Unit 6 - Quiz 1 Flashcards
What is electron shielding
The blocking of valence electron attraction by the nucleus due to the presence of inner shell electrons
Why is electron shielding important in determining trends in the periodic table
It is a factor in determining why and how the atomic radius trends are the way they are. It also determines the influence of the nucleus to the valence electrons
How is atomic radius measured
From the Nucleus to the outermost electron
What units are units are used to measure atomic radius
Picometers (pm)
What does atomic radius determine
The side of the atom
What is the periodic trend for atomic radius and why
Atomic radius decreases from left to right
Die to the increase in the number of protons, so greater force is pulling electrons closer to the nucleus
What is the group trend for atomic radius and why
Atomic radius increase from top to bottom
Due to the added energy level and shielding effect
What is Ionization energy
The amount of energy required to remove an electron from an atom in its gaseous state
It requires more energy to remove each successive electron
What is the periodic trend for ionization energy and why
Ionization increase from left to right
Atomic size is decreasing (more attraction) so harder to remove an electron
What is the group trend for ionization energy and why
Ionization energy decreases from top bottom
Atomic size in increasing (less attraction) so easier to remove electron
What is Electronegativity
Ability of an atom in a compound to attract electrons
What is the periodic trend for Electronegativity
Electronegativity increase as you move left to right
What is the group trend for Electronegativity
Electronegativity decrease as you go down a column
What are Ions
An atom or group of atoms that have a positive or negative charge
How do ions form
When electrons are transferred between atoms
