Ch. 8 Periodic Trends Flashcards
What is periodic property?
- A property of an element based on its position on the periodic table
What is the electron configuration?
-Quantum numbers described in shorthand
What is Pauli Exclusion principle?
-No two electrons can have the same set of quantum numbers in a given atom
What is the ascending size of the orbitals?
s<p><f
What is Coulombs Law?
- Interaction between charged particles
i. e. opposites attract and same charges repel
What is the thought process to get out of Coulombs Law?
- As charged particles go apart r becomes increases but energy decreases
- As charges get closer r decreases and energy increases.
What is Shielding?
-Repulsion of one electron that screen an outer orbital from the full effects of the nuclear charge
What is the effective nuclear charge?
-The charge experienced by the outer orbital electrons from the nuclear charge with the shielding of inner electrons
How do you calculate the effective nuclear charge?
Z(eff.) = Z ( charge of nucleus) - (Shielding of electrons)
What is the degenerate?
-All the same energy levels with different orientation
What is Aufbau principle in periodic trend?
-Start from the lowest energy orbital
What is Hands rule with periodic trends?
-When there’s a degenerate orbitals place electron in each before pair 2 electrons
What are the periodic trends for Effective nuclear charge?
- All groups (columns) have the same effective nuclear charge
- Left to right on a periodic table the effective nuclear charge increases
What is the atomic radius?
-The distance form the electron from the nucleus
What occurs to the atomic radius as the principal quantum numbers (n) increase?
-The electrons get further away form the nucleus
What are the periodic trends with atomic radius?
- The atomic radius increases going down periodic tables columns
- Going to the right if n doesn’t change increasing effective nuclear charge decreases atomic radius, since electrons have a greater pull cause for a smaller radius
What is ionization energy?
- The energy required to remove the highest energy electrons from a atom
- Is how easy to make a cation or pull off a valence electron
What are the trend of ionization energy?
- Moving across the P.T. left to right increases I.E.
- Moving down a group decreases ionization energy
Why does moving down a group result in a smaller ionization energy?
- Larger radius going down a column becomes easier to remove the outermost electrons
- Shielding- inner electrons block the attraction force of nucleus becomes more easy to remove an outer electron
-ex) holding a chair with body position away becomes easier for the chair to be removed
What is electronegativity?
-Is how easy it is o give an atom a (-) charge i.e. make antion
What is high electronegativity?
-An atom want an electron
What are the trend on the periodic table with electronegativity?
-Move left to right on P.T. increases in E.N.
What is the rule for transition metals electron configuration?
-The 4s is before the 3d
What is paramagnetic?
-Unpaired electron and attracted to electric field
What is diamagnetic?
-No unpaired electrons and not attracted to a magnetic field
How should the equation for group 1 (alki metal) and group 7 (halogens) be written?
2Metal + Halogen( subscript 2) —> 2(Metal)(Halogen)
How should the equation for group 2 (alki earth metal) and group 7 (halogens) be written?
Metal + (Halogen-subscript 2) –> (Metal)(Halogen-subscript 2)
Why as you move across a P.T. the I.E. increases?
- The atomic radius decreases the outer most electrons are closer to the nucleus
- The effective nuclear charge increases which means there more of an attraction from the outer electron to the nucleus
What is Lattice Energy?
-Energy associated with forming a crystalline lattice from gaseous state
What is electron affinity?
- An atom or ion is the energy change associated with the gaining or an electron by the atom in the gaseous state.
- Atom usually releases energy
