Chemistry chapter 8

Electron configuration

The distribution of electrons among the available subshells of an atom.

Orbital diagrams

Diagrams used to show how the orbitals of a subshell are occupied by electrons.

Pauli’s exclusion principle

No two electrons in an atom can have the same four quantum numbers.

Noble gas core

Inner-shell configuration corresponding to one of the noble gases.

Hund’s rule

The lowest-energy arrangement of electrons in a subshell is obtained by placing electrons into separate orbitals with the same spin before pairing.

Special electron configuration

Cu:[Ar} 4s1 3d10 

Cr:[Ar] 4s1 3d5

Paramagnetic

A substance that is weakly attracted by a magnetic field, typically due to unpaired electrons.

Diamagnetic

A substance that is not attracted by a magnetic field or is very slightly repelled.

Atomic properties; Atomic radius

Period: radius tends to decrease with increasing atomic number

Group: radius increases with the period number

Atomic properties; ionization energies

within any period the value increases as the atomic number goes up; while in the group energy decreases

Atomic properties; electron affinities

The general trend is that the value increases from left to right, though 2A and 5A have smaller affinities, while group 8a has little to no affinity

Values becomes increasingly negative with group number

Atomic properties; effective nuclear charge

The higher the effective nuclear charge the smaller the atom

First ionization energy

The amount of energy required to remove an electron from an atom in the gaseous state, in inorder to create a positive ion.

Electron affinity

The energy required to add an electron to an atom in a gaseous state to form a negative ion.

Acidic oxide

An oxide that reacts with bases.

Basic oxide

An oxide that reacts with acids.

Amphoteric oxide

An oxide that has both basic and acidic properties.

Group 1 elements

Alkali metals (ns^1) become more reactive as you go down the column.

Make basic oxides 

Formula of R2O

Group 2 elements

Alkaline earth metals (ns^2) are reactive but less so than alkali metals; reactivity increases down the group.

Make basic oxides

Formula RO

Group 3 elements (ns^2np^1)

boron is a metalloid, all others are metals

formula of R2O3

boron oxide (B2O3) is acidic

aluminum oxide (Al2O3) and gallium oxide (Ga2O3) are amphoteric

indium oxide (In2O3) and Thallium (Ti2O3) are basic

Group 4 element (ns2^np^2)

Includes Carbon nonmetal, silicon and germanium metalloid, Tin and lead metals

Formula of RO2

Carbon dioxide (CO2), silicon dioxide (SiO2), and germanium dioxide (GeO2) is acidic

Tin dioxide (SnO2) lead(IV) oxide (PbO2) is amphoteric

Group 5 elements

Includes nonmetals (nitrogen, phosphorus), metalloids (arsenic, antimony), and a metal (bismuth)

The empirical formula of R2O3 and R2O5

Molecular formula of R4O6 and R4O10

Nitrogen (N2O3, N2O5), phosphorus (P4O6, P4O10), arsenic (AS2O3, As2O5) are acidic 

Antimony(Sb2O3, Sb2O5) is amphoteric

Bismuth(Bi2O3) is basic

Group 6 elements

Chalcogens (ns^2np^4) include oxygen, sulfur, selenium (nonmetals), tellurium (metalloid), and polonium (metal).

Formula of RO2 and RO3

All except for TeO2 are acidic

PoO2 is amphoteric though more basic than TeO2

Group 7 elements

Reactive non-metals 

The molecular formula of X2 (X is a Halogen)

Generally unstable acidic oxides 

Astatine might be expected to be a metalloid(have a concise half life)

Group 8 elements

Unreactive