What atom has a stable valence electron configuration?
What atom has a stable valence electron configuration?
Group 18 elements (helium, neon, and argon are shown in Figure 2) have a full outer, or valence, shell. A full valence shell is the most stable electron configuration.
Has a stable valence electron configuration?
1 Answer. The most stable electron configuration is that of a noble gas, due to the fact that its valence shell is filled. For helium, that means two valence electrons (a duet) in the 1s sublevel, and for the rest it means eight valence electrons (an octet) in the outermost s and p sublevels.
How many valence electrons does a stable atom have?
eight electrons
Which elements have 8 valence electrons and are the most stable?
Noble gases are the least reactive of all elements. That’s because they have eight valence electrons, which fill their outer energy level. This is the most stable arrangement of electrons, so noble gases rarely react with other elements and form compounds.
Why do atoms always want 8 valence electrons?
The Significance of “8” in Chemistry The rule of 8 or the Octet rule is the tendency of atoms to have eight electrons in their valence shell. Eight electrons in this final shell allow atoms to be stable and non-reactive. Atoms tend to be reactive when their valence shell (or outermost shell) is incomplete.
Why is electron affinity highest in the top right corner?
The general trends of the electron affinity are that it increases from left to right across the periodic table due to an increase in the nuclear charge, and it increases from bottom to top due to the effect of atomic size. This results in a higher electron affinity.
How do you determine the highest electron affinity?
Unlike electronegativity, electron affinity is a quantitative measurement of the energy change that occurs when an electron is added to a neutral gas atom. The more negative the electron affinity value, the higher an atom’s affinity for electrons.
Why would a noble gas have an electron affinity value of zero?
Large atoms have low ionization energy and low electron affinity. Therefore, they tend to lose electrons and do not tend to gain electrons. Any electrons added to a noble gas would have to be the first electron in a new (larger) energy level. This causes the noble gases to have essentially zero electron affinity.
Why do metals have low ionization energies?
Why do metals have a low ionization energy? Because the valence electrons are farther away from the positively charge nucleus, so the force of attraction is low.
Which group has lowest first ionization energy?
francium
Which is the biggest atom in Group 1?
As can be seen in the figures below, the atomic radius increases from top to bottom in a group, and decreases from left to right across a period. Thus, helium is the smallest element, and francium is the largest.
Why does density increase down Group 1?
Generally, we see that in alkali metals the rate of increase of mass is greater than rate of increase of volume, therefore the density increases down the group.
Why does density increase down Group 0?
The density increases as you go down the group. As the atoms get bigger, they get heavier, and so you have an increasing mass in the same volume – the density goes up.
Does density increase with atomic mass?
Explanation: Atoms with a lower atomic mass have a greater density than the atom with the higher atomic weight because the atoms are tightly packed together. The volume of a material can change with temperature and pressure. This can also modify the density of the material.
Why are the Group 1 metal soft low melting and low density?
Alkali Metals features the large atomic radii between neighbouring atoms of Group 1. Hence, the molecules show weaker attractive forces and are soft and have low melting points.