PSEB 10+1 SAMPLE PAPER SEPTEMBER EXAM 2024
paper Chemistry Time: 3 hrs. Class-10+1 M.M. 70
Section - (A)
Each question carries 1 mark. (28x1 = 28)
1. Multiple choice questions,
(1) How many quantum numbers are there?
- (a) Two
- (b) Three
- (c) Four
- (d) Five
(2) The Balmer series falls, in which region of light?
- (a) Visible
- (b) Ultra violet
- (c) Infra red
- (d) None
(3) The electronic configuration of Na atom is
- (a) 1s²2s²2p⁶ 3s²
- (b) 1s²2s²2p⁶3s¹
- (c)1s²2s²2p⁶
- (d) None of these
(4) Which quantum number predict the subshells?
- (a) n
- (b) l
- (c) m
- d) s
Which of the following is an example of in organic compounds?
- (a) Na₂CO₃,
- (b) NaCl
- (c) CaCo₃
- (d) All of these
(6) The number of significant figures in 6.0002 are
- (a) 3
- (b) 4
- (c) 5
- (d) 6
(7) Which of the following is heteroatomic molecule?
- (a) HCI
- (b) CO₂
- (c) CO₂
- (d) All of these
(8) Th example of non-metal is
- (a) C
- (b) Al
- (c) Na
- (d) None of these
(9) How many periods are there in modern's periodic table ?
- (a) 7
- (b) 8
- (c) 9
- (d) 10
(10) The general configuration of s-block elements is
- (a) ns²
- (b) ns¹⁻²
- (c) ns¹
- (d) None of these
(11) Which of the following is called alkali metal group?
- (a) Group I
- (b) Group II
- (c) Group III
- (d) Group IV
(12) Which of the following has largest ionisation energy?
- (a) Be
- (b) B
- (c) C
- (d) N
(13) Which of the following is lewis structure of Al?
(a) Al
(b) xAI
(c) x'AIX
(d) None of these
(14) Which quantum number determine the orbitals?
- (a) n
- (b) l
- (c) m
- (d) s
(15) Which of the following involved in the formation of 𝝅 bond.
- (a) s-s orbital
- (b) s-p orbital
- (c) p-p orbital
- (d) None of these
(16) The shapes of p-orbitals are
- (a) spherical
- (b) Dumbbell
- (c) Double dumb bell
- (d) None
(17) The combining capacity of an atom is called
- (a) Oxidation number
- (b) Valency
- (c) Valence electrons
- (d) None of these
18) The loss of electrons by an atoms is called
- (a) Oxidation
- (b) Reduction
- (c) Both of these
- (d) None of these
Read the passage and answer the following questions.
Halogens have highest negative electron gain enthalpies Group 17 elements (halogens) have the general electronic configuration ns²np⁵. They just need one electron to become stable. Cl has expectedly highest electron gain enthalpy, than F. Noble gases has positive electron gain enthalpy
- (19) Which group elements have highest negative electron gain enthalpy
- (20) Which group elements are called halogen family?
- (21) Which element has highest negative electron gain enthalpy?
- (22) Which group elements has positive electron gain enthalpy?
True/False
(23) Sand dissolved in water is an example of homogeneous mixture.
(24) 𝞹 bond is a strong bond.
(25) 𝞰 is called principle quantum number.
(26) Halogens have positive electron gain enthalpy.
(27) 3f Orbital is possible.
Section - (B) Two marks each.
2. Define compound.
3. Differentiate homoatomic and heteroatomic molecule. OR
Calculate the mass of one molecule of O₂
4. Define Aufbau's rule.
5. Copper and Chromium has exceptional configuration, why? OR
Calculate the energy of a photon of light having frequency of 3.0 x 10¹⁵s⁻¹ (Planks constant = 6.63 x 10⁻³⁴ JS)
6. Define electronegativity. OR
Which of the following are isoelectronic? F⁻, Na⁺, Mg²⁺, N³⁺, Ne, Al
7. Nobel gases has positive or zero electron gain enthalpy why?
8. Why is octet rule?
9. Define heisenberg's uncertainty principle.
10. Write the empirical formulae of the following (a) Na₂CO₃, (b) H₂S₂O₈,
11. Calculate the value of l and m for n = 4.
Section - (C) Three marks questions
12. Differentiate between orbit and orbital.
OR
Differentiate between s and p bond.
13. State and explain the law of multiple proportion.
OR
A compound contain 4.07% hydrogen, 24.27% carbon and 71.65% Chlorine. Its molecular mass is 98.96. What are the empirical and molecular formulae?
14. Differentiate between oxidation number and valency.
15. Explain oxidation and reduction according to electonic concept, giving examples. (3x4=12)
Section - (D) Five marks each
16. (1) Draw the energy level diagram of N₂, molecule and also calculate the bond order
(2) Define coordinate bond.
OR
(1) Explain the hybridisation and geometry of SF₆, molecule
(2) Draw the lewis dot symbol of Oxygen and Neon atoms.
17. (1) Write the main points of Dalton's atomic theory.
(2) Define matter.
OR
(1) The size of cation is smaller than parent atom but that of anion is larger than parent atom explain.
(2) Define mole. (5x2=10)
