Introduction to college chemistry: Practice test for exam #2 Determine the number of protons, neutrons, and electrons in the following: X p+ = 22 n° = 18 e- = 18 p+ = 18 n° = 18 e- = 22 p+ = 18 n° = 22 e- = 40 p+ = 40 n° = 22 e- = 18 p+ = 18 n° = 22 e- = 18 1 points QUESTION 2 Determine the number of protons, neutrons, and electrons in the following: X p+ = 12 n° = 25 e- = 12 p+ = 12 n° = 12 e- = 13 p+ = 12 n° = 13 e- = 12 p+ = 12 n° = 13 e- = 25 p+ = 25 n° = 12 e- = 13 1 points QUESTION 3 How many moles of Cs are contained in 595 kg of Cs? 4.48 × 103 moles Cs 1.26 × 103 moles Cs 5.39 × 102 moles Cs 2.23 × 102 moles Cs 7.91 × 104 moles Cs 1 points QUESTION 4 How many moles of Kr are contained in 398 mg of Kr? 2.11 × 10-4 moles Kr 4.75 × 10-3 moles Kr 2.99 × 10-3 moles Kr 1.19 × 10-4 moles Kr 33.4 moles Kr 1 points QUESTION 5 Which of the following does NOT describe a metal? good conductor of heat tends to gain electrons found on the left side of the periodic table forms ionic compounds with nonmetals good conductor of electricity 1 points QUESTION 6 Which of the following describes a nonmetal? tend to lose electrons are poor conductors of heat are only solids found in the left side of the periodic table conducts electricity 1 points QUESTION 7 What element is defined by the following information? calcium neon rubidium oxygen chlorine 1 points QUESTION 8 What element is defined by the following information? argon neon potassium calcium zirconium 1 points QUESTION 9 The atomic number is equal to the sum of the number of protons and neutrons. the sum of the number of the neutrons and electrons. the number of the protons. the sum of the number of protons and electrons. the sum of the number of protons, neutrons, and electrons. 1 points QUESTION 10 The mass number is equal to the sum of the number of the electrons and protons. the sum of the number of protons, neutrons, and electrons. the sum of the number of protons and neutrons. the sum of the number of the neutrons and electrons. the number of protons 1 points QUESTION 11 In the same element, ions differ in the number of neutrons and protons. protons. electrons and protons. neutrons. electrons. 1 points QUESTION 12 An atom of 79 Br contains ________ protons. 44 72 79 114 35 1 points QUESTION 13 Give the number of electrons in P 3-. 15 12 14 18 19 1 points QUESTION 14 Give the number of protons in Na +. 24 11 17 10 13 1 points QUESTION 15 Give the symbol for boron. Bo Bn Bb B Br 1 points QUESTION 16 How many moles of potassium are contained in 449 g of potassium? 14.5 moles 11.5 moles 23.6 moles 0.956 moles 6.67 moles 1 points QUESTION 17 Magnesium belongs to the ________ group of the periodic table. alkaline earth metal nonmetal alkali metal transition element halogen 1 points QUESTION 18 Lithium belongs to the ________ group of the periodic table. metalloid alkali metal halogen alkaline earth metal 1 points QUESTION 19 Krypton belongs to the ________ group of the periodic table. halogen metalloid noble gas alkali earth metal 1 points QUESTION 20 Isotopes differ in the number of electrons and neutrons. beta particles. atoms. electrons. neutrons. 1 points QUESTION 21 Identify an anion. an atom that has gained an electron an atom that has lost a neutron and an electron an atom that has lost a proton an atom that has gained a proton an atom that has gained a proton and neutron 1 points QUESTION 22 Identify the cation. S2- Cl2 Cl Kr K+ 1 points QUESTION 23 Predict the charge that a calcium ion would have. 6- 2+ 1- 4- 2- 1 points QUESTION 24 Predict the charge that an ion formed from oxygen would have. 1+ 4+ 6- 2- 3- 1 points QUESTION 25 Predict the charge that the ion formed from chlorine would have. 3+ 4- 2+ 1- 1+ 1 points QUESTION 26 What mass (in g) does 0.990 moles of Kr have? 240119 g 52.8 g 83.0 g 35.6 g 240 g 1 points QUESTION 27 What mass (in kg) does 4.41 moles of copper have? 0.018 kg 0.820kg 0.280 kg 0.444 kg 0.784 kg 1 points QUESTION 28 Which of the following elements is in Group 4? Ar Po Rf Pd K 1 points QUESTION 29 Cs 2O is named cesium dioxide. dicesium dioxygen. cesium oxide. cesium(II) oxide. 1 points QUESTION 30 Determine the name for F 2O. fluorine(II) monoxide fluorate fluorine(I) oxide difluorine monoxide fluorine monoxide 1 points QUESTION 31 Give the formula for lithium dichromate. Li2CrO3 Li2Cr2O5 Li2CrO4 LiCr3O7 Li2Cr2O7 1 points QUESTION 32 Give the name for PCl 3. phosphorous chloride phosphorous trichloride phosphorous(I) chloride phosphorous(III) chloride phosphorous dichloride 1 points QUESTION 33 The chemical formula for calcium nitride is Ca(NO3)2. Ca3N2. Ca(NO2)3. Mg2N2 CaN3. 1 points QUESTION 34 The compound CO 2 is named carbon dioxide. carbonate. carbon (IV) oxide. carbonite. 1 points QUESTION 35 What is the charge on the Fe ions in Fe 2O 3? 1+ 2- 4- 3+ 3- 1 points QUESTION 36 What is the mass of 0.500 mol of chlorotrifluoromethane, CCl F 3? 104 g 52.2 g 4.78 × 10-3 g 209 g 1 points QUESTION 37 What is the molar mass of nitrogen gas? 6.02 × 1023 g/mol 1.20 × 1023 g/mol 14.0 g/mol 28.0 g/mol 1 points QUESTION 38 Write the formula for the compound formed between aluminum and sulfur. (AlS)2 Al2S2 Al2S3 Al3S AlS2 1 points QUESTION 39 Write the name for Ba 3(PO 4) 2. tribarium phosphorus tetraoxide barium(III) phosphite barium phosphite barium phosphate barium(II) phosphide 1 points QUESTION 40 Write the name for PbS. plumbic sulfide lead sulfate plumbous sulfite plumbic sulfate plumbous sulfide 1 points QUESTION 41 Calculate the mass percent composition of lithium in Li 3PO 4. 17.98% 20.82% 55.27% 30.72% 26.75% 1 points QUESTION 42 Calculate the mass percent composition of sulfur in Al 2(SO 4) 3. 35.97% 28.12% 9.372% 42.73% 21.38% 1 points QUESTION 43 Calculate the molar mass of Ca 3(PO 4) 2. 215.21 g/mol 246.18 g/mol 279.21 g/mol 87.05 g/mol 310.18 g/mol 1 points QUESTION 44 Determine the number of moles of sodium in 1.60 moles of sodium phosphate. 1.60 moles of sodium 6.40 moles of sodium 4.80 moles of sodium 3.20 moles of sodium 9.60 moles of sodium Exam number 3 will consist of: Goals 8,9,and 10 and will consist of Mole to Mole conversions, chemical reactions, stoichiometry, percent yield, Balancing chemical equations, types of chemical reactions, oxidation and reduction, kinetic molecular theory of gases. Define pressure, name common pressure measurement units, and convert between them. Define the four properties of gases and describe how they are interrelated. Describe Boyle’s law, Charles’ law, and Avogadro’s law and use these concepts to solve initial and final states problems.
