The reactivity of Group 1 elements increases as you go down the group because:
- the atoms get larger as you go down the group
- the outer electron gets further from the nucleus as you go down the group
- the attraction between the nucleus and outer electron gets weaker as you go down the group - so the electron is more easily lost
Why does the reactivity of Group 1 increase down the group?
Why does the reactivity of the Group 1 elements increase as you go down the group? As you descend group 1, there is an increasing number of electron shells, therefore increasing the distance between the positive nucleus and the negative outer electron which decreases the attraction between the two.
How does the reactivity of metals vary down the group?
Group 1 metals react by losing their one valence electron. As you go down the group, the atomic radius increases, putting the valence electron far away from the nucleus, less attracted by the nucleus and easy to let go. Therefore the reactivity increases down the group.
Why do some elements have more reactive electrons than others?
Simply stated: As you go down group 1, the number of electron shells increases – lithium has two, sodium has three, and so forth. The attraction from the positive nucleus to the negative electron is less. This makes it easier to remove the electron and makes the atom more reactive.
Why do Group 1 elements form ionic compounds?
Due to the group 1 elements forming ionic compounds, they lose their outer electron when they react and so the weaker attraction between the nucleus and the outer electron means they are able to lose that electron more easily and therefore are more reactive. Need help with Chemistry?
Why does reactivity increase down group 1 but up Group 7?
Reactivity decreases down the group. This is because group 7 elements react by gaining an electron. As you move down the group, the amount of electron shielding increases, meaning that the electron is less attracted to the nucleus.
Why does reactivity increase down group 1 and 2?
As we go down the group, the atom gets bigger. The bigger the atom, the further away the last electron. Therefore, the attraction between the nucleus and the last electron gets weaker. This makes it easier for the atom to give up the electron which increases its reactivity.
Why does the reactivity of group 1 increase as you go down the group but the reactivity of Group 7 decreases as you go down the group?
The answer to your question is quite simple. The alkali metals of group 1 grow larger in size downwards and since the effective nuclear charge remains the same as we go down group 1 the number of shells also increases and so it is easy to lose an electron and therefore as we move downwards the reactivity increases.
What increases down group 1?
Group 1 elements are known as Alkali Metals. They are called s-block elements because their highest energy electrons appear in the s subshell. Progressing down group 1, the atomic radius increases due to the extra shell of electrons for each element.
Why does reactivity increase left to right?
The farther to the left and down the periodic chart you go, the easier it is for electrons to be given or taken away, resulting in higher reactivity. Period - reactivity increases as you go from the left to the right across a period. Group - reactivity decreases as you go down the group.
Why do group 1 elements get less reactive as you go down?
the outer electron gets further from the nucleus as you go down the group. the attraction between the nucleus and outer electron gets weaker as you go down the group - so the electron is more easily lost.
Why does chemical reactivity increase from top to bottom in in group 1 but decrease from top to bottom in Group 7?
Electropositivity increases down the group of alkali metals, thus the reactivity increases down the group of alkali metals. The reactivity of halogens is due to their electronegativity. Electronegativity decreases down the group, thus reactivity of halogens decreases down the group.
Why does reactivity decreases as you go from left to right?
It is because the number of valence shells is increasing, and the attraction between valence electrons and the nucleus decreases. Therefore, the tendency to pull electrons from other atoms decreases. On moving across a period, the electronegativity of atoms increases.
Why is Group 2 more reactive down the group?
The reactivity of the group 2 elements increase as you go down the group. This is because, as explained previously, it is much easier to remove an outer shell electron as you go further down the group (lower ionisation energies).
Why does the reactivity of metals increase down in Group 2?
Effective nuclear charge decreases, there is an overall weaker attraction on the valence electrons and less energy is required to remove the electrons. Therefore ease of oxidation and chemical reactivity increases down group 2.
Why does reactivity of metals increase down a group?
Metal reactivity increases down a group because as nuclear shielding increases and the nucleus' hold on the valence electron weakens, therefore it is easier to remove valence electrons.
What group is more reactive 1 or 2 Why?
Group 1 alkali metals are more reactive than group 2 Alkaline Earth Metals.
What happens to the atom as you go down the group?
As we go down the group, the atom gets bigger. The bigger the atom, the further away the last electron. Therefore, the attraction between the nucleus and the last electron gets weaker. This makes it easier for the atom to give up the electron which increases its reactivity. Answered by Madhangi P. • Chemistry tutor.
How are atoms made?
An atom is made in such a way that the nucleus with the positive charges (protons) is in the centre and the negative charge (electrons) are arranged in shells around it. All group 1 metals have one electron in its outer shell. As we go down the group, the atom gets bigger. The bigger the atom, the further away the last electron.
Why do alkali metals lose electrons?
This is because the increased number of electron shells results in more shielding and a greater distance between the outer electrons and the nucleus, which reduces the attraction of the electrons to the nucleus.
Why does the size of an alkali metal increase down the group?
The size of alkali metal increases down the group because number shell increase. We know that electron removed readily from larger atom, therefore required less energy. It means ionization enthalpy decreases down the group due to increase in size. So electron releasing tendency of alkali metal (electropositive character ) increased hence reactivity inceased down the group. That why francium is most reactive metal.
How many electrons are in an alkali metal?
All alkali metals have one electron in the outer shell. In a reaction, this electron is lost and the alkali metal forms a +1 ion. As you go down group 1, the number of electron shells increases – lithium has two, sodium has three etc. Therefore, the outermost electron gets further from the nucleus.
What happens when you go down group 1 in the PT?
As you go down group 1 in the PT, the atoms get bigger so the other electron is “further" from the nucleus so is less strongly attracted. Also there are increasing numbers of “shells" of electrons between the outer electron and the nucleus and this “shields" the attractive charge of the nucleus. Both these effects mean that the 1st ionization energy d
Why is it easier to remove an electron from the nucleus to form K+?
because the outer electron is further from the positive charge of the nucleus; so it is easier for it to be removed to form K+. Or if you like the first ionization energy is less
How many orbitals does a noble gas have?
The electronic configuration of an atom is such that they want a complete outter electron shell, which the little guys aside, is eight orbitals. The Noble Gases all have all eight valence electrons so they are electrically stable. In other words, their just hanging out drinking beet and loving life. They gain nothing by accepting or losing an electron cause it's extremely energetically unfavorable to go from eight in the valence to anything that isn't eight. It just doesn't happen. Sodium sees the Noble Gases over there relaxing and he wants a beer too. But, he's got that single pesky electron in his valence shell. Sodium has a single oxidation state, +1, and boy would it like to be rid of that charge. Since much of the periodic table has multiple oxidation states, and usually -1 is one of them, they will happily accept or share an electron with Sodium. When that happens, Sodium suddenly has a Noble Gas-like experience because giving up or sharing an electron gives the atom eight electrons in its valence shell. Since accepting one bond isn't terribly difficult for many of the others Sodium will rush up, shove his way in and be happy. Sodium reactions can be so violent because the atom transitions from a highly energetic state to a much lower energy state that's pseudo-Noble.
Which element has the highest electropositive charge?
Because 1st group has just one valence electron and with increasing radius of atoms in the group, electron is spread over bigger surface and thus being less attracted by positive charge of nucleus - making francium the most electropositive element. That means that ionization energy is lower than that of any other alkaline metal meaning francium gets to stable octet the easiest - making it the most reactive alkaline metal.
Why are alkali metals more reactive?
Larger alkali metals means that there is less Z-effective or effective nuclear charge between the central nuclei and the valence electrons due to a screening/shielding effect. This allows them to be more reactive as they can lose electrons easily.
Do halogens gain electrons?
However in group 17 the halogens have to gain an electron. So when the size increases and the number of shells increases the attraction of electrons decreases as we move away from the nucleus and so it is difficult to gain an electron as we move downwards.
Do alkali metals grow larger as we move down group 1?
The answer to your question is quite simple.The alkali metals of group 1 grow larger in size downwards and since the effective nuclear charge remains the same as we go down group 1 the number of shells also increases and so it is easy to lose an electron and therefore as we move downwards the reactivity increases.
Does reactivity decrease as you go down group 7?
However, as you go down group 7 (the halogens), reactivity actually decreases, and the reason given is that it is harder for it to gain electrons, which contradicts the previous statement? Any ideas?
