Chapter 1 Flashcards
Neutral carbon atom has ______ single bonds
4
Carbocation has ______ single bonds
3
Carbanion has _____ single bonds and ____
3, 1 lone pair
Describe carbene
2 single bonds and 1 lone pair
Formal charge calculation
FC = valence electrons - (bonds + dots)
Charges on atoms are
REACTIVE
Charges are sites where ____________
Reactions occur
If an atom has MORE lone pairs/bonds than it does in its neutral state, it has a ______ charge
Negative
If an atom has LESS lone pairs/bonds than it does in its neutral state, it has a ______ charge
Positive
a single bond has ____ areas of overlap
1
a double bond has ____ areas of overlap
3
a triple bond has ____ areas of overlap
5
how to determine a coordination number
count the number of “things” attached to the atom
(bonds/long pairs) - double/triple bonds only count as 1
coordination number of 2
sp
linear
coordination number of 3
sp2
trigonal planar
coordination number of 4
sp3
tetrahedral
1 degree carbon
methyl
“end point”
2 degree carbon
methylene
“linker”
3 degree carbon
methine
“branch point”
4 degree carbon
quaternary
“branch point”
formal charge equation
FC = valence electrons - (bonds + dots)
if an atom gains a bond or lone pair it will have a ___ charge
-1
if an atom looses a bond or lone pair it will have a ___ charge
+1
carbocation
carbon with 3 bonds and NO lone pair
carboanion
carbon with 3 bonds and a lone pair
empty
empty
row 2 elements (BCNOF) can have __________ electrons under the octet rule
6, 8
row 3 elements (Al,Si,P,S,Cl) can have _________ electrons under the octet rule
6, 8, 10, 12, 14
a curly arrow starts where ____________ and ends ___________
where a bond/lone pair is ERASED, where a bond/lone pair is ADDED
nucleophiles
electron-rich
electrophiles
electron-poor
hydrogen with 1 proton and 0 neutrons is known as
hydrogen
hydrogen with 1 proton and 1 neutron is known as
deterium
hydrogen with 1 proton and 2 neutrons is known as
tritium
carbon with 6 protons and 6 neutrons is known as
carbon-12
carbon with 6 protons and 7 neutrons is known as
carbon-13
carbons with 6 protons and 8 neutrons is known as
carbon-14
number of protons identify an
atom
number of neutrons identify an
isotope
shape of an s orbital
sphere
shape of a p orbital
dumbbell
criteria for an organic molecule
direct C-H bond
a single bond has a ____ bond
sigma
a double bond has a ____ bond
1 sigma, 1 pi
a triple bond has a ____ bond
1 sigma, 2 pi
3 potentials for resonance to occur
A with lone pair - A+
A+ - A = A
A- with lone pair - A = A
could also be triple bond**
single bonds have ____ area(s) of overlap
1
double bonds have ____ area(s) of overlap
3
triple bonds have ____ area(s) of overlap
5
each individual sigma bond counts as ____ area(s) of overlap
1
each individual pi bond counts as ____ area(s) of overlap
2
which bond is stronger? sigma or pi
sigma
rigidity of a single bond
free rotation
rigidity of a double bond
rigid
rigidity of a triple bond
rigid
where is the area of electron density located for a sigma bond
internuclear axis
where is the area of electron density located for a pi bond
above and below the internuclear axis
what are the four types of electron-rich species
aka nucleophiles/lewis bases
A- with lone pair
A with lone pair
A triple bond A
A double bond A
what are the two types of electron-poor species
aka electrophiles/lewis acids
A+
A with incomplete octet at neutral
orbital overlap =
bond
order of bond length (longest to shortest)
single, double, triple
order of bond strength (strongest to weakest)
triple, double, single
zina
z-axis
axis connecting the nuclei
a single bond requires how much energy to break
348 kJ/mol
a double bond requires how much energy to break
613 kJ/mol
a triple bond requires how much energy to break
839 kJ/mol
does it take more energy to break a sigma or a pi bond
sigma
