Compare the chemical reactivity of chlorine and bromine. Explain your answer. Thanks in advance


Answer 1

Bromine vs Chlorine | Br vs Cl


Halogens are group VII elements in the periodic table, and all are electronegative elements and have the capability to produce -1 anions.


Bromine is denoted by the symbol Br. This is in the 4th period of the periodic table between chlorine and iodine halogens. Its electronic configuration is [Ar] 4s2 3d10 4p5. The atomic number of bromine is 35. Its atomic mass is 79.904. Bromine staChlorine is an element in the periodic table which is denoted by Cl.  It is a halogen (17th group) in the 3rd period of the periodic table. The atomic number of chlorine is 17; thus, it has seventeen protons and seventeen electrons. Its electron configuration is written as 1s2 2s2 2p6 3s2 3p5. Since the p sub level should have 6 electrons to obtain the Argon, noble gas electron configuration, chlorine has the ability to attract an electron. ys as a red-brown color liquid at room temperature.

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Which of the following is NOT true regarding Rutherford's Gold Foil experiment? - It effectively disproved the Plum Pudding Model because most of the radiation went through.
- It confirms the existence of a dense nucleus and a mostly empty atom.
- The area around the nucleus must be of low mass.
- The scattering of the beta particles confirmed that the nucleus was positively charged.



The area around the nucleus must be of low mass.


Rutherford`s experiment showed that there are some positive charges in the center of the atoms, and because they are all together, they will give a great mass to the atom.

It was quite different from Thomson`s experiment, in which it was thought that the negative charges were mixed with the positive charges, around the atom (like a Pudding Model). In Rutherford`s experiment, because the direction of beta particles, it was the prediction of the positive nucleus.

Hope this info is useful.


PLEASE ANSWER Explain why it is not possible to deduce a complete order of reactivity.





Would you expect a butane lighter to work in winter when the temperature outdoors is 25 ∘F?


No, I would not expect the lighter to work at 25 °F.

25 °F ≈ -4 °C

The boiling point of butane is -1 °C.

At -4 °C, the vapour pressure of butane is not great enough to push back against atmospheric pressure.

The lighter won't work.

As you move from left to right across a period, what happens to the atomic radii?


Taking into account the definition of atomic radius, you move from left to right across a period, the atomic radius decreases.

  • Atomic radius

First, you must know that the atomic radius represents the distance between the nucleus and the valence shell (the outermost). That is, the atomic radius is the distance between the nucleus and the electron furthest from it.

However, because the electron cloud that surrounds the nucleus has no definite limits, the size of an atom is determined by its interaction with the atoms that surround it.  So the atomic radius can be defined as half the distance between the nuclei of two adjacent atoms.

  • Effective nuclear charge

On the other hand, you must first take into account that the effective nuclear charge is the charge that the nucleus should have so that, in the absence of other electrons, the attraction of the nucleus on the electron considered would be the same as the net attraction that the electron experiences. in the real atom.

  • Atomic radius across a period

As you move from left to right through a period of the periodic table, the number of internal electrons of each of the elements in that period remains constant, but the charge on the nucleus increases.

The electrons located in the outermost orbitals then feel a greater “effective nuclear charge”, being attracted with greater force towards the nucleus. This causes the atomic radius to decrease.

In other words, as you move to the right in the same period of the periodic table, even though the atomic number increases and therefore the number of electrons also increases, the atomic radius decreases. This is because, as Z increases, the number of protons also increases, so the attraction they exert on the electrons will also increase.

Then the so-called effective nuclear charge is increasing, and for this reason the nucleus attracts electrons with greater intensity. In this way, the atomic radius decreases.

In summary, you move from left to right across a period, the atomic radius decreases.

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As you move from left to right across a period, atomic radii decreases.


  • Because the no. of protons increases in the nucleus of the atom as we move from left to right across a period on a periodic table.
  • As the number of protons increases, the force of attraction between the protons and the electrons increases.

So, the last shell gets attracted closer, the atomic size also decreases.

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