Magnesium

To find the number of formula units in 23.2 g of magnesium chloride (MgCl₂), first calculate its molar mass: Mg (24.31 g/mol) + 2Cl (2 × 35.45 g/mol) = 95.21 g/mol. Next, determine the number of moles in 23.2 g: 23.2 g ÷ 95.21 g/mol ≈ 0.244 moles. Finally, multiply the moles by Avogadro's number (6.022 × 10²³) to find the number of formula units: 0.244 moles × 6.022 × 10²³ units/mol ≈ 1.47 × 10²³ formula units.

When a magnesium atom loses an electron from its outer energy shell, it becomes a positively charged ion, specifically a magnesium ion (Mg²⁺). This loss occurs because magnesium has two electrons in its outer shell, which it tends to lose to achieve a stable electron configuration similar to that of noble gases. As a result, the atom's reactivity increases, and it can readily bond with other elements to form compounds.

Magnesium oxide (MgO) is not typically classified as an air pollutant. It is a compound that can be produced during various industrial processes, but it is generally considered to have low toxicity and minimal environmental impact when released into the air. However, in high concentrations, fine particulate magnesium oxide could potentially affect air quality and respiratory health. Overall, its status as a pollutant depends on specific circumstances and concentrations.

The dissolution of magnesium sulfate in water is a physical process. When magnesium sulfate (MgSO₄) is added to water, it separates into its constituent ions (Mg²⁺ and SO₄²⁻) but does not undergo a chemical change; the chemical identity of the compound remains unchanged. The process is reversible, as the ions can recombine to form solid magnesium sulfate upon evaporation of the water.

The seven minerals the body needs in significant amounts to stay healthy are magnesium, phosphorus, chlorine, sulfur, calcium, potassium, and sodium. These minerals play essential roles in various bodily functions, including bone health, muscle function, and fluid balance. Adequate intake of these minerals is crucial for overall health and well-being.

The reaction of magnesium metal with air when heated is an example of a combustion reaction. During this process, magnesium reacts with oxygen to form magnesium oxide, releasing significant amounts of heat and light in the form of a bright flame. This exothermic reaction is characteristic of combustion, where a substance reacts rapidly with oxygen.

The reaction between magnesium hydroxide (Mg(OH)₂) and hydrofluoric acid (HF) can be represented by the following equation:

[ \text{Mg(OH)}_2 + 2\text{HF} \rightarrow \text{MgF}_2 + 2\text{H}_2\text{O} ]

In this reaction, magnesium hydroxide reacts with hydrofluoric acid to produce magnesium fluoride (MgF₂) and water (H₂O).

Magnesium was added to copper sulfate to initiate a chemical reaction, where magnesium displaces copper from the copper sulfate solution, forming magnesium sulfate and elemental copper. This exothermic reaction releases heat, resulting in a significant rise in temperature. The reaction is highly efficient due to magnesium's high reactivity, which contributes to the notable increase in thermal energy observed.

Magnesium itself is a metal and does not classify as an acid or alkali. However, when it reacts with acids, it can produce hydrogen gas and magnesium salts, indicating its reactivity with acidic substances. In the presence of water, magnesium oxide can form magnesium hydroxide, which is a weak alkaline solution. Thus, magnesium's behavior in chemical reactions determines its classification in relation to acids and alkalis, but it is not inherently one or the other.

Ionic bonding between magnesium and chlorine occurs when magnesium, a metal, loses two electrons to achieve a stable electron configuration, becoming a positively charged ion (Mg²⁺). Chlorine, a non-metal, gains these two electrons to form two negatively charged chloride ions (Cl⁻). The electrostatic attraction between the positively charged magnesium ions and the negatively charged chloride ions results in the formation of magnesium chloride (MgCl₂), a stable ionic compound. This transfer of electrons and subsequent attraction is the essence of the ionic bonding process.

When magnesium combines with sulfur to form magnesium sulfide (MgS), magnesium is oxidized, meaning it loses electrons. In this reaction, magnesium (Mg) has an oxidation state of 0 in its elemental form and is oxidized to Mg²⁺, while sulfur (S) is reduced from an oxidation state of 0 to S²⁻. The overall process involves the transfer of electrons from magnesium to sulfur, resulting in the formation of the ionic compound MgS.

The three stable isotopes of magnesium are magnesium-24, magnesium-25, and magnesium-26, differing in their number of neutrons. Magnesium-24 has 12 neutrons, magnesium-25 has 13 neutrons, and magnesium-26 has 14 neutrons. These differences in neutron count result in variations in their atomic mass and slight differences in their nuclear properties, but they all behave similarly chemically due to having the same number of protons. The relative abundances of these isotopes in nature also vary, with magnesium-24 being the most abundant.

To calculate the number of magnesium (Mg) atoms in 2 grams of chlorophyll, we first need to determine the molar mass of chlorophyll, which is approximately 893.49 g/mol. Since chlorophyll contains 2.68% magnesium, the mass of magnesium in 2 grams of chlorophyll is 0.0536 grams. The number of moles of magnesium is calculated by dividing the mass by its atomic mass (24.31 g/mol), resulting in approximately 0.0022 moles. Finally, multiplying by Avogadro's number (6.022 x 10²³) gives about 1.32 x 10²¹ atoms of magnesium in 2 grams of chlorophyll.

To determine the mass of hydrogen produced, we first need to identify the balanced chemical reaction between magnesium and water:

[ \text{Mg} + 2\text{H}_2\text{O} \rightarrow \text{Mg(OH)}_2 + \text{H}_2 ]

Next, we calculate the moles of magnesium (4.73 g / 24.31 g/mol = 0.194 moles) and water (1.83 g / 18.02 g/mol = 0.101 moles). Since magnesium reacts with water in a 1:2 ratio, magnesium is the limiting reactant. Therefore, 0.194 moles of magnesium will produce 0.194 moles of hydrogen gas, which corresponds to about 0.194 moles × 2 g/mol = 0.388 g of hydrogen.

Acid + a Metal = a salt + hydrogen Mg + H2SO4-----> MgSO4 + H2

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