Unit 1- Trends on the Table Flashcards
Define atomic radius.
A measurement of the size of an atom in picometers.
Define electronegativity.
The relative ability of an atom, when bonded, to attract electrons
Define electron affinity.
The energy change that occurs when an electron is accepted by an atom.
Trend in ionization energy
L-> R
T-> B
Around noble gas
L-> R Increases T-> B Decreases Around noble gas After decreases dramatically
Atomic radius
L-> R
T-> B
Around noble gas
L-> R Decreases T-> B Increases Around noble gas After increases dramatically
Know how to explain using…
The two theories
Zeff and energy levels
Electron affinity
L-> R
T-> B
Around noble gas
L-> R Increases T-> B Decreases Around noble gas At noble gas decreases dramatically to
Electronegativity
L-> R
T-> B
Around noble gas
L-> R Increases T-> B Decreases Around noble gas At noble gas decreases dramatically to 0
Make sure to draw Bohr diagram to aid in explanation
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Define ionization energy.
The amount of energy required to remove an electron from an atom or ion
State and explain trends using Zeff and energy levels for reactivity
reactivity increases from left to right, this occurs because of the increasing Zeff
energy levels do not affect this Trend
decreases dramatically at the noble gas because of the low Zeff
decreases from top to bottom because of the energy level
reactivity of elements versus position on the periodic table lab
metals
decreases left to right
increases top to bottom
non metals
left to right no data
decreases top to bottom
explain why metals lose and nonmetals gain electrons when they react
use Zeff and energy levels
explain why fluorine gains one and not two electrons when it reacts
Zeff and energy levels
explain why magnesium loses two and not three electrons when it reacts
use Zeff and energy levels
