Using the electronegativity values given in the references section, show for the indicated bonds which atom acquires the partial negative charge. (To answer this question you may consult the table of electronegativity values in the table below.) (a) H3C-CI 1A 2A Li Be 1.0 1.5 (b) H-CI Na Mg 0.9 1.2 3B 4B 5B 6B 7B K Ca Sc Ti 0.8 1.0 1.3 1.5 Rb Sr Y Zr 0.8 1.0 1.2 1.4 V 1.6 <1.0 1.0-1.4 Nb Mo 1.6 1.8 Cr Mn Fe Co 1.6 1.5 1.8 Cs Ba La Hf Ta W Re Os H 2.1 8B 1.5-1.9 2.0-2.4 8122=2 Tc Ru 1.9 2.2 2.2 2.2 Ir If none of them bears the negative charge, choose none. Ni 1.8 Rh Pd Ag Cd In Sn Sb Te 1.9 1.7 1.7 1.8 1.9 2.1 2.5-2.9 3.0-4.0 3A 4A 5A 6A 7A B C N O F 2.0 2.5 3.0 3.5 4.0 Al 1B 2B 1.5 Cu Zn 1.9 1.6 Predict which indicated bond in each set is the more polar one. Si P 1.8 2.1 S 2.5 Ga Ge As Se 1.6 1.8 2.0 2.4 0.7 0.9 1.1 1.3 1.5 1.7 1.9 2.2 2.2 2.2 2.4 1.9 1.8 1.8 1.9 2.0 2.2 CI 3.0 Br 2.8 I 2.5 Pt Au Hg Tl Pb Bi Po At

Consider the generic Lewis dot symbol for an element. Which element could this symbol represent? N O C Na F Ne B Ca X.

3) For each of the compounds MgO, Br2 and HBr:(a) What are the two atoms that formed each molecule?(b) What is their electronegativity difference between the atoms in each molecule?(c) What type of bond is formed in each molecule?(d) Are the electrons shared or transferred between the atoms in each molecule?

(a) The 03 molecule has a central oxygen atom bonded to two outer oxygen atoms that are another. In the box below, draw the Lewis electron-dot diagram of the 03 molecule. Include all valid resonance structures. 0 - 0 = 0 (b) Based on the diagram you drew in part (a), what is the shape of the ozone molecule? and trigonal Bent Ozone decomposes according to the reaction represented below. 2 03(g) → 3 0₂(8) (c) The bond enthalpy of the oxygen-oxygen bond in O₂ is 498 kJ/mol. Based on the enthalpy of the reaction represented above, what is the average bond enthalpy, in kJ/mol, of an oxygen-oxygen bond in 03 ? Ozone can oxidize HSO3(aq), as represented by the equation below. [0] 1.0 x 10-5. <-> 00: HSO3(aq) + O3(aq) → HSO4 (aq) + O₂(8) A solution is prepared in which the initial concentration of HSO₂ (aq) (6.4 × 10+ M) is much larger than that of O3(aq) (1.0 × 10-5 M). The concentration of O3(aq) is monitored as the reaction proceeds, and the data are plotted in the graph below. 8.0 x…

Chemistry

Write the empirical formula for at least four ionic compounds that could be formed from the following ions: 3+ NH,, PO, Fe”, CH, CO, 0 0,0,... X Ś

Discuss the difference between covalent bonding and non-covalent interactions.

Write the empirical formula of at least four binary ionic compounds that could be formed from the following ions: Mg²+, Al³+, I, 0²- 0,0,... X

Explain in terms of the distribution of charge, why H2O is considered a nonpolar compound.

Arrange the single covalent bonds within each set in order of INCREASING polarity. If: • most polar is b • medium polarity is c • least polar is a this leads to the following input: acb (To answer this question you may consult the table of electronegativity values in the table below.) 1A 2A Li Be 1.0 1.5 Na Mg 0.9 1.2 3B 4B 5B 6B 7B K 0.8 1.0 1.3 Ca Sc Ti V Cr Mn Fe 1.5 1.6 1.6 1.5 1.8 Rb 0.8 Sr 1.0 Y 1.2 <1.0 1.0-1.4 1. a) C-H b) P-H c) Br-H Cs Ba La Hf Ta W Re Os 0.7 0.9 1.1 1.3 1.5 1.7 1.9 2.2 2. a) P-H b) O-H c) N-H Zr 1.4 1.6 1.8 1.9 2.2 H 2.1 1.5-1.9 2.0-2.4 8B Nb Mo Te Ru Rh 8222=2 Co Ni 1.8 1.8 2.5-2.9 3.0-4.0 Pd 2.2 Pt 2.2 3A 4A 5A 6A 7A B C N 0 F 2.5 2.0 3.0 3.5 4.0 Al 1.5 1B Cu 1.9 1.6 1.6 2B Zn Ga Ge 1.8 Au Hg 2.4 Si P S CI 1.8 2.1 2.5 3.0 Ag Cd In Sn 1.9 1.7 1.7 1.8 TI Pb 1.9 1.8 1.8 As Se Br 2.0 2.4 2.8 Sb Te I 1.9 2.1 2.5 Bi Po At 1.9 2.0 2.2