Question

Ammonia gas reacts with fluorine gas to form ammonium fluoride and nitrogen gas. (a) Write a balanced chemical equation for this reaction. (b) Draw a picture representing the molecular view of the reactant mixture. (c) Draw a picture representing the molecular view of the product mixture.

Short answer

(a) The balanced chemical equation is: \(2NH_3 + 4F_2 \rightarrow 2NH_4F + N_2\) (b) Reactant mixture: H | H - N - H + F - F (c) Product mixture: \( [\ H\/\/_ N - -/ | \\ H\/\/- N=N -N\/\/H / H ]^{+} \ F^- \)

Step-by-step solution

(a) Write a balanced chemical equation

To write a balanced chemical equation, first identify the reactants and products. The reactants are ammonia gas (NH3) and fluorine gas (F2), and the products are ammonium fluoride (NH4F) and nitrogen gas (N2). Next, write the chemical equation and balance the atoms on both sides. The unbalanced chemical equation is: NH3 + F2 → NH4F + N2 Now, balance the atoms on both sides: First balance nitrogen: 2NH3 + F2 → 2NH4F + N2 Then balance hydrogen and fluorine: 2NH3 + 4F2 → 2NH4F + N2 The final balanced chemical equation is: \(2NH_3 + 4F_2 \rightarrow 2NH_4F + N_2\)

(b) Molecular view of the reactant mixture

To draw the molecular view of the reactant mixture, you need to represent molecules of ammonia (NH3) and fluorine (F2). Ammonia has a trigonal pyramidal shape with a nitrogen atom (N) at the center and three hydrogen atoms (H) surrounding it. Fluorine is a diatomic molecule, consisting of two fluorine atoms (F) bonded together. Below is a simple illustration of the reactant mixture: H | H - N - H + F - F

(c) Molecular view of the product mixture

Finally, draw the molecular view of the product mixture, which consists of ammonium fluoride (NH4F) and nitrogen gas (N2). The ammonium ion (NH4+) has a tetrahedral shape with a nitrogen atom (N) surrounded by four hydrogen atoms (H). The fluoride ion (F-) is negatively charged and will be attracted to the positively charged ammonium ion. Nitrogen gas consists of two nitrogen atoms bonded together (N2). Below is a simple illustration of the product mixture: \( [\ H\/\/_ N - -/ | \\ H\/\/- N=N -N\/\/H / H ]^{+} \ F^- \) Remember that the brackets with the positive charge on the ammonium ion and the negative charge on the fluoride ion represent the ionic nature of ammonium fluoride.

Key concepts

Chemical Reactions

Understanding chemical reactions is fundamental for any aspiring chemist. Simply put, a chemical reaction is a process where reactants are transformed into products through the breaking and forming of chemical bonds. In the provided exercise, we have the reaction of ammonia gas with fluorine gas to produce ammonium fluoride and nitrogen gas. This particular type of reaction has reactants interacting to form new chemical compounds, displaying the transformative nature of chemical reactions.

To properly communicate the essence of a chemical reaction, being aware of the physical states of the reactants and products (such as gases in this case) is crucial. This information often provides hints to the conditions under which a reaction takes place, like temperature and pressure. Moreover, the colors, textures, and other qualitative attributes can offer insights into the process of the reaction which can be helpful when visualizing or conducting experiments. These reactions are not just equations on paper; they represent actual changes in the molecular structure and composition of the substances involved.

Molecular Representation

The molecular representation bridges the gap between the abstract nature of chemical formulas and the tangible world of atoms and molecules. When we depict reactants and products using structural formulas, we are essentially creating a visual map of atoms in a molecule and the bonds between them. In this exercise, for instance, drawing the molecular view of the reactant mixture involves sketching ammonia with its central nitrogen atom bonded to three hydrogen atoms, and fluorine as a pair of bonded fluorine atoms.

These visual representations are not mere doodles but have specific geometric shapes that depict the real three-dimensional arrangement of atoms in a molecule. They convey critical information about the molecule, such as its polarity and reactivity. When a student understands that the trigonal pyramidal shape of ammonia facilitates certain reactions or why diatomic molecules like fluorine are so reactive, they grasp the concepts at a deeper level. To improve comprehension, focusing on the geometry and electron distribution within these molecules can be immensely beneficial. It paints a more holistic picture rather than a collection of letters and lines.

Stoichiometry

The concept of stoichiometry is at the very heart of chemistry. It involves the quantification of the substances that participate in a chemical reaction. The exercise requires balancing of the chemical equation, which is a classic example of stoichiometry in action. It's not enough to simply list reactants and products; their ratios, based on the mole concept, are pivotal in reflecting the conservation of mass and atoms.

Understanding stoichiometry allows us to predict how much of each substance will be involved in a reaction and what amount of product will be formed. In the balanced chemical equation provided, the coefficients such as '2' for NH3 and NH4F and '4' for F2 indicate the stoichiometric ratios. These numbers show that two moles of ammonia react with four moles of fluorine to produce two moles of ammonium fluoride and one mole of nitrogen gas. By mastering stoichiometric calculations, students not only learn to balance equations but also to calculate reactant and product masses, volumes, and even energy changes during a reaction. Clear, step-by-step demonstrations of these calculations can significantly improve a student's ability to solve stoichiometry problems with confidence.