15 Questions
Which of the following best describes ionization energy?
The minimum amount of energy required to remove an electron from an atom
What are valence electrons?
Electrons located furthest from the nucleus of an atom
Why are valence electrons the first to be stripped away during ionization?
Because they are influenced the least by the positively charged nucleus
What is the unit of measurement for ionization energy?
Moles
What does the formula for ionization energy represent?
The atom or molecule after being stripped of an electron
What affects the ionization energy of an element?
The number of protons in the nucleus
How is the periodic table organized to show the ionization energy trend?
By number of valence electrons
Which group of elements in the periodic table contains the same amount of valence electrons?
Group 18
What is the trend of ionization energy across a period or row in the periodic table?
Increases from left to right
What is the trend of ionization energy down a group or column in the periodic table?
Decreases from top to bottom
Which element has a stronger positive charge in its nucleus, lithium or fluorine?
Fluorine
What is the relationship between atomic radius and ionization energy?
As atomic radius increases, ionization energy decreases
Which element has a greater positive influence on its outermost electron, lithium or cesium?
Lithium
What is the relationship between the number of electron shells and ionization energy?
As the number of electron shells decreases, ionization energy increases
Which corner of the periodic table requires more energy to strip the outermost electrons?
Top right corner
Test your knowledge on ionization energy and understand its significance in chemistry. Learn about the minimum energy required to remove the outermost electron from an atom and how it relates to valence electrons and the atom's nucleus.
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