For example, the following are the first three IEs for Mg, whose electron configuration is 1 s 22 s 22 p 63 s 2: Mg(g) → Mg +(g) + e − IE 1 = 738 kJ/mol Mg +(g) → Mg 2+(g) + e − IE 2 = 1,450 kJ/mol Mg 2+(g) → Mg 3+(g) + e − IE 3 = 7,734 kJ/mol However, IE takes a large jump when a successive ionization goes down into a new shell. This is because more than one IE can be defined by removing successive electrons (if the atom has them to begin with): A(g) → A +(g) + e − IE 1 A +(g) → A 2+(g) + e − IE 2 A 2+(g) → A 3+(g) + e − IE 3Įach successive IE is larger than the previous because an electron is being removed from an atom with a progressively larger positive charge. IE also shows an interesting trend within a given atom. Again, the trend isn’t absolute, but the general trends going across and down the periodic table should be obvious.įigure 8.20 Ionization Energy on the Periodic Table However, as you go across the periodic table and the electrons get drawn closer in, it takes more energy to remove an electron as a result, IE increases: as → PT, IE ↑įigure 8.20 "Ionization Energy on the Periodic Table" shows values of IE versus position on the periodic table. As you go down the periodic table, it becomes easier to remove an electron from an atom (i.e., IE decreases) because the valence electron is farther away from the nucleus. It is always positive because the removal of an electron always requires that energy be put in (i.e., it is endothermic). IE is usually expressed in kJ/mol of atoms. is the amount of energy required to remove an electron from an atom in the gas phase: A(g) → A + (g) + e − Δ H ≡ IE Ionization energy (IE) The amount of energy required to remove an electron from an atom in the gas phase. Referring only to a periodic table and not to Figure 8.19 "Atomic Radii Trends on the Periodic Table", which atom is smaller, Ca or Br? S is above Te on the periodic table, so Te is larger because as you go down the column, the atoms get larger.Si is to the left of S on the periodic table, so it is larger because as you go across the row, the atoms get smaller. Referring only to a periodic table and not to Figure 8.19 "Atomic Radii Trends on the Periodic Table", which atom is larger in each pair? Again, we can summarize this trend as follows: as → PT, atomic radius ↓įigure 8.19 "Atomic Radii Trends on the Periodic Table" shows spheres representing the atoms of the s and p blocks from the periodic table to scale, showing the two trends for the atomic radius. The increasing positive charge casts a tighter grip on the valence electrons, so as you go across the periodic table, the atomic radii decrease. This is because although the valence shell maintains the same principal quantum number, the number of protons-and hence the nuclear charge-is increasing as you go across the row. Going across a row on the periodic table, left to right, the trend is different. This trend can be summarized as follows: as ↓ PT, atomic radius ↑ This is because the valence electron shell is getting a larger and there is a larger principal quantum number, so the valence shell lies physically farther away from the nucleus. Such radii can be estimated from various experimental techniques, such as the x-ray crystallography of crystals.Īs you go down a column of the periodic table, the atomic radii increase. Although the concept of a definite radius of an atom is a bit fuzzy, atoms behave as if they have a certain radius. The atomic radius An indication of the size of the atom. The first periodic trend we will consider atomic radius. There may be a few points where an opposite trend is seen, but there is an overall trend when considered across a whole row or down a whole column of the periodic table. There is no other tool in science that allows us to judge relative properties of a class of objects like this, which makes the periodic table a very useful tool. The variation of properties versus position on the periodic table is called periodic trends Variation of properties versus position on the periodic table. One of the reasons the periodic table is so useful is because its structure allows us to qualitatively determine how some properties of the elements vary versus their position on the periodic table. Be able to state how certain properties of atoms vary based on their relative position on the periodic table.
0 Comments
Leave a Reply. |
AuthorWrite something about yourself. No need to be fancy, just an overview. ArchivesCategories |