Introductory Chemistry Practice Test 1 With Answer Keys

Practice Test 1 Answer Key 14) FALSE Test name: Practice Test 1 15) D 1) E 2) B 16) E 17) E 18) TRUE 3) D 4) E 19) TRUE 20) B 5) TRUE 6) C 21) D 22) B 7) C 8) E 9) D 10) D 11) D 23) TRUE 24) E 25) E 26) C 27) D 12) C 13) C 28) D Practice Test 1 29) B 44) FALSE 30) A 45) C 31) C 46) D 32) E 47) A 33) A 48) C 34) B 49) 35) C 36) A 50) 37) D 𝑑= 38) D 39) FALSE 40) D 41) B 42) C 43) D 𝑚𝑎𝑠𝑠 30.30𝑔 = 𝑣𝑜𝑙𝑢𝑚𝑒 (18.9 𝑚𝐿 − 15.5𝑚𝐿) 30.30𝑔 = 8.9𝑔/𝑚𝐿 = 3.4 𝑚𝐿 So the metal’s density is 8.9 g/mL Practice Test 1 2) ______ 1) Which process depicts a physical change? 1) ______ A) B) None of the processes above depicts a physical change. C) D) A) B) C) D) E) 1 1 1 1 1 s s s s s 2 1 2 2 2 2 2 2 2 2 p 62 s s 22 p s 22 p s 22 p s 22 p 2 2 3 6 2 6 3 6 3 6 p 6 s 23 p d 6 s 23 d s 22 d 4 4 4 3) How many pounds are represented by 764.6 mg? [1 pound = 454 g] 3) ______ A) B) C) D) E) 3.471 × 10 8 lb 1.684 lb 0.7646 lb 1.684 × 10-3 lb 347.1 lb E) 4) What is the number 3,000 written in scientific notation using the proper number of significant figures? 4) ______ 2) What is the ground state electron configuration of sulfur, whose atomic number is 16? A) B) C) D) E) 0.003 × 10−3 3.000 × 103 3 × 10−3 0.3 × 104 3 × 103 Practice Test 1 5) In the molecule BeF 2, the beryllium atom is an exception to the octet rule. 5) ______ ⊚ ⊚ 8) Which of the following terms best describes the sample of matter in the diagram? Note: different colored circles represent atoms of different elements. true false 8) ______ 6) What Kelvin temperature corresponds to 98.6°F? 6) ______ A) B) C) D) E) 310 K 31.00 K 310.2 K 132.0 K 199 K A) B) C) D) E) heterogeneous mixture None of the choices are correct. solution homogeneous mixture pure substance 9) What is the formula of the ionic compound sodium carbonate? 9) ______ 7) Which of the following is a metal in the third period? 7) ______ A) B) C) D) E) Cu Ge Mg Cl Ca A) B) C) D) E) Na(CO 3) Na 3CO 3 Na 2CO 2 Na 2CO 3 NaCO 2 2 10) What is the name of the ion whose formula is NO 3- ? Practice Test 1 10) ______ A) B) C) D) E) nitrogen trioxide ion sodium oxide ion ammonium ion nitrate ion nitride ion 13) What Group IA (1) ion has the electronic arrangement shown 1 s 22 s 2 2 p 6 13) ______ 11) Which combination of atoms is most likely to form an ionic compound if they are allowed to react with each other? A) B) C) D) E) lithium ion potassium ion sodium ion magnesium ion calcium ion 11) ______ A) metalloid and metalloid B) metal and metal C) nonmetal and nonmetal D) metal and nonmetal E) All combinations are likely to form an ionic compound. 12) Which of the following terms is defined as anything that has mass and occupies space? 12) ______ A) B) C) D) E) chemistry compound matter volume element 14) The halogens, Group VII A (17), have the lowest ionization energies of any group in the periodic table. 14) ______ ⊚ ⊚ true false 15) Which one of the following is NOT true about elements that form cations? Practice Test 1 15) ______ A) The atoms lose electrons in forming ions. B) The elements are metals. C) They have low ionization energies. D) They have high electron affinities. E) They are located to the left of the periodic table. 17) ______ A) B) C) D) E) potential energy kinetic energy electron affinity electronegativity ionization energy 18) One calorie is the amount of energy needed to raise the temperature of one gram of water one degree Celsius. 16) What is the general name given to the elements of Group IA (1)? 16) ______ A) B) C) D) E) halogens alkaline earth metals noble gases metalloids alkali metals 18) ______ ⊚ ⊚ true false 19) The hydrogen bonds between water and ammonia in a solution are intermolecular forces. 19) ______ 17) What is the energy required to remove an electron from an isolated atom? ⊚ ⊚ true false 20) Which properly represents the Lewis structure of hydrogen sulfide, H2S? Practice Test 1 22) ______ 20) ______ A) B) C) D) E) A) B) C) D) E) 21) CO 2? How many bonding electrons are in nonpolar covalent polar covalent nonpolar ionic ionic intermolecular 23) There are eight valence electrons in a chlorine anion. 23) ______ 21) ______ A) B) C) D) E) 4 2 3 8 1 22) In the compound shown below, how can the bond between carbon and chlorine be described? ⊚ ⊚ true false 24) Which of the following accounts for the fact that chlorine has an atomic mass of 35.45 amu rather than a whole number? 24) ______ A) B) C) D) E) isomers electrons radioactivity protons isotopes 25) What is the name of CuF Stock system? 2 in the Practice Test 1 25) ______ A) B) C) D) E) 28) What is the basic unit of volume in the metric system? copper(II) fluorate copper fluoride copper difluoride copper(I) fluoride copper(II) fluoride 28) ______ 26) Which compound contains a central atom with an exception to the octet rule known as an expanded octet? A) B) C) D) E) milliliter cubic centimeter millimeter liter gram 26) ______ A) B) C) D) E) 29) Which of the following elements is most likely to form a 2+ ion? NO BF 3 PF 5 CH 4 BeH 2 29) ______ 27) When a neutral atom gains one or more electrons, what type of particle is formed? 27) ______ A) B) C) D) E) a cation a proton a positron an anion an isotope A) B) C) D) E) Li Ca K Al N 30) Which ion is NOT isoelectronic (i.e. has the same electron configuration) with Ar? The electron configuration of Ar is shown. Practice Test 1 30) ______ A) B) C) D) E) 33) How many total valence electrons are in SO 4 2- ? Br − Ca 2+ Cl − S 2− K + 33) ______ 31) In Rutherford's experiment, which led to the discovery of the atomic nucleus, what type of particle or ray was fired at the gold foil target? 31) ______ A) B) C) D) E) beta neutrons alpha cathode rays gamma A) B) C) D) E) 32 2 64 12 16 34) What is the formula of the ionic compound formed when ions of calcium and nitrogen combine? 34) ______ A) B) C) D) E) Ca 2N Ca 3N CaN CaN 2 Ca 2N 2 3 32) Assuming reactions between the following pairs of elements, which pair is most likely to form an ionic compound? 32) ______ A) B) C) D) E) chlorine and oxygen carbon and chlorine fluorine and iodine copper and tin cesium and iodine 35) Draw the Lewis structures of F 2 and N 2. Which statement is true? 2, O Practice Test 1 35) ______ A) Fluorine has the shortest bond between the two atoms. B) B. Both O 2 and N 2 have double bonds connecting the atoms. C) The bond between the nitrogen atoms in N 2 is stronger than the bond in F 2 and O 2. D) All three molecules have triple bonds between the atoms. E) All three molecules have a single bond between the atoms. 36) What is the formula of the compound sulfur trioxide? 36) ______ A) B) C) D) E) SO 3 S 3O 2? S 3O S 3O 2 S(O 2) 3 37) Which statement explains why isotopes have different mass numbers? 37) ______ A) Isotopes differ in the number of electrons each contains. B) Isotopes differ in the number of protons and neutrons each contains. C) Isotopes differ in the number of protons and electrons each contains. D) Isotopes differ in the number of neutrons each contains. E) Isotopes differ in the number of protons each contains. 38) A patient needs 0.300 g of a solid drug preparation per day. How many 10.0 mg tablets must be given to the patient per day? 38) ______ A) B) C) D) E) 33.0 tablets 330. tablets 300. tablets 30.0 tablets 3.00 tablets 39) As a rule, a polar substance will be a good solvent for nonpolar solutes, and vice versa. Practice Test 1 39) ______ ⊚ ⊚ true false 42) ______ 40) Which of the following numbers has only one significant figure? 40) ______ A) B) C) D) E) 42) Hydrogen can form two different ions: a hydrogen ion (H +), and a hydride ion (H −). Which statement concerning these ions is FALSE? 3.0 × 10 1 All of the choices are correct. 3.00 0.003 30.0 41) What volume, in milliliters, will 2.00 g of air occupy if the density is 1.29 g/L? A) The H − ion is an anion formed by the gain of one electron; this ion has a full n=1 energy level. B) The hydrogen ion and the hydride ion have different sizes. C) The hydrogen ion and the hydride ion are isotopes. D) The H + ion is a cation formed by the loss of one electron; this ion has no valence electrons. E) The hydrogen ion and the hydride ion have the same number of protons. 43) Air is a/an 43) ______ 41) ______ A) B) C) D) E) 2.20 mL 1.55 × 10 2.72 × 10 1.43 mL 4.59 × 10 3 3 2 mL mL mL A) B) C) D) E) compound. molecule. element. mixture. pure substance. Practice Test 1 44) J. J. Thomson was the first to state that an atom is mostly empty space. 47) What are the three primary particles found in an atom? 44) ______ ⊚ ⊚ 47) ______ true false A) B) C) D) E) electron, neutron, and proton proton, electron, and neutrino neutron, positron, and electron electron, proton, and nucleon positron, electron, and nucleon 45) What do the dots in a Lewis symbol represent? 45) ______ A) B) C) D) E) the nucleus mass number valence electrons protons innermost (core) electrons 46) What is the value of the mass number in the isotope ? 46) ______ A) B) C) D) E) 78 126.9 53 131 184 48) Electron affinity is 48) ______ A) the energy required to remove an electron from an isolated atom. B) the force between two ions of opposite charge. C) the energy released when an isolated atom gains an electron. D) the force between two electrons in the same orbital. E) the attraction of an atom for an electron in a chemical bond. Practice Test 1 49) Draw the Lewis Structure of H3O+ in the space below. 50) You must show the calculation steps to get the points. Keep proper significant figures for full points. In the density experiment, one student measured 15.5 mL of water in a 50-mL graduate cylinder. Then she dropped a metal cube in the graduate cylinder. Now the graduate cylinder read as 18.9 mL. She weighed the metal cube’s mass as 30.30 g. What is the metal’s density?