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There are many exceptions in the very large atoms, but the two most common ones are Copper and Chromium. The 3d suborbital is more stable when either half filled, or completely filled. In the case of Chromium, one of the 4s electrons is moved to the 3d, so the configuration is [Ar]4s1 3d5. For copper, it is the same case, one of the 4s electrons is moved to the 3d suborbital to lower the overall energy, which makes the configuration [Ar] 4s1 3d10. Elements such as Niobium, Molybdenum, Ruthenium, Rhodium, Palladium, and Silver, along with a few elements in period 6 and 7 also have exceptions to the electron configuration rule. To see all of them, follow this link: http://en.wikipedia.org/wiki/Electron_configuration
What else can I help you with?
What is the electonic configurations for the following atoms of Pd?
The electron configuration of palladium is [Kr]4d10.
How do you write out the electron configurations of solutions?
Solutions are mixtures of one or more solutes dissolved in a solvent. They do not have electron configurations. Only atoms and ions have electron configurations.
Two elements in the same chemical family can have the same spectrum?
True, elements in the same chemical family have similar electron configurations, which can result in similar spectral characteristics. For example, alkali metals like sodium and potassium have similar line spectra due to their similar outer electron configurations.
What is the electron affinity value and which elements have a zero value?
Electron affinity is the energy released when an electron is added to a neutral atom. Elements with a zero electron affinity value include neon, helium, and argon because they have stable electron configurations and do not readily accept additional electrons.
What is the electronic configuration for H2O?
Electron configurations are only made for pure elements. The electron configuration for Hydrogen is 1s1. The electron configuration for Oxygen is 1s2 2s2 2p4
What are the examples of elements with predictable electron configurations?
All of the representative elements (s and p block) have predictable electron configurations. However, many of the transition elements have electron configurations that are not predicted by the rules for determining electron configuration.
Is the periodic table is most easily understood in terms of the electron configurations of the elements?
Yes, understanding the electron configurations of elements can help explain the arrangement of elements on the periodic table. Electron configurations determine an element's chemical properties, reactivity, and position within the table. The periodic table is organized based on recurring patterns in electron configurations, such as the filling of energy levels and sublevels.
Why elements are place in a group?
Elements with similar electron configurations are placed in the same group.
Which elements have electron configurations that end in ns 2 np 5?
The elements with the electron configurations that end in ns 2 and np 5 are halogens, group VII A elements.
Is true about the electron configurations of the representative elements?
Each neutral atom has a specific electron cofiguration.
What has electron configurations of noble gases by gaining one electron?
All halogens or group 17 elements.
What are the symbols for the elements with the following valence electron configurations s2d1?
The electron configuration s2d1 corresponds to the elements in group 6, period 6 of the periodic table. Therefore, the symbol for the element with this configuration would be W, which represents Tungsten.
Which elements have electron configurations that end in ns 2 and np 5?
The elements with electron configurations that end in ns 2 and np 5 are found in Group 17 of the periodic table, known as the halogens. This group includes elements such as fluorine (F), chlorine (Cl), bromine (Br), iodine (I), and astatine (At).
How do elements achieve stable electron configurations between two atoms?
protons
What can be said about the electron configurations of all the elements in a group?
Elements in a group have the same number of valence electrons, giving them similar electron configurations. The electron configurations differ by the number of filled inner shells, leading to a trend in chemical reactivity within the group. The periodic table is organized based on these similarities in electron configurations within groups.
What is the chemical behavior of different elements and what is it determined by?
The chemical behavior of different elements is determined by their electron configurations. Elements with similar electron configurations exhibit similar chemical behavior. For example, elements in the same group of the periodic table tend to have similar chemical properties due to their shared electron configurations.
The elements Li and F combine to form an ionic compound The electron configurations in this compound are the same as the electron configurations of atoms in which group?
The electron configurations of LiF will be the same as the electron configurations of atoms in Group 18 (noble gases) because Li will lose its single electron to attain a stable octet similar to the noble gases, while F will gain an electron to achieve a complete valence shell.
