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Low ionization energies are most characteristic of atoms that are?
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∙ 10y ago
electronegativity
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∙ 10y ago
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The atoms of the most active non-metals have?
large atomic radii and low ionization energies
Why do non metals have higher ionization energies than metal?
Ionization energy is the energy needed to remove an electron. Elements other than transition metals gain or lose electrons from the s and p orbitals in order gain the more stable electron configuration of a Noble gas. Metals lose electrons to become isoelectronic (that is have the same electron configuration) to a noble gas (previous to them in the periodic table), while nonmetals tend to gain electrons in order to become isoelectronic to a Noble gas (next highest on the periodic table). Since ionization energy is the energy needed to REMOVE an electron, it is low for metals which form positive ions by losing electrons to become more stable, but very high for nonmetals that tend to gain, NOT LOSE, electrons. Most transition metals tend to lose electrons as well (other than Rhenium). Transition metals lose electrons from the d orbital, but still form positive ions, so their ionization energy is also usually lower than nonmetals.
Why do elements in the top right corner have high ionization energies?
Ionization energy is the energy required to remove an electron from an atom. In the case of hydrogen, its one and only electron is very close to the nucleus, because it is in the first energy level (that electron's ground state.) So, the attraction between the nucleus (positive) and that electron (negative) is quite strong due to their closeness. As you move down group 1, the electrons get farther and farther away from the nucleus, and the attraction, predictably, decreases. This means lower ionization energy required the lower you go on the group.
Why do elements at the bottom left of the periodic table have low ionization energies?
Bottom left elements of the periodic table have low first ionization energies. Ionization energy is the minimum energy required to remove the outermost electron from an isolated gaseous atom to covert it into monovalent ion. Ionization energy depends on the electrostatic force of attractionbetween the nucleus of the atom and the outermost or valence electron. More the attraction more the energy needed.First of all the size of atoms of bottom left elements is larger as compared to other elements. Therefore, the electrons in the valence or outermost shell are at large distance from nucleus and feel less electrostatic force of attraction and are easier to remove. With increase in atomic number the number of inner shells of electron increases as a result of which shielding or screening effect increases. Since these elements have more number of inner shells so screening effect is more which further decreases the force of attraction. However, the high nuclear charge should cause more attraction but combined effect of nuclear charge, screening effect and large distance from nucleus result in decrease in attraction. Decreased attraction means it will be easier to remove valence electron and ionization energy will be low. It should be noted that only first ionization energy in case of group 1 elements and first and second ionization energy in case of group 2 elements is low but once the atoms of these elements acquire noble gas configuration by losing electrons their ionization energy becomes unusually high.
A diatomic element with a high ionization energy would most likely be?
nonmetal with high electronegativity.
The atoms of the most active non-metals have?
large atomic radii and low ionization energies
What is the differences between first and second ionization energy?
The first ionization energy is the energy that is required in order to remove the first electron from an atom in the GAS phase, the second ionization energy is the energy required to remove the second electron from an atom in the GAS phase. Ionization energy will generally increase for every electron that is removed and increases from left to right in the periodic table and moving up the periods.
Chemical properties of metal?
•They have low ionization energies •Tend to form complexes •Good conductors of heat and electricity
How Which element require the greatest amount of energy to remove an electron?
Core electrons. Probably the 1s level would require the most ionization energy to pull these electrons.
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.
Why do non metals have higher ionization energies than metal?
Ionization energy is the energy needed to remove an electron. Elements other than transition metals gain or lose electrons from the s and p orbitals in order gain the more stable electron configuration of a Noble gas. Metals lose electrons to become isoelectronic (that is have the same electron configuration) to a noble gas (previous to them in the periodic table), while nonmetals tend to gain electrons in order to become isoelectronic to a Noble gas (next highest on the periodic table). Since ionization energy is the energy needed to REMOVE an electron, it is low for metals which form positive ions by losing electrons to become more stable, but very high for nonmetals that tend to gain, NOT LOSE, electrons. Most transition metals tend to lose electrons as well (other than Rhenium). Transition metals lose electrons from the d orbital, but still form positive ions, so their ionization energy is also usually lower than nonmetals.
Some properties of non metals?
Nonmetals have high ionization energies and electronegativities. They are usually poor conductors of heat and electricity. Solid nonmetals are generally brittle, with little or no metallic luster. Most nonmetals have the ability to gain electrons easily.
What is the Definition of ionization enthalpy?
IONIZATION enthalpy is the amount of energy to lose electron from its outer most shell .
What is the difference between positively charged molecular ions and positively charged ions having group of atoms?
Molecular Ions essentially consist of the same type of atoms (most probably the atoms of the same element) and the radicals may not have the same characteristic.
Why do most element have a characteristics valence?
Valency depends upon no of electrons in outer most shell the atoms have a specific no of electrons in valence shell so they have characteristic valence .(but transition metal violate this rule).
Why do elements in the top right corner have high ionization energies?
Ionization energy is the energy required to remove an electron from an atom. In the case of hydrogen, its one and only electron is very close to the nucleus, because it is in the first energy level (that electron's ground state.) So, the attraction between the nucleus (positive) and that electron (negative) is quite strong due to their closeness. As you move down group 1, the electrons get farther and farther away from the nucleus, and the attraction, predictably, decreases. This means lower ionization energy required the lower you go on the group.
The amount of energy that is needed to remove the most loosley held electron is referred to as the what?
You are referring to the ionization enthalpy. The first ionization energy of sodium is the energy for the process Na(g) --> Na+(g) + e-(g).
