Question

1. define an isotope.
2. what would happen if the number of protons were to change in an atom?
3. another way to write isotopes is to write the name of the element then add the mass number after a dash, for example, $_{6}^{14}c$ is carbon - 14. why isnt the atomic number needed for this notation?
4. here are three isotopes of an element: $_{6}^{12}c$ $_{6}^{13}c$ $_{6}^{14}c$

a. the element is:
b. the number 6 refers to the
c. the numbers 12, 13, and 14 refer to the
d. how many protons and neutrons are in the first isotope?
e. how many protons and neutrons are in the second isotope?
f. how many protons and neutrons are in the third isotope?

Explanation:

• Question 1: Isotopes are atoms of the same element that have the same number of protons but different numbers of neutrons.
• Question 2: If the number of protons in an atom changes, it becomes an atom of a different element.
• Question 3: The atomic number is not needed in the notation because the element's name already indicates the atomic number.
• Question 4a: The element is carbon.
• Question 4b: The number 6 refers to the atomic number.
• Question 4c: The numbers 12, 13, and 14 refer to the mass number.
• Question 4d: In the first isotope (\(^{12}_{6}\text{C}\)), the number of protons is 6 (equal to the atomic number), and the number of neutrons is \(12 - 6=6\).
• Question 4e: In the second isotope (\(^{13}_{6}\text{C}\)), the number of protons is 6, and the number of neutrons is \(13 - 6 = 7\).
• Question 4f: In the third isotope (\(^{14}_{6}\text{C}\)), the number of protons is 6, and the number of neutrons is \(14 - 6=8\).

Answer:

1. Atoms of the same element with different neutron numbers.
2. It becomes a different element.
3. Element name implies atomic number.

4.

• a. Carbon
• b. Atomic number
• c. Mass number
• d. Protons: 6, Neutrons: 6
• e. Protons: 6, Neutrons: 7
• f. Protons: 6, Neutrons: 8