Exam1st

Structure of Matter Grade 10 Science lesson 03 Quiz 01

O/LScienceStructure of MatterEnglishEasy20 questions

Free G.C.E. O/L Science MCQ quiz on Structure of Matter with 20 questions in English medium. Answer each question, see the correct answer and explanation straight away, and get your score at the end. Use the study section below to review every question and answer.

සාමාන්‍ය පෙළ Science බහුවරණ ප්‍රශ්න නොමිලේ පුහුණු වන්න.

Loading...

About this quiz

Master Structure of Matter: Free Online Quiz 01 & MCQ Revision for Grade 10 Science (Lesson 03)Test and build your chemistry foundation with this free online practice test on Structure of Matter (Quiz 01), designed specifically for Grade 10 Science Unit 03. Whether you are revising for unit tests, term exams, or national syllabus assessments, this quiz breaks down foundational atomic concepts into clear, exam-standard multiple-choice questions (MCQs).Understanding the atomic framework is essential for excelling in chemical bonding, periodic trends, and chemical reactions. This first quiz in the series focuses on core atomic theories, subatomic particles, atomic notation, and electronic configurations.Key Topics Covered in Quiz 01:Evolution of the Atomic Model: Key contributions from Dalton, J.J. Thomson, Rutherford, Niels Bohr, and the modern atomic view.Subatomic Particles: Relative masses, electrical charges, and locations of protons, neutrons, and electrons within the atom.Atomic Number (Z) & Mass Number (A): Determining the number of nucleons and subatomic constituents using standard isotopic symbols (AZX).Isotopes: Defining isotopes, understanding isotopic properties, and identifying common isotopic examples (Hydrogen, Carbon, Chlorine).Electronic Configuration: Writing energy level arrangements (first 20 elements, 2, 8, 8, 2 rule) and identifying valence electrons.Key Features & Benefits:Instant Scoring & Correct Answers: Receive immediate results with detailed breakdowns to identify weak spots instantly.Curriculum-Aligned Quality: Built in alignment with Grade 10 secondary school science curricula to match authentic exam question styles.Speed & Recall Training: Enhance your speed in calculating neutron counts and determining valence electrons under timed conditions.100% Free & Mobile-Friendly: Seamlessly practice on smartphones, tablets, or computers with zero login hurdles.Who Is This Quiz For?Grade 10 students preparing for chemistry unit tests, mid-terms, and term evaluations.High school candidates reviewing basic atomic structure before tackling advanced chemical bonding.Science educators seeking a quick formative assessment or homework practice link for their students.

All questions & answers (20)

Study mode: read every question, then open the answer. Tap to show.

  1. Q1. Which subatomic particle carries a negative electrical charge?

    • A)Proton
    • B)Neutron
    • C)Electron
    • D)Positron
    Show answer & explanation

    Answer: C) Electron

    Electrons are negatively charged subatomic particles that revolve around the nucleus[cite: 53, 54].

  2. Q2. Who proposed the planetary model of the atom in 1911?

    • A)Niels Bohr
    • B)Ernest Rutherford
    • C)Dmitri Mendeleeff
    • D)Linus Pauling
    Show answer & explanation

    Answer: B) Ernest Rutherford

    Ernest Rutherford put forward the nuclear/planetary model of the atom in 1911[cite: 53, 54].

  3. Q3. What is the maximum number of electrons that can be accommodated in the third (M) energy level?

    • A)2
    • B)8
    • C)18
    • D)32
    Show answer & explanation

    Answer: C) 18

    According to electron capacity rules, the K, L, M, and N levels hold a maximum of 2, 8, 18, and 32 electrons respectively[cite: 54].

  4. Q4. The atomic number of an element is equal to the number of which particle in its atom?

    • A)Neutrons
    • B)Protons
    • C)Nucleons
    • D)Valence electrons
    Show answer & explanation

    Answer: B) Protons

    The atomic number (symbolized by Z) is defined as the number of protons in an atom of the element[cite: 55].

  5. Q5. What symbol signifies the mass number of an element?

    • A)Z
    • B)A
    • C)N
    • D)E
    Show answer & explanation

    Answer: B) A

    The mass number, representing the sum of protons and neutrons, is symbolized by A[cite: 56].

  6. Q6. What is the electronic configuration of a sodium atom (atomic number 11)?

    • A)2, 8, 1
    • B)2, 8, 2
    • C)2, 7, 2
    • D)8, 2, 1
    Show answer & explanation

    Answer: A) 2, 8, 1

    Sodium has 11 electrons distributed across its shells as 2 in K, 8 in L, and 1 in M[cite: 56, 57].

  7. Q7. Who introduced the first periodic table for classifying elements?

    • A)Ernest Rutherford
    • B)Niels Bohr
    • C)Dmitri Mendeleeff
    • D)Linus Pauling
    Show answer & explanation

    Answer: C) Dmitri Mendeleeff

    A periodic table for classifying elements was first introduced by the Russian scientist Dmitri Mendeleeff[cite: 58].

  8. Q8. In the modern Periodic Table, horizontal rows are called:

    • A)Groups
    • B)Periods
    • C)Shells
    • D)Lattices
    Show answer & explanation

    Answer: B) Periods

    Horizontal rows in the periodic table are known as periods, while vertical columns are groups[cite: 58].

  9. Q9. The period to which an element belongs is determined by:

    • A)The number of valence electrons
    • B)The number of energy levels carrying electrons
    • C)The number of neutrons
    • D)Its isotopic abundance
    Show answer & explanation

    Answer: B) The number of energy levels carrying electrons

    The period number corresponds directly to the number of energy levels (shells) that carry electrons in that atom[cite: 59].

  10. Q10. Which element has the highest electronegativity according to the Pauling scale?

    • A)Oxygen
    • B)Chlorine
    • C)Fluorine
    • D)Nitrogen
    Show answer & explanation

    Answer: C) Fluorine

    Fluorine is assigned the highest electronegativity value (4.0) on the Pauling scale[cite: 64, 65].

  11. Q11. What is the minimum energy required to remove an electron from a gaseous atom to form a unipositive ion called?

    • A)Electronegativity
    • B)First ionisation energy
    • C)Bond energy
    • D)Lattice energy
    Show answer & explanation

    Answer: B) First ionisation energy

    First ionisation energy is the minimum energy needed to remove an electron from a gaseous atom[cite: 63, 64].

  12. Q12. Across a Period from left to right in the Periodic Table, the first ionisation energy generally:

    • A)Decreases
    • B)Increases
    • C)Remains constant
    • D)Drops to zero
    Show answer & explanation

    Answer: B) Increases

    As you move from left to right across a period, the first ionisation energy increases in a regular manner[cite: 63, 64].

  13. Q13. Down a Group in the Periodic Table, the first ionisation energy:

    • A)Increases
    • B)Decreases
    • C)Remains completely unchanged
    • D)Fluctuates randomly
    Show answer & explanation

    Answer: B) Decreases

    Descending a group, ionisation energy decreases because outer electrons are further from the nucleus and shielded[cite: 64, 65].

  14. Q14. Atoms of the same element that have the same atomic number but different mass numbers are called:

    • A)Allotropes
    • B)Isomers
    • C)Isotopes
    • D)Isobars
    Show answer & explanation

    Answer: C) Isotopes

    Isotopes are atoms of the same element with differing numbers of neutrons, resulting in different mass numbers[cite: 61, 62].

  15. Q15. How many isotopes does hydrogen have?

    • A)One
    • B)Two
    • C)Three
    • D)Four
    Show answer & explanation

    Answer: C) Three

    Hydrogen has three isotopes named protium, deuterium, and tritium[cite: 61, 62].

  16. Q16. In natural chlorine gas, what is the percentage abundance of the isotope chlorine-3517Cl?

    • A)25%
    • B)50%
    • C)75%
    • D)100%
    Show answer & explanation

    Answer: C) 75%

    Chlorine gas consists of 75 parts chlorine-35 and 25 parts chlorine-37 out of a hundred[cite: 62].

  17. Q17. Which of the following elements is classified as a metalloid?

    • A)Sodium
    • B)Silicon
    • C)Sulphur
    • D)Chlorine
    Show answer & explanation

    Answer: B) Silicon

    Silicon is located near the dividing line/steps and is classified as a metalloid[cite: 65, 66, 72].

  18. Q18. How are sodium and potassium metals stored in the laboratory to prevent contact with air?

    • A)In distilled water
    • B)In paraffin oil or kerosene
    • C)In concentrated acids
    • D)In sealed glass vacuum tubes
    Show answer & explanation

    Answer: B) In paraffin oil or kerosene

    Highly reactive alkali metals like sodium are stored under paraffin oil or kerosene[cite: 67, 68].

  19. Q19. What color flame does magnesium burn with when heated in air?

    • A)Blue flame
    • B)Bright white flame
    • C)Green flame
    • D)Yellow glow
    Show answer & explanation

    Answer: B) Bright white flame

    Magnesium burns vigorously in air with a bright white flame, forming magnesium oxide[cite: 68].

  20. Q20. What is the approximate percentage by volume of nitrogen gas in the atmosphere?

    • A)21%
    • B)50%
    • C)78.1%
    • D)99%
    Show answer & explanation

    Answer: C) 78.1%

    Nitrogen exists as a free diatomic gas making up about 78.1% by volume of the atmosphere[cite: 69].

Practise with real G.C.E. O/L Science past papers

All G.C.E. O/L Science past papers →

More Science quizzes

All G.C.E. O/L Science quizzes →