**Alpha decay** is a type of radioactive decay where an unstable atom emits an alpha particle. To solve **alpha decay equations**, follow these steps:

- Identify the element and its atomic mass and atomic number given in the problem.
- Determine the type of radioactive decay.
- Write the element with the atomic mass and atomic number on the left side of the equation.
- Write the alpha particle on the right side of the equation.
- Balance the equation by ensuring the total atomic mass and atomic number on the left side are equal to the sum of the atomic mass and atomic number on the right side.
- Subtract the mass of the alpha particle from the original element’s mass to find the new atomic mass.
- Subtract the charge of the alpha particle from the atomic number of the original element to find the new atomic number.
- Use the periodic table to find the element with the new atomic number.

### Key Takeaways:

**Understanding alpha decay equations**is essential for studying radioactive decay.- Follow a step-by-step process to solve
**alpha decay equations**. - Balance the equation to ensure conservation of atomic mass and atomic number.
- Subtract the mass and charge of the particle to find the new atomic mass and atomic number.
- Refer to the periodic table to identify the new element.

## Writing Typical Radioactive Decay Equations

When it comes to writing typical **radioactive decay equations**, there are some key steps to follow. First, identify the element, its atomic mass, and atomic number given in the problem. This information will help you accurately represent the initial state of the atom undergoing decay.

Next, determine the type of radioactive decay. There are different types such as **alpha decay** and **beta decay**, each with its own unique characteristics. This information is crucial in understanding the particles involved in the decay process.

Once you have identified the type of radioactive decay, you can write the equation. Start by writing the element with its atomic mass and atomic number on the left side of the equation. Then, represent the particle involved in the decay on the right side. It is important to balance the equation by ensuring that the total atomic mass and atomic number are equal on both sides.

To find the new atomic mass and atomic number, subtract the mass and charge of the particle from the original element. Finally, you can use the periodic table to find the element with the new atomic number.

### Example:

Let’s consider an example of

alpha decay equation for Radium-226. Radium-226 has an atomic mass of 226 and an atomic number of 88. Thealpha decayequation is written as{ }. By balancing the equation, we add the new element Radon-222 (_{88}^{226}Ra → { }_{2}^{4}α{ }) on the right side. The complete nuclear reaction equation becomes_{86}^{222}Rn{ }._{88}^{226}Ra → { }_{2}^{4}α + { }_{86}^{222}Rn

### Summary:

Writing typical **radioactive decay equations** involves identifying the element and its atomic properties, determining the type of decay, writing the equation, balancing it, and finding the new atomic properties. By following these steps, you can accurately represent the process of **nuclear decay** and understand the changes occurring in the atomic structure.

## Example 1: Alpha Decay Equation for Radium-226

Let’s practice writing a typical alpha decay equation using Radium-226 as an example. Radium-226 has an atomic mass of 226 and an atomic number of 88. Alpha decay is the type of decay it undergoes. We write the equation as *${ }_{88}^{226}Ra \rightarrow { }_{2}^{4}\alpha$*. To balance the equation, we add the new element on the right side, which is Radon-222 (*${ }_{86}^{222}Rn$*). The resulting complete nuclear reaction equation is *${ }_{88}^{226}Ra \rightarrow { }_{2}^{4}\alpha + { }_{86}^{222}Rn$*.

### Alpha Decay Equation for Radium-226

Reactant | Product |
---|---|

${ }_{88}^{226}Ra$ | ${ }_{2}^{4}\alpha$ |

Radon-222 (${ }_{86}^{222}Rn$) |

From the table above, we can see that Radium-226 (${ }_{88}^{226}Ra$) undergoes alpha decay, resulting in the formation of an alpha particle (${ }_{2}^{4}\alpha$) and Radon-222 (${ }_{86}^{222}Rn$). The alpha particle is composed of two protons and two neutrons, making it a helium-4 nucleus. This reaction is representative of the alpha decay process, where an unstable nucleus emits an alpha particle to become more stable.

Understanding and being able to write **alpha decay equations** is crucial in nuclear chemistry. By following the steps outlined earlier, you can successfully write alpha decay equations for various elements. It is essential to recognize the specific type of decay and balance the equation to ensure the conservation of atomic mass and atomic number on both sides of the reaction. Alpha decay equations help us understand the fundamental processes involved in radioactive decay and provide insights into the behavior of different elements.

Now that we have explored an example of an **alpha decay equation for Radium-226**, let’s move on to another example of a different type of radioactive decay.

## Example 2: Beta Decay Equation for Carbon-14

Now let’s explore an example of a **beta decay** equation using Carbon-14. For this isotope, Carbon-14, which has an atomic mass of 14 and an atomic number of 6, undergoes **beta decay**. The beta decay equation can be written as ${ }_{6}^{14}C \rightarrow { }_{-1}^{0}e $, where an electron is emitted.

To balance the equation, we need to add the new element on the right side, which is Nitrogen-14 (${ }_{7}^{14}N $). The final complete nuclear reaction equation would be ${ }_{6}^{14}C \rightarrow { }_{-1}^{0}e + { }_{7}^{14}N $.

Beta decay is an essential process in understanding nuclear reactions. By mastering the skills to write beta decay equations, you can analyze and predict the outcomes of various radioactive decays, enabling a deeper comprehension of the behavior of different isotopes.

## FAQ

### How do I solve alpha decay equations?

To solve alpha decay equations, follow these steps: 1) Identify the element and its atomic mass and atomic number given in the problem. 2) Determine the type of radioactive decay. 3) Write the element with the atomic mass and atomic number on the left side of the equation. 4) Write the alpha particle on the right side of the equation. 5) Balance the equation by ensuring the total atomic mass and atomic number on the left side are equal to the sum of the atomic mass and atomic number on the right side. Subtract the mass of the alpha particle from the original element’s mass to find the new atomic mass. Subtract the charge of the alpha particle from the atomic number of the original element to find the new atomic number. Use the periodic table to find the element with the new atomic number.

### What are the steps to write typical radioactive decay equations?

When writing typical **radioactive decay equations**, there are key steps to follow. First, identify the element, its atomic mass, and atomic number given in the problem. Then, determine the type of radioactive decay, such as alpha or beta decay. Write the element with its atomic mass and atomic number on the left side of the equation, and the particle involved in the decay on the right side. Balance the equation by ensuring the total atomic mass and atomic number are equal on both sides. To find the new atomic mass and atomic number, subtract the mass and charge of the particle from the original element. Finally, use the periodic table to find the element with the new atomic number.

### Can you provide an example of an alpha decay equation?

Let’s practice writing a typical alpha decay equation using Radium-226 as an example. Radium-226 has an atomic mass of 226 and an atomic number of 88. Alpha decay is the type of decay it undergoes. We write the equation as ${ }_{88}^{226}Ra \rightarrow { }_{2}^{4}\alpha $. To balance the equation, we add the new element on the right side, which is Radon-222 (${ }_{86}^{222}Rn $). The resulting complete nuclear reaction equation is ${ }_{88}^{226}Ra \rightarrow { }_{2}^{4}\alpha + { }_{86}^{222}Rn $.

### How would I write a beta decay equation?

Let’s look at an example of writing a typical beta decay equation using Carbon-14. Carbon-14 has an atomic mass of 14 and an atomic number of 6. It undergoes beta decay. The equation is ${ }_{6}^{14}C \rightarrow { }_{-1}^{0}e $, where an electron is emitted. To balance the equation, we add the new element on the right side, which is Nitrogen-14 (${ }_{7}^{14}N $). The resulting complete nuclear reaction equation is ${ }_{6}^{14}C \rightarrow { }_{-1}^{0}e + { }_{7}^{14}N $.