Answer
Balanced nuclear equation:
$^{16}_{8} O + ^{16}_{8} O --\gt ^{28}_{14}Si+ ^4_{2}He$
Work Step by Step
1. Write the incomplete reaction:
- The atomic number for "O" is: 8 (See periodic table)
- As the exercise describes, 2 $^{16}_8O$ collide, and one of the products is an $\alpha$ particle $(^4_2He)$. And there must be a missing product.
$^{16}_{8} O + ^{16}_{8} O --\gt ? + ^4_{2}He$
2. Calculate the mass number of the missing atom.
- The sum of the mass numbers on the right side must be equal to that on the left side.
$16 + 16 = ? + 4$
$32 = ? + 4$
$32 - 4 = ?$
$28 = ?$
3. Calculate the atomic number of the missing atom.
- The sum of the atomic numbers on the right side must be equal to that on the left side.
$8 + 8 = ? + 2$
$16 = ? + 2$
$16 - 2 = ?$
$14 = ?$
4. Identify the symbol of the element with atomic number equal to 14 (Use a periodic table):
- It is "Si".
5. Write the symbol with the atomic and mass numbers, and write the complete nuclear equation:
$^{28}_{14}Si$
$^{16}_{8} O + ^{16}_{8} O --\gt ^{28}_{14}Si+ ^4_{2}He$
