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Entry Task: Jan 24 th -25 th Block 1

Entry Task: Jan 24 th -25 th Block 1. Turn in Entry task sheets 1 st Semester Review sheet out GRAB a Review Activity sheet (as you came in) Periodic Table out. Chemistry Final Review Sheet. Chapter 2 – Data analysis (7 questions)

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Entry Task: Jan 24 th -25 th Block 1

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  1. Entry Task: Jan 24th -25th Block 1 Turn in Entry task sheets 1st Semester Review sheet out GRAB a Review Activity sheet (as you came in) Periodic Table out

  2. Chemistry Final Review Sheet

  3. Chapter 2 – Data analysis (7 questions) • Metric prefixes and how their relative comparisons: kilo-, deci-, centi-, milli- • Scientific notation • Significant figures • Conversion factor • % by mass • % error

  4. Chapter 3 – Matter- Properties and Changes (8 questions) • Physical properties and Chemical properties AND Physical and Chemical Changes • States of matter and their general properties • Law of conservation of mass • Elements, compounds, Molecules • Chapter 4 – Structure of the atom (8 questions) • Discoveries of subatomic particles (proton-neutron-electron)- Scientist- know the general overview of experiments • Charge, location, general mass considerations of the proton, neutron, electron • Atomic number verse mass number- what are they? What particles are involved? • Isotopes- what are they?

  5. Chapter 5 – Electrons in Atoms (11 questions) • How does the spectrum relate to the energy of an electron? • What is an electron cloud verse atomic orbital? • Electron Configuration and energy associated with where it is on the configuration • Ground state verse excited state and when does it gain energy verse release energy (light). • Octet rule and valence electrons • Valence electrons and electron configuration. • Rules to filling out electron configuration

  6. Chapter 6-7 – The periodic table and periodic law • (8 questions) and Elemental Families (7 questions) • Metals, metalloids, nonmetals- properties and locations • Cations verses anions- formation, charge, and size (compared with parent atom and each other). • Given a electron configuration- locate with period/group • Trends Ionization, electronegativity, size of atom and size of ion • Energy levels and periods • Transitional elements and synthetics • 4 major families- how do they differ in reactivity, periodic trends, charges and chem./physical properties.

  7. Chapter 8 – Ionic compounds (15 questions) • General ionic bonding- what is happening to cation and anion-electron wise and charge? • Balance charges using subscript AND Using the subscript in formulas as clues to charges on ions. • Name to formula AND formula to names- KNOW transitional roman numerals and when to use them. • Polyatomic ions- what are they? How to use the parentheses and read common ion sheet. • Properties of ionic substances. • Lattice energy

  8. Chapter 9 – Covalent compounds (17 questions) • General covalent bonding- What is it? What is happening to electrons? Double/Triple bonds and differences • Know your prefixes for naming molecules. Use prefixes from formula to provide the name. • VSEPR model descriptions of bonds and lone pairs to provide shape name. • Polarity (Electronegativity) polar vs. non-polar • Lewis dot structures • Chapter 10- Chemical Reactions (14 questions) • KNOW your types of reactions • Balance different equations • Predict products from clues provided by the reactants

  9. Review Game • Pair up and sit next to your partner. • Do this NOW! Sit next to each other • NOT in lab area. • NO SINGLES!!!!! OR TRIPLES!!! • You and your partner will get a numbered piece of paper with 2 questions on it.

  10. Review Game • Put your names on the Review squares sheet. • Right Now- Answer your questions on the Review square sheet with partner. • When the wheel spins, whatever number comes up decides whose question will go. • Each person answers a question. • The audience will write down answers on Review squares sheet.

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  13. Metals and non-metals Transfers electrons Creates ions which cancel each other out. Fill valence orbits for both atoms- stable compound Sulfur hexachloride

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  16. Nonconductive Most are gases at room temperature Does not react to acids Dull in appearance Does not lose valence electrons NCl4

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  19. Low # of ve- (less than 4) are metals Higher # of ve- (more than 4) are nonmetals Zn3(PO4)2 Zinc Phosphate

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  23. Li and Na (alkali family) Be and Sr (Earth alkali family) F and I (Halogen family) Ar and Xe (Noble gas family) S2F3

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  27. Not conductive if dissolved in water Most Do not dissolve in water Low melting point Composed of nonmetals Bonded by sharing electrons Tin IV acetate Sn(C2H3O2)4

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  30. Nonmetal properties gas no rx with acid nonconductive Group 17 period 3 Cl Selenium monofluoride

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  32. Conductive if dissolved in water Dissolve in water High melting point Composed of metals and nonmetals Bonded by transferring electrons creating a charge MnO2 Manganese IV oxide

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  35. Conductive Solids at room temperature React to acids Shiny in appearance Loses valence electrons easily Dinitrogen tetraoxide

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  38. Nonmetals Share ve- Both atoms have stable and filled ve- orbits Lead II hydroxide Pb(OH)2

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  41. The number of valence electrons increase as you move from left to right. Becoming more stable Metal Metalloid  Nonmetal Noble gas Mg3N2

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  45. Elements that have a filled valence orbit ( 8 electrons) have a stable arrangement. Hg3(BO3)2 Mercury II borate

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  49. Atoms in groups have same # of ve-. Atoms in periods have the same valence orbit NBr2

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