Question

Another possible nuclear reaction leading to the formation of element-120 is between uranium-238 and nickel-64. Write a nuclear equation for this nuclear reaction.

Short answer

The nuclear reaction between Uranium-238 and Nickel-64 leading to the formation of element-120 is expressed in the nuclear equation as \( \text{{^238_92U}} + \text{{^64_28Ni}} \rightarrow \text{{^302_120Element}} + 2\text{{^1_0n}} \).

Step-by-step solution

Understand the given

Here, uranium-238 and nickel-64 are used, so uranium (U) has an atomic number of 92 and a mass number of 238 while Nickel (Ni) has an atomic number of 28 and a mass number of 64.

Apply the conservation law

When two atomic nuclei combine, their atomic numbers and mass numbers are separately conserved. This means the sum of the atomic numbers on the left of the equation should equal the sum of atomic numbers on the right. The same applies to mass numbers.

Write the nuclear equation

Write down the elements and their atomic and mass numbers. For uranium-238 and nickel-64, following the conservation law will result: \[ \text{{Uranium-238}} + \text{{Nickel-64}} \rightarrow \text{{Element-120}} + x\] Where we need to find out what x will be.

Compute for x

By subtracting the atomic number and mass number of element-120 from the sum of the atomic numbers and mass numbers of Uranium-238 and Nickel-64 respectively, we can compute for x. This will result in two neutrons.

Finalize The Nuclear Equation

The final nuclear equation is: \[ \text{{^238_92U}} + \text{{^64_28Ni}} \rightarrow \text{{^302_120Element}} + 2\text{{^1_0n}} \]

Key concepts

Nuclear Equation

In nuclear reactions, a nuclear equation is used to represent the process of two atomic nuclei combining or splitting. These equations convey the transformation of isotopes, demonstrating changes that occur at the nuclear level. Nuclear equations involve the representation of reactants and products by their chemical symbols, along with their atomic numbers and mass numbers. A crucial aspect of writing a nuclear equation involves ensuring both the atomic numbers and mass numbers are accurately recorded, as these values indicate the identity and characteristics of the nuclei involved.
In our example, when uranium-238 and nickel-64 collide, they form a new element and release other subatomic particles. This entire process is depicted in a nuclear equation, indicating how two heavy nuclei can combine to form a heavier one. For instance, written as: \[ ext{^238_{92}U} + ext{^64_{28}Ni} \rightarrow ext{^302_{120}Element} + 2 ext{^1_0n} \]This shows that uranium-238 and nickel-64 result in a new formed element-120 and two neutrons.

Atomic Number

The atomic number is a fundamental property of each chemical element. It represents the number of protons present in the nucleus of an atom. The atomic number is denoted as the subscript preceding the chemical symbol in nuclear equations.
Understanding the atomic number is crucial because it determines the composition and identity of an element within the periodic table. It remains constant for any given element, which is why it is an essential consideration when balancing nuclear equations.
When writing a nuclear equation, we must ensure that the sum of atomic numbers on the reactant side matches the sum on the product side. As in our exercise: - Uranium has an atomic number of 92. - Nickel has an atomic number of 28. These combine to maintain balance as they form a new element with atomic number 120 and two released neutrons, which have an atomic number of zero.

Mass Number

The mass number of an atomic nucleus is another key factor in nuclear reactions. It represents the total number of protons and neutrons, collectively known as nucleons, in an atom's nucleus. In nuclear equations, mass numbers are written as superscripts preceding the chemical symbol.
Understanding and using correct mass numbers is essential for tracking conservation in nuclear reactions. It reflects the mass aspects of the transition as elements collide or split, and ensures nuclear stability.
In our given nuclear reaction: - Uranium has a mass number of 238. - Nickel has a mass number of 64. When these combine, they create a new element with a mass number calculated as 302, with two remaining neutrons each with a mass number of 1 to satisfy the mass number balance.

Conservation Law

The conservation law plays a vital role in nuclear reactions as it ensures balance and understanding of the reaction process. There are two main conservation laws in nuclear reactions: conservation of atomic number and conservation of mass number. Both assert that the sum of these numbers must remain consistent from reactants to products.
The principle is crucial because it governs the behavior of subatomic particles during nuclear transformations. By ensuring these values remain balanced, we can predict the outcome of nuclear reactions and identify unknown particles or elements.
In our example: - The conservation of atomic numbers maintains that the sum of 92 (Uranium) and 28 (Nickel) equals 120 (New Element) plus the atomic number contribution from released neutrons. - For mass numbers, the sum of 238 and 64 from reactants results must equate to the combined 302 of the new element plus the product of 2 neutrons with mass number 1 each. These laws ensure that the nuclear equation is correctly balanced, adhering to fundamental physical principles.