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Chemistry Exam: Intermolecular Forces, Crystal Structures, and Solutions, Exams of Chemistry

A chemistry 1520 exam focusing on intermolecular forces, crystal structures, and solution properties. It includes short answer questions covering the strength of different intermolecular forces, their association with enthalpy of hydration, and their role in the solubility of substances. The exam also features calculations related to molarity, unit cell dimensions, and boiling point elevation, providing a comprehensive assessment of students' understanding of these key concepts in chemistry. This exam is useful for university students.

Typology: Exams

2024/2025

Available from 05/30/2025

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bg1
Name:
KG\[
CIRCLE
your
INSTRUCTOR/LECTURE
TIME:
McMills
8:35
am
CIRCLE
the
alphabet
segment
of
your
last
name:
AE
FL
M-R
Chemistry
1520
Exam
IB
Part
I.
(36
pts)
Short
Answer.
1.
(12
pts)
Choose
the
correct
answer
for
each
of
the
following:
PID:
Paris
9:40
am
Sz
a.
Ofthe
IMF
(intermolecular
forces)
listed,
which
is
the
WEAKEST?
Circle
one:
dipole-dipole
tondon
dispersion
force
H-bonding
dipole-induced
dipole
b.
Which
IMF
Is
associated
with
enthalpy
of
hydration
(AHmya)?
Circle
one:
dipole-dipole
London
dispersion
forces
H-bonding
dipole-induced
dipole
.
Which
IMF
is
responsible
for
O
being
partly
soluble
in
H0?
Circle
one:
dipole-dipole
London
dispersion
forces
H-bonding
dipole-induced
dipole
d.
For
the
compound
sulfur
hexafluoride,
which
is
the
STRONGEST
IMF
present?
Circle
one:
dipole-dipole
London
dispersion
forces
H-bonding
dipole-induced
dipole
February
14,
2025
100
points
ion-dipole
ion-dipole
lon-dipole
pf3
pf4
pf5

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Name: KG[ CIRCLE your INSTRUCTOR/LECTURE TIME: McMills 8:35 am CIRCLE the alphabet segment of your last name: AE FL M-R Chemistry 1520 Exam IB Part I. (36 pts) Short Answer.

  1. (12 pts) Choose the correct answer for each of the following:

PID:

Paris 9:40 am Sz a. Ofthe IMF (intermolecular forces) listed, which is the WEAKEST? Circle one: dipole-dipole tondon dispersion force H-bonding dipole-induced dipole b. Which IMF Is associated with enthalpy of hydration (AHmya)? Circle one: dipole-dipole London dispersion forces H-bonding dipole-induced dipole

. Which IMF is responsible for O being partly soluble in H0? Circle one: dipole-dipole London dispersion forces H-bonding dipole-induced dipole d. For the compound sulfur hexafluoride, which is the STRONGEST IMF present? Circle one: dipole-dipole London dispersion forces H-bonding dipole-induced dipole February 14, 2025 100 points ion-dipole ion-dipole lon-dipole

. (12 pts) The cubic lattice of a particular ionic compound has the following features: There is ONE CATION {A) at each CORNER of the unit cell, There is ONE CATION (A) in each FACE of the unit cell. There are FOUR ANIONS {X) within the BODY of the unit cell. . The number of cations {A) per unit cell Is:

Grdeon: 12 3 (@) s & 7

. The number of anions (X) per unit cell is: Circle one: (^12 3) @ H (^678) The empirical formula of the compound is: Circle one: @ AXy (^) AX3 AXs

AaX AsX AsXz

. What unit cell do the cations adopt? Circle one: sc bee @

(14 pts) The element tantalum (Ta} adopts a bec unit cell. Glven that the density of Ta is 16.2 g/cm?, what is the radius of a single Ta atom, In cm? Report your answer to 3 significant figures. lue.^ x 2:“"”' (^) * (^) ‘—:‘u"ou( x (^) 8.9 (^) Radlus: o & (^) o "M.I (^) fere————p et 149 xio-Y ., x 3 lew? (^). 359%xlo (^) em? ~ Vs fl.‘ Py a‘J 3.5%94xl0 P03. 3.8gixtle om

  • 4r r=al3 | 3.0 %l fum I3. I.‘flx‘°-9¢~h g (^4) [ ] (15 pts) A solution is prepared by dissolving 0.175 g of NaCl (MM = 58.44 g/mol) in 4.18 g of HCONH; {formamide). The boiling point of the NaCl/formamide solution is 215.5°C. Formamide has a molal boiling point constant, K of 3.85 *C/m. Calculate the bolling point of pure formamide in °C. Assume the solvent is nonvolatile and the sofution is ideal. Report your answer to one decimal place. Nactl L= Boiling point: o.l'-l:_, Nacl ¥ el Nacl 2 0.0029946 mel Nact 2io.0% £9.44%4 Nacd M1 0.0029948 mel Nael g et 4.18xl0 =? kj calv AT = 385°C^ ,^ o^ Hebmx^2 =^ 582° = _

AT = rhol'.---rbs.lv = $.82%¢

Toaeln (^) - (^) S.62°c = (^) Toal pubasia 2.18.$°c ~^ 6.%2°C^ a^ lfl.lo.o'c

Part Ill. Multiple Choice. Write answer on the line provided. (21 pts; 7 @ 3 pts each) A 1. Which of the following lons should have the smallest {least negative) enthalpy of hydration,

AHyya?

a. Cs* b. Rb* ¢, Ba® d. Sr** C 2. Which of the foliowing pairs is arranged with the particles of higher polarizability (^) listed first?

a i b. Mg, Mg c. Se?", 5% d.Br,

. Which of the following is expected to have the lowest vapor pressure at 350 K?

  1. 1.25 m K;S04 b. 1.00 m KsPO4 €. 1.50 m KNO3 d.1.25 mKCi D 4. Which is expected to have the lowest bolling point? a. 0.500 m NasPO, b. 1.25 m NaCl. 1.00 m Na2CO3 d. pure water C S. Carbonated drinks bubble when the bottie is opened because the temperature of the soda increases. exposure to atmospheric pressure squeezes the CO; from solution. the partial pressure of CO; above the solution is reduced. anocwatmospheric nitrogen molecules displace CO; molecules. 5_ 6. Which of the following palrs of liquids will be miscible (form a solution)? a. CClyand CH;0H €. H0 and CgHs b. CsHis and CeHig d. CaHis and H, :D 7. Asolution of sugar in water is in equilibrium with solid sugar. If additional solid sugar is added and the solution is stirred at constant temperature a supersaturated solution will form. the concentration of the solution will increase. the concentration of the solution will decrease. ap the concentration of the solution will remain the same. o