Ch. 7 Flashcards
Valence Orbital
The occupied orbital that hold the electrons involved in bonding
what can electron configuration be used for
to see the similarities and differences in properites of elements
the majority of elements in nature are found as
compounds
the pull between the electrongs and the nucleus depends on:
the magnitude of the nuclear charge and the distance between them
effective nuclear charge (Zeff)
comes from a single positive charge at the nucleus
how do the inner electrons effect the outer electrons
they shield them from the nucleus
Zeff equation
Zeff = Z - S
z-atomic number
s-shielding
where does Zeff increase on the periodic table?
left to right across a period
increase going down a column
atomic radius
the distance separating the nuclei when two atoms are bonded to each other
bonding atomic radius
is equal to half of the nucleus to nucleus distance (d)
what does knowing atomic radii allow us to estimate
bond length in molecules
atomic radius increase from
top to bottom and right to left
the size of an electron depends on
its nuclear charge, # of electrons, and the orbital the valence electrons are in
cations are _______ then their parent atoms
smaller
anions are ______ then their parent atoms
bigger
Isoelectronic series
a group of ions containing the same number of electrons
ionic radius _____ when the nuclear charge ______
decreases ; increases
Ionization Energy
the energy needed to remove an electron
First Ionization Energy
the energy needed to remove the first electron
the greater the ionization energy:
the harder to remove an electron
Ionization energy _______ as you remove electrons
increases
the greatest ionization energy occurs when
an inner electron is taken
removed electrons are always removed from
the occupied orbitals with the largest principal quantum number
electron affinity
how much energy is released from stealing an electron
Metallic character
how much an element exhibits the physical and chemical properties of metals
Metallic character _____ down a group and _____ from right to left
increases ; decreases
Metals Characteristics:
- shiny luster
- conduct heat and electricity
- malleable and ductile
- solid at room temp.
- melt at high heats
- low ionization energies
- form cations
- oxidize in chemical reactions
most metal oxides are
basic
