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Well, if you look at it in a purely elemental capacity we see trends that with an increase in electron shielding, we get a decrease in melting point.
This is said to be because with larger electron shielding we have a lower Z(eff) (effective nuclear charge) between atoms meaning weaker forces keeping them together and thus a lower melting point.
I think this is an important logical procedure when understanding why things melt and what things like Z(eff) really mean in terms of an atom's behaviour. It's a good learning tool but, outside of periodicity, I would never feel comfortable attributing a melting point to electron shielding. Good idea for elements, terrible idea for molecules.
What else can I help you with?
Are freezing and melting points characteristic properties?
Yes, freezing and melting points are characteristic properties of a substance. They are specific temperatures at which a substance changes its state from solid to liquid (melting) or from liquid to solid (freezing) under normal atmospheric pressure.
Are melting and boiling point physical properties of a substance?
Yes, melting and boiling points are physical properties of a substance. They represent specific temperatures at which a substance transitions from one phase to another - solid to liquid for melting point, and liquid to gas for boiling point.
What are the effects of pressure on melting boiling points of a substance?
Increasing pressure generally increases the melting and boiling points of a substance. This is because pressure forces molecules to be packed closer together, making it harder for them to break free from each other in the solid or liquid phase. Conversely, decreasing pressure lowers the melting and boiling points.
Which all metals have low melting and boiling points?
Some examples of metals with low melting and boiling points include mercury, cesium, and gallium. These metals have melting and boiling points significantly lower than traditional metals like iron and copper.
What are vandarwalls forces?
Van der Waals forces are weak attractive or repulsive forces that exist between molecules due to temporary fluctuations in electron density. These forces include London dispersion forces, dipole-dipole interactions, and hydrogen bonding. They play a role in determining the physical properties of substances like boiling points, melting points, and solubility.
Why is electron shielding not a factor when you examine a trend across a period?
Electron shielding is not a factor across a period because they all have the same number of electron shells! No further (extra) shells means that they are all affected by electron shielding equally.
In going down a group in the periodic table what effect does electron shielding generally have on the effective nuclear charge acting on the outermost electron in an atom?
Electron shielding increases down a group in the periodic table, as more electron shells are added. This reduces the effective nuclear charge experienced by the outermost electron, making it easier for that electron to be removed or participate in chemical reactions.
An electron in an orbital that penetrates closer to the nucleus will always experience more shielding than an electron in an orbital that does not penetrate as far?
False. Shielding is determined by the presence of other electrons between the nucleus and the electron in question, not solely by the distance from the nucleus. Even if an orbital penetrates close to the nucleus, if there are other electrons in higher energy orbitals shielding it, the shielding effect can be significant.
Do all of the noble gases have at least 3 electron shielding layers?
No, not all noble gases have at least 3 electron shielding layers. The noble gas helium (He) has only two electron shielding layers, while the remaining noble gases (Neon, Argon, Krypton, Xenon, and Radon) have three or more electron shielding layers.
How many electron shielding layers do noble gasses have?
Noble gases have 8 electron shielding layers. This is because noble gases have a full outer electron shell, so they have filled all available energy levels up to the 8th shell, leading to 8 electron shielding layers.
How many shielding atoms does magnesium have?
Magnesium has 3 electron shells.
Which ions have high melting points?
positive ions have high melting points
Do proteins have definite melting points?
Different proteins have different melting points.
Why does shielding increase as you move down a group in the periodic table?
As you move down a group in the periodic table, shielding increases because there are more electron shells surrounding the nucleus. These additional electron shells act as a barrier, reducing the attraction between the nucleus and outer electrons, thus increasing shielding.
Compared with the melting points of ionic compounds the melting points of molecular solids tend to be .?
Ionic compounds have a higher melting point.
How many shielding electrons does sulfur have?
This is a chemical element. You can find the how many electron in a single atom by using a periodic table.
The attraction of the nucleus for the outer electrons in large atoms is lessened as a result of?
The attraction of the nucleus for the outer electrons in large atoms is lessened as a result of increased electron-electron repulsions. As the number of electrons increases, these repulsions cause the outer electrons to be further away from the nucleus, reducing the effective attraction. This phenomenon contributes to the shielding effect and explains the reduced attraction of the nucleus for outer electrons in large atoms.
