WorksheetsOrganic Chemistry Exam 1
Total questions: 49
Worksheet time: 36mins
the study of carbon-containing molecules and their reactions
inorganic chemistry
organic chemistry
general chemistry
advanced organic chemistry
a bond in which a pair of electrons is shared between two atoms
anion
ionic
covalent
dipole-dipole
Tetravalent: generally forms 4 bonds
C
Trivalent: generally forms 3 bonds
N
Divalent: generally forms 2 bonds
O
Monovalent: generally forms 1 bond
H, F, Cl, Br, I
atoms most commonly bonded to carbon include:
N, Cl, S, H, O
Na, Cl, O, H, Cl, Br, Se
Br, O, Xe, H, Na, Cl
N, O, H, F, Cl, Br, I
What happens to a molecule during a chemical reaction?
bonds are broken/made
molecules collide
carbon atoms disappear
protons and electrons switch places
compounds with the same molecular formula but different structures
allylic lone pair
anion
constitutional isomers
covalent bond
Organic compounds are different from inorganic compounds in that they contain (a) atoms.
+1 charge, resides in the nucleus
proton
neutron
electron
neutrino
-1 charge, reside in orbitals (shells) outside of the nucleus
proton
neutron
electron
neutrino
0 charge, reside in the nucleus
proton
neutron
electron
neutrino
electrons found in the outermost shell of atoms
(a)
2 dots in lewis dot structures represent
(a)
each dot in a lewis dot structure represents
(a)
negatively charged ion (contains extra e-)
(a)
positively charged ion (losing e-)
(a)
in order to determine the formal charge of an atom in a given molecule, compare the number of valence electrons that it OWNS to the number of valence electrons that it NEEDS to be (a)
Practice: Consider the formal charge on the atoms in CH3O and determine if any of the atoms should have a formal charge. (C)
-1
-2
-3
no formal charge
Practice: consider the formal charge on the atoms in CH3O and determine if any of the atoms should have a formal charge (O)
-2
-3
no formal charge
-1
how strongly an atom attracts shared electrons
(a)
electrons shared between 2 atoms where electronegativity is <0.5
covalent
polar covalent
ionic
anion
electrons shared between 2 atoms with electronegativity difference 0.5 < x < 1.7
covalent
cation
ionic
polar covalent
electrons between 2 atoms are transferred and electronegativity > 1.7; the more electronegative atom owns the electrons
polar covalent
ionic
anion
covalent
the greater the difference in electronegativity, the more (a) the bond
zig-zags in a bond-line structure represent bond angles for sp2 and (a) hybridized atoms and each corner represents a carbon atom
3 lines
3 bonds
2 lines
2 bonds
1 line
1 bond
H atoms bonded structures because it is assumed that each C atom will posses enough H atoms to achieve an octet of electrons
true
false
term used to refer to probability of finding an electron (the orbital shape is 90-95% of the space where an electron "probably" is)
electron orbital
electron shell
electron cloud
electron density
a sigma bond occurs when atomic orbitals directly overlap
true
false
pi bonds are stronger than sigma bonds
true
fasle
a bond formed by side-by-side overlap of p orbitals
(a)
# of sigma bonds + # of lone pair = (a) number
the steric number translates to the dehydration of the central atom
true
false
______ geometry is described for only the atoms bonded to the central atom
shape
atomic
molecular
electron
electron group includes lone pairs
true
false
if steric number = 2, geometry will be
(a)
tetrahedral
no lone pairs (tetrahedral), one lone pair (trigonal), two lone pairs (bent)
trigonal planar
one lone pair (bent), no lone pairs (trigonal planar)
linear
linear
(a) results in a dipole-dipole moment
result when polar molecules line up their opposite charges
dipole-dipole
London dispersion
hydrogen bonding
dispersion forces
attractive force between an H bond to an electronegative atom (N, O, or F) and a lone pair of another electronegative atom
dipole-dipole
hydrogen bonding
dispersion forces
London dispersion forces
two molecules are non-polar and have an attractive force between them
London dispersion forces
dipole-dipole
dispersion forces
hydrogen bonding
polar compounds generally mix well with other polar compounds; non-polar compounds generally mix well with other non-polar compounds
true
false
what is the cardinal rule when drawing bond-line structures?
never draw more than 4 bonds to a carbon atom (octet rule)
when drawing single bonds, the direction in which the bonds are drawn is irrelevant
hybridized atoms in a straight chain should be drawn in zig-zag form
when drawing double bonds, draw all bonds as far apart as possible
characteristic groups of atoms/bonds are called (a) groups
thiol
sulfide
aromatic
amine
amide
when a carbon atom has a positive charge
carbocation
carbanion
when a carbon has a negative charge
carbocation
carbanion
formal charges must always be written/drawn
true
false
allylic lone pair
a resonance hybrid represents the pi bond of an allylic carbocation as being delocalized over all three carbon atoms
true
false
