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What is the group trend for the ionization energy for the alkali metals?
Wiki User
∙ 13y ago
As you go down the group (any group), ionization energy decreases. So in terms of ionization energy, for the alkali metals,
Lithium > Sodium > Potassium > Rubidium > Caesium > Francium
Wiki User
∙ 13y ago
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What is the trend for first ionization energy for the alkali metals?
Within the alkali metals, or group 1, the ionization energy trend is that ionization energy decreases as you move down the group from top to bottom. This is because with each step down, you add an energy level, therefore the one valence electron is farther and farther from the atom's nucleus. So, the attraction between the nucleus and that electron (its electronegativity) decreases. This makes it easier (requires less energy), making the element more reactive. For example, cesium is more reactive than rubidium, which is more reactive than potassium, which is more reactive than sodium...
Why do alkali metals have lower ionization potentials than alkaline earth metals?
Noble gases have the highest ionization energies of the elements because they don't "want" to lose any electrons. All atoms strive to have a full outer shell like the noble gases and once they reach their equilibrium, it takes a lot of energy to rip off another electron. Alkali metals, by comparison, have a large atomic radius in their period --> low electronegativity --> low ionization energy. Alkali metals have relatively large atomic radii, which means the nucleus is farther away from the electrons than in an atom with a small atomic radius. Because the electrons are far away, it is easier to rip an electron. If it is easy to take away an electron from an atom, then it has a low ionization energy. Alkali metals have lower first ionization energy than noble gases.
Is alkali metals a group 1 elements?
No that is group 2. Group 1 is called Alkali metals.
What ions would be most likely to form?
Atoms of alkaline metals: Rb, Cs, Fr, K, Na, Li. They have a low ionization potential. This potential is expressed in kJ/mol - molar ionization energy and is different for the first, second, third...n electron.
What is the family of the most active metals?
Group 1 metals or alkali metals
Alkali metal and alkaline earth metal have how many ionization energies?
Alkali metals (group 1 elements) have one valence electron. Hence have one ionization energy Alkaline earth metals (group 2 elements) have two valence electron. Hence have two ionization energy
Why do alkali metals become more reactive the farther you go down on the periodic table?
The ionization energy is lower down in the group.
Which decreases with increases atomic number group 2A?
Group IIA metals (alkali earth) become more reactive with non-metals as you go higher in atomic numbers.
Which group of the periodic table has the elements with lowest first ionization energies?
1A Alkali Metals
Which group or famil has the lowest ionization energy?
Group 1 because across group 1 to 8 nuclear force of attraction increases to a significant extent and as a result greater amount of energy is needed to remove an electron. More specifically Fr has the lowest IE and He has the highest
What is the trend for first ionization energy for the alkali metals?
Within the alkali metals, or group 1, the ionization energy trend is that ionization energy decreases as you move down the group from top to bottom. This is because with each step down, you add an energy level, therefore the one valence electron is farther and farther from the atom's nucleus. So, the attraction between the nucleus and that electron (its electronegativity) decreases. This makes it easier (requires less energy), making the element more reactive. For example, cesium is more reactive than rubidium, which is more reactive than potassium, which is more reactive than sodium...
Why do alkali metals have lower ionization potentials than alkaline earth metals?
Noble gases have the highest ionization energies of the elements because they don't "want" to lose any electrons. All atoms strive to have a full outer shell like the noble gases and once they reach their equilibrium, it takes a lot of energy to rip off another electron. Alkali metals, by comparison, have a large atomic radius in their period --> low electronegativity --> low ionization energy. Alkali metals have relatively large atomic radii, which means the nucleus is farther away from the electrons than in an atom with a small atomic radius. Because the electrons are far away, it is easier to rip an electron. If it is easy to take away an electron from an atom, then it has a low ionization energy. Alkali metals have lower first ionization energy than noble gases.
What are common physical and chemical features of alkali metals?
Examples: react violently with water, low density, low melting point, low ionization energy, monovalent, group 1, etc.
Why alkali metal have low ionization energy?
Ionization energy is the energy required to remove an electron from an atom or ion. Low ionization energy indicates that it takes less energy to remove an electron from the atom. The alkali metals are in Group I on the Periodic Table. This indicates that their atoms have only one electron (out of a possible eight) in their outermost energy level. Therefore it takes less energy to remove the single outermost electron. Moving across a period on the Periodic Table, ionization energies increase because there are more and more electrons in the outermost energy level, requiring more energy to remove an electron.
Which group metals are very reactive with one electron in the outer energy level?
Alkali metals
What is the most reactive group of metals?
in group 1, the first column on the left Edit: these would be the alkali metals.
Is alkali metals a group 1 elements?
No that is group 2. Group 1 is called Alkali metals.
