exam 1

) Read the length of the metal bar with the correct number of significant figures. 2) A) 15.00 cm B) 15.0 cm C) 20 cm D) 15 cm E) 15.000 cm

b

What answer should be reported, with the correct number of significant figures, for the following calculation? (433.621 - 333.9) × 11.900 3) A) 1.18680 × 103 B) 1.19 × 103 C) 1.187 × 103 D) 1.186799 × 103 E) 1.1868 × 103

b

An element has three stable isotopes with masses of 27.977 amu, 28.976 amu, and 29.973 amu. The heavier two isotopes have an abundance of 4.68% and 3.09%, respectively. What is the mass of the element? 6) A) 30.107 amu B) 29.251 amu C) 28.085 amu D) 28.991 amu E) 27.684 amu 1 7) How are gases different from solids and liquids? 7) A) Only gases can take the shape of their container. B) Gases are compressible. C) Gases are colorless. D) Gases can only be made up of atoms. E) The particles in a gas attract each other much more strongly than in solids and liquids. 8) Two or more substances in variable proportions, where the composition is constant throughout are 8) A) a heterogeneous mixture. B) a compound. C) a crystalline solid. D) a homogeneous mixture. E) an element. 9) Two or more substances in variable proportions, where the composition is variable throughout are 9) A) a solution. B) an amorphous solid. C) a compound. D) a heterogeneous mixture. E) a homogeneous mixture. 10) The atomic number (Z) is the number of ________ found in the nucleus of an atom. 10) A) protons and electrons B) protons C) protons and neutrons D) neutrons E) electrons 11) Which of the following statements about the phases of matter is TRUE? 11) A) In both solids and liquids, the atoms or molecules pack closely to one another. B) Liquids have a large portion of empty volume between molecules. C) Gaseous substances have long-range repeating order. D) There is only one type of geometric arrangement that the atoms or molecules in any solid can adopt. E) Solids are highly compressible. 12) A substance composed of two or more elements in a fixed, definite proportion is 12) A) a heterogeneous mixture. B) an alloy. C) a homogeneous mixture. D) a solution. E) a compound. 13) Dalton's Atomic Theory states 13) A) that energy is neither created nor destroyed during a chemical reaction. B) that matter is composed of small indestructible particles. C) that the properties of matter are determined by the properties of atoms. D) that all elements have several isotopes. E) that an atom is predominantly empty space. 2 14) All samples of a given compound, regardless of their source or how they were prepared, have the same proportions of their constituent elements. Which law does this refer to? 14) A) Law of the Conservation of Mass B) First Law of Thermodynamics C) Law of Multiple Proportions D) Law of Definite Proportions E) Law of Modern Atomic Theory 15) What does "X" represent in the following symbol? 80 35 X 15) A) bromine B) selenium C) mercury D) scandium E) chlorine 16) Determine the number of protons, neutrons and electrons in the following. 25 12 X 16) A) p+ = 25 n° = 12 e- = 13 B) p+ = 12 n° = 13 e- = 25 C) p+ = 12 n° = 25 e- = 12 D) p+ = 12 n° = 12 e- = 13 E) p+ = 12 n° = 13 e- = 12 17) Ions differ from atoms in their number of 17) A) electrons. B) neutrons and protons. C) electrons and protons. D) protons. E) neutrons. 18) What species is represented by the following information? p+ = 47 n° = 62 e- = 46 18) A) Nd B) Ag+ C) Ag D) Pd+ E) Pd 19) Silver has an atomic mass of 107.868 amu. The Ag-109 isotope (108.91 amu) is 48.16%. What is the mass, in amu, of the other isotope? 19) A) 108.47 amu B) 106.91 amu C) 106.12 amu D) 105.87 amu 20) How many moles of Kr are contained in 398 mg of Kr? 20) A) 4.75 × 10-3 moles Kr B) 2.11 × 10-4 moles Kr C) 33.4 moles Kr D) 2.99 × 10-3 moles Kr E) 1.19 × 10-4 moles Kr 3 21) How many argon atoms are contained in 7.66 × 105 mmol of argon? 21) A) 4.61 × 1026 Ar atoms B) 3.24 × 1026 Ar atoms C) 1.84 × 1028 Ar atoms D) 7.86 × 1020 Ar atoms E) 1.15 × 1028 Ar atoms 22) The vertical height of a wave is called 22) A) wavelength. B) amplitude. C) frequency. D) area. E) median. 23) Calculate the wavelength (in nm) of the blue light emitted by a mercury lamp with a frequency of 6.88 × 1014 Hz. 23) A) 206 nm B) 485 nm C) 675 nm D) 229 nm E) 436 nm 24) Which of the following occur as the energy of a photon increases? 24) A) The wavelength increases B) The frequency decreases. C) The wavelength gets shorter. D) The speed increases. E) None of the above occur as the energy of a photon increases. 25) The number of cycles that pass through a stationary point is called 25) A) wavelength. B) amplitude. C) frequency. D) area. E) median. 26) The distance between adjacent crests is called 26) A) wavelength. B) amplitude. C) frequency. D) area. E) median. 27) When two elements form two different compounds, the masses of element B that combine with 1 g of element A can be expressed as a ratio of small whole numbers. Which law does this refer to? 27) A) Law of Definite Proportions B) First Law of Thermodynamics C) Law of the Conservation of Mass D) Law of Multiple Proportions E) Law of Modern Atomic Theory 4 28) Calculate the energy of the violet light emitted by a hydrogen atom with a wavelength of 410.1 nm. 28) A) 8.13 × 10-19 J B) 4.85 × 10-19 J C) 1.23 × 10-19 J D) 5.27 × 10-19 J E) 2.06 × 10-19 J 29) Which of the following statements is TRUE? 29) A) An orbital is the volume in which we are most likely to find an electron. B) Part of the Bohr model proposed that electrons in the hydrogen atom are located in "stationary states" or particular orbits around the nucleus. C) The emission spectrum of a particular element is always the same and can be used to identify the element. D) The uncertainty principle states that we can never know both the exact location and speed of an electron. E) All of the above are true. 30) It is possible to determine the ionization energy for hydrogen using the Bohr equation. Calculate the ionization energy for an atom of hydrogen, making the assumption that ionization is the transition from n = 1 to n = Q. 30) A) +2.18 × 10-18 J B) -2.18 × 10-18 J C) +4.36 × 10-18 J D) -4.59 × 10-18 J E) +4.59 × 10-18 J 31) What are the possible orbitals for n = 3? 31) A) s, p, d B) s, p C) s D) s, p, d, f 32) What value of l is represented by an f orbital? 32) A) 1 B) 0 C) 3 D) 2 33) How many orbitals are contained in the third principal level (n = 3) of a given atom? 33) A) 7 B) 9 C) 18 D) 5 E) 3 34) Which of the following quantum numbers describes the shape of an orbital? 34) A) principal quantum number B) magnetic quantum number C) angular momentum quantum number D) spin quantum number E) Schrödinger quantum number 35) Calculate the wavelength of light associated with the transition from n = 1 to n = 3 in the hydrogen atom. 35) A) 646 nm B) 155 nm C) 136 nm D) 103 nm E) 971 nm 5 36) Which of the following quantum numbers describes the orientation of an orbital? 36) A) principal quantum number B) spin quantum number C) magnetic quantum number D) angular momentum quantum number E) Schrödinger quantum number 37) Which of the following quantum numbers describes the size and energy of an orbital? 37) A) spin quantum number B) angular momentum quantum number C) Schrödinger quantum number D) magnetic quantum number E) principal quantum number 38) Give the possible values for ml for a d orbital. 38) A) 1, 2, 3 B) -2, -1, 0, 1, 2 C) 0, 1, 2 D) -1, 0, 1 39) Describe the shape of a p orbital. 39) A) dumbbell shaped B) eight lobes C) three lobes D) four lobes E) spherical 40) Which of the following does NOT describe a metal? 40) A) good conductor of electricity B) found on the left side of the periodic table C) tends to gain electrons D) good conductor of heat E) forms ionic compounds with nonmetals 41) No two electrons can have the same four quantum numbers is known as the 41) A) Pauli exclusion principle. B) Hund's rule. C) Aufbau principle. D) Heisenberg uncertainty principle. 42) When filling degenerate orbitals, electrons fill them singly first, with parallel spins is known as 42) A) Pauli exclusion principle. B) Hund's rule. C) Aufbau principle. D) Heisenberg uncertainty principle. 43) The element that corresponds to the electron configuration 1s22s22p63s23p64s13d5 is 43) A) titanium. B) vanadium. C) manganese. D) iron. E) chromium. 44) How many valence electrons does an atom of Al possess? 44) A) 3 B) 8 C) 2 D) 5 E) 1 6 45) Give the ground state electron configuration for Cd. 45) A) [Kr]4d10 B) [Kr]5s24d10 C) [Kr]5s24d105p2 D) [Kr]5s24d8 E) [Kr]5s25d10 46) Choose the orbital diagram that represents the ground state of N. 46) A) B) C) D) E) 47) Place the following elements in order of increasing atomic radius. P Ba Cl 47) A) Ba < Cl < P B) Cl < P < Ba C) Ba < P < Cl D) Cl < Ba < P E) P < Cl < Ba 48) Place the following in order of increasing radius. Br Na Rb 48) A) Rb< Na< Br B) Rb< Br< Na C) Br< Na< Rb D) Br< Rb< Na E) Na< Rb< Br 7 49) Place the following in order of increasing IE1. K Ca Rb 49) A) Rb < Ca < K B) Ca < K < Rb C) K < Ca < Rb D) Ca < Rb < K E) Rb < K < Ca 50) Give the ground state electron configuration for Rb. 50) A) [Kr]5s1 B) [Ar]4s24p6 C) [Ar]4s23d104p6 D) [Kr]5s2 E) [Kr]5s24d2 51) Which reaction below represents the electron affinity of Li? 51) A) Li(g) + e Li(g) B) Li(g) Li(g) + e C) Li(g) + e Li(g) D) Li(g) Li(g) + e E) Li(g) + e Li(g) 52) What is the maximum number of s orbitals that are possible in a given shell? 52) A) 1 B) 3 C) 7 D) 5 E) 9 53) What is the wavelength of an electron (m = 9.11 × 10-28 g) moving at 1/5 the speed of light? 53) A) 9.36 × 10-9 m B) 4.85 × 10-10 m C) 6.73 × 10-8 m D) 1.21 × 10-11 m E) 2.42 × 10-12 m 54) Predict the charge that an aluminum ion would have. 54) A) 1+ B) 1- C) 5- D) 3+ E) 2+ 55) Identify the element that has a ground state electronic configuration of [Ar]4s23d7. 55) A) cobalt B) zinc C) rhenium D) tungsten E) calcium 56) Which element has the lowest first ionization energy? 56) A) Be B) Br C) S D) N E) Ca

6) C 7) B 8) D 9) D 10) B 11) A 12) E 13) B 14) D 15) A 16) E 17) A 18) B 19) B 20) A 21) A 22) B 23) E 24) C 25) C 26) A 27) D 28) B 29) E 30) A 31) A 32) C 33) B 34) C 35) D 36) C 37) E 38) B 39) A 40) C 41) A 42) B 43) E 44) A 45) B 46) C 47) B 48) E 49) E 50) C 9 Answer Key Testname: PRACTICE TEST 1 51) A 52) A 53) D 54) D 55) A 56) E

) If an object has a density of 8.65 g/cm3, what is its density in units of kg/m3? 4) A) 8.65 × 103 kg/m3 B) 8.65 × 10-7 kg/m3 C) 8.65 × 10-1 kg/m3 D) 8.65 × 10-3 kg/m3 E) 8.65 × 101 kg/m3

a

Convert 781K into Celsius 5) A) 1054°C B) 273°C C) 835°C D) 508°C E) 672°C

d

Determine the density of an object that has a mass of 149.8 g and displaces 12.1 mL of water when placed in a graduated cylinder. 1) A) 18.1 g/mL B) 8.08 g/mL C) 11.4 g/mL D) 1.38 g/mL E) 12.4 g/mL

e