VOCABULARY define the following terms: Unit 1 Study Guide Honors Chem 1) Electron configuration- 2) Effective nuclear charge 3) Isotope 4) Ion 5) Anion 6) Cation - 7) Isoelectronic - 8) Halogens 9) Electronegativity - 10) Electron affinity 11) Ionization energy 12) Atomic radius- 13) Valence electrons- 14) Energy level 15) Orbital- 16) Intermolecular forces 17) Intramolecular forces- 18) Excited state 19) Ground state - 20) Orbital diagram 21) Periodic law 22) Covalent bond- 23) Polar bond- 24) Nonpolar bond 25) Ionic bond 26) Wavelength- 27) Frequency- 55 multi choice Q Hints: - study old quizzes -study practice worksheets & notes -study for understanding, not memorization BOND TYPE A. How do you know how many valence electrons an element has? B. How do you know what the ionic charge is for any element on the periodic table? C. How is an ionic bond different then a covalent bond? D. How can you distinguish an ionic compound from a covalent compound? E. What are the rules for naming ionic molecules? Naming covalent molecules? F. What are the rules for writing formulas for ionic compounds? Covalent compounds? G. Rank the bond types in order of strongest to weakest: ionic, nonpolar, metallic and polar.
H. How can you tell what of bond forms between two atoms? I. Explain how intermolecular forces are different then intramolecular forces? Why are both important? J. Rank the 4 bond types in order of highest melting and boiling points to lowest melting and boiling points. Explain why some molecules require more energy to melt/boil then others. K. Volatility is the ability of a substance to evaporate rapidly. For example, rubbing alcohol spilled on the bathroom counter will evaporate faster (more volatile) then water spilled on the bathroom counter. As vapor pressure increases, volatility increases. What happens to boiling point? ATOMIC STRUCTURE A. COMPLETE THE CHART. Subatomic particle Charge Relative size B. A PICTURE OF AN ION (label the nuclear charge, protons, neutrons, and electrons) C. DRAW A PICTURE OF TWO ATOMS THAT ARE ISOTOPES (label the protons, neutrons, and electrons) How are isotopes different? How are isotopes the same?
D. What is the relationship between wavelength and amount of energy released? E. What is the formula relating frequency and wavelength for light? F. Write the ground state and excited state electron configuration for phosphorous. G. Write the electron configuration and noble gas abbreviation, and orbital diagram for the following: i) Calcium ii) Neon iii) Tungsten iv) Seaborgium
PERIODIC TABLE TRENDS A. Color or label the following PERIODIC TABLE FAMILIES on the periodic table: -halogens -alkali metals -alkaline earth metals -noble gasses -transition metals -increasing reactivity B. Metal v. Nonmetal COLOR OR LABEL THE FOLLOWING -METALS -NONMETALS -METALLOIDS C. Trends LABEL THE FOLLOWING ON THE PERIODIC TABLE -increasing atomic radius -increasing effective nuclear charge -increasing ionization energy -increasing electron affinity -increasing electronegativity -valence electrons -ionic charge
PRACTICE QUESTIONS 1. MATCH THE ELEMENT TO ITS ELECTRON CONFIGURATION a) 1s 2 2s 2 2p 6 3s 2 3p 6 4s 2 3d 10 4p 6 5s 2 Sr Re b) [Ar] 4s 2 3d 3 V V c) 1s 2 2s 2 2p 6 3s 2 3p 6 4s 2 3d 10 4p 6 5s 2 4d 10 5p 6 Sr 6s 2 4f 14 5d 10 6p 4 Po Po d) [Xe] 6s 2 4f 14 5d 5 Re 2. RANK THE ELEMENTS IN ORDER OF HIGHEST ELECTRONEGATIVITY TO LOWEST Zn, Kr, Ca, Br Kr, Br, Zn, Ca 3. RANK THE ELEMENTS IN ORDER OF MOST REACTIVE TO LEAST REACTIVE Ca, Mg, Ba Ba, Ca, Mg 4. RANK THE ELEMENTS IN ORDER OF INCREASING EFFECTIVE NUCLEAR CHARGE Al, In, Ga In, Ga, Al 5. RANK THE FOLLOWNG ATOMS IN ORDER OF SMALLEST TO LARGEST RADIUS. Cu, Br, Ca Br, Cu, Ca 6. RANK THE FOLLOWING COMPOUNDS IN ORDER OF WEAKEST BOND TYPE TO STRONGEST BOND TYPE CH4, CuCl2, Cl2 Cl2, CH4, CuCl2, 7. A light wave has a wavelength of 500 nm? What is the frequency of the wave? 3.0 x 10 8 = (5 x10-7 m) f f = 6 x 10 14 Hz 8. Which of the following is the orbital diagram for an alkaline earth metal? D a. c. b. d. 9. Which of the following is the excited state electron configuration for Mg? C a. b. c. 10. HOW MANY VALENCE ELECTRONS DO THE FOLLOWING ATOMS HAVE? a. Carbon 4 b. Strontium 2 c. Iodine 7 d. Zinc 2
11. WHICH OF THE FOLLOWING ARE ISOELECTRONIC? (circle all that apply) Ar Ca +2 Mg +2 Kr Cl -1 12. WHICH OF THE FOLLOWING ARE ISOTOPES? (circle all that apply) a. Ca-40 and Ca-42 b. Ni-64 and Zn-64 c. Ag-107 and Au-197 and Ar-40 13. FROM THE FOLLOWING PROPERTIES LISTED, IDENTIFY THE ELEMENT a. high luster, 2 valence electrons, period 3 element Mg b. nonmetal, 3 energy levels, -1 ionic charge Cl 14. HOW MANY ELECTRONS ARE AT EACH ENERGY LEVEL FOR THE FOLLOWING ATOMS? A) Calcium (Ca) B) Tin (Sn) C) Cl -1 2,8,8, 2,8,18,2 2,8,18,18, 4 15. Identify as an ionic compound, polar covalent compound, or nonpolar covalent compound. a) CaCl2 IONIC c) F2 NONPOLAR e) KCl IONIC b) SO2 POLAR d) H2O POLAR -SUBTRACT THE ELECRONEGATIVIES TO ANSWER THIS QUESTION 16. Name the following compounds 17. NH 4ClO 3 d) Ca 3(PO 4) 2 g) N 2H 4 Ammonium chlorate calcium phosphate dinitrogen tetrahydride 18. MgBr 2 e) CaCO 3 h) Na 2SiO 3 Magnesium bromide calcium carbonate sodium silicate 19. NF 3 f) Fe(NO 3) 3 i) CuCl 2 Nitrogen trifluoride iron (III) nitrite copper(ii) chloride 20. Write formulas for the following compounds. (balance charges when necessary) a) Ammonium phosphate (NH 4) 3PO 4 f) calcium nitrite Ca(NO 2) 2 b) potassium chromate K 2CrO 4 g) manganese (IV) chloride MnCl 4 c) Dinitrogen pentoxide N 2O 5 h) carbon tetrabromide CBr 4 d) tetraphosphorous decasulfide P 4S 10 i) Potassium sulfate K 2SO 4 e) Silver acetate AgC 2H 3O 2 j) dinitrogen monoxide N 2O f) k) sodium phosphide Na 3P