Podcast
Questions and Answers
The atomic radius decreases from left to right, causing the outermost electron to be closer to the ______.
The atomic radius decreases from left to right, causing the outermost electron to be closer to the ______.
nucleus
The ionisation energy value ______ as the atomic radius decreases.
The ionisation energy value ______ as the atomic radius decreases.
increases
There is a dip in ionisation energy between ______ and Boron.
There is a dip in ionisation energy between ______ and Boron.
Beryllium
Atoms with half full or completely full outermost sublevels have extra ______.
Atoms with half full or completely full outermost sublevels have extra ______.
Signup and view all the answers
The second ionisation energy refers to the energy needed to remove an electron from an ion with a ______ charge.
The second ionisation energy refers to the energy needed to remove an electron from an ion with a ______ charge.
Signup and view all the answers
A large increase in ionisation energy is observed when removing an electron from the filled n=1 energy ______.
A large increase in ionisation energy is observed when removing an electron from the filled n=1 energy ______.
Signup and view all the answers
Boron has a lower ionisation energy than Beryllium because its outermost shell is only ______ full.
Boron has a lower ionisation energy than Beryllium because its outermost shell is only ______ full.
Signup and view all the answers
The filled outer sublevel requires more energy to remove an electron from it in the ______ energy level.
The filled outer sublevel requires more energy to remove an electron from it in the ______ energy level.
Signup and view all the answers
The atomic radius is defined as half the distance between the nuclei of two atoms of the same element that are joined together by a single covalent ______.
The atomic radius is defined as half the distance between the nuclei of two atoms of the same element that are joined together by a single covalent ______.
Signup and view all the answers
As you move down the groups in the Periodic Table, the atomic radius ______ due to additional energy levels.
As you move down the groups in the Periodic Table, the atomic radius ______ due to additional energy levels.
Signup and view all the answers
The screening effect of the inner electrons reduces the pull of the positive nuclear ______ on the outer electrons.
The screening effect of the inner electrons reduces the pull of the positive nuclear ______ on the outer electrons.
Signup and view all the answers
As we move across a period in the Periodic Table, the atomic radius ______ due to an increase in effective nuclear charge.
As we move across a period in the Periodic Table, the atomic radius ______ due to an increase in effective nuclear charge.
Signup and view all the answers
The first ionisation energy is the minimum energy required to completely remove the most loosely bound ______ from a neutral gaseous atom.
The first ionisation energy is the minimum energy required to completely remove the most loosely bound ______ from a neutral gaseous atom.
Signup and view all the answers
The values of the first ionisation energy decrease down a group in the Periodic Table due to increasing atomic ______.
The values of the first ionisation energy decrease down a group in the Periodic Table due to increasing atomic ______.
Signup and view all the answers
Across a period in the Periodic Table, the ionisation energy values ______ due to increasing effective nuclear charge.
Across a period in the Periodic Table, the ionisation energy values ______ due to increasing effective nuclear charge.
Signup and view all the answers
The element labeled B is ______.
The element labeled B is ______.
Signup and view all the answers
The outermost electrons are somewhat shielded from the attractive force of the positively charged nucleus due to the ______ effect.
The outermost electrons are somewhat shielded from the attractive force of the positively charged nucleus due to the ______ effect.
Signup and view all the answers
The reason for the large decrease in first ionisation energy between elements R and S is that R has a full outer ______.
The reason for the large decrease in first ionisation energy between elements R and S is that R has a full outer ______.
Signup and view all the answers
The first ionisation energy of element H is lower than that of element G because H has a less stable ______.
The first ionisation energy of element H is lower than that of element G because H has a less stable ______.
Signup and view all the answers
Electronegativity is defined as the relative attraction that an atom has for a shared pair of ______ in a covalent bond.
Electronegativity is defined as the relative attraction that an atom has for a shared pair of ______ in a covalent bond.
Signup and view all the answers
H2O and NH3 contain intermolecular ______ bonds.
H2O and NH3 contain intermolecular ______ bonds.
Signup and view all the answers
Alkali Metals are stored under ______ to prevent reactions with oxygen.
Alkali Metals are stored under ______ to prevent reactions with oxygen.
Signup and view all the answers
Moving down the group, Alkali Metals become more reactive with ______.
Moving down the group, Alkali Metals become more reactive with ______.
Signup and view all the answers
Fluorine is the most ______ element of the halogens.
Fluorine is the most ______ element of the halogens.
Signup and view all the answers
Halogens do not exist free in nature and must be extracted from their ______.
Halogens do not exist free in nature and must be extracted from their ______.
Signup and view all the answers
The first ionisation energy is the minimum energy required to remove the most loosely-bound ______.
The first ionisation energy is the minimum energy required to remove the most loosely-bound ______.
Signup and view all the answers
The sharp increase in ionisation energy for removal of the 5th electron indicates it is the first to be removed from the ______ shell.
The sharp increase in ionisation energy for removal of the 5th electron indicates it is the first to be removed from the ______ shell.
Signup and view all the answers
Electronegativity values ______ down the groups in the Periodic Table.
Electronegativity values ______ down the groups in the Periodic Table.
Signup and view all the answers
A line emission spectrum provides evidence for the existence of ______ levels in atoms.
A line emission spectrum provides evidence for the existence of ______ levels in atoms.
Signup and view all the answers
Ionisation energy values for elements increase with ______ atomic number.
Ionisation energy values for elements increase with ______ atomic number.
Signup and view all the answers
As you go down a group, the atomic radius ______, leading to a weaker pull on electrons.
As you go down a group, the atomic radius ______, leading to a weaker pull on electrons.
Signup and view all the answers
The chemical properties of elements are determined by the number of electrons in the ______ energy level.
The chemical properties of elements are determined by the number of electrons in the ______ energy level.
Signup and view all the answers
Alkali metals have very low first ionisation energy values, making them ______ elements.
Alkali metals have very low first ionisation energy values, making them ______ elements.
Signup and view all the answers
Alkali Metals react with water to form the ______ of the metal.
Alkali Metals react with water to form the ______ of the metal.
Signup and view all the answers
The first ionisation energy ______ down the group of alkali metals.
The first ionisation energy ______ down the group of alkali metals.
Signup and view all the answers
All alkali metals react with oxygen to form ______.
All alkali metals react with oxygen to form ______.
Signup and view all the answers
Hydrogen gas is released when alkali metals react with ______.
Hydrogen gas is released when alkali metals react with ______.
Signup and view all the answers
Study Notes
Atomic Radii Trends
- Atomic radius is half the distance between nuclei of two atoms bonded together
- Atomic radius increases down a group because electrons occupy new energy levels further from the nucleus
- Increased screening effect (inner electrons shielding outer electrons) reduces pull from the nucleus
- Atomic radius decreases across a period due to increasing effective nuclear charge
- The nucleus attracts outer electrons more strongly, pulling them closer
- No increase in screening effect across a period
Ionization Energy Trends
- First ionization energy is the minimum energy to remove an outermost electron from a neutral gaseous atom
- Ionization energy decreases down a group due to increasing atomic radius
- Outer electrons are further from the nucleus and experience less attraction
- Increased screening effect reduces attraction between nucleus and outer electrons
- Ionization energy increases across a period due to increasing effective nuclear charge
- Stronger attraction between nucleus and outer electrons needed more energy
Exceptions to General Trends
- Half-filled or filled electron sublevels (especially p-sublevels) lead to increased stability
- Removing an electron from a half-filled or filled sublevel requires more energy
- Example: Nitrogen has higher ionization energy than oxygen
Electronegativity Trends
- Electronegativity is the relative attraction an atom has for shared electrons in a covalent bond
- Electronegativity increases across a period due to increasing effective nuclear charge
- Electrons are closer to the nucleus and experience stronger attraction
- Electronegativity decreases down a group due to increasing atomic radius
- Electrons are further from the nucleus, reducing attraction
Chemical Reactivity of Alkali Metals
- Highly reactive due to low first ionization energy
- Readily lose their outermost electron to form ionic compounds
- Reactivity increases down the group due to decreasing ionization energy
- Easier to remove the outer electron in larger atoms
Chemical Reactivity of Halogens
- Highly reactive nonmetals
- Easily gain an electron to form ionic compounds
- Reactivity decreases down the group due to increasing atomic radius
- Larger atoms have weaker attraction to gain electrons
Studying That Suits You
Use AI to generate personalized quizzes and flashcards to suit your learning preferences.
Related Documents
Description
This quiz covers the trends in atomic radii and ionization energy. You'll learn how these properties change down a group and across a period, including the effects of atomic structure on these trends. Test your understanding of these fundamental concepts in chemistry.
