Question

Write equations for the reaction of sodium with each of the halogens. Predict at least two physical properties that are common to all of the alkali metal halides.

Short answer

Sodium reacts with halogens to form sodium halides like NaF, NaCl, NaBr, and NaI. Common properties of alkali metal halides include high melting/boiling points and solubility in water.

Step-by-step solution

Understanding Halogens

The halogens are the elements in Group 17 of the periodic table, and they include fluorine (F), chlorine (Cl), bromine (Br), and iodine (I). These elements tend to form salts when they react with metals.

Write Reaction Equations

When sodium (Na) reacts with halogens, it forms sodium halides. The general equation is: \[ 2\,\text{Na} + \text{X}_2 \rightarrow 2\,\text{NaX} \] where \( \text{X} \) is any of the halogens (F, Cl, Br, I).For each halogen, the reactions are:- **Sodium with Fluorine**: \( 2\,\text{Na} + \text{F}_2 \rightarrow 2\,\text{NaF} \)- **Sodium with Chlorine**: \( 2\,\text{Na} + \text{Cl}_2 \rightarrow 2\,\text{NaCl} \)- **Sodium with Bromine**: \( 2\,\text{Na} + \text{Br}_2 \rightarrow 2\,\text{NaBr} \)- **Sodium with Iodine**: \( 2\,\text{Na} + \text{I}_2 \rightarrow 2\,\text{NaI} \)

Predict Common Physical Properties

Alkali metal halides, such as sodium halides, generally share common physical properties. 1. **High Melting and Boiling Points**: These compounds are typically ionic, which means they form solid lattices that require significant energy to break. 2. **Solubility in Water**: Alkali metal halides usually dissolve well in water, forming clear solutions.

Key concepts

Understanding Halogens

Halogens are fascinating elements that belong to Group 17 of the periodic table. This group includes well-known elements such as fluorine (F), chlorine (Cl), bromine (Br), and iodine (I). These elements are highly reactive and are known for their tendency to form salts when they react with metals. This salt-forming property is what gives halogens their name, derived from Greek words meaning "salt-producing."

Halogens are unique because they exist in various states under standard conditions:

• Fluorine and chlorine are gases.
• Bromine is a liquid.
• Iodine is a solid.

Despite their different physical states, all halogens share some common characteristics. They are all diatomic molecules, meaning they form molecules consisting of two atoms, e.g., F extsubscript{2}, Cl extsubscript{2}, Br extsubscript{2}, and I extsubscript{2}. This diatomic nature plays a significant role in the way they react with other elements, like sodium.

Alkali Metal Halides

When sodium reacts with halogens, the result is a class of compounds known as alkali metal halides. These compounds are the products of the reactions between alkali metals (like sodium) and halogens. The general equation for these reactions is \[ 2\,\text{Na} + \text{X}_2 \rightarrow 2\,\text{NaX} \]where \( \text{X} \) represents the halogen involved in the reaction.

Alkali metal halides are characterized by their ionic bonds, formed due to the transfer of electrons from the metal (sodium) to the non-metal (halogen). This electron transfer leads to the formation of ions:

• Sodium gives up an electron to become \( \text{Na}^+ \).
• The halogen gains an electron to become \( \text{X}^- \).

This ionic nature leads to several important physical properties, such as high melting and boiling points, due to the strong attraction between the ions in the solid lattice.

Sodium Reactions

Sodium, a soft and highly reactive metal from Group 1 of the periodic table, undergoes exothermic reactions with halogens to produce sodium halides. Let's look at these reactions one by one:

• When sodium reacts with fluorine, it forms sodium fluoride: \[ 2\,\text{Na} + \text{F}_2 \rightarrow 2\,\text{NaF} \]
• Sodium and chlorine form sodium chloride, commonly known as table salt: \[ 2\,\text{Na} + \text{Cl}_2 \rightarrow 2\,\text{NaCl} \]
• The reaction with bromine yields sodium bromide: \[ 2\,\text{Na} + \text{Br}_2 \rightarrow 2\,\text{NaBr} \]
• Finally, sodium reacts with iodine to produce sodium iodide: \[ 2\,\text{Na} + \text{I}_2 \rightarrow 2\,\text{NaI} \]

These reactions are typically vigorous and must be carefully controlled. They are illustrative of the reactivity differences observed across the halogens.

Periodic Table Group 17

Group 17 of the periodic table, where the halogens reside, is an intriguing column known for its reactive nonmetals. As we move down the group from fluorine to iodine, several trends are observable:

• The reactivity of the elements decreases. Fluorine is the most reactive, while iodine is the least.
• The atomic size increases, which leads to decreased electronegativity and decreased ability to attract electrons.
• The elements have relatively high electronegativities and affinities for electrons, a common trait across the group.

The chemistry of halogens is deeply influenced by these periodic trends. For example, their high electronegativities explain why they form negative ions so readily when reacting with metals. Understanding these trends is fundamental to grasping the chemical behavior of halogens.