Final AnswerThe givenelectron configurationsrepresent the following elements with the indicated number of unpaired electrons:1. Nitrogen (N) with 3 unpaired electrons (1s²2s²2p³).2. Neon (Ne) with 0 unpaired electrons (1s²2s²2p⁶).3. Sodium (Na) with 1 unpaired electron (1s²2s²2p⁴3s¹).4. Phosphorus (P) with 3 unpaired electrons ([Ar]4s²3d¹⁰4p³).5. Chromium (Cr) with 6 unpaired electrons ([Ar]4s¹3d⁵4p¹).ExplanationThe electron configurations provided describe thearrangementof electrons in the respective elements' electron shells. The number of unpaired electrons in an element's electron configuration is crucial for understanding its chemical behavior, especially its reactivity and ability to form bonds.1. Nitrogen (N) has an electron configuration of 1s²2s²2p³, indicating 3 unpaired electrons in itsoutermostshell. This makes nitrogen reactive, especially in forming covalent bonds.2. Neon (Ne) has a stable electron configuration of 1s²2s²2p⁶, with no unpaired electrons. It is chemically inert and doesn't readily form bonds.3. Sodium (Na) has one unpaired electron in its 3s orbital (1s²2s²2p⁶3s¹), which it easily loses to form a sodium ion (Na⁺) in chemical reactions.4. Phosphorus (P) has an electron configuration of [Ar]4s²3d¹⁰4p³, with 3 unpaired electrons in its 4p orbitals, contributing to its ability to form multiple bonds in various compounds.5. Chromium (Cr) has an electron configuration of [Ar]4s¹3d⁵4p¹, with 6 unpaired electrons. This arrangement accounts for its magnetic properties andcomplex bondingbehavior.Understanding unpaired electrons helps predict an element's reactivity and bonding patterns in chemical reactions.Learn more aboutFinal Answer:The given electron configurations represent the following elements with the indicated number of unpaired electrons:1. Nitrogen (N) with 3 unpaired electrons (1s²2s²2p³).2. Neon (Ne) with 0 unpaired electrons (1s²2s²2p⁶).3. Sodium (Na) with 1 unpaired electron (1s²2s²2p⁴3s¹).4. Phosphorus (P) with 3 unpaired electrons ([Ar]4s²3d¹⁰4p³).5. Chromium (Cr) with 6 unpaired electrons ([Ar]4s¹3d⁵4p¹).Explanation:The electron configurations provided describe the arrangement of electrons in the respective elements' electron shells. The number of unpaired electrons in an element's electron configuration is crucial for understanding its chemical behavior, especially its reactivity and ability to form bonds.1. Nitrogen (N) has an electron configuration of 1s²2s²2p³, indicating 3 unpaired electrons in its outermost shell. This makes nitrogen reactive, especially in forming covalent bonds.2. Neon (Ne) has a stable electron configuration of 1s²2s²2p⁶, with no unpaired electrons. It is chemically inert and doesn't readily form bonds.3. Sodium (Na) has one unpaired electron in its 3s orbital (1s²2s²2p⁶3s¹), which it easily loses to form a sodium ion (Na⁺) in chemical reactions.4. Phosphorus (P) has an electron configuration of [Ar]4s²3d¹⁰4p³, with 3 unpaired electrons in its 4p orbitals, contributing to its ability to form multiple bonds in various compounds.5. Chromium (Cr) has an electron configuration of [Ar]4s¹3d⁵4p¹, with 6 unpaired electrons. This arrangement accounts for its magnetic properties and complex bonding behavior.Understanding unpaired electrons helps predict an element's reactivity and bonding patterns in chemical reactions.Learn more aboutelectron configurationsbrainly.com/question/29157546#SPJ11...

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