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Subshells & orbitals
Subshells & orbitalsSubshells & orbitals
The ionisation energy graph does not increase steadily across a period
The ionisation energy graph does not increase steadily across a period
The ionisation energy graph does not increase steadily across a period
The small decreases are due to sub-shells or sub-energy levels
The ionisation energy graph does not increase steadily across a period
The small decreases are due to sub-shells or sub-energy levels
The ionisation energy graph does not increase steadily across a period
The small decreases are due to sub-shells or sub-energy levels
This means there are different energy levels within one energy level
The ionisation energy graph does not increase steadily across a period
The small decreases are due to sub-shells or sub-energy levels
This means there are different energy levels within one energy level
The ionisation energy graph does not increase steadily across a period
The small decreases are due to sub-shells or sub-energy levels
This means there are different energy levels within one energy level
All electrons in the same subshell have the same energy
The ionisation energy graph does not increase steadily across a period
The small decreases are due to sub-shells or sub-energy levels
This means there are different energy levels within one energy level
All electrons in the same subshell have the same energy
The ionisation energy graph does not increase steadily across a period
The small decreases are due to sub-shells or sub-energy levels
This means there are different energy levels within one energy level
All electrons in the same subshell have the same energy
The sub-shells are labelled s, p, d and f
The ionisation energy graph does not increase steadily across a period
The small decreases are due to sub-shells or sub-energy levels
This means there are different energy levels within one energy level
All electrons in the same subshell have the same energy
The sub-shells are labelled s, p, d and f
The ionisation energy graph does not increase steadily across a period
The small decreases are due to sub-shells or sub-energy levels
This means there are different energy levels within one energy level
All electrons in the same subshell have the same energy
The sub-shells are labelled s, p, d and f Sub-shell energy levels: s < p < d < f
The ionisation energy graph does not increase steadily across a period
The small decreases are due to sub-shells or sub-energy levels
This means there are different energy levels within one energy level
All electrons in the same subshell have the same energy
The sub-shells are labelled s, p, d and f Sub-shell energy levels: s < p < d < f
Each shell or energy level has one more sub-shell than the previous one
Each shell or energy level has one more sub-shell than the previous one
Each shell or energy level has one more sub-shell than the previous one
1st shell 1s 2nd shell 2s 2p 3rd shell 3s 3p 3d 4th shell 4s 4p 4d 4f
Each shell or energy level has one more sub-shell than the previous one
1st shell 1s 2nd shell 2s 2p 3rd shell 3s 3p 3d 4th shell 4s 4p 4d 4f
Each sub-shell has a maximum number of electrons it can hold.
Each sub-shell has a maximum number of electrons it can hold.
Each sub-shell has a maximum number of electrons it can hold.
Each sub-shell has a maximum number of electrons it can hold.
s sub-shell 2 electrons
p sub-shell 6 electrons
d sub-shell 10 electrons
f sub-shell 14 electrons
Each sub-shell has a maximum number of electrons it can hold.
Hence the 2nd energy level with an s sub-shell (2 electrons) and a p sub-shell (6 electrons) can hold a total of 8 electrons.
Each sub-shell has a maximum number of electrons it can hold.
Hence the 2nd energy level with an s sub-shell (2 electrons) and a p sub-shell (6 electrons) can hold a total of 8 electrons.
s sub-shell 2 electrons
p sub-shell 6 electrons
d sub-shell 10 electrons
f sub-shell 14 electrons
Electron Arrangement & Electronic ConfigurationElectron Arrangement & Electronic Configuration
The arrangement of electrons when written in shells or energy levels such as 2 , 9 , 1 is called the electron arrangement
The arrangement of electrons when written in shells or energy levels such as 2 , 9 , 1 is called the electron arrangement
Electron Arrangement & Electronic ConfigurationElectron Arrangement & Electronic Configuration
The arrangement of electrons when written in shells or energy levels such as 2 , 9 , 1 is called the electron arrangement
The writing of the organisation of the electrons in sub-shells (e.g. 1s2 2s2 2p3) is called the electronic configuration
The arrangement of electrons when written in shells or energy levels such as 2 , 9 , 1 is called the electron arrangement
The writing of the organisation of the electrons in sub-shells (e.g. 1s2 2s2 2p3) is called the electronic configuration
List of subshells containing electronsList of subshells containing electrons
Electronic ConfigurationElectronic Configuration
List of subshells containing electronsWritten in order of increasing energy
List of subshells containing electronsWritten in order of increasing energy
Electronic ConfigurationElectronic Configuration
List of subshells containing electronsWritten in order of increasing energySuperscripts give the number of electrons
List of subshells containing electronsWritten in order of increasing energySuperscripts give the number of electrons
Electronic ConfigurationElectronic Configuration
List of subshells containing electronsWritten in order of increasing energySuperscripts give the number of electrons
Example: Electron configuration of neon number of electrons
1s2 2s2 2p6
main shell subshell
List of subshells containing electronsWritten in order of increasing energySuperscripts give the number of electrons
Example: Electron configuration of neon number of electrons
1s2 2s2 2p6
main shell subshell
Electronic ConfigurationElectronic Configuration
Filling sub-shellsFilling sub-shells
The order of filling the sub-shells becomes more complex at higher energy levels as the energy levels/shells start to overlap
From itl.chem.ufl.edu/2045_s00/lectures/lec_11.html
The order of filling the sub-shells becomes more complex at higher energy levels as the energy levels/shells start to overlap
From itl.chem.ufl.edu/2045_s00/lectures/lec_11.html
To help you rememberTo help you remember
From: itl.chem.ufl.edu/2045_s00/lectures/lec_11.html
Writing Electronic ConfigurationsWriting Electronic Configurations
You need to be able to write electronic configuration for the first 54 elements
E.g. H(1) 1s1
Li(3) 1s2 2s1
Ne(10) 1s2 2s2 2p6
Na (11) 1s2 2s2 2p6 3s1
You need to be able to write electronic configuration for the first 54 elements
E.g. H(1) 1s1
Li(3) 1s2 2s1
Ne(10) 1s2 2s2 2p6
Na (11) 1s2 2s2 2p6 3s1
Write out electronic configurations for:
Be, O, Mg, P, Cl, Mn, Zn. Ge, Br, Sr, Ag and I.
Write out electronic configurations for:
Be, O, Mg, P, Cl, Mn, Zn. Ge, Br, Sr, Ag and I.
AnswersAnswers Be - 1s2 2s2 O - 1s2 2s2 2p4
Mg - 1s2 2s2 2p6 3s2 P - 1s2 2s2 2p6 3s2 3p3 Cl - 1s2 2s2 2p6 3s2 3p5 Mn - 1s2 2s2 2p6 3s2 3p6 4s2 3d5 Zn - 1s2 2s2 2p6 3s2 3p6 4s2 3d10 Ge - 1s2 2s2 2p6 3s2 3p6 4s2 3d10 4p2
Br - 1s2 2s2 2p6 3s2 3p6 4s2 3d10 4p5 Sr - 1s2 2s2 2p6 3s2 3p6 4s2 3d10 4p6 5s2 Ag - 1s2 2s2 2p6 3s2 3p6 4s2 3d10 4p6 5s2 4d9 I - 1s2 2s2 2p6 3s2 3p6 4s2 3d10 4p6 5s2 4d10 5p5
Be - 1s2 2s2 O - 1s2 2s2 2p4
Mg - 1s2 2s2 2p6 3s2 P - 1s2 2s2 2p6 3s2 3p3 Cl - 1s2 2s2 2p6 3s2 3p5 Mn - 1s2 2s2 2p6 3s2 3p6 4s2 3d5 Zn - 1s2 2s2 2p6 3s2 3p6 4s2 3d10 Ge - 1s2 2s2 2p6 3s2 3p6 4s2 3d10 4p2
Br - 1s2 2s2 2p6 3s2 3p6 4s2 3d10 4p5 Sr - 1s2 2s2 2p6 3s2 3p6 4s2 3d10 4p6 5s2 Ag - 1s2 2s2 2p6 3s2 3p6 4s2 3d10 4p6 5s2 4d9 I - 1s2 2s2 2p6 3s2 3p6 4s2 3d10 4p6 5s2 4d10 5p5
Shorthand Electronic ConfigurationsShorthand Electronic Configurations
To save writing out all the lover level configurations, it can be shortened by building on the last noble gas configuration
E.g. Na 1s2 2s2 2p6 3s1 or [Ne] 3s1
or K 1s2 2s2 2p6 3s2 3p6 4s1 or [Ar] 4s1
To save writing out all the lover level configurations, it can be shortened by building on the last noble gas configuration
E.g. Na 1s2 2s2 2p6 3s1 or [Ne] 3s1
or K 1s2 2s2 2p6 3s2 3p6 4s1 or [Ar] 4s1
Shorthand Electronic ConfigurationsShorthand Electronic Configurations
To save writing out all the lover level configurations, it can be shortened by building on the last noble gas configuration
E.g. Na 1s2 2s2 2p6 3s1 or [Ne] 3s1
or K 1s2 2s2 2p6 3s2 3p6 4s1 or [Ar] 4s1
For all elements on the previous slide, write their electronic configurations in the shorthand form
To save writing out all the lover level configurations, it can be shortened by building on the last noble gas configuration
E.g. Na 1s2 2s2 2p6 3s1 or [Ne] 3s1
or K 1s2 2s2 2p6 3s2 3p6 4s1 or [Ar] 4s1
For all elements on the previous slide, write their electronic configurations in the shorthand form
OrbitalsOrbitals
A 3-dimensional shape/area outside the nucleus where there is a high probability that electrons can be found
s orbitals are spherical in shape p orbitals are shaped like a peanut d orbitals are doughnut-shaped
A 3-dimensional shape/area outside the nucleus where there is a high probability that electrons can be found
s orbitals are spherical in shape p orbitals are shaped like a peanut d orbitals are doughnut-shaped
From: www.chem.queensu.ca/.../orbitals/index.htm
Filling OrbitalsFilling Orbitals Each orbital can contain a maximum of 2
electrons with opposite spins This can be shown diagrammatically using
either lines or boxes and arrows -
Each orbital can contain a maximum of 2 electrons with opposite spins
This can be shown diagrammatically using either lines or boxes and arrows -
From: http://www.xmission.com/~seldom74/chem1110int/ch03/03i.htm
Hund’s ruleHund’s rule
This diagram is also based on Hund’s Rule Orbitals within the same subshell are filled
singly first This reduces the amount of repulsion by
having two electrons in the same orbital
This diagram is also based on Hund’s Rule Orbitals within the same subshell are filled
singly first This reduces the amount of repulsion by
having two electrons in the same orbital
QuestionQuestion
Draw diagrams using lines to represent orbitals and arrows for electrons to represent:
a. F
b. Na
c. P
d. S
e. Ar
f. Al
Draw diagrams using lines to represent orbitals and arrows for electrons to represent:
a. F
b. Na
c. P
d. S
e. Ar
f. Al
Aufbau PrincipleAufbau Principle
The writing of electronic configurations is based on the Aufbau Principle, which states that orbitals with the lowest energy are filled first
The writing of electronic configurations is based on the Aufbau Principle, which states that orbitals with the lowest energy are filled first
Electronic Configuration & the Periodic Table
Electronic Configuration & the Periodic Table
The structure of the periodic table is related to the subshell electronic configuration
s block has s1 or s2 in its outer shell p block have p1 to p6 in their outer shell Transition metals have d1 to d10 in their
second last shell From the electronic configuration can work
out the group and period
The structure of the periodic table is related to the subshell electronic configuration
s block has s1 or s2 in its outer shell p block have p1 to p6 in their outer shell Transition metals have d1 to d10 in their
second last shell From the electronic configuration can work
out the group and period
From: http://www.xmission.com/~seldom74/chem1110int/ch03/03i.htm
QuestionQuestion
What period, block and group are the following elements in?
a. 1s2 2s2 2p1
b. 1s2 2s2 2p6 3s2
c. 1s2 2s2 2p6 3s2 3p6 4s1
d. 1s2 2s2 2p6 3s2 3p6 4s2 3d5
What period, block and group are the following elements in?
a. 1s2 2s2 2p1
b. 1s2 2s2 2p6 3s2
c. 1s2 2s2 2p6 3s2 3p6 4s1
d. 1s2 2s2 2p6 3s2 3p6 4s2 3d5
QuestionQuestion
What period, block and group are the following elements in?
a. 1s2 2s2 2p1 Period 2, p block, Group 3
b. 1s2 2s2 2p6 3s2 Period 3, s block, Group 2
c. 1s2 2s2 2p6 3s2 3p6 4s1 Period 4, s block, Group 1
d. 1s2 2s2 2p6 3s2 3p6 4s2 3d5 Period 4, d block, transition metals
What period, block and group are the following elements in?
a. 1s2 2s2 2p1 Period 2, p block, Group 3
b. 1s2 2s2 2p6 3s2 Period 3, s block, Group 2
c. 1s2 2s2 2p6 3s2 3p6 4s1 Period 4, s block, Group 1
d. 1s2 2s2 2p6 3s2 3p6 4s2 3d5 Period 4, d block, transition metals
