When an element is burnt in excess oxygen, is the oxide formed always:

1. a crystalline solid
2. greater in mass than the element
3. soluble in water
4. white in color

alright, i know that most oxides are not soluble in water other than group 1 elements and calcium and barium. (correct me if i'm wrong) And not all oxides are white in color. So, what about option 1 and 2? The correct answer is 2, but i don't get it, why must the oxide formed be heavier than the element?? And what kind of oxide isn't a crystalline solid?

Help, thanks!

The oxide must have a greater mass than the element as O atoms have been added. Thus CuO must have a great mass than Cu.

For 1. I suspect that they are thinking of room temperature and pressure. Thus CO2 is a gas, H2O is a liquid.

It should be answer 3 as suppose we take magnesium and oxygen

The mass of magnesium would obviously be less than when magnesium reacts with oxygen to form magnesium oxide.
Hope this helps

Well, well, well, looks like someone is getting burned (element-wise, of course)! Let's dig into these questions and shed some humorous light on the matter!

First off, let's tackle option number one: Is the oxide formed always a crystalline solid? Well, let's just say that not all oxides are as solid as a rock! Some oxides can actually be gases, liquids, or amorphous solids. So, option one might have to take a backseat on this journey!

Next up, option number two: Is the oxide greater in mass than the element? Now, imagine this scenario. You burn an element in excess oxygen, and poof! The element magically gains weight! That would be quite the sight, but unfortunately, it's not what happens in reality. The mass of the oxide formed is not necessarily greater than that of the original element. So, selective gravitational weight gain is a no-go here!

Moving along swiftly, let's address option number three: Is the oxide soluble in water? Now, here's a fun fact for you: not all oxides are welcome in the water kingdom. A lot of them are insoluble, but a few special ones, like the group 1 elements and calcium and barium, do enjoy the water's company. So, it's safe to say that most oxides are as water-soluble as a cat trying to swim!

Last but not least, option number four: Is the oxide white in color? Ah, the color of oxides! They're like a rainbow in disguise! While it's true that some oxides appear white, not all of them are! The world of oxides can showcase all sorts of colors, from red to black to even rainbow hues. So, don't be fooled by the dazzling diversity of oxide shades!

Now, let's put all our comedic knowledge together! The correct answer is option number two, the oxide is not always greater in mass than the element. As for the oxides that aren't crystalline solids, we've discovered there are quite a few forms they can take!

I hope this humorous spin on oxides has brought a smile to your face and shed some humorous light on your questions!

When an element is burnt in excess oxygen, it undergoes a chemical reaction called oxidation, resulting in the formation of an oxide. Let's break down the different options and discuss each one:

1. Is the oxide formed always a crystalline solid?
The majority of oxides are indeed crystalline solids. This means their atoms are arranged in an organized pattern, forming a crystal lattice structure. However, there are exceptions to this rule. Some oxides, especially those with low molecular weights, may exist as gases or liquids at certain temperatures and pressures. This is the case with carbon monoxide (CO) and sulfur dioxide (SO2), which are oxides that are not crystalline solids.

2. Is the oxide formed always greater in mass than the element?
Yes, the oxide formed is generally greater in mass than the element it is derived from. This is because oxidation involves the addition of oxygen atoms to the element, which increases the overall mass. For example, when iron (Fe) reacts with oxygen (O2), it forms iron(III) oxide (Fe2O3), which is heavier than the original iron. However, it is important to note that there may be exceptions in cases where an element forms multiple oxides with different stoichiometries.

3. Is the oxide formed always soluble in water?
As you correctly mentioned, most oxides are not soluble in water. Group 1 elements (such as sodium oxide, Na2O) and some alkaline earth metals (such as calcium oxide, CaO, and barium oxide, BaO) are exceptions, as their oxides are indeed soluble in water. However, the majority of oxides, especially those of transition metals and nonmetals, are insoluble in water.

4. Is the oxide formed always white in color?
No, not all oxides are white in color. The color of an oxide depends on various factors, such as the composition and structure of the compound. While many metal oxides, such as magnesium oxide (MgO) and aluminum oxide (Al2O3), are white, there are oxides that exhibit different colors. For example, copper(I) oxide (Cu2O) is red, chromium(III) oxide (Cr2O3) is green, and iron(II) oxide (FeO) is black.

To summarize, while most oxides are crystalline solids and not soluble in water, there can be exceptions. However, the oxide formed from the burning of an element in excess oxygen is generally greater in mass than the original element because it involves the addition of oxygen atoms. The color of the oxide formed can vary depending on the specific compound.

ans 3