Question

Complete the table below. If necessary, use the periodic table. $$ \begin{array}{ccccc} \begin{array}{c} \text { Nuclear } \\ \text { Symbol } \end{array} & \text { Charge } & \begin{array}{c} \text { Number of } \\ \text { Protons } \end{array} & \begin{array}{c} \text { Number of } \\ \text { Neutrons } \end{array} & \begin{array}{c} \text { Number of } \\ \text { Electrons } \end{array} \\ \hline 31 \mathrm{p} & 0 & 9 & 10 & \\ \hline & 0 & & 16 & \\ \hline & +3 & 27 & 30 & \\ \hline & & & 16 & 16 & 18 \\ \hline \end{array} $$

Short answer

Question: Complete the table for the atomic species based on the given information. The complete table of atomic species is: $$ \begin{array}{ccccc} \begin{array}{c} \text { Nuclear } \\\ \text { Symbol } \end{array} & \text { Charge } & \begin{array}{c} \text { Number of } \\\ \text { Protons } \end{array} & \begin{array}{c} \text { Number of } \\\ \text { Neutrons } \end{array} & \begin{array}{c} \text { Number of } \\\ \text { Electrons } \end{array} \\\ \hline \text { } 31 \mathrm{P} & 0 & 15 & 16 & 15 \\\ \hline \text { }16 \mathrm{S} & 0 & 16 & 16 & 16 \\\ \hline \text { }60 \mathrm{Co} ^{+3} & +3 & 27 & 30 & 24 \\\ \hline \text { } 18 \mathrm{He}^{-2} & -2 & 2 & 16 & 18 \\ \hline \end{array} $$

Step-by-step solution

First Row: 31P_15

The nuclear symbol of this species is given as 31P, which means it has 15 protons and a mass number of 31. The charge is 0, which means the atom is neutral, and there are equal numbers of protons and electrons. - Number of Protons: 15 - Number of Neutrons: mass number - atomic number = $$31 - 15 = 16$$ - Number of Electrons: 15 (due to the charge being 0)

Second Row

The atomic species in this row is neutral (charge 0), but we don't have the nuclear symbol. However, we know that the number of neutrons is 16. The fact that it's neutral means the atomic number is equal to the number of electrons. - Number of Protons: 16 (assuming same as electrons due to charge 0) - Number of Neutrons: 16 - Number of Electrons: 16 - Nuclear Symbol: _16S_32

Third Row

This species has a charge of +3, 27 protons, and 30 neutrons. The charge of +3 means that there are 3 fewer electrons than protons. - Number of Protons: 27 - Number of Neutrons: 30 - Number of Electrons: $$27 - 3 = 24$$ - Nuclear Symbol: _27Co^(+3)_60

Fourth Row

In this row, we are given the number of electrons (16) and neutrons (16), and also that there are 18 total electrons. Therefore, we need to determine the charge and the number of protons. - Number of Protons: $$18 - 16 = 2$$ - Number of Neutrons: 16 - Number of Electrons: 18 - Charge: -2 (due to having two more electrons than protons) - Nuclear Symbol: _2He_18^(-2) Now the complete table is: $$ \begin{array}{ccccc} \begin{array}{c} \text { Nuclear } \\\ \text { Symbol } \end{array} & \text { Charge } & \begin{array}{c} \text { Number of } \\\ \text { Protons } \end{array} & \begin{array}{c} \text { Number of } \\\ \text { Neutrons } \end{array} & \begin{array}{c} \text { Number of } \\\ \text { Electrons } \end{array} \\\ \hline \text { } 31 \mathrm{P} & 0 & 15 & 16 & 15 \\\ \hline \text { }16 \mathrm{S} & 0 & 16 & 16 & 16 \\\ \hline \text { }60 \mathrm{Co} ^{+3} & +3 & 27 & 30 & 24 \\\ \hline \text { } 18 \mathrm{He}^{-2} & -2 & 2 & 16 & 18 \\ \hline \end{array} $$

Key concepts

Periodic Table

The periodic table is a systematic way of organizing information about the chemical elements, allowing users to understand patterns in their properties and reactivities. It consists of rows called periods and columns known as groups or families.

Elements in the same column typically share similar properties due to having the same number of electrons in their outermost shell, which is key in dictating how they react chemically. The table is designed so that elements with similar properties fall into the same column. For example, all noble gases, which are inert, are located in the far right column.

When working with nuclear symbols and isotopes, the periodic table becomes an essential tool. It provides quick access to an element's atomic number, which is the unique number of protons in the nucleus of an atom, as well as information about its average atomic mass. The periodic table's structure aids in predicting the behavior of atoms during chemical reactions and is fundamental when it comes to the study of chemistry.

Atomic Number

The atomic number is a fundamental property of an element and is denoted by the symbol 'Z'. It represents the number of protons in the nucleus of an atom of the element. Since each element has a different number of protons, the atomic number serves as an identifier for different elements. In a neutral atom, the atomic number also indicates the number of electrons surrounding the nucleus, because the charges balance each other out.

For instance, in the homework problem, when examining the nuclear symbol 31P, the 'P' represents phosphorus on the periodic table, which has an atomic number of 15. This means that phosphorus has 15 protons. Understanding the atomic number is essential when filling out the missing information in nuclear symbols and when deducing properties of isotopes.

Mass Number

The mass number, symbolized as 'A', is the total number of protons and neutrons in an atom's nucleus and gives an approximate idea of the atomic mass of that isotope in atomic mass units (amu). Unlike the atomic number, the mass number is not fixed for a given element because elements can have different isotopes. Isotopes are atoms of the same element that have the same number of protons (and hence the same atomic number) but different numbers of neutrons.

In the exercise, the mass number helps to identify the number of neutrons by subtracting the atomic number from it. For instance, with the symbol 31P, the mass number of 31 minus the atomic number of 15 protons gives us 16 neutrons. Understanding how to utilize mass numbers is crucial for comprehending the structure of isotopes and nuclear symbols.

Atomic Charge

The atomic charge indicates the electric charge of an atom, which can affect its reactivity and interactions with other atoms. It is represented by a superscript after the element symbol and mass number. A neutral atom has an equal number of protons and electrons, resulting in no overall charge. However, an atom can lose or gain electrons, becoming an ion, and therefore carry a positive or negative charge. A positive charge indicates a deficit of electrons, while a negative charge indicates an excess.

The third row of the exercise shows a species with a +3 charge and 27 protons. The +3 charge means there are three fewer electrons than protons, resulting in 24 electrons. The atomic charge is a crucial concept in understanding the properties of ions and plays a significant role in chemical reactions and bonding.