HL Chemistry. Tuesday August 25th Tuesday, August 25, 15
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1 HL Chemistry Tuesday August 25th 2015
2 Agenda Warm-Up NONE The Atom Project - Use your class time wisely
3 HOMEWORK Questions? The Atom Project -Group Members? DUE August 31st 2015 Atomic Structure Questions DUE August 26th 2015 Topic 12.1 Study Guide HW DUE September 2nd 2015
4 The Atom Project The aim of this project is to learn about the structure of atoms including: Basic structure in terms of protons, neutrons, and electrons and their position in the atom Isotopes, radio-isotopes, and their uses Calculation of relative atomic mass from experimental data The evidence for energy levels and sub-levels within atoms Atomic emission spectroscopy Ionization energy Full electron configuration - using levels and sublevels Solution of problems involving energy levels, with the use of E=hv
5 The Atom Project Your project must meet the following requirements: Describes and explains the structure of atoms, ions and their isotopes in terms of protons, neutrons, and electrons Discusses the various isotopes of the element, their abundance, and their uses Describes the uses of some common radioisotopes Shows how atomic emission spectroscopy provides evidence for energy levels in the atom
6 The Atom Project Your project must meet the following requirements: Explains how to determine the full electron configuration of atoms (including Cr and Cu) Shows how trends ionization energy across the first 20 elements provides evidence to support the existence of energy levels and sub-levels Explains how to solve problems involving energy levels using E=hv Includes a workbook with questions testing the full range of knowledge, with mark-schemes in the back
7 Electrons in atoms Exceptions to the trend Copper (Cu) and Chromium (Cr) Cr [Ar] Cr [Ar] 4s 1 3d 5 Cu[Ar] Cu[Ar] d orbital will fill up before s orbital when it can become half full or completely full
8 Topic 12.1 Electrons in atoms In an emission spectrum, the limit of convergence at higher frequency corresponds to the first ionization energy. Trends in first ionization energy across periods account for the existence of main energy levels and sub levels in atoms. Successive ionization energy data for an element give information that shows relations to electron configurations.
9 Electrons in atoms Nature of science Experimental evidence to support theories - emission spectra provide evidence for the existence of energy levels.
10 Electron Configuration Review Emission spectra and Bohr s theory of the hydrogen atom colour violet blue blue-green red λ/nm transition n = 6 n = 5 n = 4 to n = 2 n = 3 to n = 2 to to n = 2 n = 2
11 Electron Configuration Review Emission spectra and Bohr s theory of the hydrogen atom n=6 n=5 n=4 n=3 n=2 n=1
12 Electron Configuration Review Emission spectra and Bohr s theory of the hydrogen atom Series nf ni Region of EMS Lyman 1 2,3,4,5,... UV Balmer 2 3,4,5,6,... visible and UV Paschen 3 4,5,6,7,... IR
13 Ionization Energy of Hydrogen Emission spectra and Bohr s theory of the hydrogen atom Ionization process for Hydrogen In an atom, the highest possible energy level corresponds to the frequency at which the lines converge By determining the frequency at which the spectral lines can converge (known as the convergence limit) the ionization energy can be calculated. If enough energy is supplied, the one electron in hydrogen atom can be promoted to the th level and would be said to have been ionized to H + Represented by the equation: H(g) > H + (g) + e -
14 Electrons in atoms Emission spectra and ionization Emission spectra provide experimental evidence for the existence of atomic energy levels. Ionization energy is the minimum amount of energy required to remove an electron from a neutral gaseous atom or molecule in its ground state. First ionization energy (IE1): X(g) --> X + (g) + e - Second ionization energy (IE2): X + (g) --> X 2+ (g) + e - Successive ionization energy (IEn): X (n-1)+ (g) --> X n+ (g) + e - With each successive ionization an electron is being removed from an increasingly positive species, so more energy is required. At higher energy, lines of spectra converge, forming a continuum. Outside of this limit the electron is no longer under the influence of the nucleus and has successfully been ionized.
15 Electrons in atoms Ionization energies of first 20 elements Period 1 - Ionization energy increases Period 2 - Ionization energy increases
16 Electrons in atoms Ionization energies of first 20 elements Why is this? As the electrons are removed the nuclear charge increases across a period due to the increased attraction of the nucleus to the valence electrons! The atomic radius also decreases across a period making the electrostatic force even stronger! COOL!
17 Electrons in atoms Ionization energies of first 20 elements Group 1 - Ionization energy decreases Group 2 - Ionization energy decreases
18 Electrons in atoms Ionization energies of first 20 elements Why is this? As we move down a group, more energy levels are added and making the electrostatic force weaker as the distance between the nucleus and valence electrons increases - there is also an increase in electron shielding which further decreases the strength of the electrostatic force between the nucleus and valence electrons COOL!
19 Electrons in atoms Ionization energies of first 20 elements But WAIT! What about the discrepancies to the trend?
20 Electrons in atoms Exceptions to the trend Why is this? - Be has the electron configuration 1s 2 2s 2 - B has the electron configuration 1s 2 2s 2 2p 1 The electrons in the p orbital are higher in energy and further away from the nucleus and require less energy to remove than electrons in the s orbital - Mg has the electron configuration 1s 2 2s 2 2p 6 3s 2 - Al has the electron configuration 1s 2 2s 2 2p 6 3s 2 2p 1
21 Electrons in atoms Exceptions to the trend Why is this? - N has the electron configuration 1s 2 2s 2 2p 3 - O has the electron configuration 1s 2 2s 2 2p 4 Oxygen has a p orbital that is occupied by two electrons where nitrogen only has one electron in the p orbital. This means less energy is required to remove the electron in a half filled orbital due to the fact that like charges repel one another! P orbital Nitrogen P orbital Oxygen
22 Electrons in atoms Exceptions to the trend Why is this? More stable! Less stable! Orbitals that are empty, full, or half-full are more stable and require more energy to remove electrons!
23 Ionization Energy Trends in the Periodic Table of Elements Increasing ionization energy Increasing ionization energy
24 Topic 12.1 Electrons in atoms In an emission spectrum, the limit of convergence at higher frequency corresponds to the first ionization energy. Trends in first ionization energy across periods account for the existence of main energy levels and sub levels in atoms. Successive ionization energy data for an element give information that shows relations to electron configurations.
25 HOMEWORK Questions? The Atom Project -Group Members? DUE August 31st 2015 Atomic Structure Questions - Chapter(s) DUE August 26th 2015 Topic 12.1 Study Guide HW DUE September 2nd 2015
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