Chp. 7: Periodic Properties of the Elements (first run-through)

periodicity

trends in the periodic table

Effective Nuclear Charge

the net positive charge experienced by an electron in a polyelectronic atom

How is the Effective Nuclear Charge represented in formulas?

Z_^eff

Effective Nuclear Charge Z_eff =

Z - S

What is Z in the formula for the Effective Nuclear Charge, Z_eff = Z - S?

the atomic number

What is S in the formula for the Effective Nuclear Charge, Z_eff = Z - S?

a screening constant, usually close to the number of inner electrons

Effective Nuclear Charge ____ across a period

increases

The Effective Nuclear Charge ____ down a group

increases slightly

When finding the Effective Nuclear Charge, S ___ across a period

does not change

What is the nonbonding atomic radius, or van der Waals radius?

half of the shortest distance separating two nuclei during a collision of atoms

What is another name for the the nonbonding atomic radius? The ___ radius.

van der Waals

What is the bonding ( or covalent) atomic radius?

half of the distance between nuclei in a bond

What is another name for the bonding atomic radius? The ____ radius.

covalent

In an isoelectronic series, ions have the same:

number of electrons

ionization energy

the minimum energy required to remove an electron from the ground state of a gaseous atom or ion

There is a ___ and ___ ionization energy

first ; second

What is the first ionization energy?

the energy required to remove the first electron

What is the second ionization energy?

the energy required to remove the second electron

The higher the ionization energy…

the harder it is to remove an electron

When all valence electrons have been removes, it takes _______ to remove the next electron (a core electron).

a great deal more energy

At ____ and ___, ionization decreases.

3A ; 6A

Electron Affinity

the energy change accompanying the addition of an electron to a gaseous atom

Electron Affinity is typically:

exothermic (and therefore negative for most elements)

All metals are solid at room temperature except:

mercury

Metals have ___ ionization energies

low

Metals have low ionization energies, and they form ____ easily

cations

Nonmetals have _____ electron affinity

large negative

Nonmetals have large negative electron affinity and form ____ easily

anions

Most nonmetal oxides are:

acidic

Most metal oxides are:

basic

Metals (appearance)

shiny luster, various colors, most are silvery

Nonmetals (appearance)

no luster, various colors

Metals (conductivity)

good conductors of heat and electricity

Nonmetals are dull, brittle, and:

poor conductors of heat and electricity

Nonmetals tend to form ____ or ____ in aqueous solutions

anions; oxyanions

Several metalloids are;

semiconductors (ex: computer chips)

Group 1A

alkali metals

Group 2A

alkaline earth metals

Group 6A

oxygen group/chalcogens

Group 7A

halogens

Group 8A

noble gases

Another name for the chalcogens is the ___ group.

oxygen

Alkali metals’ reactions with water are:

famously exothermic

Both alkali metals and alkaline earth metals have low densities, melting points, and ionization energies. Which group has lower measures?

alkali metals

The noble gases have ____ ionization energies.

very large

Noble gases are found as ___ gases

monoatomic