Class 7 Exam > Class 7 Notes > Chemistry Class 7 ICSE > Worksheet: Atoms Structure
Worksheet: Atoms Structure | Chemistry Class 7 ICSE PDF Download
Section A: Multiple Choice Questions
Q1. Which scientist gave the first scientific theory about atoms?
a) J.J. Thomson
b) John Dalton
c) Niels Bohr
d) Rutherford
Q2. Which particle has no charge?
a) Proton
b) Neutron
c) Electron
d) Positron
Q3. According to Thomson’s model, the atom looks like:
a) A solar system
b) A solid sphere
c) A sphere with positive charge in which electrons are embedded
d) A dense nucleus surrounded by electrons
Q4. Rutherford’s gold foil experiment proved that:
a) Atoms are solid
b) Most of an atom is empty space
c) Electrons are stationary
d) Neutrons are present in the nucleus
Q5. Two atoms having the same atomic number but different mass numbers are called:
a) Isotopes
b) Isobars
c) Ions
d) Molecules
Section B: Short Answer Questions
Q6. State two postulates of Dalton’s Atomic Theory.
Q7. Differentiate between atomic number and mass number.
Q8. Define an electron. Where is it located in an atom?
Q9. Name the three subatomic particles of an atom and state their charges.
Q10. Explain Rutherford’s gold foil experiment and its conclusions.
Section C: Long Answer Questions
Q11. Describe Bohr’s model of the atom.
Q12. What are isobars? Give one example.
Q13. Write three differences between isotopes and isobars.
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FAQs on Worksheet: Atoms Structure - Chemistry Class 7 ICSE
| 1. What is the basic structure of an atom? |  |
Ans. An atom consists of three main subatomic particles: protons, neutrons, and electrons. Protons are positively charged and found in the nucleus at the center of the atom. Neutrons have no charge and also reside in the nucleus. Electrons are negatively charged and orbit the nucleus in various energy levels or shells.
| 2. Who proposed the atomic theory and what are its main points? | |
Ans. John Dalton proposed the atomic theory in the early 19th century. The main points of this theory include: 1) All matter is made up of tiny, indivisible particles called atoms. 2) Atoms of the same element are identical in mass and properties. 3) Atoms combine in simple whole-number ratios to form compounds. 4) Chemical reactions involve the rearrangement of atoms.
| 3. How do the properties of elements depend on the structure of their atoms? | |
Ans. The properties of elements depend on the number and arrangement of their electrons, which determine how atoms interact and bond with each other. For example, elements with a full outer electron shell are generally inert and unreactive (like noble gases), while those with nearly full or empty shells are more reactive (like alkali metals and halogens).
| 4. What is the significance of the atomic number and mass number in an atom? | |
Ans. The atomic number of an atom is the number of protons in its nucleus, which determines the element's identity and its position in the periodic table. The mass number is the total number of protons and neutrons in the nucleus, which gives an approximate mass of the atom. These two numbers are crucial for understanding the atom's behavior and its isotopes.
| 5. Can you explain what isotopes are and give an example? | |
Ans. Isotopes are variants of the same element that have the same number of protons but different numbers of neutrons, resulting in different mass numbers. For example, Carbon has two stable isotopes: ¹²C, which has 6 protons and 6 neutrons, and ¹³C, which has 6 protons and 7 neutrons. Isotopes can have different physical properties and can be used in various applications, such as dating fossils.
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