Give some similarities that exist among the elements of group 7?

Answer 1

similarities in the Periodic Table are the rows show reactivity going from left to right.

left is highly reactive and right is unreactive, or stable. The columns show similar reactivity because they have the same amount of electrons.

Answer 2

Group 7 elements, also known as halogens, share similarities such as having 7 electrons in their outermost shell, high reactivity due to their tendency to gain an electron to achieve a full outer shell, and forming diatomic molecules in their elemental form (e.g., Cl2, Br2). They also have similar physical properties such as being nonmetals, having low melting and boiling points, and having colored vapors.

Answer 3

High electron affinity, high ionization energy, readily form anions, small atomic radius, high effective nuclear charge, can form ionic bonds with metals or single covalent bonds with one another or with hydrogen.

Answer 4

The elements of Group 1 are known as the "Alkali metals." These metals include:

Lithium- Li

Sodium- Na

Potassium- K

Rubidium- Rb

Cesium- Cs

Francium- Fr

One similarity is that all of them have an electron configuration that makes their "s" orbital unpaired. For example,

Lithium- [He]2s1

Sodium- [Ne]3s1

Potassium- [Ar]4s1

Rubidium- [Kr]5s1

Cesium- [Xe]6s1

Francium- [Rn]7s1

Therefore, in each element the valence electron configuraiton is ns1, where n is the period number.

Other similarities include appearance; all Group 1 elements are silvery colored metals. They are soft enough to cut through with a knife; cutting will expose a shiny surface that oxidation will dull.

These elements are also all highly reactivemetals, with reactivity increasing in descending order (Lithium least, Cesium greatest.) You might want to check out this video for proof on how reactive cesium is. http://www.YouTube.com/watch?v=sNdijknRxfU

In addition, none of these elements are found free in nature considering their highly reactive nature. For example, sodium is generally found as NaCl (salt), not just Na.

Concerning physical properties, all are soft and have low melting points and low boiling temperatures. Their density is also extremely low; for example, Li, Na, and K are less dense than even water. They have low standard enthalpies of melting and vaporization and also exhibit weak metallic bonding, because only one electron is available for bonding.

All alkali metals produce color flames. When the element is placed in a flame of fire, the heat provides enough energy to cause the outer electron to "jump" to the next energy level. When this outer electron falls back to ground state, it emits energy that emits a wavelength of visible light.

Li- red

Na- yellow

K- lilac

Rb- red

Cs- blue

For chemical properties, all alkali metals are strong reducing agents with standard electrode potentials ranging from -2.7V to -3.0V, an indication of a strong tendency to form cations (+) in solution. Alkalis can reduce oxygen, chlorine, ammonia, and hydrogen; when they react with oxygen, they tarnish.

Answer 5

their similar properties are that they tend to form electrovalent compounds,they are less reactive when compared to group one because of lowered ionization energy,they have two valence electrons and form divalent ions and all extracted by electrolysis.

Answer 6

they are all nonmetals, all exist in diatomic molecules 2.

Answer 7

They all are nonmetals.They all are diatomic molecules

Answer 8

the group number is the same number as the amount of electrons on the outer shell

Answer 9

Because they all have the 2 electrons in their outer shell.

Answer 10

they are metal and transitional elements