2. For the following two compounds between oxygen and hydrogen: 3. Tell what discoveries were made by each of the following scientists:
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1 EXTRA HOMEWORK 1A 1. When Dalton proposed that matter was composed of atoms, why was his Atomic Theory accepted? 2. For the following two compounds between oxygen and hydrogen: Mass of O Mass of H Compound A 16 grams 1 grams Compound B 16 grams 2 grams (a) Propose formulas for the two compounds assuming that each oxygen atom weighs the same as each hydrogen atom (b) Propose formulas for the two compounds assuming that each oxygen atom weighs 8 times more than each hydrogen atom (c) Propose formulas for the three compounds assuming that each oxygen atom weighs 16 times more than each hydrogen atom 3. Tell what discoveries were made by each of the following scientists: (a) J.J. Thomson (b) Lord Rutherford 4. If a model of a hydrogen atom had a diameter of 45 cm, what would have to be the diameter of the nucleus? *5. Nitrogen forms two compounds with oxygen, and their elemental proportions by mass are: Mass of N Mass of O Compound 1 14 grams 8 grams Compound 2 14 grams 16 grams Compound 3 14 grams 32 grams Assuming the atomic mass of oxygen is 16, predict the simplest formulas of these compounds assuming that (a) Nitrogen has an atomic mass of 14 (b) Nitrogen has an atomic mass of 7 (c) Nitrogen has an atomic mass of 9 1 / 3 *6. Using the masses of a proton and an electron, and the sizes of the atom and the nucleus, determine the denisity of (a) a 1 H atom (b) a 1 H nucleus
2 EXTRA HOMEWORK 1B 1. One of the primary visible emissions from helium occurs at nm. For this given wavelength of light, calculate: (a) the wavelength in meters (b) the frequency (c) the energy of a single photon in joules (d) the energy of 1 mole of photons in kilojoules 2. The energy of electromagnetic radiation needed to remove electrons from the surface of cesium atoms is 231 kj/mol. Calculate: (a) the energy of a single photon of this electromagnetic radiation in joules (b) the frequency of this electromagnetic radiation (c) the wavelength of this electromagnetic radiation, in meters (d) the wavelength of this electromagnetic radiation, in nanometers (e) identify this electromagnetic radiation as either visible light, infrared radiation, or unltraviolet radiation *3. Give the experimental evidence that supports the fact that light behaves as a wave phenomenom when traveling throught space. *4. The work function of an element is the energy required to remove an electron from the surface of the solid element. The work function for lithium is kj/mol (that is, it takes kj of energy to remove one mole of electrons from one mole of lithium atoms on the surface of lithium metal). What is the maximum wave of light that can remove an electron from an atom on the surface of lithium metal? EXTRA HOMEWORK 1C 1. What does it mean if something is quantized? 2. Draw an electronic energy diagram for a hydrogen atom, and using vertical lines show the following 3 transitions: (a) n = 5 n = 2 (b) n = 4 n = 1 (c) n = 2 n = 4 3. Calculate the de Broglie wavelength of an electron moving at 99% the speed of light. 4. What are the results of passing a beam of electrons through two slits? *5. From the Heisenberg uncertainty principle, calculate the uncertainty in position ( x) of a baseball (mass = kg) with v = m/s. (Planck s constant, h, is kgm 2 /s)
3 EXTRA HOMEWORK 1D 1. Tell whether each of the following orbital designations are allowed of forbidden based upon the Schrödinger Equation. (a) 1p (b) 3f (c) 7d (d) 6h 2. Draw a picture of each of the following orbitals. (a) 2s (b) 2p (c) 3p (d) 3d 3. Concerning the fourth energy level of a hydrogen atom, tell: (a) tell the names of each sublevel it has (b) sketch the radial probability distribution for the orbitals of each sublevel 4. Tell what each of the following designations mean. (a) n = 3 (b) n = 8 (c) 4f (d) 2s (e) 7p x (f) 5f yz 2 5. Give the maximum number of electrons in an atom that can have the following designations. (a) n = 4 (b) n = 10 (c) 6d (d) 12s (e) 5py (f) 4d xz (g) 4d z 2 6. Give the orbital notation for the following atoms: (a) C (b) O (c) P *7. Although no currently known elements contain electrons in g orbitals in the ground state, electrons in excited states can be in g orbitals. (a) give the lowest value for n for which a g sublevel exists (b) give the number of electrons that a g sublevel could hold *8. Concerning the sixth energy level of a hydrogen atom, tell: (a) tell the names of each sublevel it has (b) tell the number of orbitals the sixth energy level has
4 EXTRA HOMEWORK 1E 1. Give the electron configuration notations and the electron dot notations for the following atoms: (a) Si (b) Cr (c) Po (d) Pu 2. For the silicon atom from question 1, name and draw pictures of its occupied valence atomic orbitals. 3. Using radial probability distribution graphs, explain why the 4s sublevel fills before the 3d sublevel in the d-block elements. 4. For the following electron configuration notations of sodium, identify each as a ground state electron configuration, an excited state electron configuration, or an impossible electron configuration: (a) 1s 2 2s 2 2p 5 3s 2 (b) 1s 2 2s 2 2p 6 3d 1 (c) 1s 2 2s 2 2p 6 3s 1 (d) 1s 2 2s 2 2p 6 2d 1 5. Using the periodic table, give the number of protons, neutrons and electrons in each of the following atoms: (a) 40 Ca (b) 51 V (c) 79 Br - (d) 252 Cf 6. What is probably the most abundant isotope of thorium? *7. Why does the 2s orbital fill before the 2p orbitals in multielectron atoms? *8. Why does the 4s orbital fill before the 3d orbitals in multielectron atoms? *9. In the ground state of mercury, (a) How many electrons occupy atomic orbitals with n = 3? (b) How many electrons occupy d atomic orbitals? (c) How many electrons occupy p z atomic orbitals? (d) How many electrons have spin up? *10. Which of elements 1-36 (a) have one unpaired electron in its ground state? (b) have two unpaired ectrons in its ground state? *11. Give the electron configuration notations for the following atoms: (a) Mo (b) Ag
5 EXTRA HOMEWORK 1F 1. Indicate the isotope in each pair that is most likely to be radioactive. (a) 15 O or 16 O (b) 19 F or 20 F (c) 100 Sn or 120 Sn 2. Radioactive 110 Ag with a half-life of 24 seconds is used by forensic scientists to identify trace amounts of the element in bullet lead. How many seconds will it take for the radioactivity of a 110 Ag sample to fall to 3.125% of its original intensity? 3. The age of a rock was to be determined by 238 U dating. 238 U has a half-life of 4.5 x 10 9 years, and eventually decays into stable 206 Pb. If a sample of rock shows that 50% of its 238 U had been converted into 206 Pb, how old is the rock? 4. What is the most massive element produced by fusion in stars? *5. The equation that governs radioactive decay is: n where = n o e - (ln 2 / t 1/2)t n = the final number of radioactive atoms remaining after the decay time, t n o = the initial number of radioactive atoms t 1/2 = the half-life of the radioactive atoms t = the length of time the radioactive atoms have been decaying Radioactive tritium, 3 H, has a half-life of 12.3 years and is used as a tracer in organic chemistry reactions. How many years will it take for the radioactivity to fall to 10.0% of its original intensity?
6 EXTRA HOMEWORK 1G 1. Magnesium has the following stable isotopes: 24 Mg u 78.70% 25 Mg u 10.13% 26 Mg u 11.17% What is the value of the elemental atomic mass for magnesium calculated from these data? 2. The element indium exists in nature as two isotopes: 113 In amu 115 In amu Using the periodic table in your textbook, calculate the natural percentages of the two indium isotopes. 3. Give the mass, in grams, necessary to have one mole of atoms of each of the following elements: (a) beryllium (b) sulfur (c) nickel (d) tin 4. A sample of lead has a mass of 25.0 g. Calculate: (a) the number of moles of lead atoms. (b) the number of atoms of lead. 5. A sample of antimony contains antimony atoms. Calculate: (a) the number of moles of antimony atoms. (b) the number of grams of antimony. *6. A 13 C atom has a mass of u. What is its mass in grams? *7. A regular garden pea has a volume of about 0.5 milliliters. In contrast, the Empire State building has a volume of approximately 1 billion liters. Calculate the number of Empire State Buildings it would take to hold 1 mole of regular garden peas.
7 EXTRA HOMEWORK 1H 1. What was Mendeleev s Periodic Law, and how is it different from the modern Periodic Law. 2. What is similar about elements in the same period on the periodic table? 3. For element 120, Ubn: (a) predict its expected electron configuration notation (b) predict what other element it will most likely resemble chemically 4. Identify the atom with the largest atomic radius, and explain why: (a) Ti, Zr (b) Mn, Fe 5. Identify the atom in each pair with the largest atomic radius: (a) Si, Cl (b) Ca, Ba *6. For element 121, Ubu: (a) predict its expected electron configuration notation (b) predict what other element it will most likely resemble chemically EXTRA HOMEWORK 1I 1. Write the equations for the first, second and third ionizations of an oxygen atom. 2. Identify the atom with the greatest (most endothermic) first ionization energy, and explain why: (a) Ca, Sr (b) S, Cl (c) Be, B (d) Sb, Te 3. Elements X and Y are known to be second or third period elements on the periodic table. The first four ionization energies for elements X and Y are shown below. The units are not kj/mol. Identify elements X and Y. First Second Third Fourth Write the equations for the first, second, and third electron affinities of an oxygen atom. 5. Identify the atom with the greatest (most exothermic) first electron affinity, and explain why: (a) Rb, Cs (b) As, Se (c) Li, Be (d) Sn, Sb (e) C, Si 6. Identify the atom in each pair with (1) the greatest (most endothermic) ionization energy, and (2) the greatest (most exothermic) electron affinity: (a) Si, Cl (b) Ca, Ba *7. Identify the atom with the largest atomic radius, and explain why: (a) K, Mg (b) Co, Cd X Y
8 EXTRA HOMEWORK 1J 1. Give examples of the physical properties of metals and nonmetals. 2. Why do metals form positive ions and nonmetals form negative ions? 3. Give the most metallic element in each pair: (a) K, Ca (b) Sn, Pb 4. Give the charge of the expected ion ion for each of the following elements: (a) I (b) Rb (c) Se (d) Sr (e) As (f) In (g) Cd (h) Fe 5. Give the charges of the two ions expected for each of the following elements: (a) Tl (b) Pb (c) Bi 6. Why do the atoms of Group 1 elements form 1+ ions? 7. Why do the atoms of Group 2 elements form 2+ ions? 8. Why do atoms of the d-sublevel elements form a variety of positive ions? 9. Why do the atoms of Group 17 elements form 1- ions? 10. Why don t the atoms of Group 18 elements form ions? EXTRA 1A ANSWERS 1. Dalton s Atomic Theory explained the Law of Definite Proportion. 2. (a) HO 16, HO 8 (b) HO 2, HO (c) HO, H 2 O 3. (a) discovered the electron (b) discovered the nucleus of the atom cm or 4.5 μm *5. (a) N 2 O, NO, NO 2 (b) N 4 O, N 2 O, NO (c) N 3 O, N 3 O 2, N 3 O 4 *6. (a) 3 g/cm 3 (b) 3 x g/cm 3
9 EXTRA 1B ANSWERS 1. (a) x 10-7 m (b) x s -1 (c) x J (d) x 10 2 kj 2. (a) 3.84 x J (b) 5.79 x s -1 (c) 5.18 x 10-7 m (d) 518 nm (e) visible light *3. light passing through 2 slits produces a diffraction pattern * nm EXTRA 1C ANSWERS 1. values for a property are restricted to multiples of some small, elementary unit 2. (a) (b) (c) x m 4. a diffraction pattern is produced * x m EXTRA 1D ANSWERS 1. (a) forbidden (b) forbidden (c) allowed (d) allowed 2. (a) (b) (c) (d) (continued on next page)
10 3. (a) 4s, 4p, 4d, 4f (b) 4. (a) the 3 rd energy level of an atom (b) the 8 th energy level of an atom (c) the f sublevel in the 4 th energy level of an atom (d) the s sublevel in the 2 nd energy level of an atom, or, the s orbital in the 2 nd energy level of an atom (e) the p orbital on the x axis in the 7 th energy level of an atom (f) the f orbital in the yz 2 space in the 5 th energy level of an atom 5. (a) 32 (b) 200 (c) 10 (d) 2 (e) 2 (f) 2 (g) 2 6. (a) (b) (c) *7. (a) n = 5 (b) 18 *8. (a) 6s, 6p, 6d, 6f, 6g, 6h (b) 36
11 EXTRA BOHR ATOM ANSWERS 1. (a) x J, x J (b) the values are energy of attraction (c) x J (d) energy was released during the process (e) x 10-6 m (f) infrared radiation 2. (a) x J (b) yes, 3.78 x J > x J *3. fourth EXTRA 1E ANSWERS. 1. (a) [Ne]3s 2 3p 2. Si : (b) [Ar]4s 1 3d 5 Cr. (c) [Xe]6s 2 4f 14 5d 10 6p 4. Po :. (d) [Rn]7s 2 5f 6 Pu : 2. 3s 3p x 3p y 3. An electron in a 4s orbital has more probability inside of the inner energy level shielding than an electron in a 3d orbital, so a 4s electron will attract more strongly to the nucleus of the atom than a 3d electron, and therefore an electron in a 4s orbital is more stable than an electron in a 3d orbital 4. (a) excited (b) excited (c) ground (d) impossible 5. (a) 20 p, 20 n, 20 e (b) 23 p, 28 n, 23 e (c) 35 p, 44 n, 36 e (d) 98 p, 154 n, 98 e Th (continued on next page)
12 *7. Electrons in a 2s orbital have more probability inside the shielding of the first energy level electrons than electrons in a 2p orbital, resulting in greater attraction, and therefore a lower energy state. *8. Electrons in a 4s orbital have more probability inside the shielding of the finner energy level electrons than electrons in a 3d orbital, resulting in greater attraction, and therefore a lower energy state. *9. (a) 18 (b) 30 (c) 8 (d) 40 *9. (a) H, Li, B, F, Na, Al, Cl, K, Sc, Cu, Ga, Br (b) C, O, Si, S, Ti, Ni, Ge, Se *10. (a) [Kr]5s 1 4d 5 (b) [Kr]5s 1 4d 10 EXTRA 1F ANSWERS 1. (a) 15 O (b) 20 F (c) 100 Sn seconds x 10 9 years 4. Iron * years EXTRA 1G ANSWERS u 2. 5% 113 In, 95% 115 In 3. (a) g (b) g (c) g (d) g 4. (a) mol (b) 7.27 x atoms 5. (a) mol (b) 5.56 g * x g * billion
13 EXTRA 1H ANSWERS 1. Mendeleev - the properties of the chemical vary with their atomic masses in a systematic way. Modern - the properties of the chemical vary with their atomic numbers in a systematic way. 2. Atoms of the elements in the same period require the same number of energy levels to hold all of their electrons (they all have the same number of energy levels). 3. (a) [Uno]8s 2 (b) Ra 4. (a) Zr - The atomic radius of Zr is greater because the number of shielding energy levels is more than Ti, even though the nuclear charge is greater, so electrons in the highest occupied energy level are less attracted to the nucleus. (b) Mn The atomic radius of Mn is greater because its nuclear charge is less than that of Fe while the number of shielding energy levels remains the same, so electrons in the higheset occupied energy level are less attracted to the nucleus. 5. (a) Si (b) Ba *6. (a) [Uno]8s 2 5g 1 (b) Ac
14 EXTRA 1I ANSWERS 1. O(g) O + (g) + e - O + (g) O 2+ (g) + e - O 2+ (g) O 3+ (g) + e - 2. (a) Ca - The ionization energy of Ca is greater because the number of shielding energy levels is less than Sr, even though the nuclear charge is less, so electrons in the highest occupied energy level are more attracted to the nucleus. (b) Cl - The ionization energy of Cl is greater because its nuclear charge is greater than that of S while the number of shielding energy levels remains the same, so electrons in the higheset occupied energy level are more attracted to the nucleus. (c) Be - The removed electron in Be comes from a 2s orbital, while the removed electron in B comes from a 2p orbital. Electrons in 2s orbitals are less shielded from the nuclear charge, so they are attrached more to the nucleus. (d) Sb - The removed electron in Sb is unpaired, while the removed electron in Te is paired. Unpaired electrons experience less electron-electron repulsion, so they are attrached more to the nucleus. 3. X = Mg, Y = Be 4. O(g) + e - O - (g) O - (g) + e - O 2- (g) O 2- (g) + e - O 3- (g) 5. (a) Rb The electron affinity of Rb is greater because the number of shielding energy levels is less than Cs, even though the nuclear charge is less, so free electrons are more attracted to the nucleus. (b) Se - The electron affinity of Se is greater because its nuclear charge is greater than tht of As while the number of shielding energy levels remains the same, so free electrons are more attracted to the nucleus. (c) Li - The electron added to Li goes into a 2s orbital, while the added electron to Be goes into a 2p orbital. Electrons in 2s orbitals are less shielded from the nuclear charge, so they are attrached more to the nucleus. (d) Sn - The added electron to Sn is unpaired, while the added electron to Sb becomes paired. Unpaired electrons experience less electron-electron repulsion, so they are attrached more to the nucleus. (e) Si - In the p-block of the periodic table, adding electrons to small atoms from the second period (like C) results in large electron-electron repulsion, so their electron affinities are slightly less than atoms from the third period (like Si) 6. (a) Cl greater ionization energy, greated electron affinity (b) Ca greater ionization energy, greated electron affinity *7. (a) [Uno]8s 2 5g 1 (b) Ac
15 EXTRA 1J ANSWERS 1. metals lustrous, malleable, ductile, conductors of heat and electricity; nonmetals opposite 2. metals have low ionization energies and low electron affinities, therefore they lose electrons easily (forming positive ions) but it is difficult for them to gain electrons nonmetals have high ionization energies and high electron affinities, therefore it is difficult for them to lose electrons, but they gain electrons easily (forming negative ions) 3. (a) K (b) Pb 4. (a) 1- (b) 1+ (c) 2- (d) 2+ (e) 3- (f) 3+ (g) 2+ (h) forms more than 1 5. (a) 3+, 1+ (b) 4+, 2+ (c) 5+, Group 1 elements have one outershell electron. That electron has a low ionization energy, so it is removed easily. Further electrons are core electrons (from inner energy levels), and they have high ionization energies, so they are difficult to remove. With one electron being removed easily, those atoms form 1+ ions. Group 1 elements have low electron affinities, so they do not gain electrons. 7. Group 2 elements have two outershell electrons. Those two electrons have low ionization energies, so they are removed easily. Further electrons are core electrons (from inner energy levels), and they have high ionization energies, so they are difficult to remove. With two electrons being removed easily, those atoms form 2+ ions. Group 2 elements have low electron affinities, so they do not gain electrons. 8. For the d-sublevel elements, their outershell s electrons have low ionization energies, so they are removed easily. Their inner d electrons also have fairly low ionization energies, so they may be removed as well, forming different ions with higher positive charges. 9. Group 17 elements have one opening for an electron in their outershell electron. The electron affinity to fill that spot is high, so an electron is gained easily. Further electrons would have to go into higher energy levels, and their electron affinities would be very low, so they are difficult to gain. With one electron being gained easily, those atoms form 1- ions. Group 17 elements have high ionization energies, so they do not lose electrons. 10. Group 18 elements have high ionization energies so they do not lose electrons, and low electron affinities so they do not gain electrons.
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