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.
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You're on a roll — Here's the solution to Question 1 (a), (b), (c), and (e) from your exam paper. Question 1 a) Complete the table above by giving the values of: i) X ii) Y iii) Z Step 1: Calculate X (Neutron number for Element A). The mass number is the sum of protons and neutrons. Mass Number = Proton number + Neutron number 35 = 17 + X X = 35 - 17 X = 18 The value of X is 18. Step 2: Calculate Y (Electron number for Element A). For a neutral atom, the number of electrons is equal to the number of protons. Electron number = Proton number Y = 17 The value of Y is 17. Step 3: Calculate Z (Mass number for Element C). The mass number is the sum of protons and neutrons. Mass Number = Proton number + Neutron number Z = 3 + 4 Z = 7 The value of Z is 7. b) Elements A and B are involved in bonding. i) Give the formula of the compound formed. Step 1: Determine the valency of Element A and Element B. Element A has 17 protons and 17 electrons (electronic configuration 2, 8, 7). It tends to gain 1 electron to form an ion with a charge of 1-. Element B has 12 protons and 12 electrons (electronic configuration 2, 8, 2). It tends to lose 2 electrons to form an ion with a charge of 2+. Step 2: Write the formula of the compound. To balance the charges, two A ions (1- each) are needed for every one B ion (2+). The formula of the compound formed is BA_2. ii) Name the type of bond involved. Element B (atomic number 12) is a metal, and Element A (atomic number 17) is a non-metal. The bond formed between a metal and a non-metal involves the transfer of electrons. The type of bond involved is ionic bond. iii) Give the electronic configuration of elements A and D. Step 1: Determine the electronic configuration for Element A. Element A has an atomic number of 17. The electronic configuration is 2, 8, 7. Step 2: Determine the electronic configuration for Element D. Element D has an atomic number of 8. The electronic configuration is 2, 6. c) To which group of the Periodic Table does elements C and D fall? Step 1: Determine the group for Element C. Element C has an atomic number of 3 (electronic configuration 2, 1). It has 1 valence electron. Element C falls in Group 1. Step 2: Determine the group for Element D. Element D has an atomic number of 8 (electronic configuration 2, 6). It has 6 valence electrons. Element D falls in Group 16 (or Group VI). e) How would element C be stored in the laboratory? Element C (atomic number 3) is an alkali metal. Alkali metals are highly reactive with air and water. Element C would be stored under oil (e.g., paraffin oil or kerosene) to prevent it from reacting with oxygen and moisture in the air. Drop the next question!