Q1: What do you know about atoms?
Q2: What do you know about Dalton atomic theory? OR
Write down the main postulates of Dalton's Atomic Theory. OR
Why Dalton's atomic theory is considered as a base for modern atomic concepts.
Q3: Give an account of the experiment that led Rutherford to conclude that every atom has a positively charged nucleus that occupies a very small volume. What were the drawbacks of Rutherford's nuclear model of the atom? (Cantab Exercise Question) OR
Summarize Rutherford's model of an atom and explain how he developed this model based on the results of his famous gold-foil experiment. OR
Discuss Rutherford gold metal foil experiment in the light of structure of atom OR
Can you describe the experiment and result deduced by Rutherford for explaining atomic structure? OR
Describe the contribution that Rutherford made to the development of the atomic theory. OR
How Rutherford discovered that atom has a nucleus located at the centre of the atom?
Q4: State the postulates of Bohr's theory of the hydrogen atom. Write an expression for the nth orbit of a hydrogen atom. Also, write an expression for the radius of any orbit in the atom? Cantab Exercise Question) OR
State the postulates which Bohr suggested to overcome the shortcomings of the Rutherford's atomic model. OR
Explain how Bohr's atomic theory differed from Rutherford's atomic theory? OR
How did Bohr proved that an atom must exist? OR
Explain how Bohr helped in understanding the structure of atoms? OR
Explain how Bohr's atomic model is different from Rutherford atomic model?
Q5: How can Bohr's atomic model be applied to hydrogen atom to calculate the radius and energy of shell?
Q6: How staircase is the example of orbits or energy levels
Q7: How Quantum Mechanical Model explains the structure of an atom?
Q8: State Heisenberg Uncertainty principle.
Q9: Explore the concept of modern Quantum mechanics including the contribution of Louis de Broglie and Davission and Germer?
Q10: Explore the concept of nuclear force including binding of proton, neutron and nucleus?
Q11: What are the limitations of Bohr's atomic model?
Q12: Write down the fundamental properties of the fundamental particles of an atom? OR
Write fundamental properties of electron, proton and neutron? OR
Elaborate the concept of subatomic particles by showing their mutual relationship?
Q13: Illustrate the behavior of protons, neutrons, and electrons in an electric field?
Q14: Why atoms are neutral?
Q15: What are Radioisotopes?
Q16: Discuss atomic number or proton number in detail?
Q17: Discuss uniqueness of proton number.
Q18: Discuss nucleon number or mass number in detail.
Determining the number of protons and neutrons in an atom
Atomic Number of an element is 17 and mass number is 35. How many protons and neutrons are in the nucleus of an atom of this element?
(1) What is the charge of a particle with 19 protons and 18 electrons?
(ii) What is the charge of a particle with 7 protons and 10 electrons?
(iii) What is the difference between the mass number and the atomic mass of an element?
Write the names and symbols for the elements with the following atomic numbers:
a. 1
b. 11
c. 19
d. 82
e. 35
f. 47
g. 15
h. 2
Determining the number of protons and neutrons in an atom Atomic Number of an element is 17 and mass number is 35. How many protons and neutrons are in the nucleus of an atom of this element?
(1) What is the charge of a particle with 19 protons and 18 electrons?
(ii) What is the charge of a particle with 7 protons and 10 electrons?
(iii) What is the difference between the mass number and the atomic mass of an element?
Write the names and symbols for the elements with the following atomic numbers: a. 1 b. 11 c. 19 d. 82 e. 35 f. 47 g. 15 h. 2
Q19: Discuss the 'concept of relative atomic mass and atomic mass unit. Also discuss relative atomic masses of some elements.
Q20: Define isotopes. Discuss isotopes of Hydrogen, Carbon, Chlorine, and Uranium?
Q21: How does the discovery of isotopes contradicted Dalton's atomic theory?
Q22: Give comparison of ordinary water and heavy water.
Uranium has three isotopes with mass number 234, 235 and 238 respectively. U. 12 ^ 29 U 1 12 ^ 290 U The U isotope is used in nuclear reactors and atomic bombs, whereas the 92 ^ 238 U isotope lacks the properties necessary for these applications. U is rare. Natural abundance of Uranium isotopes is as follows. 92 ^ 214 U = 0.009% , 92 ^ 235 U = 0.72% , 92 ^ 235 U = 99.27% Fill in the blanks? 134 U has 92 215U has 92 protons, protons, electrons and electrons and neutrons neutrons
Q23: Calculate the relative atomic mass of carbon. The relative atomic mass of an element can be calculated from the relative masses of its isotopes and their relative abundance. Natural abundance of isotopes of carbon is as follows: 6 ^ 12 C = 98.8% 6 ^ 13 C = 1.1% 6 ^ 14 C = 0.009% Calculate relative atomic mass of carbon.
Q24: Explain different uses of isotopes.
Q25: Why do the chemical properties of isotopes of same element remains the same?
(1) Zinc consists of five naturally occurring isotopes: Zn, Zn, Zn, and Zn. None of these isotopes has the atomic mass of 65.41 listed for zinc on the periodic table. Explain.
(ii) Two isotopes of gallium are naturally occurring, with Gaat 60.11% (68.93 amu) and Ga at 39.89% (70.92 amu). Calculate the atomic mass for gallium using the weighted average mass method.
(iii) Two isotopes of rubidium occur naturally, with Rbat 27.83% (84.91 amu) and Rb at 27.83% (86.91 amu). Calculate the atomic mass for rubidium using the weighted average mass method.
Why do we find average atomic mass of an element?
Q: Calculate average mass of Cl use data given below:
CI
35.45-
-17 Protons
Symbol for chlorine -Atomic mass 35.45 amu
CI
CI
75.76%
24.24%
Isotope
C1-35
C1-37
Mass number
35
37
Relative abundance
75.76%
24.24%
Q26: Describe the process by which positive (cation) and negative (anions) are formed from atoms, including the role of electrons in this transformation?
Describe the formation of N x^ + and M * g ^ 2 cations.
(a) Formation of N a^ + ion:
(b) Formation of M * g ^ 2 ion:
Describe the formation of cations for the following metal atoms
(a) Li (atomic no 3)
(b) Al (atomic no 13)
Describe the formation of anions for the following non-metal atoms..
(a) oxygen (atomic no.8)
(b) Fluorine (atomic no 9)
Q27: Discuss Electronic Configuration.
Q28: How can we assign symbols for atoms and ions?
Q29: Write a note on radioactivity and how the identity of an element chan,, by radioactivity? (Cantab Exercise Question)
Q30: What is Carbon dating? OR
Explain how, through carbon dating scientists determine the age of ancient artifacts or human remains? Q31: Write a note on how radio isotopes use in medical imaging technology along applications of different isotopes?
Q32: Discuss some differences between chemical reaction and nuclear reactions?