Question

name: ____ teacher: __ date: ____ q1 chemistry: u2l2 the atomic symbol 12. which of the atoms/ions below have the same number of protons but different numbers of neutrons? a. a & e (b) b & c & d (c) d & h (d) c & f prepwork part 2: isotopes directions: read the passage below. as you read, annotate the important information and vocabulary words. then answer the questions. part 1: read & annotate: what are isotopes? atoms of the same element all have the same number of protons, which is what defines them as that element. however, atoms of the same element can have different numbers of neutrons. these variations are called isotopes. isotopes of the same element have the same chemical properties because they have the same number of protons and electrons, but they have different atomic masses due to the difference in neutrons. for example, carbon has three naturally occurring isotopes: - carbon-12 (6 protons, 6 neutrons) - carbon-13 (6 protons, 7 neutrons) - carbon-14 (6 protons, 8 neutrons) isotopic notation is a shorthand way to show the mass number (protons + neutrons), the atomic number (protons) and the chemical symbol. it can be written in two main ways: - nuclear symbol notation: ( ^{14}_6\text{c} ) → mass number = 14, atomic number = 6 - hyphen notation: carbon-14 🖊️ part 2: short answer questions 1. what do all isotopes of an element have in common? _____________ 2. *what differences exist between isotopes of the same element? _____________ 3: an atom is written as ( ^{35}_{17}\text{cl} ). how many protons, neutrons, and electrons does it have? _______________

Explanation:

Part 2: Short answer questions

1. What do all isotopes of an element have in common?

From the passage, it states that atoms of the same element (isotopes) have the same number of protons (defining the element) and same number of electrons (for neutral atoms), and same chemical properties. The key commonality for isotopes is the number of protons (atomic number) and electrons (in neutral state), and same chemical properties. But the core defining commonality from the text is the same number of protons (and electrons, and chemical properties).

The passage says isotopes of the same element can have different numbers of neutrons, leading to different atomic masses (since atomic mass ≈ protons + neutrons).

Step 1: Find number of protons

The atomic number (bottom number) in nuclear notation is the number of protons. For $^{35}_{17}\text{Cl}$, atomic number = 17, so protons = 17.

Step 2: Find number of neutrons

Mass number (top number) = protons + neutrons. So neutrons = mass number - protons = $35 - 17 = 18$.

Step 3: Find number of electrons

For a neutral atom, number of electrons = number of protons. Since this is a neutral Cl atom, electrons = 17.

Answer:

All isotopes of an element have the same number of protons (atomic number), the same number of electrons (in neutral atoms), and the same chemical properties.

2. What differences exist between isotopes of the same element?