UNE - CHEM 1011 - MIDTERM – ACTUAL EXAM PRACTICE
QUESTIONS AND 100% VERIFIED CORRECT ANSWERS | COMPLETE
EXAM PREP TESTBANK | GUARANTEED PASS | INSTANT
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CORE DOMAINS
1. Atomic Structure and Periodic Trends
2. Chemical Bonding and Molecular Geometry
3. Stoichiometry and Chemical Reactions
4. Thermochemistry and Energy Changes
5. Gases and Gas Laws
6. Solutions and Concentration Calculations
7. Chemical Equilibrium
8. Acids, Bases, and pH
9. Laboratory Safety and Measurement
10.Scientific Ethics and Professional Conduct
TABLE OF CONTENTS
1. Introduction ........................................ Page 1
2. Atomic Structure and Periodic Trends ............... Page 2
3. Chemical Bonding and Molecular Geometry ............ Page 4
4. Stoichiometry and Chemical Reactions ............... Page 6
5. Thermochemistry and Energy Changes ................. Page 8
6. Gases and Gas Laws ................................. Page 10
7. Solutions and Concentration Calculations .......... Page 12
8. Chemical Equilibrium .............................. Page 14
9. Acids, Bases, and pH .............................. Page 16
10.Laboratory Safety and Measurement ................ Page 18
11.Scientific Ethics and Professional Conduct ....... Page 19
12.Answer Key Summary ............................... Page 20
,INTRODUCTION
This assessment is designed to evaluate student understanding of core principles in
introductory general chemistry. The exam measures knowledge of atomic theory,
chemical reactions, thermodynamics, gases, solutions, equilibrium systems, and
acid–base chemistry. Questions are presented in a multiple-choice format and
include conceptual problems, quantitative calculations, and real-world laboratory
scenarios. The assessment emphasizes scientific reasoning, proper experimental
practices, regulatory laboratory safety standards, and ethical decision-making in
scientific environments. Students must demonstrate the ability to interpret
chemical data, apply theoretical concepts to practical situations, and make sound
scientific judgments consistent with professional laboratory expectations.
SECTION 1
QUESTIONS 1–35
1. Which particle determines the identity of an element?
A. Neutron
B. Electron
🔴 C. Proton
D. Nucleus
🔵 Explanation: The number of protons (atomic number) uniquely defines an
element.
2. Which unit is commonly used to express atomic mass?
,A. Joule
B. Pascal
🔴 C. Atomic mass unit (amu)
D. Kelvin
🔵 Explanation: Atomic masses are expressed in atomic mass units, defined relative
to carbon-12.
3. Which scientist proposed the nuclear model of the atom?
A. Dalton
🔴 B. Rutherford
C. Thomson
D. Bohr
🔵 Explanation: Rutherford's gold foil experiment demonstrated a dense positively
charged nucleus.
4. Which orbital can hold a maximum of two electrons?
A. s orbital
B. p orbital
C. d orbital
D. All orbitals
🔴 D. All orbitals
, 🔵 Explanation: Every atomic orbital can hold a maximum of two electrons with
opposite spins.
5. What is the charge of an electron?
A. +1
B. +2
C. 0
🔴 D. −1
🔵 Explanation: Electrons carry a negative charge with a relative value of −1.
6. Which periodic trend generally increases from left to right across a period?
A. Atomic radius
🔴 B. Electronegativity
C. Shielding effect
D. Ionic size
🔵 Explanation: Electronegativity increases across a period due to stronger nuclear
attraction.
7. Which type of bond involves the sharing of electrons?
QUESTIONS AND 100% VERIFIED CORRECT ANSWERS | COMPLETE
EXAM PREP TESTBANK | GUARANTEED PASS | INSTANT
DOWNLOAD PDF
CORE DOMAINS
1. Atomic Structure and Periodic Trends
2. Chemical Bonding and Molecular Geometry
3. Stoichiometry and Chemical Reactions
4. Thermochemistry and Energy Changes
5. Gases and Gas Laws
6. Solutions and Concentration Calculations
7. Chemical Equilibrium
8. Acids, Bases, and pH
9. Laboratory Safety and Measurement
10.Scientific Ethics and Professional Conduct
TABLE OF CONTENTS
1. Introduction ........................................ Page 1
2. Atomic Structure and Periodic Trends ............... Page 2
3. Chemical Bonding and Molecular Geometry ............ Page 4
4. Stoichiometry and Chemical Reactions ............... Page 6
5. Thermochemistry and Energy Changes ................. Page 8
6. Gases and Gas Laws ................................. Page 10
7. Solutions and Concentration Calculations .......... Page 12
8. Chemical Equilibrium .............................. Page 14
9. Acids, Bases, and pH .............................. Page 16
10.Laboratory Safety and Measurement ................ Page 18
11.Scientific Ethics and Professional Conduct ....... Page 19
12.Answer Key Summary ............................... Page 20
,INTRODUCTION
This assessment is designed to evaluate student understanding of core principles in
introductory general chemistry. The exam measures knowledge of atomic theory,
chemical reactions, thermodynamics, gases, solutions, equilibrium systems, and
acid–base chemistry. Questions are presented in a multiple-choice format and
include conceptual problems, quantitative calculations, and real-world laboratory
scenarios. The assessment emphasizes scientific reasoning, proper experimental
practices, regulatory laboratory safety standards, and ethical decision-making in
scientific environments. Students must demonstrate the ability to interpret
chemical data, apply theoretical concepts to practical situations, and make sound
scientific judgments consistent with professional laboratory expectations.
SECTION 1
QUESTIONS 1–35
1. Which particle determines the identity of an element?
A. Neutron
B. Electron
🔴 C. Proton
D. Nucleus
🔵 Explanation: The number of protons (atomic number) uniquely defines an
element.
2. Which unit is commonly used to express atomic mass?
,A. Joule
B. Pascal
🔴 C. Atomic mass unit (amu)
D. Kelvin
🔵 Explanation: Atomic masses are expressed in atomic mass units, defined relative
to carbon-12.
3. Which scientist proposed the nuclear model of the atom?
A. Dalton
🔴 B. Rutherford
C. Thomson
D. Bohr
🔵 Explanation: Rutherford's gold foil experiment demonstrated a dense positively
charged nucleus.
4. Which orbital can hold a maximum of two electrons?
A. s orbital
B. p orbital
C. d orbital
D. All orbitals
🔴 D. All orbitals
, 🔵 Explanation: Every atomic orbital can hold a maximum of two electrons with
opposite spins.
5. What is the charge of an electron?
A. +1
B. +2
C. 0
🔴 D. −1
🔵 Explanation: Electrons carry a negative charge with a relative value of −1.
6. Which periodic trend generally increases from left to right across a period?
A. Atomic radius
🔴 B. Electronegativity
C. Shielding effect
D. Ionic size
🔵 Explanation: Electronegativity increases across a period due to stronger nuclear
attraction.
7. Which type of bond involves the sharing of electrons?
