Periodic Table Worksheet #L A_ Write the electron configurations (all 3 ways) for the following elements: 1. Sulfur 1s 2s 2p 3s 3d Calcium e[a Is 2s 2p 3s 3p 3d 4s 4p 4d Write the standard and noble gas electron configurations for the following elements: Silver (u:4 0C ,6 ” Gold G.!x) 4.{ . .. ` 43′ . {{ ) t 5. Radium
The Correct Answer and Explanation is:
Electron Configurations:
1. Sulfur (S):
Sulfur has an atomic number of 16, meaning it has 16 electrons. The electron configuration is as follows:
- Full Electron Configuration:
1s22s22p63s23p41s^2 2s^2 2p^6 3s^2 3p^41s22s22p63s23p4 - Abbreviated Electron Configuration (using noble gas):
[Ne]3s23p4[Ne] 3s^2 3p^4[Ne]3s23p4
(Neon is the noble gas preceding sulfur.) - Orbital Notation: 1s ↑↓ 2s ↑↓ 2p ↑↓ ↑↓ ↑ 3s ↑↓ 3p ↑↓ ↑1s \, \uparrow\downarrow \, 2s \, \uparrow\downarrow \, 2p \, \uparrow\downarrow \, \uparrow\downarrow \, \uparrow \, 3s \, \uparrow\downarrow \, 3p \, \uparrow\downarrow \, \uparrow1s↑↓2s↑↓2p↑↓↑↓↑3s↑↓3p↑↓↑ This notation shows how the electrons occupy orbitals and sublevels.
2. Calcium (Ca):
Calcium has an atomic number of 20, so it has 20 electrons. The electron configuration is:
- Full Electron Configuration:
1s22s22p63s23p64s21s^2 2s^2 2p^6 3s^2 3p^6 4s^21s22s22p63s23p64s2 - Abbreviated Electron Configuration:
[Ar]4s2[Ar] 4s^2[Ar]4s2
(Argon is the noble gas preceding calcium.) - Orbital Notation: 1s ↑↓ 2s ↑↓ 2p ↑↓ ↑↓ ↑↓ 3s ↑↓ 3p ↑↓ ↑↓ 4s ↑↓1s \, \uparrow\downarrow \, 2s \, \uparrow\downarrow \, 2p \, \uparrow\downarrow \, \uparrow\downarrow \, \uparrow\downarrow \, 3s \, \uparrow\downarrow \, 3p \, \uparrow\downarrow \, \uparrow\downarrow \, 4s \, \uparrow\downarrow1s↑↓2s↑↓2p↑↓↑↓↑↓3s↑↓3p↑↓↑↓4s↑↓
Noble Gas Electron Configurations:
3. Silver (Ag):
Silver has an atomic number of 47, so it has 47 electrons. Its electron configuration is:
- Full Electron Configuration:
1s22s22p63s23p64s23d104p65s14d101s^2 2s^2 2p^6 3s^2 3p^6 4s^2 3d^{10} 4p^6 5s^1 4d^{10}1s22s22p63s23p64s23d104p65s14d10 - Abbreviated Electron Configuration:
[Kr]5s14d10[Kr] 5s^1 4d^{10}[Kr]5s14d10
(Krypton is the noble gas preceding silver.) - Orbital Notation: 1s ↑↓ 2s ↑↓ 2p ↑↓ ↑↓ ↑↓ 3s ↑↓ 3p ↑↓ ↑↓ 3d ↑↓ ↑↓ 4s ↑ 4d ↑↓ ↑↓1s \, \uparrow\downarrow \, 2s \, \uparrow\downarrow \, 2p \, \uparrow\downarrow \, \uparrow\downarrow \, \uparrow\downarrow \, 3s \, \uparrow\downarrow \, 3p \, \uparrow\downarrow \, \uparrow\downarrow \, 3d \, \uparrow\downarrow \, \uparrow\downarrow \, 4s \, \uparrow \, 4d \, \uparrow\downarrow \, \uparrow\downarrow1s↑↓2s↑↓2p↑↓↑↓↑↓3s↑↓3p↑↓↑↓3d↑↓↑↓4s↑4d↑↓↑↓
4. Gold (Au):
Gold has an atomic number of 79, so it has 79 electrons. Its electron configuration is:
- Full Electron Configuration:
1s22s22p63s23p64s23d104p65s24d105p66s24f145d106p67s11s^2 2s^2 2p^6 3s^2 3p^6 4s^2 3d^{10} 4p^6 5s^2 4d^{10} 5p^6 6s^2 4f^{14} 5d^{10} 6p^6 7s^11s22s22p63s23p64s23d104p65s24d105p66s24f145d106p67s1 - Abbreviated Electron Configuration:
[Xe]4f145d106s1[Xe] 4f^{14} 5d^{10} 6s^1[Xe]4f145d106s1
(Xenon is the noble gas preceding gold.) - Orbital Notation: 1s ↑↓ 2s ↑↓ 2p ↑↓ ↑↓ ↑↓ 3s ↑↓ 3p ↑↓ ↑↓ 3d ↑↓ ↑↓ 4s ↑↓ 4d ↑↓ 5s ↑↓ 4f ↑↓ ↑↓ 5d ↑↓ ↑↓ 6s ↑1s \, \uparrow\downarrow \, 2s \, \uparrow\downarrow \, 2p \, \uparrow\downarrow \, \uparrow\downarrow \, \uparrow\downarrow \, 3s \, \uparrow\downarrow \, 3p \, \uparrow\downarrow \, \uparrow\downarrow \, 3d \, \uparrow\downarrow \, \uparrow\downarrow \, 4s \, \uparrow\downarrow \, 4d \, \uparrow\downarrow \, 5s \, \uparrow\downarrow \, 4f \, \uparrow\downarrow \, \uparrow\downarrow \, 5d \, \uparrow\downarrow \, \uparrow\downarrow \, 6s \, \uparrow1s↑↓2s↑↓2p↑↓↑↓↑↓3s↑↓3p↑↓↑↓3d↑↓↑↓4s↑↓4d↑↓5s↑↓4f↑↓↑↓5d↑↓↑↓6s↑
5. Radium (Ra):
Radium has an atomic number of 88, so it has 88 electrons. Its electron configuration is:
- Full Electron Configuration:
1s22s22p63s23p64s23d104p65s24d105p66s24f145d106p67s21s^2 2s^2 2p^6 3s^2 3p^6 4s^2 3d^{10} 4p^6 5s^2 4d^{10} 5p^6 6s^2 4f^{14} 5d^{10} 6p^6 7s^21s22s22p63s23p64s23d104p65s24d105p66s24f145d106p67s2 - Abbreviated Electron Configuration:
[Rn]7s2[Rn] 7s^2[Rn]7s2
(Radon is the noble gas preceding radium.) - Orbital Notation: 1s ↑↓ 2s ↑↓ 2p ↑↓ ↑↓ ↑↓ 3s ↑↓ 3p ↑↓ ↑↓ 3d ↑↓ ↑↓ 4s ↑↓ 4d ↑↓ 5s ↑↓ 4f ↑↓ ↑↓ 5d ↑↓ ↑↓ 6s ↑↓ 7s ↑↓1s \, \uparrow\downarrow \, 2s \, \uparrow\downarrow \, 2p \, \uparrow\downarrow \, \uparrow\downarrow \, \uparrow\downarrow \, 3s \, \uparrow\downarrow \, 3p \, \uparrow\downarrow \, \uparrow\downarrow \, 3d \, \uparrow\downarrow \, \uparrow\downarrow \, 4s \, \uparrow\downarrow \, 4d \, \uparrow\downarrow \, 5s \, \uparrow\downarrow \, 4f \, \uparrow\downarrow \, \uparrow\downarrow \, 5d \, \uparrow\downarrow \, \uparrow\downarrow \, 6s \, \uparrow\downarrow \, 7s \, \uparrow\downarrow1s↑↓2s↑↓2p↑↓↑↓↑↓3s↑↓3p↑↓↑↓3d↑↓↑↓4s↑↓4d↑↓5s↑↓4f↑↓↑↓5d↑↓↑↓6s↑↓7s↑↓
Explanation:
- Full Electron Configuration lists the electrons in order of their respective orbitals, following the Pauli Exclusion Principle and Hund’s Rule.
- Abbreviated Electron Configuration uses the nearest noble gas as a shorthand for the inner electron configuration.
- Orbital Notation visually represents the orbitals and shows how electrons are distributed according to the available energy levels.
Each element’s electron configuration provides insights into its chemical properties and how it will bond with other elements. For example, elements in the same group (column) of the periodic table will have similar outer electron configurations, leading to similar chemical behaviors.
