General Chemistry University

General Chemistry Exam - Atomic Structure, Periodic Table, and Chemical Bonding

100 câu

120 phút

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Thông tin đề

Môn: General Chemistry
Kỳ thi: University
Số câu: 100 câu
Thời gian: 120 phút
Đáp án: ✓ Có giải thích

Nội dung đề (100 câu)

Câu 1.
Which scientist proposed the atomic model describing atoms as solid, indivisible spheres?
- A.
  J.J. Thomson
- B.
  J. Dalton
- C.
  E. Rutherford
- D.
  N. Bohr
Câu 2.
Which scientist discovered the electron through his experiments with cathode rays?
- A.
  J. Dalton
- B.
  N. Bohr
- C.
  J.J. Thomson
- D.
  E. Rutherford
Câu 3.
Which experiment led to the discovery of the atomic nucleus?
- A.
  Cathode ray experiment
- B.
  Gold foil (alpha particle) experiment
- C.
  Hydrogen spectrum analysis
- D.
  Oil drop experiment
Câu 4.
Which atomic model successfully explained the hydrogen emission spectrum?
- A.
  Dalton's model
- B.
  Thomson's model
- C.
  Rutherford's model
- D.
  Bohr's model
Câu 5.
What is the relative charge of a proton?
- A.
  +1
- B.
  -1
- C.
  0
- D.
  +2
Câu 6.
Which subatomic particle has a charge of 0 (electrically neutral)?
- A.
  Proton
- B.
  Electron
- C.
  Neutron
- D.
  Positron
Câu 7.
The ratio of proton mass to electron mass () is approximately:
- A.
  18
- B.
  183
- C.
  1836
- D.
  18360
Câu 8.
The atomic number Z of an element represents:
- A.
  Number of neutrons in the nucleus
- B.
  Number of protons in the nucleus
- C.
  Mass number of the atom
- D.
  Number of electrons in a molecule
Câu 9.
In a neutral atom, the number of protons is equal to the number of:
- A.
  Neutrons
- B.
  Electrons
- C.
  Mass number
- D.
  Nucleons always
Câu 10.
An atom has 11 protons and 12 neutrons. What is its mass number A?
- A.
  11
- B.
  12
- C.
  23
- D.
  1
Câu 11.
Isotopes of the same element have the same number of:
- A.
  Neutrons
- B.
  Protons
- C.
  Mass numbers
- D.
  Electrons in ions
Câu 12.
Chlorine has two isotopes: (75.4%) and (24.6%). What is the average atomic mass of chlorine?
- A.
  35.0
- B.
  35.45
- C.
  36.0
- D.
  36.5
Câu 13.
How many neutrons are in carbon-13 ()?
- A.
  6
- B.
  7
- C.
  12
- D.
  13
Câu 14.
Which symbol correctly represents deuterium (hydrogen-2)?
- A.
- B.
- C.
- D.
Câu 15.
Which of the following is true about isotopes?
- A.
  They have different chemical properties
- B.
  They have the same chemical properties
- C.
  They have the same physical properties always
- D.
  They have the same mass number
Câu 16.
Which element has only one proton in its nucleus?
- A.
  Helium
- B.
  Hydrogen
- C.
  Lithium
- D.
  Carbon
Câu 17.
How many electrons can occupy a 3p subshell in total?
- A.
  2
- B.
  6
- C.
  10
- D.
  14
Câu 18.
What is the maximum number of electrons a d subshell can hold?
- A.
  2
- B.
  6
- C.
  10
- D.
  14
Câu 19.
How many orbitals are present in an f subshell?
- A.
  1
- B.
  3
- C.
  5
- D.
  7
Câu 20.
According to Pauli's exclusion principle:
- A.
  Electrons pair up first in orbitals
- B.
  Each orbital can hold a maximum of 2 electrons with opposite spins
- C.
  Electrons fill from high to low energy
- D.
  Electrons always repel each other
Câu 21.
Hund's rule states that when filling orbitals of equal energy:
- A.
  Each orbital is filled completely before moving on
- B.
  Electrons maximize the number of unpaired electrons with parallel spins first
- C.
  Lower energy levels fill first
- D.
  Electrons pair with opposite spins
Câu 22.
What is the correct order of orbital filling according to Kleshkovski's (Aufbau) rule?
- A.
  1s, 2s, 2p, 3s, 3p, 4s, 3d, 4p
- B.
  1s, 2s, 2p, 3s, 3p, 3d, 4s, 4p
- C.
  1s, 2s, 3s, 2p, 3p, 4s
- D.
  1s, 2s, 2p, 3p, 3s, 4s
Câu 23.
Which of the following subshells does NOT exist?
- A.
  2p
- B.
  3s
- C.
  2d
- D.
  4f
Câu 24.
What is the maximum number of electrons that can occupy the 4th electron shell (n=4)?
- A.
  2
- B.
  8
- C.
  18
- D.
  32
Câu 25.
What is the correct electron configuration of sodium (Na, Z=11)?
- A.
- B.
- C.
- D.
Câu 26.
What is the correct electron configuration of the chloride ion Cl⁻ (Z=17)?
- A.
- B.
- C.
- D.
Câu 27.
How many electrons does the Fe²⁺ ion have if neutral Fe has Z=26?
- A.
  24
- B.
  25
- C.
  26
- D.
  27
Câu 28.
What is the correct electron configuration of Fe³⁺ (Z=26)?
- A.
- B.
- C.
- D.
Câu 29.
How many valence electrons does aluminum (Al, Z=13) have?
- A.
  1
- B.
  2
- C.
  3
- D.
  13
Câu 30.
An atom has the electron configuration . Which element is it?
- A.
  Sodium (Na)
- B.
  Potassium (K)
- C.
  Calcium (Ca)
- D.
  Bromine (Br)
Câu 31.
Who is credited with the discovery of the periodic law in 1869?
- A.
  John Newlands
- B.
  Antoine Lavoisier
- C.
  Dmitry Mendeleev
- D.
  Lothar Meyer
Câu 32.
What is the fundamental principle that governs the arrangement of elements in the modern periodic table?
- A.
  Increasing atomic mass
- B.
  Increasing atomic number (nuclear charge)
- C.
  Alphabetical order
- D.
  Group of similar compounds
Câu 33.
Elements in the same period of the periodic table have the same:
- A.
  Number of valence electrons
- B.
  Number of electron shells
- C.
  Chemical properties
- D.
  Atomic mass
Câu 34.
Elements in the same group (column) have the same:
- A.
  Atomic mass
- B.
  Number of electron shells
- C.
  Number of valence electrons
- D.
  Atomic radius
Câu 35.
How many periods are there in the modern periodic table?
- A.
  5
- B.
  6
- C.
  7
- D.
  8
Câu 36.
How many groups (columns) are there in the modern periodic table?
- A.
  8
- B.
  16
- C.
  18
- D.
  32
Câu 37.
How many elements does Period 1 contain?
- A.
  2
- B.
  6
- C.
  8
- D.
  18
Câu 38.
Periods 4 and 5 each contain how many elements?
- A.
  8
- B.
  18
- C.
  32
- D.
  36
Câu 39.
Which type of element typically begins each period (except Period 1)?
- A.
  An alkaline earth metal
- B.
  An alkali metal
- C.
  A halogen
- D.
  A noble gas
Câu 40.
Which type of element ends each period of the periodic table?
- A.
  An alkali metal
- B.
  A transition metal
- C.
  A halogen
- D.
  A noble gas
Câu 41.
Group A elements (main group) are those whose last electron enters:
- A.
  A d subshell
- B.
  An s or p subshell
- C.
  An f subshell
- D.
  Any inner subshell
Câu 42.
Group B (subgroup) elements are those whose last electron enters:
- A.
  An s subshell
- B.
  A p subshell
- C.
  A d subshell
- D.
  An f subshell always
Câu 43.
The element with electron configuration [Ar] belongs to which group?
- A.
  Group IIA
- B.
  Group IIB
- C.
  Group IA
- D.
  Group IB
Câu 44.
The element Sc (Z=21) with configuration [Ar] belongs to which group?
- A.
  Group IIIA
- B.
  Group IIIB
- C.
  Group IIB
- D.
  Group IVA
Câu 45.
The element Cu (Z=29) with configuration [Ar] belongs to which group?
- A.
  Group IB
- B.
  Group IA
- C.
  Group IIB
- D.
  Group IIIB
Câu 46.
An element has the configuration . In which period and group is it located?
- A.
  Period 4, group VIIB
- B.
  Period 5, group VIIB
- C.
  Period 4, group VIIA
- D.
  Period 3, group VIIB
Câu 47.
How does atomic radius generally change across a period from left to right?
- A.
  Increases
- B.
  Decreases
- C.
  Stays the same
- D.
  Doubles
Câu 48.
How does atomic radius generally change down a group?
- A.
  Increases
- B.
  Decreases
- C.
  Stays the same
- D.
  Halves
Câu 49.
How does first ionization energy generally change across a period from left to right?
- A.
  Increases
- B.
  Decreases
- C.
  Stays the same
- D.
  Doubles
Câu 50.
How does ionization energy generally change down a group?
- A.
  Increases
- B.
  Decreases
- C.
  Stays the same
- D.
  Stays the same always
Câu 51.
How does electronegativity generally change across a period from left to right?
- A.
  Increases
- B.
  Decreases
- C.
  Stays the same
- D.
  Varies randomly
Câu 52.
How does metallic character change across a period from left to right?
- A.
  Increases
- B.
  Decreases
- C.
  Stays the same
- D.
  Doubles
Câu 53.
Which element has the highest electronegativity?
- A.
  Fluorine (F)
- B.
  Chlorine (Cl)
- C.
  Oxygen (O)
- D.
  Nitrogen (N)
Câu 54.
Which of the following elements has the lowest electronegativity?
- A.
  Hydrogen (H)
- B.
  Lithium (Li)
- C.
  Cesium (Cs)
- D.
  Sodium (Na)
Câu 55.
Compared to its parent neutral atom, the radius of a cation is:
- A.
  Larger
- B.
  Smaller
- C.
  The same size
- D.
  Variable randomly
Câu 56.
Compared to its parent neutral atom, the radius of an anion is:
- A.
  Larger
- B.
  Smaller
- C.
  The same size
- D.
  Variable randomly
Câu 57.
Which of the following alkali metals has the largest atomic radius?
- A.
  Li
- B.
  Na
- C.
  K
- D.
  Cs
Câu 58.
Which element has the smallest atomic radius in Period 3?
- A.
  Na
- B.
  Al
- C.
  P
- D.
  Cl
Câu 59.
John Newlands' periodic table (1863-1866) was based on sets of:
- A.
  7
- B.
  8
- C.
  9
- D.
  10
Câu 60.
De Chancourtois' periodic table was known as:
- A.
  Tellurium helix
- B.
  Periodic law
- C.
  Octaves
- D.
  Spiral table
Câu 61.
Which of the following is a stable noble gas electron configuration?
- A.
- B.
- C.
- D.
Câu 62.
An element has the outermost electron configuration . In which period and group is it located?
- A.
  Period 5, group IIA
- B.
  Period 5, group IIB
- C.
  Period 4, group IIB
- D.
  Period 6, group IIB
Câu 63.
Group VIII B consists of how many columns in the periodic table?
- A.
  1
- B.
  2
- C.
  3
- D.
  4
Câu 64.
How many elements are in Period 6 of the periodic table?
- A.
  18
- B.
  32
- C.
  36
- D.
  50
Câu 65.
Which element has the highest first ionization energy?
- A.
  Li
- B.
  Na
- C.
  He
- D.
  F
Câu 66.
Which type of bond is formed by the electrostatic attraction between oppositely charged ions?
- A.
  Covalent bond
- B.
  Ionic bond
- C.
  Metallic bond
- D.
  Hydrogen bond
Câu 67.
Which type of bond is characteristic of metals?
- A.
  Covalent bond
- B.
  Ionic bond
- C.
  Metallic bond
- D.
  Hydrogen bond
Câu 68.
A covalent bond is formed by:
- A.
  Complete transfer of electrons
- B.
  Sharing of electron pairs between atoms
- C.
  Electrostatic attraction of ions
- D.
  A free electron cloud
Câu 69.
A polar covalent bond forms when:
- A.
  Two identical atoms bond together
- B.
  Two atoms with different electronegativities share electrons unequally
- C.
  Electrons are completely transferred
- D.
  Only ions attract each other
Câu 70.
A nonpolar covalent bond forms when:
- A.
  Two atoms have different electronegativities
- B.
  Two identical atoms share electrons equally
- C.
  Electrons are completely transferred
- D.
  A metal bonds with a nonmetal
Câu 71.
Which of the following molecules contains only nonpolar covalent bonds?
- A.
  HCl
- B.
  H₂O
- C.
  N₂
- D.
  NH₃
Câu 72.
Which of the following molecules contains a polar covalent bond?
- A.
  O₂
- B.
  Cl₂
- C.
  H₂
- D.
  H₂O
Câu 73.
The bond in the HCl molecule is classified as:
- A.
  Ionic bond
- B.
  Polar covalent bond
- C.
  Nonpolar covalent bond
- D.
  Metallic bond
Câu 74.
The bond in NaCl is best described as:
- A.
  Covalent bond
- B.
  Ionic bond
- C.
  Metallic bond
- D.
  Hydrogen bond
Câu 75.
An ionic bond is typically formed when the electronegativity difference (Δχ) between two atoms is:
- A.
  0 ≤ Δχ ≤ 1.7
- B.
  Δχ > 1.7
- C.
  Δχ = 0
- D.
  Δχ < 0
Câu 76.
A covalent bond is typically formed when the electronegativity difference (Δχ) is:
- A.
  0 ≤ Δχ ≤ 1.7
- B.
  Δχ > 1.7
- C.
  Δχ = 1.7 exactly
- D.
  Δχ < 0
Câu 77.
Which property is greater when the bond length is shorter?
- A.
  Bond energy
- B.
  Atomic radius
- C.
  Ionic radius
- D.
  Polarizability
Câu 78.
Bond energy is defined as:
- A.
  The energy required to break one mole of bonds in the gaseous state
- B.
  The length between atomic nuclei
- C.
  The polarity of a bond
- D.
  The angle between bonded atoms
Câu 79.
Bond length is defined as:
- A.
  The energy required to break a bond
- B.
  The shortest distance between two bonded atomic nuclei
- C.
  The angle between atoms
- D.
  The sharing of electrons
Câu 80.
A hydrogen bond is formed between hydrogen and an element with:
- A.
  Low electronegativity
- B.
  High electronegativity
- C.
  Zero electronegativity
- D.
  No relation to electronegativity
Câu 81.
Hydrogen bonds are commonly formed between hydrogen and which of the following elements?
- A.
  F, O, Cl, N
- B.
  C, H, N, O
- C.
  Na, K, Li
- D.
  He, Ne, Ar
Câu 82.
Intermolecular hydrogen bonds typically cause a substance to have:
- A.
  Lower boiling points
- B.
  Higher boiling points
- C.
  No change in boiling points
- D.
  Lower melting points
Câu 83.
Van der Waals bonds are characterized as:
- A.
  Directional
- B.
  Non-directional and non-saturated
- C.
  Saturated
- D.
  Highly polar
Câu 84.
Which of the following is NOT a property of van der Waals bonds?
- A.
  Non-directional
- B.
  Non-saturated
- C.
  Non-selective
- D.
  Highly polar and strong
Câu 85.
Which of the following is NOT a type of van der Waals interaction?
- A.
  Directional (Keesom) interaction
- B.
  Inductive (Debye) interaction
- C.
  Dispersion (London) interaction
- D.
  Coordinate (dative) bond
Câu 86.
The octet rule states that atoms tend to achieve a stable configuration with:
- A.
  2 electrons in their outer shell
- B.
  8 electrons in their outer shell
- C.
  8 electrons in their inner shell
- D.
  18 electrons in their outer shell
Câu 87.
In a Lewis electron-dot symbol, the dots represent:
- A.
  Protons in the nucleus
- B.
  Neutrons in the nucleus
- C.
  Valence electrons
- D.
  Inner (core) electrons
Câu 88.
A sigma (σ) bond is formed by:
- A.
  End-to-end (axial) overlap of orbitals
- B.
  Side-by-side (parallel) overlap of orbitals
- C.
  Electron transfer between atoms
- D.
  Ionic interaction
Câu 89.
A pi (π) bond is formed by:
- A.
  End-to-end (axial) overlap of orbitals
- B.
  Side-by-side (lateral) overlap of orbitals
- C.
  s-s overlap only
- D.
  Ionic interaction
Câu 90.
sp³ hybridization involves the mixing of:
- A.
  1 s orbital and 3 p orbitals
- B.
  2 s orbitals and 2 p orbitals
- C.
  1 s orbital and 2 p orbitals
- D.
  3 s orbitals and 1 p orbital
Câu 91.
The approximate bond angle in sp³ hybridization is:
- A.
  90°
- B.
  109.5°
- C.
  120°
- D.
  180°
Câu 92.
What is the molecular geometry of CH₄ (with sp³ central carbon atom)?
- A.
  Trigonal planar
- B.
  Tetrahedral
- C.
  Linear
- D.
  Bent
Câu 93.
According to VSEPR theory, what is the geometry of CO₂?
- A.
  Linear
- B.
  Trigonal planar
- C.
  Tetrahedral
- D.
  Bent
Câu 94.
What is the molecular geometry of NH₃?
- A.
  Trigonal planar
- B.
  Tetrahedral (electron)
- C.
  Trigonal pyramidal
- D.
  Bent
Câu 95.
What is the molecular geometry of H₂O?
- A.
  Linear
- B.
  Trigonal planar
- C.
  Bent (angular)
- D.
  Tetrahedral
Câu 96.
Which of the following molecules is nonpolar (has zero dipole moment)?
- A.
  HCl
- B.
  H₂O
- C.
  CO₂
- D.
  NH₃
Câu 97.
Which of the following molecules has a net dipole moment (is polar)?
- A.
  CO₂
- B.
  BeCl₂
- C.
  H₂O
- D.
  CF₄
Câu 98.
In VSEPR theory, multiple bonds (double or triple) are counted as:
- A.
  Two or three electron pairs
- B.
  One electron domain (one effective pair)
- C.
  Three electron pairs
- D.
  Zero electron pairs
Câu 99.
According to valence bond theory, the greater the overlap of atomic orbitals, the:
- A.
  Weaker the bond
- B.
  Stronger the bond
- C.
  Same bond strength always
- D.
  More polar the bond always
Câu 100.
Bond energy depends on:
- A.
  Bond length only
- B.
  Bond length and bond order
- C.
  Atomic mass only
- D.
  Number of atoms only

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