Module 6 Portage Learning Chemistry Exam test with Verified Answers
1. Amorphous particles are arranged in a random fashion
solids
2. Colligative prop- physical properties of solvents that are dependent on the
erties concentration of the solute present and the identity of the
solvent but not on the identity of the solute. They include
vapor pressure, freezing point and boiling point
3. Colloids heterogeneous mixtures which appear to homogeneous
one-phase mixtures but are actually composed of parti-
cles too small to be seen with the naked eye
4. Condensation process of gas being converted to liquid
5. Critical point the temperature above which a substance cannot exist in
the liquid phase
6. Critical pressure the lowest pressure required for the substance to exist as
a liquid at the critical point
7. Crystalline particles are arranged in one of several different orderly,
solids repeating, geometric patterns
8. Electrolytes ionic or very polar compounds which dissolve to form
solutions of ions which conduct an electric current
9. Fluids substances like liquids and gases which have no fixed
shape and so they flow
10. Ionization the splitting of molecules to form ions
11. Molality the number of moles of solute present per kilogram of
solvent
12. Molarity the number of moles of solute present per liter of solution
13. Nonelectrolytes compounds which dissolve to form solutions of molecules
which do not conduct an electric current
14. Phase any state of matter such as solid, liquid or gas
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, Module 6 Portage Learning Chemistry Exam test with Verified Answers
15. Strong elec- solutes that ionize completely
trolytes
16. Sublimation the conversion of a solid directly to the gas state
17. Surface tension the force that causes a liquid which is in contact with a gas
like air to assume a shape that has the least amount of
surface area causing the surface to act like a thin elastic
sheet
18. Triple point the temperature and pressure at which the solid, liquid and
gas phases can coexist
19. Vapor pressure pressure exerted by vapor molecules above a liquid
20. Weak elec- solutes that only partially ionize
trolytes
21. Why are liquids they can exist only within a relatively narrow range of
the least com- temperatures and pressures
mon state of mat-
ter?
22. Differentiate be- Vaporization is the conversion of liquid particles to vapor at
tween evapora- the boiling point temperature of the material. The process
tion and vapor- of liquid converting to vapor molecules can also take place
ization in a very limited manner at temperatures lower than the
boiling point and is called evaporation
23. Differentiate be- A crystal lattice is the orderly, repeating geometric pattern
tween a crystal in which the particles of a crystalline solid are arranged.
lattice and a unit The unit cell is the smallest section of the crystal lattice
cell having that arrangement of particles
24. Why does a During a phase change, the temperature of the material
phase change remains constant as all of the energy being added is
occur at one tem- being used to overcome forces of attraction between the
perature rather particles and separate them so the temperature does not
rise. Over any other portions of the temperature range,
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1. Amorphous particles are arranged in a random fashion
solids
2. Colligative prop- physical properties of solvents that are dependent on the
erties concentration of the solute present and the identity of the
solvent but not on the identity of the solute. They include
vapor pressure, freezing point and boiling point
3. Colloids heterogeneous mixtures which appear to homogeneous
one-phase mixtures but are actually composed of parti-
cles too small to be seen with the naked eye
4. Condensation process of gas being converted to liquid
5. Critical point the temperature above which a substance cannot exist in
the liquid phase
6. Critical pressure the lowest pressure required for the substance to exist as
a liquid at the critical point
7. Crystalline particles are arranged in one of several different orderly,
solids repeating, geometric patterns
8. Electrolytes ionic or very polar compounds which dissolve to form
solutions of ions which conduct an electric current
9. Fluids substances like liquids and gases which have no fixed
shape and so they flow
10. Ionization the splitting of molecules to form ions
11. Molality the number of moles of solute present per kilogram of
solvent
12. Molarity the number of moles of solute present per liter of solution
13. Nonelectrolytes compounds which dissolve to form solutions of molecules
which do not conduct an electric current
14. Phase any state of matter such as solid, liquid or gas
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, Module 6 Portage Learning Chemistry Exam test with Verified Answers
15. Strong elec- solutes that ionize completely
trolytes
16. Sublimation the conversion of a solid directly to the gas state
17. Surface tension the force that causes a liquid which is in contact with a gas
like air to assume a shape that has the least amount of
surface area causing the surface to act like a thin elastic
sheet
18. Triple point the temperature and pressure at which the solid, liquid and
gas phases can coexist
19. Vapor pressure pressure exerted by vapor molecules above a liquid
20. Weak elec- solutes that only partially ionize
trolytes
21. Why are liquids they can exist only within a relatively narrow range of
the least com- temperatures and pressures
mon state of mat-
ter?
22. Differentiate be- Vaporization is the conversion of liquid particles to vapor at
tween evapora- the boiling point temperature of the material. The process
tion and vapor- of liquid converting to vapor molecules can also take place
ization in a very limited manner at temperatures lower than the
boiling point and is called evaporation
23. Differentiate be- A crystal lattice is the orderly, repeating geometric pattern
tween a crystal in which the particles of a crystalline solid are arranged.
lattice and a unit The unit cell is the smallest section of the crystal lattice
cell having that arrangement of particles
24. Why does a During a phase change, the temperature of the material
phase change remains constant as all of the energy being added is
occur at one tem- being used to overcome forces of attraction between the
perature rather particles and separate them so the temperature does not
rise. Over any other portions of the temperature range,
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