Periodic-Trends-Lab

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Central Piedmont Community College *

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INORGANIC

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Chemistry

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Dec 6, 2023

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pdf

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1. Examine atomic radius, electronegativity, and first ionization energy of elements. 2. Create scatter plots of atomic radius, electronegativity, and 1 st ionization energy with atomic number 3. Discover periodic and group trends for these properties. Using your textbook or Internet, define the following terms IN YOUR OWN WORDS . a) Electronegativity: Electronegativity is a measure of the tendency of an atom to attract a bonding pair of electrons in a covalent bond. b) Atomic Radius: Size of an atom c) Ionization Energy: Amount of energy required to remove an electron from an atom d) Period: Horizontal row of elements e) Group: Vertical column of elements 1. Go to PTable.com and use the interactive Periodic Table to complete the lab. (Alternate PT https://www.rsc.org/periodic-table/trends ) 2. Create a data table in Excel. You may copy and paste the one I have provided. Enter the data described in Steps 3. a If you do not have Excel on your personal computer, you can access it through the CPCC Cloud . Log in using your school username and password. https://cloudgw.cpcc.edu/ 3. Record the atomic radius, electronegativity, and first ionization energy into your data table. For each property, click on the corresponding box on the left hand side of the interactive periodic table to see the values populate on the table. 4. Fill in the Noble Gas Electron Configuration for each element in the table. 5. Create a graph for Atomic Radius vs. Atomic Number . Follow the directions below to plot the graph. Video help for creating a scatter plot : https://www.youtube.com/watch?v=MfEAEmdFOBo a) On the Excel spreadsheet highlight the numbers in columns for Atomic Number and Atomic Radius b) Choose Insert --- Chart c) Choose scatter plot. – Choose the bottom right one- scatter with straight lines and markers d) Click on the Layout Tab and Chart Title. Label your first graph: Atomic Radius vs. Atomic Number e) Click on the Axis Titles and label the Vertical Axis: Atomic Radius (picometers) and horizontal axis: Atomic Number f) Click on Gridlines and turn on major gridlines for both horizontal and vertical. g) Copy and paste the graph in a word document or google doc. 6. Create a graph for Electronegativity vs. Atomic Number . Save the graph in the same Word/Google document.

7. Create a graph for 1 st Ionization Energy vs. Atomic Number . Save the graph in the same Word/Google document. 8. Include your first and last name at the top of the page and answer the analysis questions listed below. Recreate (copy/paste) this data table in Excel or Google Sheets Table 1: Properties of Elements Atomic Number Element Atomic Radius (pm) 1 st Ionization Energy (kJ/mol) Electronegativity (Pauling) Noble Gas Electron Configuration. 1 H 190 1312 2.20 1s^2 2 He 31 2372.3 N/A 1s^2 3 Li 167 520.2 0.98 1s^2 2s^1 4 Be 112 899.5 1.57 1s^2s^2 5 B 87 800.6 2.04 1s^2s^2p^1 6 C 67 1086.5 2.55 1s^2 2s^22p^2 7 N 56 1402.3 3.04 2s2 2p3 8 O 48 1313.9 3.44 2s2 2p4 9 F 42 1681 3.98 2s2 2p5 10 Ne 38 2080.7 N/A 1s2 2s2 2p 11 Na 190 495.8 0.93 3s1 12 Mg 145 737.7 1.31 3s2 13 Al 118 577.5 1.61 3s2 3p1 14 Si 111 786.5 1.90 3s2 3p2 15 P 98 1011.8 2.19 3s2 3p3 16 S 88 999.6 2.58 3s2 3p4 17 Cl 79 1251.2 3.16 3s2 3p5 18 Ar 71 1520.6 N/A 3s2 3p6 19 K 243 418.8 0.82 4s1 20 Ca 194 589.8 1.0 4s2 21 Sc 184 633.1 1.36 4s2 3d1 22 Ti 156 589.4 1.62 3d2 4s2 23 V 171 650.9 1.63 2s2 2p2 24 Cr 166 652.9 1.66 3d5 4s1 25 Mn 161 717.3 1.55 3d5 4s2 26 Fe 156 762.5 1.83 3d6 4s2 27 Co 152 760.4 1.88 3d7 4s2 28 Ni 149 737.1 1.91 3d8 4s2 29 Cu 145 745.5 1.90 3d10 4s1 30 Zn 142 906.4 1.65 3d10 4s2 31 Ga 136 578.8 1.81 3d10 4s2 4p1 32 Ge 125 762 2.01 3d10 4s2 4p2 33 As 11.4 947.0 2.18 1s2 2s2 2p6 3s1 34 Se 103 941 2.55 3d10 4s2 4p4 35 Br 94 1139.9 2.96 3d10 4s2 4p5 36 Kr 88 1350.8 3.0 3d10 4s2 4p6

1. Atomic Radius vs. Atomic number. Label the peaks and valleys with the symbol or name of the element. Under the graph answer the following questions in complete sentences. a) Summarize trends for atomic radius across a period (left to right) and down a group (top to bottom). The atomic radius generally decreases. For example, from left to right in the given data, the atomic radius decreases from H to Ne.The atomic radius generally increases. For instance, from top to bottom, the atomic radius increases from Li to Kr. b) Why does the atomic radius increase/decrease as you move from left to right across a period? The atomic radius decreases as you move from left to right across a period because electrons are added to the same energy level, but the increasing positive charge in the nucleus pulls the electrons closer, making the atomic radius smaller. c) Why does the atomic radius increase/decrease as you move from top to bottom down a group? The atomic radius increases as you move down a group because electrons are added to higher energy levels, making the electron cloud larger and the atomic radius bigger.

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2. Electronegativity vs. Atomic number . Label the peaks and valleys with the symbol or name of the element. Under the graph answer the following questions in complete sentences. a) Summarize trends for electronegativity across a period (left to right) and down a group (top to bottom). Electronegativity generally increases across a period. This means that from left to right, elements tend to attract electrons more strongly. The peak electronegativity is typically reached for the elements on the right side of the period. Electronegativity generally decreases as you move down a group. This implies that elements at the top of a group have a higher tendency to attract electrons compared to those at the bottom. b) Why does the electronegativity increase/decrease as you move from left to right across a period? As you move from left to right across a period, the atomic number increases, and the number of protons in the nucleus increases.The increased positive charge in the nucleus exerts a stronger pull on electrons, leading to higher electronegativity. c) Why does the electronegativity increase/decrease as you move from top to bottom down a group? electronegativity decreases as you move down a group because the outermost electrons are located in higher energy levels.Electrons in higher energy levels are farther from the nucleus and experience a weaker attractive force, resulting in lower electronegativity.

3. 1 st Ionization Energy vs. Atomic number . Label the peaks and valleys with the symbol or name of the element. Under the graph answer the following questions in complete sentences. a) Summarize trends for 1 st Ionization Energy across a period (left to right) and down a group (top to bottom). The 1st ionization energy generally increases across a period, meaning it requires more energy to remove the outermost electron. Elements on the right side of a period have higher 1st ionization energies. The 1st ionization energy generally decreases as you move down a group, indicating that it is easier to remove the outermost electron.Elements at the bottom of a group have lower 1st ionization energies. b) Why does the 1 st Ionization Energy increase/decrease as you move from left to right across a period? As you move from left to right across a period, the atomic number increases, and the number of protons in the nucleus increases. The increased positive charge in the nucleus exerts a stronger pull on electrons, making it more difficult to remove the outermost electron, thus increasing the 1st ionization energy. Additionally, across a period, the number of electron shells remains the same, so the outer electrons are not shielded from the increasing nuclear charge. c) Why does the 1 st Ionization Energy increase/decrease as you move from top to bottom down a group? The 1st ionization energy decreases as you move down a group because the outermost electrons are located in higher energy levels. Electrons in higher energy levels are farther from the nucleus and

experience a weaker attractive force, making them easier to remove. The increasing number of electron shells also contributes to shielding, reducing the effective nuclear charge felt by outer electrons. 4. Analyze the noble gas configurations for the elements in each main group (excluding transition metals). Describe the similarities and differences for the configurations in any group. (answer on pg 3 if space allows) 5. Fit one graph and associated questions per page (3 pages total). Include your first and last name at the top of the first page and save as a PDF to submit on Brightspace.

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