Gen chem 2 Flashcards
rows of the periodic table are called?
periods
columns of the PT are called ?
groups or families
electrons located where have the highest potential energy?
they are located in the valence shell
Offhand, what are the electron configurations for chromium and copper`
for chromium its 4s^1 3d^5
for copper its 4s^1 3d^10
what element is a metal but not considered lustrous and why?
mercury, because its a liquid under standard conditions
name ten qualities of metals, starting with high melting point?
Also what quality about metals do many of these characteristics point to?
high melting point, high densities, malleable, ductile,
Low effective nuclear charge, low electronegativity(high electropositivity), large atomic radius, small ionic radius, low ionization energy, low electron affinity(these qualities point to how metals lose electrons easily
what quality about the valence e-‘s of metals makes them good conductors of heat and electricity
its because their valence electrons are loosely bound to atoms
where are the valence electrons of active metals, transition metals, actinides and lanthanides
s subshell; s and d subshells, s and f subshells
name 9 qualities of nonmetals
brittle high ionization energy high electron affinity high electronegativity(low electropositivity) small atomic radius large ionic radius poor conductors of heat poor conductor of electricity doesn't give up electrons easily
name the metalloids
boron, silicon, germanium, arsenic, antimony, tellurium, polonium, and astatine
how does the positivity of the nucleus increase? and with this what force increases?what charge is known as?
it increases from left to right, because protons increase with atomic number!
also, because this positivity is increasing, the electrostatic attraction between the valence electron shell electrons and the nucleus will increase(this is called the effective nuclear charge)
what is the zeff a measure of? how does zeff increase on the PT?
the zeff is a measure of the net positive charge experienced by the outermost electrons—this pull is done by the inner electrons
-zeff increases from left to right within a period
why are valence electrons held less tightly as you move down a group
this is due to the increased separation between the valence electrons and the nucleus
what is the atomic radius?
how it increase?
atomic radius of an element is equal to one-half of the distance btween the centers of the two atoms of an element that are briefly in contact with each other
atomic radius increases from right to left
what does ionic radius depend on?
it depends on how the element ionizes based on its element type and group number
what does the group number of nonmetals close to the metalloid line tell us?
their group number tells us that they need more electrons than other nonmetals to get to an electronic configuration like the ones the inert gases have
how do metals close to the metalloid line achieve an inert gas like electronic configuration
they need to lose electrons for this to happen
why do metals close to the metalloid line have a greater ionic radius than inert gases?
they do because they lose electrons
what is ionization energy
it is the energy required to remove an electron from a gas species
is removing an electron from an atom exo or endothermic
endo, it always requires energy
what is a reason that valence electrons are tightly bound to an atom
how does this affect the ionization energy
atom has a high zeff, which means that the atom’s valence electrons are close to the nucleus
this makes it difficult to remove electrons and increases their ionization energy
how does ionization energy increase in a period and a group in the PT
goes up from left to right in a period and top to bottom in a group
why are elements in groups 1 and 2 called the active metals
they are called the active metals because they have lo ionization energies
how many electrons in groups 1 and 2 need to lose to get an octet
group 1 needs to lose 1; group 2, 2
