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Popular in Chemistry
This 4 page Study Guide was uploaded by Corina Johnson on Sunday February 21, 2016. The Study Guide belongs to 10886 at University of Houston taught by Simon Bott in Winter 2016. Since its upload, it has received 139 views. For similar materials see Foundations of Chemistry in Chemistry at University of Houston.
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Date Created: 02/21/16
CHEM 1301 FALL 2002 TEST 1 VERSION 1 NO CHEATING! BUBBLE IN “1” IN THE P COLUMN TO GET YOUR GRADE POSTED!!!!! [the only way you’ll find out how you did!] 1. Which of the following was not an element according to the ancient Greeks? (A) air (B) earth (C) silver (D) fire (E) water 2. Which of the following is incorrectly named as a law or theory? (A) The law of gravity that things fall to the ground (B) Dalton’s atomic theory that substances are composed of sub-microscopic particles (C) Charles’ law that the volume of a gas increases as the temperature increases (D) Avogadro’s law that the volume of a gas is proportional to the number of sub-microscopic particles (E) VSEPR theory that sub-microscopic molecules adopt shapes based on electron repulsion. 3. When 14 g of nitrogen are combined with 32 g of oxygen, the only thing produced is nitrogen dioxide and nothing else is left over. (I) how many grams of nitrogen dioxide are made? (II) How many grams of oxygen would be used to combine with 28 g of nitrogen to make nitrogen dioxide? (A) (I) 18 g (II) 32 g (B) (I) 46 g (II) 32 g (C) (I) 46 g (II) 16 g (D) (I) 46 g (II) 64 g (E) (I) 644 g (II) 46 g 4. Which of the following formulas refers to a pure element? (A) H 2O (B) H 2 2 (C) O 2 (D) Xf (E) answer to both (C) and (D) 1 5. Which assumption of Dalton’s atomic theory had to be revised or discarded because of the discovery of electrons? (A) The ultimate particles of matter are the atoms of elements, which are indivisible and indestructible. (B) All the atoms of a given element are alike in all respects. (C) The atoms of different elements differ in one or more properties. (D) Compounds are formed by combination of different kinds of atoms. (E) None of these 6. Which statement concerning the structure of the atom is correct? (A) Protons and neutrons have most of the mass and occupy most of the volume of the atom. (B) Protons and electrons have the same mass (C) Protons and electrons have the same charge (D) Protons and neutrons have most of the mass but occupy very little of the volume of the atom. (E) The number of neutrons is the same as the number of protons in a neutral atom 7. An atom of ruthenium–101 ( 10Ru) contains (A) 44 neutrons, 44 protons, 57 electrons. (B) 44 electrons, 44 protons, 101 neutrons. (C) 57 neutrons, 44 protons, 44 electrons. (D) 44 neutrons, 44 protons, 44 electrons. (E) 57 electrons, 57 protons, 44 neutrons. 8. Which of the following is NOT an alkali metal? (A) Li (B) K (C) Cs (D) Fr (E) H 9. In the following list, how many names and symbols are CORRECTLY matched? Potassium is P; N is Neon; Iron is I; Sodium is Na; Co is copper (A) all are correct (B) 1 (C) 2 (D) 3 (E) 4 10. Which of the following statements is incorrect? (A) Silicon is a metalloid (B) Aluminum is a metal (C) Bromine is malleable (D) Neon is a noble gas (E) Calcium is an alkaline earth metal 2 11. Tellurium consists of 3 common isotopes. Half of tellurium atoms have a mass of 127, and another 0.45 of them weigh 128. What is the mass of the remaining isotope? The atomic mass of tellurium is 127.6. (A) 125 (B) 126 (C) 129 (D) 130 (E) 131 12. Boron has an atomic mass of 10.8. There are two isotopes of boron – one contains 5 neutrons and the other contains 6 neutrons in the nucleus. What is the fractional abundance of the first one (the one with 5 neutrons)? (A) 0.2 or 1/5 (B) 0.25 or 1/4 (C) 0.33 or 1/3 (D) 0.5 or 1/2 (E) 0.8 or 4/5 13. Which of the following are isotopes of each other? 1. a chlorine atom with a mass of 35 2. a chlorine atom with 18 neutrons in the nucleus 3. an atom with 18 protons and 18 electrons in the nucleus 4. a sulfur atom with a mass of 36 (A) 1 and 2 (B) 2 and 3 (C) 3 and 4 (D) all of them are isotopes of each other (E) none of them are isotopes of each other 14. Rutherford's experiment was used to indicate the presence of: (A) electrons (B) protons (C) electron's energy levels (D) neutrons (E) a positive nucleus without electrons stuck to it 15. Which of the following statements is incorrect? (A) red light has a shorter wavelength than infrared (B) ultraviolet has a higher energy than violet light (C) green light has a higher frequency than blue light (D) gamma rays are the most energetic form of light (E) radiowaves have a longer wavelength than microwaves 16. A form of light has an energy of 6.75 x 10-24J. Given that h = 6.63 x 1034Js and c = 3.00 x 10 m/s, what is the wavelength of this light? -57 -48 -3 10 (A) 4.47 x 10 m (B) 1.34 x 10 m (C) 2.95 x 10 m (D) 0.0295 m (E) 1.02 x 10 m 3 17. Which of the following is incorrect? (A) The lowest energy p-subshell is the 2p (B) A maximum of 10 electrons can go into a d-subshell (C) Electrons have only certain, allowed energy values (D) A boron atom has electrons in 3 shells (E) All of these are correct 18. Which of the following represents the electron configuration of Ce? (A) [La]4f1 (B) [Xe]6s 6d 6f 1 (C) [Xe]6s 5d 4f 1 (D) [Xe]6s 5d 5f 1 (E) [Xe]6s 4f 2 19. Which feature of Bohr's atomic model is no longer accepted as true by today's scientists? (A) That most of an atom's mass is located within the nucleus (B) That electrons have only certain, allowed energy values (C) That electrons orbit the nucleus in circular2paths (D) That each shell can hold a maximum of 2n electrons (E) All of these are accepted as true today. 20. Which of the following could represent a 3p orbital? (A) (B) (C) (D) (E) None of these 4
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