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WorksheetsKEMORG Review 1 - Introduction and Recap
Total questions: 53
Worksheet time: 29mins
(1.2) 2 atoms bond in order to _____
achieve octet e- config.
achieve stability
increase electronegativity
become more acidic or basic
(1.2) Bonding that involves sharing of electrons between elements with little to no electronegativity difference
ionic
metallic
covalent
nuclear
(1.2) which of the following is a MOLECULE
Mg
NaCl
e-
H2
(1.2) How many covalent bonds can be formed from an atom with 5 valence electrons
2
3
4
5
(1.3) Lewis structures represent the actual bonding between atoms in a compound
true
false
(1.3) Which formal charge is most stable?
-3
+2
1
0
(1.4) Ethanol (CH3CH2OH) and dimethyl ether (CH3OCH3) are ______
isotopes
isomers
acids
alkanes
(1.5) Elements in 3rd row of periodic table tend to be octet exceptions, specifically
incomplete octet
expanded octet
free radicals (odd no. of e-)
even no. of e-
(1.6) what differs in between resonance structures
placement of atoms
sum of formal charges
arrangement of electrons
location of sigma electrons
(1.6) what actually occurs in a resonance hybrid
electrons split into halves or thirds for each fractional bond
electrons are expelled for more stability
electrons are delocalized over 2 or more atoms
double / triple bond changes location every millisecond
(1.6) What does curved arrow notation show?
rotation of a sigma bond
transfer of energy in a rxn
movement of electrons
bending and stretching of a bond
(1.6) what illustrates the reason why resonance is a limitation of Valence Bond Theory
oxygen is made of fractional bonds
all bonds in carbon dioxide have different lengths
monoatomic oxygen violates the octet rule
bonds in ozone are of equal strength and length
(1.6) which atom does not have resonance?
HSO4-
O3
CO3
NH4
Major contributors to resonance will look (more/less) similar to the actual structure
(a)
(1.7) What may affect the bond angle in a molecule
VSEPR
bonding electron groups
non bonding electron groups
electronegativity
(1.7) when is electron geometry the same as molecular geometry?
when there are even numbers of electrons
when there are no lone pairs
when halides are involved in the bond
when all the electron groups are lone pairs
(1.8) CH3CH2CH2CH2CH3 or CH3(CH2)3CH3 is an example of ______
lewis structures
aufbau structures
condensed structures
skeletal structures
(1.8) This is an example of _____
Lewis structures
stick and ball structures
condensed structures
skeletal structures
(1.9) hybridization in methane (4 e- groups)
sp3
sp2
sp
s
(1.9) what must occur prior to hybridization
e- promotion / excitation
bond formation
proton demotion
valence electron collision
(1.10) the pi bond in ethylene occurs on ____
p orbitals
s orbitals
hybdridized sp2 orbitals
hybridized sp3 orbitals
(1.9) What is the shape of sp, sp2, sp3 hybridized orbitals
dumbell
asymmetric dumbell
sphere
boat shape
(1.11) What bond does this describe?
symmetric with respect to bond axis, stronger, head on overlap across molecular plane
sigma
pi
delta
omega
(1.11) why are single bonds free to rotate?
single and ready to mingle~
electrons are constantly providing thrust and momentum for bond to rotate
pi bonds restrict rotation as they need to break and reform
because of short bond length between the two bonded atoms
(1.11) What is the relationship between bond length and bond strength
proportional
quadratic
inverse
unrelated
(1.12) Electronegativity __________________
increases down a group, decreases across a period
increases across a period, decreases down a group
increases down a group and across a period
decreases down a group and across a period
(1.12) Describes the share of electrons between 2 bonded atoms
bond order
bond charge
bond distribution
bond polarity
(1.12) In a polar compound, where would there be an accumulation of electrons
near the element with higher electronegativity
near the element with lower electronegativity
between the two atoms
above and below the molecular axis
(1.12) a bond with electronegativity difference of 1.7 would be
Non polar covalent
Polar covalent
Ionic
Metallic
(1.13) How do you find the net dipole moment in a molecule
parallelogram method
adding the individual dipole moments regardless of direction
subtracting the individual dipole moments regardless of direction
through mass spectroscopy
(1.13) BF3 has a polar bond but is not a polar molecule, why is that?
fluorine creates hydrogen bonds and cancels out the polarity
Boron has a unique interaction with the wave functions of the sigma bonds to remove polarity
rotation of the molecule spreads out the charge across the whole molecule instead of just fluorine through centripetal force
the dipole moments cancel out due to the geometry of BF3
(10.2) What is the general formula for an alkane
Cn H2n+2
C2n+2 Hn
Cn H2n
C2n Hn
(10.2) How do you calculate the degrees of unsaturation?
(saturated number of H - unsaturated number of H) / 2
(unsaturated number of H) / 2
(unsaturated number of H - saturated number of H)
(unsaturated number of H) x 2
(10.2) A molecule has a degree of unsaturation of 7, select which of the following are possible given this information
1 triple bond, 2 double bonds, 3 rings
0 triple bond, 3 double bonds, 2 rings
3 triple bonds, 1 double bond, 0 rings
1 triple bond, 1 double bond, 2 rings
2 triple bonds, 0 double bonds, 2 rings
(2.1 -2.4) _________ is a proton donor
BL Acid
BL Base
Lewis Acid
Lewis Base
(2.1 - 2.4, 2.8) Which definition of acids and base is the most specific
Arrhenius
Lewis
Bronsted-Lowry
(2.1 - 2.4) In an amphoteric molecule (acts as an acid or base) _______ is the acidic portion of the molecule, and _______ is the basic portion of the molecule
Hydrogen, Lone pairs
Lone pairs, Hydrogen
Lone pairs, Lone pairs
Hydrogen, Hydrogen
(2.1 - 2.4) In an acid-base reaction, the proton moves _____
from the base to the acid
from the acid to the base
(2.1 - 2.4) using a curved arrow notation, an acid and base reaction will have arrows that ___
goes from lone pair of base to hydrogen in acid
goes from lone pair of acid to hydrogen in base
goes from bond (H-A) to the acid
goes from acid to the bond (H-A)
(2.1 - 2.4) a strong acid has
high Pka value
unwilling to lose hydrogen
easily loses hydrogen
low Pka value
(2.1 - 2.4) organic acids tend to be (stronger/weaker) than inorganic acids
(a)
(2.5) Strong acids produce
weak conjugate bases
strong conjugate bases
conjugate bases of varying strength
conjugate acids
(2.5) what is the relationship of an element's electronegativity and its acidity
higher electronegativity = higher acidity
lower electronegativity = higher acidity
odd electronegativity = higher acidity
even electronegativity = higher acidity
(2.5) for Conjugate bases that are anions, (e.g. Halogens) they are more stable when
larger anion
smaller anion
higher electronegativity
lower electronegativity
(2.5) Why is trifluoroethanol more acidic than regular ethanol
the polar bonds exasperate the unequal distribution of e- in the CB
fluorine is a halogen and makes it more acidic
actually ethanol is more acidic than trifluoroethanol
fluorine pulls in charge from the CB through the sigma bonds and its high electronegativity
(2.5) How does resonance affect acidity (by comparing conjugate bases)
increases, stronger bonds due to resonance lead to stable molecule
increases, delocalization of charge stabilizes the molecule
decreases, net dipole moment is intensified and can tear the molecule apart
decreases, attraction to proton is stronger so formation of conjugate base becomes thermodynamically unfavorable
(2.5) an anion (CB) with higher s character has lower stability
true
false
(2.6 - 2.7) Organic bases
amines
CH3COOH
NaOH
H2SO4
(2.6 - 2.7) Organic bases are characterized by
strong conjugate acids
weak conjugate acids
net positive charge
net negative charge
(2.8) How do BL bases and Lewis bases differ
Lewis bases specifically donate e- to protons
BL bases are always organic
BL bases specifically donate e- to protons
Lewis bases are always organic
(2.8) In acid base reactions, the Lewis Acid is
electrophile
nucleophile
e- rich
e- poor
(2.8) if a Lewis base forms a bond with a Lewis acid, we call that bond a _____
salt bond
nucleophilic bond
coordinate covalent bond
bond of neutrality
(2.8) using curved arrow notation, the arrow will point from the ______ to the ______
acid, base
base, acid
central atom, peripheral atom
electropositive atom, electronegative atom
