DRAFT Chemistry Chapter 8: Electron Configuration and Chemical Periodicity

These will be the bold terms only - STOPPED AT PAGE 3

What are the four quantum numbers that each electron in any atom is completely described by

The first three quantum numbers (n,l, and m) describe the orbital, while the fourth quantum (m_s ) describes electron spin.

What principle states that no two electrons in the same atom can have the same four quantum numbers?

It is the pauli exclusion principle

An atomic orbital can hold….. and they must have….

They can hold a maximum of two electrons and must have opposing spins

Do electrons in the same or inner energy level shield each other to some extent?

Electrons in the same energy level

Do electrons in the same or inner energy level shield each other very effectively?

Electrons in the inner energy levels

Each energy level is split into sublevels of differing energy, how is this splitting caused by?

It is caused by by penetration and its effect on shielding

For a given n value, a lower l value indicates..

It indicates a lower energy sublevel

What is the order of sublevel energies?

s < p < d < f

What is electron configuration?

It is the distribution of electrons within the levels and sublevels of an atom.

What does the Aufbau principle specify?

It specifies that electrons are always placed in the lowest energy sublevel available

What does Hund’s rule specify?

It specifies that when orbitals of equal energy are available, the lowest energy electron configuration has the maximum number of unpaired electrons with parallel spins

What diagram shows only the highest energy sublevels being filled?

It is a partial orbital diagram

What configuration has the has the element symbol of the previous noble gas in square brackets?

It is a condensed electron configuration

Which electrons are those an atom has in common with the previous noble gas and any completed transition series.

It is inner (core) electrons

What electrons are the those in the highest energy level (highest n value)

It is outer electrons

Which electrons are those involved in forming compounds?

It is valence electrons

What types of elements have the valence electrons as the outer electrons

It is the main group elements

What type of element have the valence electrons include the outer electrons and any (n − 1)d electrons

It is the transition elements

What is the metallic radius?

It is ½ of the shortest distance between nuclei of adjacent, individual atoms in a crystal of a metal

What is the covalent radius?

It is ½ of the shortest distance between nuclei of identical, covalently bonded atoms. Use for nonmetals.

As the atomic size increases, what happens to the principal quantum number (n)?

It increases

• As n increases, the probability that the outer electrons will be farther from the nucleus increases.

As the atomic size decreases, what happens to the effective nuclear charge

It increases

• As Z_eff increases, the outer electrons are pulled closer to the nucleus

The atomic size increases down a group in the periodic table and decreases across a period applies to what group of elements?

For main group elements

What is Ionization energy (IE)?

It is the energy required for the complete removal of 1 mol of electrons from 1 mol of gaseous atoms or ions

Atoms with a low IE tend to form…

tend to form cations (+)

Atoms with a high IE tend to form…

tend to form anions (-)

What does ionization energy tend to do across groups and periods?

It tends to decrease down a group and increase across a period

What is Electron Affinity (EA)?

It is the energy change that occurs when 1 mol of electrons is added to 1 mol of gaseous atoms or ions

What is the behavior pattern for IE and EA for reactive nonmetals

These elements have high IEs and highly negative EAs.

• These elements attract electrons strongly and tend to form negative ions in ionic compounds.

What is the behavior pattern for IE and EA for reactive metals

These elements have low IEs and slightly negative EAs

• These elements lose electrons easily and tend to form positive ions in ionic compounds

What is the behavior pattern for IE and EA for noble gases

These elements have very high IEs and slightly positive EAs.

• These elements tend to neither lose nor gain electrons

Are metals, nonmetals, or metalloids easily oxidized?

Metals

What group of metals are strong reducing agents?

(LEO/GER)

With their low IEs and small EAs, the Group 1 and Group 2 metals lose electrons readily, so they are _________ and become oxidized.

What group of metals are strong oxidizing agents?

(LEO/GER)

With their high IEs and large EAs, the Group 16 and Group 17 nonmetals gain electrons readily, so they are __________ and become reduced

Main-group metals form _______, which are _______ in aqueous solution

ionic oxides, basic

Main-group nonmetals form ________, which are _____ in aqueous solution.

covalent oxides, acidic

Some metals and metalloids from amphoteric oxides, what is the behavior of amphoteric oxides?

They can act as acids or bases in water