Yes they are, but however, they do not react at the same intensity and enthusiasm. Metalloids and be both nonmetals or metals.
If you mean a group of metals that are mixed when molten, example as in steelmaking then it is called an ALLOY
Alkali metals are highly reactive. This is because they have only one electron in the valence shell, and the atom really wants to get rid of it, making it very unstable.
yes because javonna jones says so
yes group 1 is the most reactive
Caesium belong to Group (1) The Alkali metals. Since it is the lowest in the Group , except for 'Francium', its reactivity with water and oxygen is 'explosive'. Going down the Group (1) the elements are , with increasing reactivity , Lithium, Sodium, Potassium, Rubidium, Caesium, and Francium. You will not find francium in the open lab. as it is radio-active.
The chemical reactivity of transition metals is generally less than that of metals to its left (group 1 and group 2 metals). However, transition metals can exhibit various oxidation states and hence form more number of compounds than group 1 and group 2 elements.
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 in group 1 of elements increases as we go down the group (to francium) because in the alkali metals as we go down the group number of atomic shells increases so the elements with most shells will easily release their electrons in the outer most shell.
The metals that react violently with cold water are group 1 and group 2 metals. Reactivity increases going down the group and to the left of a period.
The reactivity increase down in the group.
yes, they are less reactive than group 1 and 2. These metals hardly react with air or water at all whereas Group 1 and 2 metals tarnish quickly and react with water
because of the power of each metal it goes up in reaction.
Caesium belong to Group (1) The Alkali metals. Since it is the lowest in the Group , except for 'Francium', its reactivity with water and oxygen is 'explosive'. Going down the Group (1) the elements are , with increasing reactivity , Lithium, Sodium, Potassium, Rubidium, Caesium, and Francium. You will not find francium in the open lab. as it is radio-active.
The chemical reactivity of transition metals is generally less than that of metals to its left (group 1 and group 2 metals). However, transition metals can exhibit various oxidation states and hence form more number of compounds than group 1 and group 2 elements.
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 in group 1 of elements increases as we go down the group (to francium) because in the alkali metals as we go down the group number of atomic shells increases so the elements with most shells will easily release their electrons in the outer most shell.
Metals: the farther to the left the more reactive they are. Group 1 metals, which include sodium and potassium, are so highly reactive that they do not exist in nature by themselves (only in compound form.) Non-metals: the farther to the right the more reactive they are *with the exception of group 18* which are the noble gases and do not react at all. The most reactive are group 17, which include fluorine and chlorine. These non-metals, like group 1, rarely exist by themselves because of their high reactivity.
The metals that react violently with cold water are group 1 and group 2 metals. Reactivity increases going down the group and to the left of a period.
Please check the associated link on the first group metals. It shows the reactivity of pure sodium and other group 1 elements
No. Group 1 metals (commonly called the alkali metals) have low melting points.
it is. it needs to lose 1 electron to be stable