Chem 214 - Inorganic Chemistry - Steiner

Front 1

What are the properties of metals (electronegativity and conductivity)?

Back 1

Low electronegativites.

Good electrical and thermal conductivity, due to metallic bonding (delocalised electrons).

Front 2

What are the properties of metalloids (electronegativity and conductivity)?

Back 2

Intermediate electronegatvities.

Semiconductors, due to covalent bonds (localised electrons, become partially delocalised at high temp).

Front 3

What are the properties of non-metals (electronegativity and conductivity)?

Back 3

High electronegatvities.

Insulators, molecules with covalent bonds - often large lattices.

Front 4

What electrons can serve as valence electrons?

Back 4

Only S and P electrons.

Front 5

What is the definition of the inert pair effect?

Back 5

The reluctance of heavy p-block elements to share their s-electrons. - especially seen in period 6.

Front 6

What causes the high inertness in the 6s pair?

Back 6

Due to a poorly shielding 4f-subshell and the relativistic effect.

Front 7

Eredox = ?

Back 7

Ereduction - Eoxidation

Front 8

When will a reaction proceed spontaneously?

Back 8

if Ereduction > Eoxidation

Front 9

Structure & Bonding - Metals vs Non-metals

Valence Shell?

Back 9

Metals: Electron-deficient, high energy due to low Zeff.

Non-metals: Electron-rich, low in energy due to high Zeff.

Front 10

Structure & Bonding - Metals vs Non-metals

Bonding?

Back 10

Metals: Valence electrons delocalised across the structure (metallic bonding).

Non-metals: Valence electrons are localised in bonding or non-bonding orbitals (covalent / lone pairs).

Front 11

Structure & Bonding - Metals vs Non-metals

Structure?

Back 11

Metals: Densely packed atoms, non-directional bonds.

Non-metals: Molecular or polymeric, strong directional bonds - hybridization of s & p orbitals.

Front 12

Discrete energy levels are only observed for molecules in the?

Back 12

Discrete energy levels are only observed for molecules in the gas phase

Front 13

Where is pi-bonding most effective?

Back 13

Most effective in the first row of p-block elements, atoms are small and therefore have effective overlap.

Front 14

Why does metallic character decrease down the groups?

Back 14

metallic character decreases down the groups as atoms become larger, weaker bonds - less hybridisation due to less efficient orbital overlap.

Front 15

what are allotropes and why do they occur?

Back 15

Allotropes are different modifications of the same element, can arise from different types of bonding - metallic vs covalent, sigma vs p and directional covalent bonding (which will lead to a different network structure for the same base unit)

Front 16

why is diborane electron deficient?

Back 16

it has too few electrons to form conventional 2-center 2-electron sigma bonds between all its atoms.

(BHB bridges can be described as 3-center-2-electron bonds)

Front 17

What is the type and skeletal electron pair for the formula [BnHn]2-

Back 17

Closo, n+1

Front 18

What is the type and skeletal electron pair for the formula BnHn+4?

Back 18

Nido, n+2

Front 19

What is the type and skeletal electron pair for the formula BnHn+6?

Back 19

Arachno, n+3

Front 20

What do closo clusters only feature?

Back 20

Terminal H-atoms

Front 21

What can nido and arachno clusters contain?

Back 21

Bridging and terminal H-bonds

Front 22

Define bond dissociation energy

Back 22

The measure of strength of an A-B bond; standard reaction enthalpy for the process AB(g) --> A(g) + B(g)

Front 23

Why do homo-nuclear bonds become weaker down the group?

Back 23

There is less efficient orbital overlap between the larger atoms

Front 24

What can the strength of an heteronuclear bond depend on?

Back 24

The polarity of the bond

Front 25

Define electronegativity

Back 25

electronegativity is the power of an atom in a molecule to attract electrons to itself

Front 26

define atomic radius

Back 26

half the length of a homonuclear bond

Front 27

define oxidation state

Back 27

the charge remaining on an atom when all ligands are removed heterolytically in their closed form, electrons are transfered to the more electronegative partner.

Front 28

why are compounds of 2nd and higher row p-block elements highly unstable with unpaired electrons?

Back 28

there outer spx orbitals are fairly directional and are reluctant to form pi bonds

Front 29

what is hyper-valency?

Back 29

p-block atoms with high coordination numbers that violate the octet rule

Front 30

why can some atoms have large coordination numbers?

Back 30

larger atomic radius and polar character of bonds

Front 31

What makes a material ferroelectric?

Back 31

A permanent dipole that can be reversed by application of an external electric field

Front 32

why do chlorides of p-block elements serve as important starting materials for p-block based materials/compounds?

Back 32

they are reactive Lewis Acids

Front 33

what are isoelectronic species?

Back 33

different atoms with the same number of electrons/electronic structure

Front 34

what bonding do Organometallic compounds of s-block metals have? What are they sensitive to?

Back 34

Organometallic compounds of s-block metals are largely ionic; they contain carbanions.They are very air and moisture sensitive and must be stored under inert gas atmosphere.

Front 35

Group 13 organometallics are all ...

handled under?

Back 35

- electron deficient Lewis Acids

- air sensitive

handled under inert conditions

Front 36

How does the Lewis Acidity of Group 13 organometallics change down the group?

Back 36

The acidity of organometallics decreases down Group 13.

Front 37

Oxides and hydroxides of electropositive elements are ___ and show ___ reactions?

Back 37

Oxides and hydroxides of electropositive elements are ionic and show basic reactions?

Front 38

Oxides and hydroxides of electronegative elements are ___ and show ___ reactions?

Back 38

Oxides and hydroxides of electronegative elements are covalent and show acidic reactions?

Front 39

How do you know if an oxide or hydroxide is amphoteric?

Back 39

Oxides/hydroxides of elements at the metal metalloid boundary are amphoteric

Front 40

Why does CCl4 not react with water?

Back 40

It is kinetically stable towards electrophilic attack