Electronic configuration notation for

When writing the electron configuration notation for an atom, what three principles or rules should you follow ... 

Sodium s two bright lines have wavelengths of 588.9590 nm and 589.9524 nm. What is the ground-state electron configuration notation for sodium, and how does sodium s electron configuration relate to the lines ... 

Write the electron-configuration notation for the element whose atoms contain the following number of electrons ... 

For sodium, the first ten electrons occupy Is, 2s, and 2p orbitals. Then, according to the aufbau sequence, the eleventh electron occupies the 3s orbital. The electron configuration notation and orbital diagram for sodium are written... 

Personal Tutor For an online tutorial on electron configuration notation, visit glencoe.com. 

Figure 11.14 Electron configuration notation. An electron configuration specifies the number of electrons in each sublevel for any specified atom. The value of n that represents the principal energy level is written first, followed by the letter that indicates the sublevel. The number of electrons in each sublevel is written as a superscript. 

Write the complete electron-configuration notation, the noble-gas notation, and the orbital notation for the following elements ... 

Write both the complete electron-configuration notation and the noble-gas notation for each of the elements below. (Hint See Sample Problem C.)... 

Covalent bond formation usually involves only the electrons in an atom s outermost energy levels, or the atom s valence electrons. To keep track of these electrons, it is helpM to use electron-dot notation. Electron-dot notation is an eiectron-conflguration notation in which oniy the vaience eiectrons of an atom of a particular element are shown, indicated by dots placed around the element s symbol. The inner-shell electrons are not shown. For example, the electron-dot notation for a fluorine atom (electron configuration [He]2s 2p ) may he written as follows. 

The electron configuration is the orbital description of the locations of the electrons in an unexcited atom. Using principles of physics, chemists can predict how atoms will react based upon the electron configuration. They can predict properties such as stability, boiling point, and conductivity. Typically, only the outermost electron shells matter in chemistry, so we truncate the inner electron shell notation by replacing the long-hand orbital description with the symbol for a noble gas in brackets. This method of notation vastly simplifies the description for large molecules. 

Give the notation for the valence-shell configuration (including the outermost (/-electrons) of (a) the alkali metals ... 

As the number of electrons In an atom Increases, a listing of all quantum numbers quickly becomes tedious. For example. Iron, with 26 electrons, would require the specification of 26 sets of 4 quantum numbers. To save time and space, chemists have devised a shorthand notation to write electron configurations. The orbital symbols (1 5, 2 p,... 

C08-0009. Determine the energy level diagram and shorthand notation for the electron configuration of the fluorine atom. 

C08-0058. Write the correct ground-state electron configuration, in shorthand notation, for C, Cr, Sb, and Br. 

To determine the electron configuration in this manner, start with the noble gas of the previous period and use the subshell notation from only the period of the required element. Thus, for Fe, the notation for Ar (the previous noble gas) is included in the square brackets, and the 4s23db is obtained across the fourth period. It is suggested that you do not use this notation until you have mastered the full notation. Also, on examinations, use the full notation unless the question or the instructor indicates that the shortened notation is acceptable. 

Table Al.l Electronic configuration of the elements. Elements in square brackets (e.g., [He]) imply that the electronic configurations of the inner orbitals are identical to those of the element in brackets. Thus silver (Ag, atomic number 47) has a configuration of [Kr]4(7105 1, which if written out in full would be s22s22p62s22p62d1QAs1Ap6Adw5>s1, giving 47 electrons in all. For the heavier elements (atomic number above 55), the alternative notation K, L, M is used to denote the inner shells corresponding to orbitals 1, 2 and 3 respectively. This notation is common in X-ray spectroscopy (see p. 33). (Adapted from Lide, 1990.)...

The condensed electron configuration for a nitrogen atom, for example, is [He]2s 2p. The notation [He] is used to represent Is. For a sodium atom [Z = 11), the condensed electron configuration is [Ne]3s. Here, [Ne] represents, ls 2s 2p . Be aware that condensed electron configurations are simply convenient short forms. Thus, [Ne]3s does not mean that a sodium atom is the same as a neon atom plus one electron. Sodium and neon are different elements because the nuclei of their atoms are completely different. 

The /block includes all the inner transition elements. Atoms of /block elements have filled s orbitals in the outer energy levels, as well as filled or partially filled 4/and 5/orbitals. In general, the notation for the orbital filling sequence is ns, followed by (n - 2)/, followed by (n - l]d, followed by (for period 6 elements) np. However, there are many exceptions that make it difficult to predict electron configurations. Because there are seven/orbitals, with a maximum of fourteen electrons, the /block spans fourteen groups. 

The diagram above shows the electronic configuration for carbon in orbital box notation. The two electrons in the p subshell are in different orbitals, but have parallel spins, and the electrons sharing the same orbitals in the Is and 2s subshells have opposite spins. The diagram also suggests that one of the 2p orbitals is empty. In reality, there is no such thing as an empty orbital. If an orbital is empty, then it does not exist. However, it is acceptable to show empty orbitals in this type of notation. 

The table shows the electronic configuration in spectroscopic and orbital box notation for the elements from scandium to zinc. [Ar] represents the electronic configuration of argon, which is Is 2s 2p 3s 3p . It is okay to use this shorthand here instead of writing out the full electron shells up to 3p. However, in the exam you should write out the spectroscopic notation for each element in full. 

The electronic configuration of N is is 2s 2p and for 0 it is is 2s 2p . if you write these in orbital box notation, you will see that the electron to be removed from N is from a half-full 2p subshell. As half-full subshells are also fairly stable, then more energy is required to remove an outer electron from N than from 0. Therefore the first ionisation energy of N is slightly greater than that of 0. 

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