Ionization Energy MDCAT Quiz: The energy needed to remove an electron from an atom or ion in the gas state is called ionization energy. It is an essential property to understand the reactivity of the elements and, consequently, the major factor in most of the chemical processes. Ionization energy can be used to infer how easy it is for an element to lose electrons to form a positive ion (cation). It is very instrumental in answering some questions from the MDCAT Quiz, especially regarding periodic trends, the reactivity of elements, and the stability of ions.
H2: Trends in Ionization Energy
Ionization energy varies in discernible patterns across the periodic table. Moving from left to right across any period, there is a general increase in ionization energy. This arises because atoms contract with increasing nuclear charge, thus pulling the electrons closer to the nucleus and increasing the difficulty of their removal. However, moving down a group, ionization energy decreases because atomic radii increase, and the outermost electrons are therefore farther from the nucleus and more shielded by inner electrons, making them easier to remove. Finally, elements with few electrons in the outermost shell, such as alkali metals, have low ionization energies; those with a full valence shell, such as the noble gases, have high ionization energies.
H3: Exercise on Ionisation Energy
MDCAT Quiz: Ionization energy will assess the students’ ability to understand periodic trends and the influence of atomic size, nuclear charge, and electron shielding on ionization energy. They can be asked about comparing the ionization energies between different elements or predicting the first ionization energy across periods and groups, which also includes being able to account for exceptions in trends, for example, that the group 2 elements exhibit lower ionization energies compared to group 13. Attempting these MDCAT-style quiz questions is the best practice for students looking forward with confidence to handling ionization energy questions on the actual test.
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H3: Free Flashcard for Ionization Energy
MDCAT students need to learn ionization energy and review flashcards on a daily basis in order to help them memorize important definitions and trends of the topic. With the help of these flashcards, they may quickly recall relevant information regarding this subunit. It serves as a basic tool for them to grasp very challenging concepts and develop an effective methodology of approaching test problems in relation to ionization energy.
Ionization energy is the energy required to remove a(n) ________ from a gaseous atom.
electron
Ionization energy generally ________ as you move across a period from left to right.
increases
Ionization energy generally ________ as you move down a group in the periodic table.
decreases
The ionization energy of a noble gas is ________ compared to that of a halogen.
higher
The first ionization energy is the energy required to remove the ________ electron from an atom.
outermost
Ionization energy ________ when the atomic radius increases.
decreases
The ionization energy of oxygen (O) is ________ than that of nitrogen (N).
higher
Ionization energy is usually expressed in units of ________.
electron volts (eV)
The ionization energy of an atom is inversely related to its ________.
size
Ionization energy ________ as the effective nuclear charge increases.
increases
The second ionization energy refers to the energy required to remove a second ________ from an atom.
electron
The ionization energy of an atom is affected by the ________ of the atom.
atomic radius
The ionization energy of an atom is generally ________ than the electron affinity.
higher
Ionization energy is the energy required to remove an electron from a(n) ________ state.
gaseous
The ionization energy of an atom tends to increase as its ________ increases across a period.
nuclear charge
Ionization energy is higher for ________ atoms because their electrons are closer to the nucleus.
smaller
The ionization energy of lithium (Li) is ________ than that of sodium (Na).
higher
Ionization energy is lower for ________ elements because their electrons are further from the nucleus.
larger atoms
Ionization energy is the energy required to convert an atom into a(n) ________ ion.
positive
The ionization energy of an atom depends on the ________ of its electrons.
energy levels
The ionization energy of an atom is affected by the number of ________ in its electron cloud.
electrons
Ionization energy tends to be lower for elements with a ________ electron configuration.
stable
Ionization energy increases as you move ________ a period.
from left to right
Ionization energy is typically ________ for elements with a low atomic number.
lower
The ionization energy of an atom can be determined by measuring the ________ of the atom.
potential energy
Ionization energy is higher in ________ elements because they have a greater ability to attract electrons.
non-metals
The first ionization energy of an atom is always ________ than the second ionization energy.
lower
Ionization energy is higher for atoms that are ________ in size.
smaller
Ionization energy increases as the ________ of the atom increases within a group.
nuclear charge
The ionization energy of an element is inversely proportional to the ________ of the atom.
size
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