Chemistry

Chemistry, 13.07.2019 23:00, XxMikeLearnsxX9288

Write the electron configuration including the population of all partially filled subshells for cd2+

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Chemistry, 27.06.2019 07:20, 2002babygurl

An atom consists of a small positively charged nucleus surrounded by negatively charged electrons. we organize the electrons in a logical manner. as the atomic number increases, electrons are added to the subshells according to their energy. lower energy subshells fill before higher energy subshells the order of filling is 1s, 2s, 2p, 3s, 3p, 4s, 3d, 4p, 5s, 4d, 5p, 6s, 4f, 5d, 6p, 7s, 5f, 6d, 7p. the periodic table can be used to you remember the order. give the ground-state electron configuration for silicon (si). express the complete electron configuration using superscripts where appropriate. for example, the configuration for li would be entered as 1s^22s^1.

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Chemistry, 13.07.2019 18:30, lol1516

To show the electron configuration for an atom, when would it be better to use an orbital notation than to use a written configuration with numbers, letters, and superscripts? when the aim is to use less space when the aim is to show electron spins when the aim is to show orbital shapes in subshells when the aim is to show electron distributions in shells

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Chemistry, 17.07.2019 05:10, ilopez24661

What is the basis for exceptions to the aufbau principle? electron spins are more important than energy levels in determining electron configuration. some elements have unusual atomic orbitals. ment filled and half-filled energy sublevels are more stable than partially-filled energy sublevels. electron configurations are only probable. model

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Chemistry, 24.10.2019 20:43, hdjehd

Remember that cr has a ground-state electronic configuration of [ar]4s13d5 and cu has a ground state electronic configuration of [ar]4s13d10. also, remember that when you ionize a transition metal, you always remove electrons from the ns subshell before the (n-1)d subshell. in other words, a cr3+ ion has a configuration of [ar]3d3 and not [ar]4s13d2. the reason for this is that, even though the 6 valence electrons of cr are spread out through the 4s and 3d orbitals as if the 4s and 3d subshells were the same energy, when it comes to ionizing the atom, the 4s orbital is actually slightly higher in energy so that the 4s electron is removed first. which statement(s) is/are true? i. in a calcium atom, the 2px and 3px orbitals have the same size and shape. ii. in a lithium atom, the 2s and 2p subshells have different energies. iii. the 3px, 3py, and 3pz orbitals look the same, but they point in different directions. iv. in a cr atom, a 4s electron has higher energy than a 3d electron. group of answer choices iii, iv only ii, iii only i, ii, iii, iv ii, iii, iv only iii only

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Write the electron configuration including the population of all partially filled subshells for cd2+...

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