Question: Write the full electron configuration (1s22s2,

> The atomic mass of copper is 63.55 amu. What would be the mass of 75 copper atoms? How many copper atoms are contained in a sample of copper that has a mass of 6100.8 amu?

> What is the average atomic mass (in amu) of iron atoms? What would 299 iron atoms weigh? How many iron atoms are present in a sample of iron that has a mass of 5529.2 amu?

> Using the average atomic masses for each of the following elements (see the table inside the front cover of this book), calculate the number of atoms present in each of the following samples. a. 40.08 amu of calcium b. 919.5 amu of tungsten c. 549.4 a

> What do the coefficients of a balanced chemical equation tell us about the proportions in which atoms and molecules react on an individual (microscopic) basis?

> What do we mean by the average atomic mass of an element? What is “averaged” to arrive at this number?

> How many valence electrons does each of the following atoms have? a. titanium, Z = 22 b. iodine, Z = 53 c. radium, Z = 88 d. manganese, Z = 25

> Write the general valence configuration (for example, ns1 for Group 1) for the group in which each of the following elements is found. a. barium, Z = 56 b. bromine, Z = 35 c. tellurium, Z = 52 d. potassium, Z = 19 e. sulfur, Z = 16

> The current model of the atom in which essentially all of an atom’s mass is contained in a very small nucleus, whereas most of an atom’s volume is due to the space in which the atom’s electrons move, was established by a. Millikan’s oil-drop experiment.

> Give the name and calculate the molar mass for each of the following substances. a. H3PO4 b. Fe2O3 c. NaClO4 d. PbCl2 e. HBr f. Al(OH)3

> The of electromagnetic radiation represents the number of waves passing a given point in space each second.

> Electrons found in the outermost principal energy level of an atom are referred to as electrons.

> Which of the following statements is false concerning orbitals? a. An orbital is a region of space where an electron might be found with 90% probability. b. As an electron absorbs more energy, the orbital in which it might be found becomes larger and/o

> When lithium salts are heated in a flame, they emit red light. When copper salts are heated in a flame in the same manner, they emit green light. Why do we know that lithium salts will never emit green light, and copper salts will never emit red light?

> According to Bohr, the electron in the hydrogen atom moved around the nucleus in circular paths called .

> The energy levels of hydrogen (and other atoms) are , which means that only certain values of energy are allowed.

> The lowest possible energy state of an atom is called the state.

> A beam of light can be thought of as consisting of a stream of light particles called .

> The portion of the electromagnetic spectrum between wavelengths of approximately 400 and 700 nanometers is called the region.

> The speed at which electromagnetic radiation moves through a vacuum is called the .

> Using the average atomic masses given inside the front cover of this book, calculate how many moles of each substance the following masses represent. a. 4.15 g of silicon, Si b. 2.72 mg of gold(III) chloride, AuCl3 c. 1.05 kg of sulfur, S d. 0.000901

> Consider the bright line spectrum of hydrogen shown in Fig. 11.10. Which line in the spectrum represents photons with the highest energy? With the lowest energy? Figure 11.10 when excited hydrogen atoms return to lower energy states, they

> In each of the following sets of elements, indicate which element has the smallest atomic size. a. Na, K, Rb b. Na, Si, S c. N, P, As d. N, O, F

> In each of the following sets of elements, which element would be expected to have the highest ionization energy? a. Cs, K, Li b. Ba, Sr, Ca c. I, Br, Cl d. Mg, Si, S

> What are the metalloids? Where are the metalloids found on the periodic table?

> Why do the metallic elements of a given period (horizontal row) typically have much lower ionization energies than do the nonmetallic elements of the same period?

> Which elements in a given period (horizontal row) of the periodic table lose electrons most easily? Why?

> Which of the following elements most easily gives up electrons during reactions: Li, K, or Cs? Explain your choice.

> Give some similarities that exist among the elements of Group 7.

> What types of ions do the metals and the nonmetallic elements form? Do the metals lose or gain electrons in doing this? Do the nonmetallic elements gain or lose electrons in doing this?

> The “Chemistry in Focus” segment Light as a Sex Attractant discusses fluorescence. In fluorescence, ultraviolet radiation is absorbed and intense white visible light is emitted. Is ultraviolet radiation a higher or a lower energy radiation than visible l

> For each of the following unbalanced equations, calculate how many grams of each product would be produced by complete reaction of 12.5 g of the reactant indicated in boldface. Indicate clearly the mole ratio used for the conversion. a. TiBr4(g) + H2(g)

> The “Chemistry in Focus” segment The Chemistry of Bohrium discusses element 107, bohrium (Bh). What is the expected electron configuration of Bh?

> Write the valence shell electron configuration of each of the following elements, basing your answer on the element’s location on the periodic table. a. rubidium, Z = 37 b. barium, Z = 56 c. titanium, Z = 22 d. germanium, Z = 32

> Write the valence-electron configuration of each of the following elements, basing your answer on the element’s location on the periodic table. a. uranium, Z = 92 b. manganese, Z = 25 c. mercury, Z = 80 d. francium, Z = 87

> For each of the following elements, indicate which set of orbitals is filled last. a. radium, Z = 88 b. iodine, Z = 53 c. gold, Z = 79 d. lead, Z = 82

> Based on the elements’ locations on the periodic table, how many 4d electrons would be predicted for each of the following elements? a. ruthenium, Z = 44 b. palladium, Z = 46 c. tin, Z = 50 d. iron, Z = 26

> How many 3d electrons are found in each of the following elements? a. nickel, Z = 28 b. vanadium, Z = 23 c. manganese, Z = 25 d. iron, Z = 26

> How many valence electrons does each of the following atoms have? a. rubidium, Z = 37 b. arsenic, Z = 33 c. aluminum, Z = 13 d. nickel, Z = 28

> Using the symbol of the previous noble gas to indicate the core electrons, write the electron configuration for each of the following elements. a. scandium, Z = 21 b. yttrium, Z = 39 c. lanthanum, Z = 57 d. actinium, Z = 89

> To which element does each of the following abbreviated electron configurations refer? a. [Ne]3s23p1 b. [Ar]4s1 c. [Ar]4s23d104p5 d. [Kr]5s24d105p2

> What do we mean by the frequency of electromagnetic radiation? Is the frequency the same as the speed of the electromagnetic radiation?

> Using the average atomic masses given inside the front cover of this book, calculate the indicated quantities. a. the mass in grams of 125 iron atoms b. the mass in amu of 125 iron atoms c. the number of moles of iron atoms in 125 g of iron d. the ma

> Using the symbol of the previous noble gas to indicate the core electrons, write the electron configuration for each of the following elements. a. arsenic, Z = 33 b. titanium, Z = 22 c. strontium, Z = 38 d. chlorine, Z = 17

> Would you expect the valence electrons of rubidium and strontium to reside in the 5s or the 4d orbitals? Why?

> Why do we believe that the valence electrons of calcium and potassium reside in the 4s orbital rather than in the 3d orbital?

> For each of the following, give an atom and its complete electron configuration that would be expected to have the indicated number of valence electrons. a. two b. four c. six d. eight

> The “Chemistry in Focus” segment A Magnetic Moment discusses the ability to levitate a frog in a magnetic field because electrons, when sensing a strong magnetic field, respond by opposing it. This is called diamagnetism. Atoms that are diamagnetic have

> Write the complete orbital diagram for each of the following elements, using boxes to represent orbitals and arrows to represent electrons. a. aluminum, Z = 13 b. phosphorus, Z = 15 c. bromine, Z = 35 d. argon, Z = 18

> To which element does each of the following electron configurations correspond? a. 1s22s22p63s23p64s23d104p4 b. 1s22s22p63s23p64s23d1 c. 1s22s22p63s23p4 d. 1s22s22p63s23p64s23d104p65s24d105p5

> To which element does each of the following electron configurations correspond? a. 1s22s22p63s23p2 b. 1s22s2 c. 1s22s22p6 d. 1s22s22p63s23p6

> What does the wavelength of electromagnetic radiation represent? How is the wavelength of radiation related to the energy of the photons of the radiation?

> Using the average atomic masses given inside the front cover of this book, calculate the number of atoms present in each of the following samples. a. 1.50 g of silver, Ag b. 0.0015 mole of copper, Cu c. 0.0015 g of copper, Cu d. 2.00 kg of magnesium,

> Write the full electron configuration (1s22s2, etc.) for each of the following elements. a. magnesium, Z = 12 b. lithium, Z = 3 c. oxygen, Z = 8 d. sulfur, Z = 16

> How are the electron arrangements in a given group (vertical column) of the periodic table related? How is this relationship manifested in the properties of the elements in the given group?

> When a hydrogen atom is in its ground state, in which orbital is its electron found? Why?

> Which orbital is the first to be filled in any atom? Why?

> Which of the following orbital designations is(are) not possible? a. 3f b. 5s c. 4d d. 1p

> Which of the following orbital designations is(are) possible? a. 1s b. 2p c. 2d d. 4f

> According to the Pauli exclusion principle, the electrons within a given orbital must have spins.

> According to the Pauli exclusion principle, a given orbital can contain only electrons.

> The number of sublevels in a principal energy level (increases/ decreases) as n increases.

> How does the energy of a principal energy level depend on the value of n? Does a higher value of n mean a higher or lower energy?

> Use the average atomic masses given inside the front cover of this book to calculate the mass in grams of each of the following samples. a. 0.00552 mole of calcium b. 6.25 mmol of boron (1 mmol = 1⁄1000 mole) c. 135 moles of aluminum d. 1.34 * 10-7 m

> Why can only two electrons occupy a particular orbital? What is this idea called?

> When describing the electrons in an orbital, we use arrows pointing upward and downward / to indicate what property?

> Why do we believe that the three electrons in the 2p sublevel of nitrogen occupy different orbitals?

> Answer each of the following questions. Be thorough in your answers, and provide complete support. a. Write the ground-state electron configuration for oxygen. b. Draw the orbital diagram for the ground state of oxygen. Justify your placement of elect

> Which of the following statements is(are) true regarding the atom? a. Negatively charged particles are embedded in a positively charged cloud throughout the atom. b. As verified by Rutherford, only positively charged particles called protons are found

> In the text (Section 11.6) it was mentioned that current theories of atomic structure suggest that all matter and all energy demonstrate both particle-like and wave-like properties under the appropriate conditions, although the wave-like nature of matter

> Without referring to your textbook or a periodic table, write the full electron configuration, the orbital box diagram, and the noble gas shorthand configuration for the elements with the following atomic numbers. a. Z = 21 b. Z = 15 c. Z = 36 d. Z = 3

> Without referring to your textbook or a periodic table, write the full electron configuration, the orbital box diagram, and the noble gas shorthand configuration for the elements with the following atomic numbers. a. Z = 19 b. Z = 22 c. Z = 14 d. Z =

> One bit of evidence that the present theory of atomic structure is “correct” lies in the magnetic properties of matter. Atoms with unpaired electrons are attracted by magnetic fields and thus are said to exhibit paramagnetism. The degree to which this ef

> An unknown element is a nonmetal and has a valence-electron configuration of ns2np4. a. How many valence electrons does this element have? b. Possible identities for this element include which of the following? Cl, S, Pb, Se, Cr

> Use the average atomic masses given inside the front cover of this book to calculate the mass in grams of each of the following samples. a. 0.251 mole of lithium b. 1.51 moles of aluminum c. 8.75 * 10-2 moles of lead d. 125 moles of chromium e. 4.25

> Arrange the following sets of elements in order of increasing atomic size. a. Sn, Xe, Rb, Sr b. Rn, He, Xe, Kr c. Pb, Ba, Cs, At

> In each of the following groups, which element is least reactive? a. Group 1 b. Group 7 c. Group 2 d. Group 6

> The “Chemistry in Focus” segment Fireworks discusses some of the chemicals that give rise to the colors of fireworks. How do these colors support the existence of quantized energy levels in atoms?

> Where are the most nonmetallic elements located on the periodic table? Why do these elements pull electrons from metallic elements so effectively during a reaction?

> Give some similarities that exist among the elements of Group 1.

> What are some of the physical properties that distinguish the metallic elements from the nonmetals? Are these properties absolute, or do some nonmetallic elements exhibit some metallic properties (and vice versa)?

> Write the complete orbital diagram for each of the following elements, using boxes to represent orbitals and arrows to represent electrons. a. helium, Z = 2 b. neon, Z = 10 c. krypton, Z = 36 d. xenon, Z = 54

> Where are the valence electrons found in an atom, and why are these particular electrons most important to the chemical properties of the atom?

> Although a hydrogen atom has only one electron, the hydrogen atom possesses a complete set of available orbitals. What purpose do these additional orbitals serve?

> What overall shape do the 2p and 3p orbitals have? How do the 2p orbitals differ from the 3p orbitals? How are they similar?

> Use the average atomic masses given inside the front cover of this book to calculate the number of moles of the element present in each of the following samples. a. 49.2 g of sulfur b. 7.44 * 104 kg of lead c. 3.27 mg of chlorine d. 4.01 g of lithium

> The “Chemistry in Focus” segment Plastic That Talks and Listens! discusses polyvinylidene difluoride (PVDF). What is the empirical formula of PVDF? Note: An empirical formula is the simplest whole-number ratio of atoms in a compound. This is discussed mo

> Your text describes the probability map for an s orbital using an analogy to the earth’s atmosphere. Explain this analogy.

> Section 11.6 uses a “firefly” analogy to illustrate how the wave mechanical model for the atom differs from Bohr’s model. Explain this analogy.

> What major assumption (that was analogous to what had already been demonstrated for electromagnetic radiation) did de Broglie and Schrödinger make about the motion of tiny particles?

> How does the Bohr theory account for the observed phenomenon of the emission of discrete wavelengths of light by excited atoms?

> What does it mean to say that the hydrogen atom has discrete energy levels? How is this fact reflected in the radiation that excited hydrogen atoms emit?

> Describe briefly why the study of electromagnetic radiation has been important to our understanding of the arrangement of electrons in atoms.

> The “Chemistry in Focus” segment Atmospheric Effects discusses the greenhouse effect. How do the greenhouse gases CO2, H2O, and CH4 have an effect on the temperature of the atmosphere?

> Calculate ∆H for the reaction N2H4(l) + O2(g) N2(g) + 2H2O(l) given the following data: Equation ΔH (kI) 2NH3(g) + 3N,0(g) 4N2(g) + 3H,0(/) - 1010 N,0(g) + 3H2(g) → N2Hạ(/) + H20(1) 2NH3(g) + }02(g)→ N2Ha(/

> A swimming pool, 10.0 m by 4.0 m, is filled with water to a depth of 3.0 m at a temperature of 20.2 °C. How much energy is required to raise the temperature of the water to 24.6 °C?

> Which of the following reactions is/are endothermic? a. CO2(s) CO2(g) b. NH3(g) NH3(l) c. 2H2(g) + O2(g) 2H2O(g) d. H2O(l) H2O(s) e. Cl2(g) 2Cl(g)

> Use the average atomic masses given inside the front cover of this book to calculate the number of moles of the element present in each of the following samples. a. 4.95 g of neon b. 72.5 g of nickel c. 115 mg of silver d. 6.22 µg of uranium (µ is a

> It has been determined that the body can generate 5500 kJ of energy during one hour of strenuous exercise. Perspiration is the body’s mechanism for eliminating this heat. How many grams and how many liters of water would have to be evaporated through per

> Consider the following equations: 3A + 6B 3D ∆H = -403 kJ/mol E + 2F A ∆H = -105.2 kJ/mol C E + 3D ∆H = +64.8 kJ/mol Suppose the first equation is reversed and multiplied by 1/6 , the second and third equati

> The overall reaction in commercial heat packs can be represented as 4Fe(s) + 3O2(g) 2Fe2O3(s) ∆H = -1652 kJ a. How much heat is released when 4.00 moles of iron is reacted with excess O2? b. How much heat is released when 1.00 mole