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Chapter 3: Problem 7

Give the full atomic symbol for an atom that has 16 neutrons and an atomic number of 15 .

Short Answer

Expert verified
\[_{15}^{31}\textrm{P}\]

Step by step solution

01

Identify the chemical element

Using the periodic table, find the element with an atomic number of 15. The atomic number represents the number of protons in the atom. In this case, the element with atomic number 15 is phosphorus (P).
02

Determine the mass number

The mass number is the sum of protons and neutrons in the atom. Here, we are given that there are 16 neutrons in the atom. Since the atomic number is 15 (which is the number of protons), we can calculate the mass number as follows: Mass Number = Number of Protons + Number of Neutrons Mass Number = 15 (protons) + 16 (neutrons) = 31
03

Write the atomic symbol

Now that we have identified the chemical element as phosphorus (P) and determined its mass number as 31, we can write the full atomic symbol using the standard notation: \[_{15}^{31}\textrm{P}\] This is the full atomic symbol for an atom with 16 neutrons and an atomic number of 15, which represents phosphorus-31.

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Most popular questions from this chapter

Fill in the following table for four neutral atoms: $$ \begin{array}{lcccc} & { }_{8}^{15} \mathrm{O} & ? & ? & ? \\ \hline \text { Mass number } & ? & 16 & 37 & ? \\ \text { Atomic number } & ? & 8 & ? & ? \\ \text { Number of protons } & ? & ? & ? & ? \\ \text { Number of neutrons } & ? & ? & ? & 12 \\ \text { Number of electrons } & ? & ? & 17 & 11 \\ \hline \end{array} $$

Suppose \(12.0 \mathrm{~g}\) of silicon (Si) reacts with \(70.0 \mathrm{~g}\) of oxygen \(\left(\mathrm{O}_{2}\right)\) to give \(25.6 \mathrm{~g}\) of the compound silicon dioxide \(\left(\mathrm{SiO}_{2}\right) .\) In the process, all the silicon gets used up, but some oxygen is left over. (a) For the law of conservation of matter to be obeyed, how much oxygen is unused? (b) What is the percent \(\mathrm{Si}\) in \(\mathrm{SiO}_{2} ?\) (c) What is the percent \(\mathrm{O}\) in \(\mathrm{SiO}_{2}\) ?

Regarding problem \(3.137\), do you think an atom's second ionization energy would be smaller, the same, or larger than its first ionization energy? Do you think the second ionization energy for an atom would ever be less than the first? Explain.

What is so special about the mass number and atomic mass of \({ }_{6}^{12} \mathrm{C}\) ?

Of the atoms \(\mathrm{Na}, \mathrm{Mg}\), and \(\mathrm{K}\), which should be the most difficult to ionize? Which has the smallest first ionization energy?
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