atomic theory and periodic trends

what is ionization?

the amount of energy it takes to remove an electron.

what is electronegativity?

the amount of energy needed to attract a neighbouring atom’s electron

what is atomic radius

the radius or size of the atom.

top points in her explanation for ionization?

POINT OUT WHICH ELECTRON HAS LESSER OR HIGHER IONIZATION

• talk about valence electrons and how close they are to the protons (the amount of shells)

• weaker attraction due to the distance between protons and valence electrons (for the element with lesser ionization)

• REMEMBER ELEMENTS ON THE RIGHT DO NOT WANT TO GIVE UP ELECTRONS BECAUSE THEY’RE NON METALS AND TEND TO TAKE ELECTRONS TO FINISH THE OCTET THAN GIVE AWAY.

top points in her explanation for electronegativity?

STATE WHICH ELEMENT HAS A HIGHER OR LOWER ELECTRONEGATIVITY

• talk about the amount of shells each one has (the larger the shell, the more repulsion)

• talk about the repulsion due to the amount of electrons it has and the SHIELDING AFFECT

• end with why the other atom has an easier or harder chance to attract (eg. beryllium would be able to attract electrons easily due to this atom having two shells. it’s attractions greater since the neighbouring electrons are closer to the nucleus)

• noble gases are not apart of this because it’s already a full octet (no longer looking for more electrons to attract)

top points in her explanation for atomic radius?

• talk about which element has more or less protons and electrons depending on what the question is asking for (looking at the atomic number)

• explain how more protons and electrons cause a stronger attraction making the atom smaller whereas a weaker attraction makes a larger atom. (eg. Since there is more protons and electrons in aluminum, the attraction between protons and electrons is stronger. Sodium has 11 meaning the attraction is weaker.)