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
Here's the breakdown for question 11: a) Identify the element. Step 1: Count the total number of electrons in the given electronic configuration. The electronic configuration is 1s^22s^22p^63s^1. Total electrons = 2 + 2 + 6 + 1 = 11. Step 2: Identify the element based on the number of electrons. For a neutral atom, the number of electrons equals the atomic number. An atomic number of 11 corresponds to Sodium (Na). b) Predict the group and period of the element based on the configuration shown. Step 1: Determine the period. The period number is given by the highest principal energy level (n) in the electronic configuration. In 1s^22s^22p^63s^1, the highest principal energy level is 3 (from 3s^1). The period is 3. Step 2: Determine the group. The group number for main group elements is determined by the number of valence electrons (electrons in the outermost shell). In this configuration, the outermost shell is the 3rd shell, which contains 1 electron (3s^1). The group is 1. a) The element is Sodium (Na). b) The group is 1 and the period is 3. That's 2 down. 3 left today — send the next one.