M6: Exam- Requires Respondus
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● Due No due date
● Points 100
● Questions 10
● Time Limit 120 Minutes
● Requires Respondus LockDown Browser
Attempt History
Attempt Time Score
LATEST Attempt 1 26 minutes 58 out of 100
Score for this quiz: 58 out of 100
Submitted Sep 18 at 4:24pm
This attempt took 26 minutes.
Question 1
pts
Click this link to access the Periodic Table. This may be helpful throughout the exam.
Explain the difference between amorphous and crystalline solids and give an example of each.
Your Answer:
crystalline solid have well defined edges and faces, the molecules and atoms are arrange in
defined shape and geometry throughout is called crystalline solids. the example of crystalline
solid is sodium chloride
amorphous solids are the one who donot have a defined shape or geometry their atoms are
arranged randomly and donot have a proper shape the example is glass
Amorphous solids (like glass, plastic or rubber) have their particles arranged in a random
fashion and crystalline solids (like salt, sugar, metals, quartz) have their particles arranged in
orderly, repeating, geometric patterns.
Question 2
pts
This study source was downloaded by 100000859819779 from CourseHero.com on 01-05-2023 14:04:29 GMT -06:00
https://www.coursehero.com/collection/68676003/M6-Examdocx/
, Water (H2O) with a molecular weight of 18 has a boiling point of 100oC and methane (CH4) with
a somewhat similar molecular weight of 16 has a boiling point of -161oC. This difference is
much higher than can be explained by the polarity of water. Explain what causes this
difference.
Your Answer:
the greater the forces between the atoms more it will be difficult to break that atom or compound
so result is higher boiling point, the water have strong bonding between the hydrogen and
oxygen there is a polar difference which make the hydrogen bonding strong and make it difficult
to break the water this is the reason that water boils at 100 degree celcius in comaprison on
methane it is non polar and have weak forces which is easy to break the reason why it has low
boiling point
Hydrogen bonds which are strong intermolecular attractive forces form between water
molecules requiring much more energy to separate the molecules than for other molecules.
Question 3
pts
Click this link to access the Periodic Table. This may be helpful throughout the exam.
Rank and explain how the freezing point of 0.100 m solutions of the following ionic electrolytes
compare, List from lowest freezing point to highest freezing point.
GaCl3, Al2(SO4)3, NaI, MgCl2
Your Answer:
NaI, mgcl2, GaCl3, Al2(SO4)3,
GaCl3 → Ga+3 + 3 Cl- ∆tf = 1.86 x 0.1 x 4 = 3rd
lowest FP
Al2(SO4)3 → 2 Al+3 + 3 SO4-3 ∆tf = 1.86 x 0.1 x 5 = lowest FP
NaI → Na+ + I- ∆tf = 1.86 x 0.1 x 2 =
highest FP
MgCl2 → Mg+2 + 2 Cl- ∆tf = 1.86 x 0.1 x 3 = 2nd
lowest FP
FP: Al2(SO4)3 < GaCl3 < MgCl2 < NaI
Question 4
This study source was downloaded by 100000859819779 from CourseHero.com on 01-05-2023 14:04:29 GMT -06:00
https://www.coursehero.com/collection/68676003/M6-Examdocx/
LockDown Browser
● Due No due date
● Points 100
● Questions 10
● Time Limit 120 Minutes
● Requires Respondus LockDown Browser
Attempt History
Attempt Time Score
LATEST Attempt 1 26 minutes 58 out of 100
Score for this quiz: 58 out of 100
Submitted Sep 18 at 4:24pm
This attempt took 26 minutes.
Question 1
pts
Click this link to access the Periodic Table. This may be helpful throughout the exam.
Explain the difference between amorphous and crystalline solids and give an example of each.
Your Answer:
crystalline solid have well defined edges and faces, the molecules and atoms are arrange in
defined shape and geometry throughout is called crystalline solids. the example of crystalline
solid is sodium chloride
amorphous solids are the one who donot have a defined shape or geometry their atoms are
arranged randomly and donot have a proper shape the example is glass
Amorphous solids (like glass, plastic or rubber) have their particles arranged in a random
fashion and crystalline solids (like salt, sugar, metals, quartz) have their particles arranged in
orderly, repeating, geometric patterns.
Question 2
pts
This study source was downloaded by 100000859819779 from CourseHero.com on 01-05-2023 14:04:29 GMT -06:00
https://www.coursehero.com/collection/68676003/M6-Examdocx/
, Water (H2O) with a molecular weight of 18 has a boiling point of 100oC and methane (CH4) with
a somewhat similar molecular weight of 16 has a boiling point of -161oC. This difference is
much higher than can be explained by the polarity of water. Explain what causes this
difference.
Your Answer:
the greater the forces between the atoms more it will be difficult to break that atom or compound
so result is higher boiling point, the water have strong bonding between the hydrogen and
oxygen there is a polar difference which make the hydrogen bonding strong and make it difficult
to break the water this is the reason that water boils at 100 degree celcius in comaprison on
methane it is non polar and have weak forces which is easy to break the reason why it has low
boiling point
Hydrogen bonds which are strong intermolecular attractive forces form between water
molecules requiring much more energy to separate the molecules than for other molecules.
Question 3
pts
Click this link to access the Periodic Table. This may be helpful throughout the exam.
Rank and explain how the freezing point of 0.100 m solutions of the following ionic electrolytes
compare, List from lowest freezing point to highest freezing point.
GaCl3, Al2(SO4)3, NaI, MgCl2
Your Answer:
NaI, mgcl2, GaCl3, Al2(SO4)3,
GaCl3 → Ga+3 + 3 Cl- ∆tf = 1.86 x 0.1 x 4 = 3rd
lowest FP
Al2(SO4)3 → 2 Al+3 + 3 SO4-3 ∆tf = 1.86 x 0.1 x 5 = lowest FP
NaI → Na+ + I- ∆tf = 1.86 x 0.1 x 2 =
highest FP
MgCl2 → Mg+2 + 2 Cl- ∆tf = 1.86 x 0.1 x 3 = 2nd
lowest FP
FP: Al2(SO4)3 < GaCl3 < MgCl2 < NaI
Question 4
This study source was downloaded by 100000859819779 from CourseHero.com on 01-05-2023 14:04:29 GMT -06:00
https://www.coursehero.com/collection/68676003/M6-Examdocx/
