So... this is the question which is from AP chem 2006 past paper.
Suppose that a stable element with atomic number 119, symbol Q, has been discovered.
a) write down the ground-state electron configuration of Q, showing only the valence-shell electrons.
Go to the college board website. Then go to the purple box that says student, and click on that. this willl bring up a new page. Under the box that says college board tests (near the top), click on AP. This will bring you to a new page. Go over to courses and exams, and select Chemistry as the subject. This will bring up a new page. On the sidebar, select samply questions and scoring. This will bring you to a page that has the scoring guidelines for every AP Chemistry free response exam since 2004. The first list of exams that goes farther back just has the questions, but under the scoring guidelines section you can see the answers for the questions plus explanations. Click on the 2006 Scoring Guidelines link. (Not the 2006 Form B, you have the regular one).
It will bring up a pdf that has all of the answers for 2006 AP Chemistry free response section, and how they got them. For this specific question, go down to the last page, and it will be there. I use the college board scoring guidelines for explanations for any of the recent AP Chemistry exam questions. It's a great resource for learning the material.
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To write down the ground-state electron configuration of element Q, we need to determine its position in the periodic table. Since it has an atomic number of 119, it is not a known element and does not exist in the periodic table. However, we can still determine the general pattern of electron configurations for elements and make some educated guesses.
First, let's understand the general electron configuration pattern. The electron configuration of an element is written by listing the orbitals and the number of electrons in each orbital.
The periodic table is divided into blocks: s-block, p-block, d-block, and f-block. Each block corresponds to a specific region of the periodic table where elements have similar electron configurations.
For the s-block elements (Group 1 and Group 2), the valence electrons are in the s orbital.
For the p-block elements (Groups 13 to 18), the valence electrons are in the p orbital.
For the d-block elements (transition metals), the valence electrons are in the d orbital.
For the f-block elements (inner transition metals), the valence electrons are in the f orbital.
Now, since element Q has atomic number 119, it would be located in the p-block of the periodic table (as it would be the element after Group 18).
Since it is a stable element, we can assume that it is within the main group elements (Groups 13 to 18) rather than the transition metals or inner transition metals.
Considering this information, we can write the ground-state electron configuration for element Q in the following way:
[Xe] ns^2 np^6
The [Xe] represents the electron configuration of xenon (an element in the p-block with atomic number 54). It is used to denote the filled inner shells.
The ns^2 represents the valence electrons in the outermost s orbital.
The np^6 represents the valence electrons in the outermost p orbital.
So, the ground-state electron configuration of element Q (showing only the valence-shell electrons) would be:
[Xe] ns^2 np^6
Please note that this is an educated guess based on the known patterns and rules for electron configurations. The actual ground-state electron configuration of element 119 (if it were discovered) may differ.