Unit 1 Review - Practice KEY PDF

Name: __________________________________________ Date: __________ Period: _____ Unit 1 Review Atomic Structure (protons, neutrons, electrons, average atomic mass) 1. Fill out the table below by choosing the correct answer Suba...

Name: __________________________________________ Date: __________ Period: _____ Unit 1 Review Atomic Structure (protons, neutrons, electrons, average atomic mass) 1. Fill out the table below by choosing the correct answer Subatomic particle Mass Charge Location Protons Small / Large + / - / neutral Nucleus / energy levels Electrons Small / Large + / - / neutral Nucleus / energy levels Neutrons Small / Large + / - / neutral Nucleus / energy levels 2. Describe how you use the numbers of protons, neutrons, and electrons to determine the the following a. Mass number: p + n b. Charge: p - e c. Atomic number: p 3. Sketch the following atom, labeling where each type of particle is located: 3 protons, 4 neutrons, and 2 electrons Li 1+ 4. Complete the following table Symbol Atomic number Mass number charge Protons Neutrons Electrons 25 12 Mg 12 25 0 12 13 12 Be 4 9 0 4 5 4 15 8 O2- 8 15 2- 8 7 10 23 11 Na+ 11 23 1+ 11 12 10 Mg-24 12 24 0 12 12 12 5. From the table above, identify all ions. What makes them ions? Oxygen and Sodium are ions. An ion is an atom or molecule with a net electrical charge. (Note: #p = #e is neutral) 6. From the table above, identify two rows that represent different isotopes of the same element. Explain what they share in common and what is different about them that makes them isotopes. Magnesium has two isotopes. Isotopes are atoms of the same element with different numbers of neutrons (and therefore different mass numbers) 7. Silicon has 3 isotopes - Si-28, Si-29, Si-30. If 92.23% is Si-28, 4.67% is Si-29, and 3.10% is Si-30, calculate the average atomic mass of silicon. Show your work. (28 * 0.9223) + (29 * 0.0467) + (30 * 0.0310) = 28.109 amu 8. There are 3 stable isotopes of potassium, K-39, K-40, and K-41. Given that the average atomic mass of potassium is 39.1amu, which isotope is the most abundant? K - 39 Electrons, Energy Levels, and Light 1. What is the relationship between wavelength and frequency? (when wavelength is large, frequency is ____) When wavelength is large, frequency is low. When wavelength is short, frequency is high. 2. What is the relationship between energy and frequency? When frequency is high, energy is high. When frequency is low, energy is low. 3. Which has higher frequency: Violet light or red light? (circle one) 4. Which has a longer wavelength: orange light or green light? (circle one) 5. Which has greater energy: a photon of yellow light or a photon of red light? (circle one) 6. Which has greater energy: violet light or orange light? (circle one) Emission spectra, energy levels 7. How does an electron move when it releases energy?From higher energy level to lower energy level (From excited state to ground state) 8. How does an electron move when it absorbs energy?From lower energy level to higher energy level (From ground state to excited state) Refer to the diagram to the right: 9. Which electron transition will emit light with the highest frequency? a) n=6 to n=2 b) n=2 to n=5 c) n=4 to n=2 d) n=3 to n=2 10. Which electron transition will absorb light with the highest energy? b) n=6 to n=2 b) n=2 to n=5 c) n=4 to n=2 d) n=3 to n=2 Electron configuration - Energy levels, sublevels, and orbitals 1. How many electrons can be held in one orbital of the 5d sublevel? 2 2. How many total electrons can be held by the 4s sublevel?2 3. How many total electrons can be held by the 4p sublevel? 6 4. How many total electrons can be held by the 4d sublevel? 10 5. How many orbitals are in a p-sublevel? 3  6. Which sublevels are there on the 3rd energy level? S, p, d 7. Write the full and abbreviated electron configurations in the table below Element Full electron configuration Abbreviated electron configuration Mn 1s2 2s2 2p6 3s2 3p6 4s2 3d5 [Ar] 4s2 3d5 Zr 1s2 2s2 2p6 3s2 3p6 4s2 3d10 4p6 5s2 4d2 [Kr] 5s2 4d2 8. Draw the orbital diagram (boxes/lines and arrows) for the electron configuration of nitrogen. 9. Identify the element represented by the following: Electron configuration Element 1s22s22p63s2 Mg 1s22s22p63s23p64s23d104p3 As 1s1 H 10. Identify on the periodic table the s-block, p-block, d-block and f-block 11. Write the orbital notation for the following atoms. Problem 1 is solved for you as an example (Note: REMEMBER that “p” has 3 orbitals; “d” has 5 orbitals; “f” has 7 orbitals…draw the available orbitals first) Element Orbital notation Mg Sr 1s2 2s2 2p6 3s2 3p6 4s2 3d10 4p6 5s2 Ge Mo Ca Ba 12. Explain the rule that is being violated in the following electron configurations Orbital notation Error identified 2 p electrons sharing orbital while others are empty S orbital has to fill before p 3s electrons should have opposite spin 4s orbital is missing.