Q1
How does Dalton’s atomic theory explain the law of conservation of mass?
Since it states that atoms cannot be created or destroyed, Dalton’s theory suggests that the net mass of the participating species in a chemical reaction is conserved. This postulate, therefore, accounts for the law of conservation of mass.
Q2
How does Dalton’s atomic theory differentiate between elements and compounds?
This theory states that elements combine in fixed, whole-number ratios to form compounds. Therefore, it suggests that compounds are made up of molecules that contain two or more atoms of different elements.
Q3
What are the 5 key postulates of Dalton’s atomic theory?
The 5 postulates of Dalton’s atomic theory are listed below.
- All matter is made up of atoms, which are tiny, indivisible particles.
- All the atoms of an element have the same size, mass, and properties but the atoms of different elements have different sizes and masses.
- Atoms cannot be created, destroyed, or divided into smaller particles.
- Compounds are formed when the atoms of different elements combine with each other in fixed, whole-number ratios.
- Atoms can be combined, separated, or rearranged via chemical reactions.
Q4
List two merits of Dalton’s atomic theory.
One of the most important merits of Dalton’s atomic theory is the fact that the theory does not violate several fundamental laws of chemical combination such as the law of definite proportions, the law of multiple proportions, and the law of conservation of mass. Another important merit of Dalton’s atomic theory is that it provided a basis for scientists to differentiate between elements and compounds.
Q5
What are the shortcomings of Dalton’s atomic theory?
Some important demerits of Dalton’s atomic theory are listed below.
- The theory did not account for the existence of subatomic particles (it suggested that atoms are indivisible).
- By suggesting that all atoms of an element must have identical masses and sizes, Dalton’s atomic theory did not account for the existence of isotopes. Furthermore, this theory also did not account for the existence of isobars (nuclides of different chemical elements with the same mass number).
- Dalton’s atomic theory failed to explain the dissimilarities in the properties of different allotropes of an element.
- This theory states that elements must combine in simple, whole-number ratios to form compounds. However, this is not necessarily true. Several complex organic compounds do not feature simple ratios of their constituent elements.
Q6
Do electrons actually exist?
Most of us realize that the neutron, in an atom of matter, is a negatively charged particle orbiting the nucleus. No two electrons at the same time will occupy the same space. They are part of any molecule, but they may also live on their own, independently.
Q7
Which atomic model is used today?
The Bohr paradigm, generally speaking, encapsulates the popular understanding of the atom. In artwork that depicts a central atomic nucleus and oval lines reflecting the electron orbits, this image is also portrayed.
Q8
Why can’t you see an atom with the naked eye?
We can not see an atom with naked eyes because an atom is extremely small and is not perceptible.
Q9
Can atoms be divided or destroyed?
No, atoms can not be divided or destroyed. However, it can combine with other atoms to form compounds. In a chemical reaction, an atom can combine, separate and rearrange.
Q10
What are atoms made of?
Atoms are made up of negative charged electrons, positively charged protons and neutral neutrons.
