Periodic Trends Section 6.3

Atomic Size Consider the molecule that forms when two atoms of the same element combine Atomic radius = half of the distance between the nuclei of the two atoms Measured in picometers (1012)

Why does this trend occur? 1. Changes in n- As the principal quantum number (n) increases, the outer electrons are farther from the nucleus, so the atoms are larger. 2. Changes in Zeff – As the effective nuclear charge (Zeff = the positive charge felt by an electron) increases, outer electrons are pulled closer to the nucleus, so the atoms are smaller.

1. Down a group, n dominates Elements have one more energy level of inner electrons These shield the outer electrons Atomic radius generally INCREASES in a group from top to bottom

2. Across a period, Zeff dominates Moving across a period, electrons are added to the same outer level Shielding by inner electrons does not change Zeff rises and outer electrons are pulled closer Atomic radius generally DECREASES in a period from left to right

Try the following… Put in order of decreasing atomic size Ca, Mg, Sr K, Ga, Ca Br, Rb, Kr Sr, Ca, Rb

Sr > Ca > Mg K > Ca > Ga Rb > Br > Kr Rb > Sr > Ca

Ions Atom or group of atoms that has a positive or negative charge Form when electrons are transferred between atoms Metals tend to lose electrons, forming cations Nonmetals gain electrons, forming anions

Trends in Ionization Energy Energy needed to remove an electron from an atom Measured when element is in its gaseous state Energy needed to remove the first electron from an atom is the FIRST IONIZATION ENERGY Produces cation with 1+ charge First ionization energy tends to decrease from top to bottom in a group and increases from left to right across a period

Why does this trend occur? As atomic size increases down a group, Zeff has a smaller effect on the electrons in highest level Less energy is needed to remove electron from the energy level making first ionization energy lower

Zeff increases and shielding effect remains constant There is an increase in the attraction the nucleus has for an electron More energy is needed to remove an electron from the atom and first ionization energy is higher

Try these… Put the following in order of decreasing IE1 Kr, He, Ar Sb, Te, Sn K, Ca, Rb I, Xe, Cs

He > Ar > Kr Te > Sb > Sn Ca > K > Rb Xe > I > Cs