There are four nodes total (5-1=4) and there are two angular nodes (d orbital has a quantum number =2) on the xz and zy planes. The 2s orbital would be filled before the 2p orbital because orbitals that are lower in energy are filled first. This quantum number also determines the number of orbitals per subshell. Electron configurations can be used for a variety of, including: In this subsection, the electron configurations of a few elements are illustrated. The important terms that are related to electron configuration writing are as follows. Ltd. All Rights Reserved, Get latest notification of colleges, exams and news, Electronic Configuration of First 20 Elements, Classification of Elements & Periodicity Properties. Now in the next step, start drawing the orbital diagram for selenium. Legal. Heres how you can draw the orbital diagram of selenium step by step. Required fields are marked *. What are the three rules to be followed at the time of writing the electronic configuration of elements? Explanation: A 4p orbital, which is part of the p subshell located on the fourth energy level, can hold a maximum of two electrons. For example, the electron configuration of sodium is 1s, An electron in an atom is defined by a set of four, The sequence of completely filled subshells that correspond to the electronic configuration of a, As a result, sodium's abbreviated electron configuration is. 3rd ed. As you can see, the periodic table shown in Figure 2.6.3 provides a simple way to remember the order of filling the subshells in determining the electron configuration. Batch split images vertically in half, sequentially numbering the output files. The 3p orbital is now full. Chromium atoms have 24 electrons and 24 protons with the most abundant isotope having 28 neutrons. So draw two arrows in the 2s box showing two electrons as follows: 2p6 indicates that the 2p subshell has 6 electrons. Electrons in atoms are defined by 4 quantum numbers. The Aufbau principle is thatthe electrons present in the atom will first complete the lowest energy orbital and then gradually continue to complete the higher energy orbital. This is the way electrons move from one electron orbital to the next. This is clearly shown in the figure of the orbital diagram of selenium. To maximize the total spin, the electrons in orbitals with only one electron all have the same spin (or the same values of the spin quantum number). Print. Selenium excited state electron configuration, Selenium ion(Se2-) electron configuration, electron configuration of all the elements, Californium(Cf) electron configuration and orbital diagram, Rhodium(Rh) electron configuration and orbital diagram, Molybdenum(Mo) electron configuration and orbital diagram, Thorium(Th) electron configuration and orbital diagram, Carbon(C) electron configuration and orbital diagram, Platinum(Pt) electron configuration and orbital diagram, Electron configuration through orbit(Bohr principle), Electron configuration through orbital(Aufbau principle). Therefore, the next two electrons enter the 2s orbital. After the 3d sublevel is filled, additional electrons will occupy the 4p orbitals, for a total of 6 electrons in the 4p sublevel. The Group IV - VII non-metals gain electrons until their valence shells are full (8 electrons). Electron configurations help determine an atom's valence electrons, which provides insight into its chemical behaviour. 8 Multiple Choice 2 8 00:09:34 O 4 eBook 0 5 2 and correspond to differently shaped volumes of space in which the probability of finding the electrons is high. The 2p, 3p, 4p, etc., can each hold six electrons because they each have three orbitals, that can hold two electrons each (3*2=6). The s-orbital can have a maximum of two electrons. So, the next two electrons will enter the 4s orbital and ten electrons will enter the 3d orbital. What are the exceptions to electron configuration rules? Write the ground-state electron configuration for S2-. While vanadium (to the left) added one electron to its third shell, chromium adds its electron to the third shell and has one electron from the fourth shell bumped down . So draw four arrows in the 4p box showing four electrons as follows: Thats it! A single orbital can only hold 2 electrons, therefore the s subshell has 1 orbital. Atomic energy shells are subdivided into sub-energy levels. Because each orbital is different, they are assigned specific quantum numbers: 1s, 2s, 2p 3s, 3p,4s, 3d, 4p, 5s, 4d, 5p, 6s, 4f, 5d, 6p, 7s, 5f, 6d, 7p. A more thorough explanation using quantum numbers can be found below. Using Kolmogorov complexity to measure difficulty of problems? In practice, no known atoms have electrons in the $g$ or $h$ subshells, but the quantum mechanical model predicts their existence. One of the topics of my research is the periodic table. To sum up, the 3pz orbital has 2 nodes: 1 angular node and 1 radial node. Then the next two electrons will enter the 2s orbital just like the 1s orbital. Electrons are found within the lobes. The order of the electron orbital energy levels, starting from least to greatest, is as follows: 1s, 2s, 2p, 3s, 3p, 4s, 3d, 4p, 5s, 4d, 5p, 6s, 4f, 5d, 6p, 7s, 5f, 6d, 7p. A #4p# orbital, which is part of the #p# subshell located on the fourth energy level, can hold a maximum of two electrons. The number of radial and angular nodes can only be calculated if the principal quantum number, type of orbital (s,p,d,f), and the plane that the orbital is resting on (x,y,z, xy, etc.) The 4d orbital is now full. General Chemistry Principles & Modern Applications. Why is the configuration of electrons in elements important? So, the next two electrons will enter the 4s orbital and ten electrons will enter the 3d orbital. What is Chlorine's Electron Configuration and how do you write it? Why are physically impossible and logically impossible concepts considered separate in terms of probability? (2 marks). How many electrons are in the 4p subshell of selenium? The p-subshell has three orbitals. The colors of the visible spectrum are red, orange, yellow, green, blue, and violet. Explanation: A 4p orbital, which is part of the p subshell located on the fourth energy level, can hold a maximum of two electrons. The valency of the element is determined by electron configuration in the excited state. A 4.0-kg block moving at 2.0 m/s west on a frictionless surface collides totally inelastically with a second 1.0-kg block traveling east at 3.0 m/s. (Cs, Ga, K, Bi, As), As What are some common mistakes students make with orbitals? As shown in Table 1, the s subshell has one lobe, the p subshell has three lobes, the d subshell has five lobes, and the f subshell has seven lobes. We know that the values of the quantum number l determine the number of subshells. However, electrons will never be found in between two orbitals. 4. Then the correct electron configuration of selenium in the ground state will be 1s2 2s2 2p6 3s2 3p6 3d10 4s2 4px2 4py1 4pz1. For the first shell, $n=1$, so only one value of $\ell$ is allowed: $\ell=0$, which is the $s$ subshell. Learnool.com was founded by Deep Rana, who is a Mechanical Engineer by profession and a blogger by passion. The electrons are filled in the following order: Therefore, the electron configuration of oxygen is 1s2 2s2 2p4 as shown below: Magnesium has an atomic number of 12. Angular nodes are typically flat plane (at fixed angles), like those in the diagram above. The elements that have 5, 6, or 7 electrons in the last shell receive the electrons in the last shell during bond formation. The s orbital is a closet and has one bed in it so the first floor can hold a total of two electrons. 1 b. Calculate the molar concentration of chloride ions [ Cl ] ( mol / L ) in a solution prepared by mixing 100 . The $s$ subshell has one orbital for a total of 2 electrons, The $p$ subshell has three orbitals for a total of 6 electrons, The $d$ subshell has five orbitals for a total of 10 electrons, The $f$ subshell has seven orbitals for a total of 14 electrons, The $g$ subshell has nine orbitals for a total of 18 electrons, The $h$ subshell has eleven orbitals for a total of 22 electrons, The first shell only has the $s$ subshell $\implies$ 2 electrons, The second shell has the $s$ and $p$ subshells $\implies$ 2 + 6 = 8 electrons, The third shell has the $s$, $p$, and $d$ subshells $\implies$ 2 + 6 + 10 = 18 electrons, The fourth shell has the $s$, $p$, $d$, and $f$ subshells $\implies$ 2 + 6 + 10 + 14 = 32 electrons, The fifth shell has the $s$, $p$, $d$, $f$, and $g$ subshells $\implies$ 2 + 6 + 10 + 14 + 18 = 50 electrons, The sixth shell has the $s$, $p$, $d$, $f$, $g$, and $h$ subshells $\implies$ 2 + 6 + 10 + 14 + 18 + 22 = 72 electrons, $n$, the principle quantum number defines the shell. We can write the arrangement of the 3d orbitals as follows. According to Hund's principle, the first electron will enter in the clockwise direction and the next electron will enter the 1s orbital in the anti-clockwise direction. . Then the next two electrons will enter the 3s orbital just like the 1s orbital and then the next six electrons will enter the 3p orbital just like the 2p orbital. So, the electron will enter the 4s orbital first and enter the 3d orbital when the 4s orbital is full. The arrangement of electrons in different orbits and orbitals of an atom in a certain order is called electron configuration. Which has been discussed in detail above. Px, Py, Pz. The actual filling order is more complicated. So the total number of orbitals at n=3 energy level is 9. The general electron configuration for atoms of the halogen group is, In what group of the periodic table is the element with the electron configuration [Ar]4s^2 3d^10 4p^3. Connect and share knowledge within a single location that is structured and easy to search. For the third shell, $n=3$, so the allowed values of $\ell$ are: $\ell=0$, which is the $s$ subshell, $\ell=1$, which is the $p$ subshell, and $\ell=2$, which is the $d$ subshell. Sr(NO3)2\mathrm{Sr}\left(\mathrm{NO}_{3}\right)_{2}Sr(NO3)2. Why does a neutral atom of beryllium not have any electrons in a p orbital? (3 marks). Of these colors, _______ has the most energy. The s subshell can have a maximum of 2 electrons as it has only 1 orbital. How many orbitals are there in the 4p subshell? Learn more about Stack Overflow the company, and our products. the filled 3d subshell effectively withdraws from chemistry and the subsequent trend looks much like trends in the periods 2 and 3. Then next ten electrons will enter the 4d orbital. The 2p, 3p, 4p, etc., can each hold six electrons because they each have three orbitals, that can hold two electrons each (3*2=6). Does chromium have 4 electron shells? Because the 1s orbital can only hold two electrons, the next two electrons for Ne are placed in the 2s orbital. There are two major exceptions to electron configuration: chromium and copper. The electron configuration of neon is written as the first two electrons in the electron configuration for neon will be in the 1s orbital. Each subshell contains a specified number of orbitals, and each orbital can hold two electrons. Of these colors, _______ has the most energy. Great Britian: Longman Green & Co., 1961. The magnetic quantum number can range from to +. The next three electrons will enter the 2p orbital in the clockwise direction and the next three electrons will enter the 2p orbital in the anti-clockwise direction. The Pauli Exclusion Principle states that no two electrons in the same atom can have the exact same set of quantum numbers. To write the orbital diagram of selenium(Se), you have to do the electron configuration of selenium. What are the maximum number of electrons in each shell? The 1s orbital is now filled with two electrons. The best answers are voted up and rise to the top, Not the answer you're looking for? USA: Linus Pauling, 1947. By clicking Accept all cookies, you agree Stack Exchange can store cookies on your device and disclose information in accordance with our Cookie Policy. The orbitals are filled so that the ones of lowest energy are filled first. According to the Pauli exclusion principle, an orbital can only hold a maximum of two electrons with opposite spins. The elements in Group 2A are known by what name? If there are more electrons after the 1s, and 2s orbitals have been filled, each p orbital will be filled with one electron first before two electrons try to reside in the same p orbital. So draw six arrows in the 3p box showing six electrons as follows: 4s2 indicates that the 4s subshell has 2 electrons. The numbers, (n=1,2,3, etc.) The Pauli exclusion principle states that no two electrons can have the same exact orbital configuration; in other words, the same quantum numbers. Write the ground state electron configuration for Ca2+ . He loves to learn something new everyday and believes that the best utilization of free time is developing a new skill. How many electrons can the p orbital hold? Question: How many electrons are in the 4p subshell of selenium? We also acknowledge previous National Science Foundation support under grant numbers 1246120, 1525057, and 1413739. Sub-shell s has two, sub-shell p has six and sub-shell d has 10. This electron configuration shows that the selenium ion(Se2-) acquired theelectron configuration of krypton. fourth shell holds 32 electrons; 2 in a 4s orbital; 6 in three 4p orbitals; 10 in five 4d orbitals; and 14 in seven 4f orbitals. So, the remaining electrons will enter the third orbit. This is because the $3d$-orbitals aren't filled until we get to elements from the 4th period - ie. Ques. How to write the orbital diagram for selenium? are called principal quantum numbers and can only be positive numbers. For the second shell, $n=2$, so the allowed values of $\ell$ are: $\ell=0$, which is the $s$ subshell, and $\ell=1$, which is the $p$ subshell. So, if there are open orbitals in the same energy level, the electrons will fill each orbital singly before filling the orbital with two electrons. By looking at the electron configuration of selenium, it is possible to determine how many electrons are in each sub-shell. When n = 4, The s, p, d, and f subshells correspond to l=0, l=1, l=2, and l=3 values, respectively. Ques. (Mg, Al, Si, K, S), General Chemistry Chapter 6 Thermochemistry, Mathematical Methods in the Physical Sciences, David Halliday, Jearl Walker, Robert Resnick, micro test 5 (vibrios) Genus Vibrio and Relat. You'll get a detailed solution from a subject matter expert that helps you learn core concepts. Hunds rulestates that before a second electron is filled in an orbital, every orbital in a given subshell is singly occupied by electrons. 3d 10 4s 2 4p 3: 34: Se: Selenium: p-block [Ar] 3d 10 4s 2 4p 4: 35: Br: Bromine: p . Here, all the electron-containing subshells with their number of electrons in superscript are written in a sequence. 1 N n. 8 3 4 1A BA 1 H PERIODIC TABLE OF THE ELEMENTS 2 He 1.000 2A 3A 4A 5A 6A 7A 4.003 4 5 6 7 8 o 10 Be B N F Ne 6941 9.012 10.81 1201 14.01 16.00 19.00 20.18 12 13 14 15 16 17 18 Na Mg AI SI P S a Ar 22.99 24.31 26.98 28.09 30.97 32.07 36.45 32.95 19 20 21 22 23 24 25 26 27 28 29 30 31 32 34 35 36 K Ca SC TI V Cr Mn Fe NI Zn Ga GE AS Se Br Kr 30.10 40.00 44.96 47.87 50.94 52.00 54.94 55.85 58.93 58.60 63.55 65.30 69.72 7261 74.92 78.96 79.90 83.80 37 38 39 40 41 42 43 44 45 46 47 48 49 50 51 52 53 54 Rb Sr Y Zr Nb Mo TC Ru Rh Pd Ag Cd In Sn Sb Te 1 Xe 85.47 87.62 88.91 91.22 82.91 95.94 (98) 101.07 102.91 106.42 107.87 112.41 114.82 118.71 121.76 127.60 126.30 131.29 55 56 57 72 73 74 75 76 77 78 79 80 81 82 83 84 85 36 CS Ba La Hf Ta w Re Os Ir Pt Au Hg TI Pb BI At Rn 132.91 137.39 136.91 178.49 180.95 183.84 185 21 190 23 192.22 196.08 156.97 200.59 204.38 207.19200.98 (209) (210) 87 88 89 104 105 106 107 108 109 110 111 112 113 114 115 116 Fr Ra Rf Db Sg Bh Hs Mt Ds Rg FeF2004 Feb 2018 (226) (261) (206) (267) (208) (271) (280) (285) (284) (289 (288) (280) 7 58 Ge 59 Pr 60 Nd 61 Pm 62 Sm 63 Fu 64 ca B5 Th 66 Dy 67 Ho 68 Fr 69 Tim 70 Yb LU. Atomic electron configurations follow a standard notation in which all electrons containing atomic subshells are placed in a sequence (with the number of electrons they hold written in superscript). Radial nodes are spheres (at fixed radius) that occurs as the principal quantum number increases. Using indicator constraint with two variables, Doesn't analytically integrate sensibly let alone correctly. The electronic configuration of each element is decided by the Aufbau principle which states that the electrons fill orbitals in order of increasing energy levels. Any electron present in an atom can be described by a combination of these four numbers. Therefore, the selenium atom will have two electrons in the first shell, eight in the 2nd orbit, eighteen electrons in the 3rd shell, and the remaining six electrons will be in the fourth shell. Ans. Hunds rule specifies the order in which electrons are filled in all subshell orbitals. Thus the $p$ subshell has three orbitals. The sub-energy level s can hold a maximum of two electrons, p can hold a maximum of six electrons, d can hold a maximum of ten electrons, and f can hold a maximum of fourteen electrons. This quantum number defines the shape of the orbitals (probability densities) that the electrons reside in. document.getElementById( "ak_js_1" ).setAttribute( "value", ( new Date() ).getTime() ); Your email address will not be published. Are there tables of wastage rates for different fruit and veg? This configuration shows how the 53 electrons of the iodine atom are distributed among the various . Accessibility StatementFor more information contact us [email protected] check out our status page at https://status.libretexts.org. Your email address will not be published. Twelve electrons over the electron configuration of argon reach the . The d subshell has 5 orbitals and thus can accommodate a maximum of 10 electrons. How many of valence electrons do the element in column. The orbitals are dxy, dyz, dzx, dx2-y2and dz2and each orbital can have a maximum of two electrons. That is, the number of electrons in selenium is thirty-four. So, the next six electrons enter the 4p orbital. What is the charge on the monatomic ion of nitrogen, the nitride ion? How should the electron configuration for neon be written? It only takes a minute to sign up. The p-subshell contains a total of three orbitals, given by the values of ml ml = 1 the 5px orbital ml = 0 the 5py orbital ml = 1 the 5pz orbital Since tin's 5p-subshell contains two electrons, it follows that these electrons will occupy distinct 5p-orbitals. Hence, draw the blank orbital diagram of selenium up to 4p subshell as follows: In the above orbital diagram, the box represents an orbital. The 3p orbital is now full. Electron configuration through orbitals follows different principles. These circular paths are called orbit(shell). For example, the electron configuration of Sodiumis 1s22s22p63s1. Since there are only two allowed values of spin, thus there can only be two electrons per orbital. Electron Configuration describes how theelectronsare distributed in an atom's orbitals. Also, find the total number of unpaired electrons in its ground state. To the level of an orbital, this comes down to one of the two electrons that share an orbital having spin-up, which is given by the spin quantum number #m_s = +1/2#, and the other having spin-down, which is given by #m_s = -1/2#. (2 marks). best union jobs in illinois; how to connect kindle to wifi hotspot; wood & fire neapolitan style pizza menu; leo venus and scorpio venus compatibility Each letter is paired with a specific value: An orbital is also described by its magnetic quantum number (m). The way electrons move from one orbital to the next is very similar to walking up a flight of stairs. For n=3, l has the values: 0,1 and 2. The quantum number determines the number of angular nodes; there is 1 angular node, specifically on the xy plane because this is a pz orbital. 8 Multiple Choice 2 8 00:09:34 O 4 eBook 0 5 2 This problem has been solved! (2 marks), Ans. These orbits are expressed by n. [n = 1,2,3,4 . So, the remaining four electrons enter the 4p orbital. Jayden Arevalo 2K wrote: The number of orbitals depends on the subshell. Ans. A standardized notation is used when writing electron configurations, in which the energy level and type of orbital are written first, followed by the number of electrons present in the orbital written in superscript. This means that for a d subshell , the magnetic quantum number can take 5 possible values. Save my name, email, and website in this browser for the next time I comment. The electrons in a particular subshell may be distributed among volumes of space of equal energies called orbitals. This pattern will give you the correct configuration for all but about 19 elements. Two of those electrons are in sub-shell s, while the other six are found in sub-shell p. The third energy level has a total of 18 electrons. Which subshell can hold the greatest number of electrons? The 4 th energy level contains 4s and 4p subshells. The 3d orbital is now full. Now 1s2 indicates that the 1s subshell has 2 electrons. Ques. For any atom, there are three4p orbitals. Electronic orbitals are regions within the atom in which electrons have the highest probability of being found. As is clear, the total number of unpaired electrons = 4. When the selenium atom is excited, then the selenium atom absorbs energy. Quantum numbers are parameters in the wave equation that describes each electron. The elements that receive electrons and form bonds are called anions. (b) Determine the kinetic energy of each block before and after the collision. The atomic number is the number of electrons in that element. Therefore, the electron configuration of selenium(Se*) in an excited state will be 1s2 2s2 2p6 3s2 3p6 3d10 4s2 4px1 4py1 4pz1 4dxy1. how many electrons are in the 4p subshell of selenium? The serial number of the orbit]. We've added a "Necessary cookies only" option to the cookie consent popup, Noble gas configuration and valence shell electrons, How to determine the number of electron in a shell. What exactly is an element's electron configuration? Bulk update symbol size units from mm to map units in rule-based symbology. In selenium, the first energy level has two electrons in sub-shell s. 12.) So in this case, the valency of selenium is 2. Therefore, the selenium full electron configuration will be 1s2 2s2 2p6 3s2 3p6 3d10 4s2 4p4. Enter the email address you signed up with and we'll email you a reset link. Browse other questions tagged, Start here for a quick overview of the site, Detailed answers to any questions you might have, Discuss the workings and policies of this site. Hence the electronic configuration for Cl- ion will be. Subshell labels are used to write down an atom's electron configuration. The distribution of electrons in an atom's orbitals is referred to as its electronic configuration. First, we look at the n=1 shell (the first shell). How many electrons can be accommodated in the fourth shell of an atom? Hunds principle is that electrons in different orbitals with the same energy would be positioned in such a way that they could be in the unpaired state of maximum number and the spin of the unpaired electrons will be one-way. The values of $m_\ell$ are integers and depend on the value of $\ell$: $m_\ell = -\ell,,-1,0,1,,+\ell$, $m_s$, the spin angular momentum quantum number defines the spin state of each electron. Which orbital would the electrons fill first? The ground state electron configuration of selenium is 1s2 2s2 2p6 3s2 3p6 3d10 4s2 4p4. In terms of quantum numbers, electrons in different shells will have different values of principal quantum number n. So another kind of orbitals (s, p, d, f) becomes available as we go to a shell with higher n. The number in front of the letter signifies which shell the orbital(s) are in. Electron Configuration For Selenium Selenium consists of 34 electrons distribution in its 4 orbits. There's an important distinction between "the number of electrons possible in a shell" and "the number of valence electrons possible for a period of elements". For $\ell=2$, $m_\ell$ has five possible values: $m_\ell=-2,-1,0,+1,+2$. Experts are tested by Chegg as specialists in their subject area. Predicting a group of elements' properties (elements with similar electron configurations tend to exhibit similar properties). In this case, 3-1=2, so there are 2 total nodes. Step #1: find electrons of seleniumStep #2: write electron configuration of seleniumStep #3: draw orbital diagram of selenium. By convention, the following lowercase letters are used to indicate different subshells. The 2s orbital is lower in energy than the 2p orbital. The electrons are arranged in four subshells namely s,p, d and f. The electron configuration of each atom is represented by following a standard notation. Ans. As a result, a hydrogen atom contains one electron, which is assigned to the s subshell of the first shell/orbit. How many electrons does a sulfur atom need to fill its outermost s and p subshells? 5. How many valence electron does a carbon atom have? For example the s subshell can hold a total of 2 electrons. Each has its own specific energy level and properties. The Aufbau method is to do electron configuration through the sub-energy level. a. Therefore, the electron will first enter the 1s orbital. Since Cl- has one electron extra. The main proponents of this principle are scientists Niels Bohr and Pauli. Note:The short electron configuration of selenium is [Ar] 3d104s24p4. The electron configuration of an element with an atomic number greater than 18 cannot be properly determined according to the Bohr atomic model. This would mean 2 electrons could fit in the first shell, 8 could fit in the second shell, 18 in the third shell, and 32 in the fourth shell. This can be seen in Figure \(\PageIndex{1}\). For example, the electron configuration of Sodium is 1s22s22p63s1. Each shell is composed of one or more subshells, which are themselves composed of atomic orbitals.For example, the first (K) shell has one subshell, called 1s; the second (L) shell has two subshells, called 2s and 2p; the third shell has 3s, 3p, and 3d; the fourth shell has 4s, 4p, 4d and 4f; the fifth shell has 5s, 5p, 5d, and 5f and can theoretically hold more in the 5g subshell that is not . s-orbitals can hold 2 electrons, p-orbitals can hold 6, and d-orbitals can hold 10, for a total of 18 electrons. How can this new ban on drag possibly be considered constitutional? Can carbocations exist in a nonpolar solvent? Electrons in an orbital with l = 2 are in a (n) d orbital. The energy of an orbital is calculated by adding the principal and azimuthal quantum numbers. How can I use it? Sub-shells s, p, d and f hold a maximum of two, six, 10 and 14 electrons, respectively. The p subshell has 3 orbitals. The 4p subshell is filled next by six electrons (Ga through Kr). The energy is roughly like this: $$1s < 2s < 2p < 3s < 3p < 4s < 3d < 4p < 5s$$. So, the next two electrons will enter the 4s orbital just like the 1s orbital. Arrange these solutions in order of decreasing freezing point: (a) 0.10mNa3PO40.10~m\mathrm{~Na}_3 \mathrm{PO}_40.10mNa3PO4, (b) 0.35mNaCl0.35~m\mathrm{~NaCl}0.35mNaCl, (c) 0.20mMgCl20.20~m\mathrm{~MgCl}_20.20mMgCl2, (d) 0.15mC6H12O60.15~m\mathrm{~C}_6 \mathrm{H}_{12} \mathrm{O}_60.15mC6H12O6, (e) 0.15mCH3COOH0.15~m\mathrm{~CH}_3 \mathrm{COOH}0.15mCH3COOH.