Ch. 5 - Electron Configuration and Periodic Trends Flashcards
What does the spin magnetic quantum number describe?
The direction of the spin of the electron. (ms)
What are the allowed values for ms?
1/2 or -1/2.
When is a substance diamagnetic?
When all the electrons are paired, they are repelled by magnetic fields.
When is a substance paramagnetic?
When one or more electron is unpaired, they are attracted to magnetic fields.
What is the Pauli exclusion principle?
Only two electrons with opposite spin direction may occupy each orbital.
How many electrons can an s subshell have?
2
How many electrons can a p subshell have?
6
How many electrons can a d subshell have?
10
How many electrons can an f subshell have?
14
What is Hund’s Rule?
Assign one electron to each orbital then go back and add a second electron once all orbitals are half full.
[!] What is the effective nuclear charge?
The amount of positive charge felt by an electron in a given orbital. (Zeff)
What is the periodic trend of effective nuclear charge?
Effective nuclear charge increases with atomic number.
What is the covalent radius?
Half the distance between the nuclei of two identical atoms joined by a single covalent bond.
What is the metallic radius?
Half the distance between the two nuclear of two adjacent atoms in the crystalline solid metal.
What is the van der Waals radius?
Half the distance between the nuclei of two adjacent atoms in a solid sample of noble gas.
What is the periodic trend of atomic radius?
Atomic radius increases from top to bottom and from right to left on the periodic table.
What is first ionization energy?
The energy that must be absorbed in order to remove a valence electron from a neutral atom in the gas phase. (Ei)
What is the periodic trend of the first ionization energy?
First ionization energy increases from bottom to top and from left to right on the periodic table.
What is second ionization energy?
The energy that must be absorbed to remove a valence electron from a cation (+1) in the gas phase. (Ei2)
What is electron affinity?
The energy released when a neutral atom in the gas phase acquired an extra electron in the lowest energy orbital available. (Eea)
What is the periodic trend of electron affinity?
Electron affinity increases from bottom to top and from left to right on the periodic table.
What is electronegativity?
The ability of an element to hold onto its own electrons and attract electrons from other elements. (χ)
What is the periodic trend of electronegativity?
Electronegativity increases from bottom to top and from left to right on the periodic table.
