2026 CHEM 1503 TRU _Chemical Bonding and Organic Chemistry| Learning Objectives, key concepts
and practice Questions and answers Thompson Rivers University
CHEM1503 (Chemical Bonding and Organic Chemistry)
Learning Objectives, key concepts and practice Questions
Unit: Introduction to the Course
Learning Objectives;
● Outline the historical development of chemistry.
● Provide examples of the importance of chemistry in everyday life.
● Describe the scientific method.
● Differentiate among hypotheses, theories, and laws.
● Provide examples illustrating macroscopic, microscopic, and symbolic domains.
Practice Questions with Answers and Explanations:
Part 1: Hypothesis, Law, or Theory
Q1: Falling barometric pressure precedes the onset of bad weather.
A: Law
Explanation: This is a consistent pattern observed in nature without an explanation of why it
happens—characteristic of a scientific law.
Q2: All life on Earth has evolved from a common, primitive organism through the process of
natural selection.
A: Theory
Explanation: This is a broad explanation supported by extensive evidence, which explains how
and why biological changes occur.
Q3: My truck’s gas mileage has dropped significantly, probably because it’s due for a tune-up.
A: Hypothesis
Explanation: This is a testable guess or explanation for a specific observation (worsened gas
mileage).
,Q4: The pressure of a sample of gas is directly proportional to the temperature of the gas.
A: Law
Explanation: This describes a consistent relationship between two variables (gas pressure and
temperature), typical of a scientific law.
Q5: Matter consists of tiny particles that can combine in specific ratios to form substances with
specific properties.
A: Theory
Explanation: This provides an explanation of the nature of matter based on atomic theory and
supported by evidence.
,Q6: At a higher temperature, solids (such as salt or sugar) will dissolve better in water.
A: Law
Explanation: This is a generalized statement based on consistent experimental results about
solubility.
Part 2: Macroscopic, Microscopic, or Symbolic Domains
Q7: The mass of a lead pipe is 14 lb.
A: Macroscopic
Explanation: This describes a measurable, visible quantity in the physical world.
Q8: The mass of a certain chlorine atom is 35 amu.
A: Microscopic
Explanation: Atomic mass is a property of particles too small to see directly.
Q9: A bottle with a label that reads Al contains aluminum metal.
A: Macroscopic
Explanation: The labeled bottle and its contents are observable.
Q10: Al is the symbol for an aluminum atom.
A: Symbolic (Microscopic Feature)
Explanation: "Al" is a symbolic representation for the element aluminum at the atomic level.
Part 3: Macroscopic or Microscopic Descriptions
Q11: The theory that gas pressure increases as volume decreases due to molecular motion.
A: Microscopic
Explanation: This explains behavior using particle motion at the molecular level.
Q12: The amount of heat required to melt 2 lb of ice is twice the amount needed to melt 1 lb.
A: Macroscopic
Explanation: Heat and mass are physical properties that can be observed and measured
directly.
Part 4: Mass vs Weight
Q13: Why is an object’s mass, rather than its weight, used to indicate the amount of matter it
contains?
A:
Explanation: Mass measures the amount of matter and does not change with location, while
weight depends on gravity and can vary (e.g., on the Moon vs Earth).
Part 5: Properties of States of Matter
Q14: What properties distinguish solids from liquids? Liquids from gases? Solids from gases?
A:
, Solids vs Liquids: Solids have a fixed shape and volume; liquids have fixed volume but take the
shape of their container.
Liquids vs Gases: Gases have neither fixed shape nor fixed volume.
Solids vs Gases: Solids are rigid and dense; gases are compressible and expand to fill their
container.
Part 6: Mixtures and Pure Substances
Q15: How does a heterogeneous mixture differ from a homogeneous mixture? How are they
similar?
A:
Different: Heterogeneous mixtures have visibly different components; homogeneous mixtures
look uniform.
Similar: Both consist of more than one substance physically combined.
Q16: How does a homogeneous mixture differ from a pure substance? How are they similar?
A:
Different: A homogeneous mixture contains multiple substances evenly mixed; a pure substance
contains only one kind of particle.
Similar: Both look uniform throughout.
Q17: How does an element differ from a compound? How are they similar?
A:
Different: Elements are made of one type of atom; compounds are made of two or more
different atoms chemically bonded.
Similar: Both are pure substances.
Part 7: Atoms, Molecules, and Compounds
Q18: How do molecules of elements and molecules of compounds differ? In what ways are they
similar?
A:
Different: Molecules of elements contain only one type of atom (e.g., O₂); molecules of
compounds contain two or more different types of atoms (e.g., H₂O).
Similar: Both are made of atoms bonded together.
and practice Questions and answers Thompson Rivers University
CHEM1503 (Chemical Bonding and Organic Chemistry)
Learning Objectives, key concepts and practice Questions
Unit: Introduction to the Course
Learning Objectives;
● Outline the historical development of chemistry.
● Provide examples of the importance of chemistry in everyday life.
● Describe the scientific method.
● Differentiate among hypotheses, theories, and laws.
● Provide examples illustrating macroscopic, microscopic, and symbolic domains.
Practice Questions with Answers and Explanations:
Part 1: Hypothesis, Law, or Theory
Q1: Falling barometric pressure precedes the onset of bad weather.
A: Law
Explanation: This is a consistent pattern observed in nature without an explanation of why it
happens—characteristic of a scientific law.
Q2: All life on Earth has evolved from a common, primitive organism through the process of
natural selection.
A: Theory
Explanation: This is a broad explanation supported by extensive evidence, which explains how
and why biological changes occur.
Q3: My truck’s gas mileage has dropped significantly, probably because it’s due for a tune-up.
A: Hypothesis
Explanation: This is a testable guess or explanation for a specific observation (worsened gas
mileage).
,Q4: The pressure of a sample of gas is directly proportional to the temperature of the gas.
A: Law
Explanation: This describes a consistent relationship between two variables (gas pressure and
temperature), typical of a scientific law.
Q5: Matter consists of tiny particles that can combine in specific ratios to form substances with
specific properties.
A: Theory
Explanation: This provides an explanation of the nature of matter based on atomic theory and
supported by evidence.
,Q6: At a higher temperature, solids (such as salt or sugar) will dissolve better in water.
A: Law
Explanation: This is a generalized statement based on consistent experimental results about
solubility.
Part 2: Macroscopic, Microscopic, or Symbolic Domains
Q7: The mass of a lead pipe is 14 lb.
A: Macroscopic
Explanation: This describes a measurable, visible quantity in the physical world.
Q8: The mass of a certain chlorine atom is 35 amu.
A: Microscopic
Explanation: Atomic mass is a property of particles too small to see directly.
Q9: A bottle with a label that reads Al contains aluminum metal.
A: Macroscopic
Explanation: The labeled bottle and its contents are observable.
Q10: Al is the symbol for an aluminum atom.
A: Symbolic (Microscopic Feature)
Explanation: "Al" is a symbolic representation for the element aluminum at the atomic level.
Part 3: Macroscopic or Microscopic Descriptions
Q11: The theory that gas pressure increases as volume decreases due to molecular motion.
A: Microscopic
Explanation: This explains behavior using particle motion at the molecular level.
Q12: The amount of heat required to melt 2 lb of ice is twice the amount needed to melt 1 lb.
A: Macroscopic
Explanation: Heat and mass are physical properties that can be observed and measured
directly.
Part 4: Mass vs Weight
Q13: Why is an object’s mass, rather than its weight, used to indicate the amount of matter it
contains?
A:
Explanation: Mass measures the amount of matter and does not change with location, while
weight depends on gravity and can vary (e.g., on the Moon vs Earth).
Part 5: Properties of States of Matter
Q14: What properties distinguish solids from liquids? Liquids from gases? Solids from gases?
A:
, Solids vs Liquids: Solids have a fixed shape and volume; liquids have fixed volume but take the
shape of their container.
Liquids vs Gases: Gases have neither fixed shape nor fixed volume.
Solids vs Gases: Solids are rigid and dense; gases are compressible and expand to fill their
container.
Part 6: Mixtures and Pure Substances
Q15: How does a heterogeneous mixture differ from a homogeneous mixture? How are they
similar?
A:
Different: Heterogeneous mixtures have visibly different components; homogeneous mixtures
look uniform.
Similar: Both consist of more than one substance physically combined.
Q16: How does a homogeneous mixture differ from a pure substance? How are they similar?
A:
Different: A homogeneous mixture contains multiple substances evenly mixed; a pure substance
contains only one kind of particle.
Similar: Both look uniform throughout.
Q17: How does an element differ from a compound? How are they similar?
A:
Different: Elements are made of one type of atom; compounds are made of two or more
different atoms chemically bonded.
Similar: Both are pure substances.
Part 7: Atoms, Molecules, and Compounds
Q18: How do molecules of elements and molecules of compounds differ? In what ways are they
similar?
A:
Different: Molecules of elements contain only one type of atom (e.g., O₂); molecules of
compounds contain two or more different types of atoms (e.g., H₂O).
Similar: Both are made of atoms bonded together.
