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WorksheetsCHM 101 FINAL MOCK 2025
Total questions: 42
Worksheet time: 24mins
Calculate the kinetic energy (in J) of a 75.0 kg person running at 1.78 m/s.
112 J
119 J
125 J
133 J
What is the potential energy (in kJ) of a 1360 kg car parked 36.6 m above ground? (g = 9.806 m/s²)
450 kJ
488 kJ
512 kJ
530 kJ
Calculate work (in J) when a gas expands from 46 L to 64 L against 15 atm. (1 atm·L = 101.325 J)
–27,400 J
–27,357 J
–25,000 J
–18,200 J
How much heat (in J) is absorbed by 15.0 g of water heated from 20.0°C to 50.0°C? (Cₛ = 4.18 J/g·°C)
1,500 J
1,880 J
2,100 J
2,500 J
For a system where 15.6 kJ of heat is absorbed and 1.4 kJ of work is done *on* it, what is ΔU?
14.2 kJ
15.6 kJ
17.0 kJ
18.4 kJ
A gas is compressed from 400 mL to 60.0 mL at 8.00 atm, and 140 J of heat is *released*. What is ΔU?
–135 J
+136 J
–276 J
+416 J
How much heat is released when 4.50 g of CH₄ burns? (ΔH = –890 kJ/mol)
–150 kJ
–200 kJ
–250 kJ
–300 kJ
If 2H₂(g) + O₂(g) → 2H₂O(l) releases 572 kJ, what is ΔH for H₂(g) + ½O₂(g) → H₂O(l)?
–572 kJ
–286 kJ
+286 kJ
+572 kJ
A 4.82 g metal at 115.0°C is placed in 35 mL water at 28.7°C. Final T = 34.5°C. What is Cₘₑₜₐₗ?
0.385 J/g·°C
1.25 J/g·°C
2.19 J/g·°C
4.18 J/g·°C
50.0 mL of 1.0 M HCl + 50.0 mL of 1.0 M NaOH → ΔT = 6.5°C. What is ΔH per mole of HCl?
–27 kJ/mol
–54 kJ/mol
–81 kJ/mol
–108 kJ/mol
According to Dalton’s theory, atoms of the same element are:
Identical in mass and properties
Differ only in charge
Always found in pairs
Indivisible but variable in mass
Who proposed the idea of isotopes in 1912?
J.J. Thomson
Ernest Rutherford
Frederick Soddy
Niels Bohr
In Thomson’s “plum pudding” model, electrons are embedded in:
A nucleus of protons
A sphere of positive charge
Orbiting shells
Neutron soup
Rutherford’s gold foil experiment showed the nucleus is how many times smaller than the atom?
100
1,000
10,000
100,000
The Bohr model restricts electrons to:
Elliptical orbits
No in-between states
Probability clouds
Spiral decay paths
What did Faraday’s electrolysis experiments suggest about atoms?
They contain neutrons
They have electrical component
They emit light when excited
They are mostly empty space
Which subatomic particle did J.J. Thomson discover using cathode ray tubes?
Proton
Neutron
Electron
Positron
In the quantum mechanical model, what does ψ² represent?
Electron spin direction
Orbital angular momentum
Probability density
Energy quantization
For n = 3, how many orbitals are possible?
3
6
9
18
Which quantum number defines orbital shape?
For n = 3, how many orbitals are possible?
3
6
9
18
Which quantum number defines orbital shape?
n
l
mₗ
mₛ
What is the electron configuration anomaly for chromium?
[Ar] 4s² 3d⁴
[Ar] 4s¹ 3d⁵
[Ar] 4s⁰ 3d⁶
[Ar] 4s² 3d³ 4p¹
Which principle states no two electrons can have the same four quantum numbers?
Aufbau
Hund’s
Heisenberg
Pauli exclusion
According to Hund’s rule, electrons in degenerate orbitals:
Pair immediately
Occupy separate orbitals with parallel spins
Avoid p-orbitals
Maximize opposite spins
Which element has the electron configuration [Ne] 3s¹?
Mg
Na
Al
Ne
Atomic radius decreases across a period due to:
Increased shielding
Decreased nuclear charge
Increased effective nuclear charge
Higher principal quantum number
Which factor increases ionization energy?
Larger atomic radius
Greater shielding
Higher nuclear charge
Half-filled subshell instability
Why is the first IE of Be > B?
B has higher nuclear charge
Be has a stable s-subshell
B is larger
Be has more protons
Electronegativity is highest in which corner of the periodic table?
Lower-left
Upper-left
Lower-right
Upper-right
Which element has the lowest first ionization energy?
Li
Na
K
Rb
Metals have low ionization energy because:
They have high electronegativity
Their atoms are small
Valence electrons are shielded
They form anions easily
What type of bond forms when electronegativity difference is large?
Nonpolar covalent
Polar covalent
Ionic
Metallic
In MgO, ionic bonding is stronger than in NaCl because:
Mg²⁺ and O²⁻ have higher charges
MgO has covalent character
NaCl is molecular
MgO has larger ions
Hybridization in methane (CH₄) is:
sp
sp²
sp³
dsp³
What is the bond angle in sp² hybridization?
109.5°
120°
180°
90°
Hydrogen bonding requires H bonded to:
Any electronegative atom
Small, highly electronegative atom
Any atom in period 2
Only oxygen
Which has the highest boiling point due to H-bonding?
CH₄
HCl
HF
HBr
In VSEPR theory, molecular shape minimizes:
Nuclear repulsion
Electron pair repulsion
Bond length
Orbital overlap
What holds metal atoms together?
Ionic bonds
Covalent networks
Delocalized electrons
Dipole interactions
Which property explains metal malleability?
High melting point
Delocalized electrons
Atoms roll over without breaking bonds
Ionic lattice flexibility
Sublimation is:
Liquid → gas
Solid → liquid
Solid → gas
Gas → solid
