Lecture 1 Flashcards
(44 cards)
what promotes bonding?
what types of bonds are there?
what properties are inferred from bonding?
what is the atomic number Z?
protons/neutrons
are electron energy states continuous?
no, they have discrete energy states (so levels)
what is the quantum-mechanical principle
electrons have discrete energy states
what energy level do electrons tend to occupy
the lowest available energy state
(picture of energy states– need to do)- electron energy states
when you form bonds, what electrons are important?
the lower ones are not, they are protected by the outer ones. the outer ones are more loosly bonds and they create bonds and can be moved
what are valence electrons
electrons in the outermost shell (the number)
what shells are the most stable
filled shells
what electrons are the most available for bonding
valence electrons– they try to make bonds and interact
are most elements stable?
no
what is the pauli exclusion principle
there can’t be two electrons in the same energy state (w same spins)
what to remember when identifying the valence electrons in
d is “higher” than s
what properties do valence electrons determine?
chemical
electrical
themal
optical
what side of the periodic table has electropositive elements
left (give up electrons)
what side of the periodic table has electronegative elements
right (want electrons)
are nonmetals on the right or left of the table
right
what does a large electronegativity value suggest
large tendency to acquire electrons
what is the highest value for electroneg
4.0 (on the right)
what is the lowest value for electroneg
0.7 Fr
what are the four primary bonds
ionic, covalent, mixed, and metallic
what are secondary bonds
van der waals
