Slide 20 / 102 The Periodic Law and Atomic Radii Let's examine the trend in atomic radii for the first 18 elements. Na 200 Li radius (pm) 100 H Ar Ne He 0 0 1 2 3 4 5 6 7 8 9 10 11 12 13 14 15 16 17 18 atomic number We clearly see two trends! 1. As atomic number increases down a group, the radii increase. H < Li < Na 2. As atomic number increases across a period, the radii decrease. Li > Be > B > C > N > O > F > Ne
Slide 21 / 102 The Periodic Law and Atomic Radii The distance the electrons can be from the nucleus is governed by Coulomb's law of attraction. The greater the charge, the greater the attraction between the charges, and the shorter the distance. As atomic number increases across a period, so does the nuclear charge (Z) resulting in a greater attraction and a smaller distance between the nucleus and the outermost electrons. Carbon (Z=6) Neon (Z=10) Lithium (Z=3) radii = 67 pm radii = 38 pm radii = 167 pm **Note: The size of an atom is NOT determined by the size of the nucleus. It is the electron cloud that contains most of the volume of an atom and therefore determines the radii.
Slide 22 / 102 The Periodic Law and Atomic Radii Why don't the radii continue to get smaller as the atomic number and nuclear charge increase. The quantum model explains why. Hydrogen (Z=1) 1s 1 radii = 53 pm Only a certain number of electrons are permitted within Lithium (Z=3) a given energy level, so 1s 2 2s 1 additional ones must be radii = 167 pm added to higher energy levels farther from the nucleus. Sodium (Z=11) 1s 2 2s 2 2p 6 3s 1 radii = 190 pm The core electrons shield the valence electrons from the nucleus thus diminishing the coulombic attraction and increasing the atomic radii.
Slide 23 / 102 The Periodic Law and Ionic Radii When electrons are gained or lost, the effect on the radii can be dramatic or slight but there are some certainties. If an atom gains If an atom loses electrons, the radii will electrons, the radii will increase. decrease. F + e - --> F - Ca --> Ca 2+ + 2e- 42 pm 136 pm 194 pm 99 pm When electrons are gained, When electrons are lost, the the nuclear charge is spread remaining electrons feel a over a larger number of stronger coulombic electrons, resulting in a attraction from the nucleus. weaker coulombic attraction.
Slide 24 / 102 The Periodic Law and Ionic Radii Let's rank a series of atoms and ions in order of increasing radii. Al 3+ Al Mg Mg 2+ Whenever comparing radii, use the following procedure: 1. Determine the energy level of the atom/ion. 2. For atoms in the same energy level, use the nuclear charge (Z) to determine the radii. Al 3+ Al Mg Mg 2+ Energy Level 2 3 3 2 "Z" 13 13 12 12 Al 3+ < Mg 2+ < Al < Mg radius (pm) 50 < 65 < 118 < 145
Slide 25 / 102 The Periodic Law and Ionic Radii Recall that in an isoelectronic series, the atoms/ions have the same number of electrons. In this case, Na + , Mg 2+ , Al 3+ , O 2- , and F - are all isoelectronic with Ne. As a result, they all experience the same core shielding. The ionic radii then decreases with an increasing nuclear charge. Al 3+ < Mg 2+ < Na + < F - < O 2- Z = 13 12 11 9 8
Slide 26 / 102 The Periodic Law and Ionic Radii Let's try a few more together. 1. Explain why Si has an atomic radii of 111 pm while C has an atomic radii of 67 pm despite Si having a higher nuclear charge (Z)? Si has an additional energy level, so the valence move for answer electrons are farther away and more shielded than those of C resulting in a smaller coulombic attraction.
Slide 27 / 102 The Periodic Law and Ionic Radii Let's try a few more together. 2. Explain why iron (Fe) has a smaller atomic radii - 154 pm - than does scandium (Sc) - 184 pm. Although both have the same amount of shielding, Fe has a move for answer larger Z creating a stronger coulombic attraction and a smaller radii.
Slide 28 / 102 6 Which of the following influences the atomic/ionic radii? A the number of neutrons B the amount of core electrons between the nucleus and the valence electrons Answer C the number of protons D A and B E B and C
Slide 28 (Answer) / 102 6 Which of the following influences the atomic/ionic radii? A the number of neutrons B the amount of core electrons between the nucleus and the valence electrons Answer C the number of protons E D A and B E B and C [This object is a pull tab]
Slide 29 / 102 7 The atomic radius of main-group elements generally increases down a group because __________. A effective nuclear charge increases down a group B effective nuclear charge decreases down a group Answer C effective nuclear charge zigzags down a group the principal quantum number of the valence orbitals D increases both effective nuclear charge increases down a group E and the principal quantum number of the valence orbitals increases
Slide 29 (Answer) / 102 7 The atomic radius of main-group elements generally increases down a group because __________. A effective nuclear charge increases down a group B effective nuclear charge decreases down a group Answer B C effective nuclear charge zigzags down a group the principal quantum number of the valence orbitals D increases [This object is a pull tab] both effective nuclear charge increases down a group E and the principal quantum number of the valence orbitals increases
Slide 30 / 102 8 Of the following, which gives the correct order for atomic radius for Be, Li, N, C and Ne? A Be > Li > N > C > Ne B Ne > C > N > Li > Be Answer C C > N > Ne > Li > Be D Li > Be > C > N > Ne E Ne > N > C > Be > Li
Slide 30 (Answer) / 102 8 Of the following, which gives the correct order for atomic radius for Be, Li, N, C and Ne? A Be > Li > N > C > Ne B Ne > C > N > Li > Be Answer D C C > N > Ne > Li > Be D Li > Be > C > N > Ne E Ne > N > C > Be > Li [This object is a pull tab]
Slide 31 / 102 9 Which of the following atoms would have a smaller atomic radii than Ar and why? A Fe - It has more core electrons B Si - It has fewer core electrons Answer C O - It has fewer core electrons D Ne - it has a higher nuclear charge (Z) E Ca - it has a higher nuclear charge (Z)
Slide 31 (Answer) / 102 9 Which of the following atoms would have a smaller atomic radii than Ar and why? A Fe - It has more core electrons B Si - It has fewer core electrons Answer C O - It has fewer core electrons C D Ne - it has a higher nuclear charge (Z) E Ca - it has a higher nuclear charge (Z) [This object is a pull tab]
Slide 32 / 102 10 Which ion below has the largest radius? O 2- A Li + B Answer I - C N 3- D K + E
Slide 32 (Answer) / 102 10 Which ion below has the largest radius? O 2- A Li + B Answer C I - C N 3- D K + E [This object is a pull tab]
Slide 33 / 102 11 Which of the following pairs correctly shows the proper relationship between the two atoms/ions in terms of atomic/ionic radii? A Ca < Ca 2+ B F < F - Answer C V < Mn D Ca < Be E He > Li
Slide 33 (Answer) / 102 11 Which of the following pairs correctly shows the proper relationship between the two atoms/ions in terms of atomic/ionic radii? A Ca < Ca 2+ B F < F - Answer B C V < Mn D Ca < Be [This object is a pull tab] E He > Li
Slide 34 / 102 12 Which of the following correctly states why the atomic radii do not consistently decrease as the atomic number rises throughout the periodic table? A The nuclear charge (Z) does not always increase with atomic number B The number of neutrons start to influence the Answer atomic radii C Filled energy levels shield the nucleus and diminish coulombic forces D Electrons become less negative the more there are E A higher atomic number increases the size of the radii, not decreases it.
Slide 34 (Answer) / 102 12 Which of the following correctly states why the atomic radii do not consistently decrease as the atomic number rises throughout the periodic table? A The nuclear charge (Z) does not always increase with atomic number B The number of neutrons start to influence the Answer C atomic radii C Filled energy levels shield the nucleus and diminish coulombic forces [This object is a pull tab] D Electrons become less negative the more there are E A higher atomic number increases the size of the radii, not decreases it.
Slide 35 / 102 13 Which of the following would correctly rank the following in order of decreasing atomic/ionic radii? A V 4+ > V 5+ > F > F - B V 4+ > V 5+ > F- > F Answer C V 5+ > V 4+ > F - > F D V 5+ > V 4+ > F > F - E F > F - > V 4+ > V 5+
Slide 35 (Answer) / 102 13 Which of the following would correctly rank the following in order of decreasing atomic/ionic radii? A V 4+ > V 5+ > F > F - B V 4+ > V 5+ > F- > F Answer C V 5+ > V 4+ > F - > F B D V 5+ > V 4+ > F > F - E F > F - > V 4+ > V 5+ [This object is a pull tab]
Slide 36 / 102 14 Isotopes of an element, like C-12 and C-13, are likely to have different atomic radii? Yes No Answer
Slide 36 (Answer) / 102 14 Isotopes of an element, like C-12 and C-13, are likely to have different atomic radii? Yes No Answer NO [This object is a pull tab]
Slide 37 / 102 The Periodic Law and Ionization Energy Ionization energy is the amount of energy required to remove an electron from an atom. This creates an ion, hence the name! The stronger the Coulombic attraction between the valence electron and the nucleus, the greater the energy required to remove an electron. Element Ionization Energy Li + IE --> Li + + e- 520 kJ/mol Na + IE --> Na + + e- 496 kJ/mol Less energy is required to remove sodium's electron than lithium's because sodium has a full energy level more of core electrons shielding the nuclear charge.
Slide 38 / 102 The Periodic Law and Ionization Energy Unless you're hydrogen, you've got multiple electrons that can be lost. As a result we have to distinguish between 1st, 2nd, 3rd, etc. ionization energies. Each successive ionization energy is always higher than the previous. This is due to the higher nuclear charge felt by the remaining electrons. Ionization Ionization Energy 1st: Na + IE --> Na + + e- 496 kJ/mol 2nd: Na + + IE --> Na 2+ + e- 4560 kJ/mol 3rd: Na 2+ + IE --> Na 3+ + e- 6,900 kJ/mol 4th: Na 3+ + IE --> Na 4+ + e- 9540 kJ/mol Note the huge jump in ionization energy from the 1st to the 2nd. After sodium loses it's first electron, it is isoelectronic with [Ne], with an extremely stable full s and p orbital and minimal shielding.
Slide 39 / 102 The Periodic Law and Ionization Energy The chart below clearly shows the impact of being isoelectronic with a noble gas on the ionization energy. Ionization Energy (kJ/mol) Na + Mg 2+ Al 3+ Si 4+ P 5+ S 6+
Slide 40 / 102 The Periodic Law and Ionization Energy The trend in first ionization energies mostly matches what we would expect. The ionization energy increases across a period with increasing atomic number. ( Li < Ne) The ionization energy decreases down a group with increasing atomic number due to additional core electrons from each filled energy level shielding the nucleus. ( He > Ne)
Slide 41 / 102 The Periodic Law and Ionization Energy There are however a few hiccups that need to be explained. Let's look carefully at the ionization energies of Be and B as well as N and O indicated in the circles. Shouldn't the ionization energy increase with increasing atomic number across a period? Quantum theory will explain.
Slide 42 / 102 The Periodic Law and Ionization Energy Be: [He]2s 2 N: [He]2s 2 2p 3 B: [He]2s 2 2p 1 O: [He]2s 2 2p 4 More energy is required More energy is required to to remove an electron remove an electron from from Be's full "s" orbital N's 1/2 full "p" orbital
Slide 43 / 102 The Periodic Law and Ionization Energy Let's look at another hiccup in the trend. Notice that a lot less energy is required to remove an electron from Ga (Z=31) than from Zn (Z=30). How can this be? Zinc has a full "s" and "d" orbital conferring extra stability while in gallium, the electron is being taken from a "p" orbital which is heavily shielded from the nucleus by the "d" orbital itself.
Slide 44 / 102 The Periodic Law and Ionization Energy Let's practice ranking atoms/ions in terms of ionization energy: 1. Rank the following in terms of increasing ionization energy: C Al Na+ Ne Na As with atomic radii, determine their outermost principal energy level and nuclear charge. C Al Na+ Ne Na Valence "N" 2 3 2 2 3 move for answer "Z" 6 13 11 10 11 Na < Al < C < Ne < Na + IE(kJ/mol) 496 578 1086 2081 4560
Slide 45 / 102 15 What is the ionization energy? A Energy change associated with the gain of an electron Answer B Amount of energy that is required to move an electron from an s to a p orbital C Measure of the attraction of an atom for electrons when in a compound D Pull of the neutrons on the electrons E Amount of energy required to remove an electron from an atom or ion
Slide 45 (Answer) / 102 15 What is the ionization energy? A Energy change associated with the gain of an electron Answer E B Amount of energy that is required to move an electron from an s to a p orbital C Measure of the attraction of an atom for electrons when in a compound [This object is a pull tab] D Pull of the neutrons on the electrons E Amount of energy required to remove an electron from an atom or ion
Slide 46 / 102 16 Which of the following would NOT influence the ionization energy? A The shielding from core electrons B The extent to which an orbital is full Answer C The nuclear charge D The number of principal energy levels between the valence electrons and the nucleus E All of these influence the ionization energy
Slide 46 (Answer) / 102 16 Which of the following would NOT influence the ionization energy? A The shielding from core electrons B The extent to which an orbital is full Answer E C The nuclear charge D The number of principal energy levels between the valence electrons and the nucleus [This object is a pull tab] E All of these influence the ionization energy
Slide 47 / 102 17 Which of the following elements would be expected to have a higher ionization energy than magnesium (Mg)? A Al B Ca Answer C Na D K E B
Slide 47 (Answer) / 102 17 Which of the following elements would be expected to have a higher ionization energy than magnesium (Mg)? A Al B Ca Answer E C Na D K E B [This object is a pull tab]
Slide 48 / 102 18 Which of the following correctly ranks the elements below in order of decreasing ionization energy? A Ne > O > N B Ne > N > O Answer C H > He > Ne D Li > Mg > Ga E Zn > Ga > Br
Slide 48 (Answer) / 102 18 Which of the following correctly ranks the elements below in order of decreasing ionization energy? A Ne > O > N B Ne > N > O Answer B C H > He > Ne D Li > Mg > Ga E Zn > Ga > Br [This object is a pull tab]
Slide 49 / 102 19 Which of the following elements best fits the data provided below? A Li Ionization Ionization Energy 1st: X + IE --> X + + e- 900 kJ/mol B C 2nd: X + + IE --> X 2+ + e- 1757 kJ/mol C Be 3rd: X 2+ + IE --> X 3+ + e- 14,850 kJ/mol D Ne Answer E O
Slide 50 / 102 20 Which of the following pairs are correct in terms of relative first ionization energy and why? A O 2- < Ne , due to smaller nuclear charge on oxide ion B Li > Na , due to increased shielding in the Na atom C Zn > Cu , due to a higher nuclear charge in zinc Answer D Cl > S , due to the smaller nuclear charge in sulfur E All of these
Slide 50 (Answer) / 102 20 Which of the following pairs are correct in terms of relative first ionization energy and why? A O 2- < Ne , due to smaller nuclear charge on oxide ion B Li > Na , due to increased shielding in the Na atom C Zn > Cu , due to a higher nuclear charge in zinc Answer E D Cl > S , due to the smaller nuclear charge in sulfur E All of these [This object is a pull tab]
Slide 51 / 102 21 The second ionization energy will always be higher than the first. True False Answer
Slide 51 (Answer) / 102 21 The second ionization energy will always be higher than the first. True False Answer TRUE [This object is a pull tab]
Slide 52 / 102 22 _________ have the lowest first ionization energies of the groups listed. Alkali metals A Transition elements B Halogens C Answer Alkaline eath metals D Noble gases E
Slide 52 (Answer) / 102 22 _________ have the lowest first ionization energies of the groups listed. Alkali metals A Transition elements B Halogens C Answer A Alkaline eath metals D Noble gases E [This object is a pull tab]
Slide 53 / 102 23 Of the choices below, which gives the order for decreasing first ionization energies? Cl > S > Al > Ar > Si A Ar > Cl > S > Si > Al B Answer Al > Si > S > Cl > Ar C Cl > S > Al > Si > Ar D S > Si > Cl > Al > Ar E
Slide 53 (Answer) / 102 23 Of the choices below, which gives the order for decreasing first ionization energies? Cl > S > Al > Ar > Si A Ar > Cl > S > Si > Al B Answer B Al > Si > S > Cl > Ar C Cl > S > Al > Si > Ar D S > Si > Cl > Al > Ar E [This object is a pull tab]
Slide 54 / 102 Ionization Energy and PES Ionization energy data can be determined from PES (photoelectron spectroscopy). Recall that PES looks at the energy of light required to remove electrons from an atom. Each orbital appears as a peak on the spectrum. Intensity Be (1s) Be (2s) Li (2s) Li (1s) binding energy The PES spectrum clearly shows that the core electrons require the most energy to remove. It also shows that Be has a higher 1st IE for the removal of the valence electrons than does Li. This is expected as Be has a higher "Z".
Slide 55 / 102 Ionization Energy and PES Let's interpret another PES spectra, this one of nitrogen and oxygen. O (2p) O (1s) O (2s) Intensity N (1s) N (2p) N (2s) binding energy Why is the N (2p) peak greater than the O (2p) peak? N has a half-full "p" orbital increasing the ionization energy move for answer Why is the N(2s) peak less than the O (2s) peak? O has the higher nuclear charge move for answer
Slide 56 / 102 Ionization Energy and PES Click to go to an interactive PES spectra database and answer the questions. Why is the binding energy of the electrons greater in He than H? move for answer Similar shielding but greater "Z" Which peak in the Li spectra represents the valence electrons? move for answer Peak with lower binding energy Why is the valence peak binding energy less in Li than in H? move for answer Increased shielding due to core 1s electrons, lessens coulombic force Why is the core peak (1s) binding energy greater in Li than in H? Lithium has a higher nuclear charge "Z" so higher coulombic attractions move for answer
Slide 57 / 102 24 The following PES spectrum shows the valence "p" orbital peaks for Si and for C. Which of the following would be TRUE? Intensity Answer binding energy A The Si peak is of lower energy due to it's higher nuclear charge B The Si peak is of higher energy due to the increased shielding from core electrons C The Si peak is of lower energy due to the increased shielding from core electrons D The Si peak is of higher energy due to its higher nuclear charge
Slide 57 (Answer) / 102 24 The following PES spectrum shows the valence "p" orbital peaks for Si and for C. Which of the following would be TRUE? Intensity Answer C binding energy A The Si peak is of lower energy due to it's higher nuclear charge B The Si peak is of higher energy due to the increased shielding from core electrons [This object is a pull tab] C The Si peak is of lower energy due to the increased shielding from core electrons D The Si peak is of higher energy due to its higher nuclear charge
Slide 58 / 102 25 The 3s peak for magnesium should have a higher binding energy than that of the 4s peak in calcium due to calcium's higher amount of shielding by core electrons? True False Answer
Slide 58 (Answer) / 102 25 The 3s peak for magnesium should have a higher binding energy than that of the 4s peak in calcium due to calcium's higher amount of shielding by core electrons? True False Answer TRUE [This object is a pull tab]
Slide 59 / 102 26 Below is an actual PES spectrum of palladium (Pd). Which of the following would be TRUE? (Note: the outer 5s and 4d peaks are not shown) 3d Answer 3s 3p 4s 4p A Compared to Pd, the 3d peak in Cd would be found to the left of the 3d Pd peak B Compared to Pd, the 3d peak in Rb would be of a higher binding energy due to lower nuclear charge C Compared to Pd, the 3p peak in Kr should be found to the left of the 3p peak in Pd
Slide 59 (Answer) / 102 26 Below is an actual PES spectrum of palladium (Pd). Which of the following would be TRUE? (Note: the outer 5s and 4d peaks are not shown) 3d Answer 3s 3p 4s 4p A A Compared to Pd, the 3d peak in Cd would be found to the left of the 3d Pd peak [This object is a pull tab] B Compared to Pd, the 3d peak in Rb would be of a higher binding energy due to lower nuclear charge C Compared to Pd, the 3p peak in Kr should be found to the left of the 3p peak in Pd
Slide 60 / 102 27 Based on the PES data below, what would be TRUE regarding atoms 1 and 2? 2 1 Answer 28.6 39.6 Intensity Intensity 10 10 100 100 1.40 1.09 2.45 1.72 0 0 Binding Energy Binding Energy 10 10 I. Atom 1 has a smaller atomic radii II. Atom 2 has a larger first ionization energy III. Both atoms are in the same period IV. Both atoms are in the same group C 1 and III only B II and III only A I only E I, II, III, and IV D II and IV only
Slide 60 (Answer) / 102 27 Based on the PES data below, what would be TRUE regarding atoms 1 and 2? 2 1 Answer 28.6 39.6 Intensity Intensity B 10 10 100 100 1.40 1.09 2.45 1.72 0 0 Binding Energy Binding Energy 10 10 I. Atom 1 has a smaller atomic radii II. Atom 2 has a larger first ionization energy [This object is a pull tab] III. Both atoms are in the same period IV. Both atoms are in the same group C 1 and III only B II and III only A I only E I, II, III, and IV D II and IV only
Slide 61 / 102 Ionization Energy and Metallic Character Metals are generally described as being able to lose electrons readily which promotes conductivity. Since metals lose electrons easily, they must have low ionization energies compared to non-metals. 1st Ionization Element Metal or Non-metal Energy (kJ/mol) Na metal 496 O non-metal 1314
Slide 62 / 102 Ionization Energy and Metallic Character We can predict, based on ionization energies, where the metals and non-metals are on the periodic table. semi-metals or metalloids Notice that an element becomes more metallic as the shielding increases and as the nuclear charge - for a given level of shielding - decreases.
Slide 63 / 102 Ionization Energy and Metallic Character Let's answer a few questions regarding metallic character. C 1. Why is lead considered a metal and carbon a non-metal Si despite being in the same group? Ge Sn Pb has much more shielding due Pb to more levels of core electrons move for answer thereby causing it's electrons to be lost far more easily than that of C.
Slide 64 / 102 Ionization Energy and Metallic Character Let's answer a few questions regarding metallic character. 2. Which metal would we expect to be a Cu better conductor of electricity? Ag or Cu Ag Ag due to the higher amount of shielding, causing it to ionize more easily, thereby move for answer creating mobile electrons.
Slide 65 / 102 Ionization Energy and Metallic Character Application: Elements of Life The most common elements in living things are C,H,N,O,P, and S. Interestingly, these are all non-metals. Serotonin - brain In order to form large hormone stable, yet complex, molecules, the elements must not be able to lose electrons easily. Interestingly, all metal atoms found in living things are in their 2+ 2+ ionic form (Mg 2+ , Ca 2+ , Zn 2+ , etc.)
Slide 66 / 102 28 Which of the following is the LEAST metallic of those below? A F B At Answer C Ne D Xe E Ba
Slide 66 (Answer) / 102 28 Which of the following is the LEAST metallic of those below? A F B At Answer C Ne C D Xe E Ba [This object is a pull tab]
Slide 67 / 102 29 Which of the following would be TRUE? A The higher the ionization energy, the less metallic an element will be Answer B The lower the ionization energy, the less metallic an element will be C For a given amount of core electron shielding, the higher the nuclear charge, the more metallic an element will be D Both A and C E Both B and C
Slide 67 (Answer) / 102 29 Which of the following would be TRUE? A The higher the ionization energy, the less metallic an element will be Answer A B The lower the ionization energy, the less metallic an element will be C For a given amount of core electron shielding, the higher the nuclear charge, the more metallic an [This object is a pull tab] element will be D Both A and C E Both B and C
Slide 68 / 102 30 Which of the following has the elements correctly ordered by increasing metallic character? A Li < Be < B Answer B Ca < K < Ga C Ga < Ca < K D Rb < Cs < As E Ga < As < Ba
Slide 68 (Answer) / 102 30 Which of the following has the elements correctly ordered by increasing metallic character? A Li < Be < B Answer B Ca < K < Ga C C Ga < Ca < K D Rb < Cs < As [This object is a pull tab] E Ga < As < Ba
Slide 69 / 102 Ionization Energy and Light As we have seen, EM radiation can provide the necessary energy to ionize an electron from an atom. e- photon The higher the ionization energy, the higher the frequency of light needed to ionize the electron.
Slide 70 / 102 Ionization Energy and Light Which of the following elements would require the shortest wavelength to lose an electron? Si C N Short wavelength means high energy so this would be the element with the largest ionization energy. Si C N "N" 3 2 2 move for answer "Z" 14 6 8 N has similar shielding as carbon but a higher nuclear charge so it would require the shortest wavelength to ionize an electron.
Slide 71 / 102 Ionization Energy and Light What would be the necessary wavelength required to remove one of Neon's outermost p electrons? 1. Look up 1st IE of Neon = 2081 kJ/mol 2. Convert to kJ/atom = 2081 kJ x 1 mol = 3.46 x 10 -21 kJ mol 6.022 x 10 23 atoms 3. Convert to J = 3.46 x 10 -18 J move for answer 4. Convert to v via E=h v --> v = E/h = 3.46 x 10 -18 J = 5.2 x 10 15 1/s 6.3 x 10-34 J*s 5. Convert to wavelength via v = c --> = c/ v 3 x 10 8 m*s = 5.77 x 10 -8 m = 57.7 nm 5.2 x 10 15 s
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