CH 101 1st Edition Lecture 7Outline of Last Lecture I. The Schrodinger Model of the Atom A. NodesII. Introduction to Quantum NumbersIII. The Pattern Within Energy LevelsIV. What Orbitals Look Like A. Electron ConfigurationV. Quantum Numbers on the Periodic TableOutline of Current Lecture I. Reviewing Quantum NumbersII. Atomic Structure and PropertiesA. Core ElectronsB. Valence ElectronsIII. Effective Nuclear ChargeIV. Trends on the Periodic TableCurrent LectureV. Reviewing Quantum NumbersQuantum Number Define Limits n Represents the energy level1, 2, 3, 4, 5, etc…An integer greater than, or equal to, onelOrientation 0, 1, 2, 3 etc…An integer less than the value of nmlOrbital -lto +lif l =1 ml= -1, 0, 1 <- 3 orbitalsThese notes represent a detailed interpretation of the professor’s lecture. GradeBuddy is best used as a supplement to your own notes, not as a substitute.ms Spin -½, +½ Ex) If n = 4, then what are the possible values for l, ml,and ms?l Is any integer less than n, therefore l could equal 3, 2, 1, or 0. ml Is- l to +l, thereforeml could equal -3, -2, -1, 0, 1, 2, 3 = 7 -2, -1, 0, 1, 2 = 5-1, 0, 1 = 30 = 1And ms can only equal -½, +½ VI. Atomic Structure and PropertiesC. Core Electrons – The tightly bounded electrons of filled energy levels in an atom. Core electrons are unaffected by chemical reactions because they don’t want to give or take electrons. D. Valence Electrons– The loosely bounded electrons that are on the outermost shell of an atom that are involved in chemical bonding. The valence electrons are shown as the highest energy level in the s block and the partially filled levels in whatever block it’s in. Ex) What is the valence electron configuration of Sn?Determine the electron configuration of Sn using Lecture 6 notes5s2 5p2 3d10<- Electron configuration of SnRemember that the Valence electron configuration only has the s block and the valence electrons.5s2 5p2<- The valence electron configuration, incudes s block electrons and the unfilled electrons in the p block.VII. Effective Nuclear Charge– The effective nuclear charge is the level of attraction an electron feels toward the nucleus. The effective nuclear charge can be found using this equation. Zeffective = Z - σ (Z = atomic mass) (σ = shielding constant) This equation tells you that as the atomic number goes up, the effective nuclear charge goes up. Ex) Which atom has the lowest Zeff? Pb, Ar, or SLook at the atomic numbers of these elements, Pb = 82 Ar = 18 S = 16S has the lowest Zeff<- Review the trend of effective nuclear charge and see that the lower the atomic number the lower the effective charge. VIII. Trends on the Periodic Table- On the Periodic Table, there are different trends for size, electronegativity, effective charge and ionization energy. Trend for Size of the Atom: The largest atoms are in the bottom left corner and the smaller atoms are in the top right cornerTrend for the Electronegativity of an Atom: The smaller an atom is, the more electronegative it is. This is because the smaller atoms have a stronger pull on their electron cloud and when bonded with another atom it will take some of its electrons and pull the electron cloud more toward its self. Most electronegativeLeast electronegativeTrend for the Effective Charge of an atom:The effective charge increases as you move right and as you move down, it increases with atomic number. However, the effective charge tends to drop between rows so just remember that it increases as you go right and that the upper right hand side has the Trend for the Ionization Energy of an atom: The ionization energy increases as you moveup and to the right of the periodic table. The ionization trend inversely correlates to the trend of the size of the atom. The larger the atom, the weaker the ionization energy. Thisrelationship occurs because the larger the atom is, the farther away the outer shell of electrons is from the nucleus which make is easier for that atom to lose its outer electrons, giving it a low ionization energy. High ionization energyLow ionization