periodic table. **Explanation of the Diagram:** The image showcases a simplified periodic table, highlighting the arrangement of elements with a focus on the p-block. The table is divided into several sections: - **s-Block:** The left segment includes elements such as Hydrogen (H), Lithium (Li), Beryllium (Be), Sodium (Na), Magnesium (Mg), etc. - **p-Block:** The right segment includes elements such as Boron (B), Carbon (C), Nitrogen (N), Oxygen (O), Fluorine (F), Neon (Ne), and continues downwards with other elements like Aluminum (Al), Silicon (Si), and so forth. - **d-Block and f-Block:** Located in the center and at the bottom respectively in a more complex version of the table but not the focus here. **Focus on Elements with Half-Filled p Subshells:** A half-filled p subshell occurs when there are three electrons in a p orbital. For example, the element Nitrogen (N), which has an atomic number of 7, has the electron configuration 1s² 2s² 2p³, showcasing a half-filled p subshell. To find other elements with a half-filled p subshell, you will need to look for those in similar electronic configurations in subsequent periods. This includes: - **Period 2:** Nitrogen (N) - **Period 3:** Phosphorus (P) - **Period 4:** Arsenic (As) - **Period 5:** Antimony (Sb) - **Period 6:** Bismuth (Bi) By understanding and shading these elements, students can gain insight into electron configurations and the principles behind the periodic table's structure.
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