Name Date Period Chemistry Final Exam Review Packet - Fall 2014

Transcription

1 Name Date Period Chemistry Final Exam Review Packet - Fall 2014 Periodic Table and Atomic Structure Physical properties can be intensive or extensive. Intensive properties do not change with amount of substance (Ex: color, melting point). Extensive properties do change with amount (Ex: mass, volume). Classify the following properties as extensive or intensive. mass ductility melting point color length conductivity shape smell hardness PAGE 9 OF YOUR NOTEBOOK Metals vs. Nonmetals Match the description on the left with the appropriate letter on the right. 1. Tend to form anions. 2. Good conductors of heat and electricity. A. metals 3. Found on the left side of the Periodic Table. B. nonmetals 4. Tend to form cations C. metalloids 5. Solids that tend to be brittle. 6. Malleable (bendable) 7. Lustrous (shiny) 8. Found along the staircase between metals & nonmetals 9. Found on the right side of the period table 10. Ductile (can be drawn into wires) FAMILIES / GROUPS OF THE PERIODIC TABLE PERIODIC TABLE (back cover) & PG Have characteristics of both metals and nonmetals 12. Poor conductors of heat and electricity

2 Match the property with the correct term. Each term can be used once, or more than once. indefinite volume and shape definite volume, indefinite shape particles can move/slide past one another definite volume and shape S - Solid G - Gas L - Liquid 3 phases of matter rigid - particles locked into place compressible lots of free space between particles PAGE 6, 7, & 8 not compressible little free space between particles flows easily does not flow easily Elements Periodic Table Groups: Vertical columns Also called Contains elements with similar Periods: Horizontal rows Atomic numbers from left to right across a period Dimitri Mendeleev: of the Periodic Table Arranged the elements based on density, atomic and Henry Moseley Arranged elements based on

3 Groups (Families) of the Periodic Table Group IA or 1 A. Name B. Members C. Valence electron configuration D. Properties E. Part of the -block Group 2A or 2 A. Name B. Members C. Valence electron configuration D. Properties E. Part of the -block Groups 3B through 2B or 3 through 12 A. Name given these groups as a whole B. Examples C. Properties D. Part of the -block Group 7A or 17 A. Name B. Members all nonmetals C. Valence electron configuration D. Tend to form ions with charge. FAMILIES / GROUPS OF THE PERIODIC TABLE PERIODIC TABLE (back cover) ORBITALS ON THE PERIODIC TABLE PERIODIC TABLE (back cover) & PG. 12

4 Group 8A or 18 A. Name or sometimes called inert gases, though most can be made to react. B. Members C. Properties A.Atomic Radius atomic radius indicates relative of the atom Atomic radius generally as you move down a group. This is mainly due to succeeding being filled. Atomic radius generally as you move across a period from left to right. This is mainly due to. B. Ionic Radius A positive ion is known as a. It is an atom that has electrons. A negative ion is known as a. It is an atom that has electrons. Ion radius generally as you move down a group. This is mainly due to succeeding being filled. Cation radius generally as you move across a period from left to right. This is mainly due to. Anion radius generally as move across a period from left to right. This is mainly due to. C. Ionization Energy Ionization energy is defined as the amount of energy required to remove an from an atom, producing a (a positively-charged ion). Ionization energy as you move down a group. This is mainly due to the. Ionization energy as you move left to right across a period. This is mainly due to. D. Electronegativity Electronegativity is defined as the tendency for atoms of the element to attract when they are chemically combined with atoms of another element. Electronegativity as you move down a group. This is because the from the nucleus is. Electronegativity as you move left to right across a period. This is mainly due to the. PAGE 30, 31, 32, 35 PAGE 30, 38 PAGE 30, 33, 37 PAGE 30, 39

5 PAGE 11 III. Subatomic Particles and Isotopes Isotopes are atoms of the same element that have the same number of, but different number of. Fill in the chart for the following isotopes: PAGE 10, 11 Isotope Name Nuclear Symbol Atomic Number Mass Number # of Protons # of Neutrons # of Electrons 1. calcium Average atomic mass is the average of the atomic masses of the naturally-occurring of an element. It is what is shown on the.to calculate a weighted average: multiply the mass of each isotope by its % abundance then take the sum of the above for all isotopes PAGE 11

6 Modern Atomic Theory and Electron Configuration SIGNIFICANT FIGURES Round the number at left to the number of significant figures stated in each column. Number Four significant figures Three significant figures Two significant figures ,058,268 PAGE 26 One significant figure Write the numbers below in scientific notation Number ,058,268 Scientific Notation ELECTRON CONFIGURATION Complete the following: Atom Atomic # Short hand Electron Configuration Calcium # of protons # of e- Valence Electron Electrons lost or gained Lost # of e - lost or gained Cation or Anion 2 cation Ion Not. [Ne]3s 2 3p 6 8 Group 18 INERT 9 Gain 1 Anion PERIODIC TRENDS PERIODIC TABLE (back cover) PAGE 10, 17, 18, 19, 20, 21, 22

7 Match the following [Ne] 3s 2 3p 5 1s 2 2s 2 2s 6 3s 2 3p 5 different number of neutrons Number of Protons Loss of electrons Gain of electrons Cl Number of Protons and Neutrons A. Electron configuration B. Bohr Model C. Isotope D. Atomic Number E. Cation F. Lewis dot structure G. Short hand electron configuration H. Bohr electron configuration I. Isotope Symbol J. Atomic Mass K. Anion PERIODIC TRENDS PERIODIC TABLE (back cover) PAGE 10, 17, 18, 19, 20, 21, 22 Label the following: 1s 2 2s 2 2p 6 3s 2 3p 3 PAGE 19 How do you write the short -and electron configuration? 1) Step 1: PAGE 20, 22 2) Step 2: Complete the following for Iodine: Electron Configuration: Short hand Electron Configuration: Valence Electrons: Lewis Dot: How can you determine valence electrons using the periodic table: PERIODIC TRENDS PERIODIC TABLE (back cover)

8 Complete the following table. PAGE 10, 20, 22 Element Electron Configuration Short-hand Configuration Lewis Dot Diagram Bohr Model Bohr electron configuration P F Mg HISTORY OF THE ATOM Identify the correct answer choice by circling the scientist and name of the experiment or idea. PAGE 13, Main points: All elements are composed of tiny indivisible particles called atoms Atoms of the same element are identical & atoms of different elements are different Atoms combine in predictable ratios to make compounds Atoms are rearranged in chemical reactions Scientist: (John Dalton or Demitri Mendeleev) Circle the correct answer choice Idea: (Atomic Theory or Oil Drop Experiment) Circle the correct answer choice 2. Main points: By adding a electric field, he found that the moving pieces were negative Discovered that every atom has a negative particles called electrons Proposed the plum pudding model Scientist:(John Dalton or JJ Thompson) Circle the correct answer choice Experiment:(cathode ray tube & plum pudding Model or oil drop experiment)circle the correct answer choice

9 3. Main points: Said electrons travel in orbits i. Central nucleus with electrons located in rings ii. Considered the Hydrogen atom Scientist: (Niels Bohr or Robert Millikan) Circle the correct answer choice Idea: (Plum pudding or Bohr Model) Circle the correct answer choice 4. Main Points: Matter is not infinitely divisible smallest particles called atomos Scientist: (Robert Millikan or Democritus) Circle the correct answer choice 5. Main points: Measured the mass of an electron i. 1/1840 the mass of a hydrogen atom ii. Oil Drop Experiment Scientist: (Robert Millikan or JJ Thompson) Circle the correct answer choice 6. Main points: Shot alpha (+) particles at a thin gold foil Most of the particles traveled straight through but some were deflected Scientist: (Ernest Rutherford or JJ Thompson) Circle the correct answer choice Experiment: (Gold Foil or Cathode Ray) Circle the correct answer choice 7. Main points: Showed there was a second particle in the nucleus Neutron no charge Scientist: (Ernest Rutherford or James Chadwick) Circle the correct answer choice 8. Experiments: Fill in the blank using the following: Bohr model, oil drop, gold foil, cathode ray, plum pudding

10 THE ELECTROMAGNETIC SPECTRUM AND PLANCK S CONSTANT Electromagnetic radiation is energy that travels in waves. Two types of electromagnetic waves are microwaves and gamma rays. Gamma rays have a shorter wavelength than microwaves. Which of these statements is true? a. Gamma rays travel faster than microwaves. b. Gamma rays have more energy than microwaves do. c. Gamma rays have a lower frequency than microwaves do. d. Gamma rays, but not microwaves, can travel through a vacuum. PAGE 23, 24, 25 What is the relationship between frequency and wavelength for electromagnetic waves? a. A. Frequency equals wavelength. b. B. As frequency increases, wavelength increases. c. C. As frequency increases, wavelength decreases. d. D. The relationship depends on the speed of the wave Microwaves are used to transmit information. What is the wave length of a microwave having a frequency of 2.94x10 9 Hz. Record bubble your answer to the thousandth place in the griddable below. PAGE 28 Tiny water drops in the air disperse the white light of the sun into a rainbow. What is the energy of a photon from the violet portion of the rainbow if it has a frequency of 6.86x10-4 s- 1? PAGE 28

11 Fill in the following table: You must show all your work for full credit. PAGE 28 Wavelength (m) Frequency (Hz) Energy (J) x x 10-7 Label the parts of the wave: (amplitude, wavelength, trough, and crest) PAGE 23, 24, 25 Looking at the diagram above, answer the following questions. What type of wave has the highest frequency? What type of wave has the longest wavelength? What type of wave has the lowest frequency? What type of wave has the shortest wavelength?

12 As the wavelength increases the frequency (increases or decreases)(circle one) Which type of wave has the highest energy? Which type of wave has the lowest energy? Predict the type of bonding that would occur between the following pairs of elements. Ionic = cation (metal or NH 4+ ) and anion (nonmetal or polyatomic ion) Covalent = two or more nonmetallic elements PAGE 46 A) carbon and oxygen B) copper and chlorine C) sodium and fluorine D) potassium and bromine E) carbon and chlorine F) fluorine and bromine PAGE 44, 45, 47, 48 Name of Compound Cation Anion Formula lithium sulfide aluminum oxide lithium carbonate iron (II) sulfide zinc phosphate calcium nitride Write the formulas of the following compounds. Pb 2+ - NO 3 + NH 4 OH - Na + - HCO 3 Mn CrO 4 BaF 2 BaSO 4 AgC 2H 3O 2 Mg(ClO 2) 2 PAGE 44, 45, 47, 48 1) ammonium phosphate 2) iron (II) oxide 3) carbon monoxide 4) calcium chloride 5) potassium nitrate 6) magnesium hydroxide 7) aluminum sulfate 8) copper (II) sulfate 9) lead (IV) chromate 10) diphosphorouspentaoxide

13 IONIC BONDING: PAGE 41, 43 Ionic bonding occurs when a metal transfers one or more electrons to a nonmetal in an effort to attain a stable octet of electrons. For example: Practice: Show the transfer of electrons in the following combinations. 1. Potassium and Fluorine Chemical Formula 2. Magnesium and Iodine Chemical Formula 3. Beryllium and Sulfur Chemical Formula 4. Sodium and Oxygen Chemical Formula 5. Aluminum and Bromine Chemical Formula

14 COVALENT BONDING: PAGE 51, 52 Covalent bonding occurs when two or more nonmetals share electrons, attempting to attain a stable octet of electrons. For example: PRACTICE: Show how covalent bonding occurs in each of the following pairs of atoms. Atoms may share one, two, or three pairs of electrons. 1. Hydrogen and Hydrogen (H 2) 2. Fluorine and Fluorine (F 2) 3. Oxygen and Oxygen (O 2) 4. Nitrogen and Nitrogen (N 2) 5. Carbon and Oxygen (CO 2) 6. Hydrogen and Oxygen (H 2O)

15 A metallic bond exist because of PAGE 40, 42, 46 A. Weak electrostatic attraction between the negatively charged metal atoms and negatively charged sea of electrons. B. Weak electrostatic attraction between the positively metal atoms and negatively charged anion. C. Strong electrostatic attraction between the positively charged metal atoms and negatively charged anion. D. Strong electrostatic attraction between the positively charged metal atoms and the negatively charged sea of electrons. Using VSEPR Theory, sketch the shape of the following molecules; include the molecular and electronic geometry using the VSEPR chart. Structural Pairs Bonded Pairs (σ) Lone Pairs Molecular Geometry Structure Bond angle Linear Trigonal 120 planar 2 1 Bent < Tetrahedral Trigonal pyramidal < Bent << 109.5

16 1. N 2 Sketch: Electronic Geometry: PAGE 56, 57 Molecular Geometry: 2. H 2O Sketch: Electronic Geometry: Molecular Geometry: 3. CO 2 Sketch: Electronic Geometry: Molecular Geometry: 4. NH 3 Sketch: Electronic Geometry: Molecular Geometry: 5. CH 4 Sketch: Electronic Geometry: Molecular Geometry: 6. H 2S Sketch: Electronic Geometry: Molecular Geometry: 7. BF 3 Sketch: Electronic Geometry: Molecular Geometry:

17 Identify whether each of the following is a chemical (C) or physical (P) change A small pond freezes over in the winter PAGE 59 Pure iron is melted into a liquid A firework explodes in the sky Copper sulfate and ammonia are combined and a precipitate is formed NaCl is dissolved in water Balance and label the reaction as synthesis, decomposition, single replacement, or combustion. What kind of reaction is this? PAGE 58, 61 Cu(OH) 2 CuO + H 2O What kind of reaction is this? Ca + O 2 CaO What kind of reaction is this? C 4H 10 + O 2 CO 2 + H 2O What kind of reaction is this? AlCl 3 + Cu CuCl 2 + Al

18 1) Given the following chemical reaction PAGE Identify the following: Oxidation: Oxidizing agent: Reduction: Reducing agent: 2) Balance the following chemical reaction. Identify the following: Oxidation: Oxidizing agent: Reduction: Reducing agent: 3) Identify the type of redox reaction: : PAGE 58, 61 : :