Periodic Trends Density Atomic and Ionic Radii Chapter 10 Periodic Trends Density Atomic and Ionic Radii

Density

Density Iridium (Z = 77) has the highest density. Why not Meitnerium (Z = 109?) We can predict that an element is more dense if it is closer to Iridium.

Density

Effective Nuclear Charge (Zeff) The effective nuclear charge (Zeff) of an atom is basically how well it is able to hold on to its most loosely held electron.

Atomic radius (radii) The atomic radius is essentially the size of an atom. The largest atom is Francium (Z = 87).

Atomic Radius Xylophone monkey

Rank the atoms from smallest to largest Na, K, O, N O < N < Na < K

Atomic Radius and Effective Nuclear Charge The atomic radius decreases as effective nuclear charge increases.

Effective Nuclear Charge (Zeff) The effective nuclear charge of an atom is primarily determined by: The nuclear charge The shielding effect

The Nuclear Charge (Z) Example: Carbon vs. Nitrogen Which atom would you predict to be smaller?

The Nuclear Charge (Z) Carbon Nitrogen Both atoms are in the 2nd row (period) of the periodic table. What does this tell us?

The Nuclear Charge (Z) Carbon Nitrogen The greater the number of protons in the nucleus the greater the effective nuclear charge.

Conclusion: Nitrogen is a smaller atom than carbon because nitrogen has 7 protons to pull in its two levels of electrons whereas carbon only has 6 protons holding it’s two levels of electrons. Carbon Nitrogen For atoms with the same number of energy levels the greater the number of protons in the nucleus the greater the effective nuclear charge.

The Nuclear Charge (Z) The size of atoms in the same period (row) is determined by the nuclear charge (number of protons in the nucleus).

Xylophone monkey Atomic Radius Nuclear charge explains why atoms get smaller across a period Atomic Radius Xylophone monkey

Shielding Effect. The shielding effect is when electrons between the nucleus and the outermost electrons in an atom shield or lessen the hold of the nucleus on the outermost electrons.

Shielding Effect. Why is He smaller than Ne?

Conclusion: Neon is larger than helium because it has an increased shielding effect from having two energy levels whereas helium only has one energy level. He Ne

Xylophone monkey Atomic Radius Shielding Effect explains why atoms get larger down a group Atomic Radius Xylophone monkey

Chemical Reactivity

Chemical Reactivity

Chemical Reactivity Metals tend to lose electrons when reacting. Large metal atoms are more reactive. Nonmetals tend to gain electrons when reacting. Small nonmetal atoms are more reactive.

Chemical Reactivity F Fr Metals increase in reactivity left and down. Nonmetals become more reactive up and to the right. Most reactive metal is? Most reactive nonmetal is? Fr F

Ionic Radius Ionic Radius is the size of an ion.

Size Change in Ion Formation

Rules for Ionic Radius Anions (negative ions) are “always” larger than cations (positive ions). Ionic Radius goes by the same rules as atomic radius (ions get larger as we move down and to the left). However it is necessary to treat anions and cations separately. (Anions are bigger).

Rank the ions from smallest to largest K+, N3-, Na+, O2- Na+ < K + < O2- < N3-

Homework Worksheet: Density, Atomic and Ionic Radii