Front

Why does Ionization energy increases across a period from left to right.

Back

Protons added to the nucleus which hold the electrons closer and increasing the amount of energy needed to remove an electron.

Front

Why does Ionization energy decreases down a group.

Back

Valence electrons are further away from the nucleus as energy levels are added thus taking less energy to remove the electron.

Front

Do Valence electrons increase or decrease across a period from left to right.

Back

Valence electrons increase and are the same as the group number (1A = 1 valence electron)

Front

Does Ion size increase or decreases across a period from left to right.

Back

Ion size decreases across a period from left to right because electrons are being pulled closer to the increased positive charge of the nucleus.

Front

Why does Atomic radius increases down a group and decreases across a period.

Back

This trend is due to the increasing number of energy levels as you move down a group and the increasing nuclear charge as you move across a period, which pulls the electrons closer to the nucleus.

Front

Valence electrons increase as you move from left to right across a period in the periodic table.

Back

This trend is due to the increasing nuclear charge, which attracts the valence electrons more strongly.

Front

Why does Electronegativity increase across a period from left to right

Back

As elements gain electrons they get closer to a full outer energy level to become stable. Fluorine only needs one electron to be like the noble gas Neon.

Elements with only a few electrons will give up their electrons. That energy level goes away and the next lower energy level is full.

Front

What is Electronegativity?

Back

Electronegativity is a measure of the tendency of an atom to attract electrons to get a full outer energy level and become stable.

Front

Larger atomic radius of the elements: Fluorine or Nitrogen?

Back

Nitrogen

Front

Element with the highest electronegativity

Back

Fluorine