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Chapter 26: Problem 8

Calculate A nucleus has 25 protons and 30 neutrons. What is the symbol for this nucleus?

Short Answer

Expert verified
The symbol for the nucleus is \( ^{55}_{25}\text{Mn} \).

Step by step solution

01

Identify the Element

The element is identified by the number of protons it has, also known as the atomic number. For this nucleus, there are 25 protons. Refer to the periodic table to find the element with atomic number 25, which is Manganese, denoted by the symbol \( \text{Mn} \).
02

Determine the Mass Number

The mass number of a nucleus is the sum of its protons and neutrons. For this nucleus, add 25 protons + 30 neutrons = 55. So, the mass number is 55.
03

Write the Nuclear Symbol

The nuclear symbol is written as \( ^{A}_{Z}X \), where \( A \) is the mass number, \( Z \) is the atomic number (number of protons), and \( X \) is the chemical symbol. For this nucleus, it is \( ^{55}_{25}\text{Mn} \).

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Key Concepts

These are the key concepts you need to understand to accurately answer the question.

Atomic Number
The atomic number is a fundamental concept in chemistry. It tells us the number of protons present in the nucleus of an atom. Each element has a unique atomic number, making it easy to identify elements by this value.

For example:
  • The atomic number for hydrogen is 1, because it has one proton.
  • Carbon has an atomic number of 6, due to its six protons.
  • The atomic number of manganese is 25.
The atomic number is crucial because it determines the element's identity on the periodic table. This number not only differentiates one element from another but also influences the chemical properties of the element. In our original exercise, manganese was identified purely based on its atomic number of 25, which corresponds to its 25 protons.
Mass Number
The mass number tells us the total number of protons and neutrons in an atom's nucleus. Unlike the atomic number, the mass number is not unique to each element, as isotopes of an element may have different mass numbers.

To determine the mass number:
  • Add the number of protons.
  • Add the number of neutrons.
  • Combine these two values.
For manganese in the original exercise:
  • Number of protons = 25
  • Number of neutrons = 30
  • Mass number = 25 + 30 = 55
The mass number provides insight into the isotopic composition of an element, which can differ from the atomic weight usually listed on the periodic table. Understanding isotopes and their mass numbers helps in studying nuclear properties and reactions.
Periodic Table
The periodic table is an organized chart of the chemical elements, arrayed in order of increasing atomic number. It provides essential information about each element and can be used to predict chemical behavior.

Key features of the periodic table include:
  • Elements are arranged in rows (periods) and columns (groups).
  • The atomic number increases as you move from left to right.
  • Elements with similar properties are grouped together.
  • Each element's box displays its atomic number, chemical symbol, and atomic weight.
The periodic table is a fundamental tool in chemistry and helps contextualize atomic behavior and bonding. For the original exercise, the periodic table was used to identify manganese by finding element number 25. It shows not only the identity of the elements but also trends like electronegativity and atomic radius.

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Most popular questions from this chapter

Describe What happens when a particle of matter encounters its antimatter counterpart?

Identify Determine the parent nucleus when \({ }_{86}^{219} \mathrm{Rn}\) is produced by (a) alpha decay and (b) beta decay.

Identify Which type of particle is considered elementary, leptons or hadrons?

It is observed that \({ }_{28}^{66} \mathrm{Ni}\), with an atomic mass of \(65.9291 \mathrm{u}\), decays by \(\beta\) emission. (a) Identify the daughter nucleus that results from this decay. (b) If the mass of the system decreases by \(0.0002705 \mathrm{u}\) as a result of the decay, find the energy released (in \(\mathrm{MeV}\) ).

The following nuclei are observed to decay by emitting a \(\beta^{-}\)particle: (a) \({ }_{16}^{35} \mathrm{~S}\); (b) \({ }_{82}^{212} \mathrm{~Pb}\). Write the decay reaction for each of these nuclei.
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