Sample Exam 1 – Chapters 1-3

Name:_______KEY_____________ Sample Exam 1 – Chapters 1-3 SHOW ALL WORK FOR FULL CREDIT!!!! 1. Give the symbol for each of the following elements: a. The semimetal in group IIIA. _____B_____ b. The noble gas in period 6. _____Rn_____ c. The halogen touching two semimetals. _____I_____ 2. A piece of turquoise is a blue-green solid; it has a density of 0.0957 lb/in3 and a mass of 2.5 g. Calculate the volume of the turquoise in mL. 2.5 g (1 lb/453.59g)(1 in3 / 0.0947 lb)(2.54 cm/ 1 in)3(1 mL/1 cm3) = 0.94 mL 3. Venus has a surface temperature of 730 K. What is this temperature in degrees Fahrenheit? 850 oF (2 s.f.) 4. The following are examples of chemical changes except: a. Solid iron forms rust when combined with water and oxygen. b. Butane burns with air at 1970°C. c. Sodium bicarbonate reacts with vinegar to form carbon dioxide gas. d. Sodium chloride dissolves in water at room temperature. 5. What is the correct term for a gas turning into a solid? ____deposition___ 6. What is the physical state for elemental chlorine, Cl2, at room temperature and normal pressure? a. solid b. liquid c. gas 7. An oxygen molecule travels at 975 mph at room temperature. What is the de Broglie wavelength, in m, for an oxygen molecule if the mass of one oxygen molecule is 5.31 x 10-23 g? (1 mi = 1.6093 km) Convert 975 mph into m/s first: 975 mi/hr(1 6093 km/mi)(1000m/km)(1 hr/3600 s) = 436 m/s λ = h/mv = 6.626 x 10-34 kgm2s-1 / (5.31 x 10-26 kg X 436 ms-1) = 2.86 x 10-11 m 8. Calculate the mass in grams of 4.73 x 1025 formula units of calcium phosphate, Ca3(PO4)2. 4.73 x 1025 formula units Ca3(PO4)2 (1 mol/6.02214 x 1023 formula units)( 310.178 g/ 1 mol) = 2.44 x 104 g units Ca3(PO4)2 9. Consider the colors of the visible spectrum. a. Which color has the higher energy, yellow or red? _____Yellow________ b. Which color has the lower frequency, violet or green? ____green_____ c. What is the frequency, in Hz, for orange light at 618 nm? c = νλ ν = c/λ = 2.998 x 108 ms-1/(6.18 x 10-7 m) = 4.85 x 1014 s-1 10. When the Sojourner spacecraft landed on mars in 1997, the planet was approximately 7.8 x 107 km from earth. a. How many minutes did it take for the television signal (EM radiation) to reach Earth from Mars? 7.8 x 107 km(1000 m/km)(1 sec/2.998 x 108 m)(1 min / 60 sec) = 4.3 min b. Calculate the energy, in kJ, of this transmission if the wavelength of the transmission was 71 m. (6.626 x 10-34 Js)(2.998 x 108 ms-1)1 kJ/1000J) = 2.8 x 10-30 kJ 71 m E = hν 11. Which of the following is an extensive property: a. boiling point b. density c. heat d. color 12. Determine if the following are homogeneous or heterogeneous mixtures (circle one): a. soil homogeneous heterogeneous b. brass homogeneous heterogeneous 13. Complete the following table: Mass Number, A Atomic Number, Z Neutrons, no Electrons, e- Sb 117 51 66 51 Protons, p+ 51 K+ 42 19 23 18 19 Li 6 3 3 3 3 Isotope 117 42 6 14. The element copper, Cu, is a ______________. a. metal b. metalloid c. nonmetal d. gas 15. Which of the following is equal to one mole? (Look at the molar mass since it is g/ 1 mole) b. 55.85 g Fe b. 98.90 g Sr c. 14.35 g He d. 10.15 g Mg 16. Match the scientist to their discovery Dalton JJ Thomson Rutherford JJ Thomson a. Identified the atom as a sphere of mainly positive charge with negatively charged particles dispersed throughout. Dalton b. An element is composed very tiny particles that are indivisible called atoms. Rutherford c. The atom consists of a tiny, dense, positively charged nucleus where nearly all of the mass resides. 17. If white and grey spheres represent atoms of different elements, which represents a mixture of diatomic elements? a b c d 18. What is the symbol of the atom with the following short-hand electron configurations? a. [Kr] 5s24d105p2 ______Sn________ b. [Ar] 4s13d10 ______Cu________ c. [Xe] 6s1 ______Cs________ 19. Correctly complete the orbital filling diagram for a neutral aluminum atom: 1s 2s 2p 3s 20. Write the full electron configuration from the ground state for the following: a. Se 1s22s22p63s23p64s23d104p4 b. V 1s22s22p63s23p64s23d3 c. Ni2+ 1s22s22p63s23p63d8 21. Which set of quantum numbers is NOT allowed? c. d. e. f. n = 4, l = 2, ml = 2, ms = - ½ n = 2, l = 1, ml = 0, ms = - ½ n = 3, l = 2, ml = -3, ms = - ½ n = 5, l = 0, ml = 0, ms = + ½ 3p 22. When n=5 and l = 3, what are the possible values for ml? -3, -2, -1, 0, +1, +2, +3 23. Which quantum number represents the shape of an atomic orbital? a. n b. l c. ml d. ms 24. Which one of the following alkali metal ions has the largest atomic radius? a. Rb+ b. K+ c. Na+ d. Li+ 25. Which of the following has the highest metallic character? a. Sr b. Te c. Mo d. Rb 26. Which element has the lowest ionization energy? a. F b. Cl c. Br d. I 27. Which ion is isoelectronic to a noble gas? a. Cr3+ b. Sc2+ d. Ti4+ c. Ga3+ 28. Which atom has the higher ionization energy, N or O? a. N b. O 29. Energy is _______________ when an electron changes from n = 5 to n = 2 in the hydrogen atom. a. absorbed b. emitted c. negligible d. destroyed 30. What is the molar mass of calcium phosphate, Ca3(PO4)2? a. 430.42 g/mol b. 278.18 g/mol c. 310.18 g/mol d. 279.21g/mol 31. What value remains constant between different isotopes of the same element? a. protons b. electrons c. neutrons d. mass number 32. What is the phase change associated with a substance changing from gas to liquid? a. sublimation b. freezing c. vaporization d. condensation 33. How many carbon atoms are the in 10.0 g of propane, C3H8? 10.0 g C3H8( 1 mol C3H8 / 44.0962 g)(6.02214 x 1023 molecules/ 1 mol)(3 mol C/ 1 mole C3H8) = 4.10 x 1023 C atoms 34. What mass of oxygen gas occupies a 2.50 L container at STP? 2.50 L O2 gas at STP(1 mole O2)(32.00 g O2) = 3.57 g O2 (22.41 L )(1 mole ) 35. How many potassium ions are there in 8.99 moles of potassium nitride, K3N? 8.99 mol K3N(6.02214 x 1023/1 mol)(3 K+ ions/1 mol K3N) = 1.62 x 1025 K+ ions