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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.
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What is the trend in melting point and boiling points of the elemets in group 1 and 7?
In Group 1 (alkali metals), the melting and boiling points decrease as you move down the group due to the increase in atomic size and metallic bonding. In Group 7 (halogens), the melting and boiling points increase as you move down the group due to the increase in atomic size and London dispersion forces.
Why do the properties of halogens change as you move down the group?
As we move down the group of halogens the number of shells increase (as the number of periods are increased). Thus the halogens become less reactive. Halogens react by gaining an electron to have a complete outer shell (as they have seven). As the number of shells increase, the magnetic force from the nucleus (of the protons to the electrons) decrease thus make them less likely to gain an electron from other molecules. So the ones nearer to the bottom (e.g. iodine) will be less reactive than the one nearer to the top (e.g. chlorine).
What is the trend in melting points as you go down the group of halogens?
The trend in melting points as you go down the group of halogens is that they generally increase. This is due to the increasing number of electrons and atomic size which results in stronger van der Waals forces between the atoms, leading to higher melting points.
Bromine chlorine iodine state intermolecular forces?
Bromine, chlorine, and iodine are all halogens that exist as diatomic molecules (Br2, Cl2, I2) at room temperature. They are held together by weak van der Waals forces, which exist as London dispersion forces due to the temporary dipoles formed by the movement of electrons in the molecules. These intermolecular forces increase in strength as you go down the group from bromine to iodine.
Describe the trends in the bond length between hydrogen and halogens?
The bond length between hydrogen and halogens decreases as you move down the halogen group on the periodic table. This is due to the increase in atomic size and electron shielding, leading to weaker hydrogen-halogen bonds. Additionally, bond length tends to increase in strength as you move left to right across the periodic table due to increasing electronegativity.
What is the trend in density as you go down the group of halogens?
The density increase down.
What is the trend in melting point and boiling points of the elemets in group 1 and 7?
In Group 1 (alkali metals), the melting and boiling points decrease as you move down the group due to the increase in atomic size and metallic bonding. In Group 7 (halogens), the melting and boiling points increase as you move down the group due to the increase in atomic size and London dispersion forces.
Which of the intermolecular forces are responsible for the phase behavior of the elemental halogens?
The phase behavior of the elemental halogens is primarily influenced by London dispersion forces, which are the weakest type of intermolecular forces. These forces arise due to temporary fluctuations in electron density, leading to temporary dipoles. As the size and number of electrons increase down the group from fluorine to iodine, the strength of these dispersion forces also increases, resulting in higher boiling and melting points. Consequently, while fluorine and chlorine exist as gases at room temperature, bromine is a liquid, and iodine is a solid.
Which factor is responsible for the weak attraction between diatomic molecules of the halogens group 7A?
Within the halogen group, dispersion forces account for a lot of their physical properties. Dispersion forces are caused by the random motion of electrons causing a "pile up" of electrons very briefly on a certain side of the atom. This causes a slight difference in charge across the length of the atom, which in turn causes a slight attraction or repulsion on the part of another nearby atom. Multiplied billions of times across billions of atoms, it creates a measurable force. Dispersion forces are the reason why fluorine (F) and chlorine (Cl) are gases, bromine is a liquid (Br), and iodine (I) is a solid. The more electrons there are (going top to bottom down the halogens), the more dispersion forces you have.
Why do the properties of halogens change as you move down the group?
As we move down the group of halogens the number of shells increase (as the number of periods are increased). Thus the halogens become less reactive. Halogens react by gaining an electron to have a complete outer shell (as they have seven). As the number of shells increase, the magnetic force from the nucleus (of the protons to the electrons) decrease thus make them less likely to gain an electron from other molecules. So the ones nearer to the bottom (e.g. iodine) will be less reactive than the one nearer to the top (e.g. chlorine).
Do the halogens have a higher boiling point going down the group and why is that?
Yes, halogens have a higher boiling point going down the group. This is because the atomic size increases with atomic number, leading to stronger London dispersion forces between molecules as the size increases. Consequently, more energy is required to overcome these forces, resulting in higher boiling points.
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
When you apply the brakes on your bike you are clamping down on the bikes wheel to increase the force of?
You increase the friction.
How did industrialists increase their profits?
They force the cost of their raw materials down, force the cost of labour down or replace it with machinery and force the price of the finished goods up.
How do the boiling points of the noble gases change as you go down the group helium neon argon krypton?
The boiling points of noble gases increase as you go down the group from helium to krypton. This is because the boiling point is influenced by the strength of the London dispersion forces among the atoms, which increases with molecular size. As the atomic size and mass increase down the group, the London dispersion forces also increase, resulting in higher boiling points.
What is the trend in melting points as you go down the group of halogens?
The trend in melting points as you go down the group of halogens is that they generally increase. This is due to the increasing number of electrons and atomic size which results in stronger van der Waals forces between the atoms, leading to higher melting points.
Why does reactivity of the halogens decrease down the group?
As it go down the group, the distance between the nucleus (+ve) and the last electron (-ve) becomes smaller No: BIGGER.Therefore the electrons are held in the atom very tightly more loosely by a strong weakening force from the nucleus.So, it is said as the reactivityDEcreases down the group of NON-metals which gain stronger their electrons andINcreases down the group of metals which loose those electrons.
