Physical Science Test- Unit Teacher s Use Only Student s Name Date 2016-2017 Academic Year- Term Question Number Max Score Point Scored Duration Grade minutes G Q1 Q2 Q3 Instructions Fill in your student ID in the space above. Check that you have the correct number of pages and questions Answer all the questions. Do not use pencil (except the graphs). Use black or blue ink. Write your answers in the spaces provided according to the instructions given. Write your answers clearly and neatly. Information The marks and value of individual questions are shown in round brackets next to the question. There are questions in the question paper. The total mark for the exam is... There are pages in the exam paper. You will have minutes for this exam. You need to show all the steps in your working in order to get method marks. Calculators may be used. Rules Cheating during the exam will result in an immediate reward of 0. Talking during the exam is not allowed. Sharing materials among students is not allowed. You may not ask questions during the exam. Q4 Q5 Q6 Q7 Q8 Q9 Q10 Q11 Q12 Q13 Q14 Q15 Q16 Q17 Total
Monatomic ions easily memorized using location on the periodic table Cations Anions H + Hydrogen H - Hydride Li + Lithium F - Fluoride Na + Sodium Cl - Chloride K + Potassium Br - Bromide Rb + Rubidium I - Iodide Cs + Cesium O 2- Oxide Be 2+ Beryllium S 2- Sulfide Mg 2+ Magnesium Se 2- Selenide Ca 2+ Calcium N 3- Nitride Ba 2+ Barium P 3- Phosphide Sr 2+ Strontium As 3- Arsenide Al 3+ Aluminum Monatomic cations with multiple charges or don t follow the PT pattern. Fe 2+ Iron (II) Sn 2+ Tin (II) Fe 3+ Iron (III) Sn 4+ Tin (IV) Cu + Copper (I) Pb 2+ Lead (II) Cu 2+ Copper (II) Pb 4+ Lead (IV) Co 2+ Cobalt (II) Hg2 2+ Mercury (I) Co 3+ Cobalt (III) Hg 2+ Mercury (II) Cr 2+ Chromium (II) Mn 2+ Manganese (II) Cr 3+ Chromium (III) Ag + Silver ** Ni 2+ Nickel (II) Zn 2+ /// Cd 2+ Zinc and Cadmium** ** No roman numeral is needed for silver and zinc because they do not have multiple charges. Polyatomic Ions -1 Name -2 Name C2H3O2 - Acetate O2 2- Peroxide HCO3 - Bicarbonate (hydrogen carbonate) CO3 2- Carbonate HSO4 - Bisulfate (hydrogen sulfate) SO4 2- Sulfate HSO3 - Bisulfite (hydrogen sulfite) SO3 2- Sulfite HS - Bisulfide (hydrogen sulfide) CrO4 2- Chromate NO2 - Nitrite Cr2O7 2- Dichromate NO3 - Nitrate S2O3 2- Thiosulfate OH - Hydroxide C2O4 2- Oxalate CN - Cyanide HPO4 2- Hydrogen phosphate SCN - Thiocyanate MnO4 - Permanganate -3 H2PO4 - Dihydrogen phosphate PO4 3- Phosphate PO3 3- Phosphite ClO4 - Perchlorate ** AsO4 3- Arsenate ClO3 - Chlorate ** BO3 3- ClO2 - Chlorite ** +1 Borate ClO - Hypochlorite ** NH4 + Ammonium H3O + Hydronium ** Substitute in Br or I in the series for chlorine to get eight more polyatomic ions that follow the same pattern as the chlorine series. For example BrO - is hypobromite and IO4 - is periodate.
1. In the diatomic fluorine molecule, each fluorine atom has an outer shell with the electron arrangement of the gas A) hydrogen; B) argon; C) oxygen; D) nitrogen; E) neon. 2. A nitrogen molecule A) is polar; B) contains three pairs of shared electrons; C) is unstable; D) is very soluble in water; E) none of these. 3. Which compound is predominantly covalently bonded? A) LiI B) CaC12 C) NaH D) CH4 E) KBr 4. The type of chemical bond that joins one or more elements together is determined by A) atomic mass; B) valance and arrangement of electrons; C) the arrangement of neutrons; D) the total number of electrons. 5. Which pair of elements will not form an ionic bond? A) Ba and Cl B) Ca and S C) K and O D) C and Cl 6. Chemical bonds may be produced by any of the following processes involving electrons except: A) losing; B) gaining; C) sharing; D) transferring; E) splitting. 7.. In the diatomic hydrogen molecule, each hydrogen atom has an outer shell with the electron structure of the gas A) oxygen; B) chlorine; C) helium; D) ammonia. 8.. The type of bond between hydrogen atoms and oxygen atoms in a molecule of water is A) a hydrogen bond; B) an ionic bond; C) a non-polar ionic bond; D) (a polar) covalent bond.
9. The correct electron-dot formula for sodium bromide is 10. The correct electron-dot formula for sodium chloride is 11. Write the molecular formula formed by Ba uniting with Se. A) BaSe B) BaSe2 C) Ba2Se D) Ba2Se3 E) none of these 12. Which molecule is most predictable when rubidium reacts with tellurium? A) RbTe2 B) RbTe3 C) Rb2Te D) Rb2Te3 E) none of these 13. Which is the correct formula for the combining of Ca with P? A) CaP2 B) Ca3P2 C) Ca2P3 D) CaP3 E) none of these 14. Predict the correct molecular formula for the reaction of Ra with At. A) Ra2At B) RaAt2 C) Ra2At3 D) RaAt3 E) none of these 15. Consider the general formula XBr2. Which group will for bromides with the formula above? A) IA B) IVA C) VIA D) VIIA E) none of these 16. The element A has an atomic number of 4, and the element B has an atomic number of 7. The formula of the compound formed by the combination of these elements is A) A2B; B) A3B2; C) AB2; D) A3B; E) A2B3. 17. The formula B2Z3 suggests that A) B is a nonmetal with a valence number of 2; B) Z has a valence number of 3; C) B has a valence number of +3; D) the two elements are united by covalent bonds. 18. Lithium readily reacts with all of the following except A) oxygen; B) water; C) the halogens; D) helium; E) sulfur. 19. Manganese oxide has the formula MnO2. What is the formula for manganese chlorate? A) MnClO3 B) Mn(ClO3)2 C) Mn2(C1OC)3 D) Mn(C1O3)4 E) Mn(ClO3)3
20. The type of bond formed when two atoms share a pair of electrons is called A) ionic; B) coupled; C) covalent; D) bivalent; E) conjugation. 21. Covalent bonds are usually formed by the combination of A) a metal and a nonmetal; B) a metal and a acid group; C) two nonmetals; D) very active metal and the hydroxide ion. 22. If two atoms exert equal attractions for electrons, they form A) a non-polar covalent bond; B) an ionic bond; C) a polar covalent bond; D) no bond. 23. Which of the following is not a polar molecule? A) hydrogen fluoride B) hydrogen gas (H2) C) water D) ammonia (NH3) 24. Which of the following kinds of bonds exists in a N2 molecule? A) ionic B) polar C) single D) double E) triple 25. Which molecule below will have a triple covalent bond? A) fluorine B) oxygen C) nitrogen D) hydrogen 26. Covalent bonds are most likely to be found in compound represented by the formula of A) NaCl; B) KBr; C) CH4; D) KI 27. Which one of these elements is most likely to react to produce a covalent compound? A) 2, 8, 8 B) 2, 8, 8, 2 C) 2, 8, 1 D) 2, 8, 7 E) 2, 8, 3 28. Which one is an example of a diatomic molecule? A) Mg +2 B) N2 C) He D) H2SO4 E) none of these 29. Which period contains three elements that commonly exist as diatomic molecules at S.T. P. conditions?(stp; standard temperature and pressure; 0 0 C and 1atm) A) Period 1 B) Period 2 C) Period 4 D) Period 6 E) Period 7 30. The molecules of the ordinary gaseous elements oxygen, nitrogen, hydrogen, and chlorine are A) monatomic; B) diatomic; C) composed of large numbers of atoms; D) form ionic bonds.
31. The magnesium atom has 2 electrons in its outer shell while the bromine atom has 7 outer shell electrons. The correct formula for magnesium bromide is A) MgBr; B) Mg2Br; C) MgBr2; D) Mg2Br2; E) Mg3Br2. 32. The number of atoms represented by the expression, H2SO4 is A) 1 B) 2 C) 3 D) 4 E) 7 33. Which substances is most likely a crystal as a solid? A) CO 2 B) HCl C) PF5 D) KCl 34. substance A B melting point high, 801 C 0 low, decomposes at 186 C 0 solubility per 100g water 35.7g 3.2g Conductivity When dissolved nonconductor According to the data in the table above, which of the following is the most accurate about the two substances? A) both solids contain only ionic bonding B) both solids contain only covalent bonding C) solid A contains covalent bonds and solid B contains ionic bonds D) solid A contain ionic bonds and solid B contains covalent bonds 35. Why do metals conduct electricity so well? A) Because electrons are trapped in between atoms B) Because the atoms are transferring electrons into each other s electron clouds C) Because a sea of electrons (mobile) exists throughout the material. D) Because electrons are gained by nonmetals in the process 36. An unknown white crystal is tested and found to conduct electricity when it is melted or dissolved in water. What type of bonding does it most likely have? A) ionic B) metallic C) polar covalent D) nonpolar covalent
37. What is the (IUPAC) name for FeCl 3? A) iron chloride B) iron chloride (III) C) iron trichloride D) iron (III) chloride 38. What is the (IUPAC) formula of tin (IV) oxide? A) Cu2SO4 B) Sn(OH)2 C) PbBr4 D) Sn2O4 E)SnO2 39. What is the (IUPAC) name of Cu(ClO3)2? A) Copper Chloride B) Copper Chloride (III) C) Copper trichloride D) Copper(II) chloride E) Copper(II) Chlorate 40. What is the (IUPAC) formula of Iron (II) arsenate? A) Fe2AsO4 B) Fe3AsO4 C) Fe2(AsO4)3 D) Fe3(AsO4)2 E) FeAsO4 41. What is the (IUPAC) formula of Iron (II) phosphide? A) Fe2P B) Fe3P2 C) Fe2P3 D) Fe3(PO4)2 E) FePO4 42. What is the (IUPAC) name for CoO? A) Copper Oxide B) Cobalt Oxide (II) C) Copper Chloride D) Cobalt (II) Oxide E) Cobalt(II) Peroxide