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Practice Exam: Paper 1
Topic 4: Bonding
1. What is the correct Lewis structure for hypochlorous acid, a compound containing chlorine, hydrogen and oxy- gen? A. B. C. D. 2. Which compound forms hydrogen bonds in the liquid state? A. C 2 H 5 OH C. CH 3 CHO B. CHCl 3 D. (CH 3 CH 2 ) 3 N 3. How do the bond angles in CH 4 , NH 3 and H 2 O compare? A. CH 4 = NH 3 = H 2 O B. CH 4 < NH 3 < H 2 O C. NH 3 < CH 4 < H 2 O D. H 2 O < NH 3 < CH 4 4. Which combination of the characteristics of element X, a metal, and element Y, a non metal, is most likely to lead to ionic bonding? X Y A. low ionization energy high electronegativity value B. low ionization energy low electronegativity value C. high ionization energy high electronegativity value D. high ionization energy low electronegativity value
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5. Which particles are responsible for electrical conductivity in metals? A. Anions C. Electrons B. Cations D. Protons 6. Which molecule has a non-bonding (lone) pair of electrons on the central atom? A. BF 3 C. CO 2 B. SO 2 D. SiF 4 7. When C 2 H 2 , C 2 H 4 and C 2 H 6 are arranged in order of increasing carbon-carbon bond strength (weakest bond first), what is the correct order? A. C 2 H 2 , C 2 H 4 , C 2 H 6 B. C 2 H 2 , C 2 H 6 , C 2 H 4 C. C 2 H 6 , C 2 H 4 , C 2 H 2 D. C 2 H 6 , C 2 H 2 , C 2 H 4 8. The number of electrons in the valence shell of elements A and B, are 6 and 7 respectively. What is the formula and type of bonding in a compound formed by these elements? A. A 2 B, covalent C. A 2 B, ionic B. AB 2 , covalent D. AB 2 , ionic 9. Lewis structures are represented in different ways in different parts of the world. Two ways of drawing the Lewis structure for H 3 O+^ are shown below. Which statement is correct about H 3 O+? A. The ion has a tetrahedral shape. B. The H–O–H bond angle is 120°. C. The H–O–H bond angle is 90°. D. The ion has a trigonal pyramidal shape.
15. Which statement about the bonding between carbon atoms is correct? A. In C 60 fullerene each carbon atom is covalently bonded to three other carbon atoms. B. In C 60 fullerene each carbon atom is covalently bonded to four other carbon atoms. C. In graphite each carbon atom is covalently bonded to four other carbon atoms. D. In graphite each carbon atom forms a double covalent bond with three other carbon atoms. 16. Which intermolecular forces exist between molecules of carbon monoxide, CO? A. Hydrogen bonds and Dispersion forces B. Dipole-dipole attractions and Dispersion forces C. Dispersion forces only D. Dipole-dipole attractions only 17. What is the formula of magnesium fluoride? A. Mg 2 F 3 B. Mg 2 F C. Mg 3 F 2 D. MgF 2 18. What is the shape of the ammonia molecule, NH 3? A. Trigonal planar B. Trigonal pyramidal C. Linear D. V-shaped (bent) 19. Which molecule is polar? A. CH 2 Cl 2 B. BCl 3 C. Cl 2 D. CCl 4
20. Which substance can form intermolecular hydrogen bonds in the liquid state? A. CH 3 OCH 3 B. CH 3 CH 2 OH C. CH 3 CHO D. CH 3 CH 2 CH 3 21. Which compound has a covalent macromolecular (giant covalent) structure? A. MgO(s) B. Al 2 O 3 (s) C. P 4 O 10 (s) D. SiO 2 (s) 22. The electronegativities of four different elements are given below (the letters are not their chemical symbols). Element W X Y Z Electronegativity 0.9 1.2 3.4 4. Based on this information which statement is correct? A. W is a non-metal. B. W and X form an ionic compound. C. Y is a metal. D. Y and Z form a covalent compound. 23. Which species contain a dative covalent bond? I. HCHO II. CO III. H 3 O+ A. I and II only B. I and III only C. II and III only D. I, II and III
29. Which is the best description of the bonding present in silicon dioxide, SiO 2? A. Each silicon atom forms four single covalent bonds to oxygen atoms. B. Each silicon atom forms two double covalent bonds to oxygen atoms. C. Each silicon atom forms two single covalent bonds to oxygen atoms. D. Each silicon atom forms four double covalent bonds to oxygen atoms. 30. Which statement best describes the intramolecular bonding in HCN(l)? A. Electrostatic attractions between H+^ and CN–^ ions B. Only Dispersion forces C. Dispersion forces and hydrogen bonding D. Electrostatic attractions between pairs of electrons and positively charged nuclei
