1. Name the following compounds. a. Ba(NO 3 ) 2 barium nitrate b. Ba(OH) 2 barium hydroxide

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1 1. Name the following compounds a. Ba(NO 3 ) 2 barium nitrate b. Ba(OH) 2 barium hydroxide c. KIO 3 potassium iodate d. Fe(NO 3 ) 3 iron (III) nitrate e. Cu 3 (PO 4 ) 2 copper (II) phospate f. SO 3 sulfur dioxide g. ZnSO 4 zinc sulfate h. AgNO 3 silver nitrate i. N 2 O 7 dinitrogen heptoxide 2. Give the correct formula for each of the following compounds: a. sodium dichromate Na 2 Cr 2 O 7 b. oxygen difluoride OF 2 c. calcium sulfate CaSO 4 d. dinitrogen tetrafluoride N 2 F 4 e. tin (IV) bromide SnBr 4 f. copper (II) chloride CuCl 2 g. barium carbonate BaCO 3 h. magnesium hydroxide Mg(OH) 2 3. Identify each of the following as molecular or ionic a. SeF 4 Molecular b. BaO Ionic c. LiBr Ionic d. As 4 O 6 Molecular e. SiF 4 Molecular f. CuCl Ionic g. Cs 2 O Ionic h. NH 4 HCO 3 Ionic (2 polyatomics!) i. NH 3 Molecular

2 4. Define each of the following terms a. Valence Electrons - electrons in the highest shell (energy level), is equal to the group number and are the electrons available for bonding b. Core Electrons - electrons in the lowest shells (included in the noble gas) and are not available for bonding c. Octet Rule atoms form bonds in order to have access to 8 electrons in their valence shell d. Duet Rule - atoms which form bonds in order to have access to 2 electrons in their valence shell, applies to H, Li and Be e. Ionic Bond - a transfer of electrons due to electrostatic attraction, where one atom gives an electron and the other atom accepts an electron f. Covalent Bond a sharing of 2 or more electrons to form a bond. Covalent bonds can be for 1 pairs (single), 2 pairs (double) or 3 pairs (triple) g. Diatomic Molecule atoms which exsists in nature as a molecule consisting of 2 atoms of the same kind. H O F Br I N Cl h. Polar Covalent Bond a covalent bond in which the pair of electrons are shared unequally i. Non-Polar Covalent Bond - a covalent bond in which the electron pair is shared equally, occurs between 2 of the same atom with the same electronegativity j. Electronegativity the ability of an atom to attract a pair of electrons in a bond. Helps determine bond polarity

3 5. Give the number of valence electrons for each of the following atoms and draw their Lewis dot symbols: a. Al b. Cs c. Si d. Kr e. B f. Mg g. P h. S i. Cl j. C 6. What is the octet rule and how is it is satisfied with covalent and ionic bonds? Octet rule is that atoms form bonds to have access to 8 electrons in their valence shell. Covalent bonds are where electrons are shared to achieve an octet and ionic bonds are where electrons are transferred to achieve an octet. 7. What are three ways that elements achieve octets? Sharing, Giving or Receiving electrons 8. What is the difference between a polar bond and a nonpolar bond? Polar bonds is where the shared electron pair is shared unequally, one atom pulls the bond closer to it and in a non polar bond the pair is shared equally between the 2 atoms

4 9. Draw resonance structures for the following and explain why they are necessary Necessary to show the possible structures for the molecule, the actual exists intermediate of the resonance structures a. SO 2 b. NO 3 -

5 10. What does the VSEPR Theory allow us to determine? The three dimensional arrangement of a molecule 11. Why are double and triple bonds necessary in some molecules? In order to have an octet for the atoms involved in the bond. 12. Indicate the type of bonding that would be expected for each of the following: a. NaCl = ionic b. H 2 O = covalent c. H 2 = covalent d. CoCl 2 = ionic e. C 6 H 12 O 6 = covalent 13. Draw the Lewis Structures for each of the Diatomic Molecules

6 14. Identify each of the following bonds as polar covalent or non-polar covalent a. N-N = non polar covalent b. N-O = polar covalent c. H-Cl= polar covalent d. F-F non polar covalent e. B-F= polar covalent 15. Write the ion charge for each of the following atoms a. Ca 2+ b. F 1- c. Br 1- d. K 1+ e. Ag 1+

7 16. Complete the following table Chemical Formula Lewis Electron Dot Structure Electron Geometry Molecular Geometry Polar or Nonpolar Predominant IMF O 2 H 2 O CH 3 I

8 NH 3 SO 4 2- CO CO 2

9 ClO 4 - ClO 3 -