Ch. 1: some important things to remember Flashcards
organic compounds
compounds that contain carbon
atomic number
number of protons in the nucleus
mass number
protons + neutrons
isotopes
same atomic number, but different mass numbers
atomic weight
average mass of the atoms in the element
molecular weight
sum of the atomic weights off all the atoms in the molecule
what does an atomic orbital tell us?
the volume of space around the nucleus where an electron is most likely to be found
minimum energy corresponds to….
maximum stability
an atom is most stable if…
its outer shell is either filled or contains 8 electrons
if it has no electrons of higher energy
EN is a measure of
the ability of an atom to pull its bonding electrons toward itself
electronic configuration describes…
the atomic orbitals occupied by the atom’s electrons
a proton is a …..
a hydride ion is…
positively charged hydrogen ion
negatively charged hydrogen ion
ionic bond
attraction between ions with opposite charges
covalent bond
two atoms share a pair of electrons
polar covalent bond
covalent bond between atoms with different EN
dipole
positive end and a negative end
formal charge formula
FC = # valence electrons - # of electrons the atom has to itself (lone pair electrons and one half of the bonding electrons)
lewis structures show…
- which atoms are bonded
-lone pairs
-formal charges
when the atom is neutral, how many bonds do C, N, O and H form?
C-4
N-3
O-2
H-1
carbocation has a
positively charged carbon
carboanion has a
negatively charged carbon
sigma bonds
single bonds in organic compounds
pi bonds
side to side overlap of parallel p orbitals
bond strength is measured by
bond dissociation energy
a ___ bond is stronger than a __ bond
sigma, pi
how does carbon form four bonds?
it promotes an electron from an s orbital to an empty p orbital
__, __, __ ad halogens form bonds using …
C, N, O; hybrid orbitals
no pi bonds =
sp3 hybridized
one pi bond =
sp2 hybridized
two pi bonds =
sp hybridized
a double bond consists of
one sigma bond and one pi bond
a triple bond consists of
one sigma bond and two pi bonds
the greater the electron density in the region of orbital overlap…
the stronger and shorter the bond
shorter bond =
stronger bond
