P sublevel

To illustrate how this rule works, consider an s sublevel ( = 0). Here mi can have only one value, 0. This means that an s sublevel contains only one orbital, referred to as an s orbital. For a p orbital ( = 1) mi = 1,0, or — 1. Within a given p sublevel there are three different orbitals described by the quantum numbers mi = 1, 0, and — 1. All three of these orbitals have the same energy. 

The elements in Groups 13 through 18 (six dements in each period) fill p sublevels, which have a capacity of six electrons. In the second period, the 2p sublevel starts to fill with B (Z = 5) and is completed with Ne (Z = 10). In the third period, the elements A1 (Z = 13) through Ar (Z = 18) fill the 3p subleveL... 

It is possible to explain these trends in terms of the electron configurations of the corresponding atoms. Consider first the increase in radius observed as we move down the table, let us say among the alkali metals (Group 1). All these elements have a single s electron outside a filled level or filled p sublevel. Electrons in these inner levels are much closer to the nucleus than the outer s electron and hence effectively shield it from the positive charge of the nucleus. To a first approximation, each inner electron cancels the charge of one pro-... 

Eight is therefore the "magic number" for valence-shell electrons. Taking electrons from a filled octet is difficult because they are tightly held by a high Zeff adding more electrons to a filled octet is difficult because, with s and p sublevels full, there is no low-energy orbital available. 

The s, p, d, and f levels are also called energy sublevels. The s sublevel has one orbital, an 5 orbital. The p sublevel has three orbitals, x, y, and . The d sublevel has five orbitals and therefore a total capacity of ten electrons. Examine Figure 8.10 to see how the sublevel idea fits in with the concept of energy levels. 

The correct answer is (E). Choice (E) has the noble gas configuration (of argon), which characteristically has filled s and p sublevels. 

The correct answer is (C). The orbital diagram in choice (C) shows filled s and p sublevels, which are characteristic of the nonreactive noble gases. 

The s subshell contains one orbital or region where an electron can be found. The p sublevel has three orbitals, while the d and f levels have five and seven orbitals, respectively. The shapes of the s and p orbitals are shown in Figure 3.5. 

Why can a p sublevel hold six electrons while the s sublevel can hold no more than two electrons ... 

What sublevels are contained in the hydrogen atom s first four energy levels What orbitals are related to each s suhlevel and each p sublevel ... 

Remember Each orbital can hold up to two electrons, so a p sublevel, which contains 3 orbitals, can hold up to 6 electrons (2 electrons x 3 orbitals). To find out how many total electrons a certain energy level can hold, you can do one of two things. First, you could add up the total number of electrons that each of its sublevels can hold. For example, the fourth energy level has four sublevels (s, p, d, and f), which... 

Step 4. Write the configuration, filling in up to 2 electrons in each s sublevel, up to 6 electrons in each p sublevel, up to 10 electrons in each d sub-level, and up to 14 electrons in each f sublevel. We have Is2 2s2 2p6, and that brings us up to 10 electrons. 

Were you surprised that we only placed 1 electron in the 3p sublevel Remember that when we say that a p sublevel can hold up to 6 electrons, we mean that 6 is the maximum that it can hold. In this case, we only had to place 1 electron in the final p sublevel to get up to 13 total electrons. 

The orbital notation of an element is related to the electron configuration, and both types of notation are often shown at the same time. The real difference in the two types of notation has to do with the level of detail shown. In electron configuration, no details are shown about the actual orbitals. When we see 3p4, we know that there are 4 electrons in the p sublevel, but we don t know in which orbitals the electrons are located. When we do the orbital notation for the element, we get that level of detail for the orbitals. 

Next, we will draw one circle for each orbital. Remember from the last lesson that s sublevels contain 1 orbital (as shown in Figure 3-4e on page 89), p sublevels contain 3, and the d and f sublevels hold 5 and 7 orbitals, respectively. 

Compare Figure 3-7d to the number of electrons that each sublevel can hold. You should recall that s sublevels hold 2 electrons, and the s section of the periodic table is made up of 2 columns. The p sublevels hold 6 electrons, and the p section of the periodic table is made up of 6 columns. There are 10 columns in the d section of the periodic table, just as the d sublevels hold up to 10 electrons. The f sublevels hold 14 electrons, and the f section of the periodic table has 14 columns. This connection is no coincidence rather it is a useful piece of information, which will allow you to check your electron configurations. 

Using the arrow diagram to determine the order for filling the sublevels, and placing 2 electrons in each s sublevel and 6 in each p sublevel, we run out of electrons when the 4s sublevel has 1 electron in it. We can check our answer by making sure that the sum of all the superscripts is equal to 19. 

Orbitals are regions of space located aroimd the nucleus of an atom, each having the energy of the sublevel of which it is a part. Orbitals can have different sizes and shapes. There are four types of orbitals that accommodate the electrons for all the atoms of the known elements. Two simple rules apply to these four orbitals. First, an orbital can hold a maximum of two electrons. Second, an orbital has the same name as its sub-level. There is only one s orbital with, at most, 2 electrons. A p sublevel has, at most, 6 electrons, and, thus, there are three p orbitals, each with 2 electrons. Figure 7.7 shows the shapes of s and p orbitals. 

Each s sublevel has one orbital, each p sublevel has three orbitals, each d has five orbitals, and each/sublevel has seven orbitals. Thus there are one 5s orbital, three 5p orbitals, five 5d orbitals, and seven 5/orbitals. The trend of increasing the number of orbitals by two for each succeeding sublevel continues for 5g and beyond. There are nine 5g orbitals with shapes more complex than the shapes of the 4/orbitals. 

An atomic orbital may contain two electrons at most, and the electrons must have different spins. Because each s sublevel has one orbital and each orbital contains a maximum of two electrons, each s sublevel contains a maximum of two electrons. Because each p sublevel has three orbitals and each orbital contains a maximum of two electrons, each p sublevel contains a maximum of six electrons. Using similar reasoning, we can determine that each <5 sublevel contains a maximum often electrons, and each/sublevel contains a maximum of 14 electrons (Table 11.2). 

Atomic numbers 5 through 10 are in the first row of the p block, and the p sublevels start on the second energy level. Therefore, the through 1 electrons go into the 2p sublevel. 

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