12 Questions
What is the definition of atomic radius?
Half the distance between the nuclei of two atoms of the element joined together by a single covalent bond.
What are the two reasons for the decrease in atomic radius across a period?
Increased nuclear charge and the same screening effect.
What are the three reasons for the increase in atomic radius down a group?
Extra energy levels, increased screening, and these offsetting an increase in nuclear charge.
What are the two reasons for the increase in electronegativity across a period?
Increase in nuclear charge and smaller atomic radius.
What are the three reasons for the decrease in electronegativity down a group?
Increase in atomic radius, increased screening effect, and these being more important than an increased nuclear charge.
What is the definition of 1st ionisation energy?
The minimum amount of energy required to remove the most loosely bound electron from 1 mole of gaseous atoms in their ground state.
What are the two reasons for the increase in 1st ionisation energy across a period?
Increased nuclear charge and decreased atomic radius.
What are the two reasons for the decrease in 1st ionisation energy down a group?
Increased atomic radius and increased screening.
Define Second ionisation energy.
The 2nd ionisation energy of an element is the minimum amount of energy required to remove the most loosely bound electron from each singly charged positive ion in a mole of these ions.
How does the increase in atomic radius down a group affect the trend in electronegativity?
The increase in atomic radius reduces the electronegativity, making it less attractive to electrons.
What is the relationship between the 1st ionisation energy and the atomic radius of an element across a period?
As the atomic radius decreases across a period, the 1st ionisation energy increases.
How does the increase in nuclear charge across a period affect the trend in electronegativity?
The increase in nuclear charge increases the electronegativity, making it more attractive to electrons.
Learn about the trends in atomic radius and electronegativity across periods and groups in the periodic table. Understand the factors that affect these trends, including nuclear charge, screening effects, and energy levels.
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