The Do's and Don'ts of Teaching Periodic Trends

Nuclear charge increases the attraction of the nucleus and therefore pulls the electron cloud closer to the nucleus resulting in smaller atomic radius

Atomic radius decrease as atomic numbers increase in any given period

Increase number of energy levels increases the distance over which the nucleus must pull in there for reduce the attraction for electrons

Atomic radii increase as atomic number increases down a column or group

Full energy levels provide some shielding between the nucleus and valence electrons

Atomic radii increases atomic number increases down a column or group

Effective nuclear charge increases the attraction of the nucleus and therefore holds the electrons more tightly

Ionization energy increases as atomic number increases in any given.

A drop in ionization energy occurs between groups two and three the p electrons do not penetrate the nuclear region as greatly as s electrons doing are therefore not as held tightly

Ionization energy increases an atomic number increases in any given.

A drop and ionization energy occurs between groups four and five because they increase proportion created by the first pairing of electrons always the increase in nuclear charge and thus less energy is required to remove the electron

Ionization energy increases the atomic number increases in any given.

Increased number of energy levels increases the distance over which the nucleus must pull and therefore reduces the attraction for electrons

Ionization energy decreases as atomic number increases down a column or group

Full energy levels provide some shielding between the nucleus and valence electrons

Ionization energy decreases as atomic number increases down a column or group

Effective nuclear charge increases the attraction of the nucleus and therefore it's strengthens the attraction for the electrons

Electronegativity increases as atomic number increase in any given period

Increase number of energy levels increases the distance over which the nucleus must pull in there for reduces the attraction for electrons

Electronegativity decreases as atomic number increases down a column or group

Full energy levels provide some shielding between the nucleus and valence electrons

Electric negativity decreases as atomic number increases down a column or group

Positive metal ions result from the loss of valence electrons. In many cases this means the farthest electrons are now in a small Principle Energy level then the original neutral atom

Positive ions are smaller than their respective neutral atoms

To address the ratio of protons to electrons electrons are the loss ratio of protons over electrons increases and thus the electrons are how closer and with more strength

Positive ions or smaller than their respective neutral atoms

Negative nonmetal ions result from the addition of valence electrons the primary explanation is the change in the proton up to electron ratio as electrons are added the proton electron ratio decreases and the electrons are not as closely held

Negative ions or smaller than their respective neutral atoms

Because metals react by losing electrons or loosely held electron was result in a more reactive metal this is directly tied to ionization energy with an increased number of energy levels comes increased distance from the nuclear attraction and thus a more loosely held electron available for reacting

Metals are more reactive as you move down a column

Because nonmetals tend to gain electrons as strong nuclear attraction result in a more reactive nonmetal. This means that an atom with the highest nuclear charge and the least number of energy levels should be the most reactive nonmetal (F) because it's nucleus exerts the strongest pull

Nonmetals are more reactive As you move up a column