Ch. 1: Introduction to Chemistry. Ch. 2: Matter and Change

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1 Review Sheet for Chemistry First Semester Final Refer to your class notes, worksheets, and the textbook to complete this review sheet. Study early so that you will have time to ask questions about what you don t understand. For the exam, you will need to bring 2 number 2 pencils, a scientific calculator (there will be NO sharing and NO cell phones for calculations) and you may bring a 4x6 card with formulas, equations etc that you feel you need. This will be collected with your test and must have your name on it. (MUST be a 4x6 CARD, no paper cut to 4x6- MUST be HAND written) Things you need to know: In addition to the sections below: SI Base Units- Pg 73 Metric Prefixes- Page 74 Know how to convert from one unit to another (ie: kilometers to millimeters) KNOW YOUR ELEMENTS The ones you were tested on! (name, symbol and spelling counts!) KNOW the Polyatomic Ions on Pg 257 (charge, name, formula) KNOW the Common Metal Ions with more than one charge (table on page 255) KNOW the Prefixes for Covalent molecule names (page 269) BE ABLE TO USE the Significant Figures rules Ch. 1: Introduction to Chemistry manipulated (independent) variable responding (dependent) variable observation theory steps in scientific method problem solving in chemistry Ch. 2: Matter and Change chemical change gas mixture solid chemical property heterogeneous mixture phase solution chemical reaction homogeneous mixture physical change substance compound conservation of mass physical property vapor element liquid product volume filtration mass reactant Properties of Matter Mixtures Elements and Compounds Chemical Reactions Matter: Anything that takes up space and has mass Physical Changes and Chemical Changes Define each. How can you tell the difference between the two?

2 Classify the following as physical or chemical changes: a. spoiling of milk b. bending wire c. cutting paper d. rusting of a nail Identify the following as pure substances, homogeneous mixtures or heterogeneous mixtures: a. copper b. sweetened tea c. sand and water d. calcium carbonate (CaCO 3 ) Sketch particles in the three states of matter. How close are the particles and how much do they move? Solid Liquid Gas Calculations using the Law of Conservation of Mass for Reactions 4g H 2 +?? g O 2 36g H 2 O Ch. 3: Scientific Measurement absolute zero International System scientific notation accepted value of Units (SI) significant figures and rules Celsius scale joule (J) weight vs. mass density Kelvin scale (K) energy kilogram (kg) error liter (L) experimental value meter (m) gram percent error Be able to calculate percent error, density, and convert between Kelvin and Celsius Be able to convert between scientific notation and decimal or integer numbers Identify the number of sig figs; addition, subtraction, multiplication and division with sig figs. Ch. 4: Atomic Structure atom atomic mass atomic mass unit electron group in Periodic Table isotopes mass number neutron proton period in Periodic Table

3 Be able to find the atomic mass and atomic number on the Periodic Table. Be able to calculate the number of neutrons. Know how to identify the number of electrons. Know how to identify isotopes and write their formulas. Atom 14 For this Carbon 14 isotope, 6 C Atomic number =, Mass number =, # of protons =, # of electrons =, # of neutrons =. Atomic Masses: What is the difference between the mass number for Carbon 14 and carbon s atomic mass of amu? Calculate the atomic mass of lithium is one isotope has a mass of amu and a percent abundance of 7.59% and a second isotope has a mass of amu and a percent abundance of 92.41%. Ch. 5: Models of the Atom atomic orbitals aufbau principle electromagnetic radiation electron configurations energy levels ground state of electron sublevels types of sublevels (s, p, d, f) Hund s Rule photons quantum Pauli exclusion principle spectrum principal energy level Heisenberg uncertainty principle (Honors) Be able to identify the electron configuration of elements. Electron Configurations. What element has the electron configuration [Ne]3s 2 3p 1? What does the 3 mean in 3s 2? What does the s mean? What does the 2 mean? How many valence electrons will an atom of this element have? How many electrons will an atom of this element lose to form an ion? Why? Write out the orbital configuration according to the Aufbau principle, Hund s rule and the pauli exclusion principle.

4 Emission (or bright-line) Spectrums (Honors only) What is needed for an electron to jump to a higher energy level? What happens when an excited electron falls back to its ground state? What does an emission spectrum allow one to do? Characteristics of subatomic particles Particle Mass Charge Location in atom Proton Neutron Electron Ch. 6: The Periodic Table alkali metals electronegativity metals alkaline earth metals halogens noble gases anion inner transition metals nonmetals atomic radius ionization energy transition metals cation metalloids Know the four periodic trends of ionization energy, electronegativity, ionic size and atomic size. Periodic trends Locate or define parts of the periodic table: Groups Periods Transition metals (d & f blocks) vs. Representative Elements (s & p blocks) Alkali metals, Alkaline Earth metals, Halogens, Noble Gases

5 Periodic Trends: Increasing or Decreasing from top to bottom or left to right? electronegativity Top to Bottom in a Group Left to Right across a Period ionization energy atomic size Ionic size Elements in the same have similar physical and chemical characteristics because the (group, period) they have the same number of. (atoms, protons, neutrons, electrons, valence electrons) Draw a electron dot diagram (or Lewis Dot structure) for Be and for N correct number of valence electrons showing the Be From their positions on the periodic table, what charges would the ions of Be and N have? Gains or loses electrons? Symbol for ion Gains or loses electrons? Symbol for ion N Properties of Metals vs. Nonmetals vs. Metalloids Metals Nonmetals Metalloids Luster? Malleable vs. Brittle Conducts electricity & heat? Typical state(s) at room temperature

6 Ch. 7: Ionic and Metallic Bonding chemical formula ionic compounds p. 192 Common Anions electron dot structure for ions metallic bonds halide ion octet rule ionic bonds valence electrons Key concepts: Ions Ionic Bonds and Ionic Compounds Bonding in Metals Ch. 8: Covalent Bonding covalent bond molecule triple covalent bond coordinate covalent bond nonpolar covalent bond unshared electron pair diatomic molecule polar bond structural bond double covalent bond polar covalent bond molecular formula hydrogen bonds polyatomic ion single covalent bond molecular compound electron dot structures VSPER Key concepts: 8.1 Molecular Compounds 8.2 Nature of Covalent Bonding (8.3 Honors) 8.4 Polar Bonds and Molecules Ionic vs. Molecular Compounds: Ionic bonds are formed when a and a combine. Metals lose electrons and form while nonmetals gain and electrons form. Molecular compounds form when a and a combine as they share electrons. Identify the following pairs of atoms as potentially forming an ionic or molecular compound: Mg and Cl Ag and S I and F P and Cl K and Br Sn and O

7 Covalent Bonding in Molecules Draw Lewis Structures (dot diagrams) for HCl, H 2 S, CH 2 Cl 2, and O 3. Use Lewis Structures to predict molecular shapes and polarity of molecules Identify shapes of the molecules as: Linear, Bent, Pyramidal, Trigonal Planar, or Tetrahedral. Use electronegativity values to determine if the individual bonds in the molecules above are polar. Look at the polarity of the bonds and the symmetry of the molecules above to determine if the molecules are polar (if one side of the molecule will be more negative than another). H 2.1 Li 1.0 Na 0.9 K 0.8 Be 1.5 Mg 1.2 Ca 1.0 B 2.0 Al 1.5 Ga 1.6 C 2.5 Si 1.8 Ge 1.8 N 3.0 P 2.1 As 2.0 O 3.5 S 2.5 Se 2.4 F 4.0 Cl 3.0 Br 2.8 He Ne Ar Kr Electronegativity Difference (x) 0.0 x 0.4 Type of Bond Non polar covalent 0.4 < x < 2.0 Polar covalent 2.0 x Ionic Lewis Structures & Total # of Valence Electrons Structural Formula N 2 HCl H 2 S CH 2 Cl 2 O 3 How do you know if a Bond is polar or nonpolar? How do you know if a molecule is polar or nonpolar? Properties of Ionic and Molecular Compounds Molecular Compounds Ionic Compounds Combination of elements involved (metals? nonmetals?) How is bond formed?

8 Typical state(s) at room temperature Melting and boiling points (relatively high or low?) Conduct electricity if dissolved in water? Ch. 9: Chemical Names and Formulas Know how to name ionic compounds, molecular compounds, and polyatomic ions. p. 257 Naming Molecular and Ionic Compounds Naming molecular compounds Name: N 2 O: and NO 2 Naming Ionic Compounds Name: Li 2 O and (NH 4 ) 2 SO 4 Name: FeO and Sn 3 (PO 4 ) 4 Name: NaHCO 3 and CuCl 2 Formulas of Molecular and Ionic Compounds Write formulas for the following molecular compounds: Water silicon dioxide Phosphorous trihydride dioxygen difluoride Lead (II) hydroxide chromium (III) sulfate

9 Write formulas for: Ba 2+ with OH iron (III) sulfide Na + with OH NH + 4 with PO 3 4 oxide magnesium

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