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- 1. The Moment of Truth Chemistry Style!
- 2. The electron configuration of iron is [Ar]4s 2 3d 6 . What is the electron configuration for Fe 2+ ? <ul><li>[Ar]3d 6 </li></ul><ul><ul><li>Valence electrons are in the highest energy level! </li></ul></ul>
- 3. Which Alkali Metal has the largest radius? <ul><li>Francium </li></ul><ul><ul><li>Atomic Radius increases down a group! </li></ul></ul>
- 4. What is the abbreviated electron configuration of the sulfide ion? <ul><li>[Ar] </li></ul><ul><li>Sulfide is S 2- </li></ul><ul><li>When forming ions, main group elements obtain noble gas configurations! </li></ul>
- 5. Where are the most electronegative elements found on the periodic table? <ul><li>Top Right Corner </li></ul><ul><li>These are the smallest atoms and are the most reactive nonmetals! </li></ul>
- 6. What is the ground state electron configuration of the element with atomic number 41? <ul><li>1s 2 2s 2 2p 6 3s 2 3p 6 4s 2 3d 10 4p 6 5s 2 4d 3 </li></ul><ul><li>Atomic number 41 means 41 protons. </li></ul><ul><li>In a neutral atom the number of protons and electrons are equal! </li></ul>
- 7. In a group, how does mass effect the number of core electrons? How does it effect the number of valence electrons? <ul><li>As mass increases in a group so does the number of core electrons. </li></ul><ul><li>All elements in a group have the same number of valence electrons no matter what the mass is! </li></ul>
- 8. Which element has the highest electronegativity? Cl, Ca, Sn, or Po <ul><li>Cl! It is the smallest atom! </li></ul><ul><li>Since electronegativity and ionization energy follow the same pattern, Cl also has the highest first ionization energy! </li></ul>
- 9. What is the symbol for an element with 12 protons, 13 neutrons, and 10 electrons? <ul><li>Mg 2+ </li></ul><ul><li>Protons ALWAYS determine the identity of a atom or ion! </li></ul><ul><li>The difference between the number of protons and electrons determines the charge! </li></ul><ul><li>Neutrons can vary and only effect the mass number. </li></ul>
- 10. Give an example of a compound with ionic and covalent bonding. <ul><li>Na 2 SO 4 </li></ul><ul><li>Polyatomic ions always contain covalent bonding because they are made of nonmetals. </li></ul><ul><li>The cation and the polyatomic ion bond together ionically. </li></ul>
- 11. How can you determine if a compound has ionic bonding or covalent bonding? <ul><li>A compound with ionic bonding consists of a metal and nonmetal. </li></ul><ul><li>A compound with covalent bonding consists of nonmetals only! </li></ul>
- 12. Give the shape of each of the following. H 2 Se, CH 4 , AsI 3 , CS 2 , BH 3 <ul><li>Bent, Tetrahedral, Trigonal Pyramidal, Linear, Trigonal Planar </li></ul><ul><li>Not sure about the Se, As, and S? Replace them with the first element in the group to help you out. </li></ul><ul><ul><li>For example Se and O are in the same group, so they bond with H in the same way and you know that H 2 O is bent, so H 2 Se is also! </li></ul></ul>
- 13. Which of the following are soluble in a nonpolar solvent? H 2 O, CH 4 , CO 2 , NH 3 , NaCl <ul><li>CH 4 and CO 2 </li></ul><ul><li>Both are nonpolar and like dissolves like! </li></ul>
- 14. Put the following intermolecular forces in order from weakest to strongest: Dipole, Hydrogen, London <ul><li>London, Dipole Hydrogen </li></ul>
- 15. Identify the element with the following electron configuration: 1s 2 2s 2 2p 6 3s 2 3p 5 <ul><li>Chlorine, Cl </li></ul><ul><li>NOT Cl - , the problem is asking for an element, not an ION! </li></ul>
- 16. Fill in the blanks with letters: <ul><li>A: pH 14-5.05 = 8.95 </li></ul><ul><li>B: [OH - ] = 10^ -5.05 = 8.91 x 10 -6 M </li></ul><ul><li>C: [OH - ]=1.01 x 10 -6 M </li></ul><ul><li>[H + ][OH - ] = 1.0 x 10 -14 </li></ul>C B A
- 17. Which values in the diagram will change with the addition of a catalyst? <ul><li>Only activation energy, E a </li></ul><ul><li>H reactants, H products, and ∆H are unchanged. </li></ul>
- 18. Na 2 CO 3 + HCl NaCl + H 2 O + CO 2 1. 0.455g sodium carbonate are titrate to the endpoint with 14.00mL of HCl, what is the concentration of the HCl <ul><li>0.613M HCl </li></ul>
- 19. 2. What mass of KCl is need to prepare 250.mL of 0.300M solution? <ul><li>5.55g KCl </li></ul>
- 20. 3. What volume of 0.500M NaOH is needed to prepare 250.mL of 0.200M solution? <ul><li>100. mL </li></ul>
- 21. 4. For the reaction I 2 + Br 2 ↔ 2IBr, K eq = 66.8 If the concentration of I 2 and Br 2 are each 0.199M, what is the concentration of IBr? <ul><li>1.63M IBr </li></ul>
- 22. Balance the following redox reaction: ClO 3 - + Fe Cl - + Fe 2+ <ul><li>6e - + 6H + + ClO3- Cl - + 3H 2 O </li></ul><ul><li>(Fe Fe 2+ + 2e - ) x3 </li></ul><ul><li>6H + + ClO 3 - + 3Fe Cl - + 3H 2 O + 3Fe 2+ </li></ul>

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