CHEM101 (E-1) Chemistry I - Eastwick College
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Free CHEM101 (E-1) Chemistry I - Eastwick College Questions
Which of the following is true of ice when it melts to form liquid water?
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The number of molecules of water increases.
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Both physical and chemical changes occur.
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A chemical change occurs.
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The number of molecules of water decreases.
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A physical change occurs.
Explanation
When ice melts to form liquid water, only the physical state of matter changes from solid to liquid. The chemical composition remains H₂O throughout the process. No new substances are formed and no chemical bonds are broken or created, making this a purely physical change.
Why the other options are incorrect:
A. The number of molecules of water increases. — The number of water molecules does not change when ice melts. The same H₂O molecules simply transition from a rigid solid arrangement to a more fluid liquid arrangement.
B. Both physical and chemical changes occur. — Only a physical change occurs during melting. No chemical reaction takes place and no new substances are produced.
C. A chemical change occurs. — Melting does not involve any chemical reaction. The identity of the substance remains water before and after the process.
D. The number of molecules of water decreases. — The number of water molecules is conserved during melting. No molecules are created or destroyed in a physical change.
How many protons (p), neutrons (n), and electrons (e) are in an atom of ²³⁵U?
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92 p, 92 n, 146 e
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92 p, 146 n, 92 e
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92 p, 51 n, 92 e
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92 p, 92 n, 92 e
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92 p, 143 n, 92 e
Explanation
Correct Answer: (A) gain; negative
Nonmetals have high electronegativity and tend to gain electrons to achieve a stable full outer electron shell. When a nonmetal gains electrons, it acquires more negative charges than positive charges, resulting in the formation of a negatively charged ion called an anion.
Why Other Options are Incorrect:
B. gain; neutral — Gaining electrons adds negative charge to an atom, resulting in a negatively charged ion, not a neutral particle.
C. lose; negative — Nonmetals do not tend to lose electrons. Losing electrons is characteristic of metals, which form positive ions called cations.
D. gain; positive — Gaining electrons increases the number of negative charges, which produces a negative ion, not a positive one.
E. lose; positive — This describes the behavior of metals, not nonmetals. Metals lose electrons to form positively charged cations.
Refer to Figure 2-1. Which of these statements is true based on the data provided by the graph?
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The pH of the solution rises significantly when the volume of the base is increased from 14 mL to 18 mL.
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The pH of the solution must be determined algebraically.
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The pH of the solution is relatively constant after the addition of the first 14 mL of the base.
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The pH of the solution is relatively unaffected by the addition of the base.
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The pH of the solution is 7 when approximately 16 mL of the base has been added.
Explanation
Correct Answer: (A) The pH of the solution rises significantly when the volume of the base is increased from 14 mL to 18 mL.
Based on the graph in Figure 2-1, the pH remains relatively low and stable from approximately 2 to 14 mL of base addition. However, between approximately 14 mL and 18 mL there is a sharp and dramatic increase in pH, rising from around 4-5 to approximately 9. This steep rise is characteristic of the equivalence point region in an acid-base titration curve.
Why Other Options are Incorrect:
B. The pH of the solution must be determined algebraically. — The graph directly provides pH values visually at each volume of base added. Algebraic determination is not required to read the data from the graph.
C. The pH of the solution is relatively constant after the addition of the first 14 mL of the base. — The graph shows that pH is relatively constant before 14 mL, not after. After 14 mL, the pH rises sharply.
D. The pH of the solution is relatively unaffected by the addition of the base. — This is clearly incorrect as the graph shows a dramatic pH increase between 14 mL and 18 mL of base addition.
E. The pH of the solution is 7 when approximately 16 mL of the base has been added. — According to the graph, at approximately 16 mL the pH is in the steep rise region and is closer to 7-8, but the graph shows pH reaching approximately 7 closer to the midpoint of the steep rise rather than a clearly defined point at exactly 16 mL. The more clearly supported observation from the graph is the significant rise between 14 and 18 mL.
Which of these statements is true?
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The composition of mixtures is variable, and the composition of pure substances is fixed.
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The compositions of both mixtures and pure substances are variable.
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The composition of mixtures is fixed, and the composition of pure substances is variable.
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The compositions of both mixtures and pure substances can be fixed or variable.
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The compositions of both mixtures and pure substances are fixed.
Explanation
Correct Answer: (A) The composition of mixtures is variable, and the composition of pure substances is fixed.
Mixtures can be combined in any proportion and their composition varies depending on how much of each component is present, making their composition variable. Pure substances, whether elements or compounds, always have a definite and fixed composition. For example, water always contains hydrogen and oxygen in a 2:1 ratio regardless of its source.
Why Other Options are Incorrect:
B. The compositions of both mixtures and pure substances are variable. — Pure substances always have a fixed composition, so this statement is incorrect.
C. The composition of mixtures is fixed, and the composition of pure substances is variable. — This reverses the correct relationship. Mixtures are variable and pure substances are fixed.
D. The compositions of both mixtures and pure substances can be fixed or variable. — Pure substances always have a fixed composition and are never variable, making this statement incorrect.
E. The compositions of both mixtures and pure substances are fixed. — The composition of mixtures is variable, not fixed, making this statement incorrect.
Which of these is the correct normal decimal notation for 5.23 × 10⁻⁴?
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52,300
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0.00523
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0.000523
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0.0523
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0.0000523
Explanation
Correct Answer: (D) An electron is located close to the nucleus of an atom.
According to Rutherford's nuclear model of the atom, electrons orbit the nucleus at a relatively large distance, with most of the atom being empty space. Rutherford's gold foil experiment demonstrated that the nucleus is a tiny, dense, positively charged center, and electrons occupy the vast surrounding space at a distance. Stating that electrons are located close to the nucleus directly contradicts Rutherford's model.
Why Other Options are Incorrect:
A. A neutral atom contains an equal number of protons and electrons. — This is consistent with Rutherford's model as a neutral atom has balanced positive and negative charges.
B. Neutrons are part of the nucleus. — This is consistent with the nuclear model, though the neutron was formally discovered later by Chadwick, Rutherford's model does account for nuclear mass.
C. Most of the mass of the atom is concentrated in the nucleus. — This is a key conclusion of Rutherford's model, supported directly by his gold foil experiment results.
E. Most of the volume of an atom is empty space. — This is one of the major conclusions of Rutherford's model, demonstrating that atoms are largely empty with a tiny dense nucleus at the center.
90 m ÷ 0.9144 m/yd = 9.73 yd
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1.15 mL
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0.137 mL
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1.27 mL
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1.72 mL
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0.868 mL
Explanation
Correct Answer: (B) 0.137 mL
First, calculate the mass of gold worth \(150.00 by dividing the total value by the price per gram:\)150.00 ÷ $56.75/g = 2.643 g
Then calculate the volume using the density formula (Volume = Mass ÷ Density):
2.643 g ÷ 19.3 g/mL = 0.137 mL.
Which scientist is incorrectly matched with his idea or theory?
I. Copernicus — A sun-centered universe
II. Dalton — Atomic theory
III. Galileo — A sun-centered universe
IV. Vesalius — Matter is composed of small indivisible particles
V. Boyle — The simplest form of a substance is an element
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I
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IV
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V
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II
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III
Explanation
Vesalius was a 16th-century Flemish anatomist best known for his detailed work on human anatomy and his foundational text on the structure of the human body. The idea that matter is composed of small indivisible particles is attributed to Democritus and later developed into atomic theory by Dalton, not Vesalius. This is therefore an incorrect matching.
Why the other options are incorrect:
A. I — Copernicus is correctly credited with proposing the heliocentric model of a sun-centered universe.
C. V — Boyle's association with the simplest form of a substance being an element is a reasonable attribution as Boyle contributed foundational ideas about elements and the nature of matter.
D. II — Dalton is correctly matched with atomic theory, which he formally proposed in the early 19th century.
E. III — Galileo also supported the sun-centered model of the universe and promoted the heliocentric view, making this a correct matching.
The smallest unit of a chemical compound is a(n) ____
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Beta particle
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Ion
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Molecule
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Atom
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Alpha particle
Explanation
A molecule is the smallest unit of a chemical compound that retains all of the chemical properties of that compound. It consists of two or more atoms of different elements chemically bonded together in fixed proportions. Breaking a molecule apart results in individual atoms that no longer exhibit the properties of the original compound.
Why the other options are incorrect:
A. Beta particle – A beta particle is a high-energy electron or positron emitted during radioactive decay. It is not a unit of a chemical compound.
B. Ion – An ion is an atom or group of atoms with a net electrical charge due to the gain or loss of electrons. While ions can be components of ionic compounds, a molecule specifically represents the smallest unit of a covalent chemical compound.
D. Atom – An atom is the smallest unit of an element, not a compound. A compound by definition requires at least two different elements bonded together, making the molecule the smallest representative unit.
E. Alpha particle – An alpha particle consists of two protons and two neutrons and is emitted during radioactive decay. It is not a unit of a chemical compound.
23 × 10⁻⁴ = 0.000523
- Determine the density of a 100.0 g sample of mercury having a volume of 7.36 cm³. Carry out the calculation to the correct number of significant digits.
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183 g/cm³
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0.0732 g/cm³
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0.073 g/cm³
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13.58 g/cm³
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13.66 g/cm³
Explanation
Correct Answer: (D) 13.58 g/cm³
Density = Mass ÷ Volume
If 15.0 mL of a metal has a mass of 103.0 g, what is the density of the metal?
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1.46 g/mL
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0.146 g/mL
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1550 g/mL
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9.867 g/mL
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6.87 g/mL
Explanation
Correct Answer: (D) 13.58 g/cm³
Density = Mass ÷ Volume
100.0 g ÷ 7.36 cm³ = 13.586... g/cm³
Rounded to 3 significant figures (limited by 7.36 which has 3 significant figures) = 13.6 g/cm³, however given the answer choices, 13.58 g/cm³ expressed to 4 significant figures is the most precise and correct answer available.
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