1 st Sem. Final Exam Review

1. 1st Sem. Final Exam Review Honors Chemistry

2. _________ are substances with constant composition that can be broken down into elements by chemical processes. A) Solutions B) Mixtures C) Compounds D) Quarks E) Heterogeneous mixtures

3. An example of a pure substance is A) an element. B) a compound. C) pure water. D) carbon dioxide. E) all of these

4. A Classification Of Matter Homogeneous Heterogeneous Pure Substances Mixtures Elements Compounds Nucleus Protons Atoms Electrons Neutrons

5. Chapter 1 Structured Overview Chemistry Honors Chemistry kgm2/s2 (noticed when matter changes ) (composition, structure, & properties) joules Energy Matter (possesses inertia) (the ability to do work) FxD units Types Homogeneous Heterogeneous (uniform properties) (uneven properties) Kinetic Potential (energy of motion) chemical vs. physical intensive vs. extensive (stored energy) amount makes a difference ½ mv2 New substance formed to notice it Pure Substances Definite Composition Forms Mixtures Chemical Physical blend No set ratio Property retention Physical change 100% of one thing Mechanical Elements Yes! No! Heat one kind of atom Chemical change Light Compounds Separation? Yes! Sound (Know the techniques.) more than one kind of atom Electrical Set ratio, Chemical blend, New properties

6. Which of the following is an example of a qualitative observation? A) A piece of wood is 5.3 cm long. B) Solution 1 is much darker than solution 2. C) The volume of liquid in beaker A is 4.3 mL D) The temperature of the liquid is 60°C. E) none of these

7. Express 784000000 in scientific notation. A) 7.84 x 106 B) 7.84 x 108 C) 78.4 x 107 D) 784 x 106 E) 784 x 107

8. Measured quantities, such as length, mass, or time, can best be described as: A) sometimes certain. B) always certain. C) always uncertain. D) sometimes uncertain.

9. A scientist obtains the number 1250.37986 on a calculator. If this number actually has four (4) significant figures, how should it be written? A) 1251 B) 1250.3799 C) 1250.4 D) 1.250 x 103 E) 1.250 x 10–3

10. A piece of indium with a mass of 16.6 g is submerged in 46.3 cm3 of water in a graduated cylinder. The water level increases to 48.6 cm3. The correct value for the density of indium from these data is: A) 7.217 g/cm3 B) 7.2 g/cm3 C) 0.14 g/cm3 D) 0.138 g/cm3 E) more than 0.1 g/cm3 away from any of these values.

11. The SI System Units Fundamental Derived Mass, kg Volume, Length3, m3, cm3, dm3, L ,mL Length, m (L= 1 dm3; 1 cm3= 1mL) Time, s Density, M/V, g/cm3 Temp, K (°C+273) Energy, F*D, N*m kg m2/s2 (Joule, J) Amount, mole Current, A 1 calorie = 4.184 J

12. What is the boiling point of methanol, in Kelvins, if the temperature in centrigrade (also called Celcius) is 66°C? A) -207 K B) 273 K C) -66 K D) 339 K E) not enough information is given.

13. Foundations (Measurement & Calculation) Chapter 2 Structured Overview H Chemistry • Big Bang • Natural Selection • Atomic • Gravity • Conservation of Mass Laws Science Seen again and again The Scientific Method Theory Observations Grand (Facts) Hypothesis Experiments (Explanation) (Tests) Quantitative Qualitative (Measurements) (Nature) Dimensional Analysis Scientific Notation Uncertainty S.I. System Write it percent error = Meas. – True True Value Precision v. Accuracy Units Prefixes Calculate w/ it Sig Figs (9) X 100% (7) Derived Fundamental (estimate one place) With devices dm3, L, or cm3 Volume (LxLxL) Zero Rules Force (D=m/V) Density kg m/s2 (F=ma) Calculate with g/cm3

14. The scientist who discovered the charge on the electron was A) J. J. Thomson. B) Robert Millikan. C) Ernest Rutherford. D) William Thomson. E) John Dalton.

15. The element rhenium (Re) exists as two stable isotopes and 18 unstable isotopes. Rhenium-185 has in its nucleus A) 75 protons, 75 neutrons. B) 75 protons, 130 neutrons. C) 130 protons, 75 neutrons. D) 75 protons, 110 neutrons. E) not enough information is given.

16. The element magnesium (Mg) exists as three isotopes. They are shown below with their atomic masses and their relative abundances: 24Mg 23.9850 amu (78.99%) 25Mg 24.9858 amu (10.00%) 26Mg 25.9826 amu (11.01%) What is the atomic mass of magnesium on the periodic table? A) 23.9850 amu. B) 24.9845 amu C) 24.3050 amu

17. 20Ca2+ has A) 20 protons, 20 neutrons, and 18 electrons. B) 22 protons, 20 neutrons, and 20 electrons. C) 20 protons, 22 neutrons, and 18 electrons. D) 22 protons, 18 neutrons, and 18 electrons. E) 20 protons, 20 neutrons, and 22 electrons. 40

18. By knowing the number of protons a neutral atom has, you should be able to determine A) the number of neutrons in the neutral atom. B) the number of electrons in the neutral atom. C) the name of the atom. D) two of the above. E) none of the above

19. If an atom of polonium (atomic number 84) undergoes a conversion to lead (atomic number 82) by the loss of a single particle, A  the particle lost was an alpha particle   B  the particle lost was a gamma ray       C  the particle lost was a beta particle          D  the particle lost could have been an alpha particle or a beta particle E  the particle lost was a positron

20. 0.98 g Li is equal to how many moles of Li and how many atoms of Li? A  8.6 mol; 6.0 x 1023 atoms   B  0.14 mol; 8.6 x 1022 atoms       C  0.14 mol; 6.0 x 1023 atoms      D  8.6 mol; 8.6 x 1022 atoms E  you can’t tell both quantities

21. Chapter 3... HChem. Use D.A. countingthem The Atom The MOLE Hard Little Spheres 1 mole = 6.02 x 1023 = molar mass History John Dalton Ernest Rutherford J. J. Thomson Planetary Model Proust Laviosier Gold Foil Exp. Law of Definite ______ Cathode Ray Tube Exp. Law of ______ Democritus Conservation Compostion Plum Pudding Atom is mostly… The electron (negatively charged matter) Nucleus (positive, dense core) empty model Atomic Theory These can be lost or gained Atoms are indivisible Nucleons ions 1.76x108 C/g 1.6x10-19 C Chadwick Atoms rearrange in chem rxtions e-/m ratio Charge on the electron ________ Oil-Drop Exp. All matter is comprised of atoms protons neutrons Atoms of different elements have different masses (no charge) Millikan’s (+ charge) Atomic # Mass # Ionizing radiation matter Z mass of e- A Element-A 9.11x10-28 g nuclide AX Alpha A particular atom Mass Spec. A group of Beta (Energy) Atomic masses z Gamma Weighted Averages isotopes Equations to describe these radioactive Most are…

22. Example Scenario Problem: Barack and Michelle, graduate students at the University of Chicago in the Metallurgy Dept., were rummaging through the supply room searching for metals to use in their upcoming experiment. Barack found a 10.0 gram sample of gallium in a container that had a label on it that read density = 5.91 g/cm3, and placed it in Michelle’s hand only to find that the metal melted in her palm. 1.) When gallium melts, the change associated with the process is A  physical and endothermic   B  physical and exothermic       C  chemical and endothermic      D  chemical and exothermic

23. Example Scenario Problem: Barack and Michelle, graduate students at the University of Chicago in the Metallurgy Dept., were rummaging through the supply room searching for metals to use in their upcoming experiment. Barack found a 10.0 gram sample of gallium in a container that had a label on it that read density = 5.91 g/cm3, and placed it in Michelle’s hand only to find that the metal melted in her palm. 2.) The temperature that Gallium melts is 303 K. That temperature on the centigrade scale is A  576 °C   B  303 °C       C  100. °C      D  30. °C E 0.0 °C

24. Example Scenario Problem: Barack and Michelle, graduate students at the University of Chicago in the Metallurgy Dept., were rummaging through the supply room searching for metals to use in their upcoming experiment. Barack found a 10.0 gram sample of gallium in a container that had a label on it that read density = 5.91 g/cm3, and placed it in Michelle’s hand only to find that the metal melted in her palm. 3.) If Michele poured the liquid gallium into a graduated cylinder what volume should she have found? A  59.1 mL   B  0.591 mL       C  1.69 mL      D  0.0591mL E 16.9 mL

25. Example Scenario Problem: Barack and Michelle, graduate students at the University of Chicago in the Metallurgy Dept., were rummaging through the supply room searching for metals to use in their upcoming experiment. Barack found a 10.0 gram sample of gallium in a container that had a label on it that read density = 5.91 g/cm3, and placed it in Michelle’s hand only to find that the metal melted in her palm. 4.) If Michele poured the liquid gallium into a graduated cylinder and actually found 1.58 mL for the volume, what would’ve been her percent error? A  13%  B  1.6 %       C  4.2 %      D  0.69 % E 6.5 %

26. Which of the following frequencies corresponds to light with the longest wavelength? A) 3.00 x 1013 s–1 B) 4.12 x 105 s–1 C) 8.50 x 1020 s–1 D) 9.12 x 1012 s–1 E) 3.20 x 109 s–1

27. What is the energy of a photon of blue light that has a wavelength of 450 nm? A) 6.7 x 1014 J B) 4.4 x 10–19 J C) 1.5 x 105 J D) 1.01 x 1048 J E) 5.8 x 10–19 J

28. Define the term atomic orbital as best you can….. High probability region in space where you’re likely to find an electron!

29. How many d orbitals have n = 3? A) 2 B) 5 C) 10 D) 7 E) 18

30. How many electrons can be in the 1s orbital? ____ 2s? ____ 6s? ___ 2 2 2 How many electrons can be in the 2p orbitals? ____ 3d? ____ 3f ? ___ 6 10 0 What is the shape of the 1s orbital? ________ 6s? ________ spherical spherical What is the shape of the 2p orbital? ________ 3d? ________ Clover (mostly) dumbbell

31. Write the electron configuration notation for the element Indium 1s22s22p63s23p64s23d104p65s24d105p1

32. Which of these elements has three electrons in degenerate orbitals?           A  Po          B  P          C  Hg          D  Si          E  Pd

33. The Rutherford Model could not explain… The Atom…cont’d Chapter 4 H Chem The atom does not collapse The light emitted by atoms (Photo-electric effect) For hydrogen: (Young…Double Slit) (Planck / Einstein) Wave-like Particle-like Bright-Line Spectra 3.0 x 108m/s l x n = c (What atoms have to do with it) E = h n -1312 kJ wavelength En= frequency Speed of light Quantum of energy For H: mole e- n2 (photon) Bohr Model Wave Mechanical Model Planck’s Constant… 6.6x10-34J•s electrons can have only certain energies colors are emitted when electrons jump from higher to lower energy levels The observer affects the observed What DeBroglie said Therefore Heisenberg’s Uncertainty Principle If light has a dual nature…why not matter Energy levels exist Schroedinger (Proven by looking at Bright-Line Spectra) (Max Born) Electrons are waves of chance. Sub-levels exist Electrons are standing waves…only certain energies allowed orbitals These are called: Defined as: Shown with: 1. or 2. Aufbau s (1) p (3) d (5) f (7) High probability regions in space where the electron is likely to be found Config. Pauli Filling order for atoms with more than one electron Hund’s Orbital

34. Of the following elements, which one is most likely to form an ion through the loss of two electrons?           A  sulfur          B  aluminum          C  sodium          D  strontium          E  chlorine

35. An element having the configuration [Xe]6s1 belongs to the Group:    A  halogens      B  None of these           C  alkaline earth metals  D  alkali metals     E  noble gases

36. 1. Is phosphorous a metal or non- metal? 2.Write the orbital notation for the element phosphorous. 3. What is the charge on the phosphide ion? 4. How many neutrons are in a phosphorous atom? 5. Which is bigger, the atom or the ion? nonmetal 1s22s22p63s23p3 3- You can’t tell… the ion!

37. Of the following elements, which has the lowest first ionization energy? A) Ba B) Ca C) Si D) P E) Cl

38. Chapter 5 -- H. Chemistry The Periodic Table (repetition of behavior) Terms Dobereiner know the “groups” Based on Mass Families Triads Periods Newlands Metals/Nonmetals Octaves Metalloids “father” of the periodic chart Mendeleev ←Trends Blocks left blanks First Chart Isoelectronic Moseley Valence** Based on atomic number Periodic Law **outermost s and p electrons Metallic Reactivity Reasons (based on structure) Metallic Character Atomic Size Nuclear Charge know the transition to these Ionic Size across Charge Higher Energy Levels down Ionization Energy Electron Affinity

39. Which of the following name(s) is (are) correct? 1. carbon dioxide CO2 2. ammonium chloride NH4Cl 3. acetic acid HC2H3O2 (aq) 4. barium oxide BaO A) all B) none C) 1, 2 D) 3, 4 E) 1, 3, 4 What test is used to determine if a sample of gas is CO2?

40. What is the hybridization on each oxygen atom in a molecule of oxygen? A) sp B) sp2 C) sp3 D) dsp3 E) d2sp3

41. Which of the following molecules has a dipole moment? (i.e. is a polar molecule) A) BCl3 B) SiCl4 C) PCl3 D) Cl2 E) none of these

42. General Properties Chapter 6 Honors Chem. General Properties Insoluble in water Soluble in water Conductive in sol’n Chemical Bonding Nonconductive in sol’n Lower M.P.’s Higher M.P.’s Lowers energy of system IONIC...transfer Rationale: COVALENT...sharing Accompanied by: Accompanied by: Process (steps) I.E A Blend E.A How to tell Pauling L.E. Polar Covalent… unequal sharing Person Responsible Electro- negativity 0.4-1.7 >1.7 0.0 – 0.3 differences 2-D Lewis Structures Resonance ^and 3-D** Guidelines • Count d-d+ • Connect Exceptions to octet rule Polarity of bonds Multiple Bonds • Distribute

43. Honors Chem. Molecular Shapes dictated by nonpolar polar (symmetrical) (nonsymmetrical) Polarity of Molecules V S E P R Theory shows (when atom arrangements vary) air alence isomerism **3-D Lewis Structures hell lectron epulsion from this you resonance CH4 (when one bonding arrangement is insufficient) NH3 H2O can create BF3 109.5° angles 107° angles 104.5° angle 120° angles Example# of bonds**# of lone pairsEPAShapeHybridization CH4 0 4 SO2 tet. tetrahedral sp3 1 3 NH3 trig. pyramidal tet. sp3 H2O 2 2 bent tet. sp3 <120° angle possible scenarios BF3 3 0 trig. planar trig. planar sp2 2 SO2 1 trig. planar bent sp2 CO2 2 0 linear linear sp 180° angle Multiple bonds count the same as single bonds **