Electronic Configuration Flashcards
What is an orbital?
An area of space in which there is a high probability of finding an electron.
What type of shape is an S orbital?
An S orbital is spherical.
Which energy levels have S orbitals?
Every single energy level contains 1 S orbital.
What shape are P orbitals?
P orbitals are like a 3D figure of eight shape
Which energy levels have P orbitals?
Every energy levels except the first level contains 3 P orbitals.
How many electrons can one orbital hold?
Each orbital can hold a maximum of two electrons.
How many electrons can the first energy level hold?
The first energy level can only hold two electrons.
What does the first energy level consist of?
The first energy level is made up from an S sub shell. That sub shell contains 1 S orbital.
How many electrons can the second energy level hold?
The second energy level can only hold 8 electrons.
What does the second energy level consist of?
The second energy level is made up from an S sub shell and a p sub shell.
How many orbitals are in one p sub shell?
One p sub shell contains 3 P orbitals.
How many electrons can the third energy level hold?
The third energy level can hold 18 electrons
What does the third energy level consist of?
The third energy level is made up from an ‘s sub shell’, a ‘p sub shell’ and a ‘d sub shell’.
How many orbitals makes up a d sub shell?
D sub shell is made from 5 d orbitals.
What are the three rules which determine the way in which electrons fill the orbitals?
1) Building principle- electrons always fill the lowest energy orbitals first
2) Hund’s rule- electrons never pair up in the same orbital until all orbitals of the same energy are singly occupied, and all unpaired electrons have parallel spin.
3) Pauli exclusion rule- only two electrons may occupy the same orbital, and they must do so with opposite spin
What are the two ways in which the electron configuration of an atom can be represented?
The arrow and box method
The orbital method
What are the two anomalies in electron configuration?
Chromium- 4s1 3d5
Copper- 4s1 3d10
The electron arrangement in ions is deduced by adding or removing electrons. What are the rules to tell us the order in which they should be removed?
1) remove outer shell electrons first
2) remove P electrons first then S electrons and then D electrons
3) remove paired electrons before unpaired electrons in the same sub-level
What is an orbital?
An area of space in which there is a high probability of finding an electron.
What type of shape is an S orbital?
An S orbital is spherical.
Which energy levels have S orbitals?
Every single energy level contains 1 S orbital.
What shape are P orbitals?
P orbitals are like a 3D figure of eight shape
Which energy levels have P orbitals?
Every energy levels except the first level contains 3 P orbitals.
How many electrons can one orbital hold?
Each orbital can hold a maximum of two electrons.
How many electrons can the first energy level hold?
The first energy level can only hold two electrons.
What does the first energy level consist of?
The first energy level is made up from an S sub shell. That sub shell contains 1 S orbital.
How many electrons can the second energy level hold?
The second energy level can only hold 8 electrons.
What does the second energy level consist of?
The second energy level is made up from an S sub shell and a p sub shell.
How many orbitals are in one p sub shell?
One p sub shell contains 3 P orbitals.
How many electrons can the third energy level hold?
The third energy level can hold 18 electrons
What does the third energy level consist of?
The third energy level is made up from an ‘s sub shell’, a ‘p sub shell’ and a ‘d sub shell’.
How many orbitals makes up a d sub shell?
D sub shell is made from 5 d orbitals.
What are the three rules which determine the way in which electrons fill the orbitals?
1) Building principle- electrons always fill the lowest energy orbitals first
2) Hund’s rule- electrons never pair up in the same orbital until all orbitals of the same energy are singly occupied, and all unpaired electrons have parallel spin.
3) Pauli exclusion rule- only two electrons may occupy the same orbital, and they must do so with opposite spin
What are the two ways in which the electron configuration of an atom can be represented?
The arrow and box method
The orbital method
What are the two anomalies in electron configuration?
Chromium- 4s1 3d5
Copper- 4s1 3d10
The electron arrangement in ions is deduced by adding or removing electrons. What are the rules to tell us the order in which they should be removed?
1) remove outer shell electrons first
2) remove P electrons first then S electrons and then D electrons
3) remove paired electrons before unpaired electrons in the same sub-level
