This chemistry question involves key chemical concepts and calculations. The detailed solution below walks through each step, from identifying the reaction type to computing the final answer.
ScanSolve AI Answer
Step 1: Determine the atomic number and electron configuration of Element X. From the Bohr model diagram: • First shell has 2 electrons. • Second shell has 8 electrons. • Third (outermost) shell has 7 electrons. Total number of electrons = 2 + 8 + 7 = 17. For a neutral atom, the number of electrons equals the atomic number. Therefore, the atomic number of Element X is 17. The electron configuration is 2, 8, 7. Step 2: Identify Element X and its position in the modern periodic table. The element with atomic number 17 is Chlorine (Cl). • The number of electron shells determines the period. Since Element X has 3 shells, it belongs to Period 3. • The number of valence electrons determines the group for main group elements. Since Element X has 7 valence electrons, it belongs to Group 17 (also known as Group VIIA, the Halogens). Step 3: Construct a part of the modern periodic table showing the position of Element X. Here is a section of the modern periodic table with Element X (Chlorine) highlighted: | Period | Group 16 (Chalcogens) | Group 17 (Halogens) | Group 18 (Noble Gases) | | :----- | :-------------------- | :------------------ | :--------------------- | | 2 | Oxygen (O) | Fluorine (F) | Neon (Ne) | | 3 | Sulfur (S) | Chlorine (Cl) (X) | Argon (Ar) | | 4 | Selenium (Se) | Bromine (Br) | Krypton (Kr) | The position of Element X is in Period 3, Group 17.