Chemistry

What is ionization energy

An amount of energy needed to remove an outermost electron from an atom.

What is the trend in ionization energy as you go from left to right?
Ionization energy increases as you go left to right in a period/row.

What caused this trend?

(1) Protons are increasing (2) causing coulombic attraction between the protons and electrons to increase (3) which makes it more difficult to remove an electron from an atom (therefore requiring more energy to remove an electron)

What is the trend in ionization energy as you go down a group on the periodic table?

Ionization energy decreases

Describe what is causing this trend that you described in (a)?

(1) The atomic radius increases (more electron shells) as you go down a group meaning that the outermost electrons will be further away from the nucleus. (2) The further an electron is from the nucleus, the less Coulombic Attraction there is between the outermost electrons and the protons in the nucleus. (3) Therefore, it takes less energy (ionization energy) to remove an

electron in that they are less strongly held.

What is an atomic radius?

The distance from the nucleus to the outermost electron shell/orbital.

What happens to atomic radius as you go down a group on the periodic table?

Atomic radius increases

Describe what is causing this trend that you described in (a)?

Atoms have new electron shells/orbitals each time you move down a group on the periodic table causing the atomic radius to increase.

What happens to atomic radius as you go left to right across a period ?

Atomic Radius decreases

Describe what is causing this trend that you described in (a)?

(1) As you go from left to right in a period (row), the number of protons are increasing but the number of electron orbitals are constant. (2) As the number of protons increase, so too does

Coulombic Attraction between the nucleus and the electron orbitals. (3) As a result, the electron orbitals are drawn to the nucleus causing the atomic radius to decrease.

Describe what Coulombic attraction is.

Coulombic attraction is the attractive force between charged particles (such as protons and electrons). 

Describe what Electronegativity is.

 An atom's ability to pull electrons towards itself. 

What is the trend in electronegativity as you go from left to right in a period/row? Electronegativity increases. 

Describe what is causing this trend. 

(1) Protons are increasing (2) Causing coulombic attraction between the protons and electrons to increase (3) Which increases the strength at which an atom pulls electrons towards itself. 

WHAT IS THE TREND IN ELECTRONEGATIVITY AS YOU GO DOWN A GROUP ON THE PERIODIC TABLE?

ELECTRONEGATIVITY DECREASES

DESCRIBE WHAT IS CAUSING THIS TREND THAT YOU DESCRIBED IN (A)?

(1) THE ATOMIC RADIUS INCREASES AS YOU GO DOWN A GROUP CAUSING THE OUTERMOST ELECTRONS TO BE FURTHER AWAY FROM THE NUCLEUS. (2) THE FURTHER AN ELECTRON IS FROM THE NUCLEUS, THE LESS COULOMBIC ATTRACTION THERE IS BETWEEN THE OUTERMOST ELECTRONS AND THE PROTONS IN THE NUCLEUS. (3) THEREFORE THE ATOM WILL HAVE LESS

STRENGTH TO PULL OUTER ELECTRONS TOWARDS ITSELF.