Name Date Period Unit 3 Review: Electrons and the periodic table G Chem; Coleman SHOW YOUR WORK ON ANY AND ALL CALCULATIONS. SIG FIGS MATTER. UNITS MATTER. General Questions: 1. Use the following terms (electron, energy level, excited, jumps, falls, photons, energy) to describe how an electron emits light. a) When is the electron absorbing energy? b) When is the electron releasing energy? c) What is an electron s ground state? d) What is an electron s excited state? Objective #1: I can explain the atomic emission spectrum of an element using Bohr s Model of the atom. 1. What is an atomic spectrum? Using the image below, answer the questions: 2. Which of the arrow represents electrons emitting light? 3. Which of the arrows represent electrons absorbing energy? 4. Which of the electrons emitting light would emit the lowest energy of light? Why?
Objective #2: I can use atomic emission spectra to identify an element. 1. What elements is star A composed of? 2. What elements is star B composed of? Objective 3: I can use flame tests to identify an element. 1. an unidentified poison burns blue when a sample is held in a flame. What element does it likely contain? 2. What elements would you use if you wanted to design a firework that had the colors purple, yellow and bright red? 3. What color do copper containing compounds emit when they are heated?
Objective 4: I can explain flame test emissions in terms of electron behavior. R----------------------------------------------------------------V 1. Which of the lines in the above emission spectrum is caused by electrons making the largest jump in energy levels? 2. Why does boron give a specific atomic spectrum that is different than any other atom s spectrum? Objective #5: I can calculate the frequency of a wavelength of electromagnetic radiation using c=λν, where c=speed of light = 3.00x 108m/s Objective #10: I can use the electromagnetic spectrum to identify types of light. 1. What is the frequency of a wave that has a wavelength of 4 x 10-4 m. a. What type of light is this? 2. What is the wavelength of light with a frequency of 6.22 x 1018 Hz? a. What type of light is this? Objective # 6: I can explain the relationship between wavelength, frequency and energy. 1. What happens to the frequency of a wave when its wavelength increases? 2. What happens to the energy of a wave when its frequency increases? a. What happens to the energy of a wave when its wavelength decreases? Objective #7: I can define a photon 1. What is a photon? 2. What does it mean to say that photons are quantized? Objective # 11: I can compare the different properties of light of different types of light. 1. What has more energy a red photon or a blue photon? 2. What moves faster, x-rays or infrared radiation? 3. What has a larger wavelength, ultraviolet or microwaves? 4. What has a smaller frequency, radio waves or visible light?
Objective #12: I can calculate the energy of a photon using E=hν where h=planck s constant= 6.63 x 10-34J-s 1. What is the frequency of light with a wavelength of 5.7 x 10-7 m? 2. What color of visible light is this? 3. What is the energy of light with a frequency of 2.0 x 1020 Hz? 4. What type of light is this? Objective # 13: I can describe the quantum model of the atom: 1. What is an orbital? 2. What makes and orbital different than an orbit? 3. What makes the quantum model different than Bohr s model? 4. What are the names of the sublevels? 5. How many orbitals are in each of the types of sublevels? 6. How many electrons are in an orbital? 7. Draw an s and a p orbital below: Objective #14: I can write the electron configuration and the orbital notation for any element on the periodic table. Objective #15: I can apply the Aufbau principle, Pauli Exclsion principle, and Hund s rule to write electron configurations and orbital diagrams. 1. Write the complete electron configuration and orbital notation for the following atoms F Ru As Ca Sb 2. What do the different parts of the notation 3p5 mean?
3. Which rules (Aufbau, Pauli Exclusion or Hund s) is being violated below? Objective #16: I can describe the origins of the modern periodic table. 1. The periodic table is arranged by increasing. Objective #17: I can describe the organization of the periodic table (periods, groups) and categorize elements as halogens, alkali metals, alkaline earth metals, noble gases, and transition metals: 1. Label the families by name (halogens, alkali metals, alkaline earth metals, noble gases, and transition metals) 2. What is a period? How many are there on the periodic table? a. What do elements in a period have in common? 3. What is a family (group)? How many are there on the PT? a. What do elements in a family have in common? 4. Which group of elements has the most similar properties? Why? Al, Si, P Ca, Rb, Na F, Cl, I Objective #18: I can contrast physical and chemical properties of metals, non-metals and metalloids and locate them on the periodic table. 1. Mark the line on the Periodic table above that separates the metals from the non-metals. 2. What class of elements are the following? Ca Po I Si 3. What are the properties of metals? 4. What are the properties of non-metals?
5. What are the properties of metalloids? 6. A substance is malleable, conducts electricity and heat, doesn t react with acid and is dull. What class of element is this? How do you know? 7. How do you know that a spoon is made of a metal? (give properties that prove it). Objective #19: I can explain the relationship between the electron configurations of an element, its position on the periodic table, and its chemical properties. 1. What is the electron configuration for Calcium? 2. How many valence electrons does it have? 3. What family is it in? 4. How does the electron configuration correlate to the family that it is in? Objective #20: I can state the trends of properties (atomic radius, electronegativity, ionization energy, and electron affinity) 1. What are the trends in atomic radius, ionization energy, electronegativity, and electron affinity as you Property Trend across a period Trend down a family Atomic radius Ionization energy Electronegativity Electron affinity Objective #21: I can interpret the trend shown by atomic radii, electronegativities, electron affinity, and ionization energies within the periodic table. 1. Why aren t noble gases included in electronegativity trends? 2. Why does Barium (Ba) have a larger radius than Beryllium (Be)? 3. Why does Lithium (Li) have a smaller ionization energy than Rubidium (Rb)? 4. Why does fluorine (F) have a higher electronegativity than carbon (C)? 5. Why does sulfur (S) have a lower electron affinity than Oxygen (O)?