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An atom has a first ionization energy of 496 kJmol and a second ionization energy of 4560 kJmol What group of the periodic table would the atom be in?
Wiki User
∙ 15y ago
group 1
Wiki User
∙ 15y ago
The significant jump in ionization energy from the first to the second indicates the removal of an electron from a filled energy level. This suggests the atom is in the second group of the Periodic Table, since elements in this group have a filled outer s sublevel before starting to fill the p sublevel in the subsequent period.
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What trend it does the first ionization energy follow going across the periodic table?
The first ionization energy tends to increase across a period from left to right on the periodic table. This is due to the increasing nuclear charge and decreasing atomic radius, which leads to a stronger attraction between the electrons and the nucleus.
Which of these elements has the highest first ionization energy Si or C?
Carbon (C) has a higher first ionization energy than silicon (Si). This is because as you move across a period in the periodic table, the first ionization energy generally increases due to increasing nuclear charge pulling electrons closer. Silicon is positioned to the right of carbon in the same period, resulting in a lower first ionization energy compared to carbon.
Which comes first electronegativity electron configuration periodic trends ionic radius atomic radius ionization energy or periodic table?
The periodic table comes first, as it provides the framework for organizing elements based on their properties. Electronegativity, electron configuration, periodic trends, ionic radius, atomic radius, and ionization energy are concepts that build upon the periodic table and help explain the behavior and characteristics of elements in a systematic manner.
Which has the larger sixth ionization energy Se or Br?
Selenium (Se) would have a larger sixth ionization energy compared to Bromine (Br) because as electrons are sequentially removed from an atom, it becomes increasingly difficult to remove them due to the stronger positive charge on the remaining ion. Since selenium has a higher atomic number and more protons, it will have a higher ionization energy than bromine.
Which element's second ionization energy level is large compared to its first ionization energy?
Cl
Are there any trends to the periodic table?
Atomic Radii,Ionic Radii, First Ionization Energy,Second and Higher Ionization Energies, Electron Affinity.
How is the electronagativity trend related to the first ionization energy trend?
Electronegativity and first ionization energy both increase as you move up the periodic table
How is the electronegative trend relate to the first ionization energy trend?
Electronegativity and first ionization energy both increase going up the Periodic Table.
How the electronegativity trend related to the first ionization energy trend?
Electronegativity and first ionization energy both increase going up the Periodic Table.
What trend does the first ionization energy follow going down the periodic?
The first ionization energy decreases because the outermost electron is farther from the nucleus. Apex
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.
What is ionization energy of boron?
Across a row on the periodic table ionization energy increases. Down a column, ionization energy decreases. --------------------------------------------------------- The first Ionization energy of Boron is 800.6 kJ mol-1
How does the first ionization energy change going down and across the periodic table?
As you move down a group on the periodic table, the first ionization energy generally decreases due to the increasing atomic size and shielding effect of inner electrons. Across a period, the first ionization energy generally increases because the effective nuclear charge increases, making it harder to remove an electron.
What trend it does the first ionization energy follow going across the periodic table?
The first ionization energy tends to increase across a period from left to right on the periodic table. This is due to the increasing nuclear charge and decreasing atomic radius, which leads to a stronger attraction between the electrons and the nucleus.
What other trend is similar to periodic trend for electronegativity?
The trend for first ionization energy
What trend does the first ionization energy follow in the periodic?
It decreases when going down a group.
What trends does the first ionization energy follow going across the periodic table?
The correct answer is: The ionization energy increases because there are more protons to pull on the electrons.
