Chemistry Practice Questions First Term Mid Term Test SSS 1 TO SSS 3

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Subuode Igbaga

FISRT TERM EXAMINATION

2019/2020 ACADEMIC SESSION

SUBJECT: CHEMISTRY CLASS: S.S.S 1

INSTRUCTION: ANSWER ALL QUESTIONS IN THIS SECTION

1. Chemistry is defined as ________________ (a) a branch of knowledge which produces chemicals (b) a branch of science which makes physics and biology clearer (c) the oldest branch science (d) the branch of science which deals with change in matters
2. The symbol for element potassium is ________ (a) k (b) p (c) pt (d) Cr
3. One of these profession has no need for chemistry (a) miner (b) engineer (c) philosophers (d) geologist
4. ________ is an example of gaseous elements (a) calcium (b) neon (c) potassium (d) zinc
5. The atomicity of ozone is (a) 1 (b) 2 (c) 3 (d) 4
6. Atom is ________ (a) the smallest part of a substance that can take part in a chemical change (b) the smallest part of an element which can take part in a chemical change (c) the smallest part of a compound which can take part in chemical change (d) the smallest part of a lattice which can take part in a chemical change
7. The only liquid metal on earth is ________ (a) sodium (b) carbon (c) mercury (d) gold
8. ________ can be used to pick hot objects from flame source (a) hot taker (b) test tube (c) beaker (d) thong
9. ________ can be used to dry anhydrals substance to obtain crystals (a) burette (b) reagent bottle (c) desicator (d) dryer
10. Which of the following element is not a metal (a) aluminium (b) sodium (c) chlorine (d0 magnesium
11. All are laboratory apparatus except ________ (a) licker (b) beaker (c) round bottom flask (d0 flask bottom flask
12. All physical changes are ________ (a) non – reversible (b) easily reversible (c) spontaneous (d) dark
13. ________ states that electron should be single filled into degenerate orbital before double filling (a) Aufbau (b) Paul exclusion principle (c) Hund’s ruel (d) electron rule
14. The chemical formular for calcium hydroxide is (a) Ca [0H]₃ (b) Ca0 (c) Ca0H (d) Ca[0H]₂
15. The oxidation number of carbon is CaC0₃ is ________ (a) + 2 (b) +4 (c) +3 (d) +1
16. The content of mixture are ________ combined (a) physically (b) chemically (c) biologically (d) mentally
17. All chemical changes are ________ (a) non reversible (b) basicly reversible (c) spontaneous (d0 dark
18. Which of this is the same in isotopes of an element? (a) mass number (b) number of neutron (c) number of proton and neutron (d) the atomic number
19. The rare gases are stable because they ________ (a) are mono atomic (b) have duplex or octect electronic configuration in the outermost shells of their atoms (c) have no neutrol in their nucleus (d) are volatile gases
20. A molecule is the smallest particle of ________ (a) a matter that can exist in free state (b) an element that can exist in free state (c) a lattice that can emit in a free state (d) a substance which still maintain the chemical properties of the compound

THEORY (ANSWER FOUR ONLY)

1a. Define chemistry

b. Explain the concept of scientific approach

c. List ten laboratory apparatus and give one uses of any five

2a. What is matter

b. Differentiate between mass and weight

c. Mention the states of matter and use the triangle diagram to show their inter-relationship

3a. What are elements

b. Mention the first 20 elements and give their symbols

4a. State the following

(i) Aufbau principle (ii) Hund’s rule

(iii) Paulin exclusion principle

b. Show the orbital configuration for (a) Na (b) Ne (c) K (d) Ca (e) N (f) Al (g) Cl

5a. Define mixture

b. Mention five (5)separation techniques and write short note on two only

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FISRT TERM EXAMINATION

2019/2020 ACADEMIC SESSION

SUBJECT: CHEMISTRY CLASS: S.S.S 2

INSTRUCTION: ANSWER ALL QUESTIONS IN THIS SECTION

1. The elements in the periodic table are arranged in order of their ___________ (a) mass number (b) orbital value (c) atomic number (d) molecular shape
2. Elements in the same group of periodic table have ___________ (a) the same number of valency electron (b) similar electronic configuration (c) the same number of electron (d0 similar orbital configuration
3. S-block elements of the periodic table are made up of ___________ (a) group 1, 2, 3 (b) group 3 and 4 (c) group 7 (d) group 1 and 2
4. In the rediar equation below, the value of x is? (a) 5e^– (b) 10e^– (c) 3e^– (d) 2e^–
5. The bond type in diatomic nitrogen gas is ___________ (a) double covalent bond (b) triple covalent bond (c) single covalent bond (d0 electrovalent bond
6. The flow of current in electrolysis is due to the movement of _________ (a) ions (b) charges (c) electrons (d) light
7. All these properties belong to halogen except _________ (a) they are non – metal (b) they are coloured (c) they exist as diatomic molecule (d0 they do not ionize to form univalent negative ions
8. The type of chemical reaction shown below is _________ (a) hydrolysis (b) neutralization (c) ozonolysis (d0 direct combination
9. Colrosion in iron is called _________ (a) tarnishing (b) electroding (c) rusting (d0 galvanizatin
10. In the activity series of metals, metals higher up will serve as _________(a) cathode (b) anode (c) salt bridge (d) none of the above
11. Electrolyte in the dry lechlanche cell is _________ (a) anhydrous ZnS0₄ (b) NH₄Cl paste (c) mushin bag (d) party Mn0₂
12. Which of the following decrease across the period (a) atomic size (b) electron afirmity (c) electronegativity (d0 inert tendencies
13. The major function of a salt bridge in cell is to _________ (a) smotten the electron flow (b) to provide electrolyte (c) to provide adequate driving force (d) to complete the electric
14. Calculate the mass of aluminium deposited when a current of 3.0 amperes is passing through a aluminium electrodite for 2 hour [Al = 27, 2 Faraday = 96500c] (a) 1.0g (b) 6.04g (c) 2.12g (d) 2.02g
15. One Faraday equal _________ columbs (a) 9650 (b) 96500 (c) 310 (d) 95600
16. What quantity of electricity is consumed when 10 amperes was consumed in 1 hour during electrolysis? (a) 3600 coulombs (b) 7200 coulombs (c) 72 kilo coulombs (d) 36 kilo coulombs
17. From Cl₂ + 2kBr → 2Kcl + Br₂, chlorine is _________ (a) strong reducing agent (b) an aerial (c) strong oxidizing agent (d) an electron donor
18. The oxidation number of manganese in Mno₄^– is _________ (a) +8 (b) -7 (c) +7 (d) -6
19. _________ is the colour of KMn0₄ (a) green (b) purple (c) orange (d) black
20. The IUPAC name of K₂ Cr₂ 0₇ is _________ (a) potassium chromium (ii) (b) potassium heptaoxochromium (v) (c) potassium pentaoxochrominum (vi) (d) potassium dichionate (vi)

THEORY [ANSWER ANY FOUR)

1. What is oxidation and reduction reaction under the following heading (a) addition of oxygen (b) removal of hydrogen (c) addition of electronegative element (c) electron transfer/removal of electron

b. What is oxidation number

2a. state the periodic law

b. Explain the following trends

(i) Ionic size (ii) ionization energy (iii) electron affinity (iv) electronegativity

3. Differentiate the following

(i) Electrovalent and covalent compound

(ii) Electrolytes and non – electrolyte

(iii) Weak and strong electrolyte

(iv) Conductors and non – conductors

b. What is electrolysis

a. Mention and explain the factors affecting preferential discharge of ions

b. State ionic theory

5. Consider the following redox reactions which of the species is

(i) oxidized (ii) the reduction agent (iii) reduced (iv) the oxidizing agent

(a) Cu0_(s) + C0_(g) → Cu + C0₂ (g)

(b) Cr₂ 0₇^2- + Fe²⁺ → Cr³⁺ + Fe³⁺

b. Balance this equations for the reaction occurring in acidic medium using the ion electron method

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FISRT TERM EXAMINATION

2019/2020 ACADEMIC SESSION

SUBJECT: CHEMISTRY CLASS: S.S.S 3

INSTRUCTION: ANSWER ALL QUESTIONS IN THIS SECTION

1. Citric acid appears in unripe orange while ethanoic acid appears in ___________ (a) unripe pawpaw (b) carrot (c) ethanol sourced (d) vinegar
2. Esters are employed in the following except ___________ (a) making perfumes (b) nail vanishes (c) making cement (d) making solvent for cellulose trioxonitrates
3. The name of (CH₃)₂ CHC00H is ___________ (a) propanoic acid (b) 2-methyl propanoic acid (c) dimethyl butanoic acid (d) 2,2, dimethyl propanoic acid
4. Oil can change into fat in the presence of nickel at 180⁰c through a process called ___________ (a) alkylation (b) hydrogenation (c) polymerization (d) substitution
5. All carbonhydrates contain (a) carbon and oxygen (b) carbon and hydrogen (c) carbon, oxygen, and hydrogen (d) carbon, sulphur and hydrogen
6. Ethanedioc acid is ___________ acid (a) a mineral acid (b) a common fatty acid (c) a dicarboxylic acid (d) an aromatic carboxylic acid
7. The general formula for, carbohydrate is ___________ (a) CnH₂n0 (b) CnH₂n 0n (c) C₂n Hn 0n (d) Cn H₂n + 2
8. These are not true transition element except ___________ (a) Zn (b) Sc (c) Cu (d) N
9. The name of C₅Hu C00 C₄H₉ is ___________ (a) Butyl pentanoate (b) Butyl hexanoate (c) Butyl butanoate (d) Butyl heptanoate
10. Which one is the most common iron ore? (a) Magnitite (b) spathic iron ore (c) Haematite (d) Dolomite
11. Bronze card bass are both metallic alloys, which of these constituent is common to both alloys? (a) copper (b) lead (c) silver (d) zinc
12. Conversion of coke to carbon (II) oxide in a furnace is _________ (a) Enthermic (b) Isothermic (c) exothermic (d) hyposthermic
13. The following are characteristics of the transition element with the exception of ___________ (a) coloured ions (b) variables oxidation state (c) high tendency to catenate (d) complex ion formation
14. Wrought iron is the ___________ form of ion (a) most impure (b) most brittle (c) most carbon free (d) purest
15. If the value of ∆H for a reaction is negative, it means that het reaction is ___________ (a) endothermic (b) exothermic (c) slow (d) spontaneous

H CH₃ H H H H

l l l l l l

H – C – C – C – C – C – C – H

l l l l l l

H CH₃ H H H H

The IUPAC nomenclature of the compound above is ___________ (a) 2 – dimethyl hexane (0b 2, 5 dimethyl hexane (c) 2, 2, – dimethyl hexane (d) 2, 2, – dimethyl hexane

1. If the hydrolysis of groundnut oil by potassium hydroxide is known as ___________ (a) hydrogenation (b) saponification (c) esterification (d) neutralization
2. When protein is heated to high temperature it undergoes (a) condensation (b) denaturation (c) hydrolysis (d0 polymerization
3. Which of the following substances give a brick red precipitate when heated with fehlings solution (a) alkanoaies (b) carbohydrates (c) fats and oil (d) reducing sugar
4. What is the major product formed when C₂H₅0H reacts with CH₃C00H? (a) C₂H₅ C00CH₂ (b) C₂H₅C0CH₂ (c) CH₃C00C₂H₅ (d) C₃H₇C00H

THEORY: [ANSWER FOUR QUESTIONS]

1ai. Mention 2 physical properties of alkanoic acid

ii. Mention 2 uses of alkanoic acid

b. Write out four isomers of heptanoic acid

ii. Mention 2 uses of ethyl ethanoate

c. Explain the concepts of reversible reaction and give one equation

2ai. Define saponification

ii. What are disaccharide

b. Explain with equation, the preparation of ethanoic acid

c. Mention four chemical properties of ethanoic acid and equation two

3a. Mention 2 physical properties of fats and oils

i. What are fat and oil?

ii. Mention 2 chemical properties of fats and oil

c. Mention four use of fats and oils

4a. What are transition elements?

ii. Mention four properties of transition element and explain two

b. Mention 3 types of iron

5a. Write short notes on the following

(i) Cast iron

(ii) Pig iron

(iii) Wrought iron

b. Explain zinc is not a typical transition element

ii. Using equation of reaction, explain the extraction of iron from haematite.