It decreases. This is because each period (row) you go down, the element has more shells. The more shells the less effective the positive nucleus is at attracting other negative atoms to bond with and gain an electron. It is made harder to attract because there is an increasingly bigger field of negative electrons in the way.
They get more reactive as they go up because a more reactive group 7 element will puch out (displacement reactions) a less reactive one when they are reacting with another elements espically group 1 metals because halogens only need one eletron to make them stable.Moving down the group, ionic radius increases and the attraction the halide nucleus has for valance electrons decreases - because of the greater distance reducing the amount of electrostatic attraction between nucleus and electron, and because fo greater electron shielding from core electrons.
Group 1 elements are reactive if they have low electronegativity, or easily give up their electrons to become cations,
Group 7 elements are reactive if they have high electronegativity, or easily take up other electrons to become anions
As you go down each row, electronegativity goes down due to the electron shielding effect of core electrons. lower electronegativity is more reactive for cations like group 1, but less reactive for anions like group 7
It is more reactive as you go up the group, this is because as you go up the group the electronegativity increases and therefore it's more reactive due to this property.
your mum and chemistry
The reactivity of group 17 elements differ as you move down the periods. Group 17 elements are missing 1 electron from their valance shell making them highly votile and reactive.I'll try not to make this confusing:1. As elements get bigger, they have a higher level of reactivity. (More "pull" needed from protons in the nucleus in order to keep valance shell electrons in orbit).2. As you move from left to right in the groups, you have a higher level of reactivity.3. Groups 1 and 17 have the highest levels of reactivity (except hydrogen in group 1) because they are away by only 1 valence electron.
The reactivity is increasing goinng down in the group.
describe how the reactivity of group1 elements and group 7 elements varies with increasing atomic number
Reactivity of non-metals increases as you move from left to right on the periodic table, or as group number increases. The most reactive non-metals are found in group 17.
group 18
Down the group, reactivity decreases for non metals. It increases for metals.
It is because the group 1 and 7 elements have a high reactivity. The reactivity is far too high to use on there own because the elements in these groups react with air and/or water.
Reactivity increases down the group for metals. It decreases down the group for non-metals.
The reactivity of group 17 elements differ as you move down the periods. Group 17 elements are missing 1 electron from their valance shell making them highly votile and reactive.I'll try not to make this confusing:1. As elements get bigger, they have a higher level of reactivity. (More "pull" needed from protons in the nucleus in order to keep valance shell electrons in orbit).2. As you move from left to right in the groups, you have a higher level of reactivity.3. Groups 1 and 17 have the highest levels of reactivity (except hydrogen in group 1) because they are away by only 1 valence electron.
The reactivity is increasing goinng down in the group.
The reactivity increase down in the group.
describe how the reactivity of group1 elements and group 7 elements varies with increasing atomic number
Reactivity of non-metals increases as you move from left to right on the periodic table, or as group number increases. The most reactive non-metals are found in group 17.
they become more reactive since you are moving from left to right on the Periodic Table, the elements in group 17 are the most reactive.
group 18
they become more reactive since you are moving from left to right on the Periodic Table, the elements in group 17 are the most reactive.
The electron configurations of the elements in each main group are regular and consistent:the elements in each group have the same number of valence electrons.