Question

Write a chemical equation representing the first ionization energy for lithium. use e− as the symbol for an electron.

Answer 1

$\boxed{{\text{Li}} \to {\text{L}}{{\text{i}}^ + } + {{\text{e}}^ - }}$ is the chemical equation that represents the first ionization energy of lithium.

Further Explanation:

Ionization energy is the amount of energy that is required to remove the most loosely bound valence electrons from the isolated neutral gaseous atom. It is denoted by IE. The value of IE is related to the ease of removing the outermost valence electrons. If these electrons are removed so easily, small ionization energy is required and vice-versa. It is inversely proportional to the size of the atom.

Ionization energy is further represented as first ionization, second ionization and so on. When the first electron is removed from a neutral, isolated gaseous atom, the energy needed for the purpose is known as the first ionization energy, written as  ${\text{I}}{{\text{E}}_{\text{1}}}$. Similarly, when the second electron is removed from the positively charged species (cation), the ionization energy is called the second ionization energy $\left( {{\text{I}}{{\text{E}}_2}} \right)$ and so on.

The atomic number of lithium is 3. So its electronic configuration is $1{s^2}2{s^1}$. Its outermost electron is present in 2s orbital. The amount of energy required to remove this electron of lithium atom is known as the first ionization energy of lithium.

The equation that represents the first ionization of lithium is ${\text{Li}} \to {\text{L}}{{\text{i}}^ + } + {{\text{e}}^ - }$.

Learn more:

1. The subatomic particle with the least mass: brainly.com/question/2224691

2. Number of carbon atoms in 1.3-carat diamond: brainly.com/question/4235993

Answer details:

Grade: Senior School

Subject: Chemistry

Chapter: Periodic classification of elements

Keywords: first ionization energy, lithium, electronic configuration, atomic number, electron, neutral, isolated, gaseous atom, IE1., equation, size of the atom.

Answer 2

The chemical equation representing the first ionization energy for lithium is given by;

Li → Li + e-

Further Explanation;

Ionization energy

• Ionization energy is the energy required to remove outermost electrons from the outermost energy level. Energy is required to remove an electron from an atom.
• The closer an electron is to the nucleus the more energy is required, since the electron is more tightly bound to the atom thus making it more difficult to remove, hence higher ionization energy.
• Ionization energy increases across the periods and decreases down the group from top to bottom.  
• Additionally, the ionization energy increases with subsequent removal of a second or a third electron.

First ionization energy  

• This is the energy required to remove the first electron from the outermost energy level of an atom.
• Energy needed to remove the second electron to form a divalent cation is called the second ionization energy.

Trends in ionization energy  

1. Down the group(top to bottom)

• Ionization energy decreases down the groups in the periodic table from top to bottom.
• It is because as you move down the group the number of energy levels increases making the outermost electrons get further from the nucleus reducing the strength of attraction to the nucleus.
• This means less energy will be required compared to an atoms of elements at the top of the groups.

2. Across the period  (left to right)

• Ionization energy increases across the period from left to right.
• This can be explained by an increase in nuclear energy as extra protons are added to the nucleus across the period increasing the strength of attraction of electrons to the nucleus.
• Consequently, more energy is needed to remove electrons from the nucleus.

Keywords: Ionization energy, periodic table, energy levels, electrons

Learn more about

• Ionization energy: brainly.com/question/1971327
• Trend in ionization energy: brainly.com/question/1971327
• First ionization energy: brainly.com/question/1971327

Level: High school  

Subject: Chemistry  

Topic: Periodic table and chemical families  

Sub-topic: Ionization energy