Chapter 9 Bonding Flashcards
__________ ___________ are the outer shell electrons of an atom that determines an element’s __________
valence electrons, chemistry
compared with nonmetals, the number of valence electrons in metals is generally
smaller
________ _________ are almost completely unreactive due to _________ __________
noble gases, electron configuration
Main group (A) elements tend to _______ or ________ electrons to become isoelectronic
gain or lose
isoelectronic means same __________ _________ configuration as nearest noble gas)
valence electron
recall that the 4s orbital fills _______ the 3d orbital in the first row of transition metals
before
electrons are always lost from the ______________
highest n value
two or more species having the same ___________ but different ____________ is called isoelectronic series
electronic configuration, nuclear charges
an _________ __________ is a series of two or more species that have _________ electron configurations but _________ nuclear charges
isoelectronic series, identical, different
according to ___________ atoms will gain, lose, or share electrons to acquire eight valence electrons. except for ______
octet rule, hydrogen
during ionic bond formation, electrons are _________ from one atom to another
transferred
in ionic bonds, metals _______ electrons
lose
in ionic bonds, nonmetals __________ electrons
gain
during covalent bond formation, electrons are ________ between two atoms.
shared
Shared electrons are available to _______ bonding atoms
both
sharing leads to _____________ around each atom
8 valence electrons
shared electrons =
bonds
non-bonding valence electrons=
lone pairs
electronegativity is a measure of the tendency of an atom to ________ bonding electrons to itself when it is in a molecule
attract
the higher the electronegativity (EN) value of an atom in a molecule, the more ________ it attracts the electrons (more e- hungry) in a ___________
strongly, covalent bond
The difference in EN values makes sharing ________ in a __________
unequal, covalent bond
Electronegativity increases from _________________ across a ______ and from ______________ for a _______
left to right, period —-> , bottom to top (arrow up), group
the electrical attraction of an atom for the shared electrons is called the atom’s
electron affinity
What are the numbers for FONC CL H
4, 3.5, 3, 2.5, 3, 2.1
the most electronegative elements experience an increase in ____________ and attains a __________________
electron density, partial negative charge
the less electronegative elements experience an decrease in ____________ and attains a __________________
electron density, partial positive charge
dipole consists of
two points of a positive and negative charge
when is a bond nonpolar covalent
when there is an electronegativity value of 0, electrons are shared equally by two bonded atoms
when is a bond polar covalent
when there is an electronegative difference of more than or equal to 0.1 but less than 1.9 between two bonded atoms
a bond is ionic when
there is an electronegative value of equal to or more than 2.0
the greater the electronegativity difference between two bonded atoms, the greater the percentage of
ionic character in the bond
a molecule is polar
when there is an electronegativity difference of more than zero, one region of the molecule is has a small positive charge while the other region has a small negative charge
the bonding electrons in a non-polar compound
have the same EN value, are shared equally, symmetric
Lewis structures
they show the bonding between atoms of a molecule and the lone pairs of electrons that may exist in the molecule
a lewis structure
can be drawn for any covalently bonded molecule
BF3 lewis structure
boron only gets 6 electrons
BeCl2 lewis structure
beryllium only gets 4 electrons
a single line in a lewis structure represents
single bond, shared pair of electrons
ionic bonding
occurs between a metal nonmetal, cation and ion, group 1 and group 7
in an ionic bond the elements
transfer electrons
what happens to a nonmetal in formation of an ionic bond
the nonmetal gains electrons and gets a negative ion
n^2 gives you
orbitals
a nonmetal in an ionic bond
gains electrons and forms a negative ion
nonmetals want to
gain electrons
bonds that cant be represented by lewis structures are known as
resonance
