CH 101 1st Edition Lecture 5Outline of Current Lecture I. The Original Theories of the AtomII. Memorizing the Periodic Table III. Using the Periodic Table to find the ChargeA. AnionB. CationIV. Introduction to Elements and LightCurrent LectureI. Light wavesA. How to Calculate the Wavelength and the FrequencyII. The Bohr ModelA. Absorbing energyB. Emitting energyIII. Recap of Important EquationsCurrent LectureI. Light – A form of energy known as electromagnetic radiation and exists as a wave. Depending on the frequency of the light wave, it will appear as different colors. These 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.Wavelength – The distance between crests in a wave. One wavelength looks like out of awave that looks like . Wavelength is ALWAYS measured in meters and is represented by the symbol (λ). Frequency – How many waves pass a given point in one second. The frequency is represented asthe symbol (ν). Frequency is inversely related to the wavelength, the longer the wavelength the lower the frequency and the shorter the wavelength the higher the frequency. The speed of light is c = 3.0x108 m/s. When calculating the frequency, check your answer by checking the exponent because frequencies are usually to the 14, for example 7.3x1014 is a possible frequency whereas 3.15x10-23 it not. The unit for frequency is s-1- To find the Frequency or the wavelength of a wave, use the equation c = λν (λ = Wavelength) (ν = Frequency) (c = speed of light 3.00x108 m/s)- In many questions the wavelength will be in nm when it should be in meters. The conversion between nm and m is m = 109 nm.Ex) Find the frequency of a wave with a wavelength of 700 nm.c = λν = v = c / λ Rearrange the equation so that you’re solving for frequency 700 nm = 109 m / 1 nm = 0.0000007 m <- Convert nanometers to metersv = 3.00x108 / 0.0000007 m = 4.3x1014 s-1Plug in the numbers given and you get 4.3x1014 s-1Wave Energy – The energy of light is directly proportional to the frequency of its wave. Wave energy is represented by the equation E = hν (E = Energy in Joules) (h = Plank’s constant 6.626x10-34 J(seconds)) (ν = frequency (s-1)). An easy way to check if you have found the right amount of energy is to look at the exponent. Energy is normally to the -19, so if you get an answer that looks like E = 1.07x1035 J, it is definitely not right. Ex) If the energy per photon is 3.17x10-19 J, find the energy per 1 mole of photons resulting in the units (kJ / mol).The wording may sound tricky but all the question is asking is for you to convert J to kJ and multiply by Avogadro’s number. 3.17x10-19 J = 1 kJ / 1000 J <- There are 1000 Joules in 1 kJ so divide by 10003.17x10-19 J = 1 kJ / 1000 J = 6.02x1023 / 1 mol = 191 kJ / mol <- Multiply by Avogadro’s number to get kilojoules per mol.- Different types of waves are determined by the wavelength or the frequency. The highest energy wave is a gamma ray. Gamma rays have a high frequency and a short wavelength. From highest energy to lowest energy the different types of waves are inthis order: Gamma, X-ray, UV, Visible, Infrared, Micro, and Radio. Also, waves with longer wavelengths are more of a red color and waves with shorter wavelengths have a bluish color. *Fun fact, this is why the sunset in the morning is red orange, it’s because the light waves with the longest wavelength can travel faster than those with short wavelengths therefore lighting up the sky before the blue light waves can get there.Hydrogen Atom Line Spectra – When light is shown through a tube of hydrogen, certain colors appear because the electrons jump to different energy levels, these colors are violet, blue, indigo, and red. The frequencies of these colors are red = 4.57x1014 s-1, indigo = 6.17x1014 s-1, blue = 6.91x1014 s-1, and violet = 7.31x1014 s-1. A scientist by the name of Rydberg developed an equation that can gives you the frequency when an atom jumps energy levels by using the hydrogen atom line spectra. In his equation (h = Plank’s constant 6.626x10-34 Js), (R = Rydberg’s constant 3.29x1015 s-1), (n2(low) = The lowest energy level), and (n2(high) = The highest energy level).- The Rydberg equation -> Etransition = ( hR / n2(low)) - ( hR / n2(high)) Ex) What is the change in energy for the n = 3 to n = 4 transition?E = ((6.626x10-34)( 3.29x1015) / (3)2) – ((6.626x10-34)( 3.29x1015) / (4)2) <- Plug into the equationE = (2.42x10-19) – (1.36x10-19) <- Solve for the total energy of each energy level, then subtract them to find the change in energyE = 1.05x10-19 <- Total change in energy for the n = 3 to n = 4 transition. II. The Bohr Model – The Bohr model was created when electrons were thought to act as particles, the model have many different levels that all very in distance from the nucleus with n = 1 being the closest to the nucleus and having the lowest energy. The jump between n = 1 and n = 2 is always going to be greater than the distance between any of the other energy levels. The equation Elevel = - Z2 hR / n2 gives you the energy of the electron in the Bohr model. In this equation (Z = the atomic number of the atom), (h = Plank’s constant), (R = Rydberg’s constant) (n = the energy level). This equation is only used when an atom has one electron in the outer shell such as the ion O7+.- Energy levels on the Bohr model are shown as:Ex) What is the energy of the electron in the ion He1+ if it is in the n = 3 energy level?E = - Z2 hR / n2 <- Plug into the equationE = - ((2)2 (6.626x10-34)( 3.29x1015)) / (3)2 <- Solve and don’t forget the negative sign in front of the equationE = -9.68x10-19 J <- Answer, make sure it’s in Joules A. Absorbing energy- When an electron jumps to a higher energy level is absorbing and increasing energy. If an electron jumps from n = 1 to n = 2, it is absorbing energy. When asked to find the highest or the lowest energy absorption transition remember that the lower the energy levels, the farther the jump. Ex) Determine the highest energy absorption. A) n = 2 to n = 5 B) n = 5 to n = 4 C) n = 1 to n = 3Start by knowing that the jump from n = 1 to n = 2 is larger than the jump from n = 2 to any higher energy level.The answer is C) n = 1 to n = 3 because the jump contains the lowest energy levels meaning thatit had to jump farther