Chemistry Chapter 5 Quiz Key PDF

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chapter 5 quiz with corrected answer marked...

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Chapter 5 Chemistry Quiz 1. The Lewis dot symbol consists of the symbol for the element surrounded by dot(s). What does the dot or dots represent? core electrons valence electrons atomic number atomic mass electron configuration 2. How many dots does the Lewis dot symbol for magnesium have around it? 7 1 2 0 3 3. The Lewis dot symbol for the chloride ion is

Cl − 4. Which of the following is an ionic compound H2S I2 NH3 CCl4 KI

5. Which of these ionic solids would have the largest lattice energy? BaSO4 NaF SrO CsI CaBr2 6. The lattice energy for ionic crystals increases as the charge on the ions ________ and the size of the ions ________. increases; decreases decreases; increases increases; increases decreases; decreases 7. Which pair of elements would be most likely to form an ionic compound? F and Al P and Br C and S Zn and K Al and Rb 8. What is the formula for the ionic compound formed by calcium ions and nitrate ions? Ca2NO2 CaNO3 Ca3N2 Ca2NO3 Ca(NO3)2 9. Which is the correct formula for copper(II) phosphate? Cu(PO4)2 Cu(PO3)2 Cu2PO3 Cu2PO4 Cu3(PO4)2 10. The formula for sodium sulfide is ________. NaS Na2S SeS K2S NaS2

11. The chemical formula for iron(II) nitrate is ________. Fe2(NO3)3 Fe(NO3)2 Ir(NO2)2 Fe(NO2)2 Fe2N3 12. Potassium permanganate is a strong oxidizer that reacts explosively with easily oxidized materials. What is its formula? KMnO3 K(MnO4)2 K2MnO4 KMnO4 13. Ferric oxide is used as a pigment in metal polishing. Which of the following is its formula? Fe2O3 Fe2O5 FeO FeO3 Fe2O 14. What is the name of Ba(NO2)2 ·3 H2O? trihydrobarium(II) nitrite barium nitrate trihydrate barium nitrite barium nitrite trihydrate barium(II) nitrite trihydrate 15. Iron(III) chloride hexahydrate is used as a coagulant for sewage and industrial wastes. What is its formula? FeCl3·6H2O Fe3Cl(H2O)6 FeCl3(H2O)6 Fe(Cl·6H 2O)3 Fe3Cl·6H2O 16. Which of the following is the oxoanion of bromine called the bromate ion? BrO4 2– BrO – BrO2 2– BrO32–

BrO3 –

17. Which of these compounds is most likely to be covalent? CaO CsOH LiF Sr(NO3)2 NF3 18. The compound, P4S10, is used in the manufacture of safety matches. What is its name? phosphorus decasulfide phosphorus sulfite tetraphosphorus decasulfide phosphorus sulfide phosphoric sulfide 19. What is the name of ClO– ion? perchlorate perchlorite chlorite chlorate hypochlorite 20. Which of the following is a molecular formula for a compound with an empirical formula of CH? C3H9 C4H10 C6H6 C2H6 21. Which of the following is a molecular formula for a compound with an empirical formula of CH2O and a molar mass of 150. g/mol? C5H10 O5 CH 2O C3 H 6 O 3 C7H18 O3 22. Which of the following is an empirical formula of a compound that is 52.15 percent C, 13.13 percent H, and 34.73 percent O? C3HO6 C4H12O2 CH6O2 C2H6O

23. Calculate the molar mass of Ca(BO2)2·6H2O 183.79 g/mol 233.80 g/mol 174.89 g/mol 143.71 g/mol 273.87 g/mol 24. What is the percent sodium in sodium carbonate? 11.3% 45.3% 43.4% 21.7% 27.7%

25.

25. Calculate the number of moles in 17.8 g of the antacid magnesium hydroxide, Mg(OH)2. 2.32 mol 3.28 mol 0.431 mol 0.305 mol 0.200 mol 26. How many moles are present in 17.4 g of lead? 10.06 moles 0.0840 moles 1.05×10 25moles 11.9 moles 0.0994 moles 27. Determine the number of ammonia molecules in 4.85 g of ammonia. ( N A= 6.022×1023mol –1) 2.92×10 23molecules 4.73×10 –25molecules 1.24×10 23molecules 1.71×10 23molecules 5.83×10 –24molecules

28. What is the mass of 1.21×10 20atoms of sulfur? ( NA= 6.022×10 23mol –1)

32.

2.00 mg 2.00×10 –4g 6.44 mg 3.88×10 21g 32.06 g 29. The density of water is 1.00 g/mL at 4°C. How many water molecules are present in 6.25 mL of water at this temperature? ( NA= 6.022×10 23mol –1) 6.02 ×10 23molecules 6.27×10 23molecules 0.347 molecules 2.09×1023 molecules 3.76 ×10 24 molecules 30. Which of the following substances is a molecule, but not a compound? Ar CS2 O2 CO32– SO2...