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Comprehensive Overview of Chapter 1 & 2 Solutions in Chemistry

This document provides detailed solutions for Chapters 1 and 2 of a chemistry course. It covers various concepts including the states of matter (solid, liquid, gas), types of mixtures (homogeneous vs heterogeneous), density calculations, the conservation of mass, empirical and molecular formulas, and the properties of different chemical compounds. These solutions include multiple-choice questions and explanations to enhance understanding of core chemistry principles, making them ideal for students preparing for exams or seeking to solidify their grasp of key concepts.

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Comprehensive Overview of Chapter 1 & 2 Solutions in Chemistry

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  1. Chapter 1 HW Solutions

  2. Ch 1.1 – 1.3 • #2 • A) solid • B) gas • C) liquid • D) gas

  3. #4 • A) homogeneous mixture • B) heterogeneous mixture • C) pure substance • D) mixture (hetero vs. homo can’t be determined by visual inspection)

  4. #8 • A) Be B) Cs C) F • D) Mn E) As F) Xe G) P • H) Sc

  5. #10 • A) Barium • B) Californium • C) Molybdenum • D) Selenium E) Thallium • F) Vanadium G) Gold • H) Zirconium

  6. #11 • A is a compound – rationale CO2 produced • B is probably compound because it is a white solid

  7. Ch1.4 – 1.6 • #18a

  8. 18b

  9. 18 c, d, e

  10. 18 f, g

  11. #20

  12. #24 • Vol = length3; density = mass/vol

  13. #27 • Thickness=volume/area

  14. CH 1.7 – 1.9

  15. #34 • A) 4 • B) 3 • C) ambiguous 5,6, or 7 • D) 6 • E) 6

  16. #36 • A) 1.44 X 105 • B) 9.75 X 102 • C) 8.90 X 105 • D) 6.76 X 104 • E) 3.40 X 104 • F) –6.56

  17. #38 • A) -2.3 X 103 • B) 8.260 X 107 • C) 3.4 X 104 • D) 7.62 X 105

  18. #41

  19. #43 a-d

  20. #43 e & f

  21. #45

  22. Chapter 2 HW Solutions

  23. 2.1 – 2.3 • #2 • 6.500 g compound - .384 g H = 6.116g S • Conservation of Mass • Atoms are not created or destroyed so if a compound has only H and S and .384 grams is H the rest must be sulfur

  24. #4 integer ratio indicates combining F units that are indivisible

  25. #5 • Evidence that cathode rays were negatively charged was the electric and magnetic field deflected the ray the same way it would a negative charge and that the negative plate exposed to the cathode rays acquired a negative charge.

  26. #11

  27. #14 • A) 32P has 15 p, 17n, 15 e • B) 51Cr has 24p, 27n • C) 60Co has 27 p, 33 n

  28. Ch 2.4 – 2.5 • #20 • A) Lithium (metal) B) scandium (metal) • C) germanium (Metalloid) D) ytterbium (metal) • E) manganese (metal) F) gold (metal) • G) tellurium (metalloid)

  29. #21 • A) K, alkali metals (metal) • B) I, halogens (nonmetal) • C) Mg, alkaline earth metals (metal) • D) Ar, noble gases (nonmetal) • E) S, chalcogens (nonmetals)

  30. #23 • An empirical formula shows the simplest ratio of the different atoms in a molecule. • A molecular formula shows the exact number and kinds of atoms in a molecule. • A structural formulas shows how these atoms are arranged.

  31. #26 • A) 4 • B) 6 • C) 9

  32. #28 • See board • A) Draw C2H5Br (1-bromo-ethane) • B) Draw C2H7N ( dimethylamine) • C) Draw CH2Cl2 ( dichloromethane) • D) Draw NH2Cl (chloroamine)

  33. #30 • A) SN • B) C7H15 • C) C3H5O • D) P2O3 • E) C3H5F4 • F)SiO3

  34. #32 • A) Ba2+ • B) La2+ or La3+ • C) Ga3+ • D) S2- • E) Br -

  35. #61

  36. Chapter 2.6 – 2.7 #38 • Molecular (all atoms are nonmetals) c) SCl2 • Ionic (formed by a cation and an anion, usually contains a metal cation)— a) Sc2O3 b) NaI d) Ca(NO3) 2 e) FeCl3 f) LaP g) CoCO3 h) (NH4) 2SO4

  37. #39 • A) ClO2- B) Cl- C) ClO3- • D) ClO4- E) ClO-

  38. #42 • A) silver sulfide • B) barium phosphate • C) magnesium chlorate • D) strontium sulfite • E) cobalt (II) bromide (cobaltous bromide) • F) tin (II) iodide (stannous iodide) • G) chromium (III) nitrate (chromic nitrate)

  39. #42 continued • H) zinc hydrogen phosphate (notice the lack of roman numerals—it has a definite charge of +2) • I) silver perchlorate (notice the lack of roman numerals—it has a definite charge of +1) • J) ammonium dichromate

  40. #44 • A) Mg3N2 • B) FeSO3 • C) Cr2(CO3)3 • D) CaH2 • E) Mg(HCO3)2 • F) KClO • G) Cu(C2H3O2)2

  41. #46 • A) HBr • B) H2SO3 • C) HNO2 • D) carbonic acid • E) chloric acid • F) acetic acid

  42. #48 • A) dinitrogen monoxide • B) nitrogen monoxide • C) nitrogen dioxide • D) dinitrogen pentoxide • E) dinitrogen tetroxide

  43. #58 • A) alkali metal – K • B) an alkaline earth metal – Ca • C) a noble gas – Ar • D) a halogen – Br • E) a metalliod – Ge • F) a nonmetal in 1A – H • G) a metal that forms a 3+ charge- Al • H) a nonmetal that forms a 2- charge – O • I) a metal that resembles Al - Ga

  44. #62 • A) Nickel (II) oxide, 2+ • B) Manganese (IV) oxide, 4+ • C) Chromium (III) oxide, 3+ • D) Molybdenium (VI) oxide, 6+

  45. #63 • Fe3S4 could be aq homo mixture where the Fe2+ and the Fe3+ ions are portions of the lattice structure

  46. #64 • A) IO3- • B) IO4- • C) IO- • D) HIO • E) HIO4 (or H5IO6)

  47. #67 • A) potassium nitrate • B) sodium carbonate • C) calcium oxide • D) hydrochloric acid • E) magnesium sulfate • F) magnesium hydroxide

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