[Kr] 4d10 5s1
Just by looking at your Periodic Table you should see that this element is silver.
The [Kr] indicates it follows krypton on the table and you just need to count to '10'+'1' = '11' to come out there.
Atom numbers Kr=36, Ag=47, difference 11 (of coarse)
The element with the ground-state electron configuration Kr 4d10 5s2 5p5 is iodine (I).
iodine
The electron configuration for oxygen is 1s2 2s2 2p4. The electron configuration for sulfur is 1s2 2s2 2p6 3s2 3p4.
The long form of the electron configuration of einsteinium (Es) is [Rn] 5f11 7s2.
The electron configuration of curium (Cm) is [Rn] 5f^7 6d^1 7s^2.
The electron configuration of lithium (Li) is 1s2 2s1, with 3 electrons distributed in the 1s and 2s orbitals. The electron configuration of fluorine (F) is 1s2 2s2 2p5, with 9 electrons distributed in the 1s, 2s, and 2p orbitals.
The electron configuration of boron is 1s2 2s2 2p1. When boron becomes an ion, it typically loses its outer electron to achieve a stable electron configuration. Therefore, the electron configuration of a boron ion is typically 1s2 2s2.
The predicted electron configuration of bohrium is [Rn]5f14.6d5.7s2.
Transition metals have ground-state electron configurations that differ from the predicted ones due to the exchange of electrons between the ns and (n-1)d subshells. This exchange stabilizes the d orbitals, leading to configurations that are closer to half-filled or fully filled d subshells. Examples include chromium ([Ar] 3d^5 4s^1) and copper ([Ar] 3d^10 4s^1).
[Rn] 5f14 6d10 7s2 7p3 (predicted)2, 8, 18, 32, 32, 18, 5 (predicted)
The atomic number of dubnium is 105. It is a synthetic element with the symbol Db.
Noble gases have predictable electron configurations as they have completely filled outer electron shells (e.g. helium, neon). Transition metals also have predictable electron configurations based on their position on the periodic table and electron filling rules (e.g. iron, copper).
An elements property can be best predicted from the group it is in the Periodic Table. Groups (the columns of the tables) of elements have similar properties due to their similar electron configuration of the valence shell.
The groundstate for Sodium (11-Na) is: 1S2 , 2S2, 2P6, 3S1 If you count the ^powers you notice it'll sum to 11, when Sodium is excited the outermost electron (3S1) will be excited from the 3S shell to the next shell up which is the 3P shell. The "core" electron configuration doesn't change so the first excited state is simply: 1S2 , 2S2, 2P6, 3P1 For the next excited state the electron that is now in the 3P shell will transition to the 4S shell before the 3D shell
The electron configuration of lithium (Li) is 1s2 2s1, with 3 electrons distributed in the 1s and 2s orbitals. The electron configuration of fluorine (F) is 1s2 2s2 2p5, with 9 electrons distributed in the 1s, 2s, and 2p orbitals.
The electron configuration for oxygen is 1s2 2s2 2p4. The electron configuration for sulfur is 1s2 2s2 2p6 3s2 3p4.
The long form of the electron configuration of einsteinium (Es) is [Rn] 5f11 7s2.
The electron configuration of curium (Cm) is [Rn] 5f^7 6d^1 7s^2.
The electron configuration of Cl is 1s2 2s2 2p6 3s2 3p5. This represents the distribution of electrons in the various energy levels and orbitals of a single chlorine atom.