Answer:
<h2>Ionic</h2><h3>
Evidence: It can be proved by a simple experiment, sand doesn't dissolve in water but NaCl (table salt) does. (excluding cases like BaSO4 and sugar and amino acids)</h3>
Cause: The electrostatic bonds among ions in a lattice only hold them together like two magnets with unlike poles facing each other. The water molecules can split them through the similar process with several molecules ganging up on them, the H+ parts of the molecules attracts the anion and O2- part; the cations. If this electrostatic attraction is big enough, the bonds between the solid's ions break (into separate ions). And so the solid dissolves. This is usually the case with most.
Why not covalent structures?: Sure, covalent solids have a low m.p and b.p for low inter<em>molecular </em>forces, the covalent bonds here are strong and cannot easily be 'pulled apart' by water molecules. They usually have stronger inter<em>molecular </em>forces than that of water.
But... if their inter<em>molecular </em>forces are weaker or similar, sure they can dissolve easily. Like any often-used alcohol (glacial).
B - Sediment . Many layers of sediment slowly built up into a rock which turn into a fossil .
Answer:
Hey there!
Density=Mass/Volume
Density=1.2/4555
Density=2.63e-4g/cm^3
Let me know if this helps :)
Naphthalene balls are used to protect clothes from insects because, when they deteriorate, they create a gas that kills some insects. The naphthalene ball gradually decreases because naphthalene goes through sublimation at room temperature.
For this question, we can use relations for pH and pOH. We calculate as follows:
pOH = -log [OH-]
pOH = -log [<span>1.83x10^-7 M]
pOH = 6.74
pH + pOH = 14
pH = 14 - 6.74
pH = 7.26
pH = -log [H3O+]
7.26 = -log[H3O+]
[H3O+] = 5.46 x 10^-8 M
Hope this answers the question. Have a nice day.</span>