potassium-a metal that catches fire whet it reacts with water,
chlorine-a green poisonous gas
bromine-a reddish brown liquid
lithium-the least reactive of the alkali metals
neon-an nonreactive gas
iron-a metal with very high melting point
I am not certain what the question is.
Bromine: when cool, it is a liquid. Check its boiling point.
Iron: depends on what you mean by "high" mp. "High" is not a very specific term. If I were describing iron, I would focus on malleability, tensile strength, ability to form strong alloys.
well i meant to ask if they are correct, because i had to match them
Potassium metal does NOT catch fire when added to water. The reaction with water is
2K + 2H2O ==> H2 + 2KOH
The reaction is vigorous and it is exothermic. I think it's the hydrogen gas (not K metal) that catches fire.
DrBob222 is wrong.potassium burns with lilac flame when react with water.(of cuz if the reaction is too small,lilac flame is difficult to be observed)
Potassium is a metal that catches fire when it reacts with water. This reaction is highly exothermic, meaning it releases a large amount of heat. To understand why this happens, let's look at the atomic structure of potassium.
Potassium (K) has an atomic number of 19, which means it has 19 protons and 19 electrons. The electrons in an atom are arranged in energy levels or shells. The outermost shell of potassium contains one electron. This electron is relatively far from the positively charged nucleus of the atom, making it easy to remove.
When potassium reacts with water, the electrons in the outer shell are easily lost, creating a potassium ion (K+). The ion is attracted to the negative part of the water molecule, which is the oxygen atom. The resulting reaction releases energy in the form of heat and produces potassium hydroxide (KOH) and hydrogen gas (H2). The heat generated during this reaction is sufficient to ignite the hydrogen gas, causing the potassium to catch fire.
Chlorine, on the other hand, is a green poisonous gas. It is an element found in Group 17 of the periodic table, also known as the halogens. Chlorine (Cl) has atomic number 17. Its electron configuration places it in need of one additional electron to complete its outer shell. To achieve this stable electron configuration, chlorine readily accepts an electron from another atom, becoming a negatively charged chloride ion (Cl-).
Due to its strong electronegativity, chlorine can form compounds with other elements by gaining electrons. Its reactivity makes it toxic to many living organisms, which is why it is often used as a disinfectant for water treatment and swimming pools.
Moving on to bromine, it is a reddish-brown liquid. Like chlorine, bromine (Br) is also a halogen. It has atomic number 35, and its electron configuration is similar to chlorine. Bromine is highly reactive and toxic, primarily because it readily accepts electrons to complete its outer shell. Its liquid state is due to its relatively low boiling point, which is around 59 °C (138 °F). Below this temperature, bromine exists as a reddish-brown liquid, but it can also evaporate to form a toxic reddish-brown gas.
Now, let's discuss lithium. It is the least reactive of the alkali metals. Lithium (Li) is an element found in Group 1 of the periodic table. It has atomic number 3 and is known for its low density and high reactivity compared to other metals. However, among the alkali metals (Group 1 elements), lithium exhibits the least reactivity.
The reactivity of alkali metals is due to their tendency to lose an electron from their outer shell to achieve a stable configuration. Lithium possesses a single electron in its outer shell, making it relatively easier to remove compared to the other alkali metals. Despite being the least reactive, lithium still reacts vigorously with water and oxygen, producing lithium hydroxide (LiOH) and lithium oxide (Li2O), respectively.
Moving on to neon, it is a nonreactive gas. Neon (Ne) is an element found in Group 18 of the periodic table, known as the noble gases. These gases have full outer electron shells, making them stable and nonreactive. Neon, with atomic number 10, has a complete octet in its outer shell, meaning it has eight electrons in that shell. Due to its electron configuration, neon is chemically inert and does not readily form compounds or react with other elements.
Lastly, iron is a metal with a very high melting point. It is a transition metal with atomic number 26. Iron (Fe) is known for its characteristic properties, including its high melting point, which is around 1,538 °C (2,800 °F). The high melting point of iron is attributed to its metallic bonding. In a metallic bond, the valence electrons of the metal atoms are delocalized, meaning they are not associated with any specific atom and can move freely throughout the metal lattice. This electron mobility and the resulting strong attraction between positive metal ions and the delocalized electrons contribute to the high melting point of iron.