Quantum Numbers/Atomic Orbitals
Electron Configurations
Periodic Properties
Ionic and Molecular Bonding
Naming
Lewis Structure/Formal Charge/Resonance
100
Which statement best describes an atomic orbital?
A. Exact path of an electron around the nucleus
B. Region where the electron is most likely to be found
C. Fixed circular electron orbit
D. Region containing exactly two electrons
E. Lowest energy shell for an electron
B. Region where the electron is most likely to be found
100
Which element has the electron configuration:
[Ne] 3s² 3p³
A. Si
B. P
C. S
D. Cl
E. Al
B. P
100
Atomic radius generally _____ across a period.
Decreases
100
What bond is formed by electron transfer between a metal and a nonmetal?
Ionic Bond
100
Name Na₂SO₄
Sodium sulfate
100
Total valence electrons in NH₃?
8
200
Which quantum number determines orbital shape?
A. n
B. mℓ
C. ℓ
D. ms
E. Z
C. ℓ
200
How many valence electrons does manganese (Mn) have?
A. 2
B. 5
C. 7
D. 10
E. 12
C.7
200
Which element has the highest ionization energy?
A. Na
B. Cl
C. Ar
D. Mg
E. K
C. Ar
200
Bond order of a double bond equals:
2
200
Fe₂O₃
Iron(III) oxide
200
Which molecule contains exactly two lone pairs on the central atom?
A. NH₃
B. H₂O
C. CO₂
D. CH₄
E. BF₃
B. H₂O
300
How many orbitals exist in the 4p subshell?
A. 1
B. 3
C. 5
D. 7
E. 9
B. 3
300
Which is the correct electron configuration of Fe³⁺?
A. [Ar] 3d⁵
B. [Ar] 3d³ 4s²
C. [Ar] 3d⁶
D. [Ar] 3d⁴ 4s¹
E. [Kr] 4d⁵
A. [Ar] 3d⁵
300
Which species has the largest radius?
A. O
B. O²⁻
C. F⁻
D. Ne
E. Na⁺
B. O²⁻
300
Which compound contains ONLY covalent bonds?
A. NaCl
B. CaF₂
C. H₂O
D. MgO
E. KBr
C. H₂O
300
N₂O₅
Dinitrogen pentoxide
300
In the best Lewis structure of CO, what is the formal charge on carbon?
A. −1
B. 0
C. +1
D. +2
E. −2
A. −1
400
Which set of quantum numbers is allowed?
A. n=3, ℓ=3, mℓ=0
B. n=4, ℓ=2, mℓ=−3
C.n=2, ℓ=2, mℓ=1
D.n=5, ℓ=1, mℓ=0
E. n=3, ℓ=1, mℓ=2
D.n=5, ℓ=1, mℓ=0
400
Which element does NOT follow the predicted Aufbau filling order?
A. Ca
B. Cr
C. Zn
D. Ar
E. K
B. Cr
400
Which statement explains increasing ionization energy across a period?
A. Increasing shielding
B. Increasing electron pairing
C. Increasing orbital size
D. Increasing effective nuclear charge
E. Decreasing nuclear charge
D. Increasing effective nuclear charge
400
Which bond is expected to be the strongest?
A.Double Bond
B. Triple Bond
C. Single Bond
B. Triple Bond
400
An oxyanion of chlorine contains one fewer oxygen atom than chlorate (ClO₃⁻). What is the correct name and formula of this ion?
A. Hypochlorite, ClO⁻
B. Chlorite, ClO₂⁻
C. Chloride, Cl⁻
D. Perchlorate, ClO₄⁻
E. Chlorate, ClO₃⁻
B. Chlorite, ClO₂⁻
400
Which resonance structure is most stable?
A. Structure with formal charges far from zero
B. Structure with a negative charge on the least electronegative atom
C. Structure minimizing formal charges and placing a negative charge on the most electronegative atom
D. Structure with the maximum number of bonds
E. Structure with the largest central atom
C. Structure minimizing formal charges and placing a negative charge on the most electronegative atom
500
An electron has quantum numbers n=4, ℓ=3.
Which subshell does this electron occupy?
A. 4f
B. 4p
C. 4s
D. 4d
E. 3d
A. 4f
500
Which ion achieves a pseudo-noble-gas configuration?
A. Ca²⁺
B. Na⁺
C. Sn4⁺
D. Al³⁺
E. K⁺
C. Sn4⁺
500
An element shows a large jump between the 3rd and 4th ionization energies.
Which group is it most likely in?
A. Group 1
B. Group 2
C. Group 17
D. Group 15
E. Group 13
E. Group 13
500
What is the fractional bond order in the most reasonable structure of the phosphate (PO43-) anion?
A. 1
B. 2 1/3
C. 1 1/3
D. 1 1/4
E. 1 1/2
D. 1 1/4
500
Which compound is named correctly?
A. Copper chloride
B. Copper chlorine
C. Copper(I) chloride
D. Copper monochloride
E. Copper dichloride
C. Copper(I) chloride
500
Which structure is MOST stable for NCO⁻ ?
3rd option