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What is the trend in melting points as you go down the group of halogens?
Wiki User
∙ 11y ago
The melting point is greater.
Wiki User
∙ 11y ago
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Name two elements that are side by side on the periodic table that do not reflect the general trend in melting points for the periods?
The Two Element That Are Side By Side by side on the periodic table would be Sr (Strontium) and Y (Yttrium) because they do nit follow trend across the period for melting points.
Explain how the trends in melting point and boiling point differ from the other periodic trends?
Instead of generally increasing or decreasing trend, melting and boiling points reach two different peaks as d and p orbitals fill. -Darryn
Does the dispersion force increase down the halogens?
Yes, dipersion forces increase moving down the halogens, ie from fluorine to chlorine, then bromine, and then iodine. This is a general trend in most groups due to increasing numbers of electrons farther from the nucleus. However, it is especially evident in the halogens. Fluorine is the least polarizable element because of it's electronegativity and the proximty of the electrons to the nucleus (there is a high effective nuclear charge). In iodine, the electronegativity is lower and the electrons are father from the nucleus. Thus, it has much higher dispersion forces caused by temporary dipoles. The trend is true for the rest of the halogens as well.
What is the group trend in p-block element?
Atomic radius increases down the group
What is the Group trend Atomic radius?
Atomic radius increases down the group. This is because of the increase in number of shells.
What is the trend in density as you go down the group of halogens?
The density increase down.
Which trend decreases for metals down a group?
Melting Point
What is the trend in the boiling points of the halogens?
The boiling point and the melting point of halogens is increasing from fluorine to iodine. Boiling points of halogens are: - Fluorine: -188,12 0C - Chlorine: -34,04 0C - Bromine: 137,8 0C - Iodine: 184,3 0C
Name two elements that are side by side on the periodic table that do not reflect the general trend in melting points for the periods?
The Two Element That Are Side By Side by side on the periodic table would be Sr (Strontium) and Y (Yttrium) because they do nit follow trend across the period for melting points.
Which trend decreases for metals down a group atomic radiusreactivity or melting point?
Melting points generally decrease as you go down a group for group I and group II metals. This does not apply to the transition metals. Reactivity of metals increases down a group due to a larger size and less effective charge between the nucleus and valence electrons. Atomic radius increases due to a higher principle number of electrons.
Identify the trend in melting point from lithium to caesium?
From lithium to caesium the melting point is decreasing.
Explain how the trends in melting point and boiling point differ from the other periodic trends?
Instead of generally increasing or decreasing trend, melting and boiling points reach two different peaks as d and p orbitals fill. -Darryn
What is the general trend of the melting points of hydrides across the period?
we dont have periods because we are men and we are just the way we are P.s (SEN<SHAGGY<PATRA using his chinese fone)
Why caesium is liquid at nearly room temperature?
Why not? Or, in other words, there's not really a "why" to explain here; it's an extension of a well-established trend (unlike mercury, which is a liquid at room temperature while all the metals around it are solid and there's no such trend that would predict its dramatically lower melting point). The trend for alkali metals is that they have lower melting points as you move down the table. By the time you get to caesium, it's only a little above room temperature, and the theoretical melting point for francium is even lower than that (but still slightly above room temperature).
What is the general trend within a family or a group?
describe the general trend in size going from top to bottom of any group or family
Why does rubidium not follow the general trend of ionization energy in its group?
I suppose that this trend is normal.
Does the dispersion force increase down the halogens?
Yes, dipersion forces increase moving down the halogens, ie from fluorine to chlorine, then bromine, and then iodine. This is a general trend in most groups due to increasing numbers of electrons farther from the nucleus. However, it is especially evident in the halogens. Fluorine is the least polarizable element because of it's electronegativity and the proximty of the electrons to the nucleus (there is a high effective nuclear charge). In iodine, the electronegativity is lower and the electrons are father from the nucleus. Thus, it has much higher dispersion forces caused by temporary dipoles. The trend is true for the rest of the halogens as well.
