Atomic properties and periodicity Flashcards

1
Q

What is the electrostatic effect like in many-electron atoms?

A

Electrons feel electrostatic attraction to the nucleus and repulsion from other electrons
This means the net attraction to the nucleus is reduced
Each electron is partially shielded

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2
Q

What is the equation to work out effective nuclear charge?

A

= “true” nuclear charge - shielding

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3
Q

What symbol is given to nuclear charge?

A

Z

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4
Q

What symbol is given to effective nuclear charge?

A

Z*

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5
Q

What symbol is given to shielding?

A

σ

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6
Q

Why is the energy to remove the first electron lower than the energy to remove the second?

A

Lower due to repulsion from the second electron and shielding

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7
Q

What are the two effects of penetration of 2s close to the nuclear?

A
  • Increases the nuclear attraction for a 2s electron over that of 2p
  • Decrease the shielding of 2s electrons by 1s electrons
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8
Q

Why is the effective nuclear charge of a 2s electron greater than that of a 2p?

A

2s is more stable

The energy of a 2s orbital is lower than that of a 2p

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9
Q

What does the lobe do and act as?

A

Penetrates and acts as a shield

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10
Q

What does shielding and penetration result in?

A

The splitting of orbitals with the same principle quantum number into different energy leveks

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11
Q

What are Slater’s rules used for?

A

To calculate effective nuclear charge values

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12
Q

What is the first of Slater’s rules?

A

Write the electronconfiguration of the atom and group the orbitals as [1s] [2s,2p] etc, putting s and p together

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13
Q

What are the contributions for total shielding (σ) used by Slater? (Rule 2)

A

0 from all electrons in groups to the right
0.35 from each of the electrons in the same group (ns, np)
0.3 for 1s
0.85 from each electron in the n-1 shell
1 from each electron in lower shells

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14
Q

What is the third of Slater’s rules?

A

The shielding is then subtracted from the nuclear charge (Z) to find the effective nuclear charge (Z*)

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15
Q

Example. Calculate the effective nuclear charge of Mg? Z=12

A

[1s²][2s²,2p⁶][3s²]
= (1x0.35) + (8x0.85) + (2x1) = 9.15
= 12-9.15 = 2.85

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16
Q

What is the effect of Z* on atomic radii?

A

Similar properties down the same group
Increase in the value of n for the highest-energy electrons
Increase in the overall size of the atom

17
Q

What are valence electrons important for?

A

They are responsible for the chemical properties of the atom and are involved in chemical bonding

18
Q

What are the core electrons important for?

A

Act as a shield for valence electrons

19
Q

Why don’t we need to write core electrons in electron configuration?

A

They do not play an important part in bonding or chemistry

20
Q

What is the definition of ionisation energy?

A

Energy required to remove the highest-energy electron from the atom in the gas phase to produce a cation

21
Q

What are the trends down group 1?

A

Small decrease in ionisation energy
Increase in atom size
Similar physical and chemical properties

22
Q

What are the trends across the first row?

A

Z* increases rapidly
Large increase in ionization energy across the row
Decrease in atom size

23
Q

When going down a group, how does Z* increase?

A

Slowly

24
Q

When going across a row, how does Z* increase?

A

Quickly

25
Q

What do bonds to more electronegative atoms become when you go across a row?

A

More covalent

26
Q

What do bonds to more electronegative atoms become when you go down a group?

A

More ionic