Orbital Shapes. Quantum Numbers
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1 Orbital Shapes Quantum Numbers Atom Electron Configurations Electron Configuration complete description of orbitals occupied by all the electrons in an atom for atoms in ground state electrons occupy energy shells, subshells and orbitals that give the lowest energy for the atom start with 1s orbital and work up 1
2 Electron Configurations Electron Configurations for orbitals with same energy (degenerate) such as the three 2p orbitals half-fill each orbital with first 3 electrons go back and pair electrons with 4, 5 and 6 Hund s Rule electrons pair only after each orbital in a subshell is occupied by a single electron C: 1s 2 2s 2 2p 2 1s 2s 2p or: [He] 2s 2 2p 2 Electron Configurations and the Periodic Table 2
3 Valence Electrons Chemically similar behavior occurs among elements within a group in the periodic table. Valence electrons electrons held in outer shell Core electrons electrons held in filled inner shells Electron Configurations of Transition Elements d subshell being filled valence electrons - s and p electrons in outermost shell plus electrons in incompletely filled (n - 1)d subshell (n - 1)d orbitals are filled after ns orbitals and before filling np orbitals Co: [Ar] half-filled d subshells are favored if possible (Hund s Rule) Cr: [Ar] 3d 3d 4s 4s Example 5 What family of elements is characterized by having an ns 2 np 3 valence-electron configuration? Group 5A 3
4 Ion Electron Configurations Metal atoms lose electrons to form cations with a positive charge equal to the group number. Nonmetal atoms gain electrons to form anions with a negative charge equal to the A group number minus eight. Ca (Group 2) Ca 2+ O (Group 6A) O 2- Transition Metal Ions The ns electrons are at a higher energy than the (n-1)d electrons so they are always removed before the (n-1)d electrons when TMs form cations. Fe Fe e- Fe 0 [Ar] Fe 2+ [Ar] 3d 4s 3d 4s Magnetic Properties of Compounds Diamagnetic atoms and ions with all electrons paired (will be repelled by magnetic field) Paramagnetic atoms and ions with unpaired electrons (will be attracted to magnetic field) 4
5 Periodic Trends: Atomic Radii move down periodic table increasing n as n gets larger that shell s radius increases atomic size (radius) increases as you move down the periodic table atomic size (radius) decreases as you move right in the periodic table Periodic Trends: Atomic Radii Periodic Trends: Atomic Radii 5
6 Example 6 Which will be closer to the nucleus, the n = 3 electron shell in Ar or the n = 3 electron shell in Kr? Kr because # protons is higher Bond Length Example 7 Predict which will be greater, the P Br bond length in PBr 3 or the As Br bond length in AsBr 3? As Br atomic radius of As > P 6
7 Example 8 Arrange the following atoms in order of increasing atomic radius: K, Mg, Ca Mg < Ca < K Periodic Trends: Ionic Radii radii of ions of elements in same group increase in size going down the group radius of cation always smaller than that of neutral atom from which derived radius of anion always larger than that of neutral atom from which derived Periodic Trends: Ionic Radii 7
8 Periodic Trends: Ionization Energies ionization energy energy needed to remove one electron from atom s- and p-block elements first ionization energies decrease down a group and across a period Periodic Trends: Ionization Energies Periodic Trends: Ionization Energies 8
9 Example 9 Predict which of the following atoms C, Si, N or P has the lowest first ionization energy. Si Periodic Trends: Electron Affinities electron affinity (EA) energy change when an electron is added to a gaseous atom to form 1- ion measure of attraction an atom has for an additional electron large negative value indicates a ready acceptance of an electron F(g) + e- F-(g) Periodic Trends: Electron Affinities electron affinity (EA) energy change when an electron is added to a gaseous atom to form 1- ion measure of attraction an atom has for an additional electron large negative value indicates a ready acceptance of an electron F(g) + e- F - (g) Ne + e- Ne- ΔE = EA = -328 kj/mol EA > 0 kj/mol 9
10 Periodic Trends: Electron Affinities 10
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