C373 General Chemistry I with Lab
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Free C373 General Chemistry I with Lab Questions
Rutherford’s gold foil experiment provided evidence for:
- Electrons orbiting in fixed paths
- A dense, positive nucleus
- Neutrons in the nucleus
- Quantized energy levels
Explanation
Rutherford’s gold foil experiment involved directing alpha particles at a thin sheet of gold foil. Most particles passed through, but a few were deflected at large angles. This showed that atoms are mostly empty space, with a small, dense, positively charged center that repelled the alpha particles. This discovery led to the nuclear model of the atom, identifying the nucleus as the core where most of the atom’s mass and positive charge reside.
Correct Answer:
A dense, positive nucleus
Which reaction produces a gas?
- NaCl + AgNO₃
- CaCO₃ + 2HCl
- KBr + Cl₂
- Fe + CuSO₄
Explanation
The reaction between calcium carbonate and hydrochloric acid, CaCO₃ + 2HCl → CaCl₂ + H₂O + CO₂, produces carbon dioxide gas. The other reactions either form precipitates (NaCl + AgNO₃ → AgCl) or involve redox processes without gas formation (KBr + Cl₂ and Fe + CuSO₄).
Correct Answer:
CaCO₃ + 2HCl
In 2Al + 3Cl₂ → 2AlCl₃, how many grams of AlCl₃ are produced from 54.0 g Al?
- 133.5 g
- 267.0 g
- 66.8 g
- 200.3 g
Explanation
First, convert aluminum mass to moles: 54.0 g ÷ 26.98 g/mol = 2.002 mol Al. From the balanced equation, 2 mol Al produce 2 mol AlCl₃, giving a 1:1 molar ratio. Thus, 2.002 mol Al produce 2.002 mol AlCl₃. The molar mass of AlCl₃ is (26.98 + 3 × 35.45) = 133.33 g/mol. Therefore, 2.002 mol × 133.33 g/mol = 267.0 g of AlCl₃.
Correct Answer:
267.0 g
The molecular geometry of XeF₄ is:
- Seesaw
- Square planar
- Square pyramidal
- Octahedral
Explanation
Xenon tetrafluoride (XeF₄) has six regions of electron density around the central xenon atom—four bonding pairs and two lone pairs. According to VSEPR theory, the electron geometry is octahedral, but the two lone pairs occupy positions opposite each other to minimize repulsion. This results in a square planar molecular geometry.
Correct Answer:
Square planar
Which pair has the highest lattice energy?
- NaF
- KBr
- MgO
- CsI
Explanation
Lattice energy increases with higher ionic charges and decreases with larger ionic radii. Among the given compounds, MgO consists of Mg²⁺ and O²⁻ ions, both carrying double charges. The strong electrostatic attraction between these highly charged ions results in a much greater lattice energy compared to the other compounds, which contain singly charged ions. Therefore, MgO has the highest lattice energy due to both high charge magnitude and relatively small ionic sizes.
Correct Answer:
MgO
What is the formula for tin(II) nitrite?
- SnNO₂
- Sn(NO₂)₂
- Sn₂NO₂
- Sn(NO₃)₂
Explanation
Tin(II) indicates that the tin ion has a +2 charge (Sn²⁺). The nitrite ion (NO₂⁻) carries a −1 charge. To balance the charges, two nitrite ions are required for every tin ion, resulting in the formula Sn(NO₂)₂. Parentheses are used around NO₂ because it is a polyatomic ion that appears more than once in the formula.
Correct Answer:
Sn(NO₂)₂
Convert 4.50 × 10⁻⁶ g to micrograms (μg).
- 0.00450 μg
- 4.50 μg
- 4500 μg
- 0.00000450 μg
Explanation
To convert grams to micrograms, multiply by 1,000,000 (since 1 g = 1 × 10⁶ μg). Therefore, 4.50 × 10⁻⁶ g × 1 × 10⁶ μg/g = 4.50 μg. The significant figures remain three because the original value has three significant figures, and unit conversion does not affect the number of significant figures.
Correct Answer:
4.50 μg
A compound contains 35.9% C, 6.7% H, and 57.4% O. Its empirical formula is:
- CH₂O
- C₂H₄O
- C₃H₆O₃
- C₆H₁₂O₆
Explanation
To find the empirical formula, assume 100 g of the compound, which means 35.9 g C, 6.7 g H, and 57.4 g O. Convert each to moles: C = 35.9 ÷ 12.01 = 2.99 mol; H = 6.7 ÷ 1.008 = 6.65 mol; O = 57.4 ÷ 16.00 = 3.59 mol. Divide each by the smallest number of moles (2.99), giving a ratio of approximately C₁H₂.₂O₁. After rounding to whole numbers, this simplifies to CH₂O. Therefore, the empirical formula is CH₂O.
Correct Answer:
CH₂O
Which compound contains primarily ionic bonds?
- CO₂
- NaCl
- CH₄
- N₂
Explanation
Ionic bonds form between metals and nonmetals through the transfer of electrons. In NaCl, sodium (a metal) transfers an electron to chlorine (a nonmetal), forming Na⁺ and Cl⁻ ions held together by strong electrostatic forces. The other compounds—CO₂, CH₄, and N₂—consist of nonmetals only and are held together by covalent bonds, not ionic bonds. Therefore, NaCl is the compound that contains primarily ionic bonds.
Correct Answer:
NaCl
A 4.00 L sample of N₂ at 300 K and 2.00 atm is heated to 600 K at constant pressure. New volume?
- 2.00 L
- 4.00 L
- 6.00 L
- 8.00 L
Explanation
Using Charles’s Law (V₁/T₁ = V₂/T₂) at constant pressure, V₂ = V₁ × (T₂/T₁). Substituting values: V₂ = 4.00 L × (600 K / 300 K) = 4.00 × 2 = 8.00 L. Therefore, the volume doubles when the temperature is doubled at constant pressure.
Correct Answer:
8.00 L
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