109 年 國立成功大學地球科學研究所甲組《普通化學》

Which of the following compound(s) is thermodynamically more stable than an $\mathrm{N_2}$ molecule?

(A) $\mathrm{N_2O}$
(B) $\mathrm{NO}$
(C) $\mathrm{NO_2}$
(D) $\mathrm{N_2H_4}$
(E) $\mathrm{NH_3}$

A certain metal fluoride crystallizes in such a way that the fluoride ions occupy simple cubic lattice sites, while the metal atoms occupy the body centers of half the cubes.

What is the formula for this metal fluoride?

(A) $\mathrm{MF_2}$
(B) $\mathrm{M_2F}$
(C) $\mathrm{MF}$
(D) $\mathrm{MF_6}$
(E) $\mathrm{M_2F_3}$

Which of the following is the correct order of boiling points for $\mathrm{KNO_3}$, $\mathrm{CH_3OH}$, $\mathrm{C_2H_6}$, and $\mathrm{Ne}$?

(A) $\mathrm{KNO_3}<\mathrm{CH_3OH}<\mathrm{C_2H_6}<\mathrm{Ne}$
(B) $\mathrm{CH_3OH}<\mathrm{Ne}<\mathrm{C_2H_6}<\mathrm{KNO_3}$
(C) $\mathrm{Ne}<\mathrm{C_2H_6}<\mathrm{KNO_3}<\mathrm{CH_3OH}$
(D) $\mathrm{Ne}<\mathrm{C_2H_6}<\mathrm{CH_3OH}<\mathrm{KNO_3}$
(E) $\mathrm{C_2H_6}<\mathrm{Ne}<\mathrm{CH_3OH}<\mathrm{KNO_3}$

Consider two liquids, $\mathrm{A}$ and $\mathrm{B}$. Liquid $\mathrm{A}$ exhibits stronger intermolecular forces than liquid $\mathrm{B}$.

Which of the following statements is true?

(A) The surface tension and viscosity of liquid $\mathrm{A}$ are greater than those of liquid $\mathrm{B}$.
(B) The surface tension of liquid $\mathrm{A}$ is greater than that of liquid $\mathrm{B}$; the viscosity of liquid $\mathrm{B}$ is greater than that of liquid $\mathrm{A}$.
(C) The surface tension of liquid $\mathrm{B}$ is greater than that of liquid $\mathrm{A}$; the viscosity of liquid $\mathrm{A}$ is greater than that of liquid $\mathrm{B}$.
(D) The surface tension and viscosity of liquid $\mathrm{B}$ are greater than those of liquid $\mathrm{A}$.
(E) The surface tension of liquid $\mathrm{A}$ is greater than that of liquid $\mathrm{B}$, but the viscosities of the two liquids are the same.

Which one of the following is the strongest intermolecular force experienced by noble gases?

(A) Hydrogen bonding
(B) Dipole–dipole interactions
(C) London dispersion forces
(D) Ion–ion interactions
(E) Covalent bonding

Boron naturally occurs in two isotopic forms. The more common isotope is ${}^{11}\mathrm{B}$ (atomic mass $11.01\ \mathrm{amu}$), which is $80.00\%$ abundant. The average atomic mass of boron is $10.81$.

What is the mass of the other isotope?

(A) $10.91\ \mathrm{amu}$
(B) $10.01\ \mathrm{amu}$
(C) $11.00\ \mathrm{amu}$
(D) $11.01\ \mathrm{amu}$
(E) $10.81\ \mathrm{amu}$

The $K_{\mathrm{w}}$ of water at $25^\circ\mathrm{C}$ is $1\times10^{-14}$. If the autoionization of water is endothermic, which of the following statements is correct for water at $50^\circ\mathrm{C}$?

(A) $K_{\mathrm{w}}$ is larger than $1\times10^{-14}$.
(B) $K_{\mathrm{w}}$ is smaller than $1\times10^{-14}$.
(C) $K_{\mathrm{w}}$ is $1\times10^{-14}$.
(D) The $\mathrm{pH}$ value is larger than $7$.
(E) The $\mathrm{pH}$ value is $7$.

Which of the following solutions has the titration curve on the right?

🖼️【此處有附圖，請對照原卷】

(A) $\mathrm{NH_3}$
(B) $\mathrm{CO_3^{2-}}$
(C) $\mathrm{HCN}$
(D) $\mathrm{PO_4^{3-}}$
(E) $\mathrm{NaOH}$

How many of the following oxides are amphoteric?

$\mathrm{Al_2O_3}$, $\mathrm{Ga_2O_3}$, $\mathrm{BeO}$, $\mathrm{MgO}$, $\mathrm{CaO}$, $\mathrm{SrO}$, $\mathrm{BaO}$, $\mathrm{RaO}$

(A) $1$
(B) $2$
(C) $3$
(D) $4$
(E) $5$

How many of the following processes involve an increase in the entropy of the system?

Melting of a solid, sublimation, freezing, diffusion, evaporation of a liquid

(A) $1$
(B) $2$
(C) $3$
(D) $4$
(E) $5$

A certain first-order reaction has a half-life of $40\ \mathrm{min}$. How much time is required for this reaction to be $87.5\%$ complete?

(A) $20\ \mathrm{min}$
(B) $40\ \mathrm{min}$
(C) $80\ \mathrm{min}$
(D) $120\ \mathrm{min}$
(E) $160\ \mathrm{min}$

For the reaction $\mathrm{A}+\mathrm{B}\rightarrow\text{products}$, the following data were obtained:

What is the experimental rate law?

(A) $\mathrm{Rate}=k[\mathrm{A}]$
(B) $\mathrm{Rate}=k[\mathrm{B}]$
(C) $\mathrm{Rate}=k[\mathrm{A}][\mathrm{B}]$
(D) $\mathrm{Rate}=k[\mathrm{A}]^2[\mathrm{B}]$
(E) $\mathrm{Rate}=k[\mathrm{A}][\mathrm{B}]^2$

The following are produced by radioactive processes. Which one has mass but no charge?

(A) Alpha particle
(B) Beta particle
(C) Gamma ray
(D) Neutron
(E) Positron

How many of the following molecules have a free radical?

Superoxide, peroxide, nitric oxide, carbon monoxide, nitrous oxide, ozone

(A) $1$
(B) $2$
(C) $3$
(D) $4$
(E) $5$

A chemist needs to prepare a buffered solution using one of the following acids (and its sodium salt):

$\mathrm{HA}$ ($K_{\mathrm{a}}=1.35\times10^{-3}$)
$\mathrm{HB}$ ($K_{\mathrm{a}}=1.1\times10^{-5}$)
$\mathrm{HC}$ ($K_{\mathrm{a}}=6.4\times10^{-5}$)
$\mathrm{HD}$ ($K_{\mathrm{a}}=3.5\times10^{-7}$)
$\mathrm{HE}$ ($K_{\mathrm{a}}=1.89\times10^{-8}$)

To prepare a solution buffered at $\mathrm{pH}=5.10$, which system will work best?

(A) $\mathrm{HA}$ and its sodium salt
(B) $\mathrm{HB}$ and its sodium salt
(C) $\mathrm{HC}$ and its sodium salt
(D) $\mathrm{HD}$ and its sodium salt
(E) $\mathrm{HE}$ and its sodium salt

Regarding a $\mathrm{B_2}$ molecule, which of the following statements is true?

(A) The bond order of the $\mathrm{B_2}$ molecule is two.
(B) The highest occupied molecular orbital (HOMO) is $\sigma_{2p}$.
(C) The lowest unoccupied molecular orbital (LUMO) is $\sigma_{2p}^{*}$.
(D) The $\mathrm{B_2}$ molecule is a paramagnetic species.
(E) The lowest unoccupied molecular orbital (LUMO) is $\pi_{2p}^{*}$.

How many “three-center bonds” does a diborane molecule ($\mathrm{B_2H_6}$) have?

(A) $1$
(B) $2$
(C) $3$
(D) $4$
(E) $5$

Please indicate the order of wavelength for the following radiation (in decreasing order).

(I) Microwave frequency
(II) Radio frequency
(III) Infrared light
(IV) $\gamma$-ray frequency

(A) I, II, III, IV
(B) IV, III, I, II
(C) II, I, III, IV
(D) III, IV, I, II
(E) IV, III, II, I

Which of the following statements is NOT true?

(A) The reaction constant might change when the reaction temperature changes.
(B) The reaction constant won't change when the concentration of reactants changes.
(C) The reaction constant might change when the catalyst is added to the reaction.
(D) The activation energy for a reaction might change when the catalyst is added.
(E) The activation energy for a reaction might change when the reaction temperature changes.

Please balance the following equation ($o$, $p$, $q$, $x$, $y$, $z$ are reaction coefficients). What is the sum of all coefficients, $o+p+q+x+y+z$?

(A) $18$
(B) $20$
(C) $22$
(D) $24$
(E) $26$

The graph shows the concentration of reactants versus reaction time in four different first-order reactions. Which reaction has the largest reaction rate constant?

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(A) I
(B) II
(C) III
(D) IV
(E) The same

Which of the following plots shows that the reaction $\mathrm{A}\rightarrow\mathrm{B}$ is a second-order reaction?

$[\mathrm{A}]$: the concentration of $\mathrm{A}$.

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(A) Figure 1
(B) Figure 2
(C) Figure 3
(D) Figure 4

The formation rate of dichromate ($\mathrm{Cr_2O_7^{2-}}$) ions is $0.32\ \mathrm{mol\,L^{-1}\,s^{-1}}$ in the reaction

What is the reaction rate of chromate ions ($\mathrm{CrO_4^{2-}}$) in the reaction?

(A) $0.16\ \mathrm{mol\,L^{-1}\,s^{-1}}$
(B) $0.32\ \mathrm{mol\,L^{-1}\,s^{-1}}$
(C) $0.64\ \mathrm{mol\,L^{-1}\,s^{-1}}$
(D) $1.28\ \mathrm{mol\,L^{-1}\,s^{-1}}$

Which of the following is NOT determined by the principal quantum number $n$ of the electron in a hydrogen atom?

(A) The energy of the electron
(B) The minimum wavelength of the light needed to remove the electron from the atom
(C) The size of the corresponding atomic orbital(s)
(D) The shape of the corresponding atomic orbital(s)
(E) All of these are determined by $n$.

The observed osmotic pressure for a $0.10\ \mathrm{M}$ solution of $\mathrm{FeCl_3}$ at $27^\circ\mathrm{C}$ is $7.38\ \mathrm{atm}$.

What are the expected and experimental values for $i$ (van't Hoff factor)? The gas law constant is $0.082\ \mathrm{L\,atm\,K^{-1}\,mol^{-1}}$.

(A) Expected value is $4$, experimental value is $3.8$.
(B) Expected value is $4$, experimental value is $3.6$.
(C) Expected value is $4$, experimental value is $3.0$.
(D) Expected value is $3$, experimental value is $3.8$.
(E) Expected value is $3$, experimental value is $3.6$.

Which of the following statements is NOT true?

(A) The $2s$ and $2p$ orbitals are degenerate in a hydrogen atom.
(B) The $2s$ orbital has two nodes which are areas of zero electron probability.
(C) The $d$ orbital has $5$ subshells.
(D) The dependence of the wave function on the angular momentum quantum number determines the shapes of the atomic orbital.
(E) The $d$ orbitals are degenerate in the $\mathrm{Fe^{2+}}$ free ion, but not in the $[\mathrm{FeCl_4}]^{2-}$ complex.

For an unstable proton-rich nuclide, which of the following decay processes is most unlikely to occur in order to reach a stable nucleus?

(A) $\beta^{-}$ emission
(B) Proton emission
(C) Positron production
(D) Electron capture
(E) $\alpha$-particle production

Which of the following is a buffer solution with the best capacity?

(A) $1.0\ \mathrm{L}$ solution containing $0.50\ \mathrm{M}$ $\mathrm{NaOH}$ and $0.50\ \mathrm{M}$ $\mathrm{HCl}$
(B) $1.0\ \mathrm{L}$ solution containing $0.05\ \mathrm{M}$ $\mathrm{NaOCl}$ and $0.50\ \mathrm{M}$ $\mathrm{HOCl}$
(C) $1.0\ \mathrm{L}$ solution containing $0.50\ \mathrm{M}$ $\mathrm{NH_4OH}$ and $0.50\ \mathrm{M}$ $\mathrm{NH_4Cl}$
(D) $1.0\ \mathrm{L}$ solution containing $0.50\ \mathrm{M}$ $\mathrm{NaCl}$ and $0.50\ \mathrm{M}$ $\mathrm{HCl}$
(E) $1.0\ \mathrm{L}$ solution containing $0.50\ \mathrm{M}$ $\mathrm{NaF}$ and $0.05\ \mathrm{M}$ $\mathrm{HF}$

Mixing $500\ \mathrm{mL}$ of $0.20\ \mathrm{M}$ $\mathrm{CH_3COOH}$ solution and $500\ \mathrm{mL}$ of $0.20\ \mathrm{M}$ $\mathrm{CH_3COONa}$ solution, what is the final $\mathrm{pH}$ value?

$K_{\mathrm{a}}$ for $\mathrm{CH_3COOH}=1.8\times10^{-5}$.

(A) $6.25$
(B) $4.85$
(C) $3.75$
(D) $5.25$
(E) $5.75$

The structure of pentose is shown in the right figure. How many carbon atoms with chirality are in this molecule?

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(A) $1$
(B) $2$
(C) $3$
(D) $4$
(E) $5$

What amount of $\mathrm{Al_{(s)}}$ can be produced from $\mathrm{Al_2O_3}$ if $5$ moles of electrons are supplied? The atomic mass of $\mathrm{Al}$ is $26.98$.

(A) $135\ \mathrm{g}$
(B) $67\ \mathrm{g}$
(C) $45\ \mathrm{g}$
(D) $81\ \mathrm{g}$
(E) $54\ \mathrm{g}$