Which of the following is a complete nuclear symbol for an element with 7 protons, 8 neutrons, and 10 electrons?(1 point)

Question

(note: ignore the line to the left of the symbol that is between the 2 numbers for all
the answers)
14
7 𝑁
3 − N
14
7
3−
15
7 𝑁
15 3 −
7 N 3−
14
7
14 N 𝑁 2 −
7
2−
N
15
7
+

Answer 1

To determine the correct complete nuclear symbol for an element with 7 protons, 8 neutrons, and 10 electrons, we need to analyze the information:

1. Element Identification: The atomic number, which is the number of protons, is 7. This corresponds to the element nitrogen (N).

2. Mass Number Calculation: The mass number is the sum of protons and neutrons. Here, the mass number is: \[ \text{Mass Number} = \text{Protons} + \text{Neutrons} = 7 + 8 = 15 \]

3. Charge Calculation: The element has 7 protons (positive charge) and 10 electrons (negative charge). The overall charge is: \[ \text{Charge} = \text{Protons} - \text{Electrons} = 7 - 10 = -3 \] Therefore, the ion has a charge of 3−.

Now, we can represent the complete nuclear symbol in the standard format, which is: \[ \text{Mass Number} , , \text{Element Symbol} , \text{Charge} \] So in this case, the complete nuclear symbol for the element is: \[ ^{15}_{7}N^{3-} \]

Among the options you provided, the correct representation of this is:

• \( 15 , 7 , N , 3− \)

Thus, the correct answer is: 15 \( _7 \) N \(^{3-}\).