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Chem > 13.0 Periodicity > Flashcards

13.0 Periodicity Flashcards

1
Q

Why do the first row of d block elements have similar physical and chemical properties?

A

Relatively small range in atomic radii

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2
Q

Why are the d block elements similar in atomic radii

A

Electron shielding from the 3d level causes a small increases for the effect of increasing nuclear charge on the 4s electrons

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3
Q

Physical properties of Transitional metals

A

-High electrical and thermal conductivity
-High melting point
-malleable
-High tensile strength
-Ductile
-Iron, Cobalt and nickel are ferromagnetic

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4
Q

Why are all the 4s and 3d electrons involved in bonding and form the delocalized sea of electrons

A

The 4s and 3d levels are close in energy

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5
Q

Chemical Properties of Transitional metals

A

-Form compounds with more than one oxidization number
-Form a variety of complex ions
-Form colour compounds
-Acts as catalysts

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6
Q

Why is Zn not a Transitional metal?

A

Zinc does not show properties of transitional metals as it has full 3d level in standard and ionized states.

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7
Q

Why do Transitional metals show multiple oxidization states?

A

Due to successive ionization energy

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8
Q

Why is the successive ionization energy for Transitional metals gradual compared to something like Ca+3

A

the 4s and 3d levels in the transitional metals are closer together, for the calcium the third electron must be removed from the inner 3p level and dictates a huge jump in energy requirement.

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9
Q

What oxidization number is common for Sc to Cr?

A

+3

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10
Q

What oxidization is common past Cr and why?

A

+2, increased nuclear charge of the later elements makes it hard to ionize to +3

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11
Q

What element has the highest oxidization state in transitional metals?

A

manganese, it decreases by -1 after manganese.

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12
Q

What properties do oxidization of transitional metals after +3 show?

A

covalent

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13
Q

What does compounds with high oxidization state tend to be?

A

Oxidizing agents. E.g. potassium dichromate VI

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14
Q

What is a coordinate bond?

A

Covalent bond formed by a lone pair of electrons from one atom

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15
Q

What are lignads?

A

a species that uses a lone pair of electrons to form coordinate bond with the central metal ion

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16
Q

What is a complex?

A

Central ion that is surrounded by molecules or ions which possesses a lone pair of electrons

17
Q

What are ligands in terms of Acid and bases?

A

Lewis bases

18
Q

How are coordination numbers determined?

A

The number of coordinate bonds from the ligands to the central ion

19
Q

Different ligands show what?

A

different colours

20
Q

What shape does a coordination number of 2 show?

A

Linear

21
Q

What shape does a coordination number of 4 show?

A

Square planer, tetrahedral

22
Q

What shape does a coordination number of 6 show?

A

octahedral

23
Q

Why do transition metals show magnetic properties?

A

they contain unpaired electrons

24
Q

Diamagnetism?

A

Very weak magnetic field, has paired electrons

25
Q

Paramagnetism?

A

Has unpaired electrons, stronger than diamagnetism. Magnetic field produced is proportional to the applied field and direction.

26
Q

Feromagnetism?

A

Some times produces magnetic fields greater than the applied field. Stays magnetic. Fe, Co, Ni

27
Q

What are domains in magnetism?

A

unpaired electrons lined up with parallel spin regions

28
Q

what transitional metal is most paramagnetic?

A

Cr

29
Q

Why are transitional metals coloured?

A

Partially filled d electrons

30
Q

What colour is Zn solution?

A

Colourless

31
Q

What happens to d orbital when producing colour?

A

it splits into two sub level

32
Q

Factors Affecting colour

A

Nuclear charge of metal
Charge density of the ligand
Geometry of the complex
number of d electrons/oxidization state

33
Q

When a colour is absorbed which colour is transmitted?

A

the complimentary colour

34
Q

Lower energy on the spectrochemical series equals to?

A

longer wavelength and vice versa.

Chem (12 decks)

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