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Use the periodic table to identify the element with the following electron configuration:A. 1s2 2s2 2p6 3s2 enter the symbol of the elementB. Krypton 5s2 4d6 enter the symbol of the elementC. How many unpaired electrons are present in a ground-state atom from the halogen family: enter a number, such as 0, 1, 2, etcD. unpaired electrons in the 5A column: enter a number, such as 0, 1, 2, etcE. unpaired electrons in the 6B column enter a number, such as 0, 1, 2, etc

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greycheckers
I can only answer 2 of the problems since the direction of the rest are confusing/unclear.
A) Magnesium (Mg)
B) Ruthenium (Ru)
Histrionicus

The element with the following electron configuration -

  • A. 1s2 2s2 2p6 3s2 - Mg
  • Krypton 5s2 4d6 - Ru
  • halogen (..s2, p5) - 1
  • unpaired electron in 5a - 3
  • unpaired electron in 6b - 4

The atomic number is defined as the number of electrons or protons present in an atom.

  • Atomic number = Number of electrons = Number of protons
  • magnesium atom found in nature has 12 protons, 12 neutrons, and 12 electrons
  • Ruthenium has an atomic number of 44, that is, it contains 44 electrons distributed in atomic orbitals and its nucleus has 44 protons and 57 neutrons
  • The ground state of an electron, the energy level it normally occupies, is the state of lowest energy for that electron therefore halogen - ..s2, p5 so one.
  • Group 5A (15) elements such as nitrogen have five electron valences that mean they have three unpaired electrons.
  • Group 6B has 4 unpaired electrons as this column.

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