What are the metalloids? Where are the metalloids found on the periodic table?
> Write the formula and calculate the molar mass for each of the following substances. a. carbon dioxide b. aluminum phosphate c. iron(III) carbonate d. lead(II) nitrate e. strontium chloride
> Define the amu. What is one amu equivalent to in grams?
> If baking soda (sodium hydrogen carbonate) is heated strongly, the following reaction occurs: 2NaHCO3(s) Na2CO3(s) + H2O(g) + CO2(g) Calculate the mass of sodium carbonate that will remain if a 1.52-g sample of sodium hydrogen carbon
> Boron nitride reacts with iodine monofluoride in trichlorofluoromethane at 230°C to produce pure nitrogen triiodide and by-product (BF3). BN + 3IF NI3 + BF3 a. What mass of iodine monofluoride must be used to produce 30.0 g of nitrogen tr
> Calcium carbide, CaC2, can be produced in an electric furnace by strongly heating calcium oxide (lime) with carbon. The unbalanced equation is CaO(s) + C(s) CaC2(s) + CO(g) Calcium carbide is useful because it reacts readily with water
> “Smelling salts,” which are used to revive someone who has fainted, typically contain ammonium carbonate, (NH4)2CO3. Ammonium carbonate decomposes readily to form ammonia, carbon dioxide, and water. The strong odor of the ammonia usually restores conscio
> Describe in your own words how the molar mass of the compound below may be calculated. 1 CH4 molecule
> The of a substance is the mass (in grams) of 1 mole of the substance.
> Consider the reaction represented by the chemical equation C(s) + O2(g) CO2(g) Because the coefficients of the balanced chemical equation are all equal to 1, we know that exactly 1 g of C will react with exactly 1 g of O2. True or
> Which of the following statements is true for the reaction of nitrogen gas with hydrogen gas to produce ammonia (NH3)? Choose the best answer. a. Subscripts can be changed to balance this equation, just as they can be changed to balance the charges when
> Although mass is a property of matter we can conveniently measure in the laboratory, the coefficients of a balanced chemical equation are not directly interpreted on the basis of mass. Explain why.
> The vigorous reaction between aluminum and iodine gives the balanced equation: 2Al(s) + 3I2(s) 2AlI3(s). What do the coefficients in this balanced chemical equation tell us about the proportions in which these substances react on a macroscop
> Write the formula and calculate the molar mass for each of the following substances. a. barium chloride b. aluminum nitrate c. iron(II) chloride d. sulfur dioxide e. calcium acetate
> What does it mean to say that the balanced chemical equation for a reaction describes the stoichiometry of the reaction?
> What quantity serves as the conversion factor between the mass of a sample and how many moles the sample contains?
> Which weighs less, 0.25 mole of xenon atoms or 2.0 moles of carbon atoms?
> Which has the smaller mass, 1 mole of He atoms or 4 moles of H atoms?
> If an average fluorine atom has a mass of 3.16 * 10-23 g, what is the average mass of a chlorine atom in grams?
> If an average sodium atom has a mass of 3.82 * 10-23 g, what is the mass of a magnesium atom in grams?
> What mass of cobalt contains the same number of atoms as 57.0 g of fluorine?
> What mass of hydrogen contains the same number of atoms as 7.00 g of nitrogen?
> Consider a sample of silver weighing 300.0 g. How many atoms of silver are present in the sample? What mass of copper would you need for the copper sample to contain the same number of atoms as the silver sample?
> Suppose you have a sample of sodium weighing 11.50 g. How many atoms of sodium are present in the sample? What mass of potassium would you need to have the same number of potassium atoms as there are sodium atoms in the sample of sodium?
> Give the name and calculate the molar mass for each of the following substances. a. KHCO3 b. Hg2Cl2 c. H2O2 d. BeCl2 e. Al2(SO4)3 f. KClO3
> There are 6.022 * 1023 zinc atoms present in g of zinc.
> There are iron atoms present in 55.85 g of iron.
> 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
> 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
> Write the full electron configuration (1s22s2, etc.) for each of the following elements. a. phosphorus, Z = 15 b. calcium, Z = 20 c. potassium, Z = 19 d. boron, Z = 5
> 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
