Atoms first occupy the 4f level in the Lanthanide series, beginning with Cerium (Ce).
The period number on the periodic table tells you which energy level (shell) of an atom is being filled. The subshell within that energy level is determined by the block in which the element is located on the periodic table. For example, elements in the s-block fill the s subshell, elements in the p-block fill the p subshell, and so on.
The actinides family corresponds to the 5f subshell. This subshell can hold a maximum of 14 electrons and is located in the seventh period of the periodic table. The actinides are a series of elements with atomic numbers 89 to 103.
Chromium is located in the d-block of the periodic table because it has its outermost electrons in the d orbital. Specifically, chromium has the electron configuration [Ar] 3d5 4s1, which places it in the d-block between groups 3 and 4. This electron configuration gives chromium its unique properties and allows it to form various oxidation states.
D orbitals start to get filled after the 3p orbitals in the periodic table. They are typically filled after filling the 4s orbital, as the 3d orbitals are the next to be filled in the transition metal series.
the outer shell electrons of the transition elements (middle section) go into the 'd' orbital e.g. Cobalt (Co) 1s2 2s2 2p6 3s2 3p6 4s2 3d7 The 4s orbitals get filled up before the 3d orbitals because it takes less energy to fill the 4s orbital
The period number on the periodic table tells you which energy level (shell) of an atom is being filled. The subshell within that energy level is determined by the block in which the element is located on the periodic table. For example, elements in the s-block fill the s subshell, elements in the p-block fill the p subshell, and so on.
4f
The actinides family corresponds to the 5f subshell. This subshell can hold a maximum of 14 electrons and is located in the seventh period of the periodic table. The actinides are a series of elements with atomic numbers 89 to 103.
Argon has completely filled M shell (or 3p orbital)
Chromium is located in the d-block of the periodic table because it has its outermost electrons in the d orbital. Specifically, chromium has the electron configuration [Ar] 3d5 4s1, which places it in the d-block between groups 3 and 4. This electron configuration gives chromium its unique properties and allows it to form various oxidation states.
The element with atomic number 47 is silver (Ag). In its neutral state, the electron configuration of silver is [Kr] 4d^10 5s^1. This means the 4d subshell is being filled by the electrons of silver.
In the elements from scandium (Sc, atomic number 21) to zinc (Zn, atomic number 30), the d subshell is being filled by electrons. Specifically, these elements are part of the transition metals, where the 3d subshell is progressively filled. As you move from scandium to zinc, the number of electrons in the 3d subshell increases from 1 in scandium to 10 in zinc.
D orbitals start to get filled after the 3p orbitals in the periodic table. They are typically filled after filling the 4s orbital, as the 3d orbitals are the next to be filled in the transition metal series.
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the outer shell electrons of the transition elements (middle section) go into the 'd' orbital e.g. Cobalt (Co) 1s2 2s2 2p6 3s2 3p6 4s2 3d7 The 4s orbitals get filled up before the 3d orbitals because it takes less energy to fill the 4s orbital
An element with the electron configuration Ne3s^23p^5 is in period 3 of the periodic table. The electron configuration indicates that the element has 3 energy levels, with the last electron being in the 3p subshell.
Leaving spaces and gaps in the periodic table allowed for prediction of new elements and their properties, which were later discovered and filled in. This vindicated the decision to leave gaps, as it demonstrated the power of the periodic table in organizing and predicting the properties of elements.