Structure and Bonding Questions and Answers - Chemistry Form 2 Topical Revision

Questions

1. Ethanol is a liquid at room temperature but does not conduct electricity. Explain.
2. 1. Distinguish between a covalent bond and a co-ordinate bond.
   2. Draw a diagram to show bonding in an ammonium ion. (N = 7, H = 1)
3. 1. Explain why the metals magnesium and aluminium are good conductors of electricity.
   2. Other than cost, give two reasons why aluminium is used for making electric cables while magnesium is not.
4. Explain why the boiling point of ethanol is higher than that of hexane. (Relative molecular mass of ethanol is 46 while that of hexane is 86).
5. What is meant by dative covalent bond?
6. Sodium and Magnesium belong to the same period on the periodic table and both are metals. Explain why magnesium is a better conductor of electricity than sodium.
7. Using dots and crosses to represent electrons, draw the structures of the following:
   1. Phosphorous chloride (PCl₃)
   2. Hydroxonium ion (H₃O⁺)
8. Between aluminium and copper which one is a better conductor? Explain
9. Water has a boiling point of 100oC while hydrogen chloride has a boiling point of -115^oC. Explain
10. Explain why luminous flame is capable of giving out light and soot
11. When blue litmus paper is dipped in a solution of aluminium chloride it turns red. Explain
12. Carbon and Silicon are in the same group of the periodic table. Silicon (IV) Oxide melts at 2440^oC while solid Carbon (IV) Oxide sublimes at -70^oC. In terms of structure and bonding, explain this difference
13. Element A has an atomic number of 6 and b has an atomic number of 9:
    1. Write the electron arrangements for elements A and B
    2. Using dot (•) and cross (x)diagram, show how A and B combine to form a compound
14. 1. Explain why aluminium is a better conductor of electricity than magnesium
    2. Other than cost and ability to conduct, give a reason why aluminium is used for making cables while magnesium is not
15. Explain how electrical conductivity can be used to distinguish between magnesium oxide and silicon (IV) oxide
16.   
    1. The diagram below represents part of the structure of sodium chloride crystal
       
       The position of one of the sodium ions in the crystal is shown as;
       1. On the diagram, mark the positions of the other three sodium ions
       2. The melting and boiling points of sodium chloride are 801^oC and 1413^oC respectively. Explain why sodium chloride does not conduct electricity at 25^oC, but does not at temperatures between 801C and 1413C
    2. Give a reason why ammonia gas is highly soluble in water
    3. The structure of ammonium ion is shown below; 
       
       Name the type of bond represented in the diagram by N → H
    4. Carbon exists in different crystalline forms. Some of these forms were recently discovered in soot and are called fullerenes
       1. What name is given to different crystalline forms of the same element
       2. Fullerenes dissolve in methylbenzene while the other forms of carbon do not. Given that soot is a mixture of fullerenes and other solid forms of carbon, describe how crystals of fullerenes can be obtained from soot
       3. The relative molecular mass of one of the fullerenes is 720. What is the molecular mass of this fullerene
17. Explain the following observations:-
    1. NaCl allows electric current to pass through them in molten state
    2. Graphite is a non-metal yet it is a conductor of electricity
18. Study the table below and answer the questions that follow:-
    

    Substance		A	B	C	D	E	F
    Melting Point (oC )		801	113 119	-39	5	-101	1356
    Boiling point (oC)		1410	445	457	54	-36	2860
    Electrical Conductivity	Solid	Poor	Poor	Good	Poor	Poor	Poor
    	Liquid	Good	Poor	Good	Poor	Poor	Poor

    Identify with reasons the substances that:
    1. Have a metallic structure (1½mk)
    2. Have a molecular structure and exist in the liquid state at room temperature and pressure
    3. Suggest a reason why substance B has two melting points
    4. Substances A and C conduct electric current in the liquid state. State how the two substances differ as conductors of electric current
19.   
    1. Sodium metal tarnishes when exposed to the air where a white powder is formed on its surface. A small piece of this sodium metal was dropped into 25g of ethanol and 1200cm³ of hydrogen gas was evolved at r.t.p. The unreacted ethanol was evaporated and a white solid remained. (Na=23, molar gas volume at r.t.p = 24dm³, C=12, O =16, H=1)
       1. Write a chemical equation for the reaction between ethanol and sodium metal
       2. Determine the mass of sodium that reacted with ethanol
       3. What mass of ethanol evaporated?
       4. The ethanol was evaporated at 80oC, while the white solid remained unaffected at this temperature. What is the difference in structure of ethanol and the white solid?
    2.   
       1. Name an inorganic liquid which liberates hydrogen gas with sodium metal
       2. What two differences would you observe if similar pieces of sodium were dropped separately into small beakers containing equal amount of ethanol and the liquid named in (b)(i) above respectively
    3.   
       1. Give the name of the white powder formed on the original piece of sodium metal
       2. Explain how the white powder named in (c)(i) is formed
20. The grid below represents part of the periodic table. The letters do not represent actual symbols of the elements. Study it and answer the questions that follow:-
    
    
    1. What type of bond would you expect in the compound formed between H and F. Explain
    2.   
       1. Which of the elements J and M will have a greater atomic radius? Explain
       2. Elements F and N are in the same group of periodic table. How do their atomic radius compare? Explain
    3. An element W has atomic number 15. Indicate the position it would occupy in the table above
    4. What is the name given to elements X – Z?
    5. Why is J used in electric cables where Q is not
    6. P and J are termed as metalloids. What does the term metalloid mean?
    7. How would you expect the reactivity of H and M to compare? Explain
21.   
    1. Part of the periodic table is given below study it and answer the questions that follow.
       The letters do not represent the actual elements
       
       
       1. What type of bond is formed when Y reacts with Z. Explain
       2. Explain the difference in the atomic radii of element A and B
       3. Explain the difference in the reactivity of Z and B
    2. Study the information in the table below and answer the questions that follow:
       

       Element	Electronic configuration	Ionization energy KJmol-1
       P	2:1	519
       Q	2:8:1	494
       R	2:8:8:1	418

       (The letters do not represent the actual symbols of the elements)
       1. What is meant by ionization energy?
       2. Element R has the lowest ionization energy. Explain
       3. When a piece of element Q is placed on water it melts and a hissing sound is produced as it moves on the water surface. Explain these observations
       4. Write the equation for the reaction between element Q and water
22. The table below shows the elements in the third period, the oxides of the third period and their properties. The letters are not the actual symbols of the elements. Study the information and answer the questions that follow:
    

    Element	Atomic number	Atomic radius(nm)	Oxide	State at RT	Oxide melting point ºC
    M	11	0.191	M2O	Solid	1132
    N	……… ……..	0.160	NO	Solid	2852
    P	13	0.130	………	Solid	2072
    Q	14	0.118	QO2	……….	1610
    R	………	0.110	………	Solid	580
    S	16	0.102	SO2	………	-75
    T	17	0.099	TO2	Gas	-60
    V	18	0.095	X	X	X

    1.  
       1. Complete the table above
       2. Explain the trend in the atomic radius across the period
       3. Explain why the oxide of element V does not exist
    2. 1. Name the type of structure and bond in the following oxide
          

          Oxide	Structure	Bond type
          NO
          TO2

          
          
       2. Using dots and crosses to represent electrons. Show the bonding in the oxide, QO₂
    3. 1. Explain why elements P conducts electricity but T does not
       2. The oxide of P reacts both acids and alkalis. Give the name of this kind of oxide
23. The table below gives information about elements A₁, A₂, A₃ and A₄
    

    Element	Atomic number	Atomic radius (nm)	Ionic radius (nm)
    A1	3	0.134	0.74
    A2	5	0.090	0.012
    A3	13	0.143	0.050
    A4	17	0.099	0.181

    1. In which period of the periodic table is element A₂? Give a reason
    2. Explain why the atomic radius of:
       1. A₁ is greater than that of A₂
       2. A₄ is smaller than its ionic radius
       3. Select the element which is in the same group as A₃
       4. Using dots (•) and cross (x) to represent outermost electrons, draw a diagram to show the bonding in the compound formed when A₁ reacts with A₄
24. The atomic number of element P is 11 and that of Q is 8
    1. Write down the possible formula of the compound formed between P and Q
    2. Using dots (•) and crosses(x) to represent electrons draw a diagram to represent the bonding in the compound in (a) above
25. Name the type of bonding and structure found in: -
    1. Ice
    2. Magnesium chloride
26. Use the scheme to answer the questions that follow:
    
    
    1. Identify solid N ……………………………………………………………….
    2. Write a balanced equation for the formation of Q
    3. Write the formula of the complex ion formed when sodium hydroxide is added to solution L in excess
27. 1. Using dots (•) and crosses (x) to represent electrons show bonding in: 
       1. NH₂⁻ ( N=7, H=1)
       2. S₈ (S = 16)
    2. Show bonding in Carbon (II) Oxide by use of (—) or ( → ) to represent bonds.
28. In terms of structure and bonding, explain why diamond is the hardest naturally occurring substance
29. Identify the bond types in the diagram
30. Elements A, B, C, and D are not actual symbols, have atomic numbers 19, 9, 12 and 10 respectively.
    1. Which two elements represent non-metals
    2. Write the formula of the compound formed between elements B and C and identity the bond present in the compound
31. 1. Distinguish between a covalent and dative bond
    2. Explain why nitrogen gas reacts with oxygen at very high temperature
       
32. Draw a dot (•) and cross (x) diagram to show bonding in:-
    1. Ammonium ion (NH₄⁺) (N = 7.0, H= 1) 
    2. Silane (SiH₄) (Si= 14, H = 1)
33. Below is a table oxides of some period three elements
    

    Oxides	Na2O	P4O6	SO2	Cl2O
    State at room temp	Solid	Solid	Gas	Gas

    
    
    1. Give the systematic name of Cl₂O
    2. Explain why Na₂O exists as a solid whereas SO₂ is a gas at room temperature
34. The table below shows properties of period three chlorides
    

    Formular of compound	NaCl	MgCl2	AlCl3	SiCl4
    Bp (oC)	1470oC	1420oC	180oC	60oC

    
    Explain why AlCl₃ solid has a much lower boiling point than MgCl₂ solid

Answers

1. Ethanol contains molecules ✓1 which are not✓1 responsible for electrical conductivity
2. 1. A covalent bond is formed by equal contribution of the shared electrons by the atom. ✓1
      Co-ordinate bond is where the shared electrons are contributed by one of the atoms.✓1
   2.  
      
3. 1. Have delocalized valency electrons ✓1
   2. Aluminium is a better conductor/Aluminium has three delocalized electrons while magnesium has 2. ✓1 It is resistant to corrosion.
4. In addition to vander waals forces, strong hydrogen✓bonds exist in ethanol. These bonds require ✓more energy to break.
5. Is a covalent bond in which the shared pair of electrons comes from the same atom
6. Magnesium has more delocalized electrons than sodium
7. 1. Phosphorous chloride (PCl₃)
      
      
   2. Hydroxonium ion (H₃O⁺)
      
      
8. Aluminium – it has more delocalized (3) electrons than copper (2e^-)
9. Hydrogen chloride has got only Van der waal while water has H-bonds in addition to Van der waal forces which are stronger
10. It contains white hoe carbon particles (½mk) that allow to give out light (½mk). When those particles cool down (½mk) they turn black and settle down as soot.(½mk)
11. Aluminium chloride hdrolyses √1 in solution producing hydroxonium ions √½ which turn blue litmus paper red. √½
12. Silicon (IV) oxide forms giant √1 atomic structure of strong covalent√½ bonds having high melting point. Carbon (IV) oxide is simple molecular substance of weak intermolecular √½ attraction forces√1 9the Van der Walls’ forces) that have low melting point.
13. 1. A: 2,4√ ½
       B: 2,7√ ½
14. 1. Because aluminium √1 has more delocalized √1 electrons than magnesium.
    2. It does not corrode. √1
15. Magnesium oxide has a giant ionic √ ½ structure while silicon (IV) Oxide has a giant atomic structure. MgO in molten state √ ½ contains delocalized ions √ ½ which conduct electricity while SiO₂ has no ions present √
16.   
    1.   
       2. At 25^oC, sodium chloride is in solid form. Ions cannot move. Between 801^oC and 1413^oC sodium chloride is in liquid state, ions are mobile
    2. Both ammonia and water are polar molecules and hydrogen bonds are formed
    3. N→H//co-ordinate bond/Dative bond
    4.   
       1. Allotrope
       2. Add methylbenzene to soot in a beaker. Shake and filter. Warm the filtrate to concentrate it. Allow the concentrate to cool for crystals to form. Filter to obtain crystals of fullerene
       3. ⁷²⁰/₁₂ = 60
17.   
    1. NaCl has mobile ions in molten state and in aqueous solution
    2. Graphite has delocalized electrons in the structure which carry electric current
18.   
    1. C; Reason:- Good conductor of electricity in both molten and solid state..
    2. D-Its melting point is below room temp. and boiling point above room temp.
    3. It exist in allotropic form.
    4. A conducts electricity by use of mobile ions while C conducts by use of delocalized electrons.
       Both must be correct for the 1 mk.
19.   
    1.   
       1. 2Na_(s) +2CH₃CH₂OH_(l) → 2CH₃CHONa_(aq) + H_2(g)
       2. Mole ratio btn Na: H = 2:1
          Mole of Holes H₂ = 1200cm³
                                      2400cm³
          = 0.05moles
          Moles of Na = 0.05 x 2
          = 0.1moles
          Mass of Na = 0.1 x 23
          = 2.3g of sodium
       3. Mole ration C₂H₅OH:H₂
          Moles of C₂H₅OH = 0.05 x 2
          = 0.1moles
          mass of C₂H₅OH reacted = 0.1 x 46
          = 4.6g
          Mass evaporated = 50 - 4.6
          = 45.4g of C₂H₅OH
       4. – Has molecular structure – with hydrogen bonds being molecules While - C₂H₅ONa – has giant ionic structure with ionic bonds
    2.   
       1. Water
       2. In ethanol – sinks in water and stream of bubbles observed /seen While in water – floats on water and darts on water
          - Hissing sound is heard (any two)
20.   
    1. ionic or electrovalent
       F is metal and H is non metal.
    2.   
       1. J atomic radius decrease a long a period from left to right nuclear change attraction increase positive nuclear change increase due to increase in the number of protons.
       2. F has a smaller atomic radius than N level down the grown.
    3. W is group 5 period 3
    4. Transition metals.
    5. J has 3 valence electrons which and delocalizal whole Q has only 2 electron:hence J has high electrical conductivity due to high number of decalized electron.
    6. The reactions have both metallic and non metal properties
    7. H is more reactive than M non metal reactivity increase up the group due to decrease in electro negativity down the group.
21.  
    1.  
       1. Ionic bond
          Y losses that is gained by Z
       2. Atomic radius of A is larger than that of B has higher nuclear charge than A
          Electrons in B are drawn closer to the nucleus( ½mk)
       3. Z is more reactive than B
          Z has a smaller atomic radius so will readily attract extra electron
    2. 1. Energy needed to remove an electron from an atom in gaseous state
          
       2. R has a largest atomic radius; (½mk)
          Therefore the electron is easily lost 
       3. Reacts vigorously with water producing gas bubbles that give the hissing sound and propels the metal
          The metal floats on water as it is light
       4. 2Q_(s) + H₂O_(l) → 2QOH_(aq) + H_2(g)
22.  
    1.  
       1.  
          

          Atomic number	Oxide formula	State at RT
          N-12	P2O3	Q - solid
          R- 15	R2O5	S- Gas

          
          
       2. The atomic radius decreases across the period from M to V. Due to increasing nuclear charge// increasing number of protons which pulls the outermost electrons closer to the nucleus
       3. Element V is chemically stable// stable electronic configuration does not gain or loss// share electrons with oxygen to form an oxid
    2.  
       1.  
          

          Oxide	Structure	Bond type
          NO	Giant ionic	Ionic/ electro valent
          TO2	Simple covalent/ molecular	Covalent

          (½ mark each – total 2 marks)
    3. 1. P is a metal with valency electrons free to move but T is a non- metal// molecular has no free valency electrons// molecules are electrically neutral
       2. Amphoteric oxide
23.   
    1. Period 2 its electronic arrangement is 2,3, or it has two energy levels.
       - Accept shells or orbitals in place of energy levels
    2. 1. - Across a period nuclear charge increases from, left to right exerting greater pull/attraction on available electrons
       2. - A₄ gains an electron and the incoming electron is repelled by other electrons or electron cloud increases
       3. A₂
       4.  
          
24.   
    1. P₂Q √ reject QP₂
    2.  
       
25.  
    1. Ice : Bonding : - Covalent √ ½ ½ mk
       Structure : - Simple molecular √ ½ ½ mk 2mks
    2. Magnesium chloride : Bonding : - Ionic √ ½ ½ mk
       Structure: - Giant ionic ½ mk
26.  
    1. Zinc oxide √1 ZnO (1 mk)
    2. ZnO_(s) + H₂SO_4(aq) √1 → ZnSO_4(aq) + H₂O_(l) (1 mk)
    3. Zn(OH)₄ √1 (1 mk)
       
       
       
       
27.  
    
28. Diamond has giant atomic structure in each carbon atom√ ½ is bonded to four other √ ½ carbon atoms arranged in regular tetrahedron shape in all direction forming rigid (strong)√ ½ mass of atoms due to uniformity of covalent bonds between the atoms√ ½ (2mk)
29. 3 Covalent √1 bonds and one dative √1 bond
30.  - CB₂
    - Ionic bond
31. 1. Covalent bond is bond between non-metal atoms where shared electrons are donated equally by all the atoms involved.
       Dative bond is a bond in which shared electrons are donated by one atom.
    2. The presence of triple bond in nitrogen requires very high temperatures to break
32.  
     
33. 1. Chlorine (I) Oxide
    2. - Na₂O has stronger ionic bond between ions in it, while SO₂ has a weak Van der walls bond between its molecule
       - ∴Na₂O requires more heat energy to weaken or break the ionic bonds than SO₂ requires breaking Van der walls bonds
34. AlCl₃ has simple molecular structures with weak Vander waals between the molecules MgCl₂ has giant ionic structures with strong ionic bonds
    Due to insoluble coating of aluminum oxide which prevents any reaction √1