Periodic Trends 5 Flashcards
As you _ atomic radius decreases
Move across a period from left to right
Why atomic radius decreases when you move from left to right of a period
The effective nuclear charge increases as electrons are added to the energy level
As electrons are added to the energy level which is
The same distance from the nucleus
Atomic radius increases from top to bottom in a group as
The effective nuclear charge decreases
Effective nuclear charge decreases due to
More electrons in more energy levels
Magnesium has a larger atomic radius (is bigger) than
Chlorine
Magnesium is bigger than chlorine because
It is to the left on periodic table
Magnesium has 12 protons and _ neutrons
12
Chlorine has 17 protons and _ neutrons
18
Ionic radius is the distance between the center of
The nuclei of two ions that barely touch
Ionic radius increases for
Nonmetals moving across a period
Effective nuclear charge definition
Force of attraction exerted by the protons
Ionic radius increases for nonmetals moving across a period because
Effective nuclear charge decreases as number of electrons exceeds number of protons
For a neutral atom _ are equal (2)
Atomic radius
Ionic radius
Ionic radius increases as
Ion gains electrons
In atoms that have a charge _ are unequal
Atomic radius
Ionic radius
Ionic radius _ for metals moving left to right across a period
Decreases
Reason why metal’s ionic radius decreases from left to right
Because they lose elections (effective nuclear charge increases)
The greater the nuclear charge, the more power being used to
Pull the electrons more tightly together
IE stands for
Ionization energy
Ionization energy is the energy required to remove one or more electron from _
A neutral atom in the gas phase
Not all atoms can _
Give up electrons easily
In materials that hold electrons loosely the _ is relatively easy to pull off
Electron that is farthest from the nucleus
IE decreases from _ to _ in a group
Top
Bottom
As you move down a group, size increases as
Electrons are added in energy levels farther from the nucleus
The bigger the atoms, the less
Ionization energy is needed to pull the electrons off
Farther away electrons are from nucleus, (bigger atom)
The weaker the attraction of the nucleus
IE increases going from _ to _ across the periodic table
Left
Right
As you move across a period, the effective nuclear charge increases as ()
Electrons are added at the same distance from the nucleus (making it harder to remove electrons)
