For example - Nature of Matter, 8e Neil Jespersen, Alison Hyslop

Chemistry The Molecular Nature of Matter, 8e Neil Jespersen, Alison Hyslop

(Solutions Manual All Chapter)

• / 4

Chapter 0 0-1 Chapter Zero A Very Brief History of Chemistry

Practice Exercises 0.1 This answer is student dependent.For example

Chapter 1: Measurements – Careful observations on the laboratory scale

Chapter 2: Elements – Atomic theory

Chapter 3: The Mole – Careful observations on the laboratory scale

Chapter 4: Reactions – Atomic theory

Chapter 5: Reduction Oxidation Reactions – Atomic theory

Chapter 6: Thermochemistry – Energy changes

Chapter 7: Quantum Chemistry – Atomic theory

Chapter 8: Bonding I – Atomic theory

Chapter 9: Bonding II – Geometric shapes of molecules and Atomic theory

Chapter 10: Gases – Careful observations on the laboratory scale

Chapter 11: Solids and liquids - Careful observations on the laboratory scale

Chapter 12: Solutions – Careful observations on the laboratory scale and Energy changes Chapter 13: Kinetics – Careful observations on the laboratory scale and Energy changes Chapter 14: Equilibrium – Careful observations on the laboratory scale and Energy changes Chapter 15: Acids and Bases I – Careful observations on the laboratory scale and Geometric shapes of molecules Chapter 16: Acids and Bases II – Careful observations on the laboratory scale and Geometric shapes of molecules Chapter 17: Solubility – Careful observations on the laboratory scale and Energy changes

Chapter 18: Thermodynamics – Energy changes

Chapter 19: Electrochemistry – Energy changes

Chapter 20: Nuclear chemistry – Atomic theory and Energy changes

Chapter 21: Metal complexes – Atomic theory and Geometric shapes of molecules

Chapter 22: Organic Chemistry – Geometric shapes of molecules and Energy changes 0.2 Nucleosynthesis would occur at temperatures around 1 billion degrees and a high density of nucleons.

0.3 Only light elements were synthesized during the big bang because the temperature was too high for the heavier elements to form.

0.4 Core and enriched layers or nuclei are needed for nucleosynthesis in stars because the enriched layers are the lighter layers, which react to form the heavier nuclei. The heavier nuclei are more dense and move to the center of the star. Experimental evidence for the concept of nucleosynthesis lies in the layers of the stars and that stars have different compositions and that the most abundant elements are the lightest ones. Iron is the heaviest element in stars since the nucleosynthesis of iron absorbs heat and causes the collapse of the red giant and a supernova, thus preventing larger nuclei from forming. Supernovas provide for the synthesis of heavier elements because the extremely high temperature of the supernova makes the atomic collisions 2 / 4

Chapter 0 0-2 strong enough for the nuclei to combine.94 240 Pu , 94 electrons. The bottom number is the atomic number, found on the periodic table (number of protons). The top number is the mass number (sum of the number of protons and the number of neutrons). Since it is a neutral atom, it has 94 electrons.

0.5 Most of the hydrogen that exists today was formed within the first three minutes of the formation of the universe.

0.6 Such elements are formed in supernovas and collisions between two neutron stars.

0.7 Supernovas allow atomic nuclei to capture free neutrons.

0.8 Pu has an atomic number of 94; i.e., 94 protons. A Pu isotope that has 146 neutrons thus has atomic mass of 94 + 146 = 250. Assuming that the atom is neutral, it has the name number of electrons as protons; i.e., 94.

0.9 35

17 Cl contains 17 protons, 17 electrons, and 18 neutrons.We can discard the subscript 17 on the symbol since the 17 tells the number of protons which is information that the symbol "Cl" also provides. In addition, the number of protons equals the number of electrons in a neutral atom, so the symbol "Cl" also indicates the number of electrons. The 35 is necessary to state which isotope of chlorine is in question and therefore the number of neutrons in the atom.

0.10 2.24845 × 12 u = 26.9814 uCopper is 63.546 u 12 u = 5.2955 times as heavy as carbonAny other atom could have been used as the standard for atomic mass, for example oxygen used to be the standard, and one atomic mass unit was 1/16 the mass of oxygen, but that was before they took into account the isotopes of oxygen. Scientists needed to use one isotope of an element.(0.199 × 10.0129 u) + (0.801 × 11.0093 u) = 10.8 u (0.90483 × 19.992 u) + (0.00271 × 20.994 u)

• (0.09253 × 21.991 u) = 20.18 u

0.11 Average mass of copper: 63.546 u. Mass of

12 C = 12 u. Thus, 63.546/12 = 5.3 times as heavy.

0.12 Based on a need to avoid confusion between disciplines, hydrogen and oxygen are no longer used as the standard for the definition of the size of the atomic mass unit.Wikipedia has a brief overview: https://en.wikipedia.org/wiki/Dalton_(unit)#History. If scientists were to choose 1/2 of a C-12 atoms as the baseline measure, that would match

the data for naturally occurring water: 18 u.

0.13 (0.199 × 10.0129) u + (0.801 × 11.0093) u = 10.8110 u.

0.14 (0.90483 × 19.992) u + (0.00271 × 20.994) u + (0.09253 × 21.991) u = 20.181 u

Review Questions 0.1 This answer will be student dependent.

0.2 #2 In any sample of a pure element, all the atoms are identical in mass.#5 Atoms are indestructible.

0.3 This answer will be student dependent.

0.4 This answer will be student dependent. The cubic shape of the crystals hints that the atoms are arranged in a cubic pattern. 3 / 4

Chapter 0 0-3 0.5 This answer will be student dependent. Some answers might be the shape of salt crystals or the sharp edges of quartz.

0.6 If a reaction gives off heat, the substances must have less energy than when the reaction started.

0.7 This answer will be student dependent. Some answers might be vinegar mixing with sodium bicarbonate. The atoms would have to give off heat to lose energy.

0.8 This answer will be student dependent. An answer might be an enzyme.

0.9 (a) Hydrogen, helium, and lithium; (b) Carbon, argon, oxygen, silicon, and elements up to iron; (c) elements heavier than iron 0.10 The formation of iron causes the core of a red giant to cool and then the star collapses creating a very high density core which heats up and explodes creating a supernova.

0.11 Hydrogen 0.12 The earth's core is made of iron and nickel, they are denser than aluminum and more abundant than lead.

0.13 The different melting points, densities, and crystallization of the elements. The separation of elements and minerals is still occurring in the form of earthquakes and volcanic eruptions.

0.14 Elements that result from atomic fission of uranium include barium, iodine, caesium, xenon, and strontium. Hydrogen molecules and helium atoms move so quickly in the atmosphere that they’re lost to space more quickly than other elements.

0.15 A balance to measure mass and graduated cylinders 0.16 Conservation of mass derives from the postulate that atoms are not destroyed in normal chemical reactions. The Law of Definite Proportions derives from the notion that compound substances are always composed of the same types and numbers of atoms of the various elements in the compound.

0.17 This is the Law of Definite Proportions, which guarantees that a single pure substance is always composed of the same ratio of masses of the elements that compose it.

0.18 Protons, 1 1 p

• , +1 charge

Electron,

e

• , –1 charge

Neutron,

1 n , no charge 0.19 Nearly all of the mass is located in the nucleus, because this is the portion of the atom where the protons and the neutrons are located.

0.20 A nucleon is a subatomic particle found in the atomic nucleus. We have studied neutrons and protons.

0.21 The charge-to-mass ratio of the electron was determined b y J.J. Thomson using a cathode ray tube. Electrons were generated and passed through the tube to a detection screen. The ratio of e/m was determined by applying an electric and magnetic field, at 90° to each other, to the electrons and observing to what degree they were bend when the fields were applied.

• / 4