QuestionWhich atom can be a -1.0 ion with 13.0 electrons? (A) Al (B) Mg (C) Na (D) Si (E) P

Studdy Solution

STEP 1

Assumptions1. The ion has a charge of -1.0. The ion has13.0 electrons3. The atomic number of an atom is equal to the number of protons in its nucleus4. A neutral atom has an equal number of protons and electrons5. An ion is formed when an atom gains or loses electrons, resulting in a net charge

STEP 2

We need to find the atomic number of the ion. Since the ion has a charge of -1.0, it means it has one more electron than the number of protons. So, we can find the number of protons (which is also the atomic number) by subtracting1 from the number of electrons.
$Atomic\, number = Number\, of\, electrons - Charge$

STEP 3

Now, plug in the given values for the number of electrons and the charge to calculate the atomic number.
$Atomic\, number =13.0 - (-1.0)$

STEP 4

Calculate the atomic number.
$Atomic\, number =13.0 - (-1.0) =14.0$

STEP 5

Now that we have the atomic number, we can identify the atom. The atomic number is14, which corresponds to Silicon (Si) in the periodic table.
So, the atom that could exist as a -1.0 ion with13.0 electrons is Silicon (Si).

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