Using condensed electron configurations and Lewis electron-dot symbols to depict the monatomic ions formed from each of the following reactants, predict the formula of the compound the ions produce.
1) K and P
To determine the formula of the compound formed by the monatomic ions K and P, we need to first write the condensed electron configurations for each element:
1) K (Potassium): [Ar] 4s1
2) P (Phosphorus): [Ne] 3s2 3p3
Next, we need to determine the charges of the resulting monatomic ions. This can be done by looking at the group number for each element in the periodic table. The group number tells us the number of valence electrons.
1) K is in Group 1, so it has 1 valence electron. By losing this electron, it forms a +1 ion: K+1
2) P is in Group 15, so it has 5 valence electrons. By gaining 3 electrons, it forms a -3 ion: P-3
Now, we can represent the monatomic ions using Lewis electron-dot symbols:
1) K+1: The Lewis electron-dot symbol for K+1 is shown by placing the symbol "K" with a superscript "+1" and representing 1 dot (representing the lost electron) around it.
Lewis electron-dot symbol: K+1: :K:
2) P-3: The Lewis electron-dot symbol for P-3 is shown by placing the symbol "P" with a superscript "-3" and representing 5 dots (representing the 3 gained electrons) around it.
Lewis electron-dot symbol: P-3: :P:::.
Lastly, using the charges of the monatomic ions, we can determine the formula of the compound. Since the charges must balance, the number of each ion in the formula is equal to the absolute value of the other ion's charge.
The formula for the compound formed by the monatomic ions K+1 and P-3 is K3P.
To predict the formula of the compound formed by the monatomic ions of K and P, let's first determine the electron configurations and Lewis dot symbols for each of these elements.
1) K (Potassium):
The electron configuration of potassium is: 1s^2 2s^2 2p^6 3s^2 3p^6 4s^1
The condensed electron configuration for potassium is: [Ar] 4s^1
The Lewis electron-dot symbol for potassium is:
K
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2) P (Phosphorus):
The electron configuration of phosphorus is: 1s^2 2s^2 2p^6 3s^2 3p^3
The condensed electron configuration for phosphorus is: [Ne] 3s^2 3p^3
The Lewis electron-dot symbol for phosphorus is:
P
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Next, we need to consider the charges of each ion. K is in Group 1 of the periodic table, so it will lose one electron to form a positive ion with a charge of +1. P is in Group 15, so it will gain three electrons to form a negative ion with a charge of -3.
Now, let's represent the electron configuration and charge for each ion:
K+: [Ar] 4s^0
P3-: [Ne] 3s^2 3p^6
To determine the formula of the compound formed by these ions, we need to find the lowest common multiple of the charges. In this case, the lowest common multiple of +1 and -3 is 3. This means we need three K+ ions to balance the charge of one P3- ion.
The formula of the compound formed is K3P.
We can't draw Lewis structures on the boards but I think the formula you are looking for is K3P.
I will leave it for you to draw the condensed electron configuration.