Second Term Revision Chemistry SS 1 Second Term Lesson Notes

SECOND TERM EXAMINATION

Subject: Chemistry Class: SS1 Time:2hrs

Section A: Objective

Instruction: Answer all question in this section.

1. Which of the three state of matter has no fixed shape, no fixed volume and least dense (a) Gas (b) Liquid (c) Solid (d) Crystal
2. Covalent compounds usually dissolved in non-polar ­­­­­­­­­­­­­­­­­_________ (a) Solution (b) Solvent (c) Substance (d) Conductor
3. Diatomic molecules of elements are formed by covalent ___________ (a) Combination (b) covalency (c) Electrovalency (d) Parings
4. The K shell can hold maximum number of ___________ (a) 18 electrons (b) 2 electrons (c) 32 electrons (d) 50 electrons
5. _____________ compound readily dissolves in water. (a) Covalent compound (b) Hydrogen compound (c) Co-hensive compound (d) Ionic compound
6. ____________ are liquids which conducts electricity (a) Electrolytes (b) Electrons (c) Crystal (d) Non- electrolytes
7. In Mg Mg²⁺ + 2e^– connotes that Mg _________ (a) Gains two electron (b) Donates two electron (c) Removes on two electrons (d) None of the above
8. Water has _______ lone pairs in covalent molecules. (a) 2 (b) 1 (c) 3 (d) 4
9. Convert 840mmHg to Nm^-2 (a) 1.03 x 10⁵ Nm^-2 (b) 1.13 x 10⁵ Nm^-2 (c) 13.1 x 10⁵ Nm^-2 (d) 1.11 x 10⁵ Nm^-2
10. Which of the following explains the physical behavior of gas. (a) Boyle’s law (b) Charle’s law (c) Kinetic theory of gases (d) Avogardo’s law
11. _________ collides with the container’s wall when confined (a) Solid particles (b) Gas particles (c) Liquid particles (d) None of the above
12. In vapour pressure, Liquid particles Vapour particles the K in the arrow stands for (a) Condense (b) Everporate (c) Evaporation (d) Saturated vapour pressure
13. One of the following or more are true according to boyle’s law
14. Pressure increase as volume increase
15. Pressure increase as volume decrease
16. Pressure increase volume decreases and vice versa
17. Temperature decreases as volume increases
18. Iii and I (b) iii only (c) ii and iv (d) I and ii
19. __________ is a substance which produce hydrogen ion as the only positive ion when dissolved in water (a) Salts (b) Covalent Ion (c) Strong acid (d) Base (e) Acid
20. A certain amount of gas occupies 5.0dm³ at 2atm and 10^oC. Calculate the number of moles present. (R=0.082 atmdm³ mol^-1 k^-1) (a) 0.222 moles (b) 0.4309 moles (c) 1.435 moles (d) 8.0324 moles
21. In the below equation X stands for ­­­­­­­_________ XH₂O_(g) + O_2(g) 2H₂O (a) -2 (b) 4 (c) 6 (d) 2
22. Q is an element with the electronic configuration of 1s²2s²2p⁶3s²3p⁵. (a) Ca (b) Li (c) O (d) Cl
23. The four types of orbital in sub levels of shells and they are (a) spdf (b) KLMNO (c) P_x P_y P_z p_a (d) None of the above
24. _____________ shows direction of an electron and it denoted by sharing the range of value of + or – (a) spin quantum number (b) Magnetic quantum number (c) Principal quantum number (d) Energy level
25. Melting of ice to become a substance in liquid state is a _______ (a) Chemical change (b) Metallic change (c) Physical Change (d) All of the above
26. All of the following elements ionize by electron gain except (a) Oxygen (b) Chlorine (c) Nitrogen (d) Calcium
27. The weakest attractive forces that can be observed between two molecule is (a) Ionic (b) Covalent (c) Van der waals (d) Coordinate covalent
28. In H-Cl, the dash (-) is (a) Single bond (b) Double bond (c) Boyle’s bond (d) None of the above
29. After combinations _________ are formed (a) Ion (b) Ions (c) electrons (d) Cataions

The diagram above represents the formation of a (a) Metallic Bond (b) Covalent bond (c) An electrovalent bond (d) Co-ordinate covalent bond

1. According to Kinetic theory,an increase in temperature cause the kinetic energy of particles to (a) Decrease (b) Increases (c) Be zero (d) Remain constant
2. Graham’s law of diffusion is expressed mathematically as (a) Rate varies density (b) Rate varies 1/density (c) Rate varies 1/√(density)² (d) Rate varies (density)²
3. In general gas equation T2 can be calculated by
4. T1 T2 P1/V2 P2
5. P2 V2 T1/P1 V1
6. P2 V2 T1/P1 V1
7. P1 V1 T1/P2 V2
8. Ii only (b) I and ii (c) iii only (d) iii and ii
9. A gas has it’s moles to be 1.5mol at a temperature of -15^oC. What is it’s temperature in Kelvin? (a) 299K (b) 305K (c) 258K (d) 250K

-273 0 Temperature

The above graph is a graphical illustration of

1. Graham’s law of diffusion (b) Boyle’s law (c) Charle’s law (d) Gay Lussac’s law

Section B

Instruction : Answer 3 questions in this section. All working must be clearly shown where it is required (NOTE: Question 2 is compulsory)

1a. State the following laws with their mathematical expressions and graphical illustrations

1. Boyle’s law
2. Charle’s law
3. Graham’s law of diffusion

1b. Explain Hydrogen bonding using water molecule (2H2O) as a case of study.

2a. what is (i) an acid (ii) a base

2b. Define Valency with vivid examples.

2c. Given the table below table, Use the table to answer (I – iv)

Formation of XY

1. X represent what? and Y represents what?
2. The bond that takes place between X and Y is a __________ bond?
3. Copy and complete the table (2 Marks)
4. Write out the equation of the reaction.

3a. List and explain 5 types of chemical bonding with at least one example.

3b.Highlight four properties of ionic (Electrovalent) bond.

3c. what is the volume at S.T.P of a fixed mass of gas that occupies 700cm³ at 25^o and 0.84 X 10⁵Nm^-2 pressure?

4a. A sample of gas has a volume of 500mcm³ at 45⁰ C. What volume will the gas occupy at 4⁰ C when the pressure remains constant?

4b. Explain the three states of matter with Vivid examples.

4c. state the following (I) Hund’s rule (ii) Aufbau principle

5a. Write out the electronic configuration of the first Twenty element (In tabular Form).

5b. Define (i) water of crystallization (ii) Deliquescence.