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Chapter 16: Problem 6

Suppose \({ }_{14}^{35} \mathrm{Si}\) undergoes beta emission. Write a nuclear reaction for this spontaneous change.

Short Answer

Expert verified
The balanced nuclear equation for the beta emission of \({}_{14}^{35}\text{Si}\) is: \({}_{14}^{35}\text{Si} \to {}_{15}^{35}\text{P} + {}_{-1}^{0}\text{e}\)

Step by step solution

01

Identify the new element

When a neutron converts into a proton during beta emission, the atomic number (number of protons) of the nucleus increases by 1. In the case of \({}_{14}^{35}\text{Si}\), the atomic number is initially 14. After beta emission, the atomic number will be 15. We can use the periodic table to find that the element with an atomic number of 15 is Phosphorus (P). Step 2: Balance the nuclear equation
02

Balance the nuclear equation

In a balanced nuclear equation, the sum of atomic numbers (subscripts) and mass numbers (superscripts) on the left side of the equation must equal the sum on the right side. For beta emission, an electron is released, which is represented by \({}_{-1}^{0}\text{e}\). The mass number of the electron is 0, and its atomic number is -1. Now we can balance the nuclear equation for beta emission: \({}_{14}^{35}\text{Si} \to {}_{15}^{35}\text{P} + {}_{-1}^{0}\text{e}\) So, the balanced nuclear equation for the beta emission of \({}_{14}^{35}\text{Si}\) is: \({}_{14}^{35}\text{Si} \to {}_{15}^{35}\text{P} + {}_{-1}^{0}\text{e}\)

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Most popular questions from this chapter

Discuss the benefits and problems associated with using nuclear fission to produce electricity.

Which has the larger binding energy per mole of nucleons, \({ }_{2}^{4}\) He (molar mass \(4.00150 \mathrm{~g} / \mathrm{mol}\) ) or \({ }_{3}^{6} \mathrm{Li}\) (molar mass \(6.01348 \mathrm{~g} / \mathrm{mol}\) )? [Useful masses: proton, \(1.00730 \mathrm{~g} / \mathrm{mol}\); neutron, \(1.00870 \mathrm{~g} / \mathrm{mol} ;\) electron, \(0.00055 \mathrm{~g} / \mathrm{mol}]\)

Positron emission moves us one step to the left in the periodic table, and alpha emission moves us two steps to the left. Does this mean that, for a given parent isotope, the daughter isotope resulting from two successive positron emissions is the same as the daughter isotope resulting from one alpha emission?

Complete this nuclear reaction, and name the decay process: \({ }_{4}^{8} \mathrm{Be}+? \rightarrow{ }_{3}^{8} \mathrm{Li}\)

The tantalum isotope \({ }_{73}^{186} \mathrm{Ta}\) is radioactive and decays by converting a neutron to a proton. (a) Where is this atom likely to lie in the band of stability? (b) Write a nuclear reaction for this decay process. (c) Which type of decay is this?
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