Brainscape's Knowledge GenomeTM

Browse over 1 million classes created by top students, professors, publishers, and experts.


See full index

Inorganic Chemistry University > Polyatomic Molecules > Flashcards

Polyatomic Molecules Flashcards

You may prefer our related Brainscape-certified flashcards:
Periodic Table flashcards Chemistry 101 flashcards AP® Chemistry flashcards Organic Chemistry 101 flashcards
1
Q

Molecules with 2 electron pairs around central atom?

A

AX2 Linear 180 degrees

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
2
Q

Molecules with 3 electron pairs around central atom?

A

AX3 Trigonal planar 120 degrees

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
3
Q

Molecules with 4 electron pairs around central atom?

A

AX4 Tetrahedral 109.5 degrees

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
4
Q

Molecules with 5 electron pairs around central atom?

A

AX5 Trigonal bipyramid 120 and 90 degrees

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
5
Q

Molecules with 6 electron pairs around central atom?

A

AX6 Octahedral 90 degrees

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
6
Q

Molecules with 7 electron pairs around central atom?

A

AX7 Pentagonal bipyramidal 72 and 90 degrees

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
7
Q

Three bonding pairs one lone pair?

A

AX3E Trigonal pyramidal 107.8 degrees

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
8
Q

Two bonding pairs one lone pair?

A

AX2E Bent 95 degrees

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
9
Q

Four bonding pairs one lone pair?

A

AX4E See saw/sawhorse 103 degrees

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
10
Q

Three bonding pairs two lone pairs?

A

AX3E2 T shaped 87 degrees

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
11
Q

Five bonding pairs one lone pair?

A

AX5E Square based pyramid 85 degrees

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
12
Q

Four bonding pairs two lone pairs?

A

AX4E2 Square planar less than 90 degrees

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
13
Q

Two bonding pairs two lone pairs?

A

AX2E2 V shapes 104.5 degrees

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
14
Q

One bonding pair three lone pairs?

A

AXE3 Linear

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
15
Q

Hard acids?

A

If a molecules or ion has largely electrostatic, ionic interactions, small or highly charged centre, it will be classed as a hard acid or base, more electronegative an atom the harder it will be
Hard acids prefer to complex with hard bases H+ Mg2+ BF3 Ti4+ Mn+ Fe3+

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
16
Q

Hard bases?

A

F-, OH2, NH3, O2-

17
Q

Soft acids?

A

Largely covalent interactions soft acids or bases, soft-soft interactions are more orbital based and a soft acid would prefer to complex with soft bases
Cu+ Pd2+ Hd2+ Pt2+

18
Q

Soft bases?

A

Br- PH3 BH3 I- CN-

19
Q

Chelate effect?

A

A complex containing 5 or 6 membered rings is more stable than the one without the chelate ring, for example complexes with 3 chelate rings are approximately 2 times more stable than those with six mono dentate ligands, this is a combined kinetic and thermodynamic effect since it is tropically driven. the increase in disorder in the reaction involving the chelate lianas is positive and means this reaction is highly favoured

20
Q

Kf?

A

If Kf is large the ligand binds more tightly to the metal centre than H2O
If Kf is small the ligands bind less tightly than H2O

21
Q

Delta isomers?

A

Right hand screw

22
Q

Lambda isomers?

A

Left hand screw

23
Q

Ligand?

A

Group or atom that gives a metal centre a pair of electrons, normally through an available lone pair

24
Q

Order of repulsion?

A

LP-LP > LP-DB > LP-SB > DB-DB > DB-SB > SB-SB

25
Q

Ligands and charge?

A 
en neutral
pn neutral
biped neutral 
phen neutral
[acac]- 1 minus
[ox]2- 2 minus
dien neutral 
terry neutral 
[edta]4- 4 minus
26
Q

Hard ligands?

A

Small electronegative donor atoms, hard metals carry a high charge or have high charge density, bonding between hard metals and hard ligands has a high degree of ionic character

27
Q

Soft ligands?

A

Soft metals have a lower charge and tend to be larger and more polarisable, ligands that have larger more polarisable donor atoms, the bonding between soft metals and soft ligands has a high degree of covalent character

28
Q

Examples of hard metals?

A

Ti4+ VO2+ Sc3+ Cr3+ Fe3+ Co3+ Cr2+ Mn2+

29
Q

Examples of intermediate metals?

A

Fe2+, Co2+, Ni2+, Cu2+, Zn2+, Rh3+, Ir3+, Ru3+, Os3+

30
Q

Examples of soft metals?

A

Cu+, Ag+, Au+, Pd2+, Cd2+, Pt2+, Hg2+

31
Q

Examples of hard ligands?

A

F-, Cl-, OH-, O2-, NO3-, SO42-, CO32-, H2O, NH3

32
Q

Examples of intermediate ligands?

A

Br-, N3-, NCS-, NO2-, SO32-

33
Q

Examples of soft ligands?

A

H-, R-, CN-, I-, SCN-, CO, PR3, SR2

Inorganic Chemistry University (13 decks)

Brainscape helps you reach your goals faster, through stronger study habits.
© 2024 Bold Learning Solutions. Terms and Conditions