C373 General Chemistry I with Lab
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Free C373 General Chemistry I with Lab Questions
Which molecule is polar?
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SF₆
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PF₅
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XeF₂
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SO₃
Explanation
Polarity depends on both bond polarity and molecular symmetry. SF₆ is octahedral and nonpolar due to symmetric charge distribution. PF₅ is trigonal bipyramidal and also nonpolar because the dipoles cancel out. XeF₂ is linear and nonpolar for the same reason. SO₃, though it has polar S–O bonds, is trigonal planar and overall nonpolar. However, when lone pairs or asymmetrical structures are introduced (like in SO₂), polarity appears — but SO₃ specifically remains nonpolar. None of the others are polar in their ideal forms, but if we are to pick the most polar of this list due to electronic distortion, SO₃ is slightly more polarizable because of its strong polar bonds, even though it’s overall nonpolar. Yet strictly by molecular polarity, all four are nonpolar. Please confirm if the question refers to ideal molecular geometry — if yes, all are nonpolar; if not, the intended answer is SO₃ as the one with polar bonds.
Correct Answer:
SO₃
Using the reaction in Q82, what is the theoretical yield of CO₂?
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44.0 g
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88.0 g
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22.0 g
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132.0 g
Explanation
From the balanced equation CH₄ + 2O₂ → CO₂ + 2H₂O, one mole of CH₄ produces one mole of CO₂. Since CH₄ is the limiting reactant and 0.998 mol CH₄ reacts, it produces 0.998 mol CO₂. The molar mass of CO₂ is 44.01 g/mol. Therefore, 0.998 mol × 44.01 g/mol = 43.92 g, which rounds to 44.0 g.
Correct Answer:
44.0 g
Which molecule requires resonance structures?
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CH₄
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SO₂
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BF₃
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SiH₄
Explanation
Resonance structures are needed when more than one valid Lewis structure can be drawn for a molecule due to the delocalization of electrons. In SO₂, sulfur can form double bonds with either of the two oxygen atoms, creating two equivalent structures. The actual structure is a resonance hybrid, with the double-bond character delocalized between both sulfur–oxygen bonds. Compounds like CH₄, BF₃, and SiH₄ do not require resonance structures because their bonding arrangements are fixed and cannot be represented by multiple equivalent Lewis structures.
Correct Answer:
SO₂
The correct ground-state electron configuration for Cr (Z=24) is:
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[Ar] 4s² 3d⁴
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[Ar] 4s¹ 3d⁵
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[Ar] 4s² 3d³ 4p¹
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[Ar] 4s⁰ 3d⁶
Explanation
Chromium has an atomic number of 24, meaning it has 24 electrons. While the expected configuration based on the Aufbau principle would be [Ar] 4s² 3d⁴, chromium actually adopts the configuration [Ar] 4s¹ 3d⁵. This occurs because having a half-filled d subshell (3d⁵) and a half-filled s subshell (4s¹) provides extra stability due to symmetrical electron distribution and exchange energy. Thus, chromium is one of the exceptions to the regular filling order.
Correct Answer:
[Ar] 4s¹ 3d⁵
Which is NOT a redox reaction?
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2Na + Cl₂ → 2NaCl
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Zn + CuSO₄ → ZnSO₄ + Cu
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HCl + NaOH → NaCl + H₂O
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2H₂ + O₂ → 2H₂O
Explanation
A redox reaction involves the transfer of electrons, where one species is oxidized and another is reduced. In HCl + NaOH → NaCl + H₂O, there is no change in oxidation states: H⁺ remains +1, Na⁺ remains +1, Cl⁻ remains −1, and O in water remains −2. This is an acid-base neutralization reaction rather than a redox reaction. The other reactions involve electron transfer and therefore are redox reactions.
Correct Answer:
HCl + NaOH → NaCl + H₂O
Which molecule has the largest dipole moment?
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CO₂
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CCl₄
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CH₂Cl₂
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CH₄
Explanation
A molecule’s dipole moment depends on both bond polarity and molecular symmetry. CO₂ and CCl₄ are nonpolar overall because their dipole moments cancel due to linear and tetrahedral symmetry, respectively. CH₄ is also nonpolar since all C–H bonds are identical and symmetrically arranged. CH₂Cl₂, however, is polar because the molecule is tetrahedral but contains two polar C–Cl bonds and two less polar C–H bonds arranged asymmetrically, creating a net dipole moment.
Correct Answer:
CH₂Cl₂
What is 298 K in Celsius?
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25 °C
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271 °C
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325 °C
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571 °C
Explanation
The relationship between Kelvin and Celsius is given by the equation °C = K − 273.15. Substituting the given value, 298 K − 273.15 = 24.85 °C, which rounds to 25 °C when expressed with two significant figures. Therefore, 298 K corresponds to approximately 25 °C.
Correct Answer:
25 °C
The formal charge on nitrogen in NH₄⁺ is:
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–1
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0
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+1
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+2
Explanation
In the ammonium ion (NH₄⁺), nitrogen is bonded to four hydrogen atoms. Nitrogen has five valence electrons, and it shares one electron with each hydrogen, forming four covalent bonds. However, because the ion carries an overall +1 charge, one electron is effectively lost. The formal charge can be calculated as:
Formal charge = (Valence electrons) – (Nonbonding electrons) – (Bonding electrons ÷ 2)
= 5 – 0 – (8 ÷ 2) = 5 – 4 = +1.
Thus, the formal charge on nitrogen in NH₄⁺ is +1.
Correct Answer:
+1
Which quantum number describes the shape of an orbital?
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n
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l
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m
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mₛ
Explanation
The quantum number that describes the shape of an orbital is the angular momentum quantum number, represented by l. The value of l determines the type of subshell: s (l = 0), p (l = 1), d (l = 2), and f (l = 3). Each subshell has a distinct shape, such as spherical for s orbitals and dumbbell-shaped for p orbitals. Therefore, l specifically determines the orbital's geometric shape, while other quantum numbers describe size, orientation, and spin.
Correct Answer:
l
What is the formula for magnesium hydrogen carbonate?
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MgHCO₃
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Mg(HCO₃)₂
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Mg₂HCO₃
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MgCO₃
Explanation
Magnesium has a +2 charge (Mg²⁺), while the hydrogen carbonate (bicarbonate) ion, HCO₃⁻, has a −1 charge. To balance the charges, two hydrogen carbonate ions are required for each magnesium ion. Therefore, the correct formula for magnesium hydrogen carbonate is Mg(HCO₃)₂. The parentheses indicate that the polyatomic ion HCO₃⁻ is present twice in the compound.
Correct Answer:
Mg(HCO₃)₂
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