chapters 3 and 4 Flashcards
ionic bonding
the complete transfer of valence electrons
covalent bonding
sharing of electrons
polar bonds
unequal sharing of electrons
general trend of electronegativity
increases going left to right and up a column
VSEPR theory
structures surrounding and atom is determined by minimizing electron pair repulsions
chemical bond
force that holds atoms together
bond energy
required energy to break a bond
bond length
distance where energy is minimal
nonmetallic elements achieve a noble gas configuration by _____ electrons
sharing
metals are _____
cations
nonmetals are _____
anions
cation is generally _____ than parent atom
smaller
anions are generally _____ than parent atom
larger
ion size______ going down a group
increases
ions generally adapt ______ configurations in ionic compounds
noble gas electron
isoelectronic ions
ions containing the same number of electrons
______ protons means ______ attraction and _______ ions
more, greater, smaller
electronegativity
ability of an electron to attract shared electrons to itself
lattice energy
change in energy that takes place when separated gaseous ions are packed together to form an ionic solid
all compounds with _____% or more ionic character are considered to be ionic solids
50
delocalization of electrons
eletrons free to move through entire molecule
as number of shared electrons _____ bond length _____
increases, shortens
energy terms with bond breaking have a ____ sign
positive
energy terms with bond making have a ___ sign
negative
list the exceptions to the octet rule
boron, and any row 3 or lower
resonance
when more than one correct lewis structure can be drawn
formal charge formula
valence-non bonding-bonding/2
valence electron formula
lone pairs+ 1/2(shared electrons)
how to name type 1 compounds
cation first anion 2nd
cation takes name from element
anion named by taking root of element name and adding -ide
how to name type 2 compounds
same as type one
cation first then anion
must specify the charge
add -ide to the end
how to name type 3 compounds
first element named with full name
2nd element named like anion
prefixes for the nunber of atoms
mono prefix not used for first element