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- Title: 1301Review1
- Type: Notes
- School: U. Houston
- Course: CHEM 1301
- Term: Fall
TEST 1301 1 REVIEW SHEET You need to read chapters 1 through 4 All is fair game unless I announce otherwise on Wednesday before the test. Introductory Stuff Scientific Method Atoms and Molecules; Dalton s Theory 1. (A) 2. (A) (C) 3. Know history, types of matter Know terms elements and compounds know the definitions. Understand formulas Know the parts of it and the laws it explained Which of the following is an example of heterogeneous matter? Coffee (B) Diamond (C) Wood (D) Air Which of the following is an example of homogeneous matter? Seawater (assume no particulates) Earth's atmosphere (assume no particulates) (B) (D) Bronze (an alloy of copper and tin) All of the above are homogeneous mixtures Which of the following Greek philosophers developed a theory of matter based upon small, but indivisible, pieces? Socrates (B) Democritus (C) Aristotle (D) Plato (A) 4. Which assumption of Dalton s atomic theory had to be revised or discarded because of the existence of stable isotopes? The ultimate particles of matter are the atoms of elements, which are indivisible and indestructible. All the atoms of a given element are alike in all respects. The atoms of different elements differ in one or more properties. Compounds are formed by combination of different kinds of atoms. Which of the following is a pure, elemental substance? Br2 (B) SO2 (C) H2O (D) H2O2 (A) (B) (C) (D) 5. (A) Structure of an atom: Protons, neutrons and electrons: protons same as atomic number (from Periodic Table) Electrons same as protons in neutral atom Mass (written in top left hand corner) protons + neutrons Isotopes Protons and Neutrons in nucleus (Rutherford s expt.) Electrons round outside General structure: 6. The first scientist to propose that the atom had a dense nucleus which occupied only a small fraction of the volume of the atom was Heisenberg (B) Bohr. (C) De Broglie (D) Rutherford. (A) 1 7. When alpha particles were shot at a gold foil target, most of the particles were undeflected. This indicated to Rutherford that the gold foil was continuous matter. (B) the mass of the gold atoms was spread out thinly. the atoms of gold were mostly empty space. (D) the alpha particles had great penetrating power. the alpha particles had charges opposite to those on the nuclei According to the experiments of Ernest Rutherford, where can a majority of a given atom's mass be found? Scattered randomly throughout an approximately cube-shaped atom At the center of an approximately spherical atom In concentric layers of spherical shape As small pieces orbiting a common center in circular paths The structure of individual atoms can roughly be described as: A massive, positively charged center and mostly empty space An even mixture of mass and charge scattered throughout a spherical shape Positively charged, low-mass pieces in orbit around a massive, negatively charged center Massive, positively charged pieces in orbit around a low-mass, negatively charged center The number of neutrons in the nucleus of a specific atom is equal to its (B) mass number. (C) atomic number. (D) mass number - atomic number. (A) (C) (E) 8. (A) (B) (C) (D) 9. (A) (B) (C) (D) 10. (A) atomic mass. 11. (A) (B) 12. (A) (B) (C) (D) 13. (A) (B) (C) (D) 14. (A) (B) (C) (D) In all neutral atoms, there are equal numbers of protons and neutrons. positrons and electrons. (C) (D) neutrons and electrons. electrons and protons. Which statement concerning the structure of the atom is correct? Protons and neutrons have most of the mass and occupy most of the volume of the atom. Electrons have most of the mass and occupy most of the volume of the atom. Electrons have most of the mass but occupy very little of the volume of the atom. Protons and neutrons have most of the mass but occupy very little of the volume of the atom. Which statement is true? The nucleus of an atom contains neutrons and electrons. The atomic number of an element is the number of protons in one atom. The mass number of an atom is the number of protons in the nucleus plus the number of electrons. The number of electrons outside the nucleus is the same as the number of neutrons in the nucleus. How is the term "mass number" defined for a given atom or isotope? As the mass of one mole of that element or isotope As the sum of the protons, neutrons, and electrons it contains As the sum of the protons and neutrons its nucleus contains As the number of protons its nucleus contains 2 15. (A) 16. How many neutrons does the nucleus of the phosphorus-32 isotope have? 15 (B) 16 (C) 17 (D) 32 An atom of strontium 90 (90Sr) contains (B) 38 electrons, 38 protons, 90 neutrons. (D) 52 electrons, 38 protons, 38 neutrons. (A) 38 electrons, 38 protons, 52 neutrons. (C) 52 electrons, 52 protons, 38 neutrons. 17. Select the answer that lists the correct atomic number, number of neutrons and mass number for 80Br (B) 80, 46, 35 (C) 35, 45, 80 (D) 35, 80, 45 (E) 35, 46, 81 (A) 45, 80, 35 18. (A) 19. (A) (D) 12 3 The species 1H, 1H, and 1H represent three allotropes. (B) isomers. (C) homologs. (D) isotopes. Elemental tin has several isotopes. All of them have the same: number of protons number of neutrons (B) (E) total number of neutrons and protons total number of neutrons and electrons (C) mass number Periodic Table Atom types arranged by order of atomic number Things in groups have similar properties Mass is weighted related mass = [(mass of isotope 1 x % of 1) + (mass of 2 x % of 2) ] /100 Know first 36 names/symbols. Know special groups: 1st = alkali metals (e. g. Na) last = noble gases (e. g. He) 4th to last = pnictogens (e. g. N) 20. (A) 21. (A) 22. (A) 23. (A) 2nd = alkaline earth metals (e. g. Mg) 2nd to last = halogens (e. g. Cl) middle block = transition metals 3rd to last = chalcogens (e. g. O) What is the name given to the element with the symbol "P"? Polonium (B) Protactinium (C) Phosphorus (D) Palladium What is the name of the element whose symbol is "Co" ? Carbon (B) Chromium (C) Coal (D) Cobalt By what chemical symbol do we know the element chromium? Cr (B) Co (C) C (D) Cs What chemical symbol has been given to the element sodium? S (B) K (C) Na (D) Sr 3 24. (A) 25. (A) 26. (A) 27. (A) 28. (A) 29. (A) 30. (A) 31. Which of the following elements are largely unreactive substances? alkali metals (B) noble gases (C) halogens (D) alkaline earth metals Which of the following is a non-metal? lithium (B) bromine (C) mercury, Hg (D) bismuth, Bi Which of the following is a metal? nitrogen (B) phosphorus (C) arsenic (D) thallium, Tl Which of the following is a metalloid? carbon (B) sulfur (C) germanium (D) iridium, Ir A column of the periodic table is called a group (B) period (C) isotopic mixture (D) pillar A row of the periodic table is called a group (B) period (C) isotopic mixture (D) family What name is commonly given to the elements of Group IA of the periodic table? Alkaline earth metals (B) Transition metals (C) halogens (D) Alkali metals Lithium forms compounds which are used in dry cells and storage batteries and in high-temperature lubricants. It has two naturally occurring isotopes, 6Li (isotopic mass = 6.015121 amu) and 7Li (isotopic mass = 7.016003 amu). Lithium has an atomic mass of 6.9409 amu. What is the percent abundance of lithium-6? 86.66% (B) 46.16% (C) 7.503% (D) 6.080% (A) 32. Silicon, which makes up about 25% of Earth s crust by mass, is used widely in the modern electronics industry. It has three naturally occurring isotopes, 28Si, 29Si, and 30Si. Calculate the atomic mass of silicon. Isotope 28 Si 29 Si 30 Si Isotopic Mass (amu) 27.976927 28.976495 29.973770 (B) Abundance % 92.23 3.10 4.67 (C) 28.7260 amu (D) 28.0855 amu (A) 29.2252 amu 28.9757 amu Stuff about light: 33 (A) (C) Select the arrangement of electromagnetic radiation which goes from lowest energy to greatest energy. radio, visible, infrared, ultraviolet visible, ultraviolet, infrared, gamma rays (B) (D) microwave, infrared, visible, ultraviolet X-radiation, visible, infrared, microwave 4 34. (A) (C) 35. Select the arrangement of electromagnetic radiation which goes from lowest to highest wavelength radio, infrared, ultraviolet, gamma rays gamma rays, infrared, radio, ultraviolet (B) (D) radio, ultraviolet, infrared, gamma rays gamma rays, ultraviolet, infrared, radio Calculate the energy in joules of microwave radiation of wavelength 12.7 centimeters (h = 6.63 x 10-34 J sec; speed of light = 3 x 108 meters/sec.) 4.87 x 1019 J (B) 7.30 x 10-19 J (C) 3.61 x 10-18 J (D) 1.56 x 10-24 J (A) Bohr Model for the Atom Atomic Spectra only lines Specific Energies Quantized energy levels, explained by ORBITS. THINK OF ORBITS AS SHELLS with a maximum number of electrons = 2n2 Quantum Electrons considered waves or particles. DE BROGLIE. Heisenberg can t know position and energy/velocity etc ORBITALS where electrons probably are Defined by SHELLS SUBSHELLS s p d f 36. (A) 37. (A) 38. contain contain contain contain 1 s orbital 3 p orbitals 5 d orbitals 7 f orbitals spherical dumbbell shape 4-leaf clover shape double 4-leaf clover shape smallest = 1s smallest = 2p smallest = 3d smallest = 4f split into n SUBSHELLS which split into ORBITALS The scientist who was first to propose that electrons in an atom could have only certain energies was Heisenberg (B) Bohr. (C) De Broglie (D) Rutherford. The concept that particles of matter could have wave properties was proposed by Heisenberg (B) Bohr. (C) De Broglie (D) Rutherford. The principle which states that one cannot know the exact position and velocity of a particle simultaneously was proposed by Heisenberg (B) Bohr. (C) De Broglie (D) Rutherford. (A) 39. (A) (B) (C) (D) Atomic orbitals developed using quantum mechanics describe regions of space in which one is most likely to find an electron describe exact paths for electron motion give a description of the atomic structure which is essentially the same as the Bohr model allow scientists to calculate an exact volume for the hydrogen atom 5 40. (A) (B) (C) (D) 41. (A) (B) (C) (D) 42. (A) 43. (A) 44. What is the main difference between "classical physics" and "quantum physics"? Quantum physics requires the speed of light to be a constant value. Classical physics requires that only certain, allowed values for energy be used. Quantum physics requires that only certain, allowed values for energy be used. Quantum physics can only describe the behavior of very small objects, like atoms and molecules. Which feature of Bohr's atomic model is no longer accepted as true by today's scientists? That most of an atom's mass is located within the nucleus That electrons have only certain, allowed energy values That electrons orbit the nucleus in circular paths That each principal quantum level can hold a maximum of 2n2 electrons The orbitals of 2p electrons are often represented as being elliptical. (B) tetrahedral. (C) spherical. (D) dumbbell shaped How many electrons can be "stored" in a completely filled 4f sublevel? 14 (B) 10 (C) 7 (D) 28 For any given value of n greater than or equal to 2, how many electrons can be "stored" in a completely filled p-block of elements? 10 (B) 3 (C) 6 (D) 5 (A) 45. Within a given n-level, which of the following is the correct order in which subshells become filled with electrons? s, p, d, f (B) p, s, f, d (C) s, p, f, d (D) d, s, p, f (A) Electron configuration fill in electrons in order of energy orbitals Max of 2 electrons per orbital Use Periodic Table to determine order Can shorthand as [previous noble gas] valence electrons Members of same group have same number of valence electrons 46. Which of the following is the correct electron configuration of rubidium (Note: Both the number of electrons and the proper filling order in terms of energy must be present in the answer you select)? 1s22s22p63s23p63d104s24p64d1 1s22s22p62d103s23p63d103f1 (B) (D) 1s22s22p63s23p64s24d104p65s1 1s22s22p63s23p64s23d104p65s1 (A) (C) 47. (A) 48. Which electron configuration is impossible? 1s22s22p63s2 (B) 1s22s22p63s23p6 (C) 1s22s22p62d2 (D) 1s22s22p63s1 A bismuth (Bi) atom has one more electron than a lead atom. Into which energy sub level does this added electron go? 5p (B) 6p (C) 6s (D) 7s (A) 6 49. (A) (C) 50. (A) 51. (A) (D) 52. (A) 53. (A) 54. The electronic configuration of the manganese (Mn) atom is 1s22s22p63s23p64s2 4d5 1s22s22p63s23p64s24p5 (B) (D) 1s22s22p63s23p63d7 1s22s22p63s23p64s23d5 What is the electronic configuration of Uranium? [Rn]7s26d15f3 (B) [Ra]7s27d17f3 (C) [Rn]7s26d16f3 (D) [Rn]7s27d15f3 Which represents the electronic structure of the element having the atomic number 17? 1s22p83d7 1s22s22p42d23s23p43d1 (B) (E) 1s22s22p63s23p5 1s22p22d63f7 (C) 1s22s83p7 The electron configuration of the two outer subshells of vanadium, element number 23, is 4s33d2 (B) 4s24p3 (C) 4s23d3 (D) 4s13d4 In has the valence electron configuration 5s25p1 (B) 3s23p5 (C) 3s23p3 (D) 5s25p3 An atom has a valence shell electron configuration of ns1. To which group of metals in the periodic table does it belong? transition (B) alkaline earth (C) rare earths (D) alkali (A) 55. (A) How many valence electrons does an ordinary chlorine atom contain? 7 (B) 6 (C) 8 (D) 5 Properties of Atoms Happy Atoms Only Noble gases are happy All others want same electron configuration (same number of electrons as Noble gases) Ionize: metals lose electrons; gain positive charge; CATIONS Non-metals lose electrons; gain negative charge; ANIONS How many protons are present in a 127I- ion? 72 (B) 127 (C) 54 (D) 53 (E) 73 56. (A) 57. (A) Which pair of particles has the same number of electrons? Cl , Ca2+ (B) Br , Se (C) Ne, Ar (D) Al3+, P3 7 58. (A) (B) (C) (D) 59. (A) (C) 60. (A) 61. (A) 62. (A) 63. (A) (D) 64. (A) 65. (A) 66. (A) 67. (A) In what respect does an atom of magnesium differ from a magnesium ion (Mg2+)? The ion has a more stable electronic arrangement than the atom. The positive charge on the nucleus of the ion is two units greater than the nuclear charge on the atom. The ion has two more protons than the atom. The ion has two more electrons than the atom. What do these have in common? the same number of protons the same number of electrons Which ion has twenty six electrons? Cr2+ (B) Fe2+ (C) Ni2+ (D) Cu2+ 20Ne 19F (B) (D) 24Mg2+ the same number of neutrons the same size Which ion is not likely to form from its atoms? Al3+ (B) S2(C) As3(D) K+ (E) Mg+ What charge would you expect to find on a selenide ion? 0 (B) +2 (C) +1 (D) -2 (E) -1 The ions most commonly formed by calcium, aluminum and bromine are: Ca+, Al2+, BrCa2-, Al5-, Br+ (B) (E) Ca2+, Al5-, BrCa2+, Al3+, Br(C) Ca2-, Al3+, Br- Which one of these has an electronic configuration different from the others? Ar (B) Mg2+ (C) K+ (D) S2 Which element, isotope, or ion listed below contains 16 protons, 17 neutrons, and 18 electrons? 33 Ar2- (B) 33 2- S (C) 33 Cl (D) 34 2- S Which of the following atoms or ions is, as written, in violation of the "octet rule"? O3(B) Sr2+ (C) PP3(D) Ne Which of the following atoms or ions complies with the "octet rule"? Mg2+ (B) Ar (C) Br(D) All of the above Answers: C D B B A | D C B A D | D D B C C | A C D A C | D A C B B | D C A B D | C D B D D | BCAAC|CDACA|DCBDA|BCADA|DAACC|EDEBB|AD 8
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