TASK 1 1. The arrangement of valence electrons for the noble gases below is an octet, except … . A. Xe D.Ne B. Kr C. Ar E.H 2. The stability of noble gases is used as a benchmark for other atoms, so that these atoms try to achieve an electron configuration like that of the nearest noble gas by carrying out the methods below, except … . A. releasing electrons B. capturing electrons C. pairing electrons D. accepting electron pairs E. accepting at least two pairs of electrons 3. Elements with electron configurations: 2, 8, 8, 2, if it will bind other elements to form a compound, then the best step with ... . A. release of 1 electron, so that it is charged 1+ B. release of 2 electrons, so that it is charged 2+ C. capture of 1 electron, so that it is charged 1- D. capture of 2 electrons, so that it is charged 2- E. pairs 2 electrons with 2 other electrons 4. An element with an electron configuration: 2, 6. The tendency of this element when it will bond with other elements is ... . A. release of 2 electrons, so charged 2+ B. release of 4 electrons, thus charged 4+ C. absorption of 2 electrons, thus charged 2-
D. absorption of 4 electrons, thus charged 4- E. pairs of 6 electrons 5. Atom 12A has characteristic… . A. 4 valence electrons B. tends to lose 4 electrons C. there are 2 electrons in the outermost shell D. tends to gain 4 electrons E. tends to pair 4 electrons 6. The following elements form positive ions, except … A. 11Na B. 19K C. 20Ca D. 35Br E. 37Rb 7. It is known that the data for a compound are: (i) ionic bonds (ii) bond formula XY2 (iii) when dissolved in water conducts electricity From these data, X is a group element … . A. IA B. VIA C. IIA D. VIIA E. IIIA 8. Among the elements of group IVA which have special properties because they can forming a bond chain is an element of … .
A. silicon D. antimony B. arsenic C. carbon E. bismut 9. The tendency of positively charged atoms is … . A. has a large electron affinity B. has a small ionization energy C. has a large electronegativity D. has a large ionization energy E. has a moderate electronegativity 10. The following elements tend to capture electrons is ... . A. 11Na B.12Mg C.13Al 11. It is known that the 7N D. 16S E. 18Ar , 8Oh, 9F, 10Ne, 11Na, 12Mg, 16S, 19K, and 20Ca. Couple in elements below have the same valence electrons, except … . A. K+ and Ca2+ D. Na+ and O– B. Mg2+ and S2– E.Ne+ and O– C. N– and F+ 12. The bond that occurs between a highly electropositive atom and a highly electronegative atom is called a bond… A. ion B. single covalent C. double covalent D. triple covalent E. covalent coordination
13. Element 19X reacts with 16Y to form a compound with bonds ... and formula chemical… A. ion; XY B.ions; XY2 C.ions; X2 Y D.covalent; XY E. covalent; X2 14. Element X with the configuration: 2, 8, 8, 2, will bond with element Y with the configuration: 2, 8, 18, 7. The chemical formula and type of bond that occurs is... . A. XY, ion D. XY, covalent B. XY2 , ion E. XY2 , covalent C. X2 Y, ion 16. The following groups of compounds which are entirely ionic bonds are … . A. CaCl2 , CaO, H2 O, and N2 O D. KCl, NaCl, SrCl2 , and PCl5 B. MgCl2 , SrO, NO2 , and SO2 E. BaCl2 , CaCl2 , CaO C. KCl, CaO, NaCl, and MgCl2 17. 17. The following pairs of compounds have covalent bonds, except … . A. H2 SO4 and NH3 B. H2 O and HCl C. CH4 and KCl D. HNO3 and CO2 E. SO3 and PCl5 18. The elements are known: 8A, 12B, 13C, 16D, and 17E. Which of the following pairs has a covalent bond?...
A. A and D D. C and D B. B and C E. C and E C. B and D 19. The group of compounds below which are all covalently bonded are … . A. Cl2 O7 , CO2 , HCl, and NaCl D. H2 O, HCl, SF6 , and CCl4 B. SO2 , SO3 , CH4 , and CaCl2 E. NH3 , NO2 , CO, and MgO C. Ag2 O, N2 O3 , C2 H2 , and CO2 20. 20. Molecules of the following elements that have double covalent bonds are ... . A. H2 (atomic number H = 1) B. O2 (atomic number O = 8) C. N2 (atomic number N = 7) D. F2 (atomic number F = 9) E. Cl2 (Cl atomic number = 17) 21. Molecules of the following elements that have triple covalent bonds are ... . A. H2 (atomic number H = 1) B. O2 (atomic number O = 8) C. N2 (atomic number N = 7) D. F2 (atomic number F = 9) E. Cl2 (Cl atomic number = 17) 22. The following compounds have single covalent bonds, except … . A. H2 O (atomic number H = 1 and O = 8 ) B. HCl (atomic number H = 1 and Cl = 17) C. NH3 (atomic number N = 7 and H = 1) D. CH4 (atomic number C = 6 and H = 1) E. CO2 (atomic number C = 6 and O = 8)
23. The following compounds that have 2 double covalent bonds are… A. SO2 (atomic number S = 16 and O = 8) B. SO3 (atomic number S = 16 and O = 8) C. CO2 (atomic number C = 6 and O = 8) D. NO2 (atomic number N = 7 and O = 8) E. Al2 O3 (atomic number Al = 13 and O = 8) 24. Compounds Cl2 O3 (atomic number Cl = 17, O = 8) have covalent bonds coordinating as much…. A.1 B. 2 C. 3 D. 4 E. 5 25. The following compounds are polar, except … . A.CO B. H2 O C. BF3 D.CO2 E.SO3
TASK 2 1. Why do the elements in nature tend to form compounds (bond with other elements)? 2. Mention the tendency of elements when they combine to form compounds! 3. Mention the conditions of an inclined atom: a. positively charged b. negatively charged 4. What is taken by the carbon atom which has atomic number 6, in order can achieve stability (combined with other atoms)? 5. What is special about carbon atoms? 6. What is an ionic bond? 7. State the properties of ionic compounds! 8. An atom has the following data. No. Element Atomic Number Element Atomic Number 1. X 11 Y 17 2. Z 12 Y 17 3. X 11 A 16 4. Z 12 A 16 5. B 13 A 16 If the pairs of elements above form a compound, a. Name the bonds that occur b. determine the chemical formula
9. Why can Cl2 be formed, but Na2 cannot be formed? (atomic number Cl = 17, Na = 11) 10. What is a covalent bond? 11. State the types of bonds in the following compounds, including ionic bonds or bonds covalent? a. HC b. H2O c. Ag2 O d. FeCl3 e. KCl f. CuS g. ZnCl2 h. K2 SO4 i. HNO3 12. Using a Lewis structure, describe the occurrence of a covalent bond and state the type single, double, or coordination covalent bonds in: a. Cl2 f. C2 H2b . CO2 g. C2 H6c . NH3 h. CCl4 d. SO3 i. N2 j. OF2 e. H2 S (atomic number H = 1, C = 6, N = 7, O = 8, F = 9, S = 16, and Cl = 17) 13. What is meant by the failure of the octet law? 14. Give examples of compounds that fall under the octet law failure! 15. Explain the difference between polar and nonpolar compounds, and give each each example (at least three compounds)! 12. Using a Lewis structure, describe the occurrence of a covalent bond and state the type single, double, or coordination covalent bonds in: a. Cl2 f. C2 H2b . CO2 g. C2 H6c . NH3 h.
CCl4 d. SO3 i. N2 j. OF2 e. H2 S (atomic number H = 1, C = 6, N = 7, O = 8, F = 9, S = 16, and Cl = 17) 13. What is meant by the failure of the octet law? 14. Give examples of compounds that fall under the octet law failure! 15. Explain the difference between polar and nonpolar compounds, and give each each example (at least three compounds)!