CHEM103/ CHEM 103 Module 6 – General
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Q: What is an amorphous solid?
Answer
A solid where the particles are arranged randomly and do not have any order. (Ex. Plastic
and Rubber)
Q: What is a colligative property?
Answer
properties that depend on the concentration of solute particles but not on their identity.
Includes the boiling point, freezing point, and vapour pressure.
Q: What is a colloid?
Answer
Appears to be a homo-geneous mixture but is actually composed of separate particles that is
too small to be able to see.
Q: What is condensation?
Answer
Occurs when gas is cooled to become a liquid (occurs at 100C)
Q: What is the critical point?
Answer
A point in a substance where it is reaching a temperature that the substance cannot exist in
a liquid state
Q: What is the critical pressure?
Answer
The lowest pressure required for a substance to exist in the liquid state
Q: What is a crystalline solid?
Answer
A particle that is arranged in an orderly fashion of one of seven geometric patterns
Q: What is an electrolyte?
Answer
Compounds that are ionic or very polar and dissolve into ions which conduct an electric
current.
Q: What is a fluid?
Answer
Particles are free to move (slide) around each other but will take the shape of any container
it is in
Q: What is ionization?
Answer
The amount of energy required to remove an electron from an atom. Takes place when a
solvent causes the molecules of an electrolyte to dissociate into ions.
Q: What is molality?
Answer
The moles of a solute that is present per kilogram of the solvent
Q: What is molarity?
Answer
The moles of a solute that is present per litre of solution
Q: What is a non-electrolyte?
Answer
Compounds that don't dissolve into ions and stays as a molecules when dissolved
Q: What is a phase?
Answer
Any state of matter such as a solid, liquid, or gas
Q: What is a strong electrolyte?
Answer
A substance that completely (100%) ionizes (Ex. HCl, HBr)
Q: What is sublimation?
Answer
Occurs when solids are directly converted to a gas state
Q: What is surface tension?
Answer
The surface acts like a thin elastic sheet. Occurs from an unbalanced cohesive forces where
particles in the center of the liquid is attracted to other particles on all sides but the
particles on the surface is attracted to other particles below them but aren't attracted to
particles above them. This results in the surface particles being pulled inward.
Q: What is the triple point?
Answer
The temperature and pressure that allows for solids, liquids, and gases to coexist
Q: What is the vapour pressure?
Answer
The pressure that is exerted by freely translating vapour molecules above liquid molecules
Q: What are weak electrolytes?
Answer
A substance that only partially ionizes (1-10%) (Ex. HF, NH3)
Q: Explain how and why the presence of a solute affects the BP of water
Answer
A solute presence will lower the VP of a solvent by occupying some of the space near the
surface of the water. This decrease in VP results in the increase of the temperature to raise
the VP to atmospheric pressure. Therefore, elevating the BP
Q: Why are liquids the least common state of mater?
Answer
Because there is a relatively small range of temperatures that liquids can exist in
Q: What is the difference between evaporation and vapourization?
Answer - Vapourization is the conversion of liquid particles to vapour at the BP of the material - Evaporation is the process of converting liquid particles to vapour at a temperature below
the BP
Q: Explain why the vapour pressure of a liquid increases with increased temperatures
Answer
As the temp increases the vibrations and rotations become intense enough to overcome the
forces that keep the molecules together. The molecules begin to undergo translation motion
allowing the molecules to convert to the vapour state and these exert a pressure above the
still-existing liquid molecules called the VP of the substance
Q: Explain water's concave meniscus in terms of cohesive and adhesive forces
Answer - Cohesive forces are the attractions between particles of the same type - Adhesive forces are the attractions between particles of one type and another type - These cohesive and adhesive forces combine to cause liquids to form a meniscus in a glass
tube. A liquid with strong cohesive tries to roll itself into a ball to minimize surface tension
but it's also attracted to the walls of any tube by adhesive forces. Causing the water to form
a concave meniscus
Why does diffusion take place quickly in a gas, more slowly in a liquid, and not at all in a
solid?
Answer
Diffusion is the non-energy-requiring movement of particles from regions of higher to
lower concentrations. Diffusion in a liquid occurs more slowly than in a gas since the gas
particles are moving more rapidly. Solids don't show the property of diffusion since the
particles in a solid can only vibrate around a fixed point rather than move through the
sample
Differentiate between a crystal lattice and a unit cell
Answer
A crystal lattice is the orderly, repeating geometric pattern in which the particles of a
crystalline solid are arranged. The unit cell is the smallest section of the crystal lattice
having that arrangement of particles
Why is liquid H2O more dense than ice H2O?
Answer
Ice has empty spaces between the molecules in its structures compared to H2O liquid
List and describe the two components of a solution
Answer - The minor component (aka solute) which is being dissolved in a solution - The major component (aka solvent) which is doing the dissolving in the solution
Describe and define the Tyndall Effect
Colloids can be distinguished from solutions by the use of a beam of light which is scattered
by colloids but is un-scattered (organized) through the solution, known as Tyndall Effect
Explain why sugar can be made to dissolve more quickly by grinding it to a fine crystal
Grinding sugar to fine crystals increases the surface area of the crystal and this makes it
dissolve more quickly b/c the solute particles dissolve by leaving the surface of their bulk
structure which is in contact with the solvent
Why does a bottle of a soda "fizz" when it's opened?
When a bottle of soda is being opened, the pressure above the solution decreases and some
of the CO2 bubbles off since a lower pressure allows the gas molecules in the solution to
escape.
Why does a temp increase usually increase the solubility of a solid?
Dissolving most solids is an endothermic process (absorbs heat). Adding heat causes any
dissolving process to change in the direction that consumes the added energy. For a solid or
liquid, heat is absorbed as the solute dissolves in water so a solid or liquid is more soluble at
higher temps.
Explain how and why the presence of a solute affects the VP of a solvent
The presence of a solute lowers the VP of a solvent b/c some of the solute particles occupy
the space near the surface of the liquid replacing some of the solvent particles thereby
decreasing the rate at which solvent particles can enter the vapour.
Explain how and why the presence of a solute affects the FP of a solvent
The presence of a solute lowers the FP of a solvent by forcing solvent molecules away from
the growing solid crystal. In order. for the solvent molecules to reach the crystal and add
themselves to the freezing solid, they must be slowed down to a lower kinetic energy by
decreasing the temp.
Describe the behaviour of a weak electrolyte and a strong electrolyte when placed in the
conductivity apparatus which has the metal strips and light bulb.
Solutions containing ions conduct electrical causing the light bulb to glow so the bulb would
glow brightly with a strong electrolyte and dimly with a weak electrolyte.
calorie (cal)
unit of heat or other energy; the amount of energy required to raise 1 gram of water by 1
degree Celsius; 1 cal is defined as 4.184 J
endothermic process
chemical reaction or physical change that absorbs heat
energy
the capacity to supply heat or do work
exothermic process
chemical reaction or physical change that releases heat
joule (J)
SI unit of energy; 1 joule is the kinetic energy of an object with a mass of 2kg moving with a
velocity of 1 m/s, 1 J = 1 kg m2/s and 4.184 J = 1 cal
kinetic energy
energy of a moving body, in joules, equal to 1/2mv^2
potential energy
energy of a particle or system of particles derived from relative position, composition, or
condition
thermal energy
kinetic energy associated with the random movement of atoms or molecules
thermochemistry
study of measuring the amount of heat absorbed or released during a chemical reaction or a
physical change
which of the following substances would you expect to have a relatively high chemical
potential energy: Wood, Gasoline, Chalk, Water, Hydrogen Gas?
Wood, gasoline, hydrogen gas
heat (q)
transfer of thermal energy between two substances
surroundings
all matter other than the system being studied
system
portion of matter undergoing a chemical or physical change being studied
temperature
intensive property of matter that is a quantitative measure of "hotness" and "coldness"
When 50.0 mL of 0.10 M HCl(aq) and 50.0 mL of 0.10 M NaOH(aq), both at 22.0 °C, are
added to a coffee cup calorimeter, the temperature of the mixture reaches a maximum of
28.9 °C degrees. Would the amount of heat measured for this reaction be greater, lesser, or
remain the same if we used a calorimeter that was a poorer insulator than a coffee cup
calorimeter? Explain your answer
Lesser; more heat would be lost to the coffee cup and the environment and so ΔT for the
water would be lesser and the calculated q would be lesser
When solid ammonium nitrate dissolves in water, the solution becomes cold. This is the
basis for an "instant ice pack". When 3.21 g of solid NH4NO3 dissolves in 50.0 g of water at
24.9 °C in a calorimeter, the temperature decreases to 20.3 °C. Would the amount of heat
absorbed by the dissolution appear greater, lesser, or remain the same if the experimenter
used a calorimeter that was a poorer insulator than a coffee cup calorimeter? Explain your
answer.
Lesser; heat from the environment would make ΔT smaller since the heat can affect the
temperature of the reaction system, and the calculated q would be lesser
chemical thermodynamics
area of science that deals with the relationships between heat, work, and all forms of energy
associated with chemical and physical processes
enthalpy (H)
is an energy like internal energy (E). The most important attribute of H is ΔH = Qp, the
heat transferred at constant pressure
expansion work (pressure-volume work)
work done as a system expands or contracts against external pressure
first law of thermodynamics
internal energy of a system changes due to heat flow in or out of the system or work done on
or by the system
internal energy (E)
sum of all kinetic and potential energies of the molecules in the system. It is the change in E
that is useful to understand, and it is expressed through the first law of thermodynamics,
ΔE = q + w.
heat capacity (C)
extensive property of a body of matter that represents the quantity of heat required to
increase its temperature by 1 degree Celsius (or 1 kelvin)
calorimeter
a device used to measure the amount of heat absorbed or released during chemical or
physical processes
specific heat capacity (c)
intensive property of a substance that represents the quantity of heat required to raise the
temperature of 1 gram of the substance by 1 degree Celsius (or 1 kelvin)
bomb calorimeter
device designed to measure the energy change for processes occurring under conditions of
constant volume; commonly used for reactions involving solid and gaseous reactants or
products
calorimetry
process of measuring the amount of heat involved in a chemical or physical process
Which can happen during a physical change?
A) Molecules can move more rapidly and freely and change states
B) The molecules in a substance break into smaller molecules.
C) The molecules in a substance react with other molecules.
D) The molecules in a substance are destroyed.
Molecules can move more rapidly and freely and change states
How many oxygen atoms are found in one molecule of nitric acid, HNO3?
A) 1
B) 2
C) 3
D) 4
3
How many phosphorous atoms are found in three molecules of magnesium phosphate,
3Mg3(PO4)2?
A) 1
B) 2
C) 3
D) 6
6
Which of the following is a synthesis reaction?
A) 2H2 + O2 → 2H2O
B) 2H2O2→ 2H2O + O2
C) CaCO3 → CaO + CO2
D) 2AgNO3 + Zn → 2Ag + Zn(NO3)2
2H2 + O2 → 2H2O
Which is a chemical property of iron?
A) Its tendency to react with oxygen
B) Its melting point
C) Its strength under compression
D) Its hardness
Its tendency to react with oxygen
Which equation shows a physical change?
A) Pb(NO3)2 (aq) + 2KI(aq) → 2KNO3(aq) + PbI2(s)
B) HCl(aq) + NaOH(aq) → NaCl(aq) + H2O(l)
C) 2H2O(l) → 2H2(g) + O2(g)
D) H2O(g) → H2O(s)
H2O(g) → H2O(s)
Which property of matter allows convection currents to form?
A) Fluids rise if they are less dense than the matter around them.
B) The molecules in solids do not vibrate very quickly.
C) Electromagnetic waves carry energy.
D) Liquids take the shape of their container.
Fluids rise if they are less dense than the matter around them.
A burning piece of coal glows red on a lab table. A student wants to prevent the coal from
transferring heat to him. He sets up a metal shield between himself and the coal to prevent
convection. Why will this not completely stop all of the heat transfer?
A) The metal shield will heat up, and then heat the air on the student's side of the shield.
B) The metal shield will cause more radiation to reach the student.
C) The metal shield will not prevent heat transfer by conduction.
D) The metal shield cannot block the flow of fluids.
The metal shield will heat up, and then heat the air on the student's side of the shield.
What must be true for any endothermic reaction?
A) The chemical bonds of the products have more energy than the chemical bonds of the
reactants.
B) There are more products than there are reactants.
C) There must be a phase change from solid to liquid or from liquid to gas.
D) The reaction must take place in a sealed container held at constant volume.
The chemical bonds of the products have more energy than the chemical bonds of the
reactants.
A student notices that a reaction takes place faster when the temperature is higher. Which
best explains why this happens?
A) At higher temperatures, the molecules collide more frequently.
B) The heat of the solution breaks apart chemical bonds.
C) As the particles move more quickly, they can more easily avoid each other.
D) Catalysts cannot be effective at high temperatures.
At higher temperatures, the molecules collide more frequently.
A chemist finds that when platinum is added to a reaction, the reaction speeds up. He
thinks the platinum may be acting as a catalyst. What measurement should the chemist
make to determine whether it is a catalyst?
A) Measure the mass of the platinum before and after the reaction.
B) Measure the temperature of the solution before and after the reaction.
C) Measure the change in volume of the solution.
D) Measure the amount of gas released by the reaction.
Measure the mass of the platinum before and after the reaction.
Which would you most expect to be an unstable atom?
A) A carbon (C) atom with 6 protons and 6 neutrons
B) An iron (Fe) atom with 26 protons and 27 neutrons
C) A helium (He) atom with 2 protons and 2 neutrons
D) A curium (Cm) atom with 96 protons and 85 neutrons
A curium (Cm) atom with 96 protons and 85 neutrons
Americium-241 decays into neptunium-237. Which correctly describes this process of
radioactive decay?
A) An unstable nucleus decays into a more stable nucleus
B) Energy in the nucleus is converted into mass
C) The strong nuclear force splits the nucleus apart.
D) The atom loses four protons.
An unstable nucleus decays into a more stable nucleus
Gamma rays are often used to kill microorganisms in food, in an attempt to make the food
safer. Some people contend that this irradiated food is actually less safe to eat. Which, if
true, would most effectively dispute their idea?
A) Irradiated food only emits alpha particles, which are harmless.
B) Irradiated food is shown to not be radioactive.
C) Irradiated food only contributes to background radiation.
D) Irradiated food has molecules that undergo transmutation.
Irradiated food is shown to not be radioactive.
How do the forces in nuclear and chemical reactions differ?
A) Both reactions only need to overcome weak electrostatic forces.
B) Chemical reactions must overcome the strong nuclear force
C) Nuclear reactions must overcome much stronger forces.
D) Nuclear reactions must overcome intermolecular forces.
Nuclear reactions must overcome much stronger forces.
Why do chemical reactions not produce radioactive particles?
A) Chemical reactions make the nuclei of atoms more stable.
B) Chemical reactions only release gamma rays.
C) Only electrons are involved in chemical reactions.
D) Mass is not conserved in chemical reactions.
Only electrons are involved in chemical reactions.
Which of these statements about power plants is true?
A) Coal-fired plants give off pollution even when operating correctly.
B) Nuclear plants give off radiation even when operating correctly.
C) Coal-fired plants give off no pollution when operating correctly.
D) Nuclear plants give off greenhouse gases when operating correctly.
Coal-fired plants give off pollution even when operating correctly.
Which is the most valid reason a group of people might oppose the storage of spent fuel
rods in their community?
A) The fuel rods will remain radioactive for a long time.
B) The fuel rods contribute to global warming.
C) The fuel rods may cause a nuclear meltdown.
D) The fuel rods do not emit radioactive particles.
The fuel rods will remain radioactive for a long time.
Which of the following aspects of biotechnology is not considered to be a moral or ethical
issue?
A) Research and testing on animals
B) Cloning living material
C) Reducing research cost
D) Damaging the environment
Reducing research cost
Which is one way that an advance in biotechnology can produce unintended consequences
that harm the environment?
A) Genetically modified plants require less water to grow.
B) Patients using insulin pumps live longer than those without the pumps
C) Pesticides can prevent insects from destroying crops.
D) Genes implanted into a species of plant can spread to other plants.
Genes implanted into a species of plant can spread to other plants.
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