Question

Ionization energy of sodium is same as that of (a) Electronegativity of \(\mathrm{Na}^{+}\) (b) Electron affinity of Ne (c) Ionisation energy of \(\mathrm{Mg}\) (d) Electron affinity of \(\mathrm{Na}^{+}\)

Short answer

The ionization energy of sodium is not the same as any given options.

Step-by-step solution

Understanding Ionization Energy

Ionization energy is the amount of energy required to remove an electron from an atom or ion in its gaseous state. For sodium (Na), this process involves removing the outermost electron, converting it into \( Na^+ \). Its ionization energy is relatively low due to its position in the periodic table.

Analyzing Electronegativity of Na⁺

Electronegativity refers to an atom's ability to attract electrons in a chemical bond. Since \( Na^+ \) is a positive ion, it does not seek to attract electrons as much as neutral atoms would. Therefore, its electronegativity is generally low or undefined.

Understanding Electron Affinity of Ne

Electron affinity is the amount of energy released when an electron is added to an atom in the gas phase. Neon (Ne), a noble gas, has a full valence shell and does not readily accept additional electrons, resulting in very low or positive electron affinity values.

Comparing Ionization Energies

Sodium (Na) and magnesium (Mg) are adjacent elements on the periodic table. However, magnesium, which is in group 2, has a higher ionization energy than sodium, which is in group 1, due to its higher nuclear charge.

Understanding Electron Affinity of Na⁺

The electron affinity of \( Na^+ \) would involve adding an electron to a positively charged ion to form neutral sodium, essentially a reverse process to the electron removal in ionization energy. This process for \( Na^+ \) does not measure the same energy as the ionization energy of neutral sodium.

Key concepts

Electronegativity

Electronegativity is an important chemical property that describes how strongly an atom can attract and hold onto electrons in a chemical bond. It helps explain why certain elements form bonds in specific ways.
- A positive ion, such as \( Na^+ \), typically has low electronegativity. This is because it is already deficient in electrons and is not in a strong position to attract more.
- Electronegative values are more typically assigned to neutral atoms rather than ions like \( Na^+ \).
When comparing atoms across the periodic table, elements like fluorine have extremely high electronegativity values. This makes them very effective at attracting electrons from other atoms. Understanding electronegativity helps explain molecular bonding and reactivity in chemistry.

Electron Affinity

Electron affinity measures the amount of energy released when an electron is added to an isolated atom in its gaseous state, leading to the formation of a negative ion. It is a key concept in understanding how elements interact with electrons.
- Neon (Ne), a noble gas, has very low or even positive electron affinity. This is because it already has a full outer shell of electrons, making it energetically unfavorable to add more.
- Elements that release energy when gaining an electron have negative electron affinity values, indicating that the process is exothermic. In contrast, noble gases tend to resist gaining electrons.
Electron affinity is useful in predicting the behavior of atoms in chemical reactions, especially regarding energy changes when forming ions.

Periodic Table

The periodic table is a comprehensive chart that organizes elements based on increasing atomic number and recurring chemical properties. It is an essential tool in chemistry, providing insight into the behavior of elements.
- Elements are arranged in rows called periods and columns called groups or families. Similarities in properties occur within groups due to common electron configurations.
- Sodium (Na) and magnesium (Mg) are neighbors on the periodic table. Magnesium, being in group 2 (alkaline earth metals), has a higher ionization energy than sodium from group 1 (alkali metals) due to its higher nuclear charge.
Understanding the layout of the periodic table helps in predicting the properties of elements and their potential reactions, making it a crucial framework for learning chemistry.