Chapter 8 Flashcards
What is electron configuration?
Shows the particular orbitals that electrons occupy for an atom
How do the arrows in an orbital diagram show the spin of the electron?
An arrow up shows +1/2
An arrow down shows -1/2
What is the Pauli exclusion principle?
States that no two electrons in an atom can have the same four quantum numbers
What does degenerate mean?
Orbitals that all have the same energy
Ex 3s 3p 3d orbitals all have same energy
What is coulomb’s law?
Describes the attractions and repulsions between charged particles
States that the potential energy (E) of two charged particles depends on their charges (q1 and q2) and their separation (r)
What is the equation of Coulomb’s law given energy of charged particles and their charges?
E=1/4piee0 (q1q2/r)
e0=constant
r=separation
Q1 and q2= their charges
How is potential energy affected by like charges?
The potential energy is positive and decreases as the particles get further apart
How is the potential energy affected by opposite charges?
The potential energy is negative and becomes more negative as the particles get closer together
What is shielding in multielectron atoms?
The repulsion of one electron by other electrons
What is penetration in atoms?
Bringing another electron so close to the nucleus that it penetrates the electron cloud and experiences the positive charge of the nucleus
Which has lower energy the 1s orbital or the 1d orbital?
1s
What is the Aufbau Principle?
The pattern of orbital filling
Electrons full atomic orbitals of the lowest available energy levels first
What is Hund’s rule?
States that when filling degenerate orbitals, electrons fill them singly first, with parallel spins
The way of filling orbitals
All arrows up first then add arrows down
What are valence electrons? How do you determine an atoms valence electrons?
Those in the outermost principal energy level
Use the electron configuration and the electrons of the highest n number it has are the valence electrons
1s2 2s2 2p6 3s2 3p2
4 valence electrons
Or by group number
Why do we write the 3d orbital with the 4s orbital?
Because the 4s orbital is lower in energy than the 3d
What are the special cases of electron configuration for CE and Cu?
Cr- 4s1 3d5
Cu- 4s1 3d10
What determines the chemical properties of elements?
Example?
The number of valence electrons they contain
Ex: noble gases have full valence shell and are generally stable
Alkali metals are most reactive since they have 1 valence electron
How is the binding atomic radius defined for metals and nonmetals?
Nonmetals- one half the distance between two of the atoms bonded together
Metals- one half the distance between two of the atoms next to each other in a crystal of the metal
What is the trend in the periodic table for the atomic radii?
Decreases up and to the right of the table
What is the formula for finding the effective nuclear charge?
Zeff=Z-S
Zeff= effective nuclear charge
Z= actual nuclear charge
S= charge shielded by other electrons
What’s the difference between core electrons and outermost electrons in terms of shielding?
Core electrons efficiently shield electrons in the outermost principal energy level from nuclear charge
Outermost electrons do not efficiently shield one another from nuclear charge
When changing the electron configuration of cations and anions what do you take electrons from first if you run out of an energy level?
THE NEXT HIGHEST N NUMBER NOT ENERGY LEVEL
EX: V (AR) 4s2 3d3
V2+ (Ar) 4s0 3d3
What does paramagnetic mean?
If an atom or ion contains unpaired electrons it is attracted by an external magnetic field
One up arrow without a down arrow
What does diamagnetic mean?
An atom or ion in what all electrons are paired and is not attracted to an external magnetic field
All up arrows with down arrows
How are the sizes of atoms affected by cations and anions?
Cations are much smaller than their corresponding atoms
Anions are much larger than their corresponding atoms
What does isoelectric mean?
Ions with the same number of electrons
Why are not all isoelectric ions the same size?
Because some have more protons resulting in a stronger positive mass pulling on the same amount of electrons
What is ionization energy? What is it’s trend across the periodic table?
The energy required to remove an electron
Always positive
Increases up the periodic table and to the right
What is the difference between forst ionization and second ionization energy?
First is the energy to remove the first electron
Second is the energy to remove the second and is much larger
What is the electron affinity? What is it’s trend on the periodic table?
The energy change associated with the gaining of an electron by the atom in gaseous state
Usually negative
Increases (negatively) to the right and up the periodic table
What is metallic character? What is it’s trend on the periodic table?
The properties associated with metals
Decreases to the right and up the periodic table
What is the rule when dealing with atomic radii with elements with the same amount of electrons?
The greater the ionic charge, the smaller the ionic radii
