Question: A chunk of ice at room temperature

> Three elements have the electron configurations 1s22s22p63s2, 1s22s22p63s23p4, and 1s22s22p63s23p64s2. The first ionization energies of these elements (not in the same order) are 0.590, 0.999, and 0.738 MJ/mol. The atomic radii are 104, 160, and 197 pm.

> Compare the ionization energies of each pair of atoms. State the atom with the larger ionization energy for each pair. Symbol of Atom with the Larger lonization Energy Pair He and Kr Na and Al Cl and I

> Compare the atomic sizes of each pair of atoms. State the larger atom for each pair. Pair Symbol for Larger Atom F and B C and N B and Al

> Give the electron configurations for the following atoms. Use the noble gas notation. Element Electron Configuration K Ве Zr Se

> Identify the following three elements. a. The ground-state electron configuration is [Kr]5s24d105p4. b. The ground-state electron configuration is [Ar]4s23d104p2. c. An excited state of this element has the electron configuration 1s22s22p43s1.

> Give the electron configurations for the following atoms. Do not use the noble gas notation. Write out the complete electron configuration. Element Electron Configuration Ca Са B H Ве

> Which of the following statements is(are) true? a. The 2s orbital in the hydrogen atom is larger than the 3s orbital also in the hydrogen atom. b. The Bohr model of the hydrogen atom has been found to be incorrect. c. The hydrogen atom has quantized e

> An excited atom can release some or all of its excess energy by emitting a(n) and thus move to a lower energy state.

> Determine the maximum number of electrons that can have each of the following designations: 2f, 2dxy, 3p, 5dyz, and 4p.

> Calculate the percent by mass of each element in the following compounds. a. ZnO b. Na2S c. Mg(OH)2 d. H2O2 e. CaH2 f. K2O

> In each of the following sets of elements, indicate which element has the smallest atomic size. a. Ba, Ca, Ra b. P, Si, Al c. Rb, Cs, K

> In each of the following sets of elements, indicate which element shows the most active chemical behavior. a. B, Al, In b. Na, Al, S c. B, C, F

> Which of the following statements about the periodic table is false? a. Elements in the same column have similar reactivities because their valence electrons tend to be located in the same types of orbitals. b. A series of ions that are isoelectronic (

> Write the shorthand valence shell electron configuration of each of the following elements, basing your answer on the element’s location on the periodic table. a. nickel, Z = 28 b. niobium, Z = 41 c. hafnium, Z = 72 d. astatine, Z = 85

> Arrange the following atoms in order of increasing size (assuming all atoms are in their ground states). a. [Kr]5s24d105p6 b. [Kr]5s24d105p1 c. [Kr]5s24d105p3

> Using the symbol of the previous noble gas to indicate core electrons, write the valence shell electron configuration for each of the following elements. a. titanium, Z = 22 b. selenium, Z = 34 c. antimony, Z = 51 d. strontium, Z = 38

> Rank the following elements in order of increasing atomic size: Ge, S, F, Rb, Mn.

> What name is given to the series of ten elements in which the electrons are filling the 3d sublevel?

> How many valence electrons does each of the following atoms have? a. nitrogen, Z = 7 b. chlorine, Z = 17 c. sodium, Z = 11 d. aluminum, Z = 13

> What does the ground state of an atom represent?

> Calculate the percent by mass of each element in the following compounds. a. HClO3 b. UF4 c. CaH2 d. Ag2S e. NaHSO3 f. MnO2

> Write the complete orbital diagram for each of the following elements, using boxes to represent orbitals and arrows to represent electrons. a. scandium, Z = 21 b. sulfur, Z = 16 c. potassium, Z = 19 d. nitrogen, Z = 7

> Write the full electron configuration (1s22s2, etc.) for each of the following elements. a. bromine, Z = 35 b. xenon, Z = 54 c. barium, Z = 56 d. selenium, Z = 34

> Element X, which has a valence shell configuration of ns2np4, was isolated in a laboratory. Which of the following statements is(are) true concerning element X? a. Element X has chemical properties similar to those of the halogens. b. Element X has six

> Based on the ground-state electron configuration of iodine, how many electrons occupy the p and d orbitals?

> How does the attractive force that the nucleus exerts on an electron change with the principal energy level of the electron?

> Light waves move through space at a speed of meters per second.

> The energy of a photon of visible light emitted by an excited atom is the energy change that takes place within the atom itself.

> An atom has a small charged core called the nucleus, with charged electrons moving in the space around the nucleus.

> The random motions of the components of an object constitute the of that object.

> Consider the reaction B2H6(g) + 3O2(g) B2O3(s) + 3H2O(g) ∆H = -2035 kJ Calculate the amount of heat released when 54.0 g of diborane is combusted.

> Using the average atomic masses given inside the front cover of this book, calculate the mass in grams of each of the following samples. a. 2.17 moles of germanium, Ge b. 4.24 mmol of lead(II) chloride (1 mmol = 1/1000 mol) c. 0.0971 mole of ammonia,

> The specific heat capacity of graphite is 0.71 J/g °C. Calculate the energy required to raise the temperature of 2.4 moles of graphite by 25.0 °C.

> Which of the following processes is(are) exothermic? a. combustion of methane (e.g., Bunsen burner) b. melting of ice c. evaporation of acetone (e.g., fingernail polish remover) d. steam condensing on a cold surface

> Calculate the enthalpy change when 5.00 g of propane is burned with excess oxygen according to the reaction C3H8(g) + 5O2(g) 3CO2(g) + 4H2O(l) ∆H = -2221 kJ/mol

> Calculate ∆E for each of the following. a. q = -47 kJ, w = +88 kJ b. q = +82 kJ, w = +47 kJ c. q = +47 kJ, w = 0 d. In which of these cases do the surroundings do work on the system?

> A system releases 213 kJ of heat and has a calculated ∆E of -45 kJ. How much work was done on the system?

> If 7.24 kJ of heat is applied to a 952-g block of metal, the temperature increases by 10.7 °C. Calculate the specific heat capacity of the metal in J/g °C.

> If 10. J of heat is applied to 5.0-g samples of each of the substances listed in Table 10.1, which substance’s temperature will increase the most? Which substance’s temperature will increase the least?

> Calculate the amount of energy required (in joules) to heat 2.5 kg of water from 18.5 °C to 55.0 °C.

> The specific heat capacity of gold is 0.13 J/g °C. Calculate the specific heat capacity of gold in cal/g °C.

> What quantity of heat energy would have to be applied to a 25.1-g block of iron in order to raise the temperature of the iron sample by 17.5 °C? (See Table 10.1.) Table 10.1 The Specific Heat Capacities of Some Common Substances Specific

> Using the average atomic masses given inside the front cover of this book, calculate the number of moles of each substance contained in the following masses. a. 2.01 * 10-2 g of silver b. 45.2 mg of ammonium sulfide c. 61.7 µg of uranium d. 5.23 kg o

> Students often confuse what is meant by heat and temperature. Define each. How are the two concepts related?

> It takes 1.25 kJ of energy to heat a certain sample of pure silver from 12.0 °C to 15.2 °C. Calculate the mass of the sample of silver.

> Calculate the amount of energy required (in calories) to heat 145 g of water from 22.3 °C to 75.0 °C.

> Perform the indicated conversions. a. 85.21 cal into joules b. 672.1 J into calories c. 8.921 kJ into joules d. 556.3 cal into kilojoules

> Which of the following statements is(are) true? a. Energy is changed in form in a process, but it is not produced or consumed. b. Heat is a flow of energy between two objects due to a temperature difference in the two objects. c. In an exothermic reac

> Which of the following is an endothermic process? a. combustion of gasoline in a car engine b. sublimation of carbon dioxide; CO2(s) CO2(g) c. water condensing on a cold pipe d. freezing juice to make popsicles

> What do we mean by entropy? Why does the entropy of the universe increase during a spontaneous process?

> Does a double-displacement reaction such as NaCl(aq) + AgNO3(aq) AgCl(s) + NaNO3(aq) result in a matter spread or in a concentration of matter?

> If a reaction occurs readily but has an endothermic heat of reaction, what must be the driving force for the reaction?

> Calculate the number of moles of sulfur atoms present in each of the following samples. a. 2.01 g of sodium sulfate b. 2.01 g of sodium sulfite c. 2.01 g of sodium sulfide d. 2.01 g of sodium thiosulfate, Na2S2O3

> What does it mean to say that “energy spread” and “matter spread” are driving forces in chemical reactions?

> What was tetraethyl lead used for in the petroleum industry? Why is it no longer commonly used?

> What does natural gas consist of? Where is natural gas commonly found?

> Where did the energy stored in wood, coal, petroleum, and natural gas originally come from?

> The “Chemistry in Focus” segment Burning Calories discusses calories in food. If a food is said to contain 350 calories per serving, determine this value in terms of joules.

> The total energy of the universe is .

> The enthalpy change for a reaction that occurs at constant pressure is (higher than/lower than/the same as) the heat for that reaction.

> In the “Chemistry in Focus” segment Firewalking: Magic or Science?, it is claimed that one reason people can walk on hot coals is that human tissue is mainly composed of water. Because of this, a large amount of heat must be transferred from the coals to

> The “Chemistry in Focus” segment Coffee: Hot and Quick(lime) discusses self-heating cups of coffee using the chemical reaction between quicklime, CaO(s), and water. Is this reaction endothermic or exothermic?

> What quantity of heat is required to raise the temperature of 55.5 g of gold from 20 8C to 45 8C? (See Table 10.1.) Table 10.1 The Specific Heat Capacities of Some Common Substances Specific Heat Capacity (Jig °C) Substance water (/)* (liquid) 4.184

> Calculate the number of moles of carbon atoms present in each of the following samples. a. 1.271 g of ethanol, C2H5OH b. 3.982 g of 1,4-dichlorobenzene, C6H4Cl2 c. 0.4438 g of carbon suboxide, C3O2 d. 2.910 g of methylene chloride, CH2Cl2

> If 100. J of heat energy is applied to a 25-g sample of mercury, by how many degrees will the temperature of the sample of mercury increase? (See Table 10.1.) Table 10.1 The Specific Heat Capacities of Some Common Substances Specific Heat Capacity (

> If 125 J of heat energy is applied to a block of silver weighing 29.3 g, by how many degrees will the temperature of the silver increase? (See Table 10.1.) Table 10.1 The Specific Heat Capacities of Some Common Substances Specific Heat Capacity (Jig

> What quantity of heat energy must have been applied to a block of aluminum weighing 42.7 g if the temperature of the block of aluminum increased by 15.2 °C? (See Table 10.1.) Table 10.1 Table 10.1 The Specific Heat Capacities of Some Comm

> If 69.5 kJ of heat is applied to a 1012-g block of metal, the temperature of the metal increases by 11.4 8(C. Calculate the specific heat capacity of the metal in J/g 8(C.

> Perform the indicated conversions. a. 91.74 kcal into calories b. 1.781 kJ into calories c. 4.318 * 103 J into kilocalories d. 9.173 * 104 cal into kilojoules

> What is the kinetic energy of a particle of mass m moving through space with velocity ν?

> Perform the indicated conversions. a. 625.2 cal into kilojoules b. 82.41 kJ into joules c. 52.61 kcal into joules d. 124.2 kJ into kilocalories

> Arrange the following substances in order of increasing mass percent of nitrogen. a. NO b. N2O c. NH3 d. SNH

> The chemical formula for aspirin is C9H8O4. What is the mass percent for each element in 1 mole of aspirin? (Give your answer to four significant figures.) carbon % hydrogen % охудen %

> Convert the following numbers of kilojoules into kilocalories. (Remember: kilo means 1000.) a. 652.1 kJ b. 1.00 kJ c. 4.184 kJ d. 4.351 * 103 kJ

> Calculate the number of molecules present in each of the following samples. a. 3.54 moles of sulfur dioxide, SO2 b. 3.54 g of sulfur dioxide, SO2 c. 4.46 * 1025 g of ammonia, NH3 d. 4.46 * 1025 moles of ammonia, NH3 e. 1.96 mg of ethane, C2H6

> How are the different types of electromagnetic radiation similar? How do they differ?

> a. How many atoms of carbon are present in 1.0 g of CH4O? b. How many atoms of carbon are present in 1.0 g of CH3CH2OH? c. How many atoms of nitrogen are present in 25.0 g of CO(NH2)2?

> Calculate the number of moles for each compound in the following table. Compound Mass Moles Magnesium phosphate 326.4 g Calcium nitrate 303.0 g Potassium chromate 141.6 g Dinitrogen pentoxide 406.3 g

> Convert the following numbers of calories into kilocalories. (Remember: kilo means 1000.) a. 8254 cal b. 41.5 cal c. 8.231 * 103 cal d. 752,900 cal

> Convert the following numbers of calories or kilocalories into joules and kilojoules (Remember: kilo means 1000.) a. 75.2 kcal b. 75.2 cal c. 1.41 * 103 cal d. 1.41 kcal

> If it takes 654 J of energy to warm a 5.51-g sample of water, how much energy would be required to warm 55.1 g of water by the same amount?

> If 8.40 kJ of heat is needed to raise the temperature of a sample of metal from 15 °C to 20 °C, how many kilojoules of heat will be required to raise the temperature of the same sample of metal from 25 °C to 40 °C?

> Topical hydrocortisone is often used to treat a variety of skin conditions, such as insect bites, eczema, and rashes. Each molecule of hydrocortisone contains 21 atoms of carbon (plus other atoms). The mass percentage of carbon in hydrocortisone is 69.58

> Write the conversion factors that would be necessary to perform each of the following conversions: a. an energy given in calories to its equivalent in joules b. an energy given in joules to its equivalent in calories c. an energy given in calories to

> What mass of sodium hydroxide has the same number of oxygen atoms as 100.0 g of ammonium carbonate?

> A system absorbs 215 kJ of heat, and 116 kJ of work is done on it. Calculate ∆E.

> Calculate the number of molecules present in each of the following samples. a. 4.75 mmol of phosphine, PH3 b. 4.75 g of phosphine, PH3 c. 1.25 * 10-2 g of lead(II) acetate, Pb(CH3CO2)2 d. 1.25 * 10-2 moles of lead(II) acetate, Pb(CH3CO2)2 e. a sampl

> The percent by mass of nitrogen is 46.7% for a species containing only nitrogen and oxygen. Which of the following could be this species? a. N2O5 b. N2O c. NO2 d. NO e. NO3

> What is meant by potential energy? Give an example of an object or material that possesses potential energy.

> How many anions are there in 5.00 g of calcium bromide?

> For an endothermic process, q will have a (positive/negative) sign.

> If q for a process is a positive number, then the system is (gaining/losing) energy.

> Calculate ∆E for each of the following cases. a. q = +65 kJ, w = -22 kJ b. q = +200. kJ, w = -73 kJ c. q = -18 kJ, w = -40. kJ

> The energy, E, of a system represents the sum of the kinetic and potential energies of all particles within the system.

> What do we mean by thermodynamics? What is the first law of thermodynamics?

> Consider the following unbalanced chemical equation: H2S(g) + O2(g) SO2(g) + H2O(g) Determine the maximum number of moles of SO2 produced from 8.0 moles of H2S and 3.0 moles of O2.

> Consider the following unbalanced chemical equation. LiOH(s) + CO2(g) / Li2CO3(s) + H2O(l) If 67.4 g of lithium hydroxide reacts with excess carbon dioxide, what mass of lithium carbonate will be produced?

> Calculate the mass in grams of each of the following samples. a. 0.994 mole of benzene, C6H6 b. 4.21 moles of calcium hydride c. 1.79 * 10-4 moles of hydrogen peroxide, H2O2 d. 1.22 mmol of glucose, C6H12O6 (1 mmol = 1⁄1000 mole) e. 10.6 moles of tin

> A 0.4230-g sample of impure sodium nitrate (contains sodium nitrate plus inert ingredients) was heated, converting all the sodium nitrate to 0.2339 g of sodium nitrite and oxygen gas. Determine the percent of sodium nitrate in the original sample.

> Consider the following unbalanced chemical equation for the combustion of pentane (C5H12): C5H12(l) + O2(g) CO2(g) + H2O(l) If a 20.4-gram sample of pentane is burned in excess oxygen, what mass of water can be produced, as